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Alevel Chemistry AQA > 3.1.3 Bonding > Flashcards

3.1.3 Bonding Flashcards

1
Q

Substance

A

Made out of one repeating unit

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2
Q

What is a mixture

A

Made out of different repeating units

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3
Q

What is a compound?

A

A substance containing atoms of more than one element

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4
Q

What is the electron sea model

A

Metals are made up of a lattice of cation surrounded by a sea of delocalised electrons.

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5
Q

How do delocalised electrons allow a metal to conduct electricity

A

They are freely moving throughout the metal and are charged

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6
Q

What is metallic bonding?

A

The electrostatic attraction between cations and delocalised electrons.

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7
Q

Why are metals malleable and ductile?

A

The layers of cations can slide over each other without breaking any metallic bonding

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8
Q

Why do metals have high melting and boiling point?

A

They have strong electrostatic attraction between the cation and delocalised electrons

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9
Q

Why does the melting point of metals increase across a period?

A

Group 1 metals form + charges
Group 2 metals form 2+ charges
Group 3 metals form 3+ charges
This means that as they go across the melting point increases as they form metallic bonding with more higher charged cations

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10
Q

Down a group, the melting point….

A

Decreases.

This is because the size of the cations increase which means theres a larger distance between the nucleus and outer electrons so there are weaker attraction

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11
Q

State and explain the general trend in melting point if the period 3 metals.

A

Across a period the charge of the cation increases, so there is a stronger attraction between the cation and delocalised electrons.

This stronger attraction means the strength of the metallic bonding increases across a period and so therefore the melting point too

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12
Q

What are positively charge ions called?

A

Cations

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13
Q

What are negatively charged ions called?

A

Anions

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14
Q

Define ionic bonding.

A

Electrostatic forces of attraction between oppositely charged ions formed by electrons transfer

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15
Q

What are the simplest ion

A

a single atom which have either lost/gain electrons so that they’ve got a full outer shell.

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16
Q

What are ionic crystals called?

A

giant lattice of ions.

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17
Q

Is the melting a point of ionic compounds high or low?

A

High

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18
Q

Charge of sliver

A

+

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19
Q

Charge of Zinc

A

2+

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20
Q

Charge of iron

A

2+/ 3+

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21
Q

Charge of copper

A

+\2+

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22
Q

Charge of lead

A

2+\4+

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23
Q

Sulfate ion and charge

A

So4(2-)

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24
Q

Nitrate ion and charge

A

NO3(-)

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25
Q

Manganate ion and charge

A

MnO4(2-)

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26
Q

Phosphate ion and charge

A

PO4 (3-)

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27
Q

Hydrogen carbonate ion and charge

A

HCO3(-)

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28
Q

Hydroxide ion and charge

A

OH(-)

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29
Q

What state can ionic compounds conduct electricity

A

Liquid or molten as they are free to move around.

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30
Q

Why do ionic compounds have high melting and boiling points?

A

There is a strong attraction between the cations and anions

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31
Q

The larger the charge between two charges the ___ the ionic bonding is

A

Stronger

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32
Q

The ____ the distance between two ions the _____ the ionic bonding

A
  1. Larger
  2. Weaker
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33
Q

Down a group the size of ions…

A

Increases

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34
Q

When are covalent bonds formed

A

When atoms share a pair of electrons

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35
Q

Examples of micromolecular structures

A
  1. Graphite
  2. Diamond
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36
Q

what is the structure of graphite?

A

Carbon is arranged in sheets of flat hexagon. The fourth outer electron of each carbon atom is delocalised.

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37
Q

what property graphite used as dry lubricant and pencils

A

the weak bonds between the layers in graphite are easily broken, so the sheets can slide over.

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38
Q

explain why graphite is a good electrical conductor.

A

the delocalised electrons in graphite aren’t attached to any carbon. Therefore, are free to move and can conduct electricity.

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39
Q

Explain why graphite has a very high melting point.

A

They have strong covalent bonds which need high amounts of energy to overcome.

40
Q

Explain why graphite is insoluble in any solvent.

A

The covalent bond s are too strong to break so therefore they aren’t able to dissolve.

41
Q

Substance made of molecules have

A
  1. Low melting and boiling point
  2. Dont conduct electricity
42
Q

what is diamond made up of?

A

it is made up of carbon atoms. Each carbon atom is covalently bonded to four other carbon atoms. They arrange themselves in a tetrahedral shape.

43
Q

Properties of diamond:

A
  1. very high melting point
  2. good thermal conductor
  3. can’t dissolve in any solvent.
44
Q

What is a dative bond

A

One atom contributes both electrons to the shared pair

45
Q

To have a dative bond you need..

A

A dative bond donor- a lone pair of electrons

46
Q

What is valence bond theory?

A

It states that if two atoms have orbitals which contain unpaired or single electrons then the orbitals will overlap, forming a covalent bond.

