Chemistry Notes

1
Chemistry Notes

• Covalent Bonding Diagrams

2
An Addendum to Lewis Structures

• Carbon and silicon are exceptions to the pattern
  of how to place electrons in a Lewis Dot
  Structure.

3
An Addendum to Lewis Structures

• This is because they have hybrid orbitals (where
  the s and p sublevels blend together and have
  four equal energy orbitals.)

4
Covalent Bonding

• A covalent bond occurs between two non-metals
• Electrostatic bonding does not occurin other
  words, there is no give and take of electrons

5
It ends up being a tug of war of electrons
Where the electrons end up somewhere in the
middle.
6
Single Bonds

• A single bond occurs when one pair of electrons
  is shared by two atoms.
• This pair of bonded electrons is called a shared
  pair.

7
Double and Triple Bonds

• Double bonds occur when two atoms have two shared
  pair of electrons
• Triple bonds occur when two atoms share three
  pair of electrons

8
Covalent Bonding Diagrams

• Like the ionic bonding diagrams, first draw the
  dot diagram for each element
• Now, however, the electrons are not being given
  away or taken, but shared so signify a pair
  being shared by circling both electrons.

9
Covalent Bonding Diagrams

• Every element should have eight electrons (count
  each shared pair as two).
• If there is more than one of each element in the
  compound, you have to have a central atom.

10
Covalent Bonding Diagrams

• The center atom will be the one with the most
  spots to bond to.

11
Hydrogen

• Since hydrogen is in the first energy level, it
  will not need 8 valence electrons to be stableit
  will only need 2.

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H2
13
H2O
14
Cl2
15
O2
16
N2
17
CCl4
18
CO2
19
HCN
20
PCl3
21
H2O2
22
C2H4
23
CSF2
24
CO