General Chemistry 1101

Front 1

limiting reactant

Back 1

completely consumed in a chemical reaction/limits the amount of products

Front 2

Acetate

Back 2

C2H3O2-

Front 3

Carbonate

Back 3

CO3^2-

Front 4

Hydrogen Carbonate/bicarbonate

Back 4

HCO3^-

Front 5

Hydroxide

Back 5

OH^-

Front 6

Nitrite

Back 6

NO2^-

Front 7

Nitrate

Back 7

NO3^-

Front 8

Chromate

Back 8

CrO4^2-

Front 9

Dichromate

Back 9

Cr2O7^2-

Front 10

Phosphate

Back 10

PO4^3-

Front 11

Hydrogen phosphate

Back 11

HPO4^2-

Front 12

Dihydrogen phosphate

Back 12

H2PO4^-

Front 13

Ammonium

Back 13

NH4^+

Front 14

Hypochlorate

Back 14

ClO-

Front 15

Chlorite

Back 15

ClO2^-

Front 16

Chlorate

Back 16

ClO3^-

Front 17

Perchlorate

Back 17

ClO4^-

Front 18

Permanganate

Back 18

MnO4^-

Front 19

Sulfite

Back 19

SO3^2-

Front 20

Hydrogen sulfite; bisulfite

Back 20

HSO3^-

Front 21

Sulfate

Back 21

SO4^2-

Front 22

Hydrogen Sulfate; bisulfate

Back 22

HSO4^-

Front 23

Cyanide

Back 23

CN-

Front 24

Peroxide

Back 24

O2^2-

Front 25

six strong acids (names)

Back 25

Perchloric acid

Nitric acid

Sulfuric acid

Hydrochloric acid

Hydrobromic acid

Hydrolic acid

Front 26

six strong acids (equations)

Back 26

HClO4

HNO3

H2SO4

HCl

HBr

HI

Front 27

proton

Back 27

charge: +1

mass: 1.67 * 10^-27 kg

Front 28

neutron

Back 28

charge: 0

mass: 1.67 *10^-27

Front 29

electron

Back 29

charge: -1

mass: .00091*10^-27

Front 30

desinty

Back 30

mass/volume

Front 31

intensive property

Back 31

a property independent of the amount of the substance

Front 32

Boyle's law

Back 32

the volume of gas is inversely proportionate to its pressure

Front 33

Charles's law

Back 33

the volume of gas is directly proportionate to its temperature

Front 34

Avogadro's law

Back 34

the volume of a gas is directly proportion to the amount (in moles)

Front 35

ideal gas law

Back 35

PV = nRT

Front 36

oxidizing agent

Back 36

causes the oxidation (losing electrons) of another substance; always reduced

Front 37

acid

Back 37

substance that produces H+ ions in aqueous solution

Front 38

Base

Back 38

substance tat produces OH- ions in aqueous solution

Front 39

molecular equation

Back 39

a chemical equation showing the complete, neutral formulas for every compound in a reaction

Front 40

complete ionic equation

Back 40

showing all of the species as they are actually present in solutions

Front 41

net ionic equation

Back 41

only species that change

Front 42

spectator ions

Back 42

do not participate in the reaction

Front 43

molarity (M)

Back 43

amount of moles in solute / volume of solution in L

Front 44

percent yield

Back 44

(actual yield/theoretical yield) * 100

Front 45

actual yield

Back 45

amount of product actually produced by a chemical reaction

Front 46

theoretical yield

Back 46

amount of a product that can be made in a chemical reaction based in the limiting reactant

Front 47

1 liter = 1,000 mL = 1,000cm^3

Back 47

1 liter = 1.057 qt

Front 48

1 gallon = 3.785 L

Back 48

1Kg = 2.205 lb

Front 49

1 lb = 453.59 g

Back 49

1 oz = 28.35

Front 50

1km = .6214 miles

Back 50

1 meter = 39.37 inches = 1.094 yd

Front 51

1 ft = 30.48 cm

Back 51

1 in = 2.45 cm

Front 52

hydrate prefixes

Back 52

hemi = 1/2

mono = 1

di - 2

tri - 3

tetra - 4

penta - 5

hexa - 6

hepta - 7

octa - 8

Front 53

naming binary molecular compounds (composed of hydrogen and a nonmetal)

Back 53

hydro + base name of nonmetal + ic + acid

Front 54

naming binary molecular compounds

Back 54

prefix + name of first element + prefix + base name of second element + ide

Front 55

volume at STP -> #moles <- volume at STP

Back 55

/ 22.4 and * 22.4

Front 56

mass -> #moles <- mass

Back 56

/ and * atomic mass

Front 57

# particles -> # moles<- # of particles

Back 57

/ and * by 6.02 * 10^23