Chem Exam 1 Material

Front 1

Density =

Back 1

mass / volume

Unit: kg/m^3

density of water = 1g/cm^3 or 1kg/L

Front 2

Tera (T)

Back 2

10^12

Front 3

giga (G)

Back 3

10^9

Front 4

mega (M)

Back 4

10^6

Front 5

kilo (k)

Back 5

10^3

Front 6

deci (d)

Back 6

10^-1

Front 7

centi (c)

Back 7

10^-2

Front 8

milli (m)

Back 8

10^-3

Front 9

micro (u)

Back 9

10^-6

Front 10

nano (n)

Back 10

10^-9

Front 11

pico (p)

Back 11

10^-12

Front 12

Celcius to Fahrenheit

Back 12

degrees in C x 1.8 + 32

Front 13

Fahrenheit to Celcius

Back 13

degrees in F -32 / 1.8

Front 14

?K

Back 14

K = C + 273.15

O degrees K = -273.15 degrees C

Front 15

1 lb = ? g

Back 15

453.6 g

Front 16

1 in = ? cm

Back 16

2.54 cm

Front 17

1 mi = ? km

Back 17

1.609 km

Front 18

1 km = ? mi

Back 18

0.6515 mi

Front 19

Avogadro's number (N>A)

Back 19

6.022 x 10^23

Front 20

C2H6

Back 20

Ethane

Front 21

C3H8

Back 21

Propane

Front 22

C4H10

Back 22

Butane

Front 23

C5H12

Back 23

Pentane

Front 24

C6H14

Back 24

Hexane

Front 25

C7H16

Back 25

Heptane

Front 26

C8H18

Back 26

Octane

Front 27

C9H20

Back 27

Nonane

Front 28

C10H22

Back 28

Decane

Front 29

NH4+

Back 29

ammonium

Front 30

NO3-

Back 30

nitrate

Front 31

PO4^3-

Back 31

phosphate

Front 32

CO3^2-

Back 32

carbonate

Front 33

SO4^2-

Back 33

sulfate

Front 34

CH4

Back 34

Methane

Front 35

Cations

NH4+

Back 35

Ammonium

Front 36

H3O+

Back 36

Hydronium

Front 37

Hg2^2+

Back 37

Mercury (I)

Front 38

Anions

C2H3O2-

Back 38

Acetate

Front 39

N3-

Back 39

Azide

Front 40

CO3^2-

Back 40

Carbonate

Front 41

ClO3-

Back 41

Chlorate

Front 42

ClO2-

Back 42

Chlorite

Front 43

CrO4^2-

Back 43

Chromate

Front 44

CN-

Back 44

Cyanide

Front 45

Cr2O7^2-

Back 45

dichromate

Front 46

H2PO4-

Back 46

dihydrogen phosphate

Front 47

HCO3-

Back 47

Hydrogen carbonate or bicarbonate

Front 48

HPO4^2-

Back 48

Hydrogen phosphate

Front 49

HSO4-

Back 49

Hydrogen sulfate or bisulfate

Front 50

OH-

Back 50

hydroxide

Front 51

ClO-

Back 51

hypochlorite

Front 52

NO3-

Back 52

Nitrate

Front 53

NO2-

Back 53

Nitrite

Front 54

C2O4^2-

Back 54

Oxalate

Front 55

ClO4-

Back 55

perchlorate

Front 56

MnO4-

Back 56

permanganate

Front 57

O2^2-

Back 57

peroxide

Front 58

PO4^3

Back 58

phosphate

Front 59

PO3^3-

Back 59

phosphite

Front 60

SO4^2-

Back 60

sulfate

Front 61

SO3^2-

Back 61

Sulfite

Front 62

SCN-

Back 62

thiocyanate

Front 63

1 meter = ? Inches

Back 63

39.4 inches

Front 64

1 kg = ? Grams

Back 64

1000 grams

Front 65

1 kg = ? Grams

Back 65

1000 grams

Front 66

1 kg = ? Lbs

Back 66

2.20 lbs

Front 67

1 lb = ? Grams

Back 67

454 grams

Front 68

Mixture

Back 68

Two or more substances are physically mixed, but not chemically combined

Front 69

Compound

Back 69

Pure substances consisting of two or more elements always in the same proportion. Ex: H2O