47
Q

Sigma bonds

A

Overlap end on

48
Q

Pi bonds

A

Overlap side on

49
Q

What will an oxygen-oxygen double bond form

A

One pi bond and one sigma bond

50
Q

What will two nitrogen atoms form when triple bonded?

A

1 sigma bond and 2 pi bond

51
Q

What do double bonds consist of?

A

All double bonds consist of one sigma bond and one pi bond.

52
Q

What do single bonds consist of

A

Sigma bonds

53
Q

What is electronegativity

A

An atoms’s ability to attract electrons in a covalent bond

54
Q

What are the two factors that determine the strength of ionic bonding?

A

1.The charge.
Larger charge=stronger ionic bonding

  1. Larger ions.
    Larger ions = weaker ionic bonding.
55
Q

What is an isoelectric ion?

A

Ions with the same number of electrons

56
Q

How could we determine the size of isoelectric ions?

A

As they have the same number of electrons, the ions with the higher nuclear changes is the smallest.

57
Q

Are ionic compounds soluble or insoluble?

A

Soluble in water

58
Q

Can ionic compounds conduct electricity?

A

Yes! When they are molten

59
Q

What are atoms in molecules held together by?

A

Covalent bonds

60
Q

What is a molecule?

A

An uncharged group of two or more atoms stuck together

61
Q

What is a covalent bond?

A

When two atoms share a pair of electrons.

62
Q

What are the two factors that affect the length of a covalent bond?

A
  1. The size of the atoms
    Larger atoms form longer bonds
  2. Single,double or triple bond.
    Single is the longest and triple is the shortest .
63
Q

The shorter a bond, the ____ the covalent bond is.

A

Stronger

64
Q

What is a dative covalent bond?

A

When one atom contributes both electrons to the shared pair.

65
Q

What is a dative bond represented with?

A

——>

66
Q

When do dative bonds form?

A

Generally with species that have a lone pair.

67
Q

Do covalent bonds have higher or low melting and boiling points?

A

Low melting and boiling point!

68
Q

Can covalent compound conduct electricity?

A

No they can’t

69
Q

Where does the electron pair typically lie?

A

Close to the more electronegative atoms

70
Q

What are the trend in electronegativity across a period?

A

It increases across a group of

71
Q

What are the trends in Electronegativity across a period?

A

Increases across a period.

72
Q

What are the trends in Electronegativity across a period?

A

Increases across a period.

73
Q

What are the trends in Electronegativity down a group?

A

Decreases down a group

74
Q

What are intermolecular forces?

A

Forces between molecules.

75
Q

What are the three types of intermolecular forces?

A

Dipole-dipole
Van der waals
Hydrogen bonding

76
Q

What are dipole dipole forces?

A

These form between molecules with permanent dipoles/ polar molecules.

77
Q

What is hydrogen bonding?

A

When a hydrogen is directly bonded to a N/O/F

78
Q

What are van der waals forces?

A

When the movement of of electrons in a molecules create s temporary dipoles

79
Q

What force do all molecules have?

A

Wan der waals forces

80
Q

When melting and boiling a substance what gets weakened?

A

The intermolecular forces not the bonding eg covalent bonds

81
Q

Are non polar molecules soluble?

A

No they aren’t
Only polar are soluble

82
Q

What are molecular solids?

A

Solids that are held together by intermolecular forces

83
Q

Examples of intermolecular solids?

A

Ice
Iodine

84
Q

What is a macromolecule?

A

A massive Covalently bonded molecule which consists of thousands of atoms

85
Q

When a lattice is made up of macromolecules what do we call it?

A

Giant covalent lattice

86
Q

What is diamond?

A

A macromolecule held together by covalent bonds between carbon atoms

87
Q

In diamond each carbon atom bonds to how many other carbon atoms?

A

4 other carbon atoms

88
Q

In graphite each carbon atom bonds to how many other carbon atoms ?

A

3 different carbon atoms

89
Q

What is graphite?

A

A macromolecule with sheets held by intermolecular forces (vdw).

90
Q

What are allotropes?

A

The different structures that can form when atoms of that element bond together.
Eg carbon made diamond and graphite

91
Q

Why do graphite have delocalised electrons?

A

In graphite, each carbon uses 3 electrons to make single bonds to other carbon atoms. This leaves one electron in the 2p orbital. These 2p orbitals overlap and have delocalised electrons.- bonding between carbons are strong due to this

92
Q

Why can graphite conduct electricity but diamond can’t?

A

Graphite has delocalised electrons which can move freely between each layer and carry a charge. Diamonds outer electrons are in a covalent bond so there are not delocalised electrons to carry a charge.

93
Q

Why is graphite so soft?

A

As to separate the layers in graphite you only need to break the weak intermolecular forces between them.

94
Q

Why is diamond so hard?

A

You need to break strong C-C bonds

95
Q

Why do graphite and diamond have high melting points?

A

as you need to break the string covalent bonds between the carbon atoms

Alevel Chemistry AQA (24 decks)

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