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C3- BONDING > 3.7- BONDING AND PHYSICAL PROPERTIES > Flashcards

3.7- BONDING AND PHYSICAL PROPERTIES Flashcards

1
Q

What is matter?

A

anything with mass

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2
Q

What is matter made of?

A

tiny particles- it is particulate

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3
Q

As the particles in matter are in motion, what do they have?

A

kinetic energy

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4
Q

What is the arrangement of particles in solids?

A

regular

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5
Q

What is the arrangement of particles in liquids?

A

random

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6
Q

What is the arrangement of particles in gases?

A

random

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7
Q

What is the evidence for solids having a regular arrangement of particles?

A

crystal shape have straight edges

solids have definite shapes

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8
Q

What is the evidence for liquids having a random arrangement of particles

A

none direct but a liquid changes shape to fill bottom of its container

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9
Q

What is the evidence for gases having a random arrangement of particles

A

none direct but a gas will fill its container

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10
Q

What is the spacing like in solids?

A

close

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11
Q

What is the spacing like in liquids?

A

close

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12
Q

What is the spacing like in gases?

A

far apart

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13
Q

What is the evidence for close spacing in solids?

A

solids are not easily compressed

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14
Q

What is the evidence for close spacing in liquids?

A

liquids are not easily compressed

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15
Q

What is the evidence for far apart spacing in gases?

A

gases are easily compressed

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16
Q

What is the movement of particles of solids like?

A

vibrating about a point

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17
Q

What is the movement of particles of liquids like?

A

rapid ‘jostling’

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18
Q

What is the movement of particles of gases like?

A

rapid

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19
Q

What is the evidence for the movement of particles in solids vibrating about a point?

A

diffusion is very slow

solids expand on heating

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20
Q

What is the evidence for the movement of particles in liquids rapidly ‘jostling’?

A

diffusion is slow

liquid evaporates

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21
Q

What is the evidence for the movement of particles in gases being rapid?

A

diffusion is rapid

gases exert pressure

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22
Q

What happens when you first heat a solid and supply energy to the particles?

A

makes them vibrate more about a fixed position

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23
Q

What does heating a solid and supplying energy tot he particles slightly increase?

A

slightly increases average distance between particles and so solid expands

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24
Q

What do you do turn a solid into liquid?

A

supply more energy to it than just heating the solid

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25
Q

Why is more energy needed when turning a solid into a liquid?

A

to weaken forces that act between particles , holding them together in solid state

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26
Q

What is the energy needed to turn a solid into liquid called?

A

enthalpy change of melting

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27
Q

What does not change while a solid is melting?

A

temperature

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28
Q

Why does the temperature not change while the solid is melting?

A

heat energy provided is absorbed as forces between particles weakened

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29
Q

What is the enthalpy?

A

heat energy change measured under constant pressure whilst temperature depends on average K.E. of particles and so is related to their speed- greater the energy, faster they go

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30
Q

when you heat a liquid what happens to the particles?

A

supply energy to particles which makes them move more quickly-more K.E.

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31
Q

What happens to the spacing in liquids when it’s heated?

A

on average, particles move a little further apart so liquids also expand on heating

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32
Q

What must you do to turn a liquid into a gas?

A

supply enough energy to break all intermolecular forces between particles

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33
Q

What does a gas consist of?

A

particles that are far apart + moving independently

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34
Q

What is the energy needed to turn a liquid into gas called?

A

enthalpy change of vaporisation

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35
Q

Is there temperature change when a liquid turns to gas?

A

no

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36
Q

What do the particles gain when you heat a gas and what do they do?

A

gain K.E. and move faster

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37
Q

What happens to the spacing in gases when they’re heated?

A

get much further apart and so gases expand a great deal on heating

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38
Q

What state of matter are crystals?

A

solids

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39
Q

What arrangement do the particles have in crystals?

A

regular arrangement

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40
Q

What are the particles in a crystal held together by?

A

forces of attraction

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41
Q

What could the forces of attraction between the particles in a crystal be?

A

strong bonds- covalent, metallic or ionic

or weak intermolecular forces- van der Waals, dipole-dipole, or hydrogen bonds

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42
Q

What does the strength of the forces of attraction between the particles in a crystal affect?

A

physical properties of crystals

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43
Q

What happens to the melting temperature and enthalpy of fusion, the stronger the force between particles in a crystal?

A

higher melting temp and greater enthalpy of fusion

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44
Q

What are the 4 basic crystal types?

A

ionic, metallic, molecular and macromolecular

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45
Q

What do ionic compounds have between the oppositely charged ions?

A

strong electrostatic attractions

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46
Q

Example of a typical ionic crystal?

A

sodium chloride, NaCl

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47
Q

What is the melting point of ionic compounds like?

