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A Level Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Define ionic bond

A

The force of attraction between oppositely charged ions.

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2
Q

Which electrons are involved in bonding?

A

Outer electrons.

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3
Q

Elements form ions to achieve what?

A

The electronic structure of a noble gas.

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4
Q

In a solid ionic compound oppositely charged ions attract and do what? how?

A

Form a lattice by electrostatic attraction.

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5
Q

Ionic compounds, low or high m.p? why?

A

High, because lattice.

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6
Q

What is a lattice?

A

A regularly repeating pattern of + and - ions.

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7
Q

Formula for carbonate?

A

CO3^2-

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8
Q

Formula for sulphate?

A

SO4^2-

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9
Q

Formula for nitrate?

A

NO3^-

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10
Q

Formula for nitrate?

A

NO3^-

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11
Q

Formula for phosphate?

A

PO4^3-

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12
Q

Formula for phosphate?

A

PO4^3-

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13
Q

Formula for hydroxide?

A

OH^-

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14
Q

Formula for ammonium?

A

NH4^-

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15
Q

In a solid metal the metal is present as what?

A

Ions.

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16
Q

What happens to the electrons the metal loses to becomes ions?

A

Become delocalised and form a sea around the regularly spaced ions.

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17
Q

What holds the metal together?

A

The attraction between the delocalised e-s and the ions.

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18
Q

What are two qualities of metals?

A

Malleable, conductors

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19
Q

What is the force of attraction between ions and e-s?

A

Electrostatic.

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20
Q

When does a giant ionic structure conduct?

A

In solution or molten.

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21
Q

What arrangement to giant ionic structures have?

A

Regular crystal.

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22
Q

Do covalent structures conduct electricity?

A

No.

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23
Q

How are simple covalent structures arrangened?

A

Isolated molecules with WIF.

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24
Q

Where are the strong bonds in covalent structures?

A

Between atoms.

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25
Q

High or low m.p for simple covalent?

A

Low, gases at room temp.

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26
Q

How are simple covalent structures arrangened?

A

Isolated molecules with WIF.

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27
Q

What arrangement do simple covalent have?

A

Regular crystal.

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28
Q

Giant covalent, high or low m.p?

A

High, solid at room temp.

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28
Q

Giant covalent, high or low m.p?

A

High, solid at room temp/

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29
Q

Do giant covalent conduct heat?

A

Yes.

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30
Q

What giant covalent conducts electricity?

A

Graphite.

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31
Q

What is a covalent bond?

A

A shared pair of electrons.

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32
Q

What do covalent bonds form between?

A

Non-metals.

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33
Q

What is a dative bond?

A

When one atom donates both e-s needed to bond.

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34
Q

What is needed for a dative bond?

A

One atom must have a lone pair and the other atom must have a vacant orbital for the pair.

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35
Q

Dative is also called?

A

Coordinate.

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36
Q

What are the five types of crystal types?

A

Monatomic, simple molecular, ionic, giant covalent and metallic.

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37
Q

Monatomic substances are all what at room temp?

A

Gases.

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38
Q

Ionic m.p and why?

A

High, lots of energy needed to break strong electrostatic attractions.

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39
Q

Ionic electrical conductivity and why?

A

Conducts when molten or dissolved in water, ions are free to move, water disrupts lattice and ions are free to move and carry the charge.

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40
Q

Ionic strength and why?

A

Hard but brittle, strong electrostatic forces between ions.

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41
Q

Ionic solubility and why?

A

Ions are free to move as water disrupts lattice.

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42
Q

Give an example of ionic.

A

Sodium chloride.

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43
Q

Simple molecular m.p and why?

A

Low, VDW forces between molecules are weak.

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44
Q

Simple molecular electrical conductivity and why?

A

No, electrons held in covalent bonds, no charged particles.

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45
Q

Simple molecular strength and why?

A

Soft and easy to break, VDW forces weak.

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46
Q

Simple molecular solubility and why?

A

Doesn’t dissolve in water, only dissolves in non polar solvents.

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47
Q

Example of simple molecular?

A

Iodine, I2.

