1. Ionic and Covalent Bonding
Ionic Transfer
Covalent Share

2. What holds bonded atoms together?
Bond when valence electrons interact
The (+) nucleus of one atom attracts the (-) ion from another like magnets

3. Bonds can bend and stretch
Bonds are not really rigid, like the stick in ball and stick models
They act more like springs.

4. Ionic bonds are a transfer of electrons
Ionic Bonds have positively charged ions attracted to negatively charged ion.
Cations (+) are positive, metals
CAT PAWS CATions are PAWsitive
*Anions (-) are negative, non-metals
Metal + Non-Metal have ionic bonds and are therefore call Ionic Compounds

5. Ionic Compounds Are in the form of network solids They are neutral
Each (+) and (-) ion form a formula unit

6. Characteristics of Ionic Compounds
High Melting points
Strong Bonds
Brittle
Dissolve in water
Solid states do not conduct electricity
Liquid state does conduct electricity

7. Metallic Bonds Conduct Electricity Flexible Ductile Malleable
“Sea” of electrons formed

8. Covalent Bonding
A covalent bond is formed by a shared pair of electrons between two atoms.

9. Molecules Share more than 1 pair of electrons
Bonds may be…..
Single- 1 shared electron pair represented by 1 line. Requires some energy to break
Double- 2 shared electron pair represented by 2 lines. Requires more energy to break
Triple-3 shared electron pair represented by 3 lines. Requires the most energy to break

10. Polarity Polar means two opposite ends
Not all electron pairs are shared the same
They are attracted to one nucleus more than the other
This is a polar covalent bond

11. Ionic Compounds Polyatomic ions Poly- means many or more than one
These are two or more atoms bonded together with an overall charge
Most polyatomic ions are negative
Parentheses will group polyatomics in a compound Mg(NO3)2
An –ate ending means there is an oxygen atom involved in the polyatomic ion