Cl

1

• Cl-

chloride
2

• Na

sodium
3

• Cu2

Copper (II)
4

• Al3 SO42-

Al2(SO4)3
5

• SnO2

Tin(IV) oxide
6

• SnO

Tin(II) oxide
7
Octet Rule Exceptions

• Period 1 only 2 valence electrons is a full
  shell
• B often has only 6 valence electrons
• P S may have 10 or 12 valence electrons

8
Covalent Bond

• one or more pairs of electrons are shared by two
  atoms.

9
Molecule

• atoms held together by covalent bonds.

10
Diatomic Molecules

• 2 atoms of one element bonded together
• H2 N2 O2 F2 Cl2 Br2 I2

11
Lewis Electron Diagrams

• Dots represent valence electrons.
• written on 4 sides around symbol
• 2 electrons on same side are paired

12
Write the Lewis structures for

• Calcium
• Chlorine
• Potassium

13
Draw Electron Dot Diagrams for the following

• Mg, O, Ar, H, P, Na, I

14
Forming a bond
15

• Single Bond one pair of shared electrons (2 e-)
• Double Bond two pair of shared electrons (4 e-)
• Triple Bond three pair of shared electrons (6
  e-)

16
Lewis Structures

• a pair of electrons is represented with a dash
  instead of 2 dots
• is single bond
• is a double bond
• ? is a triple bond

17
Sigma Bond, ?

• a single covalent bond with an electron pair that
  is shared by the overlap of bonding orbitals

18
Pi Bond, ?

• a bond formed when parallel orbitals overlap to
  share electrons

19
Bond lengths

• Smaller atoms have shorter bond lengths.
• Multiple bonds are shorter than single bonds.

20
Bond strength

• Shorter bonds are stronger than longer bonds

21
Molecular Compounds

• similar naming to ionic
• least electronegative comes first
• prefixes show numbers of atoms in molecule

22

• SO2 sulfur dioxide
• CCl4 carbon tetrachloride
• SiS2 silicon disulfide

23
Prefixes

• mono 1
• di 2
• tri 3
• tetra 4
• penta 5

• hexa 6
• hepta 7
• octa 8
• nona 9
• deca 10

24
Name the following

• N2O5
• SO2
• SiO2
• PCl3

Dinitrogen pentoxide
Sulfur dioxide
Silicon dioxide
Phosphorus trichloride