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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
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Chapter 6 Chemical Bond Visual Concepts
Click below to watch the Visual Concept. Visual Concept
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Chapter 6 Ionic Bonding Visual Concepts
Click below to watch the Visual Concept. Visual Concept
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Chapter 6 Covalent Bonding Visual Concepts
Click below to watch the Visual Concept. Visual Concept
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Comparing Polar and Nonpolar Covalent Bonds
Visual Concepts Chapter 6 Comparing Polar and Nonpolar Covalent Bonds Click below to watch the Visual Concept. Visual Concept
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Using Electronegativity Difference to Classify Bonding
Visual Concepts Chapter 6 Using Electronegativity Difference to Classify Bonding Click below to watch the Visual Concept. Visual Concept
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Covalent Bonding Nonpolar-covalent – equal distribution of shared electrons Polar-covalent – unequal attraction of shared electrons
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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?
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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
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