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H Chemistry > Unit 1 > Flashcards

Unit 1 Flashcards

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1
Q

metallic bonding

A

high MPs

good conductors of electricity

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2
Q

high MPs

good conductors of electricity

A

metallic bonding

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3
Q

covalent molecular

A

strong covalent bonds between atoms

weak LDFs between molecules

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4
Q

strong covalent bonds between atoms

weak LDFs between molecules

A

covalent molecular

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5
Q

covalent network

A

strong covalent bonds between atoms

very high MPs

carbon (as diamond and graphite), silicon, boron

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6
Q

strong covalent bonds between atoms

very high MPs

carbon (as diamond and graphite), silicon, boron

A

covalent network

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7
Q

what does strong covalent bonds mean for MPs

A

higher MPs

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8
Q

monatomic elements

A

nobles gases

weak LDFs

MPs increase as you go down the group

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9
Q

LDF strength increases as the ______ __ _______ increases

A

LDF strength increases as the number of electrons increases

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10
Q

LDF strength __________ as the number of electrons increases

A

increases

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11
Q

what does stronger LDFs mean for MPs

A

higher MPs

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12
Q

what should you refer to when comparing MPs

A

bonding, forces

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13
Q

what is covalent radius a measure of

A

the size of an atom

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14
Q

what is the measurement of the size of an atom

A

the covalent radius

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15
Q

what is the covalent radius

A

half the distance between the nuclei of the two covalently bonded atoms of an element

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16
Q

half the distance between the nuclei of the two covalently bonded atoms of an element

A

what is the covalent radius

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17
Q

going across a period, covalent radius _______

A

decreases

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18
Q

going ______ __ _______, covalent radius decreases

A

period

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19
Q

going down a group, covalent radius ________

A

increases

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20
Q

going _____ __ ______, covalent radius increases

A

down a group

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21
Q

going across a period, the nuclear charge ______

A

increases

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22
Q

going ______ _ _____, the nuclear charge increases

A

going across a period, the nuclear charge increases

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23
Q

going across a period, the nuclear charge ______

A

increases

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24
Q

going across a period, the number of filled electron shells _____ ___ _____

A

stays the same

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25
Q

going _____ ___ ______, the number of filled electron shells stays the same

A

across a period

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26
Q

what does an increase in nuclear charge mean

A

electrons being more strongly attracted to the nucleus
–> covalent radius decreases

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27
Q

as you go down a group, an extra ___ __ _____ is added

A

shell of electrons

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28
Q

as you go _____ ___ ______, an extra shell of electrons is added

A

down a group

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29
Q

why does covalent radius increase as you go down a group

A

an extra shell of electrons is added

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30
Q

what does an extra shell of electrons is added as you go down a group mean for covalent radius

A

the covalent radius increases

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31
Q

shielding effect

A

Each extra layer of electrons shields outer electrons from the positive nucleus so that the outer electrons are less strongly attracted to the nucleus

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32
Q

Each extra layer of electrons shields outer electrons from the positive nucleus so that the outer electrons are less strongly attracted to the nucleus

A

shielding effect

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33
Q

going down a group, the electronegativity __________

A

decreases

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34
Q

going ______ ____ __ ___, the electronegativity decreases

A

down a group

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35
Q

going across a period, the electronegativity _______

A

increases

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36
Q

going _____ __ _______, the electronegativity increases

A

across a period

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37
Q

what 2 factors influence electronegativity and covalent radius

A

nuclear charge

number of filled electron shells

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38
Q

what does an increase in nuclear charge cause

A

the atom attracts bonded electrons more strongly

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39
Q

the atom attracts bonded electrons more strongly

A

increase in nuclear charge

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40
Q

what happens when the number of filled electron shells increases

A

outer electrons are further from the nucleus

AND

less strongly attracted to the nucleus

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41
Q

outer electrons are further from the nucleus

AND

less strongly attracted to the nucleus

A

what happens when the number of filled electron shells increases

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42
Q

going down a group, the ionisation energy _________

A

decreases

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43
Q

going _____ _ ____, the ionisation energy decreases

A

down a group

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44
Q

going across a period, the ionisation energy _______

A

increases

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45
Q

going ____ __ _____, the ionisation energy increases

A

across a period

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46
Q

covalent bond

A

atoms share pairs of electrons

two positive nuclei held together by their shared attraction for shared pair of electrons

