Compounds have high melting and boiling points

When 2 atoms share electrons.
Single bonds - sigma bonds.
Double bonds - pi bonds, stronger and shorter than single bonds, but NOT double the strength

Network (covalent) bonds: Very hard, very high melting/boiling points

1) Count number of valence electrons total
2) Arrange atoms around least electronegative atom
3) Add electrons to surrounding atoms to fill octet rule
4) Add remaining to central atom
5) If less than octet, then add double bonds. Else, if octet or more than octet, then that is okay.

Different structures of the same formula

BeH₂
BF₃
PCl₅
SF₄
SF₆

Electrons repel one another, so when atoms come together to form a molecule, the molecule will assume shape that keeps electron pairs as far apart as possible.

Central atom forms hybrid orbitals

Double/triple bonds treated as single bonds (but will occupy slightly more space)

Lone pairs also have slightly more repulsive strength, so will occupy a little more space.

0 lone pairs: linear

0 lone pairs: trigonal planar

1 lone pair: bent

0 lone pairs: tetrahedral

1 lone pair: trigonal pyramidal

2 lone pairs: bent

0 lone pairs: trigonal bipyramidal

1 lone pair: seesaw

2 lone pairs: t-shaped

3 lone pairs: linear

0 lone pairs: octahedral

1 lone pair: square pyramidal

2 lone pairs: square planar

3 lone pairs: t-shaped

4 lone pairs: linear

Freedom of movement of electrons makes them good conductor of heat/electricity, malleable, and ductile

Metals composed of smaller nuclei - stronger

In order of weakest to strongest:

London Dispersion foces

Dipole-dipole forces

Hydrogen Bonds (F, O, N)

Description