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AQA A Level Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

Give an example of an ionic substance

A

Sodium chloride

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2
Q

Give an example of a molecular substance

A

Methane gas

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3
Q

Give an example of a macromolecular substance

A

Graphite/ Diamond

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4
Q

Give an example of a metallic substance.

A

Magnesium

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5
Q

What is co-ordinate bonding a type of?

A

Covalent bond

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6
Q

What is another name for a co-ordinate bond?

A

Dative covalent bond

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7
Q

Why do molecules adopt certain shapes?

A

The bonding pairs of electrons repel each other equally

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8
Q

What do straight lines mean on 3d drawings of molecules?

A

It is on the same plane as the paper

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9
Q

What do wedges mean on 3d drawings of molecules?

A

In front of the plane of the paper

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10
Q

What do dashed lines mean on 3d drawings of molecules?

A

Behind the plane of the paper

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11
Q

What is the name of a molecule with 2 bonding pairs?

A

Linear

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12
Q

What is the bond angle of a molecule with 2 bonding pairs?

A

180 degrees

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13
Q

What is the name of a molecule with 3 bonding pairs?

A

Trigonal planar

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14
Q

What is the bond angle of a molecule with 3 bonding pairs?

A

120 degrees

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15
Q

What is the name of a molecule with 4 bonding pairs?

A

Tetrahedral

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16
Q

What is the bond angle of a molecule with 4 bonding pairs?

A

109.5 degrees

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17
Q

What is the name of a molecule with 5 bonding pairs?

A

Trigonal bipyramidal

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18
Q

What are the bond angles of a molecule with 5 bonding pairs?

A

90 degrees and 120 degrees

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19
Q

What is the name of a molecule with 6 bonding pairs?

A

Octahedral

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20
Q

What is the bond angle of a molecule with 6 bonding pairs?

A

90 degrees

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21
Q

When a lone pair is present in a molecule is the repulsion of electrons equal?

A

NO

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22
Q

What is the order of repulsion for electrons? (greatest to weakest)

A

lone pair : lone pair > lone pair : bonding pair > bonding pair : bonding pair

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23
Q

What is the name of the molecule where there are 4 electron regions, but one of those is a lone pair?

A

Pyramidal

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24
Q

What is the bond angle of the molecule where there are 4 electron regions, but one of those is a lone pair?

A

107 degrees

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25
Q

What is the name of the molecule where there are 4 electron regions, but two of those are lone pairs?

A

Bent

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26
Q

What is the bond angle of the molecule where there are 4 electron regions, but two of those are lone pairs?

A

104.5 degrees

27
Q

What is the name of the molecule where there are 3 electron regions, but one of those is a lone pair?

A

Non-linear

28
Q

What is the bond angle of the molecule where there are 3 electron regions, but one of those is a lone pair?

A

117.5 degrees

29
Q

When are ions form?

A

When electrons are transferred from one atom to another

30
Q

What does electrostatic attraction hold together?

A

Positive and negative ions

31
Q

What structure does ionic bonding form?

A

Lattice

32
Q

When do you get an ionic compound?

A

When oppositely charged ions come together and form ionic bonds

33
Q

Describe the electrical conductivity of ionic compounds.

A

Conduct electricity when they’re molten or dissolved - not when solid

34
Q

Why can ionic compounds conduct electricity in liquids but not in solids?

A

Ions are free to move and carry charge in liquids
Fixed in position by strong ionic bonds in solids

35
Q

Describe the melting point of ionic compounds.

A

Have high melting points
Giant ionic lattices are held together by strong electrostatic forces
Takes loads of energy to overcome these forces

36
Q

Describe the solubility of ionic compounds.

A

Tend to dissolve in water
Water molecules are polar and pull the ions away from the lattice and cause it to dissolve

37
Q

When do molecules form?

A

When two or more atoms bond together

38
Q

What are molecules held together by?

A

Strong covalent bonds

39
Q

Describe single covalent bonds.

A

Contains a shared pair of electrons
Both of the positive nuclei are attracted electrostatically to the shared pair of electrons

40
Q

What are simple covalent compounds?

A

Compounds that are made up of lots of individual molecules
Atoms in molecules are held together by strong covalent bonds
Molecules within compound held by IMFs

41
Q

What determines the properties of simple covalent compounds?

A

The IMFs between the molecules

42
Q

What are the properties of simple covalent structures?

A

Have low melting and boiling points
Are electrical insulators

43
Q

Describe the structure of graphite.

A

The carbon atoms in graphite are arranged in sheets of flat hexagons covalently bonded with three bonds each
Fourth electron of each carbon atom is delocalised
Sheets of hexagons bonded together by weak van der Waals forces

44
Q

Name 5 of graphite’s properties.

A

It is a lubricant
Electric current can flow
Has a low density
Has a very high melting point
Insoluble

45
Q

Why is graphite a lubricant?

A

Weak bonds between the layers in graphite are easily broken so the sheets can slide over each other

46
Q

Why can an electric current flow in graphite?

A

The delocalised electrons are free to move along the sheets so an electric current can flow

47
Q

Why does graphite have a low density?

A

Layers are quite far apart compared to the length of the covalent bonds

48
Q

Why does graphite have a very high melting point?

A

Because of the strong covalent bonds in the hexagon sheets

49
Q

Why is graphite insoluble in any solvent?

A

Covalent bonds in the sheets are too strong to break

50
Q

Describe the structure of diamond.

A

Each carbon atom is bonded to four other carbon atoms
Atoms arrange themselves in a tetrahedral shape.

51
Q

Name 5 properties of diamond.

A

Has a very high melting point
Extremely hard
Good thermal conductor
Can’t conduct electricity
Doesn’t dissolve in any solvent

52
Q

Define electronegativity.

A

The ability of an atom to attract the pair of electrons in a covalent bond towards itself.

53
Q

What are the two factors that affect electronegativity?

A

Nuclear charge
Atomic radius / shielding

54
Q

How does nuclear charge affect electronegativity?

A

Increase in nuclear charge (no of protons) and no change in shielding
Increased attraction of bonding pair of electrons to nucleus

55
Q

How does atomic radius / shielding affect electronegativity?

A

Increase in electron shells (energy levels) means more shielding of nuclear charge
Weaker attraction of bonding pairs of electrons to nucleus

56
Q

Is C-H a polar bond?

A

No

56
Q

What element has the highest electronegativity on the periodic table?

A

Fluorine

57
Q

What is the general trend of electroneagtivity?

A

Increases across period
Decreases down group

58
Q

What is a polar molecule?

A

Charge is not symmetrically distributed so that one are is slightly positively charged and the other negatively charged
It has a permanent dipole

59
Q

What must a molecule have to be a polar molecule?

A

An asymmetrical distribution of polar bonds

60
Q

Name the intermolecular forces in order of increasing strength.

A
  1. Van der Waals forces
  2. Dipole-dipole forces
  3. Hydrogen bonding
61
Q

Where do van der Waals act?

A

Between ALL atoms and molecules

62
Q

Where do dipole-dipole forces work?

A

Act between polar molecules.

63
Q
A

AQA A Level Chemistry (4 decks)

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