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47
Q

atoms share pairs of electrons

two positive nuclei held together by their shared attraction for shared pair of electrons

A

covalent bond

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48
Q

polar covalent bonds

A

formed when the attraction of atoms for the pair of bonding electrons is different

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49
Q

formed when the attraction of atoms for the pair of bonding electrons is different

A

polar covalent bonds

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50
Q

ionic bonds

A

the electrostatic attraction between positive and negative ions

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51
Q

the electrostatic attraction between positive and negative ions

A

ionic bonds

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52
Q

what do ionic compounds form

A

lattice structures of oppositely charged ions

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53
Q

what compounds forms lattice structures of oppositely charged ions

A

ionic compounds

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54
Q

bonding continuum

A

pure covalent bonds —– polar covalent bonds —— ionic bonding

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55
Q

pure covalent bonds —– polar covalent bonds —— ionic bonding

A

bonding continuum

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56
Q

the larger the difference in electronegativity, the more ______ the bond will be

A

polar

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57
Q

the larger the difference in _________, the more polar the bond will be

A

electronegativity

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58
Q

what can a large difference in electronegativity cause to form

A

ions

59
Q

non metal to metal bonding

A

ionic bonding most of the time

60
Q

is a pure covalent bond polar?

A

it is non polar

61
Q

van der Waals forces

A

intermolecular forces acting between molecules

62
Q

LDFs exist between ___ molecules and atoms

A

all

63
Q

when are LDFs formed

A

a result of electrostatic attraction between temporary dipoles and induced dipoles caused by movement of electrons in atoms and molecules

64
Q

a result of electrostatic attraction between temporary dipoles and induced dipoles caused by movement of electrons in atoms and molecules

A

LDFs

65
Q

what are LDF strengths related to

A

the number of electrons within a molecule or atom

66
Q

when is a molecule described as polar

A

if it has a permanent dipole

67
Q

pdp to pdp dipole interactions are ____ than LDFs

A

stronger

68
Q

LDFs are ____ than pdp to pdp dipole interactions

A

weaker

69
Q

hydrogen bonds are highly ____

A

polar

70
Q

hydrogen bonds are _____ than other pdp-pdp interactions

A

stronger

71
Q

hydrogen bonds are stronger than other ______ _______

A

pdp-pdp interactions

72
Q

hydrogen bonds are ______ than covalent bonds

A

weaker

73
Q

hydrogen bonds are weaker than ________ _____

A

covalent bonds

74
Q

the MPs and BPs of polar substances are ______ than that of non polar substances with similar number of electrons

A

higher

75
Q

the MPs and BPs of ______ substances are higher than that of ______ substances with similar number of electrons

A

polar, non polar

76
Q

compare the melting points of polar substances with that of non polar substances with similar no. of electrons

A

polar has higher MPs and BPs than non polar

77
Q

why do hydrogen, water and hydrogen fluoride have unexpectedly high MPs and MPs

A

because they have hydrogen bonds

78
Q

what effect does hydrogen bonding have on ice

A

it is an expanded structure that causes ice to have a lower density than water at low temps

79
Q

it is an expanded structure that causes ice to have a lower density than water at low temps

A

the effect of hydrogen bonds on ice

80
Q

hydrogen bonds and MPs

A

hydrogen bonds cause substances to have higher than expected MPs and BPs

81
Q

2 features to consider when predicting solubility

A
  1. presence of H-O or N-O bonds (hydrogen bonds)
  2. spatial arrangement of polar covalent bonds (could be a permanent dipole)
82
Q

what are ionic compounds held together by in the solid state

A

ionic bonds

83
Q

LDF are caused by

A

temporary dipoles

84
Q

pdp pdp are caused by

A

permanent dipoles

85
Q

weakest type of intermolecular forces

A

LDFs

86
Q

what are non polar molecules held together by

A

LDFs

87
Q

what are polar molecules held together by

A

pdp pdp interactions or hydrogen bonds

88
Q

when are ionic compounds formed

A

when two atoms bond where there is a large difference in electronegativity

89
Q

what forms when two atoms bond where there is a large difference in electronegativity

A

ionic compounds

90
Q

what can covalent compounds can be classed as

A

polar or non polar

91
Q

when are polar covalent bonds formed

A

when atoms with two atoms with different electronegativity values form a covalent bond

92
Q

what forms when atoms with two atoms with different electronegativity values form a covalent bond

