Lecture B1 Lewis Dot Structures and Covalent Bonding
|
|
- Delphia Lang
- 5 years ago
- Views:
Transcription
1 Lecture B1 Lewis Dot Structures and Covalent Bonding
2 G.N. Lewis & Linus Pauling Two American Chemists G. N. Lewis Linus Pauling
3 The Covalent Bond 1. First proposed by G.N. Lewis in his seminal 1916 J. Am. Chem. Soc. publication (before QM was discovered!). 2. Lewis proposed that Covalent bonds consist of shared pairs of electrons. e created a powerful empirical formalism (Lewis dot structures) for understanding bonding in simple compounds. 3. Linus Pauling created a picture of covalent bonding that employed Quantum Mechanics (and won the 1954 Nobel Prize for it).
4 G.N. Lewis, circa the cubical atom.
5 G.N. Lewis, Journal of the American Chemical Society 38 (1916) 762.
6 G.N. Lewis, Journal of the American Chemical Society 38 (1916) 762. I2 molecule
7 ...we still think about covalent bonds the way G.N. Lewis did. In contrast to ionic bond, electrons are shared, not transferred......if the atoms are identical, then electrons are equally shared - an example of a perfectly nonpolar covalent bond.
8 In covalent bond formation, atoms go as far as possible toward completing their octets by sharing electron pairs. Covalent bonds are drawn as lines. Lone pairs are drawn as pairs of dots. I I I2 molecule
9 Lewis dot structures provide a simple, but extremely powerful, formalism for representing covalent bonding in molecules. a single bond, consisting of a pair of electrons.
10 Lewis dot structures provide a simple, but extremely powerful, formalism for representing covalent bonding in molecules. a nonbonding pair of electrons: a lone pair
11 Lewis dot structures provide a simple, but extremely powerful, formalism for representing covalent bonding in molecules. Note: no geometric information!
12 Lecture B1 Systematic Method for Creating Lewis Dot Structures
13 Lewis Dot Structures can be produced by following a sequence of steps. Let s produce a Lewis Dot Structure for: N4 + (the ammonium ion). Step 1: Count valence electrons: N = 5 4 x = 4 x 1 = 4 + = -1 Total = 5+4-1= 8 electrons = 4 bonds and lone pairs.
14 Lewis Dot Structures can be produced by following a sequence of steps. Let s produce a Lewis Dot Structure for: N4 + (the ammonium ion). Step 1: Count valence electrons: N = 5 4 x = 4 x 1 = 4 + = -1 Total = 5+4-1= 8 electrons = 4 bonds and lone pairs. N Step 2: Arrange the atoms (identify a central atom, if possible). +
15 Lewis Dot Structures can be produced by following a sequence of steps. Let s produce a Lewis Dot Structure for: N4 + (the ammonium ion). Step 1: Count valence electrons: + N = 5 4 x = 4 x 1 = 4 + = -1 Total = 5+4-1= 8 electrons = 4 bonds and lone pairs. Step 2: Arrange the atoms (identify a central atom, if possible). N Step 3: Place electron pairs on the atoms as either bonds or lone pairs.
16 Lewis Dot Structures can be produced by following a sequence of steps. Let s produce a Lewis Dot Structure for: N4 + (the ammonium ion). Step 1: Count valence electrons: + N = 5 4 x = 4 x 1 = 4 + = -1 Total = 5+4-1= 8 electrons = 4 bonds and lone pairs. Step 2: Arrange the atoms (identify a central atom, if possible). N Step 3: Place electron pairs on the atoms as either bonds or lone pairs.
17 Lewis Dot Structures can be produced by following a sequence of steps. Let s produce a Lewis Dot Structure for: N4 + (the ammonium ion). Step 1: Count valence electrons: + N = 5 4 x = 4 x 1 = 4 + = -1 Total = 5+4-1= 8 electrons = 4 bonds and lone pairs. Step 2: Arrange the atoms (identify a central atom, if possible). N Step 3: Place electron pairs on the atoms as either bonds or lone pairs. Step 4: Count electrons and compare with known count. If octet rule is satisfied for all atoms and the electron count is right, you re done. 8 valence electrons around N!
18 Lecture B1 Lewis Dot Structures Multiple Bonds
19 G.N. Lewis, Journal of the American Chemical Society 38 (1916) 762.
20 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 1: Count the valence electrons: 3 x C = 12 6 x = 6 x 1 = 6 O = 6 Total = = 24 electrons = 12 bonds or lone pairs.
