1. What will be on the test on 10-30?
Chapters 4,5 and 7
Note: You will be given a periodic table and copy of conversions page from the back of the book.
You need to bring a green scantron and you are allowed ½ sheet of paper on which you can write equations, etc.

2. 1. Naming Covalent Compounds See Study Assignment from Lab 2
1. Naming Covalent Compounds See Study Assignment from Lab 2. Lewis Dot structures: See Study Assignment from Lab See also: Resonance and exceptions to the octet rule
Must obey the Octet Rule: the tendency for atoms to seek 8 electrons in their outer shells
Must have the correct number of valence electrons around each atom in the molecule.
Halogens
Like to be terminal
Like to have one single bond and 3 lone pairs (non-bonding electrons)
Carbon
Likes to have 4 single bonds and no lone pairs
A double bond counts as two singles
A triple bond counts as three singles
Likes to be central
Likes to bond to other carbons

3. 2. Lewis Dot structures: Silicon Likes to do what carbon does Oxygen
Likes to have two single bonds and 2 lone pairs
Sulfur
Likes to do what oxygen does, but may expand its octet
Nitrogen
Likes to have 3 single bonds and one lone pair
Phosphorus
Likes to do what nitrogen does, but may expand its octet
Hydrogen
Likes to be terminal with only one single bond
No lone pairs!
Boron
Likes 3 bonds and no lone pairs (sextet-exception to the octet rule)

4. 2. VSEPR Opposite charges attract while like charges repel each other.
Protons and electrons attract each other, but two electrons repel each other.

5. Valence Shell Electron Pair Repulsion Theory
VSEPR theory:
Electrons repel each other
Electrons arrange in a molecule themselves so as to be as far apart as possible
Determines molecular geometry

6. This was removed due to size limits on website…

7. You will need the information from this table only for determining molecular geometry (similar to quiz)

8. 3. Electronegativity
The measure of the ability of an atom to attract electrons to itself
Increases across period (left to right) and
Decreases down group (top to bottom)
fluorine is the most electronegative element
francium is the least electronegative element

9. Non-Polar Covalent Bond:
Types of Bonding
ENCl = 3.0
= 0
Covalent
Non-Polar Covalent Bond:
Difference in electronegativity values of atoms is 0.0 – 0.4
Electrons in molecule are equally shared
Examples: Cl2, H2, CH4
ENCl = 3.0
ENH = 2.1
3.0 – 2.1 = 0.9
Polar Covalent
Polar Covalent Bond:
Difference in electronegativity values of atoms is 0.4 – 2.0
Electrons in the molecule are not equally shared
The atom with the higher EN value pulls the electron cloud towards itself
Partial charges
Examples: HCl, ClF, NO

10. Ionic Bond: Difference in EN above 2.0
ENCl = 3.0
ENNa = 1.0
3.0 – 0.9 = 2.1
Ionic
Ionic Bond:
Difference in EN above 2.0
Complete transfer of electron(s)
Whole charges

12. Molecular Polarity (Examples)

13. Figure 4.5
Examples

14. 5. Molar Mass
The mass, in grams, of one mole of any element or compound
Abbreviated with capital, italicized M
Unit = grams/mole = g/mol
Also called Formula Mass and Formula Weight

15. Chapter 5, continued
Avogadro’s number, calculations involving molecular weight, moles to mass, etc. See Worksheet for Chapter 5 and see related problems at the end of the chapter.

16. 5. Chemical Reactions Writing Chemical Equations
A chemical equation uses chemical formulas and other symbols showing what reactants are the starting materials in a reaction and what products are formed.
The reactants are written on the left.
The products are written on the right.
Coefficients show the number of moles of a given element or compound that react or are formed.

17. 5. Introduction to Chemical Reactions Balancing Chemical Equations
Study assignment for balancing chemical equations.
Page 191 and 193.
stoichiometry, % yield: Calculations using the balanced reaction
See Worksheet and related problems at the end of the chapter. Limiting reagent problems will not be included until the final.

18. Types of reactions: Combination, Decomposition, Single Replacement, Double Replacement
Combustion reaction involves the burning of a compound, usually a hydrocarbon, in oxygen to form heat, carbon dioxide and water

19. 6. Oxidation and Reduction A. General Features
Oxidation is the loss of electrons from an atom.
Reduction is the gain of electrons by an atom.
Both processes occur together in a single reaction called an oxidation−reduction or redox reaction.
A redox reaction always has two components, one that is oxidized and one that is reduced.
A redox reaction involves the transfer of electrons from one element to another.

20. 5. Oxidation and Reduction A. General Features
Zn loses 2 e− to form Zn2+, so Zn is oxidized.
Cu2+ gains 2 e− to form Cu, so Cu2+ is reduced.

21. 5. Oxidation and Reduction A. General Features
Cu2+ gains 2 e−
Zn Cu2+
Zn Cu
Zn loses 2 e–
Each of these processes can be written as an
individual half reaction:
Oxidation half reaction: Zn
Zn e−
loss of e−
Reduction half reaction:
Cu e− Cu
gain of e−

22. 5. Oxidation and Reduction
Zn Cu2+
Zn Cu
oxidized
reduced
A compound that is oxidized while causing another
compound to be reduced is called a reducing agent.
Zn acts as a reducing agent because it causes
Cu2+ to gain electrons and become reduced.

23. 5. Oxidation and Reduction
Zn Cu2+
Zn Cu
oxidized
reduced
A compound that is reduced while causing another
compound to be oxidized is called an oxidizing agent.
Cu2+ acts as an oxidizing agent because it causes
Zn to lose electrons and become oxidized.

24. 5.4 Oxidation and Reduction A. General Features

25. 5, Oxidation and Reduction Examples of Oxidation–Reduction Reactions
Zn MnO2
ZnO Mn2O3

26. Chapter, 7
Properties of Gases
Problems using the Gas Laws: See worksheet…
Intermolecular Forces
Properties related to melting point, boiling point
Anything that is on the power point presentations can be included on the test, except for solubility section (precipitation reactions), and limiting reactant..