Chemical Bonding

AB₂

Linear

AB₂E

Linear Bent

AB₃

Trigonal Planar

AB₄

Tetrahedral

AB₃E

Trigonal-Pyramidal

AB₂E₂

Bent 

AB₅

Trigonal-Bipyramidal 

AB₆

Octahedral

A pair of non-bonding electrons

A lone pair is defined as

Molecular Shape 

What is the VSEPR theory used to predict?

bent 

Which of the following shapes has an unshared pairs of electrons on the central atom? 

Trigonal Pyramidal

What molecular geometry would PH₃ have?

False

A molecule with a lone pair on the central atom would have the same electron and molecular geometry

Central Atom 

A = 

all atoms attached to the central atom

B =

Lone pair (e-) on the central atom

C =

180

Linear angle?

120

Linear bent angle?

120

Trigonal Planar

109.5

tetrahedral 

109.5

trigonal-pyramidal

109.5

bent

90

trigonal-bipyramidal

90

Octahedral

Covalent Bonding

bond caused by sharing of e- pairs between 2 atoms

non polar covalent bonds

equal sharing of e-

polar covalent bonds

unequal sharing of e-

Ionic Bonding

bond caused by electrical attraction between cations and anions, where e- are completely transferred

Metallic Bonding

metallic → metal-metal

0 - 0.3

nonpolar

0.3 - 1.7

Polar 

1.7 - 3.3 

Ionic 

independently

atoms rarely exist…..

electron dot notation

an electron configuration notation where valence electrons are indicated by dots placed around an element symbol

Octet rule

chemical compounds tend to form so that each atom has 8 e- in its valence shell