1. Chemical Bonding
A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together.
Atoms combine to minimize potential energy, which makes them more stable.
It is in the breaking and forming of chemical bonds that the vast majority of Chemistry takes place.

2. Types of Chemical Bonds
Metallic Bonds
Metal bonded with metal
Valence electrons are shared in an electron sea
Ionic Bonds
Metal bonded with nonmetal
Valence electrons are transferred from positive ions to negative ions
Covalent Bonds
Nonmetal bonded with a nonmetal
Valence electrons are shared in electron pairs

3. Ionic Bonding The chemical bonding between metals and nonmetals
  Ionic compound – composed of positive and negative ions that are combined so that the numbers of positive and negative charges are equal.
Bonding between atoms with an electronegativity difference generally greater than 2.0
strongly attracted to each other as a result of the electrostatic forces involved.

4. Let’s Remember
Ionic Bond = Metal + Nonmetal

5. Ionic Bond Continued
In ionic bonds atoms completely give up electrons to other atoms.
There is a transfer of electrons from one atom to the other to form ionic compounds.

6. Ionic Bond Example:
Lithium “gives or transfers” one electron to Fluorine! A new ionic bond is formed :
Lithium Fluoride!

7. Covalent bonds
In covalent bonding, a nonmetal and a nonmetal bond together to form a compound.
The compound is called a molecule.
But rather than losing or gaining electrons, atoms now share an electron pair.

8. Covalent Bonding
Covalent compound - a molecule formed by covalent bonds, in which the atoms share one or more pairs of valence electrons.
Covalent bonds have atoms with electronegativities that are about the same or with a difference that is less than 1.5.

9. Octet Rule
Nonmetal atoms combine so that each atom has a total of eight valence electrons by sharing electrons.
The hydrogen atoms do not follow the octet rule. They have a total of two electrons, similar to the noble gas helium, He.
After bonding, each chlorine atom has a total of eight valence electrons surrounding it.
Cl2
PCl3
H2S

10. Multiple Bonds
Depending on the atoms multiple bonds between nonmetals can form.
If two atoms only share one electron pair (2 e-), the atoms form a single bond.
Ex: F2
If two atoms share two electron pairs (4 e-), the atoms form a double bond.
Ex: O2
If two atoms share three electron pairs (6 e-), atoms form a triple bond.
Ex: N2

11. Covalent Compound Example
Carbon shares its valence electrons with oxygen’s to form two sets of double bonds to form – Carbon Dioxide

12. Metallic Properties
Electrons in metals become “delocalized electrons” from the metal atoms.
The electrons move around the atoms.
This causes metal
s to be good conductors of electricity.
Electricity is the flow of electrons which is already occurring in metals.

13. Metallic Properties Cont.
Metals can be hammered into shape (bend) into thin sheets or other shapes.
This property is called malleability.
Metals can also be drawn into wires.
This is called ductility.

14. Metallic Bonding
Metals hold on to their valence electrons very weakly.
Think of them as positive ions (cations) floating in a sea of electrons.