Exam 1

Question 1

How do you calculate solute?

Answer 1

M1V1= M2V2 so V1=M2V2/M1

Question 2

How do you determine the reduced and oxidized elements?

Answer 2

The compound that GAINS charge is oxidized and is therefore the reducing agent

The compound that LOSES charge is reduced and is therefore the oxidizing agent

Question 3

What salts are soluble? (hint: there are 4 rules)

Answer 3

Compounds containing alkali metal ions (Li+, Na+, K+, Rb+, Cs+) and the ammonium ion (NH4+)
Nitrates (NO3-), Bicarbonates (HCO3-), and Chlorates (ClO3-)
Halides (Cl-, Br-, I-) EXCEPT Ag+, Hg2 +2, and Pb+2)
Sulfates (SO4 -2) EXCEPT sulfates of Ag+, Ca +2, Sr +2, Ba +2, Hg2 +2, and Pb +2

Question 4

What compounds are insoluble? (hint: there are two rule)

Answer 4

Carbonates (CO3 -2), Phosphates (PO4 -3), Chromates (CrO4 -2), and Sulfides (S -2) EXCEPT Compounds containing alkali metal ions (Li+, Na+, K+, Rb+, Cs+) and the ammonium ion (NH4+)

Hydroxides (OH-) EXCEPT Compounds containing alkali metal ions (Li+, Na+, K+, Rb+, Cs+) and the Ba+2 ion

Question 5

How do you calculate molarity?

Answer 5

moles/volume= Molarity

Question 6

What is the unit of 1 mole?

Answer 6

6.02 x 10^23

Question 7

What is the first rule for naming ionic compounds?

Answer 7

Major Metal Group + Non-Metal

Ex: NaCl = sodium chloride

Question 8

What is the second rule for naming ionic compounds?

Answer 8

Non-major Group Metal + Non-Metal

Ex: CuO + copper (II) oxide vs Cu2O = Copper (I) Oxide

Question 9

What is the rule for naming covalent compounds (non-metal + non-metal)?

Answer 9

mono= one
di= 2
tri= 3
etc.

Question 10

What oxoanions follow this naming pattern: hypo—ite?

Answer 10

ClO- (hypochlorite)
BO- (hypobromite)
IO- (hypoiodite)

Question 11

What oxoanions follow this naming pattern: —ite?

Answer 11

ClO2- (chlorite)
BrO2- (bromite)
IO2- (iodite)
NO2- (nitrite)
SO3 2-(sulfite)
PO3 3-(phosphite)

Question 12

What oxoanions follow this naming pattern: —ate?

Answer 12

ClO3- (chlorate)
BrO3- (bromate)
IO3- (Iodate)
NO3- (Nitrate)
SO4 2-(Sulfate)
PO4 3- (Phosphate)
CO3 2-(Carbonate)

Question 13

What oxoanions follow this naming pattern: per—ate?

Answer 13

ClO4- (perchlorate)
BrO4- (perbromate)
IO4- (Periodate)

Question 14

What do hypo—ite oxoanions become when they contain acids?

Answer 14

hypo—ous acid (add the H before the compound)

Question 15

What do —ite oxoanions become when they contain acids?

Answer 15

—ous acid (add the H before the compound)

Question 16

What do —ate oxoanions become when they contain acids?

Answer 16

—ic acid (add the H before the compound)

Question 17

What do per—ate oxoanions become when they contain acids?

Answer 17

per—ic acid (add the H before the compound)

Question 18

10^9?

Answer 18

G (giga)

Question 19

10^6?

Answer 19

M (mega)

Question 20

10^3?

Answer 20

k (kilo)

Question 21

10^-2?

Answer 21

c (centi)

Question 22

10^-3?

Answer 22

m (milli)

Question 23

10^-6?

Answer 23

u (micro)

Question 24

10^-9?

Answer 24

n (nano)

Question 25

10^-12?

Answer 25

p (pico)

Question 26

What are the rules for assigning oxidation numbers?

Answer 26

1. The sum of the oxidation numbers of all the atoms in a species must equal the net charge of the species 2.In compounds, the oxidation number of the metals in Group 1A is +1, Group 2A is +2, Boron and Aluminum is +3, and Fluorine is -1 3. In compounds, the oxidation number of hydrogen is +1 4. In compounds, the oxidation number of oxygen is -2