CHAPTER 3 CHEMICAL BONDING NUR FATHIN SUHANA BT AYOB SMK SULTAN ISMAIL, JB
|
|
- Betty Turner
- 5 years ago
- Views:
Transcription
1 CHAPTER 3 CHEMICAL BONDING NUR FATHIN SUHANA BT AYOB SMK SULTAN ISMAIL, JB
2 LEARNING OUTCOMES (ionic bonding) 1. Describe ionic (electrovalent) bonding such as NaCl and MgCl 2
3 LEARNING OUTCOMES (metallic bonding) 1. Explain metallic bonding in terms of electron sea model
4 LEARNING OUTCOMES (intermolecular forces : van der Waals forces and hydrogen bonding) 1. Describe the hydrogen bonding and van der Waals forces (permanent, temporary and induced dipole) 2. Deduce the effect of van der Waals between molecules on the physical properties of substances 3. Deduce the effect of hydrogen bonding (intermolecular and intramolecular)on the physical properties of substances
5 TYPES OF CHEMICAL BONDING 1. Metal and non-metal : Electron transfer and ionic bonding Metal atom (low IE) loses its valence electrons, non metal (high negative EA) gains electrons 2. Non-metal with non-metal : Electron sharing and covalent bonding A shared electron pair is considered to be localized between the two atoms 3. Metal with metal : Electron pooling and metallic bonding Electron sea model
6 Subtopic 4.1 LEWIS STRUCTURE
7 LEWIS SYMBOLS 1. When atoms react to form chemical bonds, only the electrons in the outermost valence shells are involved 2. Valence shell electrons of an atom represented either by cross ( X ) or a dot ( ) 3. It known as Lewis structures or electron-dot structures 4. E.g
8 LEWIS SYMBOLS
9 RELATIONSHIP BETWEEN GROUP AND VALENCE ELECTRON Group no. Example Electronic configuration 1 Sodium Lewis diagram 2 Magnesium 13 Aluminium 14 Silicon 15 Phosphorus 16 Sulphur 17 Chlorine 18 Argon
10 HOW TO WRITE LEWIS SYMBOL Eg. N (Z = 7) Electron configuration : 1s 2 2s 2 2p 3 (valence electron = 5) 1. Identify no. of valence electron 2. Place one dot at a time on the four side (top, bottom, right, left) 3. Pair up the dots until all are used
11 KEEP IN MIND! 1. Lewis symbols do not show the electron configuration of the valence electron 2. E.g C (Z =6) Electron configuration : 1s 2 2s 2 2p 2 3. C has 4 unpaired dots because it form 4 bonds
12 KEEP IN MIND! 4. Element in the same group : Similar valence electron configuration Similar Lewis dot symbols 5. E.g. N gains three electron to form N 3 (-3 charge) N can form three covalent bonds Cl gains one electron to form Cl (-1 charge) Cl can form one covalent bond
13 LEWIS SYMBOL EXERCISE 1 Write Lewis dot symbols for the following atoms: (a) K (b) Ca (c) Be (d) Ga (e) O (f) Br (g) N (h) I (i) As (j) F (k) Mg (l) S
14 LEWIS SYMBOL EXERCISE 2 Write Lewis dot symbols for the species according to the following electronic configuration: (a)p : 1s 2 2s 2 2p 6 3s 1 (b) Q : 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 (c) R : 1s 2 2s 2 2p 6 3s 2 3p 4 (d) S : 1s 2 2s 2 2p 3 (e) T : 1s 2 2s 2 2p 1 (f) U : 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 (g) V : 1s 2 2s 2 2p 6 3s 2 3p 2 (h) W : 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 5 14
15 OCTET RULE 1. An atom other than H tends to form bonds (by losing or gaining or sharing electron) until it is surrounded by eight valence electron 2. It can be achieved by ; E.g : Transfer of electrons Li (Z=3) + F (Z =9) 1s 2 2s 1 1s 2 2s 2 2p 5 Li + F 1s 2 1s 2 2s 2 2p 6
16 OCTET RULE E.g. sharing of electron
17 ELECTRON CONFIGURATION OF IONS Noble gas configuration ( 8 valence electron) Eg. 1s 2 2s 2 2p 6 (Ne) Pseudonoble gas configuration eg. [Kr] 4d 10 Half-filled orbitals e.g 3d 5
18 STABILITIES OF IONS Form stable ions (duplet/octet) Noble Gas Configuration Valence electronic configuration: ns 2 np 6 Example: 1) Na Na + + e - 1s 2 2s 2 2p 6 3s 1 2) F + e - F - 1s 2 2s 2 2p 5 18
19 NOBLE GAS CONFIGURATION 1. Atoms may lose or gain enough electron so as to forms stable ion with octet (or duplet) configuration (ns 2 np 6 ) 2. Eg. Na Na + + e 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 = [Ne] + e 1s 2 2s 2 2p 6 3s 2 3p 5 1s 2 2s 2 2p 6 3s 2 3p 6 = [Ar]
