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Chapter 4 - Chemical Bonds
4.1 The Art of Deduction: Stable Electron Configurations
Octet Rule
Inert Gas Electron Configuration
Sodium can lose a valence electron. In doing so, its core electrons are like the noble gas,
neon.
Chlorine can gain an electron, and in doing so, its electron structure becomes like argon.
4.2 Lewis Electron-Dot Structures
Valence Electrons
Core Electrons
Lewis Dot Structure
Electron dot structure
Radical – unpaired electron
Use the periodic table to determine the number of valence electrons
Lewis dot symbols use “dots” to represent valence electrons.
4.3 Sodium Reacts with Chlorine
Ionic Bond - ions
Metal + Nonmetal
Metal loses electrons
Nonmetal gains electrons
Electrostatic attraction
Crystal lattice
4.4 Using Lewis Symbols: More Ionic Compounds
Potassium + chlorine
Sodium + bromine
Magnesium + oxygen
Potassium + oxygen
Magnesium + nitrogen
4.5 Formulas and Names of Binary Ionic Compounds
Covalent bond
Nonpolar covalent
Identical nonmetals
C-H
4.7 Unequal Sharing: Polar Covalent Bonds
Electronegativity
Polar covalent
4.8 Polyatomic Molecules: Water, Ammonia, and Methane
Polyatomic molecules
4.9 Polyatomic Ions
Polyatomic ions
Table 4.4 lists the common polyatomic ions to be discussed
4.10 Rules for Writing Lewis Formulas
4.11 Odd-Electron Molecules: Free Radicals
Radical
4.12 Molecular Shapes: The VSEPR Theory
Shapes of molecules
VSEPR
Valence shell electron pair repulsion
Orbital Geometry
Molecular Geometry
Linear
Bent
Trigonal planar or triangular
Pyramidal
Table 4.6 lists bonding and the shapes of molecules
4.13 Shapes and Properties: Polar and Nonpolar Molecules
4.14 A Chemical Vocabulary
Problems:
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4.4
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