AP Chemistry - Unit 3 Bonding

Linear

1-2 constituents

0 lone pairs

180 degrees

sp

Bent

2 constituents

1 lone pair

<120 degrees

sp2 or sp3 depending on lone pairs

Trigonal Planar

3 constituents

0 lone pairs

120 degrees

sp2

Tetrahedral

4 constituents

0 lone pairs

109.5 degrees

sp3

trigonal pyramidal

3 constituents

1 lone pair

107.3 degrees

bent (tet)

2 constituents

2 lone pairs

104.5 degrees

trigonal bipyramidal

5 constituents

0 lone pairs

90, 120 degrees

sp3d

see saw

4 constituents

1 lone pair

<90, <120, <180 degrees

t shaped

3 constituents

2 lone pairs

<90, <180 degrees

linear (5)

2 constituents

3 lone pairs

180 degrees

octahedral

6 constituents

0 lone pairs

90 degrees

sp3d2

square pyramidal

5 constituents

1 lone pair

<90 degrees

square planar

4 constitutes

2 lone pairs

90 degrees

Pi Bonds

non-hybridized orbitals; axial; double or triple bonds (1/2 is pi)

Sigma Bonds

single bonds; direct overlap; planar (equatorial)

Ionic Compound

• metal and nonmetal

Polar Covalent

• 2 nonmetals

• difference in electronegativity is between 1.6-0.5

• geom. asymmetrical and different elements

Covalent

• 2 nonmetals

• Diff in electronegativity is <0.5

• symmetrical geom.

Electronegativity Trend. Why?

Increases left to right and up

• smaller atomic radius has stronger nuclear pull, attracts electrons more

Lattice Energy

the energy required (released) to form an ionic compound

• less=weaker

Steps to form ionic salt compound

1) elements in ground state

2) vaporize to gas (endo)

3) break individual bonds (exo)

4) bond 2 together (exo - lattice energy)