General, Organic, and Biological Chemistry. Fourth Edition Karen Timberlake. Chapter 5. Compounds and Their Bonds Pearson Education, Inc.

Size: px
Start display at page:

Download "General, Organic, and Biological Chemistry. Fourth Edition Karen Timberlake. Chapter 5. Compounds and Their Bonds Pearson Education, Inc."

Transcription

1 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds 2013 Pearson Education, Inc.

2 Electrons and Reactivity Atoms contain a very small nucleus packed with neutrons and positively charged protons. a large volume of space around the nucleus that contains the negatively charged electrons. It is the electrons that determine the physical and chemical properties of atoms. Elements react in order to achieve the same electronic structure of the nearest noble gas 2013 Pearson Education, Inc. Chapter 3, Section 3 2

3 Electrons and Reactivity Atoms contain a very small nucleus packed with neutrons and positively charged protons. a large volume of space around the nucleus that contains the negatively charged electrons. It is the electrons that determine the physical and chemical properties of atoms. Elements react in order to achieve the same electronic structure of the nearest noble gas 2013 Pearson Education, Inc. Chapter 3, Section 3 3

4 Ionic and Covalent Bonds Atoms form octets to become more stable. by losing, gaining, or sharing valence electrons. by forming ionic or covalent bonds Pearson Education, Inc. Chapter 5, Section 1 4

5 Covalent Compounds Covalent compounds are formed when nonmetals share valence electrons forming a covalent bond. Covalent compounds consist of molecules, which are discrete groups of atoms, such as: water, H 2 O 2 H atoms + 1 O atom carbon dioxide, CO 2 1 C atom + 2 O atoms glucose, C 6 H 12 O 6 6 C atoms + 12 H atoms + 6 O atoms 2013 Pearson Education, Inc. Chapter 5, Section 1 5

6 Ionic Compounds Ionic compounds are formed when metal atoms transfer electrons to nonmetal atoms resulting in the formation of ionic bonds. Ionic compounds we use every day include: table salt NaCl baking soda NaHCO 3 milk of magnesia Mg(OH) Pearson Education, Inc. Chapter 5, Section 1 6

7 Ionic Compounds, Minerals Precious and semiprecious gemstones are also examples of ionic compounds called minerals. Sapphires and rubies are made of aluminum oxide (Al 2 O 3 ), which is an ionic compound. Their brilliant colors come from the presence of other metals such as chromium, which make rubies red and iron and titanium, which make sapphires blue 2013 Pearson Education, Inc. Chapter 5, Section 1 7

8 Octet Rule The octet rule is the tendency for atoms to share or transfer electrons to obtain a stable configuration of 8 valence electrons Pearson Education, Inc. Chapter 5, Section 1 8

9 Octet Rule The octet rule is associated with the stability of the noble gases except for He, which is stable with 2 valence electrons (duet). Valence Electrons He 1s 2 2 Ne 1s 2 2s 2 2p 6 8 Ar 1s 2 2s 2 2p 6 3s 2 3p 6 8 Kr 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p Pearson Education, Inc. Chapter 5, Section 1 9

10 Metals Form Positive Ions Metals form positive ions called cations by a loss of their valence electrons. with the electron configuration of the nearest noble gas. that have fewer electrons than protons. Group 1A (1) metals ion 1+ Group 2A (2) metals ion 2+ Group 3A (3) metals ion Pearson Education, Inc. Chapter 5, Section 1 10

11 Formation of a Sodium Ion, Na + Sodium achieves an octet by losing its one valence electron Pearson Education, Inc. Chapter 5, Section 1 11

12 Charge of Sodium Ion, Na + With the loss of its valence electron, a sodium ion has a 1 + charge. ion Na atom Na + charge 2013 Pearson Education, Inc. Chapter 5, Section 1 12

13 Formation of Magnesium Ion, Mg 2+ Magnesium achieves an octet by losing its two valence electrons Pearson Education, Inc. Chapter 5, Section 1 13

14 Charge of Magnesium Ion, Mg 2+ With the loss of two valence electrons magnesium forms a positive ion with a 2 + charge. Mg atom Mg 2+ ion charge 2013 Pearson Education, Inc. Chapter 5, Section 1 14

15 Formation of Negative Ions In ionic compounds, nonmetals achieve an octet arrangement. gain electrons. form negatively charged ions called anions with 3, 2, or 1 charges Pearson Education, Inc. Chapter 5, Section 1 15

16 Formation of a Chloride Ion, Cl Chlorine achieves an octet by adding one more electron to its 7 valence electrons Pearson Education, Inc. Chapter 5, Section 1 16

17 Charge of a Chloride Ion, Cl By gaining one electron, the chloride ion has a 1 charge. charge 2013 Pearson Education, Inc. Chapter 5, Section 1 17

18 Ionic Charge from Group Numbers Ions achieve the electron configuration of their nearest noble gas by forming positive ions with a charge equal to its Group number. Group 1A (1) = 1 + Group 2A (2) = 2 + Group 3A (3) = 3 + negative ions with a charge obtained by subtracting 8 or 18 from its Group number Pearson Education, Inc. Chapter 5, Section 1 18

19 Some Typical Ionic Charges 2013 Pearson Education, Inc. Chapter 5, Section 1 19

20 Group Numbers for Some Positive and Negative Ions 2013 Pearson Education, Inc. Chapter 5, Section 1 20

21 Chapter 5 Compounds and Their Bonds 5.2 Writing names and formulas for ionic compounds 2013 Pearson Education, Inc Pearson Education, Inc. Chapter 5, Section 1 21

22 Ionic Compounds Ionic compounds consist of positive and negative ions. have attractive forces between the positive and negative ions called ionic bonds. have high melting and boiling points. are solid at room temperature Pearson Education, Inc. Chapter 5, Section 1 22

23 Salt Is an Ionic Compound Sodium chloride, or table salt, is an example of an ionic compound Pearson Education, Inc. Chapter 5, Section 1 23

24 Formulas of Ionic Compounds The chemical formula of an ionic compound represents the element symbols and subscripts, which represent the lowest whole-number ratio of ions. In the formula of an ionic compound, the sum of positively and negatively charged ions is always zero Rule of Zero Charge the charges are balanced Pearson Education, Inc. Chapter 5, Section 1 24

25 Charge Balance for NaCl, Salt In NaCl, a Na atom loses its valence electron. a Cl atom gains an electron. the symbol of the metal (sodium) is written first, followed by the symbol of the nonmetal (chlorine) Pearson Education, Inc. Chapter 5, Section 1 25

26 Charge Balance In MgCl 2 In MgCl 2, a Mg atom loses two valence electrons. two Cl atoms gain one electron each. subscripts indicate the number of ions needed to give charge balance. the symbol of the metal (magnesium) is written first, followed by the symbol of the nonmetal (chlorine) Pearson Education, Inc. Chapter 5, Section 1 26

27 Writing Formulas For Binary Ionic Compounds Binary ionic compounds are made from 2 elements, a metal and a nonmetal. Charge balance is used to write the formula for sodium nitride, a compound containing Na + and N 3. The metal ion is written first, followed by nonmetal, subscripts indicate how many of each 2013 Pearson Education, Inc. Chapter 5, Section 1 27

28 Charge Balance in Na 2 S In sodium sulfide, Na 2 S, two Na atoms lose one valence electron each. one S atom gains two electrons. subscripts show the number of ions needed to give charge balance. The group of ions with the lowest ratio of ions in an ionic compound is called a formula unit Pearson Education, Inc. Chapter 5, Section 1 28

29 Formula from Ionic Charges Write the ionic formula of the compound containing Ba 2+ and Cl. Write the symbols of each ion. Ba 2+ Cl Balance the charges. Ba 2+ Cl (two Cl needed) Cl Write the metal first, followed by the nonmetal,, using a subscript to represent the number of. Cl ions. BaCl Pearson Education, Inc. Chapter 5, Section 1 29

30 Writing Names For Binary Ionic Compounds The name of an Binary ionic compound is made up of 2 elements. has the name of the metal ion written first. has the name of the nonmetal ion written second using the first syllable of its element name. followed by ide. has a space separating the name of the metal and nonmetal Pearson Education, Inc. Chapter 5, Section 1 30

31 Charges of Representative Elements 2013 Pearson Education, Inc. Chapter 5, Section 3 31

32 Naming Binary Ionic Compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 32

33 Naming Mg 3 N 2 Step 1 Identify the cation and anion. The cation from Group 2A (2) is Mg 2+, and the anion from Group 5A (15) is N 3. Step 2 Name the cation by its element name. Cation: Mg 2+ is magnesium Step 3 Name the anion by using the first syllable of its element name followed by ide. Anion: nitrogen becomes nitride, N 3 Step 4 Write the name for the cation first and the name for the anion second. Mg 3 N 2 is magnesium nitride Pearson Education, Inc. Chapter 5, Section 1 33

34 What do you notice about these names and formulas? Chemical Formula Fe 2 O 3 FeCl 2 PbS AlP CuF 2 SnI 4 KBr Written Form iron(iii) oxide iron(ii) chloride lead(ii) sulfide aluminum phosphide copper(ii) fluoride tin(iv) iodide potassium bromide 2013 Pearson Education, Inc. Chapter 5, Section