20 STABILITIES OF IONS A completely filled orbital but not the noble gas configuration Pseudo Noble Gas Configuration Example: Valence electronic configuration: ns 2 np 6 nd 10 or ns 2 np 6 nd 10 nf 14 1) 31 Ga : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 1 Ga 3+ : 2) 29 Cu : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 1 Cu + : 1 20
21 PSEUDO-NOBLE GAS CONFIGURATION 1. The (n-1) d 10 configuration of a p-block metal atom that empties its outer level 2. Eg. Sn 4+ + e [Kr] 4d 10 5s 2 5p 2 [Kr] 4d 10 Zn : 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 Zn 2+ : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 (pseudonoble gas configuration )
22 STABILITIES OF IONS A special stability of half-filled d orbital Half-filled Orbital Configuration Example: Valence electronic configuration: nd 5 1) 25 Mn : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2 Mn 2+ : 2) 26 Fe : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 6 4s 2 Fe 3+ : 22
23 HALF-FILLED ORBITALS 1. Some transition metal atoms form cations that have electron configuration associated with half-filled d orbital (d 5 ) 2. E.g. Mn Mn 2+ 2e [Ar] 3d 5 4s 2 [Ar] 3d 5 Fe : 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 6 Fe 3+ : 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 (stability of half-filled 3d orbital)
24 IONIC BONDING Electron transfer theory Strength of ionic bond Properties of ionic compound
25 IONIC BONDING 1. Attractive electrostatic force between positive and negative ions 2. Sometimes called : electrovalent bond 3. Ionic bonds are usually formed between metallic elements (Group 1, 2 and 13) and non-metallic elements (Group 15,16 and 17)
26 IONIC BONDING Metal atom (more electropositive) Non-metal atom (more electronegative)
27 FORMATION OF IONIC BONDS 1. By transferring electrons 2. Total number of electron lost by metal atoms = total number of electron gained by the nonmetal atoms 3. E.g. Li Li + + e ******************************************
28 HOW TO SHOW ELECTRON TRANSFER 1. Three ways : a. Electron configurations Eg. Li + F 1s 2 2s 1 1s 2 2s 2 2p 5 Li + 1s 2 F 1s 2 2s 2 2p 6
29 HOW TO SHOW ELECTRON TRANSFER 1. Three ways : b. Orbital diagram Eg. Li + F Li + F
30 HOW TO SHOW ELECTRON TRANSFER 1. Three ways : b. Lewis e-dot symnbol Eg. LiF + F [Li] + [ F ] -
31 Exercises 3: By using Lewis structure, show how the ionic bond is formed in the compounds below. ( a ) KF ( b ) BaO ( c ) Na 2 O
32 LEWIS SYMBOL EXERCISE 4 The element X has one electron and the element Y has six electrons in their outermost shell respectively. (a) (b) (c) What is the formula of the compound formed between the elements X and Y? Name the type of bond formed in (a) Draw the Lewis structure to show the formation of compound in (a) 32
33 Ionic bond is very strong, therefore ionic compounds: 1. Have very high melting and boiling points 2. Hard and brittle 3. Can conduct electricity when they are in molten form or aqueous solution because of the mobile ions
34 LEWIS STRUCTURE 1. Two dimensional structural formula consists of e-dot symbols that show each atom and its neighbors, the bonding pairs and the lone pairs that fill each atom s outer shell 2. E.g
35 WRITING LEWIS STRUCTURE 1. Step 1 Draw skeletal structure of compound showing what atoms are bonded to each other Put at least negative electron negative atom in the center F E.g F N F Electronegativity N = 3.0 F = 4.0 N = Central atom F = Surrounding atom
36 WRITING LEWIS STRUCTURE 2. Step 2 : Count total no. of valence electrons E.g. NF 3 F F N F Atom N X 1 F X 3 Total No. of valence electron 5e x 1 = 5e 7e x 3 = 21e 26 e
37 WRITING LEWIS STRUCTURE 2. Step 2 : For polynomials ions, add one electron for negative charge of the ion, or subtract one electron for each positive charge E.g NH 4 + Atom No. of valence electron N X 1 5e x 1 = 5e H X 4 1e x 4 = 4e + 1 charge 1e Total 8 e
