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AQA GCSE Chemistry > C3 - Structure and Bonding > Flashcards

C3 - Structure and Bonding Flashcards

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1
Q

What structure are giant ionic compounds arranged in?

A

an ionic lattice structure

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2
Q

What is ionic bonding?

A

A metal and a non-metal with opposite charges are attracted to each other due to the electrostatic force.

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3
Q

Three types of bonding

A
  • ionic
  • covalent
  • metallic
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4
Q

What happens to the particles in a body when it melts?

A

The particles gain more energy which breaks the bonds between the particles meaning they can more freely move around.

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5
Q

Does the temperature increase, decrease or stay the same when a body is changing state?

A

The temperature stays the same. The energy being transferred from the surroundings is used to break or join the bonds between the particles in the body.

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6
Q

How many electrons can the first 3 shells hold?

A

1st : 2
2nd : 8
3rd : 8

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7
Q

Why are some atoms stable and some unstable?

A

Stable atoms have filled outer shells
Unstable atoms have incomplete outer shells

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8
Q

define ion

A

an atom with a + or - electrical charge

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9
Q

When can ionic compounds conduct electricity?

A

When they are molten. This is because the ions break free from the lattice structure and electrons are then free to move around - this means they can conduct an electrical current.

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10
Q

Why are most ionic compounds dissolvable in water?

A

A water molecule has a slight positive and negative charge so it can break apart the ionic compound.

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11
Q

What is covalent bonding?

A

Covalent bonding is when multiple non-metal atoms share electrons.

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12
Q

define intramolecular

A

strong bonds inside molecules

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13
Q

define intermolecular

A

a weaker force of attraction that acts between molecules

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14
Q

3 examples of giant covalent structures

A
  • sand (SiO2)
  • diamond (C)
  • graphite (C)
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15
Q

Why are simple covalent molecules gases at room temperature?

A

the molecules are so small that the intermolecular forces are very weak and don’t take much energy to break.

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16
Q

properties of diamond

A
  • high melting and boiling point
  • crystalline shape (not lattice)
  • does not conduct electricity
  • very hard
  • each carbon is bonded to 4 other carbons
17
Q

define hardness

A

the measure of resistance to deformation, e.g. indentation or a scratch

18
Q

properties of graphite

A
  • electrical conductor - each carbon has a delocalised electron
  • soft and slippery - layers slide off easily, used as a lubricant
  • each carbon is bonded to 3 other carbons
19
Q

what are fullerenes

A

giant covalent molecules of carbon atoms with hollow shapes. an allotrope of carbon

20
Q

1 example of a fullerene

A

buckminsterfullerene - C60

aka buckyball

21
Q

properties of fullerenes

A
  • high tensile strength
  • good electrical conductor
  • good thermal conductor
22
Q

what is graphene

A

one atom thick layer of carbon arranged in a hexagonal lattice

23
Q

properties of graphene

A
  • excellent electrical conductor
  • low density
  • very reactive
  • strong for its mass
24
Q

properties of metals

A
  • high melting and boiling points
  • good electrical conductor
  • good thermal conductor
  • malleable
  • ductile
  • sonorous
  • dense
  • strong
25
Q

properties of giant ionic compounds

A
  • form cubic shapes
  • bad electrical conductor unless molten
  • dissolves in water
  • high melting and boiling points
26
Q

How do metals bond?

A

Metallic bonding is when metals bond. They bond because there is an electrostatic attraction between the metal ions (really just the nucleus) and the sea of electrons.

27
Q

define strength

A

how much force can be applied until a body breaks apart

28
Q

Why are metallically bonded structures malleable?

A

The layers in the metal slide over each other when a force is applied.

29
Q

define alloy

A

a mixture of a metal and at least 1 other element

30
Q

Why are alloys stronger than pure metals?

A

alloys are stronger because the mixture of atoms with different radii disrupts the lattice structure causing more difficulty for layers to slide over each other

31
Q

Why do nanoparticles behave differently

A
  • they have a large surface area : volume ratio making them more reactive
  • they are so small quantum mechanics govern them

AQA GCSE Chemistry (6 decks)

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