35 Metals with Variable Ion Charge Most transition metals (3-12) and Group 4A (14) metals form 2 or more positive ions, except Zn 2+, Ag +, and Cd 2+, which form only one ion Pearson Education, Inc. Chapter 5, Section 1 35

36 Metals with Variable Charge The names of transition metals with two or more positive ions (cations) use a Roman numeral after the name of the metal to identify the ion charge Pearson Education, Inc. Chapter 5, Section 1 36

37 Naming Ionic Compounds with Variable Charge Metals 2013 Pearson Education, Inc. Chapter 5, Section 1 37

38 Naming FeCl 2 Step 1 Determine the charge of the cation from the anion. Analyze the Problem Pearson Education, Inc. Chapter 5, Section 1 38

39 Naming FeCl 2 Step 2 Name the cation by its element name and use a Roman numeral in parentheses for the charge. Fe 2+ = iron(ii) Step 3 Name the anion by using the first syllable of its element name followed by ide. Cl = chloride Step 4 Write the name for the cation first and the name for the anion second. iron(ii) chloride 2013 Pearson Education, Inc. Chapter 5, Section 1 39

40 Examples of Names of Compounds with Variable Charge Metals 2013 Pearson Education, Inc. Chapter 5, Section 1 40

41 What do you notice about these names and formulas? Chemical Formula (NH 4 ) 2 S CoSO 4 Fe(OH) 3 Ca 3 (PO 4 ) 2 NH 4 NO 3 Written Form ammonium sulfide cobalt (II) sulfate iron (III) hydroxide calcium phosphate ammonium nitrate 2013 Pearson Education, Inc. Chapter 5, Section

42 Polyatomic Ions A polyatomic ion is a group of atoms. has an overall ionic charge. Examples: NH + 4 ammonium OH hydroxide NO 3 nitrate NO 2 nitrite CO 2 3 carbonate PO 3 4 phosphate HCO 3 hydrogen carbonate (bicarbonate) 2013 Pearson Education, Inc. Chapter 5, Section 1 42

43 Some Names of Polyatomic Ions The names of common polyatomic anions end in ate. NO 3 nitrate PO 3 4 phosphate with one oxygen less, end in ite NO 2 nitrite PO 3 3 phosphite with hydrogen attached, use prefix hydrogen (or bi). HCO 3 hydrogen carbonate (bicarbonate) HSO 3 hydrogen sulfite (bisulfite) 2013 Pearson Education, Inc. Chapter 5, Section 1 43

44 Compounds Containing Polyatomic Ions Polyatomic ions must be associated with an ion of opposite charge. form ionic bonds with ions of opposite charge to achieve charge balance. Example: charge balance: Ca 2+ calcium NO 3 nitrate ion Ca(NO 3 ) 2 calcium nitrate 2013 Pearson Education, Inc. Chapter 5, Section 1 44

45 Some Compounds with Polyatomic Ions 2013 Pearson Education, Inc. Chapter 5, Section 1 45

46 Guide to Naming Compounds with Polyatomic Ions 2013 Pearson Education, Inc. Chapter 5, Section 1 46

47 Name K 2 SO 4 Step 1 Identify the cation and polyatomic ion (anion). Cation: K + Anion: SO 2 4 Step 2 Name the cation, using a Roman numeral if needed. K + = potassium ion Step 3 Name the polyatomic ion. SO 2 4 = sulfate ion Step 4 Write the name or the compound, cation first and the polyatomic ion second. K 2 SO 4 = potassium sulfate 2013 Pearson Education, Inc. Chapter 5, Section 1 47

48 Guide to Writing Formulas for Compounds with Polyatomic Ions 2013 Pearson Education, Inc. Chapter 5, Section 1 48

49 Write the Formula for Aluminium Hydroxide Step 1 Identify the cation and polyatomic ion (anion). Al 3+ and OH Step 2 Balance the charges Pearson Education, Inc. Chapter 5, Section 1 49

50 Write the Formula for Aluminium Hydroxide Step 3 Write the formula, cation first, using the subscripts from charge balance. Al(OH) Pearson Education, Inc. Chapter 5, Section 1 50

51 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds 5.5 Covalent Compounds: Sharing Electrons 2013 Pearson Education, Inc. Lectures 2013 Pearson Education, Inc. Chapter 5, Section 1 51

52 Covalent Bonds Covalent bonds form when atoms of nonmetals share electrons to complete octets. Valence electrons are not transferred, but shared to achieve stability Pearson Education, Inc. Chapter 5, Section 1 52

53 Formation of H 2 In the simplest covalent molecule, H 2, the H atoms increase attraction as they move closer. share electrons to achieve a stable configuration. form a covalent bond Pearson Education, Inc. Chapter 5, Section 1 53

54 Formation of H Pearson Education, Inc. Chapter 5, Section 1 54

55 Electron-Dot Formulas of Covalent Molecules In a fluorine (F 2 ) molecule, the F atoms share one of their valence electrons. acquire an octet. form a covalent bond Pearson Education, Inc. Chapter 5, Section 1 55

56 Elements That Exist as Diatomic Molecules These seven elements share electrons to form diatomic, covalent molecules. BrINClHOF! Remember it! 2013 Pearson Education, Inc. Chapter 5, Section 1 56

57 Bonding Patterns of Some Nonmetals The number of covalent bonds a nonmetal forms is usually equal to the number of electrons it needs to acquire a stable electron configuration. Typical bonding patterns for some nonmetals are shown in the table below Pearson Education, Inc. Chapter 5, Section 1 57

58 Bonding Patterns of Some Nonmetals Biological molecules tend to be made out of H, O,N, and C mostly. Bonding tendency rule for H, O, N, C HONC 1234 Rule Hydrogen tends to form 1 bond Oxygen tends to form 2 bonds Nitrogen tends to form 3 bonds Carbon tends to form 4 bonds 2013 Pearson Education, Inc. Chapter 5, Section 1 58

59 Electron-Dot Formulas for Some Covalent Compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 59

60 Guide to Drawing Electron-Dot Formulas 2013 Pearson Education, Inc. Chapter 5, Section 1 60

61 Draw the Electron-Dot Formula for NH 3 Step 1 Determine the arrangement of atoms. In NH 3, N is the central atom and is bonded to three H atoms. Step 2 Determine the total number of valence electrons. Total valence electrons for NH 3 = 8 e 2013 Pearson Education, Inc. Chapter 5, Section 1 61

62 Draw the Electron-Dot Formula for NH 3 Step 3 Attach each bonded atom to the central atom with a pair of electrons Pearson Education, Inc. Chapter 5, Section 1 62

63 Draw the Electron-Dot Formula for NH 3 Step 4 Place the remaining electrons using single or multiple bonds to complete the octets. 8 valence e 6 bonding e = 2 e remaining Use the remaining 2 e to complete the octet around the N atom Pearson Education, Inc. Chapter 5, Section 1 63

64 Exceptions to the Octet Rule Not all atoms have octets. Some can have less than an octet, such as H, which requires only 2 electrons, B, which requires only 3 electrons, and Be, which requires only 4 electrons. Some can have expanded octets, such as P, which can have 10 electrons, S, which can have 12 electrons, and Cl, Br and I, which can have 14 electrons 2013 Pearson Education, Inc. Chapter 5, Section 1 64

65 Single and Multiple Bonds In many covalent compounds, atoms share two or three pairs of electrons to complete their octets. In a single bond, one pair of electrons is shared. In a double bond, two pairs of electrons are shared. In a triple bond, three pairs of electrons are shared Pearson Education, Inc. Chapter 5, Section 1 65

66 Draw the Electron-Dot Formula for CS 2 Step 1 Determine the arrangement of atoms. In CS 2, C is the central atom and is bonded to two S atoms Pearson Education, Inc. Chapter 5, Section 1 66

67 Draw the Electron-Dot Formula for CS 2 Step 2 Determine the total number of valence electrons. Total valence electrons for 2013 Pearson Education, Inc. Chapter 5, Section 1 67

68 Draw the Electron-Dot Formula for CS 2 Step 3 Attach each bonded atom to the central atom with a pair of electrons. A pair of bonding electrons (single bond) is placed between each S atom and the central C atom Pearson Education, Inc. Chapter 5, Section 1 68

69 Draw the Electron-Dot Formula for CS 2 Step 4 Place the remaining electrons using single or multiple bonds to complete the octets. 16 valence e - 4 bonding e = 12 e remaining The remaining 12 electrons are placed as six lone pairs of electrons on both S atoms. However, this does not complete the octet for the C atom Pearson Education, Inc. Chapter 5, Section 1 69

70 Draw the Electron-Dot Formula for CS 2 Step 4 Continued: Double and Triple Covalent Bonds: To complete the octet for the C atom, it needs to share an additional lone pair from each of the S atoms, forming a double bond with each S atom Pearson Education, Inc. Chapter 5, Section 1 70

71 A Nitrogen Molecule has a Triple Bond In a nitrogen molecule, N 2, each N atom shares 3 electrons, each N atom attains an octet, and the sharing of 3 sets of electrons is called a triple bond Pearson Education, Inc. Chapter 5, Section 1 71

72 Resonance Structures Resonance structures are two or more electron-dot formulas for the same arrangement of atoms. related by a double-headed arrow ( ). written by changing the location of a double bond between the central atom and a different attached atom Pearson Education, Inc. Chapter 5, Section 1 72

