Sem 2 Final

Question 1

Acid Naming and Formulas
Hydro___ic acid?

Answer 1

-Nonmetal ends in “ide”
-ex. hydrofluoric acid

Question 2

Acid Naming and Formulas
___ic acid?

Answer 2

-Nonmetal ending is “ate”
-ex. sulfuric acid

Question 3

Acid Naming and Formulas
___ous acid?

Answer 3

-Nonmetal ending is “ite”
-ex. sulfurous acid

Question 4

What is a neutralization reaction?

Answer 4

A reaction between an acid and a base
-water will always be a product

Question 5

Net Ionics
-define electrolytes

Answer 5

-ionic compounds dissolved in water, their ions will conduct electricity

Question 6

Net Ionics
-what is a precipitate?

Answer 6

The water-insoluble product formed from precipitate reactions
-If an ionic compound forms a solid, it is a precipitate

Question 7

Net Ionics
-what are spectator ions?

Answer 7

Ions that appear on both side of the reaction

Question 8

How do you write net ionic equations?
(what are the steps?)

Answer 8

1. Balanced Formula Equation
2. Determine the Solubility
3. Aq. (soluble)- split the compound, add charges. Subscripts become coeffs, mult subscripts and balance equation
4. cancel spectator ions
5. rewrite including state of matter symbols and omit spectator ions

Question 9

What is a redox reaction?

Answer 9

A reaction involving the transfer of electrons
-ex. batteries, light bulbs, rusting, everything electrical
-reactions always occur on the negative end

Question 10

What is oxidation?

Answer 10

the loss of e-

Question 11

What is reduction?

Answer 11

the gain of e-

Question 12

Remember….

Answer 12

OIL RIG!
-Oxidation Is Losing
-Reduction Is Gaining

Question 13

Oxidation numbers

Answer 13

Signifies the number of charges an atom would have in a molecular or ionic compound if the e- were transferred completely

Question 14

Rules for Assigning Oxidation Numbers

Answer 14

1. Each atom in a pure element has an oxidation value of 0
   -ex. diatomics
2. Monatomic ions have oxidation numbers equal to their charge
   -ex. Mg+2= +2
3. Metals- their charge is their oxidation number
   -ex. NaCl, Na=+1, Cl=-1
4. Oxidation number for H is +1, O is -2 in most compounds
   a. When H forms acids, +1, when it isn’t an acid, -1
   b. H2O2 O=-1
5. Sum of ox. #s must be 0 for a neutral compound, for polyatomics it must be equal to the ion charge
6. F, Cl, Br, and I always have an ox. # of -1 except when combined with Oxygen