38 WRITING LEWIS STRUCTURE 3. Step 3 : complete an octet (8 e ) for all atoms except H (2 e ) Complete the surrounding atoms first electrons not involved in bonding shown as lone pairs E.g Check : 8 e x 3 = 24 e + 2 e 26 e
39 DRAWING LEWIS STRUCTURE CH 4 1 Determine central atom & count valence e - Central atom : 2 Draw single bond & calculate the non-bonding e - (NBe - ) 3 Complete the octet of the terminal atom 4 Place any remaining e - at the central atom 5 Form double or triple bond if octet rule is not satisfied 39
40 DRAWING LEWIS STRUCTURE NO Determine central atom & count valence e - Central atom : 2 Draw single bond & calculate the nonbonding e - (NBe - ) 3 Complete the octet of the terminal atom 4 Place any remaining e - at the central atom 5 Form double or triple bond if octet rule is not satisfied
41 WRITING LEWIS STRUCTURE 4. Step 4 : If a central atom does have an octet, make a multiple bond by changing a lone pair from one of the surrounding atoms into a bonding pair to the central atom. E.g N = N N N
42 STRENGTH OF IONIC BONDS 1. The strength of an ionic bond is a measure of the electrostatic attraction between the ions 2. F Q+ Q d 2 Q + = charge + ve ion Q = charge ve ion d = distance between the ions F = force of attraction 3. The smaller the ions and/or the higher charge on ions > the stronger attraction between ions > the stronger the ionic bond 4. E.g Compound NaCl NaBr Melting point/
43 STRENGTH OF IONIC BONDS 4. The melting point of sodium chloride is higher than that of sodium bromide. This shows that the ionic bond in NaCl is stronger than that in NaBr 5. This is because the Cl ion is smaller than that of Br ion Ion Na + Cl Br Ionic radius/nm Electrostatic attraction between Na + and Cl is stronger.
44 STRENGTH OF IONIC BONDS 1. The melting point of sodium chloride and magnesium chloride are : Compound NaCl MgCl 2 Melting point/ Cation radius/nm The Mg 2+ ion is smaller in size than in Na + ion. On top of that, Mg 2+ has higher charge 3. As a result, the ionic bond in MgCl 2 is stronger than that in NaCl. This accounts for the higher melting of MgCl 2.
45 BOND LENGTH 2. For a given pair of atoms, Bond length : single > double > triple E.g. C C > C = C > C C (154 pm) (134 pm) (121 pm) Bond order increase Stronger bond Shorter bond As the number of bonds between the carbon increase, the bond length decreases because C are held more closely and tightly together As the number of bonds between two atoms increases, the bond grows shorter and stronger * Lebih panjang > lebih mudah break
46 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to the octet rule such as BF 3, NO, NO 2, PCl 5, SF 6 ) 2. Explain the concept of overlapping and hybridisation of the s and p orbitals such as BeCl 2, BF 3, CH 4, N 2, HCN, NH 3, H 2 O molecules 3. Predict and explain the shapes of and bond angles in molecules and ions using the principle of valence valence shell electron pair repulsion, e.g. linear, trigonal planar, tetrahedral, trigonal bipyramid, octahedral, v-shaped, seesaw and pyramidal 4. Explain the existence of polar and non-polar bonds (including C- Cl, C-N, C-O, C-Mg) resulting in polar or/and non-polar molecules
47 LEARNING OUTCOMES (covalent bonding) 5. Relate bond lengths and bond strengths with respect to single, double and triple bonds 6. Explain the inertness of nitrogen molecule in terms of its strong triple bond and nonpolarity 7. Describe typical properties associated with ionic and covalent bonding in terms of bond strength, melting point and electrical conductivity 8. Explain the existence of covalent character in ionic compounds such as Al 2 O 3, All 3, and Lil 9. Explain the existence of coordinate (dative covalent) bonding such as H 3 O +, NH 4 +, Al 2 Cl 6, and [Fe (CN) 6 ]³ˉ
48 COVALENT BOND 1. Covalent bond is force of attraction between two adjacent nuclei and the electrons that are shared together between them 2. The covalent bond is usually formed between non-metallic elements 3. There are some exceptions. For example, beryllium and aluminium are metals, but they form covalent bonds with chlorine. E.g. BeCl 2, AlCl 3
