1. Chemical Bonding

2. To Predict the nature of a chemical bond using electronegativities
How to form ions to stable electron configurations
How to predict physical properties based upon bonding (mp, etc.)‏
How to write Lewis Structures and multiple bonding
What is VSEPR Theory, and how is it used to predict the geometry of a molecule
What is Bond Polarity and how do we predict solubility in polar and non-polar solvents

3. Force that holds two atoms together
Formed by the attraction of a positive ion for a negative ion or by sharing electrons.

4. Ionic Radius K Cl- K+ Cl Anions Negative Ion (O2- ) Non-metals
Cations
Anions
Positive Ion (Be 2+)
Metals
Lose electrons
Radius gets smaller!
Negative Ion (O2- )
Non-metals
Add electrons
Radius gets larger! K
Cl- K+ Cl

5. Periodic Table Organization
Metalloids
Metals
Non-Metals

6. Metals and Non-metals Non-metals Metals Dull Brittle Poor conductors
Shiny
Malleable
Ductile (pulled into wires)
Conduct heat and electricity
Low specific heat
High mp / bp
Solids
Lose electrons
Dull
Brittle
Poor conductors
Low melting/boiling points
Varied properties
Varied phases

7. Reaction of a metal with a non-metal Transfer of Electrons
Metal loses electron/s
Non-Metal gains
Bond is an electrostatic attraction of ions
Cation (+)‏
Anion (-)‏
Ionic Bonds

8. Ionic Compounds Conducts electricity Crystal lattice – strong forces
High mp and bp
Hard – not easily crushed

9. Metals and Non-metals Non-metals Metals Dull Brittle Poor conductors
Shiny
Malleable
Ductile (pulled into wires)
Conduct heat and electricity
Low specific heat
High mp / bp
Solids
Lose electrons
Dull
Brittle
Poor conductors
Low melting/boiling points
Varied properties
Varied phases

10. Covalent Compounds Weaker forces between molecules
Odor – volatile liquids and gases– evaporates easily
Lower mp and bp
Softer compounds – more easily ground into powder

11. Covalent Bonding
Reaction of two or more non-metals
Sharing Electrons
Bond is attraction of nuclei to shared electrons

12. Electronegativity Increases
Pull of electrons in a covalent bond
“Attraction” of atoms towards an electron
Fluorine is “the man”
Electronegativity Increases

13. Nature of a chemical bond
Use difference in electronegativities to predict type of bonding
Nature of a chemical bond
100 %
3.40
1.70
0.00
50 %
0 %
Ionic Character
0.40
Ionic
Non-polar Covalent
Polar Covalent

14. Identify each of the following as either ionic, polar covalent, or non-polar covalent
Fr 0.6 Li 1.0 Na 0.9 H 2.1 C 2.5 O 3.5 Br 2.8 F 4.0 Cl 3.0
LiF CO2
NaCl HCl
Fr2O FrF
CH4 NaBr
4.0 – 1.0 = 3.0
> Ionic
3.5 – 2.5 = 1.0
< 1.7 – Polar Covalent
3.0 – 2.1 = 0.9
< 1.7 – Polar Covalent
3.0 – 0.9 = 2.1
> Ionic
4.0 – 0.6 = 3.4
> Ionic
3.5 – 0.6 = 2.9
> Ionic
2.5 – 2.1 = 0.4
= 0.4– Nonpolar
2.8 – 0.9 = 1.9
> Ionic

15. Reaction of a Metal and Non-Metal
Transfer of electrons from the metal to the non-metal to form noble gas electron configuration
example
Na + Cl Na+ Cl - ▪ :
Metal Loses
Non-Metal Gains

16. K + + F - : : Sr+2 + O -2 : Al+3 + N -3 : : 2 K+ + O -2 : :
Write the equation for each reaction using Lewis Dot Structures:
Octet
Metal loses; Non-metal gains
K + F
Sr + O
Al + N
K + O + K
Cl + Ca + Cl : : ▪
K F -
Sr O -2
Al N -3
2 K O -2
Ca Cl -1 ▪ : ▪ : : : ▪ : ▪ : : ▪ : ▪ ▪ : : ▪ : ▪ :

17. Conducts electricity in aqueous solution
Brittle
High Melting
Strong attraction between ions
Conducts electricity in aqueous solution
ELECTROLYTE
Conducts electricity in the molten state
Ions become mobile