21 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 2: Arrange the atoms: Identify a central atom. If you have C or O to choose from, go with C. O C C C
22 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 3: Place 12 electron pairs on the atoms. O C C C
23 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 3: Place 12 electron pairs on the atoms. O C C C Nine Bonds, Three Lone Pairs
24 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 4: Check for the octet rule. oops -- only 6 e! O C C C Nine Bonds, Three Lone Pairs
25 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 4: Check for the octet rule. Better! O C C C Ten Bonds (one double bond), Two Lone Pairs Done!
26 ...another example: Let s produce a Lewis Dot structure for: acetone: (C3)2CO. Step 4: Check for the octet rule. O C C C This takes practice, but then becomes tedious. Getting the polyatomic arrangement can be problematic.
27 ow about Double 07 (Nitrogen)? Step 1: 10 valence electrons/five bonds and lone pairs
28 ow about Double 07 (Nitrogen)? Step 1: 10 valence electrons/five bonds and lone pairs Step 2: Arrange atoms. N N
29 ow about Double 07 (Nitrogen)? Step 1: 10 valence electrons/five bonds and lone pairs Step 2: Arrange atoms. Step 3: Fill in electron pairs and bonds. N N
30 ow about Double 07 (Nitrogen)? Step 1: 10 valence electrons/five bonds and lone pairs Step 2: Arrange atoms. Step 3: Fill in electron pairs and bonds. N N
31 ow about Double 07 (Nitrogen)? Step 1: 10 valence electrons/five bonds and lone pairs Step 2: Arrange atoms. Step 3: Fill in electron pairs and bonds. Step 4: Octet rule obeyed! N N A Triple Bond!
32 multiple bonds have higher bond dissociation energies...
33 A quantitative comparison of CC bonds N2 Bond Dissociation Energy: 941 kj mol -1
34 bond lengths are inversely correlated with bond energies - shorter bonds are stronger... Double 07 is very strong!
35 Lecture B1 Lewis Dot Structures Formal Charge
36 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs.
37 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs. Step 2: Arrange the atoms. Go with Carbon in the center. S C S
38 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs. Step 2: Arrange the atoms. Go with Carbon in the center. S C S Step 3: Fill in the electron pairs.
39 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs. Step 2: Arrange the atoms. Go with Carbon in the center. S C S Step 3: Fill in the electron pairs.
40 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs. Step 2: Arrange the atoms. Go with Carbon in the center. S C S Step 3: Fill in the electron pairs. Step 4: Check for the octet rule.
41 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs. Step 2: Arrange the atoms. Go with Carbon in the center. S C S Step 3: Fill in the electron pairs. Step 4: Check for the octet rule. Good!
42 Let s produce a Lewis Dot structure for carbon disulfide, CS2. Step 1: Count valence electrons: C = 4 2 x S = 6 x 2 = 12 Total = = 16 e/8 electron pairs. Step 2: Arrange the atoms. Go with Carbon in the center. S C S Step 3: Fill in the electron pairs. Step 4: Check for the octet rule. BUT wait, what about?? C S S
43 To decide between these two candidate structures, we need to calculate the formal charges on the atoms.
44 Less formal charge is better. Thus, SCS wins! SCS wins!
45 Carbon dioxide, CO2, is isoelectronic with carbon disulfide, CS2.
46 Nitrous oxide, N2O, is also isoelectronic with carbon disulfide, CS2.
47 Lecture B1 Lewis Dot Structures Resonance
48 When multiple Lewis Dot Structures exist that are differentiated only by the positions of the electrons (the positions of the atoms are identical), the ACTUAL structure is a weighted average of these resonance structures. We predict that the three N-O bonds in the nitrate ion are identical in length.
49 Another Example: We predict that the two C-O bonds in the acetate ion are identical in length.
50 And Another Example: Benzene
51 Two resonance structures for benzene... We predict that all of the C-C bonds in benzene have the same length.
52 So normally, Chemists represent benzene like this:
53 Lecture B1 Lewis Dot Structures Exceptions to the Octet Rule
54 In the benzene, the actual structure is the average of the possible resonance structures, but this is often not the case when resonance structures with a range of formal charge values are possible. In this case, the actual structure will be a weighted average of the available resonance structures. A what? an example: Grades are often computed using a weighted average. Suppose that homework counts 10%, quizzes 20%, and tests 70%. If Pat has a homework grade of 92, a quiz grade of 68, and a test grade of 81, then Pat's overall grade = (0.10)(92) + (0.20)(68) + (0.70)(81) = 79.5 ow do we weight resonance structures?