49 COVALENT BOND Bonding pair electron Lone pair electron
50 Covalent compounds: Compounds may have these covalent bonds: i. Single bond ii. Double bond iii. Triple bond.
51 Lewis structure of water H + O + H H O H 2e - 8e - 2e - or single covalent bonds H O H
52 Double bond two atoms share two pairs of electrons O C O or O C O 8e - 8e - 8e - double bonds double bonds
53 Triple bond two atoms share three pairs of electrons N N or N N 8e - 8e - triple bond triple bond
54 RESONANCE STRUCTURE 1. Two or more Lewis structure for a single molecule that cannot be represented accurately by only one Lewis structure 2. E.g. Ozone (O 3 ) 6 e X 3 = 18e
55 FORMAL CHARGE 1. Difference between the valence electron in an isolated atom and the number of electron assigned to that atom in a Lewis structure 2. Formal charge of atom : No. of valence electron [ No. of lone pair electron + half of bonding electron] No. of valence electron [ No. of lone pair electron + No. of bonds]
56 FORMAL CHARGE Negative FC -- on more electronegative atom Positive FC -- on more electropositive atom FORMAL CHARGE (FC) Is used to find the most stable Lewis structure The sum of the FC of the atoms must equal the charge on the molecule or ion FC should be as small as possible 56
57 FORMAL CHARGE 1. Formal charge : O of O O = = 1 : O of O = O = = 0 : middle O = [6 2 3 ] =
58 SELECTING THE BEST RESONANCE STRUCTURE 1. Select the structure with : All zero formal charge Small formal charge Negative formal charges are placed on the more electronegative atoms
59 EXAMPLE Calculate the formal charge for each atom of the following compounds: (a) H I H C H I H (b) H N H I H (c) H O H (d) O O O (e) O S O (f) O N O O - 59
60 EXAMPLE 1) Draw all the possible Lewis structure of COCl 2. 2) Predict the most plausible structure.
61 SOLUTION 1) 2) The most plausible structure is (2) Formal charge is determined before completing a Lewis structure to predict the most stable structure because formal charge closest to zero.
62 EXCEPTION TO OCTET RULE 1. Molecular species that do not follow the octet rule fall under two categories ; Molecules in which atom has less than an octet (Incomplete octet) Molecules with an odd number of electrons Molecules in which an atom has more than an octet (Expanded octet)
63 EXCEPTION TO OCTET RULE 1. Incomplete octet: Electron - deficient molecules The central atoms have fewer than eight electrons around them E.g BeH 2 H Be H Be 2H Total *Be, B, Al incomplete 1 X 2e = 2e 2 x 1e = 2e 4e Other examples : BeCl 2, BCl 3, BF 3
64 EXCEPTION TO OCTET RULE 2. Odd electron molecules : free radicals Contain an unpaired electron The central atoms have fewer than eight electrons around them E.g NO N O Total 1 X 5e = 5e 1 x 6e = 6e 11e Most odd electrons molecules have a central atom from an-odd numbered group, such as N (Group 15) and Cl (Group 17) Other example : NO 2
65 EXCEPTION TO OCTET RULE 3. Expanded octet Central atoms have more than eight electrons around them Central atoms are normally elements of Period 3 or higher : d orbital available E.g SF 6 S F Total 1 X 6e = 6e 6 x 7e = 42e 48e Other examples : PCl 5, SO 4 2
66 EXERCISE Draw the Lewis structure of the following molecules and state the special features at the central atoms. (a) NO (b) TeCl 4 (c) AlBr 3 (d) XeF 2 66
67 Coordinate Covalent Bond (Dative Bond) 1. Coordinate bond is formed when one of the atom donates both electron (lone pair electron) 2. Known as dative covalent bond or dative bond 3. The atom contributes two electrons to form the coordinate bond is called the donor atom. 4. The atom which accepts the electron pair from the donor atom is called the acceptor atom
68 Coordinate Covalent Bond (Dative Bond) Example 1 : 1. Ammonium ion, NH The nitrogen atom in an ammonia molecules has a lone pair of electrons 3. Thus, the nitrogen atom can act as a donor atom. In contrast, the hydrogen ion has an empty 1s orbital. Thus, hydrogen ion (H + ) can act as an acceptor atom. 4. The formation of a coordinate bond in the ammonium ion can be represented by Lewis structure as follows: H H H N H + H + H N H H +
69 : : Coordinate Covalent Bond (Dative Bond) Example 2: 1. Oxonium ion, H 3 O + 2. The oxygen atom in the water molecule has two lone pairs of electrons. 3. An oxonium ion is formed when one of the lone pairs of electrons is used to form a coordinate bond with a hydrogen ion. 4. The oxonium ion is called the hydroxonium ion or the hydronium ion H H O O + H + H H H +
Subtopic 4.2 MOLECULAR SHAPE AND POLARITY
Subtopic 4.2 MOLECULAR SHAPE AND POLARITY 1 LEARNING OUTCOMES (covalent bonding) 1. Draw the Lewis structure of covalent molecules (octet rule such as NH 3, CCl 4, H 2 O, CO 2, N 2 O 4, and exception to
