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Chem A-level > 3.1.3 Bonding Knowledge > Flashcards

3.1.3 Bonding Knowledge Flashcards

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1
Q

what type of bonding is in a substance with only metal elements?

A

metallic bonding in a giant metallic lattice; electrostatic attraction between positive metal ions and delocalised electrons

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2
Q

what type of bonding is in a substance with metal and non-metal elements?

A

ionic bonding in a giant ionic lattice; electrostatic attraction between oppositely charged ions

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3
Q

what type of bonding is in a substance with only non-metal elements?

A

covalent bonding

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4
Q

what type of bonding is in C, Si, or SiO2?

A

covalent in a macromolecular structure; covalent bonds between atoms

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5
Q

what type of bonding is in the substance if it has H-F, H-O, or H-N bonds?

A

covalent bonding between atoms in a simple molecular structure with hydrogen bonding between molecules

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6
Q

what type of bonding is the substance if it has covalent bonds and is polar?

A

covalent bonding between atoms in a simple molecular structure with permanent dipole-dipole attractions between molecules

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7
Q

what type of bonding is the substance if it has covalent bonds and is not polar?

A

covalent bonding between atoms in a simple molecular structure with induced dipole-dipole attractions between molecules

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8
Q

what are the 3 types of bonding?

A

metallic, ionic, covalent

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9
Q

what are the 2 types of covalently bonded structures?

A

macromolecular and simple molecular

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10
Q

what is the structure of metallic bonding?

A

giant metallic lattice

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11
Q

what is the structure of ionic bonding?

A

giant ionic lattice

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12
Q

what is the type of bonding in a simple molecular structure?

A

Covalent bonds between atoms. IMF between molecules.

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13
Q

what are the particles within a metallic structure?

A

positive metal ions, delocalised electrons

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14
Q

what are the particles within an ionic structure?

A

negative and positive ions

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15
Q

what are the particles within a macromolecular structure?

A

atoms

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16
Q

what are the particles within a simple molecular structure?

A

molecules

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17
Q

define metallic bonding

A

Metallic bonding is the strong electrostatic attraction of positive metal ions surrounded by a sea of delocalised electrons

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18
Q

is the bonding stronger in Mg or Na, and why?

A
  • the bonding in magnesium is stronger than in sodium because:
  • Mg²⁺ ions have a higher charge than Na⁺ ions (2+ vs +)
  • Mg²⁺ has double the number of delocalised electrons than Na⁺
  • Mg²⁺ ion is smaller than Na⁺ ion
  • therefore, Mg²⁺ has a greater electrostatic attraction to the sea of delocalised electrons, than Na⁺
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19
Q

what are the properties of metals?

A
  • All metals are good electrical and thermal conductors
  • the majority of metals are very strong
  • metals are malleable and ductile
  • generally high MP and BP
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20
Q

why are metals good electrical and thermal conductors?

A

The delocalised electrons help transfer energy through the metal very efficiently and can flow and carry charge

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21
Q

why are the majority of metals very strong?

A

there is a strong electrostatic attraction between the positive metal ions and delocalised electrons

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22
Q

why are metals malleable and ductile?

A

the layers of metal ions can slide past one another

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23
Q

what makes a metal have a higher MP or BP than another metal?

A

the strength of the metallic bonds

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24
Q

define ionic bonding

A

strong electrostatic attraction between oppositely charged ions

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25
Q

what are the physical properties of an ionic substance?

A
  • high MP/BP
  • electrical conductivity when aqueous or molten
  • brittle, shatter easily
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26
Q

what is the charge on an ammonium ion?

A

1+

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27
Q

what is the formula of an ammonium ion?

A

NH₄⁺

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28
Q

What is the formula of a hydroxide ion?

A

OH⁻

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29
Q

what is the charge on a hydroxide ion?

A

1-

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30
Q

what is the formula of a nitrate ion?

A

NO₃⁻

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31
Q

what is the charge on a nitrate ion?

A

1-

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32
Q

what is the formula of a nitrite ion?

A

NO₂⁻

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33
Q

what is the charge on a nitrite ion?

A

1-

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34
Q

what is the formula of a hydrogencarbonate ion?

A

HCO₃⁻

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35
Q

what is the charge on a hydrogencarbonate ion?

