Chapter 4 Compounds and Stoichiometry

Question 1

A mole

Answer 1

a quantity of any substance (atoms, molecules, dollar bills) equal to the number of particles that are found in 12 grams of carbon-12.

Question 2

Avogadro’s number

Answer 2

6.022X10^23mol-1

Question 3

Molar mass

Answer 3

the mass of one mole of a compound; usually measured in grams per mole.

Question 4

Moles=

Answer 4

Mass of sample(g)/ Molar mass (g/mol)

Question 5

Gram equivalent weight

Answer 5

a measure of the mass of a substance that can donate one equivalent of the species of interest.
Molar mass/n
n=number of particles of interest

Question 6

Normality=

Answer 6

the ratio of equivalents per liter; it is related to molarity by multiplying the molarity by the number of equivalents present per mole of compound.

Question 7

Molarity=

Answer 7

number of moles of dissolved solute per liter of solution.
Normality/n

Question 8

Equivalents=

Answer 8

moles of the species of interest; equivalents are most often seen in acid-base chemistry(hydrogen ions or hydroxide ions) and oxidation-reduction reactions(moles of electrons or other ions).
Mass of compound(g)/Gram equivalent weight (g)

Question 9

Empirical Formula

Answer 9

is the smallest whole-number ratio of the elements in a compound

Question 10

Molecular Formula

Answer 10

either the same as or a multiple of the empirical formula; it gives the exact number of atoms of each element in a compound.

Question 11

Percent Composition

Answer 11

Mass of element in formula/Molar mass

Question 12

Combination Reactions

Answer 12

Occur when two or more reactants combine to form one product

Question 13

Decomposition Reactions

Answer 13

Occur when one reactant is chemically broken down into two or more products.

Question 14

Combustion Reactions

Answer 14

Occur when a fuel and an oxidant (typically oxygen) react, forming the products water and carbon dioxide (if the fuel is a hydrocarbon)

Question 15

Displacement Reactions

Answer 15

Occur when one or more atoms or ions of one compound are replaced with one or more atoms or ions of another compound.

Question 16

Single-displacement reactions

Answer 16

Occur when an ion of one compound is replaced with another element.

Question 17

Double-displacement reactions

Answer 17

Occur when elements from two different compounds trade places with each other to form two new compounds.

Question 18

Neutralization reactions

Answer 18

Are those in which an acid reacts with a base to for a salt (and, usually, water).

Question 19

Theoretical yield

Answer 19

is the maximum amount of product that can be generated as predicted from the balanced equation, assuming that all of the limiting reactant is consumed, no side reactions have occurred, and the entire product has been collected.

Question 20

Actual Yield

Answer 20

the amount of product one actually obtains during the reaction.

Question 21

Percent yield=

Answer 21

Actual yield/Theoretical yield

Question 22

Coulomb’s law

Answer 22

The force of attraction or repulsion between two charged bodies is directly proportional to the product of their charges and inversely proportional to the square of the distance between them. The distance between nuclei in ionic bonds is inversely proportional to the force. Therefore, ionic compounds with long bond distances are much more weakly held together.

Question 23

Fe^2+

Answer 23

Ferrous(Iron(ll))

Question 24

Fe^3+ (Iron(lll))

Answer 24

Ferric

Question 25

Cu^+(Copper(l))

Answer 25

Cuprous

Question 26

Cu^2+ (Copper(ll))

Answer 26

Cupric

Question 27

H^-

Answer 27

Hydride

Question 28

F^-

Answer 28

Fluoride

Question 29

O^2-

Answer 29

Oxide

Question 30

S^2-

Answer 30

Sulfide

Question 31

N^3-

Answer 31

Nitride

Question 32

P^3-

Answer 32

Phosphide

Question 33

All monatomic anions end in….

Answer 33

Ide.

Question 34

-ous and -ic endings…….

Answer 34

-ous endings can also be used to indicate lesser charge, while -ic endings indicate greater charge.

Question 35

NO2^-

Answer 35

Nitrite

Question 36

NO3^-

Answer 36

Nitrate

Question 37

SO3^2-

Answer 37

Sulfite

Question 38

SO4^2-

Answer 38

Sulfate

Question 39

Oxyanions

Answer 39

When an element forms two oxyanions, the name of the one with less oxygen ends in -ite, and the one with more oxygen ends in -ate.

Question 40

ClO^-
ClO2^-
ClO3^-
ClO4^-

Answer 40

Hypochlorite
Chlorite
Chlorate
Perchlorate(Hyper)

Question 41

HCO3^-
HSO4^-
H2PO4^-

Answer 41

Hydrogen carbonate or bicarbonate
Hydrogen sulfate or bisulfate
Dihydrogen phosphate

Question 42

NH4^+

Answer 42

Ammonium

Question 43

C2H3O2^-

Answer 43

Acetate

Question 44

CN^-

Answer 44

Cyanide

Question 45

MnO4^-

Answer 45

Permanganate

Question 46

SCN^-

Answer 46

Thiocyanate

Question 47

CrO4^2-

Answer 47

Chromate

Question 48

Cr2O7^2-

Answer 48

Dichromate

Question 49

BO3^3-

Answer 49

Borate

Question 50

What metal is not typically found in nature in their uncharged state because they are highly reactive to moisture. Instead they are found as salts…..

Answer 50

Alkali metals, alkaline earth metals

Question 51

Phosphate

Answer 51

Anion PO4^3-

Question 52

Hypochlorite

Answer 52

Anion ClO^-

Question 53

Ammonium

Answer 53

Cation NH4^+

Question 54

Phosphide

Answer 54

Anion P^3-

Question 55

Bicarbonate

Answer 55

Anion HCO3^-

Question 56

Nitrite

Answer 56

Anion NO2^-

Question 57

Chromium(ll)

Answer 57

Cation Cr^2+

Question 58

1/8

Answer 58

.125

Question 59

2/8

Answer 59

.25

Question 60

3/8

Answer 60

.375

Question 61

4/8

Answer 61

.50

Question 62

5/8

Answer 62

.625

Question 63

1/9

Answer 63

.111

Question 64

2/9

Answer 64

.222

Question 65

3/9

Answer 65

.333

Question 66

Acetone

Answer 66

C3H6O