More informationChapter 7 Chemical Bonding and Molecular Structure
Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal
More informationChapter 7. Chemical Bonding I: Basic Concepts
Chapter 7. Chemical Bonding I: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationSMK SULTAN ISMAIL JB, NUR FATHIN SUHANA BT AYOB
SMK SULTAN ISMAIL JB, NUR FATHIN SUHANA BT AYOB POLAR AND NON POLAR BONDS BOND POLARITY 1. Atoms with different electronegative from polar bonds (difference in EN) 2. Depicted as polar arrow : 3. Example
More informationCHAPTER 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 informationEdexcel Chemistry A-level
Edexcel Chemistry A-level Topic 2 - Bonding and Structure Flashcards What are ions? What are ions? Charged particles that is formed when an atom loses or gains electrons What is the charge of the ion when
More informationCh 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 informationUnit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules
Unit 1 Module 1 Forces of Attraction page 1 of 10 Various forces of attraction between molecules 1. Ionic bonds 2. Covalent bonds (also co-ordinate covalent bonds) 3. Metallic bonds 4. Van der Waals forces
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 7 CHEMICAL BONDING & MOLECULAR STRUCTURE The Ionic Bond Formation of Ions The
More informationChapter 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 informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8. Basic Concepts of Chemical Bonding 8.1 Lewis Symbols and the Octet Rule When atoms or ions are strongly attracted to one another, we say that there is a chemical bond between them. In chemical
More informationCHEMICAL BONDING. Chemical bond is the force which holds two or more atoms or ions together in a stable molecule.
SN Kansagra School CHEMISTRY CHAPTER - 2 CHEMICAL BONDING STD. X Chemical bond is the force which holds two or more atoms or ions together in a stable molecule. AN ATOM An atom is the smallest unit of
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationChapter 8. Chemical Bonding: Basic Concepts
Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely
More informationChemical Bonding Basic Concepts
Chemical Bonding Basic Concepts Valence electrons are the outer shell electrons of an atom. The valence electrons are the electrons that particpate in chemical bonding. Group e - configuration # of valence
More informationChemical Bonding AP Chemistry Ms. Grobsky
Chemical Bonding AP Chemistry Ms. Grobsky What Determines the Type of Bonding in Any Substance? Why do Atoms Bond? The key to answering the first question are found in the electronic structure of the atoms
More informationClass XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry
Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents
More informationClass XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry
Class XI Chapter 4 Chemical Bonding and Molecular Structure Chemistry Question 4.1: Explain the formation of a chemical bond. A chemical bond is defined as an attractive force that holds the constituents
More informationChapter 6 Chemical Bonding
Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between
More informationIts Bonding Time. Chemical Bonds CH 12
Its Bonding Time Chemical Bonds CH 12 What is a chemical bond? Octet Rule: Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its
More informationChapter 8: Concepts of Chemical Bonding
Chapter 8: Concepts of Chemical Bonding Learning Outcomes: Write Lewis symbols for atoms and ions. Define lattice energy and be able to arrange compounds in order of increasing lattice energy based on
More informationChapter 8 The Concept of the Chemical Bond
Chapter 8 The Concept of the Chemical Bond Three basic types of bonds: Ionic - Electrostatic attraction between ions (NaCl) Metallic - Metal atoms bonded to each other Covalent - Sharing of electrons Ionic
More informationSTD-XI-Science-Chemistry Chemical Bonding & Molecular structure
STD-XI-Science-Chemistry Chemical Bonding & Molecular structure Chemical Bonding Question 1 What is meant by the term chemical bond? How does Kessel-Lewis approach of bonding differ from the modern views?
More informationClass XI: Chemistry Chapter 4: Chemical Bonding and Molecular Structure Top Concepts
1 Class XI: Chemistry Chapter 4: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical species
More informationUnit 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 informationIB Topics 4 & 14 Multiple Choice Practice
IB Topics 4 & 14 Multiple Choice Practice 1. Which compound has the shortest C N bond? CH 3NH 2 (CH 3) 3CNH 2 CH 3CN CH 3CHNH 2. Which of the following series shows increasing hydrogen bonding with water?