73 Writing Resonance Structures for SO 2 Sulfur dioxide has two resonance structures. Step 1 Determine the arrangement of atoms. In SO 2, the S atom is the central atom. O S O Step 2 Determine the total number of valence electrons. Total valence electrons for 2013 Pearson Education, Inc. Chapter 5, Section 1 73

74 Writing Resonance Structures for SO 2 Step 3 Attach each bonded atom to the central atom with a pair of electrons Pearson Education, Inc. Chapter 5, Section 1 74

75 Writing Resonance Structures for SO 2 Step 4 Place the remaining electrons using single or multiple bonds to complete the octets. The remaining 14 electrons are drawn as lone pairs of electrons to complete the octets of the O atoms, but not the S atom Pearson Education, Inc. Chapter 5, Section 1 75

76 Writing Resonance Structures for SO 2 Step 4 Continued: To complete the octet for S, an additional lone pair from one of the O atoms is shared to form a double bond. Because the shared lone pair of electrons can come from either O atom, two resonance structures can be drawn Pearson Education, Inc. Chapter 5, Section 1 76

77 Learning Check FNO 2, a rocket propellant, has two resonance structures. One is shown below. What is the other resonance structure? 2013 Pearson Education, Inc. Chapter 5, Section 1 77

78 Solution FNO 2, a rocket propellant, has two resonance structures. One is shown below. What is the other resonance structure? 2013 Pearson Education, Inc. Chapter 5, Section 1 78

79 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds 5.6 Naming and Writing Covalent Formulas 2013 Pearson Education, Inc. Lectures 2013 Pearson Education, Inc. Chapter 5, Section 1 79

80 Names of Covalent Compounds When naming a covalent compound, the first nonmetal in the formula is named by its element name, and the second nonmetal is named using the first syllable of its element name, followed by ide. Prefixes are used to indicate the number of atoms present for each element in the compound, and because two nonmetals can form two or more different compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 80

81 Prefixes Used in Naming Covalent Compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 81

82 Some Covalent Compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 82

83 Guide to Naming Covalent Compounds with Two Nonmetals 2013 Pearson Education, Inc. Chapter 5, Section 1 83

84 Naming Covalent Compounds, SO 2 Analyze the Problem. Symbols of Elements S Name sulfur oxygen Subscripts 1 2 Prefix (none) understood di Step 1 Name the first nonmetal by its element name. In SO 2, the first nonmetal (S) is sulfur. O 2013 Pearson Education, Inc. Chapter 5, Section 1 84

85 Naming Covalent Compounds, SO 2 Step 2 Name the second nonmetal by using the first syllable of its name followed by ide. The second nonmetal (O) is named oxide. Step 3 Add prefixes to indicate the number of atoms (subscripts). Because there is one sulfur atom, no prefix is needed. The subscript two for the oxygen atoms is written as the prefix di. The name of SO 2 is sulfur dioxide Pearson Education, Inc. Chapter 5, Section 1 85

86 Learning Check Name the covalent compound P 2 O Pearson Education, Inc. Chapter 5, Section 1 86

87 Solution Name the covalent compound P 2 O 5. Analyze the Problem. Symbols of Elements P O Name phosphorus oxygen Subscripts 2 5 Prefix di penta Step 1 Name the first nonmetal by its element name. In P 2 O 5, the first nonmetal (P) is phosphorus Pearson Education, Inc. Chapter 5, Section 1 87

88 Solution Step 2 Name the second nonmetal by using the first syllable of its name followed by ide. The second nonmetal (O) is named oxide. Step 3 Add prefixes to indicate the number of atoms (subscripts). The subscript for the two P atoms is di; the subscript for the five oxygen atoms is penta. The name of P 2 O 5 is phosphorus pentoxide. When the vowels o and o, or a and o appear together (pentaoxide), the first vowel is omitted Pearson Education, Inc. Chapter 5, Section 1 88

89 Guide to Writing Formulas for Covalent Compounds 2013 Pearson Education, Inc. Chapter 5, Section 1 89

90 Writing Formulas of Covalent Compounds Write the formula for sulfur hexafluoride. Analyze the Problem. Name sulfur hexafluoride Symbols of Elements S F Subscripts 1 6 (from hexa) Step 1 Write the symbols in order of the elements in the name. S F Step 2 Write any prefixes as subscripts. Prefix hexa = 6 Formula: SF Pearson Education, Inc. Chapter 5, Section 1 90

91 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds The Shape of Molecules 2013 Pearson Education, Inc. Lectures 2013 Pearson Education, Inc. Chapter 5, Section 1 91

92 Valence-Shell Electron-Pair Repulsion Theory (VSEPR) In the valence-shell electron-pair repulsion (VSEPR) theory, the electron groups around a central atom are arranged as far apart from each other as possible. have the least amount of electron-electron repulsion. are used to predict the molecular shape Pearson Education, Inc. Chapter 5, Section 1 92

93 Molecular Shape why does it matter? Watson and Crick with their famous 3-D model of DNA How did they know? Shape of molecules important as it influences their physical and chemical behavior 2013 Pearson Education, Inc. Chapter 5, Section 1 93

94 What Determines the 3-D Shape of a Molecule? Need to understand electrostatic repulsion (electron clouds around the central atom in a molecule are going to repel each other) Need to draw Lewis structures Need to differentiate between lone pair electrons and bonding pair electrons around the central atom in a molecule Need to apply a theory based on all of the above 2013 Pearson Education, Inc. Chapter 5, Section 1 94

95 Lewis Structure Lone pair e- (nonbonding e- domain) Bonding pair e- (bonding domain) Electron pairs are also called domains Electron domains try to stay out of each others way (to minimize repulsion) 2013 Pearson Education, Inc. Chapter 5, Section 1 95

96 Valence Shell Electron Pair Repulsion Theory VSEPR, for short Proposed by English chemist Ron Gillespie in the 1950s Based on Lewis structures of molecules and electron repulsion 2013 Pearson Education, Inc. Chapter 5, Section 1 96

97 VSEPR Theory Rules 1. In a molecule, electron domains (pairs) will orient themselves around the central atom in an arrangement that minimizes the repulsions among them. 2. The three dimensional orientation of the outer atoms around the central atom depends on the numbers and types of e- domains 3. Lone pair electrons count as 1 electron domain; single, double or triple bonding pair electrons count as 1 electron domain Pearson Education, Inc. Chapter 5, Section 1 97

98 Shapes of Molecules The three-dimensional shape of a molecule can be predicted by the number of bonding groups (bonding domains) and lone-pair electrons (nonbonding domains) around the central atom in the molecule VSEPR theory (valence-shell-electron-pair repulsion) Pearson Education, Inc. Chapter 5, Section 1 98

99 Molecules with Two Electron Domains In a molecule of BeCl 2, there are two electron groups bonded to the central atom, Be (Be is an exception to the octet rule). to minimize repulsion, the arrangement of two electron groups is 180, or opposite each other. the shape of the molecule is linear Pearson Education, Inc. Chapter 5, Section 1 99

100 Molecules With Three Electron Domains In a molecule of BF 3, three electron groups are bonded to the central atom B (B is an exception to the octet rule). repulsion is minimized with 3 electron groups at angles of 120. the shape is trigonal planar Pearson Education, Inc. Chapter 5, Section 1 100

101 Three Electron Domains with a Lone Pair In a molecule of SO 2, S has 3 electron groups; 2 electron groups bonded to O atoms and one lone pair. repulsion is minimized with the electron groups at angles of 120, a trigonal planar arrangement. the shape is determined by the two O atoms bonded to S, giving SO 2 a bent (~120 ) shape Pearson Education, Inc. Chapter 5, Section 1 101

102 Four Electron Domains In a molecule of CH 4, there are four electron groups around C. repulsion is minimized by placing four electron groups at angles of 109, which is a tetrahedral arrangement. the four bonded atoms form a tetrahedral shape Pearson Education, Inc. Chapter 5, Section 1 102

103 Four Electron Groups with a Lone Pair In a molecule of NH 3, three electron groups bond to H atoms, and the fourth one is a lone (nonbonding) pair. repulsion is minimized with 4 electron groups in a tetrahedral arrangement. the three bonded atoms form a pyramidal (~109 ) shape Pearson Education, Inc. Chapter 5, Section 1 103

104 Four Electron Groups with Two Lone Pairs In a molecule of H 2 O, two electron groups are bonded to H atoms and two are lone pairs (4 electron groups). four electron groups minimize repulsion in a tetrahedral arrangement. the shape with two bonded atoms is bent (~109 ) Pearson Education, Inc. Chapter 5, Section 1 104

105 Molecular Shapes for 2 and 3 Bonded Atoms 2013 Pearson Education, Inc. Chapter 5, Section 1 105

106 Molecular Shapes for 4 Bonded Atoms 2013 Pearson Education, Inc. Chapter 5, Section 1 106

107 Guide to Predicting Molecular Shape (VSEPR Theory) 2013 Pearson Education, Inc. Chapter 5, Section 1 107

108 Predicting the Molecular Shape of H 2 Se Step 1 Draw the electron-dot formula. In the electron-dot formula for H 2 Se, there are four electron groups, including two lone pairs of electrons around Se Pearson Education, Inc. Chapter 5, Section 1 108