55 An example: Which is the better Lewis Dot representation for the phosphate ion, PO4 3-?
56 An example: Which is the better Lewis Dot representation for the phosphate ion, PO4 3-? We have to look at the formal charge arguments here. The structure shown at right has fewer formal charges, but... P has 10 electrons - is this ok?
57 An example: Which is the better Lewis Dot representation for the phosphate ion, PO4 3-? If 10 electrons is okay for P, then less charge is better.
58 An example: Which is the better Lewis Dot representation for the phosphate ion, PO4 3-? If 10 electrons is okay for P, then less charge is better. P can use its d electrons to expand its valence shell. More than 8 electrons = "hypervalent"
59 What if a second double bond is added? - formal charge on that O goes from -1 to 0 - formal charge on P goes from 0 to -1 - total number of formal charges is unchanged. - electron count on P goes from 10 to 12. If 12 electrons is okay for P, then is it better to charge P or O?
60 Actually, all of these resonance structures contribute to the weighted average resonance hybrid that is observed. lower weighting factor higher weighting factor lower weighting factor We need more information to determine the exact weighting factors. Pauling will introduce the concept of electronegativity to help with this.
61 Final example: Rank these Lewis dot resonance structures for cyanate (NCO - ) from best to worst:
62 Final example: Rank these Lewis dot resonance structures for cyanate (NCO - ) from best to worst: 1 2 Again, Pauling's concept of electronegativity will help with this. 3
63 Another exception to the octet rule: 1. Be, B, and Li can be electron deficient. examples: note: no formal charges here...
64 Another exception to the octet rule: 1. Be, B, and Li can be electron deficient. examples: what about this resonance structure?
65 Another exception to the octet rule: 1. Be, B, and Li can be electron deficient. examples: a smaller weighting factor for this structure
66 Another exception to the octet rule: 2. Non metals in period 3 or higher can accommodate more than 8 electrons by employing d-orbitals. examples: We talked about this one before.
67 Another exception to the octet rule: 2. Non metals in period 3 or higher can accommodate more than 8 electrons by employing d-orbitals. examples: Sulfur can do this too.
68 Another exception to the octet rule: 2. Non metals in period 3 or higher can accommodate more than 8 electrons by employing d-orbitals. examples: Even Xenon gets in on the act!
69 Lecture B1 Bond Polarity and Electronegativity
70 Pauling realized that covalent bonds between different nuclei will not be symmetric in electron density (probability): Linus Pauling
71 This will lead to a pair of net positive and negative partial charges that will result in a DIPOLE MOMENT for the molecule: or dipole moment = charge x distance Linus Pauling
72 This will lead to a pair of net positive and negative partial charges that will result in a DIPOLE MOMENT for the molecule: dipole moment = charge x distance 1 Debye = 1D = x C m Named after Peter J. W. Debye Dutch Physicist Nobel Prize in Chemistry 1936 Peter J. W. Debye
73 This will lead to a pair of net positive and negative partial charges that will result in a DIPOLE MOMENT for the molecule: Cl Dipole Moment: 1.08D Linus Pauling
74 Pauling proposed a number to quantitate the ability of an atom to polarize a bond: "Pauling Electronegativity" χ (chi) Electronegativity ranges from 0.7 to 4.0. It is unitless!
75 Three terms that are often confused: Ionization energy: the energy required to remove an electron from an atom or ion. Electron affinity: the energy change associated with the addition of one electron to an atom or ion. Electronegativity: the ability of an atom in a molecule to draw bonding electrons to itself. Important: this is a dimensionless parameter - not an energy.
76 Dipole Moments and Pauling Electronegativity Cl Dipole Moment: 1.08D χcl - χ = = 0.9 Electron density is higher on the atom with higher electronegativity. Linus Pauling
77 Dipole Moments and Pauling Electronegativity F Dipole Moment: 1.83D χf - χ = = 1.9 Cl Dipole Moment: 1.08D χcl - χ = = 0.9 Br Dipole Moment: 0.82D χbr - χ = = 0.7 Electronegativity differences correlate with dipole moment values. Linus Pauling
78 Rank these Lewis dot resonance structures for cyanate (NCO - ) from best to worst: 1 2 We can go back and use electronegativity to rank Lewis dot resonance structures. χn = 3.0 and χo = 3.5. Thus the negative charge prefers to reside on the Oxygen. 3
79 Generalizing, any bond will possess a bond dipole moment with a magnitude that is proportional to the difference in electronegativity between the bonding partners. + N For example, even though N4 + has no dipole moment, the four covalent bonds in the ammonium ion are between two elements with different electronegativities: χn - χ = = 0.9, and therefore EAC has a bond dipole moment. The fact that the four dipole moments cancel is a matter of geometric structure. That is the NEXT topic -- VSEPR Theory!
