Chemistry - Ch 8

1

mono

2

di

3

tri

4

tetra

5

penta

6

hexa

7

hepta

8

octa

9

nona

10

deca

Bond-dissociation energy

amount of energy needed to break bonds

Inverse relationship

bond length and bond energy

Bond length

the distance between two bonded nuclei

Ionic bonds

a metal and a non-metal, transfer electrons

Covalent/Molecular bonds

a non-metal and a non-metal, share electrons

unshared pairs of electrons influence:

molecular shape

Lewis structures can *predict*:

molecular shape

Valence electrons determine:

shape

0 - 0.5

nonpolar covalent

0\.5 - 2.1

polar covalent

2\.1 - 3.3

ionic

Polarity is related to:

Bond Strength

Linear

Bent

Trigonal Planar

Trigonal Pyramidal

Tetrahedral

Diatomic Molecules

N, H, O, Cl, F, Br, I

A region of high probability where electrons are shared

Molecular orbital

Molecular bonds lengths are averages (because:)

The bonds are flexible

Which atom is most likely to form a triple covalent bond

Carbon