109 Predicting the Molecular Shape of H 2 Se Step 2 Arrange the electron groups around the central atom to minimize repulsion. The four electron groups around Se would have a tetrahedral arrangement. Step 3 Use the atoms bonded to the central atom to determine the molecular shape. Two bonded atoms give H 2 Se a bent shape with a bond angle of ~ Pearson Education, Inc. Chapter 5, Section 1 109

110 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds A closer look at bonding type the concept of electronegativity 2013 Pearson Education, Inc Pearson Education, Inc. Chapter 5, Section 1 110

111 General Rules for Bond Type Negative complex ions Ionic Bond Nonmetal Nonmetal Covalent Bond Metal 2013 Pearson Education, Inc. Chapter 5, Section 1 111

112 Ionic or Covalent? So far, we have been employing the following generalization for the type of bonding holding atoms together in a substance Generalization metal + nonmetal = ionic bond nonmetal + nonmetal = covalent bond Reality Bonding type is on a continuum, from 100% ionic to 100% covalent! 100% covalent 100% ionic 2013 Pearson Education, Inc. Chapter 5, Section 1 112

113 Bonding Conundrum Arose in the 1930 s from American Chemist Linus Pauling s work on the nature of the chemical bond. Pauling realized that there was some inbetweeness with the bonding in many substances Calculated the ability of elements to attract electrons to themselves when bonding Called this ability the Electronegativity of the element 2013 Pearson Education, Inc. Chapter 5, Section

114 Determining Predominant Bond type Electronegativity is a relative measure of the tendency for atoms of an element to attract electrons to themselves in a chemical bond. Originated with American chemist Linus Pauling ( ), a 2x Nobel Prize winner who did most of his work at Cal Poly Tech, but finished his career at Stanford 2013 Pearson Education, Inc. Chapter 5, Section 1 114

115 2013 Pearson Education, Inc. Chapter 5, Section 1 115

116 Electronegativity (EN) Values of the Elements Scale ranges from 0.7 to Pearson Education, Inc. Chapter 5, Section 1 116

117 Electronegativity Electronegativity is a measure of an atom s ability to attract electrons to itself in a chemical bond increases from left to right, going across a period on the periodic table. decreases going down a group on the periodic table. is high for the nonmetals, with fluorine as the highest. is low for the metals and transition metals Pearson Education, Inc. Chapter 5, Section 1 117

118 Trends in Periodic table 2013 Pearson Education, Inc. Chapter 5, Section 1 118

119 Periodic trends in electronegativity Electronegativity decreases down a group because: Atomic radius increases, valence e- further away from nucleus, decreases pulling power of nucleus Electronegativity increases from left to right across a period because: Atomic radius decreases, valence e- closer to the nucleus, increases pulling power of nucleus 2013 Pearson Education, Inc. Chapter 5, Section 1 119

120 Bonding and Electronegativity According to Pauling, the difference in the electronegativity values of the two atoms involved in a chemical bond can be used to predict the type of bond that forms. Pauling Classified chemical bonds into the following three types, based on differences in electronegativity Ionic Polar Covalent Nonpolar Covalent 2013 Pearson Education, Inc. Chapter 5, Section 1 120

121 Electronegativity and Bond Type It is the difference in the electronegativies (ΔEN) of two bonded atoms that determines the predominant bond type ΔEN 0.4 Nonpolar covalent bond (e- shared equally between atoms) ΔEN 0.5 to 1.7 polar covalent bond, (e- shared unequally) ΔEN > 1.7 ionic bond (e- transferred) Pearson Education, Inc. Chapter 5, Section 1 121

122 Bond Character Summary a) Nonpolar covalent bond electrons shared equally b) Polar covalent bond e- not shared equally, more electronegative atom has greater share of e- cloud c) Ionic bond e- transferred from one atom to other, creates a + and ion 2013 Pearson Education, Inc. Chapter 5, Section 1 122

123 Nonpolar Covalent Bonds A nonpolar covalent bond occurs between nonmetals. has an equal or almost equal sharing of electrons. has almost no electronegativity difference (0.0 to 0.4). Examples: Atoms Electronegativity Type of Bond Difference 2013 Pearson Education, Inc. Chapter 5, Section 1 123

124 Example of Nonpolar Covalent Bonds Diatomic elements e.g. H 2 Bonds between P and H = = Pearson Education, Inc. Chapter 5, Section 1 124

125 Polar Covalent Bonds A polar covalent bond occurs between nonmetal atoms that do not share electrons equally. has a moderate electronegativity difference (0.5 to 1.7). Examples: Atoms Electronegativity Type of Bond Difference 2013 Pearson Education, Inc. Chapter 5, Section 1 125

126 Comparing Nonpolar and Polar Covalent Bonds 2013 Pearson Education, Inc. Chapter 5, Section 1 126

127 Result of differences in electronegativity: More electronegative element has greater share of e- cloud, it is electron rich Less electronegative element is e- poor Creation of partial charges on the atoms in the bond (bond dipoles) + and Pearson Education, Inc. Chapter 5, Section 1 127

128 Example: Bond between H and Cl Electronegativity values H= 2.1, Cl = 3.0 e- cloud pulled towards Cl atom = Polar Covalent Bond electron poor region H electron rich region Cl e - rich H Cl + - e - poor Direction e- cloud being pulled 2013 Pearson Education, Inc. Chapter 5, Section

129 Bond Polarity and Dipoles Bonds become more polar as the difference in electronegativity values of bonding atoms increases. Polar covalent bonds have a separation of charges called a dipole. The positive and negative ends of the dipole are indicated by the lowercase Greek letter delta with a positive or negative sign, δ+ and δ-, or an arrow that points from the positive to the negative charge Pearson Education, Inc. Chapter 5, Section 1 129

130 Ionic Bonds An ionic bond occurs between metal and nonmetal ions. is a result of electron transfer. has a large electronegativity difference (1.8 or more). Examples: Atoms Electronegativity Type of Bond Difference 2013 Pearson Education, Inc. Chapter 5, Section 1 130

131 Determining Predominant Bond Type Look at the electronegativity values of atoms involved in bond Calculate electronegativity difference ( EN) If the bond is polar covalent, draw arrow in direction that e- cloud is pulled (more electronegative atom) Also use lower case Greek symbol for delta,, along with + or - sign 2013 Pearson Education, Inc. Chapter 5, Section 1 131

132 Electronegativity and Bond Types 2013 Pearson Education, Inc. Chapter 5, Section 1 132

133 Predicting Bond Types 2013 Pearson Education, Inc. Chapter 5, Section 1 133

134 Learning Check Use the electronegativity difference to identify the type of bond between the following atoms as nonpolar covalent (NP), polar covalent (P), or ionic (I). A. K N B. N O C. Cl Cl D. B Cl 2013 Pearson Education, Inc. Chapter 5, Section 1 134

135 Solution Use the electronegativity difference to identify the type of bond between the following atoms as nonpolar covalent (NP), polar covalent (P), or ionic (I). A. K N 2.2 ionic (I) B. N O 0.5 polar covalent (P) C. Cl Cl 0.0 nonpolar covalent (NP) D. B Cl 1.0 polar covalent (P) 2013 Pearson Education, Inc. Chapter 5, Section 1 135

136 Polar Molecules A polar molecule contains polar bonds. has a separation of positive and negative charge. called a dipole, indicated with + and. has dipoles that do not cancel. + H Cl NH 3 dipole Dipoles do not cancel Pearson Education, Inc. Chapter 5, Section 1 136

137 Nonpolar Molecules A nonpolar molecule contains nonpolar bonds Cl Cl H H or has a symmetrical arrangement of polar bonds Pearson Education, Inc. Chapter 5, Section 1 137

138 Guide to Determination of Polarity 2013 Pearson Education, Inc. Chapter 5, Section 1 138

139 Molecular Polarity, H 2 O Determine the polarity of the H 2 O molecule. Step 1 Determine if the bonds are polar covalent or nonpolar covalent. From the electronegativity table, O 3.5 and H 2.1 gives a difference of 1.4, which makes the O H bonds, polar covalent Pearson Education, Inc. Chapter 5, Section 1 139

140 Molecular Polarity, H 2 O Determine the polarity of the H 2 O molecule. Step 2 If the bonds are polar covalent, draw the electron-dot formula and determine if the dipoles cancel or not. The four electron groups of oxygen are bonded to two H atoms. Thus, the H 2 O molecule has a net dipole, which makes it a polar molecule Pearson Education, Inc. Chapter 5, Section 1 140

141 Polar Molecules A polar molecule contains polar bonds. has a separation of positive and negative charge. called a dipole, indicated with + and. has dipoles that do not cancel. + H Cl NH 3 dipole Dipoles do not cancel Pearson Education, Inc. Chapter 5, Section 1 141

142 Learning Check Determine the shape of each of the following molecules and whether they are polar or nonpolar. Explain. 1. PBr 3 2. HBr 3. Br 2 4. SiBr Pearson Education, Inc. Chapter 5, Section 1 142

143 Solution Determine the shape of each of the following molecules and whether they are polar or nonpolar. Explain. 1. PBr 3 pyramidal; polar; dipoles don t cancel 2. HBr linear; polar; one polar bond (dipole) 3. Br 2 linear; nonpolar; nonpolar bond 4. SiBr 4 tetrahedral; nonpolar; dipoles cancel 2013 Pearson Education, Inc. Chapter 5, Section 1 143