CHAPTER 8 BONDING: GENERAL CONCEPTS
Advanced Chemistry Name Hour Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 8 BONDING: GENERAL CONCEPTS Day Plans for the day Assignment(s)
More informationChapter 8. Ions and the Noble Gas. Chapter Electron transfer leads to the formation of ionic compounds
Chapter 8 Chemical Bonding: General Concepts 1 8.1 Electron transfer leads to the formation of ionic compounds Ionic compounds form when metals and nonmetals react The attraction between positive and negative
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 Versus Covalent Bonding
Ionic Versus Covalent Bonding Ionic compounds are formed when electrons are transferred from one atom to another The transfer of electrons forms ions Each ion is isoelectronic with a noble gas Electrostatic
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 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 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 informationChapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More informationChapter 4 Lecture Outline. Copyright McGraw-Hill Education. Permission required for reproduction or display.
Chapter 4 Lecture Outline 1 Copyright McGraw-ill Education. Permission required for reproduction or display. 4.1 Introduction to Covalent Bonding Covalent bonds result from the sharing of electrons between
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 informationGeometry of Covalent Compounds
Geometry of Covalent Compounds Introduction This laboratory exercise will give you experience working with molecular model sets so you will better understand the geometries of small covalent molecules.
More informationNature of the Chemical Bond; Lewis Structures & Chemical Bonding
Nature of the Chemical Bond; Lewis Structures & Chemical Bonding CHEM 107 T. Hughbanks Energetics of Ionic Bonding Problem #7.37: formation of KI ion pair from neutral atoms of K, I K (g) + I (g) K + (g)
More informationBig Idea: Ionic Bonds: Ionic Bonds: Metals: Nonmetals: Covalent Bonds: Ionic Solids: What ions do atoms form? Electron Electron
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More informationCH 222 Chapter Seven Concept Guide
CH 222 Chapter Seven Concept Guide 1. Lewis Structures Draw the Lewis Dot Structure for cyanide ion, CN -. 1 C at 4 electrons = 4 electrons 1 N at 5 electrons = 5 electrons -1 charge = + 1 electron Total
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 informationsharing or transferring electrons between atoms covalent ionic polar covalent Quantitative description: Quantum mechanics
Chapter. 3 Chemical Bonding: The Classical Description Two or more atoms approach -> their electrons interact and form new arrangements of electrons with lower total potential energy than isolated atoms
More informationProblems and questions How is a molecule or polyatomic ion held together? Why are atoms distributed at strange angles? Why are molecules not flat?
1 Cocaine 2 Problems and questions ow is a molecule or polyatomic ion held together? Why are atoms distributed at strange angles? Why are molecules not flat? Can we predict the structure? ow is structure
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 informationMore Chemical Bonding
More Chemical Bonding Reading: Ch 10: section 1-8 Ch 9: section 4, 6, 10 Homework: Chapter 10:.31, 33, 35*, 39*, 43, 47, 49* Chapter 9: 43, 45, 55*, 57, 75*, 77, 79 * = important homework question Molecular
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 informationChapter 8. Chemical Bonding I: Basic Concepts
Chapter 8 Chemical Bonding I: Basic Concepts Topics Lewis Dot Symbols Ionic Bonding Covalent Bonding Electronegativity and Polarity Drawing Lewis Structures Lewis Structures and Formal Charge Resonance
More informationCHEM 110 Exam 2 - Practice Test 1 - Solutions
CHEM 110 Exam 2 - Practice Test 1 - Solutions 1D 1 has a triple bond. 2 has a double bond. 3 and 4 have single bonds. The stronger the bond, the shorter the length. 2A A 1:1 ratio means there must be the
More informationCHAPTER 12 CHEMICAL BONDING
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 12 CHEMICAL BONDING Day Plans for the day Assignment(s) for the day 1 Begin Chapter
More informationPeriodic Trends. Homework: Lewis Theory. Elements of his theory:
Periodic Trends There are various trends on the periodic table that need to be understood to explain chemical bonding. These include: Atomic/Ionic Radius Ionization Energy Electronegativity Electron Affinity
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 informationChemistry: The Central Science
Chemistry: The Central Science Fourteenth Edition Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds Three basic types of bonds Ionic Electrostatic attraction between ions Covalent Sharing of
More informationCovalent Bonding Introduction, 2. Chapter 7 Covalent Bonding. Figure 7.1 The Hydrogen Molecule. Outline. Covalent Bonding Introduction, 1. Figure 7.
