1. Chapter 6 Chemical Bonding
Section 1 Introduction to Chemical Bonding
Chapter 6
Chemical Bonding
Ionic bonding – results from electrical attraction between cations and anions
Covalent bonding – results from sharing electron pairs between two atoms

2. Chapter 6 Chemical Bond Visual Concepts
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Visual Concept

3. Chapter 6 Ionic Bonding Visual Concepts
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Visual Concept

4. Chapter 6 Covalent Bonding Visual Concepts
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Visual Concept

5. Comparing Polar and Nonpolar Covalent Bonds
Visual Concepts
Chapter 6
Comparing Polar and Nonpolar Covalent Bonds
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Visual Concept

6. Using Electronegativity Difference to Classify Bonding
Visual Concepts
Chapter 6
Using Electronegativity Difference to Classify Bonding
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Visual Concept

7. Covalent Bonding
Nonpolar-covalent – equal distribution of shared electrons Polar-covalent – unequal attraction of shared electrons

8. Chapter 6 Chemical Bonding Sample Problem A
Section 1 Introduction to Chemical Bonding
Chapter 6
Chemical Bonding
Sample Problem A
Use electronegativity values listed in Figure 20 from the previous chapter in your book, on page 161, and Figure 2 in your book, on page 176, to classify bonding between sulfur, S, and the following elements: hydrogen, H; cesium, Cs; and chlorine, Cl. In each pair, which atom will be more negative?

9. Chapter 6 Chemical Bonding Sample Problem A Solution
Section 1 Introduction to Chemical Bonding
Chapter 6
Chemical Bonding
Sample Problem A Solution
The electronegativity of sulfur is 2.5. The electronegativities of hydrogen, cesium, and chlorine are 2.1, 0.7, and 3.0, respectively. In each pair, the atom with the larger electronegativity will be the more-negative atom.
Bonding between Electroneg. More-neg-
sulfur and difference Bond type ative atom
hydrogen 2.5 – 2.1 = 0.4 polar-covalent sulfur
cesium – 0.7 = 1.8 ionic sulfur
chlorine – 2.5 = 0.5 polar-covalent chlorine