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AP chem > chapter 1 - 3 > Flashcards

chapter 1 - 3 Flashcards

1
Q

acetate

A

C2H3O2(-)

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2
Q

BrO2(-)

A

bromite

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3
Q

ClO4(-)

A

perchlorate

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4
Q

hypochlorite

A

ClO(-)

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5
Q

BrO3(-)

A

bromate

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6
Q

bromite

A

BrO2(-)

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7
Q

C2H3O2(-)

A

acetate

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8
Q

BrO4(-)

A

perbromate

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9
Q

C2O4(2-)

A

oxalate

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10
Q

bisulfite

A

HSO3(-)

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11
Q

bisulfate

A

HSO4(-)

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12
Q

bicarbonate

A

HCO3(-)

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13
Q

bisulfide

A

HS(-)

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14
Q

bromate

A

BrO3(-)

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15
Q

ammonium

A

NH4(+)

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16
Q

BrO(-)

A

hypobromite

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17
Q

accuracy

A

how close to accepted value

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18
Q

alkali metals

A

1+ charge (hydrogen is not alkali)

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19
Q

alkaline earth metals

A

2+ charge

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20
Q

anion

A

negatively charged ion

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21
Q

atomic mass

A

average of all isotopes; mass of atom in amu; addition of protons and neutrons

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22
Q

atomic number

A

(Z) number of protons

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23
Q

avogadro’s number

A

6.022*10^23atoms/1mol

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24
Q

ball and stick model

A

the kind that you use in a lab with a ball and then a long stick showing a bond

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25
Q

binary compounds

A

a compound containing two elements

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26
Q

carbonate

A

CO3(2-)

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27
Q

j.j thomson

A

cathode ray tubes which emanated from the negative electrode and was repelled by the negative pole. He postulated that it was a stream of negatively charged particles (electrons). He measured the charge to mass ratio; plum pudding model - electrons are like raisins dispersed in a pudding of positive charge

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28
Q

cation

A

positively charged ions

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29
Q

chlorate

A

ClO3(-)

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30
Q

chemical change

A

can only be observed when a substance is changed into another substance. ex: flammability, corrosiveness, reactivity

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31
Q

chemical formula

A

shows the number of each element in the molecule.

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32
Q

chlorite

A

ClO2(-)

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33
Q

chromate

A

CrO4(2-)

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34
Q

chromatography

A

physical process; separates substances on the bases of differences in the ability of substances to adhere to the solid surface; ink chromatography - dyes to a paper

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35
Q

chromium ion

A

Cr3+

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36
Q

ClO(-)

A

hypochlorite

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37
Q

ClO2(-)

A

chlorite

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38
Q

ClO3(-)

A

chlorate

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39
Q

CO3(2-)

A

carbonate

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40
Q

compounds

A

made up of two or more different kind of elements

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41
Q

Copper ion charges

A

2+, 1+

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42
Q

covalent bonds

A

bonds between atoms by sharing electrons; result is called a molecule; occurs between two nonmetals

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43
Q

Cr2O7(2-)

A

dichromate

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44
Q

CrO4(2-)

A

chromate

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45
Q

dalton

A

created law of multiple proportions; dalton’s atomic theory: each element is made up of atoms, atoms of an element are identical, chemical compounds are formed when different elements combine with on another, chemical reaction involve the reorganization of elements

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46
Q

density

A

mass per unit volume; D=m/V; common unites are g/mL, g/cm^3

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47
Q

determinate error

A

systematic error; all results are skewed in one direction

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48
Q

dichromate

A

Cr2O7(2-)

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49
Q

distillation

A

physical process; uses the differences in volatility of substances to separate a homogeneous mixture into its components; heat the substance and as one component boils it rises and goes through cooling chamber which then returns it into liquid into another container.

