1. 6.1 Introduction to Chemical Bonding
Ch. 6 Bonding
6.1 Introduction to Chemical Bonding

2. Chemical Bonds atoms rarely exist alone
when atoms are bonded together, they have less potential energy and are more stable
What is potential energy?
chemical bond – mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together

3. Ionic Bonds
results from electrical attraction between large numbers of cations and anions
atoms donate or accept electrons from each other

4. Covalent Bonds
results from sharing of electron pairs between two atoms
the electrons shared belong to both atoms

5. Covalent Bonds when electrons are shared unevenly Polar Covalent
Nonpolar Covalent
when electrons are shared evenly

6. Ionic vs. Covalent

7. Ionic vs. Covalent
bonding usually does not fall in one category or the other, but somewhere in between
type of bond depends on the elements differences in electronegativities

8. Ionic vs. Covalent Difference in electronegativities
Percent Ionic Character
Ionic
> 1.7
> 50 %
Polar Covalent
0.3 – 1.7
5 – 50 %
Nonpolar Covalent
0 – 0.3
0 – 5 %

9. Polarity Polar- uneven distribution of charge
Show partial charges on structure by using  (lowercase delta)

10. Determine whether each of the following bonds will be:
ionic, polar covalent, OR nonpolar covalent

11. S and H
=0.4
polar covalent
S and Cs
=1.8
ionic
C and Cl
=0.5

12. Cl and Ca
=2.0
ionic
Cl and O
=0.5
polar covalent
Cl and Br
nonpolar covalent

13. Patterns What kind of patterns do you see? metals + nonmetals = ionic
nonmetals + nonmetals = covalent