
1. Types of Chemical Bonds
1.1. Ionic
1.1.1. Ions of opposite charge
1.1.2. Generally result of metals and nonmetals; ex. NaCl
1.2. Covalent
1.2.1. Electrons shared
1.2.1.1. Single Bonds; ex. H2
1.2.1.2. Multiple Bonds; Double or Triple Bonds
1.3. Metallic
1.3.1. "Sea of Electrons"
1.3.1.1. High thermal conductivity
1.3.1.2. Malleable
1.3.1.3. Ductable
2. Lewis Symbols & the Octet Rule
2.1. Lewis Symbol
2.1.1. Chemical symbol w/ dots for valence electron(s)
2.2. Octet Rule
2.2.1. Atoms WILL have eight valence electrons
2.2.1.1. Gain
2.2.1.2. Lose
2.2.1.3. Share
2.2.2. Exceptions to the Rule
2.2.2.1. Molecules and polyatomic ions containing an odd number of electrons
2.2.2.2. Molecules and polyatomic ions in which an atom has fewer than an octet of valence electrons
2.2.2.3. Molecules and polyatomic ions in which an atom has more than an octet of valence electrons
3. Bond Polarity & Electronegatvity
3.1. Bond Polarity
3.1.1. Nonpolar covalent bond = electrons shared equally
3.1.2. Polar covalent bond = electrons shared unequally
3.2. Electronegativity
3.2.1. Ability of atom in a molecule to attract e- to itself
3.2.2. Greater the electronegativity = greater ability to attract e-
4. Lewis Structures
4.1. Representation of the covalent bonding in a molecule
4.2. Shared electron pairs shown as lines
4.3. Unshared electron pairs shown as dots
4.4. Resonance Structures
4.4.1. Two or more Lewis Structures = good descriptions of single molecule
4.4.1.1. GIve more accurate description of real molecule
5. Bond Strength (Bond Enthalpy) and Multiple Bonds
5.1. Bond Strength (Enthalpy)
5.1.1. Energy required to break a chemical bond
5.1.2. Expressed in units of kJ mol-1
5.2. Multiple Bonds
5.2.1. Sigma bonds
5.2.1.1. Formed by orbitals overlapping end-to-end w/ electron density concentrated b/w the nuclei
5.2.2. Pi bond
5.2.2.1. Formed by side-to-side overlapping orbitals w/ electron density concentrated above & below plane of the nuclei
6. Hybrid Orbitals and Molecular Orbitals
6.1. Hybrid Orbitals
6.1.1. Mixing of different kinds of atomic orbitals on same atom
6.1.2. Process of mixing atomic orbitals = hybridization
6.2. Molecular Orbitals
6.2.1. Allowed state for an electron in a molecule
7. Molecular Shapes
7.1. Shape determined by bond angles
7.2. Bond angles + bond lengths = shape and size of molecule
7.3. Basic Molecular Shapes
7.3.1. Linear
7.3.2. Trigonal Planar
7.3.3. Trigonal bipyramidal
7.3.4. Tetrahedral
7.3.5. Octahedral
7.4. VSEPR Model
7.4.1. Used to determine shape of molecule
7.4.2. Based on idea electron domains are negatively charged and repel one another