A

high melting points

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48
Q

Why do ionic compounds have high melting points?

A

because of strong electrostatic attractions that extend throughout structure
these require a lot of energy to break for ions to move apart from one another

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49
Q

What do metals exist as? (hint-lattice)

A

lattice of positive ions embedded in a delocalised sea of electrons

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50
Q

What attraction is there throughout the metal crystals?

A

attraction of positive to negative extends throughout the crystal

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51
Q

What is the high melting temperature in metals due to?

A

strong metallic bonds

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52
Q

What do molecular crystals consist of?

A

molecules held in a regular array by intermolecular force

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53
Q

What do the covalent bonds in molecular crystals hold together?

A

covalent bonds WITHIN molecule hold atoms together

54
Q

Where do covalent bonds not act in a molecular crystal?

A

do not act BETWEEN molecules

55
Q

What is the melting temperatures of molecular crystals like?

A

low melting temperatures

56
Q

What is the enthalpies of melting like for molecular crystals?

A

low enthalpies of melting

57
Q

Why do molecular crystals have low melting temperatures and low enthalpies of melting?

A

intermolecular forces much weaker than covalent, ionic or metallic bonds

58
Q

What is an example of a molecular crystal?

A

iodine

59
Q

What holds pairs of iodine atoms together to form I2 molecules? (molecular crystals)

A

strong covalent bonds

60
Q

Do iodine molecules have a large number of electrons?

A

yes

61
Q

What does iodine molecules having a large number of electrons cause?

A

van der Waals forces strong enough to hold molecules together as solid

62
Q

As van der Waals forces are much weaker than covalent bonds, what properties does it give iodine? (3)

A

crystals soft + break easily

low melting temp + sublimes readily to form gaseous iodine molecules

doesn’t conduct electricity as there are no charged particles to carry charge

63
Q

Are covalent compounds always made up of small molecules?

A

no

64
Q

In some substances where do the covalent bonds extend? (macromolecular crystals?

A

extend throughout compound

65
Q

What typical property of a giant structure held together with strong bonds do substances with covalent bonds extending throughout the compound have? (macromolecular crystals)

A

high melting temperature

66
Q

Examples of macromolecular crystals? (2)

A

diamond and graphite

67
Q

What are diamond and graphite made up of?

A

carbon only

68
Q

What are diamond and graphite called in association with carbon?

A

polymorphs and allotropes of carbon

69
Q

Why are diamond and graphite very different materials?

A

their atom are differently bonded + arranged

70
Q

What does diamond consist of?

A

pure carbon with covalent bonding between every carbon atom

71
Q

Why is diamond a giant structure?

A

bonds spread throughout the structure

72
Q

How many electrons does a carbon have in its outer shell?

A

four electrons

73
Q

How many single covalent bonds does each carbon atom form in diamond?

A

forms 4 single covalent bonds with other carbon atoms

74
Q

What do the four electrons pairs of each carbon in diamond do?

A

repel each other, following rules of electron pair repulsion theory

75
Q

Where do the bonds point in three dimensions? (diamond)

A

point to corners of a tetrahedron (bond angles of 109.5°

76
Q

What is the positions of the carbon atoms like in diamond?

A

each carbon atom is in an identical position in the structure, surrounded by 4 other carbon atoms

77
Q

What do the carbon atoms in diamond form?

A

giant three-dimensional lattice of strong covalent bonds

78
Q

What properties does diamond have? (3)

A

very hard material (one of the hardest known)

very high melting temp, over 3700K

doesn’t conduct electricity as there are no free charged particles to carry charge

79
Q

What does graphite consist of?

A

pure carbon but atoms bonded + arranged differently from diamond

80
Q

How many sorts of bonding does graphite have?

A

2

81
Q

What are the 2 sorts of bonding that graphite have?

A

strong covalent

weaker van der Waals forces

82
Q

How many single covalent bonds does each carbon atom form in graphite?

A

3 single covalent bonds

83
Q

What is the shape of the graphite molecule and what bond angles?

A

flat trigonal arrangement, sometimes called trigonal planar, with bond angle of 120°

84
Q

What does each carbon atom forming 3 single covalent bonds in graphite leave?

A

leaves each carbon atom with a ‘spare ‘ electron in a p-orbital that’s not part of the 3 single covalent bonds

85
Q

What does the flat trigonal arrangement/ trigonal planar in graphite produce?

A

two-dimensional layer of linked hexagons of carbon atoms

86
Q

What do the p-orbital of the carbon atoms in the graphite with the ‘spare’ electron do?

