Types of bonds

1
Types of bonds

• Ionic
• Covalent
• metallic

2
Covalent bonding

• Results from the sharing of electrons pairs
  between two atoms.

3
Covalent bonding

• Electronegativity difference
• Bonding story
• Bond length
• Bond energy
• Octet

4
Octet exceptions

• H
• B
• S
• Xe

5
Metallic bonding

• Bonding that results from the attraction between
  metal atoms and the surrounding sea of
  electrons
• Delocalized electrons electrons that freely
  move around empty orbitals overlap, electrons
  very mobile making a sea of electrons

6
Metallic bonds

• Sea of electrons
• Metallic properties
• Luster
• Malleability
• Ductility
• Heat of vaporization

7
Lewis structures

• Valence electrons by dots.
• Lone pair unshared pair

8
Multiple bonds

• Single bond
• Double bond
• Triple bond
• Strength?

9
How can you tell if a bond is ionic or covalent?

• A bond is rarely purely ionic or covalent.
  Usually falls somewhere between the two extremes.
• Diatomic covalent

10
electronegativity

• Measure of an atoms ability to attract
  electrons.
• The degree to which bond is ionic or covalent
  depends on the difference in electronegativities.

11
How to do

• Look up the electronegativities of the atoms
  involved on a chart.
• Subtract the two numbers
• Find where they fall on the ionic- covalent scale.

12
Polar

• Polar an unequal sharing of electrons that
  lends a molecule to be partially negative at one
  end and partially positive at another. Water is
  an example.

13
Reading the chart

• Values above 1.7 are ionic, the closer you are to
  3.3 the more ionic.
• Values under 1.7 are covalent.
• Values under 0.3 are nonpolar -covalent
• Values between 1.7 and .3 are polar -covalent