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48
Q

What does I2 do at room temp?

A

Sublime, solid into gas. Forms purple vapour when heated.

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49
Q

What forces can hold molecular substances together?

A

Van der Waals (VDW), dipole dipole, hydrogen bonding.

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50
Q

Ice is what crystal type?

A

Simple molecular.

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51
Q

Ice m.p and b.p and why?

A

M.p = 0C, b.p = 100C, hydrogen bonding raises expected temp, stronger intermolecular forces.

52
Q

Ice electrical conductivity and why?

A

No, no charged particles.

53
Q

Ice strength, why?

A

Breaks easily but hard, H bonding.

54
Q

Diamond is an example of what?

A

Giant covalent.

55
Q

In diamond C has what?

A

4 covalent bonds with 4 other C atoms.

56
Q

What shape is diamond?

A

Tetrahedral.

57
Q

M.p of diamond and why?

A

High, break strong covalent bonds.

58
Q

Diamond electrical conductivity and why?

A

No, no free e-s.

59
Q

Diamond solubility?

A

No.

60
Q

Graphite is an example of what?

A

Giant covalent.

61
Q

In graphite what does each C do?

A

Bond to 3 other C.

62
Q

Graphite m.p and why?

A

High, lots of strong covalent bonds, lots of energy needed to break them.

63
Q

Graphite electrical conductivity and why?

A

Yes, free e-s move through structure (plane of hexagons).

64
Q

Graphite strength and why?

A

Soft, weak VDW hold structure together.

65
Q

Graphite solubility?

A

No.

66
Q

Strength of metallic bonding increases as?

A

Free e-s per atom increases, charge on + ion increases, size of + ion is smaller.

67
Q

What makes metals shiny?

A

Free e-s cause metals to reflect light.

68
Q

Metallic m.p and why?

A

High, + ions and free e-s held together by strong electrostatic forces.

69
Q

Metallic electrical conductivity and why?

A

High, free e-s carry charge through structure.

70
Q

Metallic strength and why?

A

Malleable and ductile, hammered into shape and drawn into wires, layers of ions slide over eachother.

71
Q

Metallic solubility and why?

A

No, + ions and free e-s held together by strong electrostatic forces.

72
Q

Define electronegativity.

A

The power of an atom to attract the pair of e-s in a covalent bond.

73
Q

What elements have the highest electronegativity?

A

FONCl.

74
Q

Define polarity.

A

The unequal sharing of e-s between atoms covalently bonded together.

75
Q

What bond would be nonpolar and example?

A

2 atoms that are the same, eg. F2.

76
Q

What bond would be polar and example?

A

2 atoms have different electronegativity. eg. HF.

77
Q

What do we show using partial charges?

A

Which side of the molecule is more + or -.

78
Q

What symbol do we use for partial charges?

A

δ+ and δ-.

79
Q

Polar bonds have some what?

A

Ionic character.

80
Q

Across a period, left to right, electronegativity does what?

A

Increases.

81
Q

Up a group electronegativity does what?

A

Increases.

82
Q

What are the factors that affect electronegativity?

A

Nuclear charge, atomic radius, shielding.

83
Q

Explain nuclear charge.

A

More protons, stronger attraction from nucleus to bonding pair of e-s.

84
Q

Explain atomic radius.

A

Closer the bonding pair of e-s to the nucleus the stronger the attraction between the two.

85
Q

Explain shielding?

A

The less shells of e-s shielding and repelling the bonding e-s the stronger the attraction between the bonding pair of e-s and the nucleus.

86
Q

Why does electronegativity decrease down a group?

A

Atomic radius gets larger, more shielding by e-s in inner shells, so less attraction between the nucleus and the bonding pair of e-s.

87
Q

Why dies electronegativity across a period increase?

A

Nuclear charge increases, no. of inner e-s stay the same, atomic radius decreases, so stronger attraction between nucleus and bonding pair of e-s.

88
Q

Low electronegativity indicates what bonding?

A

Covalent.

89
Q

High electronegativity indicates what bonding?

A

Ionic.

90
Q

In what molecules do VDW forces occur?