144 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds 5.9 Attractive Forces in Compounds 2013 Pearson Education, Inc. Lectures 2013 Pearson Education, Inc. Chapter 5, Section 1 144

145 States of Matter The fundamental difference between states of matter is the distance between particles Pearson Education, Inc. Chapter 5, Section 1 145

146 States of Matter Because in the solid and liquid states particles are closer together, we refer to them as condensed phases Pearson Education, Inc. Chapter 5, Section 1 146

147 The States of Matter The state a substance is in at a particular temperature and pressure depends on two antagonistic entities: The kinetic energy of the particles The strength of the attractions between the particles 2013 Pearson Education, Inc. Chapter 5, Section 1 147

148 Ionic Compounds In ionic compounds, ionic bonds require large amounts of energy to break. hold positive and negative ions together. explain their high melting points Pearson Education, Inc. Chapter 5, Section 1 148

149 What about covalent compounds? The attractions between molecules are not nearly as strong as the intramolecular attractions that hold compounds together Pearson Education, Inc. Chapter 5, Section 1 149

150 Intermolecular Forces They are, however, strong enough to control physical properties such as the state a molecular compound will be in at room temperature, its melting and boiling point Pearson Education, Inc. Chapter 5, Section 1 150

151 Intermolecular Forces In addition, they are responsible for the shapes of protein molecules, DNA, water s unique properties, the structure of the cell membrane, etc 2013 Pearson Education, Inc. Chapter 5, Section 1 151

152 Covalent Compounds In covalent compounds, the attractive forces between solid and liquid molecules are weaker than ionic bonds. require less energy to break. explain why their melting points are lower than ionic compounds. These attractive forces include dipole-dipole attractions, dispersion forces, and hydrogen bonding Pearson Education, Inc. Chapter 5, Section 1 152

153 Intermolecular Forces They are, however, strong enough to control physical properties such as boiling and melting points, vapor pressures, and viscosities Pearson Education, Inc. Chapter 5, Section 1 153

154 Dipole-Dipole Attractions In covalent compounds, polar molecules exert attractive forces between molecules called dipole-dipole attractions. dipole dipole forces 2013 Pearson Education, Inc. Chapter 5, Section 1 154

155 Dipole-Dipole Attractions, Hydrogen Bonds In covalent compounds, some polar molecules form strong dipole attractions called hydrogen bonds, which occur between the partially positive hydrogen atom of one molecule and a lone pair of electrons on a nitrogen, oxygen, or fluorine atom in another molecule Pearson Education, Inc. Chapter 5, Section 1 155

156 Dispersion Forces Dispersion forces are weak attractions between nonpolar molecules. caused by temporary dipoles that develop when electrons are not distributed equally. Nonpolar molecules form attractions when they form temporary dipoles Pearson Education, Inc. Chapter 5, Section 1 156

157 London Dispersion Forces While the electrons in the 1s orbital of helium would repel each other (and, therefore, tend to stay far away from each other), it does happen that they occasionally wind up on the same side of the atom Pearson Education, Inc. Chapter 5, Section 1 157

158 London Dispersion Forces At that instant, then, the helium atom is polar, with an excess of electrons on the left side and a shortage on the right side Pearson Education, Inc. Chapter 5, Section 1 158

159 London Dispersion Forces Another helium nearby, then, would have a dipole induced in it, as the electrons on the left side of helium atom 2 repel the electrons in the cloud on helium atom Pearson Education, Inc. Chapter 5, Section 1 159

160 London Dispersion Forces London dispersion forces, or dispersion forces, are attractions between an instantaneous dipole and an induced dipole Pearson Education, Inc. Chapter 5, Section 1 160

161 London Dispersion Forces These forces are present in all molecules, whether they are polar or nonpolar. The tendency of an electron cloud to distort in this way is called polarizability Pearson Education, Inc. Chapter 5, Section 1 161

162 Factors Affecting London Forces The shape of the molecule affects the strength of dispersion forces: long, skinny molecules (like n-pentane tend to have stronger dispersion forces than short, fat ones (like neopentane). This is due to the increased surface area in n-pentane Pearson Education, Inc. Chapter 5, Section 1 162

163 Factors Affecting London Forces The strength of dispersion forces tends to increase with increased molecular weight. Larger atoms have larger electron clouds, which are easier to polarize Pearson Education, Inc. Chapter 5, Section 1 163

164 Which Have a Greater Effect: Dipole-Dipole Interactions or Dispersion Forces? If two molecules are of comparable size and shape, dipole-dipole interactions will likely be the dominating force. If one molecule is much larger than another, dispersion forces will likely determine its physical properties Pearson Education, Inc. Chapter 5, Section 1 164

165 Comparison of Bonding and Attractive Forces 2013 Pearson Education, Inc. Chapter 5, Section 1 165

166 Intermolecular Forces Affect Many Physical Properties The strength of the attractions between particles can greatly affect the properties of a substance or solution Pearson Education, Inc. Chapter 5, Section 1 166

167 Melting Points and Attractive Forces The stronger the attractive force between ions or molecules, the higher the melting points. Ionic compounds, have the strongest attractive force and, therefore the highest melting points. Covalent molecules have less attractive forces than ionic compounds and, therefore lower melting points Pearson Education, Inc. Chapter 5, Section 1 167

168 Melting Points and Attractive Forces The attractive forces between covalent molecules vary in magnitude; the stronger the attractive force, the higher its melting point. Hydrogen bonds are the strongest type of dipole dipole attractions, requiring the most energy to break, followed by dipole dipole forces. Dispersion forces are the weakest, requiring even less energy to break them, and therefore have lower melting points than hydrogen bonds and dipole dipole forces Pearson Education, Inc. Chapter 5, Section 1 168

169 Melting Points of Selected Substances 2013 Pearson Education, Inc. Chapter 5, Section 1 169

170 Learning Check Identify the main type of attractive forces for each of the following compounds: ionic bonds, dipole dipole, hydrogen bonds or dispersion. 1. NCl 3 2. H 2 O 3. Br 2 4. KCl 5. NH Pearson Education, Inc. Chapter 5, Section 1 170

171 Solution Identify the main type of attractive forces for each of the following compounds: ionic bonds, dipole dipole, hydrogen bonds or dispersion. 1. NCl 3 dipole dipole 2. H 2 O hydrogen bonds 3. Br 2 dispersion 4. KCl ionic bonds 5. NH 3 hydrogen bonds 2013 Pearson Education, Inc. Chapter 5, Section 1 171

Chapter 5 Compounds and Their Bonds

Chapter 5 Compounds and Their Bonds General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds Electrons and Reactivity Atoms contain a very small nucleus packed with neutrons and positively

More information

Chapter 5 Compounds and Their Bonds

Chapter 5 Compounds and Their Bonds General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 5 Compounds and Their Bonds A closer look at bonding type the concept of electronegativity General Rules for Bond Type

More information

Chapter 4 Compounds and Their Bonds. Octet Rule. Metals Form Positive Ions. Ionic and Covalent Bonds. Formation of a Sodium Ion, Na +

Chapter 4 Compounds and Their Bonds. Octet Rule. Metals Form Positive Ions. Ionic and Covalent Bonds. Formation of a Sodium Ion, Na + Chapter 4 Compounds and Their Bonds Octet Rule 4.1 Octet Rule and Ions An octet Is 8 valence electrons. Is associated with the stability of the noble gases. Helium (He) is stable with 2 valence electrons

More information

Chemistry 51 Chapter 5 OCTET RULE & IONS

Chemistry 51 Chapter 5 OCTET RULE & IONS OCTET RULE & IONS Most elements, except noble gases, combine to form compounds. Compounds are the result of the formation of chemical bonds between two or more different elements. In the formation of a

More information

Metals with Variable Charge

Metals with Variable Charge Metals with Variable Charge Most transition metals (3-12) and Group 4A (14) metals form 2 or more positive ions, except Zn 2+, Ag +, and Cd 2+, which form only one ion. 2013 Pearson Education, Inc. Chapter

More information

Ionic and Molecular Compounds

Ionic and Molecular Compounds Ionic and Molecular Compounds Chapter 6 Ch. 6 Ionic and Molecular Compounds 6.1 Ions: Transfer of Electrons 6.2 Writing Formulas for Ionic Compounds 6.3 Naming and Writing Ionic Formulas 6.4 Polyatomic

More information

Ionic and Molecular Compounds

Ionic and Molecular Compounds Ionic and Molecular Compounds Chapter 6 Ch. 6 Ionic and Molecular Compounds 6.1 Ions: Transfer of Electrons 6.2 Writing Formulas for Ionic Compounds 6.3 Naming and Writing Ionic Formulas 6.4 Polyatomic

More information

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms, Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the

More information

Chapter 6 Inorganic and Organic Compounds: Names and Formulas

Chapter 6 Inorganic and Organic Compounds: Names and Formulas Chapter 6 Inorganic and Organic Compounds: Names and Formulas 6.1 Octet Rule and Ions 1 Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with

More information

IB Chemistry. Chapter 4.1

IB Chemistry. Chapter 4.1 IB Chemistry Chapter 4.1 Chemical Bonds Atoms or ions that are strongly attached to one another Chemical bonds will form if potential energy decreases (becomes more stable) 2 Valence Electrons Valence

More information

Bonding and structure: Forces Between Particles

Bonding and structure: Forces Between Particles Bonding and structure: Forces Between Particles NOBLE GAS CONFIGURATIONS An electronic configuration that is characterized by two electrons in the valence shell of helium and eight electrons in the valence

More information

Chapter 7. Ionic & Covalent Bonds

Chapter 7. Ionic & Covalent Bonds Chapter 7 Ionic & Covalent Bonds Ionic Compounds Covalent Compounds 7.1 EN difference and bond character >1.7 = ionic 0.4 1.7 = polar covalent 1.7 Electrons not shared at

More information

4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups.