More informationCHEMICAL 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 informationSL Score. HL Score ! /30 ! /48. Practice Exam: Paper 1 Topic 4: Bonding. Name
Name Practice Exam: Paper 1 Topic 4: Bonding SL SL Score! /30 HL Score! /48 1. What is the correct Lewis structure for hypochlorous acid, a compound containing chlorine, hydrogen and oxygen? A. B. C. D.
More informationDownloaded from
Points to Remember Class: XI Chapter Name: Chemical Bonding and Molecular Structure Top Concepts 1. The attractive force which holds together the constituent particles (atoms, ions or molecules) in chemical
More informationCh 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 informationAll chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table
UNIT VIII ATOMS AND THE PERIODIC TABLE 25 E. Chemical Bonding 1. An ELECTROSTATIC FORCE is All chemical bonding is based on the following relationships of electrostatics: The greater the distance between
More informationAtoms 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 informationFill in the chart below to determine the valence electrons of elements 3-10
Chemistry 11 Atomic Theory IV Name: Date: Block: 1. Lewis Diagrams 2. VSEPR Lewis Diagrams Lewis diagrams show the bonding between atoms of a molecule. Only the outermost electrons of an atom (called electrons)
More informationUnit 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 informationUnit 3 - Chemical Bonding and Molecular Structure
Unit 3 - Chemical Bonding and Molecular Structure Chemical bond - A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together 6-1 Introduction
More informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds An attractive force that holds two atoms together in a more complex unit Three basic types of bonds Ionic Electrons are transferred from one
More informationBonding: 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 informationBonding 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 informationChemistry I Chemical Bonding / Molecular Geometry / Intermolecular Forces Lecture Notes
Chemistry I Chemical Bonding / Molecular Geometry / Intermolecular Forces Lecture Notes Since most elements do not have a filled outer shell, they attempt to achieve an octet arrangement by combining with
More informationChapter 9 Ionic and Covalent Bonding
Chem 1045 Prof George W.J. Kenney, Jr General Chemistry by Ebbing and Gammon, 8th Edition Last Update: 06-April-2009 Chapter 9 Ionic and Covalent Bonding These Notes are to SUPPLIMENT the Text, They do
More informationBonding: 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 informationCHEMICAL BONDING. Valence Electrons. Chapter Ten
CHEMICAL BONDING Chapter Ten Valence Electrons! The electrons occupying the outermost energy level of an atom are called the valence electrons; all other electrons are called the core electrons.! The valence
More informationChemical 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 informationUnit 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 informationUnit 7: Basic Concepts of Chemical Bonding. Chemical Bonds. Lewis Symbols. The Octet Rule. Transition Metal Ions. Ionic Bonding 11/17/15
Unit 7: Basic Concepts of Chemical Bonding Topics Covered Chemical bonds Ionic bonds Covalent bonds Bond polarity and electronegativity Lewis structures Exceptions to the octet rule Strength of covalent
More informationChapter 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 informationAP Chemistry. Unit #7. Chemical Bonding & Molecular Shape. Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING. Discrete molecules formed
AP Chemistry Unit #7 Chemical Bonding & Molecular Shape Zumdahl Chapters 8 & 9 TYPES OF BONDING BONDING INTRA (Within (inside) compounds) STRONG INTER (Interactions between the molecules of a compound)
More informationCHAPTER 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 informationEnd of chapter exercises
End of chapter exercises Problem 1: Give one word/term for each of the following descriptions. 1. The distance between two adjacent atoms in a molecule. 2. A type of chemical bond that involves the sharing
More informationName Date Class MOLECULAR COMPOUNDS. Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides
8.1 MOLECULAR COMPOUNDS Section Review Objectives Distinguish molecular compounds from ionic compounds Identify the information a molecular formula provides Vocabulary covalent bond molecule diatomic molecule
More informationChapter 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 informationTest Review # 4. Chemistry: Form TR4.11A
Chemistry: Form TR4.11 REVIEW Name Date Period Test Review # 4 Bonding. The electrons of one atom are attracted to the protons of another. When atoms combine, there is a tug of war over the valence electrons.
More informationLesson 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 information2011, Robert Ayton. All rights reserved.
Chemical Bonding Outline 1. Lewis Dot Structures 2. Bonds 3. Formal Charges 4. VSEPR (Molecular Geometry and Hybridzation) 5. Common Resonance Structures and Dimerization Review 1. Lewis Dot Structures
More informationREVIEW: VALENCE ELECTRONS CHEMICAL BONDS: LEWIS SYMBOLS: CHEMICAL BONDING. What are valence electrons?