A

merge above and below the plane of the carbon atoms in each layer

87
Q

When the p-orbitals merge above and below of the plane of the carbon atoms in each layer, what can the electrons do? (graphite)

A

electrons can move anywhere within the layer- delocalised

88
Q

What does the delocalised electrons from the p-orbitals merging add on to? (graphite)

A

adds to strength of bonding

89
Q

What does the delocalised electrons allow graphite to do?

A

conduct electricity

90
Q

What can the delocalised electrons do? (graphite)

A

travel freely through material

91
Q

Which plane does graphite conduct along and which one does it not ?

A

only conduct along hexagonal planes, not at right angles to them

92
Q

Are there covalent bonds between the layers of the carbon atoms in graphite?

A

no

93
Q

How are the layers of carbon atoms in graphite held together?

A

weaker van der Waals forces

94
Q

What does the weak intermolecular force of attraction (VDW) between the carbon layers in graphite mean?

A

layers can slide across one another

95
Q

What does the layers of carbon being able to slide across one another make graphite?

A

makes graphite soft and flaky

96
Q

What is graphite used in?

A

lead in pencils

97
Q

What does graphite being flaky allow? (in reference to pencil)

A

allows graphite layers to transfer from pencil to paper

98
Q

Properties of graphite (3)

A

soft material
very high melting temp + in fact breaks down before it melts- because of strong network of covalent bonds, which make it a giant structure
conducts electricity along planes of hexagons

99
Q

When was the first other form of pure carbon discovered?

A

when chemists were looking for molecules in outer space

100
Q

What do new forms of pure carbon structures include? (2)

A

closed cages of carbon atoms

tubes called nanotubes

101
Q

What is the most famous other form of pure carbon?

A

buckminsterfullerene, C60

102
Q

How are atoms arranged in buckminsterfullerene?

A

arranged in football-like shape

103
Q

What property best tells us what sort of bonding you have?

A

electrical conductivity

104
Q

What conducts electricity well? (2)

A

metals and alloys

105
Q

What are alloys?

A

mixture of metals

106
Q

Do metals and alloys conduct electricity well in a solid and liquid state?

A

yes

107
Q

Why do metals and alloys conduct electricity well in a solid and liquid state?

A

due to their metallic bonding

108
Q

How is current carried in metals and alloys?

A

current carried by delocalised electrons that hold metal ions together

109
Q

When do ionic compounds conduct electricity?

A

in liquid state (or when dissolved in water)

110
Q

When don’t ionic compounds conduct electricity?

A

when they’re solid

111
Q

How is current carried in ionic compounds?

A

by movement of ions towards electrode of opposite charge

112
Q

What are the ions able to do when the ionic compound is liquid or dissolved in water?

A

ions free to move

113
Q

What happens to the ions when ionic compounds are in solid states?

A

fixed rigidly in position

114
Q

Generally do covalent bonded substances conduct electricity?

A

do not conduct electricity in either solid or liquid state

115
Q

Why do covalent bonded substances generally not conduct electricity in solid or liquid states?

A

no charged particles to carry current

116
Q

Are covalent compounds soluble in water?

A

often insoluble in water

117
Q

What happens when covalently bonded substances do react with water?

A

react to form ions, i.e. ethanoic acid

118
Q

What can the solution do when covalently bonded substances are dissolved in water?

A

can then conduct electricity

119
Q

What does structure describe?

A

arrangement in which atoms, ions or molecules are held together in space

120
Q

What is the property that best tells us if a structure is giant or simple molecular?

A

melting (or boiling) point

121
Q

What is the melting (and boiling) points of simple molecular compounds like?

A

low melting (and boiling) points

122
Q

What is the melting (and boiling) points of giant structures generally like?

A

high melting (and boiling) points

123
Q

How are all molecular compounds bonded?

A

covalently bonded

124
Q

What sort of bonding must all compounds with low melting (and boiling) points have?

A

covalent bonding

125
Q

What structure can a compound with covalent bonding have?

A

either a giant structure or simple molecular structure

126
Q

As a compound with covalent bonding can either be a giant structure or simple molecular structure, what can the melting (and boiling) point be like?

A

may have either a high or low melting (and boiling) point

127
Q

What do you do when you heat melt + boil simple molecular compounds?

A

breaking intermolecular forces between molecules, not covalent bonds within them

128
Q

What determines the melting (and boiling) points of simple molecular compounds?

A

strength of intermolecular forces

129
Q

What are the 3 types of intermolecular forces in order of increasing strength?

A

van der Waals

dipole-dipole forces

hydrogen bonds

130
Q

Where do van der Waals forces act?

A

between all atoms

131
Q

Where do dipole-dipole forces act?

A

between molecules with permanent dipoles

132
Q

Where do hydrogen bonds act?

A

between molecules formed when highly electronegative atoms (oxygen, nitrogen and fluorine) + hydrogen atoms are covalently bonded

C3- BONDING (7 decks)

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