Covalent Bonding Introduction, 2 William L. Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 7 Covalent Bonding Electron density Electrons are located between nuclei Electrostatic
More informationBonding - Ch. 7. Types of Bonding
Types of Bonding I. holds everything together! II. All bonding occurs because of III. Electronegativity difference and bond character A. A between two atoms results in a when those two atoms form a bond.
More informationChemistry 1000 Lecture 15: Covalent bonding and Lewis structures
Chemistry 1000 Lecture 15: Covalent bonding and Lewis structures Marc R. Roussel October 3, 2018 Marc R. Roussel Covalent bonding October 3, 2018 1 / 24 Lewis diagrams Covalent bonding Covalent bond: a
More informationChemical Bonding II. Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds Hybridization MO theory
Chemical Bonding II Molecular Geometry Valence Bond Theory Phys./Chem. Properties Quantum Mechanics Sigma & Pi bonds ybridization MO theory 1 Molecular Geometry 3-D arrangement of atoms 2 VSEPR Valence-shell
More informationChapter 6. Table of Contents. Section 1 Covalent Bonds. Section 2 Drawing and Naming Molecules. Section 3 Molecular Shapes. Covalent Compounds
Covalent Compounds Table of Contents Section 1 Covalent Bonds Section 2 Drawing and Naming Molecules Section 3 Molecular Shapes Section 1 Covalent Bonds Bellringer Make a list of the elements that form
More informationTheories of Covalent Bonding Molecular Geometry and Hybridization of Atomic Orbitals
Chapter 10 Theories of Covalent Bonding and ybridization of Atomic Orbitals Drawing Lewis Structures 1) Place least electronegative element as the central atom. Recognize that C,S,P and N are often central
More informationChemical Bonding. The Octet Rule
Chemical Bonding There are basically two types of chemical bonds: 1. Covalent bonds electrons are shared by more than one nucleus 2. Ionic bonds electrostatic attraction between ions creates chemical bond
More informationChemical Bonding I: Covalent Bonding. How are atoms held together in compounds?
I: Covalent Bonding How are atoms held together in compounds? IONIC or COVALENT bonds or forces For most atoms, a filled outer shell contains 8 electrons ----- an octet Atoms want to form octets when they
More informationLecture 17 - Covalent Bonding. Lecture 17 - VSEPR and Molecular Shape. Lecture 17 - Introduction. Lecture 17 - VSEPR and Molecular Shape
Chem 103, Section F0F Unit VI - Compounds Part II: Covalent Compounds Lecture 17 Using the Valence-Shell Electron-Pair Repulsion (VSEPR) Theory to predict molecular shapes Molecular shape and polarity
More informationConcepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds. David A. Katz Pima Community College Tucson, AZ
Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds David A. Katz Pima Community College Tucson, AZ Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction
More information11/14/2014. Chemical Bonding. Richard Philips Feynman, Nobel Laureate in Physics ( )
Chemical Bonding Lewis Theory Valence Bond VSEPR Molecular Orbital Theory 1 "...he [his father] knew the difference between knowing the name of something and knowing something" Richard Philips Feynman,
More informationChapter 13: Phenomena
Chapter 13: Phenomena Phenomena: Scientists measured the bond angles of some common molecules. In the pictures below each line represents a bond that contains 2 electrons. If multiple lines are drawn together
More information6.1 Intro to Chemical Bonding Name:
6.1 Intro to Chemical Bonding Name: A. Chemical bond Favored by nature because: 3 main types of bonds 1. 2. 3. B. Ionic Bonds C. Covalent Bonds D. Metallic Bond E. Bond Determination RECALL: Electronegativity
More informationCovalent Bonding 10/29/2013
Bond Energies or Bond Dissociation Energies Tables 8.4 and 8.5 on page 72 gives a list of the energy required to dissociate or break bonds. This value is used to determine whether covalent bonds will form
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 informationREVIEW ANSWERS EXAM 3 GENERAL CHEMISTRY I Do not hesitate to contact the instructor should you have any questions.
REVIEW ANSWERS EXAM 3 GENERAL CEMISTRY I Do not hesitate to contact the instructor should you have any questions. 1) Predict which of the following has the largest atomic radius: potassium (K) OR selenium
More informationWhat is a Bond? Chapter 8. Ionic Bonding. Coulomb's Law. What about covalent compounds?