REVIEW: VALENCE ELECTRONS 13 CHEMICAL BONDING What are valence electrons? Which groups on the periodic table readily give up electrons? What group readily accepts electrons? CHEMICAL BONDS: What are chemical
More informationElectrons and Molecular Forces
Electrons and Molecular Forces Chemistry 30 Ms. Hayduk Electron Configuration Atomic Structure Atomic Number Number of protons in the nucleus Defines the element Used to organize the periodic table 1 Bohr
More informationEx. 1) F F bond in F = 0 < % covalent, no transfer of electrons
#60 Notes Unit 8: Bonding Ch. Bonding I. Bond Character Bonds are usually combinations of ionic and covalent character. The electronegativity difference is used to determine a bond s character. Electronegativity
More informationCovalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B
Covalent Bonding 1. Obtain the number of valence electrons for each of the following atoms from its group number and draw the correct Electron Dot Notation (a.k.a. Lewis Dot Structures). a. K b. N c. Cl
More informationFor more info visit Chemical bond is the attractive force which holds various constituents together in a molecule.
Chemical bond:- Chemical bond is the attractive force which holds various constituents together in a molecule. There are three types of chemical bonds: Ionic Bond, Covalent Bond, Coordinate Bond. Octet
More informationName 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 informationChemical Bonding Chapter 8
Chemical Bonding Chapter 8 Get your Clicker, 2 magnets, goggles and your handouts Nov 15 6:15 PM Recall that: Ionic-Involves the transfer of electrons - forms between a metal and a nonmetal Covalent-Involves
More informationCHEMISTRY XL-14A CHEMICAL BONDS
CHEMISTRY XL-14A CHEMICAL BONDS July 16, 2011 Robert Iafe Office Hours 2 July 18-July 22 Monday: 2:00pm in Room MS-B 3114 Tuesday-Thursday: 3:00pm in Room MS-B 3114 Chapter 2 Overview 3 Ionic Bonds Covalent
More informationChapter 8: Bonding. Section 8.1: Lewis Dot Symbols
Chapter 8: Bonding Section 8.1: Lewis Dot Symbols The Lewis electron dot symbol is named after Gilbert Lewis. In the Lewis dot symbol, the element symbol represents the nucleus and the inner electrons.
More informationCHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols
CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen
More informationNa Cl Wants to lose ONE electron! Na Cl Ionic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding.
BONDING Chemical Bond Attraction that holds atoms together Types include IONIC, METALLIC, or COVALENT Differences in electronegativity determine the bond type Ionic Bond TRANSFER of electrons between atoms
More informationCHAPTER-4 CHEMICAL BONDING AND MOLECULAR STRUCTURE
CHAPTER-4 CHEMICAL BONDING AND MOLECULAR STRUCTURE OCTET RULE- During a chemical reaction the atoms tend to adjust their electronic arrangement in such a way that they achieve 8 e - in their outermost
More informationChapter 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 informationBonding. Honors Chemistry 412 Chapter 6
Bonding Honors Chemistry 412 Chapter 6 Chemical Bond Mutual attraction between the nuclei and valence electrons of different atoms that binds them together. Types of Bonds Ionic Bonds Force of attraction
More informationChapter 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 informationCHAPTER 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 information1. What is the formula for the compound formed by calcium and nitrogen?