4/25/2017. VSEPR Theory. Two Electron Groups. Shapes of Molecules. Two Electron Groups with Double Bonds. Three Electron Groups. Chapter 10 Lecture Chapter 10 Bonding and Properties of Solids and Liquids 10.3 Shapes of Molecules and Ions (VSEPR Theory) Learning Goal Predict the three-dimensional structure of a molecule or a polyatomic

More information

Naming Simple Compounds

Naming Simple Compounds Naming Simple Compounds Ionic Compounds Ionic compounds consist of positive and negative ions. have attractions called ionic bonds between positively and negatively charged ions. have high melting and

More information

Unit 4: Chemical Bonds. Chapter 7-9

Unit 4: Chemical Bonds. Chapter 7-9 Unit 4: Chemical Bonds Chapter 7-9 Objectives 26 Identify the number of valence electrons for elements and their Lewis dot structure 27 Define the terms cation and anion including radius size and charge

More information

Chemical Bonds. Chapter 6

Chemical Bonds. Chapter 6 Chemical Bonds Chapter 6 1 Ch. 6 Chemical Bonding I. How and Why Atoms Bond A. Vocabulary B. Chemical Bonds - Basics C. Chemical Bonds Types D. Chemical Bonds Covalent E. Drawing Lewis Diagrams F. Bond

More information

Gilbert Kirss Foster. Chapter 4. Chemical Bonding. Understanding Climate Change

Gilbert Kirss Foster. Chapter 4. Chemical Bonding. Understanding Climate Change Gilbert Kirss Foster Chapter 4 Chemical Bonding Understanding Climate Change Chapter Outline 4.1 Types of Chemical Bonds 4.2 Naming Compounds and Writing Formulas 4.3 Lewis Structures 4.4 Electronegativity,

More information

Chapter 8 Covalent Boding

Chapter 8 Covalent Boding Chapter 8 Covalent Boding Molecules & Molecular Compounds In nature, matter takes many forms. The noble gases exist as atoms. They are monatomic; monatomic they consist of single atoms. Hydrogen chloride

More information

Chapter 6. Preview. Objectives. Molecular Compounds

Chapter 6. Preview. Objectives. Molecular Compounds Section 2 Covalent Bonding and Molecular Compounds Preview Objectives Molecular Compounds Formation of a Covalent Bond Characteristics of the Covalent Bond The Octet Rule Electron-Dot Notation Lewis Structures

More information

CHAPTER 12 CHEMICAL BONDING

CHAPTER 12 CHEMICAL BONDING CHAPTER 12 CHEMICAL BONDING Core electrons are found close to the nucleus, whereas valence electrons are found in the most distant s and p energy subshells. The valence electrons are responsible for holding

More information

CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING

CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING CHAPTER 6: CHEMICAL NAMES AND FORMULAS CHAPTER 16: COVALENT BONDING 6.1 Introduction to Chemical Bonding A chemical bond is a mutual electrical attraction between the nuclei and valence electrons of different

More information

Chemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds

Chemical Bonding. Section 1 Introduction to Chemical Bonding. Section 2 Covalent Bonding and Molecular Compounds Chemical Bonding Table of Contents Section 1 Introduction to Chemical Bonding Section 2 Covalent Bonding and Molecular Compounds Section 3 Ionic Bonding and Ionic Compounds Section 4 Metallic Bonding Section

More information

NOTES: Unit 4: Bonding

NOTES: Unit 4: Bonding Name: Regents Chemistry: Mr. Palermo Student Version NOTES: Unit 4: Bonding Name: 1. Ion 2. Positive/Negative ion 3. Stable Octet 4. Diatomic Molecules 5. Electronegativity 6. Ionic Bond 7. Covalent Bond

More information

ELECTRONS. Construct your own electron dot diagram Choose one element & drag the correct number of VALENCE Br electrons around it.

ELECTRONS. Construct your own electron dot diagram Choose one element & drag the correct number of VALENCE Br electrons around it. Ch. 6 - Chemical Bonds Chemical reactivity depends on electron configuration. Remember the Stable Octet rule: when the highest energy level occupied is filled with electrons (8 electrons for most atoms),

More information

Lesson 1: Stability and Energy in Bonding Introduction

Lesson 1: Stability and Energy in Bonding Introduction Lesson 1: Stability and Energy in Bonding Introduction Chemical bonding is the simultaneous attraction of two positive nuclei to negative electrons. Chemical bonding is said to be the glue that holds particles

More information

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Sixth Edition by Charles H. Corwin Chapter 12 Chemical Bonding by Christopher Hamaker 2011 Pearson Education, Inc. Chapter 12 1 Chemical Bond Concept

More information

Chapter 6. Chemical Bonding

Chapter 6. Chemical Bonding Chapter 6 Chemical Bonding Section 6.1 Intro to Chemical Bonding 6.1 Objectives Define chemical bond. Explain why most atoms form chemical bonds. Describe ionic and covalent bonding. Explain why most chemical

More information

Ionic and Covalent Bonds

Ionic and Covalent Bonds Chapter 6 Lecture Chapter 6 Ionic and Molecular Compounds 6.1 Ions: Transfer of Electrons Learning Goal Write the symbols for the simple ions of the representative elements. Fifth Edition Octet Rule An

More information

Chapter 12. Chemical Bonding

Chapter 12. Chemical Bonding Chapter 12 Chemical Bonding Chemical Bond Concept Recall that an atom has core and valence electrons. Core electrons are found close to the nucleus. Valence electrons are found in the most distant s and

More information

Chapter 6: Ionic and Molecular Compounds

Chapter 6: Ionic and Molecular Compounds Chapter 6: Ionic and Molecular Compounds 1. Recall that the group number indicates the number of valence electrons for any element in that group. Each noble gas has eight valence electrons (except helium,

More information

Ionic and Covalent Compounds: Structures and Properties Examples of Lewis Dot Structures for the Representative Elements

Ionic and Covalent Compounds: Structures and Properties Examples of Lewis Dot Structures for the Representative Elements Ionic and Covalent Compounds: Structures and Properties Examples of Lewis Dot Structures for the Representative Elements Chemical bond: Attractive force between 2 atoms in a compound Lewis Dot Structure:

More information

Chapter 6. Ionic and Molecular Compounds. Lecture Presentation. Karen C. Timberlake Pearson Education, Inc.

Chapter 6. Ionic and Molecular Compounds. Lecture Presentation. Karen C. Timberlake Pearson Education, Inc. Lecture Presentation Chapter 6 Ionic and Molecular Compounds Chapter 6 Readiness Key Math Skills Using Positive and Negative Numbers in Calculations (1.4B) Solving Equations (1.4D) Core Chemistry Skills

More information

Chapter 4: Forces Between Particles

Chapter 4: Forces Between Particles Chapter 4: Forces Between Particles NOBLE GAS CONFIGURATIONS An electronic configuration that is characterized by two electrons in the valence shell of helium and eight electrons in the valence shell of

More information

Formula Writing. (nonmetals) METALS. oxidation number-number assigned to keep track of electron gain or loss. lose electron. gain electron anion

Formula Writing. (nonmetals) METALS. oxidation number-number assigned to keep track of electron gain or loss. lose electron. gain electron anion Formula Writing oxidation number-number assigned to keep track of electron gain or loss lose electron + cation METALS - gain electron anion (nonmetals) cation is written first anion is second positive

More information

CHAPTER 3 Ionic Compounds. General, Organic, & Biological Chemistry Janice Gorzynski Smith

CHAPTER 3 Ionic Compounds. General, Organic, & Biological Chemistry Janice Gorzynski Smith CHAPTER 3 Ionic Compounds General, Organic, & Biological Chemistry Janice Gorzynski Smith CHAPTER 3: Ionic Compounds Learning Objectives: q Octet Rule & Predicting ionic Charges q Ionic Bonds q Formation

More information

Ch 6 Chemical Bonding

Ch 6 Chemical Bonding Ch 6 Chemical Bonding What you should learn in this section (objectives): Define chemical bond Explain why most atoms form chemical bonds Describe ionic and covalent bonding Explain why most chemical bonding

More information

Unit 9: CHEMICAL BONDING

Unit 9: CHEMICAL BONDING Unit 9: CHEMICAL BONDING 1 Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to

More information

Chapter 6: Chemical Bonding

Chapter 6: Chemical Bonding Chapter 6: Chemical Bonding Learning Objectives Describe the formation of ions by electron loss/gain to obtain the electronic configuration of a noble gas. Describe the formation of ionic bonds between

More information

What is Bonding? The Octet Rule. Getting an Octet. Chemical Bonding and Molecular Shapes. (Chapter Three, Part Two)

