1. BONDING AND NOMENCLATURE
A ReView

2. REVIEW State the main reason why chemical bonding occurs.
Chemical bonding occurs because atoms want CHEMICAL STABILITY. They want a Noble Gas valence electron number.
The atom gets a full energy level by losing or gaining electrons to form an octet.
This is the most stable formation.

3. REVIEW 2. Describe chemical stability.
describes an atom whose outer energy level is completely filled with all the electrons allowed at that level (a Noble Gas number of electrons).

4. REVIEW 3. Describe ionic bonds and what happens to the electrons.
involves a TRANSFER of electrons from one atom to another.
is held together by electric/electrostatic force (+/-).
happens between positive ions and negative ions.

5. REVIEW 4. Describe covalent bonds and what happens to the electrons.
Atoms with similar electron affinities tend to SHARE electrons.
There are not enough electrons for each individual atom to have a full octet. Neither atom wants to lose electrons; both want to gain them.

6. REVIEW
5. Compare and contrast ionic and covalent bonds.

7. REVIEW
6. Distinguish between a nonpolar molecule and a polar molecule.
Nonpolar molecule: molecule that shares electrons equally and does not have oppositely charged ends.
Polar Molecule: molecule with a slightly positive end and a slightly negative end as a result of electrons being shared unequally.

8. REVIEW A chemical formula tells: what type of atoms are present.
7. Explain what a chemical formula represents.
A chemical formula tells:
what type of atoms are present.
the number of each type of atom present.
ratio of one atom to another.
H2O Cl2 Al2O3

9. REVIEW
8. Determine the ions forms by representative elements.

10. REVIEW
9. Write the names and formulas for ionic compounds.

11. REVIEW 9. Write the names and formulas for ionic compounds.
Potassium fluoride CaS
Nickel (II) phosphide K2S
Aluminum chloride Na3P
Iron (III) oxide BaI2

12. REVIEW
10. Be able to use some representative polyatomic ions in nomenclature.
Nickel (II) nitrate CaSO4
Aluminum carbonate NaHCO3
Magnesium hydroxide NH4Cl

13. copper (II) sulfate pentahydrate
REVIEW
11. Write the names and formulas for hydrates.
Example: CuSO4  5H2O
ionic compound prefix+hydrate
copper (II) sulfate pentahydrate
CaCl2 ∙ 2H2O
Iron (II) sulfate hexahydrate

14. REVIEW 12. Write the names and formulas for covalent compounds. Rules:
Use prefixes to identify the number of atoms present.
If only one of the first atom (nonmetal), then NO prefix is used.
Last element ends in “ide”.
1. Write the symbol of the first element adding a subscript of the number of atoms present. If only one of the first atom (nonmetal), then NO number is used.
2. Write the symbol of the second element adding a subscript of the number of atoms present.

15. REVIEW 12. Write the names and formulas for covalent compounds.
P4S tricarbon dioxide
NO dinitrogen tetroxide
SCl carbon diselenide
PCl tetraphosphorus heptasulfide

16. REVIEW 13. Know the vocabulary words. 14. Know the four SAT words.
agriculture (n.) farming
arid (adj.) excessively dry
arable (adj.) suitable for growing crops
terrestrial (adj.) relating to the land