A

polar covalent bond

93
Q

in a polar covalent bond, which atom is assigned the negative charge

A

the atom with the higher electronegativity value

94
Q

in a polar covalent bond, what is the the atom with the higher electronegativity value assigned

A

negative charge

95
Q

in a polar covalent bond, which atom is assigned the positive charge

A

the atom with the lower electronegativity value

96
Q

in a polar covalent bond, what is the the atom with the lower electronegativity value assigned

A

positive charge

97
Q

what are the attractions between covalent molecules known as

A

van der Waals

98
Q

when are non polar covalent bonds formed

A

when two atoms with the same electronegativity form bonds

99
Q

what bonds form when two atoms with the same electronegativity form bonds

A

non polar covalent bonds

100
Q

what do symmetrical compounds with polar bonds form

A

non polar molecules

101
Q

polar molecules are attracted to each other by ____ or ________

A

pdp pdp or hydrogen bonding

102
Q

non polar molecules are attracted to each other by _____

A

LDFs

103
Q

when do pdp pdp interactions occur

A

in molecules with a permanent dipole

104
Q

hydrogen bonds occur between hydrogen and ..

A

fluorine, oxygen, or nitrogen

105
Q

stronger intermolecular forces means…

A

higher MPs and BPs

higher viscosity

106
Q

____ dissolves _____

A

like dissolves like

107
Q

polar substances dissolve in _____ liquids

A

polar

108
Q

nonpolar substances dissolve in _____ liquids

A

non polar

109
Q

Why is it important to control the rate of reactions

A

So that they are….

economically viable (they will result in a good yield of products and profits for the company)

AND

safe (the reaction does not progress too quickly potentially causing explosions).

110
Q

economically viable (they will result in a good yield of products and profits for the company)

AND

safe (the reaction does not progress too quickly potentially causing explosions).

A

Why is ur important to control rates of reactions

111
Q

As the reactants are used up, what happens to the reactant rate

A

It will decrease, the reactions slows down

112
Q

Average rate equation

A

Delta quantity
——————
Delta time

113
Q

Delta quantity
——————
Delta time

A

Average rate equation

114
Q

Relative rate equation

A

1
—
T

115
Q

1
——
T

A

Relative rate

116
Q

Units for reaction rate

A

S^-1

117
Q

S^-1

A

Units for reaction rate

118
Q

For a reaction to occur, what must happen

A

The reactants molecules must collide with enough energy

119
Q

What requires the reactants molecules must collide with enough energy

A

A chemical reaction

120
Q

Activation energy, Ea

A

The minimum kinetic energy required for a reaction to occur

121
Q

Why must reactant molecules collide with enough energy

A

To overcome the repulsive forces (caused by outer electrons)

122
Q

Activated complex

A

intermediate stage

a high energy, unstable arrangement of atoms

123
Q

An intermediate stage is reached in which a high energy, unstable arrangement of atoms is formed called the activated complex.

A

Activated complex

124
Q

What is given out when the new product bonds are formed

A

Energy is given out

125
Q

What happens when new bonds are formed when forming products

(2 points)

A

Energy is given out

AND

The atoms are rearranged into the product molecules

126
Q

What must happen for a successful collision to occur

A

The collision geometry must be right
—> the reactants molecules have to be facing the right way

127
Q

what happens to reducing agents

A

they are oxidised

128
Q

what agents are oxidised

A

reducing agents

129
Q

electronegativity of reducing agents

A

low

130
Q

what agents have low electronegativities

A

reducing agents

131
Q

what agents form positive ions

A

reducing agents

132
Q

what ions do reducing agents form

A

positive ions

133
Q

where are the strongest reducing agents

A

top right of page 12

134
Q

what happens to oxidising agents

A

they are reduced

135
Q

what agents are reduced

A

oxidising agents

136
Q

what electronegativity do oxidising agents have

A

high electronegativity

137
Q

what agents have high electronegativity

A

oxidising agents

138
Q

what agents form negative ions

A

oxidising agents

139
Q

what ions do oxidising agents form

A

negative ions

140
Q

where are the strongest oxidising agents

A

bottom left of page 12

141
Q

what are found at the bottom left of page 12

A

strongest oxidising agents

142
Q
A
143
Q

Symmetry affect on polar bonds

A

Cancels polarity

H Chemistry (3 decks)

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