Front 70

Homogenous mixture

Back 70

Aka: solution: composition is uniform throughout the sample. Ex: air

Front 71

Heterogeneous mixture

Back 71

The components do not have a uniform composition throughout the sample. Ex: mixture of oil and water

Front 72

Atomic number

Back 72

Is equal to the number of protons in the nucleus of an atom and is used to identify each element

Front 73

Mass number

Back 73

Mass number = # of protons + # of neutrons

Front 74

Isotopes

Back 74

Atoms of the same element that have different numbers of neutrons. This causes their mass numbers to differ but not their chemical behavior. Atomic symbol has mass on top left and atomic number bottom left

Front 75

Cations

Back 75

Metals in ionic compounds lose their valence electrons to form positively charged ions

Front 76

Anions

Back 76

nonmetals form negative ions when they gain electrons to attain an octet (8 valence electrons)

Front 77

Ionic Compounds

Back 77

consist of positive and negative ions, held together by strong attractions between oppositely charged ions called ionic bonds

Front 78

Naming Ionic Compounds

Back 78

cation (metal) by its element name, anion (nonmetal) by its name with ending replaced with -ide

ex: Sodium Fluoride

Front 79

Metals with a variable charge

Back 79

transition metals typically form two or more kinds of positive ions because they lose their outer electrons as well as electrons from a lower energy level

ex: Cu+ = Copper (I)

Fe^2+ = Iron (II), etc.

Front 80

Polyatomic Ions

Back 80

an ionic compound with 3 or more elements

only one is positively charged: NH4+

Front 81

Naming Polyatomic Ions

Back 81

most end in -ate, the -ite ending is used for the names of related ions that have one less O atom

Front 82

Bases

Back 82

(Arrhenius theory) are ionic compounds that dissociate into a metal ion and hydroxide ions (OH-) when they dissolve in water

Front 83

Typical bases

Back 83

named hydroxides:

NaOH ; Sodium hydroxide

KOH ; Potassium hydroxide

Ca(OH)2 ; Calcium hydroxide, etc.

Front 84

Acids

Back 84

substances that produce H+ when they dissolve in water

Front 85

Naming Acids

Back 85

when an acid dissolves in water to produce hydrogen ion and a simple nonmetal anion, the prefix hydro is used before the name of the nonmetal and its -ide ending is changed to acid

ex: HCl ; hydrochloric acid

HNO3 ; nitric acid

H2SO4 ; sulfuric acid

Front 86

Hydrates

Back 86

Compounds that incorporate one or more H2O

ex: LiCl.H2O (.) means hydrate ; monohydrate

BaCl.2H20 ; dihydrate

Front 87

Alcohols

Back 87

Class of organic compounds that contains the hydroxyl (-OH) group bonded to a carbon atom

ex: CH3OH ; methanol

CH3CH2OH ; ethanol

Front 88

Carboxylic Acid

Back 88

contain -COOH

ex: CH3CH2COOH ; propanoic acid

Front 89

Finding the Limiting Reactant

Back 89

Convert all info to moles (grams given in problem divided by the molar mass of the element or compound

Whichever number is smaller is your limiting reactant

Front 90

Finding the empirical formula

Back 90

1. Convert all info to moles

2. divide all answers by the smallest answer=this equals your ratio for the empirical formula

Front 91

Finding standard (molecular) formula

Back 91

Figure out molar mass of entire compound

determine what amount that is compared to the amount given in the problem (ex: 270g/mol given and the molar mass is about 135g this means that you need to double the empirical formula NaS2O3 = Na2S4O6

Front 92

Calculating theoretical yield

Back 92

take the amount of limiting reactant X the molar mass of the compound = answer in grams

Front 93

Calculating percent yield

Back 93

take grams given in question (actual yield) and divide by theoretical yield answer X 100