Chapter 8 What is a Bond? A force that holds atoms together. Why? We will look at it in terms of energy. Bond energy- the energy required to break a bond. Why are compounds formed? Because it gives the
More informationAdapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction
Adapted from CHM 130 Maricopa County, AZ Molecular Geometry and Lewis Dot Formulas Introduction A chemical bond is an intramolecular (within the molecule) force holding two or more atoms together. Covalent
More informationAP Chemistry Chapter 7: Bonding
AP Chemistry Chapter 7: Bonding Types of Bonding I. holds everything together! I All bonding occurs because of! Electronegativity difference and bond character A. A difference in electronegativity between
More informationLewis Structures. X } Lone Pair (unshared pair) } Localized Electron Model. Valence Bond Theory. Bonding electron (unpaired electron)
G. N. Lewis 1875-1946 Lewis Structures (The Localized Electron Model) Localized Electron Model Using electron-dot symbols, G. N. Lewis developed the Localized Electron Model of chemical bonding (1916)
More informationChem 115: Chapter 9 Dr. Babb
Periodic Properties of the Atom Properties that depend on position of element in the periodic table. Factors that affect the periodic properties: 1. Principal quantum number of valence shell (n valence
More informationGeometry of Covalent Compounds
Geometry of Covalent Compounds Introduction This laboratory exercise will give you experience working with molecular model sets so you will better understand the geometries of small covalent molecules.
More informationLewis Structures and Molecular Shapes
Lewis Structures and Molecular Shapes Drawing Lewis Structures Determine from formula if ionic or covalent Count the electrons If ionic : add valence # to charge if (-), subtract if (+) - = 7+1 electrons;
More informationCHEM 101: CHAPTER 11: CHEMICAL BONDS: THE FORMATION OF COMPOUNDS FROM ATOMS
1 CHEM 101: CHAPTER 11: CHEMICAL BONDS: THE FORMATION OF COMPOUNDS FROM ATOMS PERIODIC TRENDS: See pages 214-216, 221 Table 11.3, and 227 + 228 of text. Lewis Structures of Atoms: The Lewis Dot Diagram
More informationChapter 8 & 9 Concepts of Chemical. Bonding
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 8 & 9 Concepts of John D. Bookstaver St. Charles Community College St. Peters, MO 2006,
More informationDipole Moment, Resonance. Dr. Sapna Gupta
Dipole Moment, Resonance Dr. Sapna Gupta Dipole Moment This indicates whether a molecule is polar or not. Dipole moment ( ) is when a molecule can move in presence of an electric current. The higher the
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 informationThe role of atomic radius in ion channel selectivity :
5.111 Lecture Summary #10 Readings for today: Sections 2.14-2.16 (2.15-2.17 in 3rd ed), Section 2.5 (2.6 in 3rd ed) and Section 2.6 (2.7 in 3rd ed). Read for Lecture #11: Section 2.7 (2.8 in 3rd ed) Resonance,
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 informationCHEMISTRY - BURDGE-ATOMS FIRST 3E CH.6 - REPRESENTING MOLECULES.
!! www.clutchprep.com CONCEPT: ELECTRON-DOT SYMBOLS Before we look at the first two bonding models, we have to figure out how to depict the valence electrons of bonding atoms. In the electron-dot symbol,
More informationChapter 9 Molecular Geometry and Bonding Theories
Chapter 9 Molecular Geometry and Bonding Theories molecular shapes the VSEPR model molecular shape and molecular polarity covalent bonding and orbital overlap hybrid orbitals multiple bonds 9.1 Molecular
More informationH-H bond length Two e s shared by two Hs: covalent bonding. Coulomb attraction: Stronger attraction for e Fractional charge A dipole
8 Bonding: General Concepts Types of chemical bonds Covalent bonding Ex. 2 E (kj/mol) Repulsions of nucleus and e s r 0 458 0.074 r (nm) Zero interaction at long distance - bond length Two e s shared by
More informationBonding in Chemistry. Chemical Bonds All chemical reactions involve breaking of some bonds and formation of new ones where new products are formed.
CHEMICAL BONDS Atoms or ions are held together in molecules or compounds by chemical bonds. The type and number of electrons in the outer electronic shells of atoms or ions are instrumental in how atoms
More informationValence Bond Theory - Description
Bonding and Molecular Structure - PART 2 - Valence Bond Theory and Hybridization 1. Understand and be able to describe the Valence Bond Theory description of covalent bond formation. 2. Understand and
More informationBONDING. My Name is Bond. Chemical Bond
BONDING My Name is Bond. Chemical Bond PART 1: Ionic & Covalent Bonding Chemical Bonds! A chemical bond is an attraction between 2 atoms or ions.! Bonding occurs because it lowers the energy of the system.!
More informationChapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry Periodic Trends in Atomic Properties Learning Objective
Chapter 11 Chemical Bonds: The Formation of Compounds from Atoms Advanced Chemistry 11.1 Periodic Trends in Atomic Properties Discuss the atomic trends Metals are located on the left side of the periodic
More informationMolecular Geometry & Polarity
Molecular Geometry & Polarity Learn Shapes you will Because the physical and chemical properties of compounds are tied to their structures, the importance of molecular geometry can not be overstated. Localized
More informationChapter 8. Bonding: General Concepts. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents (8.1) (8.2) (8.3) (8.4) (8.5) (8.6) (8.7) (8.8) Types of chemical bonds Electronegativity Bond polarity and dipole moments Ions: Electron
More informationChemical Bonding Petrucci, Harwood and Herring: Chapters 10 and 11
Chemical Bonding Petrucci, Harwood and Herring: Chapters 10 and 11 Aims: To look at bonding and possible shapes of molecules We will mainly do this through Lewis structures To look at ionic and covalent
More informationChapter 4: Covalent Bonding and Chemical Structure Representation
Chapter 4: Covalent Bonding and Chemical Structure Representation The Octet Rule -An atom with 8 electrons (an octet ) in its outer shell has the same number of valence electrons as the noble gas in the
More informationChapter 6 Chemistry Review
Chapter 6 Chemistry Review Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The electrons involved in
More informationChapter 9 The Shapes of Molecules Cocaine
Chapter 9 The Shapes of Molecules 1 Cocaine 10.1 Depicting Molecules & Ions with Lewis Structures 2 Number of Covalent Bonds 3 The number of covalent bonds can be determined from the number of electrons
More informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8. Basic Concepts of Chemical Bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule 8.2 Ionic Bonding Consider the reaction between sodium and chlorine: Na(s) + ½ Cl 2 (g) NaCl(s) H o f
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 informationCHEMISTRY. Chapter 9 The Basics of Chemical Bonding. The Molecular Nature of Matter. Jespersen Brady Hyslop SIXTH EDITION
CEMISTRY The Molecular Nature of Matter SIXT EDITIN Jespersen Brady yslop Chapter 9 The Basics of Chemical Bonding Copyright 2012 by John Wiley & Sons, Inc. Chemical Bonds Attractive forces that hold atoms
More informationORGANIC CHEMISTRY. Meaning of Organic?
ORGANIC CHEMISTRY Meaning of Organic? Initially scientists believed there was a special force in living organisms -this was assumed the unique component of organic material In 1828 Wöhler synthesized urea
More informationChapter 8. forces of attraction which hold atoms or ions together. 3 fundamental types of bonding. Ionic - metals & nonmetals
Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds forces of attraction which hold atoms or ions together 3 fundamental types of bonding Ionic - metals & nonmetals Covalent - nonmetals (semimetals)
More informationSection 12: Lewis Structures
Section 12: Lewis Structures The following maps the videos in this section to the Texas Essential Knowledge and Skills for Science TAC 112.35(c). 12.01 Electronegativity Chemistry (5)(C) 12.02 Electron
More information13 Bonding: General Concepts. Types of chemical bonds. Covalent bonding Ex. H 2. Repulsions of nuclei and e s. Zero interaction at long distance
13 Bonding: General Concepts Types of chemical bonds Covalent bonding Ex. 2 E (kj/mol) epulsions of nuclei and e s r 0 458 0.074 r (nm) - bond length Two e s shared by two s: covalent bonding Zero interaction
More informationDO NOT OPEN UNTIL INSTRUCTED TO DO SO. CHEM 110 Dr. McCorkle Exam #5. While you wait, please complete the following information:
DO NOT OPEN UNTIL INSTRUCTED TO DO SO CHEM 110 Dr. McCorkle Exam #5 While you wait, please complete the following information: Name: Student ID: Turn off cellphones and stow them away. No headphones, mp3
More informationOutline 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 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 informationWarm-Up. Write down the equation for Coulomb s Law AND write a sentence that describes how it connects to ionic bonding.
