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Chemistry 101 > Unit 3 > Flashcards

Unit 3 Flashcards

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1
Q

hydrogen

A

H+

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2
Q

lithium

A

Li+

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3
Q

sodium

A

Na+

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4
Q

potassium

A

K+

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5
Q

rubidium

A

Rb+

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6
Q

cesium

A

Cs+

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7
Q

beryllium

A

Be+2

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8
Q

magnesium

A

Mg+2

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9
Q

calcium

A

Ca+2

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10
Q

strontium

A

Sr+2

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11
Q

Barium

A

Ba+2

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12
Q

aluminum

A

Al+3

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13
Q

silver

A

Ag+

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14
Q

nickel

A

Ni+2

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15
Q

zinc

A

Zn+2

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16
Q

cadmium

A

Cd+2

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17
Q

copper (I)

A

Cu+

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18
Q

copper(II)

A

Cu+2

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19
Q

iron (II)

A

Fe+2

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20
Q

iron(III)

A

Fe+3

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21
Q

tin(II)

A

Sn+2

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22
Q

tin(IV)

A

Sn+4

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23
Q

lead(II)

A

Pb+2

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24
Q

lead(IV)

A

Pb+4

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25
Q

cobalt(II)

A

Co+2

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26
Q

cobalt(III)

A

Co+3

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27
Q

mercury(I)

A

Hg2 +2

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28
Q

mercury(II)

A

Hg+2

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29
Q

ammonium

A

NH4+

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30
Q

suffix change

A

anions

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31
Q

ide, ite, ate

A

anions

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32
Q

hydride

A

H-

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33
Q

fluoride

A

F-

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34
Q

chloride

A

Cl-

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35
Q

bromide

A

Br-

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36
Q

iodide

A

I-

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37
Q

oxide

A

O-2

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38
Q

sulfide

A

S-2

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39
Q

selenide

A

Se-2

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40
Q

telluride

A

Te-2

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41
Q

nitride

A

N-3

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42
Q

phosphide

A

P-3

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43
Q

nitrate

A

NO3-

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44
Q

nitrite

A

NO2-

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45
Q

sulfate

A

SO4 -2

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46
Q

sulfite

A

SO3 -2

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47
Q

hydroxide

A

OH-

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48
Q

acetate

A

CH3CO2

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49
Q

cyanide

A

CN-

50
Q

carbonate

A

CO3 -2

51
Q

hypochlorite

A

CIO-

52
Q

chlorite

A

CIO2-

53
Q

chlorate

A

CIO3-

54
Q

perchlorate

A

CIO4-

55
Q

chromate

A

CrO4 -2

56
Q

dichromate

A

Cr2O7 -2

57
Q

permanganate

A

MnO4 -2

58
Q

bicarbonate

A

HCO3-

59
Q

bisulfate

A

HSO4-

60
Q

bisulfite

A

HSO3-

61
Q

phosphate

A

PO4 -3

62
Q

hydrogen phosphate

A

HPO4 -2

63
Q

dihydrogen phosphate

A

H2PO4-

64
Q

transfer e-

A

ionic bonding

65
Q

metal and nonmetal

A

ionic bonding

66
Q

ionic compound

A

ionic bonding

67
Q

share e-

A

covalent bonding

68
Q

nonmetal and metalloid

A

covalent bonding

69
Q

molecular compound

A

covalent bonding

70
Q

molecular element (7 diatomic elements)

A

covalent bonding

71
Q

size of an atom

A

atomic radii

72
Q

we know atoms are what shape

A

spheres

73
Q

t or f atoms are all the same size

A

false

74
Q

as we move down a group, the atomic radius

A

increases

75
Q

as we move across a period from left - right the atomic radius

A

decreases

76
Q

why does atomic radius increase as we go down a group

A

we have a larger number of energy levels and larger atomic radius because of it

77
Q

why does atomic radii decrease as we move left - right across a period

A

we have a larger number of protons and electrons

78
Q

electrons are pulled closer to nucleus

A

larger attraction

79
Q

radius smaller

A

larger attraction

80
Q

size of monoatomic ions

A

spheres

81
Q

what are smaller than their corresponding atoms

A

cations

82
Q

what are larger than their corresponding atoms

A

anions

83
Q

why are cations smaller than their corresponding atoms

A

with a smaller number of energy, cation has a smaller radius than its corresponding

84
Q

extra electrons cause what

A

some additional repulsions between the electrons

85
Q

what do electrons do to minimize additional repulsions

A

expand outward

86
Q

when electrons expand outward the

A

radius increases

87
Q

same number of electrons

A

isoelectronic series

88
Q

process of removing an electron from an atom is called

A

ionization

89
Q

amount of energy required to remove an electron from an isolated atom in the gas phase

A

ionization energy

90
Q

in each period which elements have the largest ionization energy

A

noble gases

91
Q

in each period which elements have the smallest ionization energy

A

alkai metals

92
Q

in each period which elements have similar ionization energies

A

transition metals

93
Q

why do the noble gases have the largest ionization energies in each period

A

don’t want to lose their NGEC; make removing e- as difficult as possible (large ionization energy)

94
Q

why do alkai metals have the smallest ionization energies

A

want to lose electron to get NGEC so make it as easy as possible; making small ionization energy

95
Q

amount of energy absorbed when an electron is added to an isolated atom in the gas phase

A

electron affinity

96
Q

why do the transition metals within a period all have similar ionization energies

A

lose same e- (same amount of energy, similar ionization energies)

97
Q

tendency of an atom to attract electrons towards itself when chemically combined with other atoms

A

electronegativity

98
Q

atom has a strong desire to attract electrons

A

large electronegativity

99
Q

atom has little desire to attract electrons toward itself

A

small electronegativity

100
Q

e- are shared equally between the 2 atoms; occurs when 2 atoms involved have the same (or similar) electronegativities

A

nonpolar covalent bond

101
Q

small difference in electronegativity

A

nonpolar covalent bond

102
Q

electrons are shared but aren’t shared equally

A

polar covalent bond

103
Q

occurs when there is a noticeable difference in the electronegativity of the 2 atoms included

A

polar covalent bond

104
Q

medium size difference in electronegaitivty

A

polar covlanet bond

105
Q

force of attraction between two molecules

A

intermolecular force

106
Q

this particular example is an example of a hydrogen bond

A

intermolecular bond

107
Q

only occurs when a hydrogen is attracted to either N,O,F

A

N-H O-H F-H

108
Q

the smallest electrically neutral collection of ions

A

formula unit

109
Q

no difference or very small difference in electronegativities

A

nonpolar covalent

110
Q

electrons are shared equally between the two atoms

A

nonpolar covalent

111
Q

no charges are present

A

nonpolar covalent

112
Q

atoms are connected by covalent bonds

A

nonpolar covalent

113
Q

medium size difference in electronegativities

A

polar covalent

114
Q

electrons are shared unequally between the two atoms

A

polar covalent

115
Q

partial charges are present

A

polar covalent

116
Q

atoms are connected by covalent bonds

A

polar covlanent

117
Q

large difference in electronegativities

A

ionic bond

118
Q

electrons are transferred from one atom to another

A

ionic

119
Q

full charges are present

A

ionic

120
Q

ions are not connected

A

ionic bond

Chemistry 101 (8 decks)

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