What is Bonding? The Octet Rule. Getting an Octet. Chemical Bonding and Molecular Shapes. (Chapter Three, Part Two) Chemical Bonding and Molecular Shapes (Chapter Three, Part Two) What is Bonding? Bonding describes how atoms interact with each other in an attractive sense. There are three types of bonding: Ionic bonding

More information

Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons

Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent bonds there is a of electrons to get an

More information

Unit 9: CHEMICAL BONDING

Unit 9: CHEMICAL BONDING Unit 9: CHEMICAL BONDING 1 Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to

More information

Chemistry 101 Chapter 12 Chemical Bonding

Chemistry 101 Chapter 12 Chemical Bonding Chemistry 101 Chapter 12 Chemical Bonding Octet rule-duet role: when undergoing chemical reaction, atoms of group 1A-7A elements tend to gain, lose, or share sufficient electrons to achieve an electron

More information

Chapter 6. Preview. Lesson Starter Objectives Chemical Bond

Chapter 6. Preview. Lesson Starter Objectives Chemical Bond Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in

More information

Unit Six --- Ionic and Covalent Bonds

Unit Six --- Ionic and Covalent Bonds Unit Six --- Ionic and Covalent Bonds Electron Configuration in Ionic Bonding Ionic Bonds Bonding in Metals Valence Electrons Electrons in the highest occupied energy level of an element s atoms Examples

More information

Chapter 6. Preview. Lesson Starter Objectives Chemical Bond

Chapter 6. Preview. Lesson Starter Objectives Chemical Bond Preview Lesson Starter Objectives Chemical Bond Section 1 Introduction to Chemical Bonding Lesson Starter Imagine getting onto a crowded elevator. As people squeeze into the confined space, they come in

More information

CHM101 Lab Chemical Compounds Grading Rubric

CHM101 Lab Chemical Compounds Grading Rubric Name Team Name CHM101 Lab Chemical Compounds Grading Rubric To participate in this lab you must have splashproof goggles, proper shoes and attire. Criteria Points possible Points earned Lab Performance

More information

Solutions and Intermolecular Forces

Solutions and Intermolecular Forces Solutions and Intermolecular Forces REVIEW Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction between ions Covalent Sharing of electrons Metallic Metal atoms bonded to several other

More information

Chapter 7 Chemical Bonding

Chapter 7 Chemical Bonding Chapter 7 Chemical Bonding 7.1 Ionic Bonding Octet rule: In forming compounds atoms lose, gain or share electrons to attain a noble gas configuration with 8 electrons in their outer shell (s 2 p 6 ), except

More information

CHAPTER 12: CHEMICAL BONDING

CHAPTER 12: CHEMICAL BONDING CHAPTER 12: CHEMICAL BONDING Problems: 1-26, 27c, 28, 33-34, 35b, 36(a-c), 37(a,b,d), 38a, 39-40, 41-42(a,c), 43-58, 67-74 12.1 THE CHEMICAL BOND CONCEPT chemical bond: what holds atoms or ions together

More information

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES

More information

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share

More information

CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS

CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS CHEMICAL BONDING IONIC BONDS COVALENT BONDS HYDROGEN BONDS METALLIC BONDS IONIC BONDING When an atom of a nonmetal takes one or more electrons from an atom of a metal so both atoms end up with eight valence

More information

CP Covalent Bonds Ch. 8 &

CP Covalent Bonds Ch. 8 & CP Covalent Bonds Ch. 8 & 9 2015-2016 Why do atoms bond? Atoms want stability- to achieve a noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent

More information

Test Bank for Introductory Chemistry Essentials 5th Edition by Tro

Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Sample Introductory Chemistry, 5e (Tro) Chapter 10 Chemical Bonding 10.1 True/False Questions 1) Bonding theories are used to predict

More information

Types of bonding: OVERVIEW

Types of bonding: OVERVIEW 1 of 43 Boardworks Ltd 2009 Types of bonding: OVERVIEW 2 of 43 Boardworks Ltd 2009 There are three types of bond that can occur between atoms: an ionic bond occurs between a metal and non-metal atom (e.g.

More information

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin

INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Lecture INTRODUCTORY CHEMISTRY Concepts and Critical Thinking Seventh Edition by Charles H. Corwin Chemical Bonding by Christopher G. Hamaker Illinois State University Chemical Bond Concept Recall that

More information

Molecular Compounds Compounds that are bonded covalently (like in water, or carbon dioxide) are called molecular compounds

Molecular Compounds Compounds that are bonded covalently (like in water, or carbon dioxide) are called molecular compounds Chapter 8: Covalent Bonding Section 1: Molecular Compounds Bonds are Forces that hold groups of atoms together and make them function as a unit. Two types: Ionic bonds transfer of electrons (gained or

More information

He 1s 2 2 Ne 1s 2 2s 2 2p 6 8 = Ar 1s 2 2s 2 2p 6 3s 2 3p 6 8 = O 1s 2 2s 2 2p 4 6 = S 1s 2 2s 2 2p 6 3s 2 3p 4 6 = 2 + 4

He 1s 2 2 Ne 1s 2 2s 2 2p 6 8 = Ar 1s 2 2s 2 2p 6 3s 2 3p 6 8 = O 1s 2 2s 2 2p 4 6 = S 1s 2 2s 2 2p 6 3s 2 3p 4 6 = 2 + 4 Bonding is the joining of two atoms in a stable arrangement. CHAPTER 7: IONIC COMPOUNDS There are two different kinds of bonding: 1. Ionic bonds result from the transfer of electrons from one element to

More information

Chemical Bonding: Chemical Formulas HL

Chemical Bonding: Chemical Formulas HL Name: Chemical Bonding 5. Chemical Bonding: Chemical Formulas Ionic Bonding Covalent Bonding Electronegativity Shapes of Molecules and Intermolecular Forces Objectives -understand that compounds can be

More information

Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie

Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie Intramolecular Bonding Chapters 4, 12 Chemistry Mr. McKenzie What determines the type of intramolecular bond? An intramolecular bond is any force that holds two atoms together to form a compound; 3 types

More information

CHAPTER 8 Ionic and Metallic Bonds

CHAPTER 8 Ionic and Metallic Bonds CHAPTER 8 Ionic and Metallic Bonds Shows the kind of atoms and number of atoms in a compound. MgCl 2 NaCl CaCO 3 Al 2 O 3 Ca 3 (PO 4 ) 2 Chemical Formulas Al: Cl: counting atoms AlCl 3 Pb: N: O: Pb(NO

More information

Introduction to Chemical Bonding

Introduction to Chemical Bonding Chemical Bonding Introduction to Chemical Bonding Chemical bond! is a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together Why are most

More information

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons

Covalent Bonding. In nature, only the noble gas elements exist as uncombined atoms. All other elements need to lose or gain electrons In nature, only the noble gas elements exist as uncombined atoms. They are monatomic - consist of single atoms. All other elements need to lose or gain electrons To form ionic compounds Some elements share

More information

Chemical Nomenclature

Chemical Nomenclature Chemical Nomenclature Learn names you will Review: Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that

More information

Chapter 8 H H H H. Molecular Compounds & Covalent Bonding. Why do covalent bonds form? 8.1 Molecular Compounds. Properties of Molecular Compounds

Chapter 8 H H H H. Molecular Compounds & Covalent Bonding. Why do covalent bonds form? 8.1 Molecular Compounds. Properties of Molecular Compounds Chapter 8 Molecular Compounds & Covalent Bonding Why do covalent bonds form? If only group 5A, 6A, 7A atoms existed, ionic bonds can t form. NNMETALS Each atom needs electrons so they are not willing to

More information

Chemical Nomenclature Chapter 2.5-8

Chemical Nomenclature Chapter 2.5-8 Chemical Nomenclature Chapter 2.5-8 Octet Rule An octet is 8 valence electrons is associated with the stability of the noble gases does not occur with He, which is stable with two valence electrons (duet)

More information

Chemistry B11 Chapter 4 Chemical bonds

Chemistry B11 Chapter 4 Chemical bonds Chapter 4 Chemical bonds Octet rule: when undergoing chemical reaction, atoms of group 1A7A elements tend to gain, lose, or share sufficient electrons to achieve an electron configuration having eight

More information

UNIT 5.1. Types of bonds

UNIT 5.1. Types of bonds UNIT 5.1 Types of bonds REVIEW OF VALENCE ELECTRONS Valence electrons are electrons in the outmost shell (energy level). They are the electrons available for bonding. Group 1 (alkali metals) have 1 valence

More information

Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure

Cartoon courtesy of NearingZero.net. Chemical Bonding and Molecular Structure Cartoon courtesy of NearingZero.net Chemical Bonding and Molecular Structure Chemical Bonds Forces that hold groups of atoms together and make them function as a unit. 3 Major Types: Ionic bonds transfer

More information

Formation of Ions. Ions formed when atoms gain or lose valence e - to achieve a stable octet

Formation of Ions. Ions formed when atoms gain or lose valence e - to achieve a stable octet Ionic Bonding Formation of Ions Ions formed when atoms gain or lose valence e - to achieve a stable octet Cation Positively charged ion Forms when atom loses electrons Anion negatively charged ion Forms