IB Chem 1 Name Topic 4 Bonding - Sample Test Problems 1. What is the formula for the compound formed by calcium and nitrogen? A. CaN B. Ca 2 N C. Ca 2 N 3 D. Ca 3 N 2 2. Element X is in group 2, and element
More informationAS91164 Bonding, structure, properties and energychanges Level 2 Credits 5
AS91164 Bonding, structure, properties and energychanges Level 2 Credits 5 LEWIS DIAGRAMS, SHAPES OF MOLECULES, POLAR AND NON POLAR MOLECULES Lewis diagrams: use dots (or x) to represent electrons, show
More informationDownloaded from
CHAPTER-4 CHEMICAL BONDING AND MOLECULAR STRUCTURE OCTET RULE- During a chemical reaction the atoms tend to adjust their electronic arrangement in such a way that they achieve 8 e - in their outermost
More informationbond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction
bond energy- energy required to break a chemical bond -We can measure bond energy to determine strength of interaction ionic compound- a metal reacts with a nonmetal Ionic bonds form when an atom that
More informationTest 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 informationChemical Bonding I: Basic Concepts
Chapter 8 Chemical Bonding I: Basic Concepts Dr. A. Al-Saadi 1 Chapter 8 Preview Ionic Bonding vs. covalent bonding. Electronegativity and dipole moment. Bond polarity. Lewis structure: ow to draw a Lewis
More informationIonic 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 information8.1 Types of Chemical Bonds List and define three types of bonding. chapter 8 Bonding General Concepts.notebook. September 10, 2015
chapter 8 Bonding General Concepts.notebook Chapter 8: Bonding: General Concepts Mar 13 11:15 AM 8.1 Types of Chemical Bonds List and define three types of bonding. Bonds are forces that hold groups of
More informationChapter 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 informationChapter 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 informationModels Of Chemical Bonding. Chapter Nine. AP Chemistry
Models Of Chemical Bonding Chapter Nine AP Chemistry Q. Why do atoms bond? A. To lower the potential energy between positive and negative particles. Atoms like humans seek to become more stable. Metals
More informationCOVALENT BONDING CHEMICAL BONDING I: LEWIS MODEL. Chapter 7
Chapter 7 P a g e 1 COVALENT BONDING Covalent Bonds Covalent bonds occur between two or more nonmetals. The two atoms share electrons between them, composing a molecule. Covalently bonded compounds are
More informationNOTES: 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 informationChemical 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 informationNotes: Covalent Bonding
Name Chemistry Pre-AP Notes: Covalent Bonding Period The main focus of this unit is on the covalent bond; however, we will briefly treat the ionic and metallic bond as well. I. Chemical Bonding Overview
More informationChapter 8 Basic concepts of bonding
Chapter 8 Basic concepts of bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule When atoms or ions are strongly attracted to one another, we say that there is a chemical bond between them. Types
More informationCartoon 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 informationElements react to attain stable (doublet or octet) electronic configurations of the noble gases.
digitalteachers.co.ug Chemical bonding This chapter teaches the different types and names of bonds that exist in substances that keep their constituent particles together. We will understand how these
More informationChapters and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity
Chapters 7.1-2 and 7.4 plus 8.1 and 8.3-5: Bonding, Solids, VSEPR, and Polarity Chemical Bonds and energy bond formation is always exothermic As bonds form, chemical potential energy is released as other
More informationCHEM 1305 Introductory Chemistry
CHEM 1305 Introductory Chemistry Introductory Chemistry: Concepts and Critical Thinking 7 th Edition, Charles H. Corwin Chapter 12. Chemical Bonding Modified by: Dr. Violeta F. Coarfa 1 Chemical Bond Concept
More informationIonic Bond TRANSFER of electrons between atoms. Ionic Bonding. Ionic Bonding. Ionic Bonding. Attraction that holds atoms together
BONDING Chemical Bond Attraction that holds atoms together Types include IONIC, METALLIC, or COVALENT Differences in electronegativity determine the bond type Ionic Bond TRANSFER of electrons between atoms
More informationDEFINITION. The electrostatic force of attraction between oppositely charged ions
DEFINITION The electrostatic force of attraction between oppositely charged ions Usually occurs when a metal bonds with a non-metal Ions are formed by complete electron transfer from the metal atoms to
More informationChemistry 101 Chapter 9 CHEMICAL BONDING
CHEMICAL BONDING Chemical bonds are strong attractive force that exist between the atoms of a substance. Chemical bonds are commonly classified into 3 types: Ionic Bonding Ionic bonds form between metals
More informationChapter 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 informationI. Multiple Choice Questions (Type-I)
I. Multiple Choice Questions (Type-I) 1. Isostructural species are those which have the same shape and hybridisation. Among the given species identify the isostructural pairs. (i) [NF 3 and BF 3 ] [BF
More information2 Bonding and structure Answers to Exam practice questions
Pages 77 80 Exam practice questions 1 a) Bonding between atoms in a metal is the result of electrostatic attractions between positive metal ions in a lattice and delocalised electrons in the outer shell
More informationChapter 9. Chemical Bonding I: The Lewis Model. HIV-Protease. Lecture Presentation
Lecture Presentation Chapter 9 Chemical Bonding I: The Lewis Model HIV-Protease HIV-protease is a protein synthesized by the human immunodeficiency virus (HIV). This particular protein is crucial to the
More informationCh8 Test. Multiple Choice Identify the choice that best completes the statement or answers the question.
h8 Test Multiple hoice Identify the choice that best completes the statement or answers the question. 1. n ionic bond is. a. attraction of an atom for its electrons. b. attraction of atoms for electrons
More informationCHEMICAL 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 information1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that
20 CHEMISTRY 11 D. Organizing the Elements The Periodic Table 1. Following Dalton s Atomic Theory, By 1817, chemists had discovered 52 elements and by 1863 that number had risen to 62. 2. In 1869 Russian
More information