A

1-

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36
Q

what is the formula of a chlorate (I) ion?

A

ClO⁻

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37
Q

what is the charge on a chlorate (I) ion?

A

1-

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38
Q

what is the formula of a chlorate (V) ion?

A

ClO₃⁻

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39
Q

what is the charge on a chlorate (V) ion?

A

1-

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40
Q

what is the formula of a carbonate ion?

A

CO₃²⁻

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41
Q

what is the charge on a carbonate ion?

A

2-

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42
Q

what is the formula of a sulfate ion?

A

SO₄²⁻

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43
Q

what is the charge on a sulfate ion?

A

2-

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44
Q

what is the formula of a sulfite ion?

A

SO₃²⁻

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45
Q

what is the charge on a sulfite ion?

A

2-

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46
Q

what is the formula of a dichromate ion?

A

Cr₂O₇²⁻

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47
Q

what is the charge on a dichromate ion?

A

2-

48
Q

what is the formula of a phosphate ion?

A

PO₄³⁻

49
Q

define a covalent bond

A

A covalent bond is a shared pair of electrons between two atoms

49
Q

what is the charge on a phosphate ion?

A

3-

50
Q

how many covalent bonds does each carbon have in diamond?

A

4

51
Q

what is the structure of diamond?

A

macromolecular - tetrahedral

52
Q

what are the properties of diamond?

A
  • has a very high melting point
  • is very hard
  • is a non-conductor
53
Q

why is diamond a non-conductor?

A

there are no delocalised electrons or free-moving charged particles to carry current/energy

54
Q

how many covalent bonds does each carbon have in graphite?

A

3

55
Q

what is the structure of graphite?

A

macromolecular - arranged in layers which can slide over each other

56
Q

why can layers slide over each other in graphite?

A

layers held together by weak IMF

57
Q

what are the properties of graphite?

A
  • malleable
  • conductor
  • high melting point
58
Q

why is graphite malleable?

A

arranged in layers which can slide over each other; layers held together by weak IMF

59
Q

why is graphite a conductor?

A

each carbon atom has a delocalised electron which can carry charge/current through the structure

60
Q

why do simple molecular structures have a low BP/MP?

A
  • when a simple molecular substance melts/boils it is the IMF that are broken
  • IMF are much weaker than covalent bonds so simple molecular compounds have low MP
61
Q

write the ionic formula for lithium oxide

A

Li₂O

62
Q

write the ionic formula for calcium nitrate

A

Ca(NO₃)₂

63
Q

how many bonds does beryllium usually form?

A

2

64
Q

how many bonds does boron usually form?

A

3

65
Q

how many bonds does carbon usually form?

A

4

66
Q

how many bonds does nitrogen usually form?

A

3

67
Q

how many bonds does oxygen usually form?

A

2

68
Q

how many bonds does fluorine usually form?

A

1

69
Q

draw the dot-cross diagram for oxygen

A
  • each atom has 6 valence electrons
  • Oxygen likes to form 2 bonds, so must form a double bond
70
Q

draw the dot-cross diagram for N₂H₄

A
  • hydrogen likes to form 1 bond - nitrogen likes to form 3
  • because nitrogen likes to form more bonds, put the bond between nitrogen and nitrogen in first
  • then add the hydrogens
71
Q

Draw the dot-cross diagram for C₂H₂

A
  • carbon likes to form 4 bonds - hydrogen can only form 1 bond
  • therefore the bonds Hydrogen can make are with carbon, and the carbons must triple bond to each other to gain 8
72
Q

what is a lone pair?

A

a pair of valence electrons that are not shared with another atom

73
Q

what is a bonding pair?

A

The electron pair being shared by the atoms

74
Q

what is a coordinate bond?

A

A coordinate bond is a shared electron pair which have both come from the same atom

75
Q

how is a coordinate bond represented?

A

by an arrow - the direction of the arrow points from the atom which donates to pair of electrons, to the atom which accepts the pair of electrons

76
Q

what are the features of a coordinate bond?

A

once a coordinate bond has formed, it behaves in exactly the same way as a covalent bond - same length and strength

77
Q

draw a diagram to represent the coordinate bond in an ammonium ion

A
78
Q

what is Valence Shell Electron Pair Repulsion Theory?