More information

Unit 9: CHEMICAL BONDING

Unit 9: CHEMICAL BONDING Unit 9: CEMICAL BNDING Unit 9: Bonding: 1. Electronegativity 2. Intramolecular Bonding 3. Intermolecular Bonding 4. Drawing Lewis Structures 5. Lewis Structures for Polyatomic Ions 6. Exceptions to the

More information

Unit 5: Covalent Bonding and Acids

Unit 5: Covalent Bonding and Acids Unit 5: Covalent Bonding and Acids Bonds are Forces that hold groups of atoms together and make them function as a unit. Two types: 1) Ionic bonds transfer of electrons (gained or lost; makes formula unit)

More information

NOTES: UNIT 6: Bonding

NOTES: UNIT 6: Bonding Name: Regents Chemistry: Mr. Palermo NOTES: UNIT 6: Bonding www.mrpalermo.com Name: Key Ideas Compounds can be differentiated by their chemical and physical properties. (3.1dd) Two major categories of

More information

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H

More information

Naming Ionic Compounds with Two Elements

Naming Ionic Compounds with Two Elements Chapter 6 Lecture Chapter 6 Ionic and Molecular Compounds 6.3 Naming and Writing Ionic Compounds Fifth Edition Naming of Ionic Compounds In the name of an ionic compound, the positive ion (first ion) is

More information

CHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM)

CHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM) CHEMICAL BONDING [No one wants to be alone] The Marrying of Atoms (AIM) Associate Degree in Engineering Prepared by M. J. McNeil, MPhil. Department of Pure and Applied Sciences Portmore Community College

More information

CHEMISTRY Matter and Change Section 8.1 The Covalent Bond

CHEMISTRY Matter and Change Section 8.1 The Covalent Bond CHEMISTRY Matter and Change Section Chapter 8: Covalent Bonding CHAPTER 8 Table Of Contents Section 8.2 Section 8.3 Section 8.4 Section 8.5 Naming Molecules Molecular Structures Molecular Shapes Electronegativity

More information

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond

Bonding: Part Two. Three types of bonds: Ionic Bond. transfer valence e - Metallic bond. (NaCl) (Fe) mobile valence e - Covalent bond Bonding: Part Two Three types of bonds: Ionic Bond transfer valence e - Metallic bond mobile valence e - Covalent bond (NaCl) (Fe) shared valence e - (H 2 O) 1 Single Covalent Bond H + H H H H-atoms H

More information

Molecule 2 atoms chemically combined, smallest part of compound

Molecule 2 atoms chemically combined, smallest part of compound Chemical Bonds 008: Chemical Bonds Bonding: the way atoms are attracted to each other to form molecules, determines nearly all of the chemical properties we see. And, as we shall see, the number 8 is

More information

Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas.

Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. CHEMICAL BONDING Atoms have the ability to do two things in order to become isoelectronic with a Noble Gas. 1.Electrons can be from one atom to another forming. Positive ions (cations) are formed when

More information

THE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS

THE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS 1 THE ST. MICHAEL SCHOOL THIRD FORM CHEMISTRY MANUAL 3 SYMBOLS AND FORMULAE, CHEMICAL BONDING AND CHEMICAL EQUATIONS COMPILED BY G.WALKER, L.WORRELL, T. HARDING REFERENCE BOOKS Anne Tindale Chemistry A

More information

Ionic, Covalent, Metallic

Ionic, Covalent, Metallic Ionic, Covalent, Metallic Physical Properties of Types of Compounds IONIC COVALENT METALLIC Attractive/force strength Melting/Boiling point Strong Weak Varies High Low Varies Vapor pressure Low High Varies

More information

Scientists learned that elements in same group on PT react in a similar way. Why?

Scientists learned that elements in same group on PT react in a similar way. Why? Unit 5: Bonding Scientists learned that elements in same group on PT react in a similar way Why? They all have the same number of valence electrons.which are electrons in the highest occupied energy level

More information

Chemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together

Chemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together Chemical Bond An attraction between the nuclei and valence electrons of different atoms, which binds the atoms together When atoms form chemical bonds their valence electrons move around. This makes atoms

More information

Chapter 12 Structures and Characteristics of Bonds Objectives

Chapter 12 Structures and Characteristics of Bonds Objectives Objectives 1. To learn about ionic and covalent bonds and explain how they are formed - what holds compounds together? 2. To learn about the polar covalent bond are all covalent bonds equal? 3. To understand

More information

Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts

Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Name AP CHEM / / Chapter 8 Outline Bonding: General Concepts Types of Chemical Bonds Information about the strength of a bonding interaction is obtained by measuring the bond energy, which is the energy

More information

Outline Introduction: Multiple bonds, Bond. strength. Naming molecules Drawing Lewis Structures Molecular shapes and VSEPR theory Bond Polarity

Outline Introduction: Multiple bonds, Bond. strength. Naming molecules Drawing Lewis Structures Molecular shapes and VSEPR theory Bond Polarity Covalent Bonding Outline Introduction: Multiple bonds, Bond strength Naming molecules Drawing Lewis Structures Molecular shapes and VSEPR theory Bond Polarity Why do atoms bond? Recall that noble gases

More information

Bonding. Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms

Bonding. Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms Chemical Bonding Bonding Chemical Bond: mutual electrical attraction between nuclei and valence electrons of different atoms Type of bond depends on electron configuration and electronegativity Why do

More information

Unit 4. Bonding and Nomenclature

Unit 4. Bonding and Nomenclature Unit 4 Bonding and Nomenclature A. Vocabulary Chemical Bond attractive force between atoms or ions that binds them together as a unit bonds form in order to decrease potential energy (PE) increase stability

More information

Cartoon courtesy of NearingZero.net. Unit 3: Chemical Bonding and Molecular Structure

Cartoon courtesy of NearingZero.net. Unit 3: Chemical Bonding and Molecular Structure Cartoon courtesy of NearingZero.net Unit 3: Chemical Bonding and Molecular Structure Bonds Forces that hold groups of atoms together and make them function as a unit. Ionic bonds transfer of electrons

More information

Bonding Practice Problems

Bonding Practice Problems NAME 1. When compared to H 2 S, H 2 O has a higher 8. Given the Lewis electron-dot diagram: boiling point because H 2 O contains stronger metallic bonds covalent bonds ionic bonds hydrogen bonds 2. Which

More information

Science 1206 Ch. 3 - Chemical names, formulas and equations

Science 1206 Ch. 3 - Chemical names, formulas and equations Science 1206 Ch. 3 - Chemical names, formulas and equations 3.1 - Ionic and molecular compounds (pp. 98-107) Compounds A compound is a pure substance made of a combination of elements. The elements are

More information

Chemical bonding & structure

Chemical bonding & structure Chemical bonding & structure Ionic bonding and structure Covalent bonding Covalent structures Intermolecular forces Metallic bonding Ms. Thompson - SL Chemistry Wooster High School Topic 4.1 Ionic bonding

More information

Honors Chemistry - Unit 9 Chapter 6: Bonding & Molecular Structures. Unit 9 Packet Page 1 of 14

Honors Chemistry - Unit 9 Chapter 6: Bonding & Molecular Structures. Unit 9 Packet Page 1 of 14 Honors Chemistry - Unit 9 Chapter 6: Bonding & Molecular Structures Unit 9 Packet Page 1 of 14 Vocab Quiz: UT Due: Test Date: Quiz Date(s): FORMULAS/CONSTANTS Memorize VSEPR Chart First 6 Shapes!! OBJECTIVES:

More information

Intermolecular Forces, Liquids, & Solids

Intermolecular Forces, Liquids, & Solids , Liquids, & Solids Mr. Matthew Totaro Legacy High School AP Chemistry States of Matter The fundamental difference between states of matter is the distance between particles. States of Matter Because in

More information

CHEM 121 Introduction to Fundamental Chemistry. Summer Quarter 2008 SCCC. Lecture 5.

CHEM 121 Introduction to Fundamental Chemistry. Summer Quarter 2008 SCCC. Lecture 5. CHEM 121 Introduction to Fundamental Chemistry Summer Quarter 2008 SCCC Lecture 5 http://seattlecentral.edu/faculty/lcwest/che121 Forces Between Particles Noble Gas Configurations Ionic Bonding Ionic Compounds

More information

Noble Gas Configuration What they noticed is that all the noble gases have the same number of electrons in their valence shell.

Noble Gas Configuration What they noticed is that all the noble gases have the same number of electrons in their valence shell. Chem101 - Lecture 4 Forces Between Particles Forces between Particles The chemical and physical properties of matter result from interactions that take place between their constituent particles, i.e. their

More information

Structure and IM Forces Practice Problems

Structure and IM Forces Practice Problems Structure and IM Forces Practice Problems 1) An ionic compound 1) A) hasa net positive charge. B) hasa net negative charge. C) contains only cations. D) contains covalent bonds between anions and cations.

More information

Chem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept

Chem 1075 Chapter 12 Chemical Bonding Lecture Outline. Chemical Bond Concept Chem 1075 Chapter 12 Chemical Bonding Lecture Outline Slide 2 Chemical Bond Concept Recall that an atom has and electrons. Core electrons are found to the nucleus. Valence electrons are found in the s

More information

Ionic and Covalent Bonding

Ionic and Covalent Bonding 1. Define the following terms: a) valence electrons Ionic and Covalent Bonding the electrons in the highest occupied energy level always electrons in the s and p orbitals maximum of 8 valence electrons

More information