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50
Q

electrolysis of water

A

chemical process; using electricity to decompose water into oxygen and hydrogen gas

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51
Q

empirical formula

A

when the ratio of molecules is most simplified

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52
Q

ending for monatomic anions

A

-ide

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53
Q

fahrenheit to celsius

A

F=9/5(C)+32

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54
Q

filtration

A

physical process; pour mixture through a filter which separates liquids from solids

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55
Q

elements

A

made up of a unique kind of atom

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56
Q

gas

A

spread very far apart; a lot of mobility

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57
Q

H3O(+)

A

hydronium

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58
Q

halogens

A

1- charge; form diatomic molecules

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59
Q

HCO3(-)

A

bicarbonate

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60
Q

heterogeneous

A

the mixture is not uniform throughout

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61
Q

homogeneous

A

is uniform throughout; if it has a variable composition it will be a homogenous mixture

62
Q

how do you name an acid if the anion does contain oxygen?

A

if the anion ends in -ate you change it to the suffix -ic; if the anion ends in -ite you change it to the suffix -ous.

63
Q

how do you name an acid if the anion does not contain oxygen?

A

add the prefix hydro- and the suffix -ic

64
Q

HS(-)

A

bisulfide

65
Q

HSO3(-)

A

bisulfite

66
Q

HSO4(-)

A

bisulfate

67
Q

hydronium

A

H3O(+)

68
Q

hydroxide

A

OH(-)

69
Q

hypobromite

A

BrO(-)

70
Q

hypoiodite

A

IO(-)

71
Q

indeterminate error

A

random error; can never be perfect!

72
Q

IO(-)

A

hypoiodite

73
Q

IO2(-)

A

iodite

74
Q

IO3(-)

A

iodate

75
Q

IO4(-)

A

periodate

76
Q

iodate

A

IO3(-)

77
Q

iodite

A

IO2(-)

78
Q

ion

A

atoms or group of atoms that has a net positive or negative charge

79
Q

ionic bonding

A

bonds form due to force of attraction between oppositely charged ions

80
Q

ionic solid

A

A solid consisting of oppositely charged ions

81
Q

iron ion charges

A

3+, 2+

82
Q

isotopes

A

atoms with same number of protons but different number of neutrons; same chemical properties

83
Q

kelvin to celsius

A

K=C+273.15

84
Q

law of conservation of mass

A

total mass is not changed by a chemical change

85
Q

law of definite porportion

A

if you combine H and O in the ratio 2:1 you will get water. water will always have that ratio. the ratio of compounds will always be the same.

86
Q

law of multiple proportions

A

if two elements form more than one compound, then the ratios of the masses of the second element which combine with a fixed mass of the first element will always be ratios of small whole numbers.

87
Q

lead ion charge

A

2+

88
Q

electron

A

found outside the nucleus; negatively charged; determines chemical properties

89
Q

length

A

base unit is the meter; measure of distance

90
Q

liquid

A

molecules spread farther apart, more mobility

91
Q

manganese ion charge

A

2+

92
Q

mass

A

measured in kg; a measure of the amount of material n an object

93
Q

mass percent of an element

A

(mass of element in a compound/mass of compound)*100%

94
Q

matter

A

anything that has mass and takes up space

95
Q

mercury ion charge

A

Hg(2+); Hg2(2+)

96
Q

metals

A

Metals have characteristic physical properties such as efficient conduction of heat and electricity, malleability (they can be hammered into thin sheets), ductility (they can be pulled into wires), and (often) a lustrous appearance. Chemically, metals tend to lose electrons to form positive ions.

97
Q

metals that form more than one cation

A

observed for most transition metals, many actinides, and the heaviest elements of groups 13–15

98
Q

metals that form only one cation

A

usually in groups 1-3,12,13

99
Q

milikan

A

performed experiments including charged oil drops, allowed him to determine the magnitude of the electron charge and the mass of the electron from thomson’s charge to mass ratio.