A

All.

91
Q

In what molecules does dipole dipole forces occur?

A

Polar covalent bonds.

92
Q

In what molecules does hydrogen bonding occur?

A

When H is bonded to NOF.

93
Q

Which force is weakest?

A

VDW.

94
Q

What force is strongest?

A

Hydrogen bonding.

95
Q

How do VDW forces work?

A

e-s in a molecule are constantly moving and may be unequally distributed, causing a temporary dipole on the molecule.

96
Q

When do VDW forces occur?

A

When a temporary dipole on one molecule induces a dipole on a neighbouring molecule.

97
Q

VDW increases as?

A

Size of molecule increases, point of contact between molecules increases, straight chain hydrocarbons (weaker if branched), the shape of the molecule.

98
Q

What will dipole dipole occur with?

A

With two molecules with permanent dipoles.

99
Q

When does hydrogen bonding occur?

A

When H is bonded to NOF.

100
Q

Why does hydrogen bonding occur?

A

Because H only has 2 e-s in the covalent bond, if they are pulled away from the atom the nucleus is exposed.

101
Q

What is the ‘H-bond’ in hydrogen bonding?

A

The attraction between a lone pair on the NOF to the δ+ H on a neighbouring molecule.

102
Q

What is the evidence for H bonding?

A

HF, H2O, and NH3 all have higher than average b.p.

103
Q

In liquid water what do the h bonds do?

A

Break and reform easily as molecules move about.

104
Q

When water freezes what happens to the H bonds.

A

Molecules are no longer free to move and H bonds hold the molecules in fixed positions.

105
Q

What is the difference in the molecule density between water and ice?

A

Ice is slightly less closely packed.

106
Q

Because ice is less dense than water where does it form?

A

On top of water.

107
Q

Why is ice forming on top of water beneficial for life?

A

Insulates ponds during winter so fish can survive.

108
Q

Where does hydrogen bonding also occur?

A

Alcohol, DNA.

109
Q

What types of line do we use to represent bonding?

A

Normal line, wedge, dashed line.

110
Q

What do the shapes of molecules and ions depend on?

A

Total no. of e- pairs around the central atom.

111
Q

What are the two types of e- pairs?

A

Bonding and non bonding.

112
Q

Define a bonding pair.

A

e-s in a covalent bond.

113
Q

Define a non bonding pair.

A

Lone pairs.

114
Q

What do e- pairs do to other e- pairs?

A

Repel as far as possible.

115
Q

Which pairs repel further?

A

Lone pairs.

116
Q

2 e- pairs and 2 bonding pairs makes what shape and angle?

A

Linear, 180 degrees.

117
Q

3 e- pairs and 3 bonding pairs makes what shape and angle?

A

Trigonal planar, 120 degrees.

118
Q

3 e- pairs and 2 bonding pairs makes what shape and angle?

A

Bent, 118 degrees.

119
Q

4 e- pairs and 4 bonding pairs makes what shape and angle?

A

Tetrahedral, 109.5 degrees.

120
Q

4 e- pairs and 3 bonding pairs makes what shape and angle?

A

Pyramidal, 107 degrees.

121
Q

4 e- pairs and 2 bonding pairs makes what shape and angle?

A

Bent, 104.5 degrees.

122
Q

5 e- pairs and 5 bonding pairs makes what shape and angle?

A

Trigonal bipyramidal, 120 and 90 degrees.

123
Q

5 e- pairs and 4 bonding pairs makes what shape and angle?

A

Trigonal bipyramidal, 119 and 89 degrees.

124
Q

5 e- pairs and 3 bonding pairs makes what shape and angle?

A

Trigonal planar or T-shape, 120 or 89 degrees.

125
Q

6 e- pairs and 6 bonding pairs makes what shape and angle?

A

Octahedral, 90 degrees.

126
Q

6 e- pairs and 5 bonding pairs makes what shape and angle?

A

Distorted square pyramid, 89 degrees.

127
Q

6 e- pairs and 4 bonding pairs makes what shape and angle?

A

Square planar, 90 degrees.

A Level Chemistry (26 decks)

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