Chapter 5 - Chemical Bonds
Bond
Octet Rule
Inert Gas Electron Configuration
Valence Electrons
Core Electrons
Lewis Dot Structure
Electron dot structure
Radical – unpaired electron
Ionic Bond - ions
Metal + Nonmetal
Metal loses electrons
Nonmetal gains electrons
Electrostatic attraction
Crystal lattice
Covalent bond
Nonpolar covalent
Identical nonmetals
C-H
electronegativity
Polar covalent
Polyatomic molecules
Polyatomic ions
Exceptions to octet rule
Radical
B, Be, Al
Expanded octet
Shapes of molecules
VSEPR
Valence shell electron pair repulsion
Orbital Geometry
Molecular Geometry
Linear
Bent
Trigonal planar or triangular
Pyramidal
Tetrahedral
Kinetic molecular theory
Solid
Liquid
Gas
All matter composed of tiny, discrete particles called molecules
Molecules of a gas in rapid constant motion & move in a straight line
Molecules of gas tiny compared with distances between them
There is very little attraction between molecules of a gas
Because they are so far apart, molecules collide with one another, and energy
is conserved in these collisions – although one molecule can gain energy at
the expense of another
Temperature is a measure of the average kinetic energy of the gas molecules
Polar and nonpolar molecules
Attractive Forces
Kinetic Energy
Temperature
Ionic Substance
Formula units
Ionic bond – salts
Molecules
Intramolecular forces – bonding
Intermolecular forces
Hydrogen bonding OH, NH, FH
Dipolar forces
Polar covalent bond
Lack of symmetry
London dispersion forces
Solutions
Homogeneous
Solute & solvent
Like dissolves like
Ion-ion vs Ion-dipole
Problems: 5.1, 5.3, 5.4, 6, 10,
13, 20, 24, 28, 32, 34a, 34c,
56, 58, 68, 70a, 74, 78, 80,
83, 84, 86, 88, 90, 92, 102,
106