100
Q

mixture

A

a material made up of two or more different chemical substances which are not chemically bonded; can be separated using physical methods

101
Q

MnO4(-)

A

permanganate

102
Q

naming oxyanions

A

In cases where only two oxyanions are known for an element, the name of the oxyanion with more oxygen atoms ends in -ate, and the name of the oxyanion with fewer oxygen atoms ends in -ite; The halogens and some of the transition metals form more extensive series of oxyanions with as many as four members. In the names of these oxyanions, the prefix per- is used to identify the oxyanion with the most oxygen (so that ClO4− is perchlorate and ClO3− is chlorate), and the prefix hypo- is used to identify the anion with the fewest oxygen (ClO2− is chlorite and ClO− is hypochlorite).

103
Q

neutron

A

neutral charge

104
Q

NH4(+)

A

ammonium

105
Q

Nickel ion charge

A

2+

106
Q

nitrate

A

NO3(-)

107
Q

nitrite

A

NO2(-)

108
Q

NO2(-)

A

nitrite

109
Q

NO3(-)

A

nitrate

110
Q

noble gases

A

0 charge

111
Q

nonmetals

A

they tend to gain electrons in reactions with metals to form
negative ions. Nonmetals often bond to each other by forming covalent bonds.

112
Q

rutherford

A

directed alpha particles (positively charged particles) to thin sheet of metal foil; most of the particles passed through but some were deflected at large angles; created the model of the nuclear atom - dense center of positive charge (the nucleus)

113
Q

nucleus

A

small compared to the overall size of the atom; extremely dense - most of the atom’s mass; contains protons and neutrons

114
Q

O2(2-)

A

peroxide

115
Q

OH(-)

A

hydroxide

116
Q

order for naming ionic compounds

A

cation first, then anion

117
Q

oxalate

A

C2O4(2-)

118
Q

oxyanions

A

Polyatomic anions that contain a single metal or nonmetal atom plus one or more oxygen atoms

119
Q

perbromate

A

BrO4(-)

120
Q

percent yield

A

(actual yield/theoretical yield)*100%

121
Q

percent yield

A

(actual yield/theoretical yield)*100%

122
Q

perchlorate

A

ClO4(-)

123
Q

period

A

horizontal rows of elements

124
Q

periodate

A

IO4(-)

125
Q

permanganate

A

MnO4(-)

126
Q

peroxide

A

O2(2-)

127
Q

phosphate

A

PO4(3-)

128
Q

phosphite

A

PO3(3-)

129
Q

physical change

A

can be observed without changing a substance into another substance. ex: boiling point, density, mass ,volume

130
Q

PO3(3-)

A

phosphite

131
Q

PO4(3-)

A

phosphate

132
Q

proton

A

determines that atoms identity; found in the nucleus; always the same number as electrons for neutral atom.

133
Q

pure substance

A

it is homogenous and it has only one variable composition; has constant composition

134
Q

precision

A

proximity of several measurements to each other

135
Q

groups/families

A

elements in the same vertical columns; have similar chemical properties

136
Q

S2O3(2-)

A

thiosulfate

137
Q

SCN(-)

A

thiocyanate

138
Q

silver ion charge

A

+

139
Q

SO3(2-)

A

sulfite

140
Q

SO4(2-)

A

sulfate

141
Q

solid

A

typically most dense (not true of water)

142
Q

solution

A

a homogenous mixture

143
Q

space filling model

A

is when atoms are shown as round balls and they are all kinds touching.

144
Q

structural formula

A

the diagram showing how the molecule is bonded.

145
Q

sulfate

A

SO4(2-)

146
Q

sulfite

A

SO3(2-)

147
Q

thiocyanate

A

SCN(-)

148
Q

thiosulfate

A

S2O3(2-)

149
Q

tin ion charge

A

2+; 4+

150
Q

volatility

A

how readily substances become gasses; used in distillation

151
Q

weight

A

the force acting on the object due to gravity

152
Q

zinc ion charge

A

2+

AP chem (3 decks)

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