A

Bonding pairs and lone pairs of electrons are arranged in charged clouds that repel each other; to minimise repulsion, electron pairs try to get as far apart as possible

79
Q

summarise the strength of repulsion of different bonds according to VSEPR theory

A
  • lone pairs repel more than bonding pairs
  • lone pair⇒lone pair is strongest repulsion
  • then lone pair⇒bonding pair
  • bonding pair⇒bonding pair is weakest repulsion
80
Q

draw the VSEPR diagram for a water molecule; give its shape name and bond angle

A
  • name: bent/non-linear
  • bond angle: 104.5
81
Q

what is the bond angle in a bent/v-shaped molecule with 2LP and 2BP?

A

104.5

82
Q

what is the shape of a molecule with 2 LP and 2 BP?

A

bent/non-linear

83
Q

draw the VSEPR diagram for boron trifluoride; give its shape name and bond angle

A
  • shape: trigonal planar
  • bond angle: 120
84
Q

what is the bond angle in a trigonal planar molecule?

A

120

85
Q

what is the shape of a molecule with 3 BP?

A

trigonal planar

86
Q

draw the VSEPR diagram for methane; give its shape name and bond angle

A
  • shape: tetrahedral
  • bond angle: 109.5
87
Q

what is the bond angle in a tetrahedral molecule?

A

109.5

88
Q

what is the shape of a molecule with 4 BP?

A

tetrahedral

89
Q

draw the VSEPR diagram for Phosphorus pentachloride; give its shape name and bond angle

A
  • shape: trigonal bipyramidal
  • bond angle: 120 and 90
90
Q

what is the bond angle in a trigonal bipyramidal molecule?

A

120 and 90

91
Q

What is the shape of a molecule with 5 BP?

A

trigonal bipyramidal

92
Q

draw the VSEPR diagram for sulphur hexafluoride; give its shape name and bond angle

A
  • shape: octahedral
  • bond angle: 90
93
Q

what is the bond angle in an octahedral molecule?

A

90

94
Q

what is the shape of a molecule with 6 BP?

A

octahedral

95
Q

draw the VSEPR diagram for Dichlorocarbene; give its shape name and bond angle

A
  • shape: bent/v-shaped
  • bond angle: 117.5
96
Q

what is the bond angle in a bent/v-shaped molecule with 2 BP and 1 LP?

A

117.5

97
Q

what is the shape of a molecule with 2BP and 1 LP?

A

bent/v-shaped

98
Q

draw the VSEPR diagram for ammonia; give its shape name and bond angle

A
  • shape: pyramidal
  • bond angle; 107
99
Q

what is the bond angle in a pyramidal molecule?

A

107

100
Q

what is the shape of a molecule with 3 BP and 1 LP?

A

pyramidal

101
Q

draw the VSEPR diagram for sulphur tetrafluoride; give its shape name and bond angle

A
  • shape name: seesaw
  • bond angle: 119 and 89
102
Q

what is the bond angle in a seesaw molecule?

A

119 and 89

103
Q

what is the shape of a molecule with 4BP and 1 LP?

A

seesaw

104
Q

draw the VSEPR diagram for iodine pentafluoride; give its shape name and bond angle

A
  • shape name: square pyramidal
  • bond angle: 89
105
Q

what is the bond angle in a square pyramidal molecule?

A

89

106
Q

what is the shape of a molecule with 5 BP and 1 LP?

A

square pyramidal

107
Q

what is the shape of a molecule with 1 BP and 2 LP

A

linear

108
Q

what is the shape of a molecule with 2BP?

A

linear

109
Q

draw the VSEPR diagram for iodine trifluoride; give its shape name and bond angle

A
  • shape name: T-shaped
  • bond angle: 90
110
Q

what is the shape of a molecule with 3BP and 2LP?

A

T-shaped

111
Q

what is the bond angle in a T-shaped molecule?

A

90

112
Q

draw the VSEPR diagram for xenon tetrafluoride; give its shape name and bond angle

A
  • shape name: square planar
  • bond angle: 90
113
Q

what is the shape of a molecule with 4BP and 2LP?

A

square planar

114
Q

what is the bond angle in a square planar molecule?

A

90

Chem A-level (10 decks)

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