Warm-Up Write down the equation for Coulomb s Law AND write a sentence that describes how it connects to ionic bonding. Chemical Bonding Ionic Bonding Which spheres below are K + cations and which are
More informationExperiment 21 Lewis structures and VSEPR Theory
Experiment 21 Lewis structures and VSEPR Theory Introduction 1. Lewis Structures and Formal Charge LG.N. Lewis, at the University of California at Berkeley devised a simple way to understand the nature
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 8. Basic Concepts of Chemical Bonding. Lecture Presentation. John D. Bookstaver St. Charles Community College Cottleville, MO
Lecture Presentation Chapter 8 of Chemical John D. Bookstaver St. Charles Community College Cottleville, MO Chemical Bonds Three basic types of bonds Ionic Electrostatic attraction between ions. Covalent
More information!"##$%&'()$*+,%'-./'
!"##$%&()$*+,%-./ 0,1,%$234%5$1673896:2:567$2(),#6;+%& 6!#6+)! CHAPTER 3-4: Concepts to Know! The difference between ionic and covalent bonds! Define cations and anions! Predict cation/anion
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 informationBonding - Ch Types of Bonding
Types of Bonding I. holds everything together! II. All bonding occurs because of III. Electronegativity difference and bond character A. A between two atoms results in a when those two atoms form a bond.
More informationDrawing Lewis Structures
Chapter 2 - Basic Concepts: molecules Bonding models: Valence-Bond Theory (VB) and Molecular Orbital Theory (MO) Lewis acids and bases When both of the electrons in the covalent bond formed by a Lewis
More informationChapter 8. Basic Concepts of Chemical Bonding
Chapter 8. Basic Concepts of Chemical Bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule 8.2 Ionic Bonding positive and negative ions form an ionic lattice, in which each cation is surrounded
More informationMolecular Geometry and Polarity 1
Experiment Molecular Geometry and Polarity 1 Objectives At the end of this activity you should be able to: o Write Lewis structures for molecules. o Classify bonds as nonpolar covalent, polar covalent,
More informationChemical Bonds, Lewis Structures, Bond Order, and Formal Charge
Chemical Bonds, Lewis Structures, Bond Order, and Formal Charge PRELAB ASSIGNMENT Read the entire laboratory write up. Write an objective, any hazards associated with this lab, and answer the following
More informationTopic 4: Chemical Bonds. IB Chemistry SL Ms. Kiely Coral Gables Senior High
Topic 4: Chemical Bonds IB Chemistry SL Ms. Kiely Coral Gables Senior High 5th PERIOD Bell Ringer - review of 4.1 Quiz (revised) 1. What is the formula of a compound formed by magnesium and phosphate?
More informationStructure and Bonding. Dr. Sapna Gupta
Structure and Bonding Dr. Sapna Gupta Origins of Organic Chemistry Initially thought to be chemicals that were obtained from plants and animals only. Thought to have a vital force as they from natural
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 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 informationMolecular Geometry and Bonding Theories. Molecular Shapes. Molecular Shapes. Chapter 9 Part 2 November 16 th, 2004
Molecular Geometry and Bonding Theories Chapter 9 Part 2 November 16 th, 2004 8 Molecular Shapes When considering the geometry about the central atom, we consider all electrons (lone pairs and bonding
More informationOf The Following Cannot Accommodate More Than An Octet Of Electrons
Of The Following Cannot Accommodate More Than An Octet Of Electrons This is most common example of exceptions to the octet rule. their empty d orbitals to accommodate additional electrons. A case where
More informationWorksheet 5 - Chemical Bonding
Worksheet 5 - Chemical Bonding The concept of electron configurations allowed chemists to explain why chemical molecules are formed from the elements. In 1916 the American chemist Gilbert Lewis proposed
More informationChapter 8. Bonding: General Concepts
Chapter 8 Bonding: General Concepts Chapter 8 Questions to Consider What is meant by the term chemical bond? Why do atoms bond with each other to form compounds? How do atoms bond with each other to form
More informationCHEMICAL BONDS. Electrical forces. Reflect a balance in the attractive and repulsive forces between electrically charged particles
CHEMICAL BONDS Chemical Bonds: Electrical forces. Reflect a balance in the attractive and repulsive forces between electrically charged particles Lewis Theory of Bonding: Electrons play a fundamental role
More informationChemistry 121: Topic 4 - Chemical Bonding Topic 4: Chemical Bonding
Topic 4: Chemical Bonding 4.0 Ionic and covalent bonds; Properties of covalent and ionic compounds 4.1 Lewis structures, the octet rule. 4.2 Molecular geometry: the VSEPR approach. Molecular polarity.
More informationCh. 8 Chemical Bonding: General Concepts. Brady & Senese, 5th Ed
Ch. 8 Chemical Bonding: General Concepts Brady & Senese, 5th Ed Index 8.1. Electron transfer leads to the formation of ionic compounds 8.2. Lewis symbols help keep track of valence electrons 8.3. Covalent
More information