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GCSE Chemistry > Structures > Flashcards

Structures Flashcards

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1
Q

4 types of structures

A

Giant Ionic Lattice
Covalent Molecular
Giant Covalent Structure
Giant Metallic Structure

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2
Q

Giant ionic lattice example

A

Sodium chloride
Magnesium Oxide

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3
Q

Giant Ionic Lattice Properties

A

1) High Melting / Boiling Point
2) Hard but brittle
3) Soluble in Water
4) Conducts electricity when molten of in a solution

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4
Q

Why does a giant ionic lattice have a high melting point

A

To melt, a large number of strong ionic bonds must be broken. This requires a large amount of energy

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5
Q

why is a giant ionic lattice hard but brittle

A

A slight shift in ions can move the layer of ions. Ions of the same charge repel each other

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6
Q

Why is a giant ionic lattice soluble in water

A

Water molecules surround ions and hydrate them

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7
Q

Why does a giant ionic lattice conduct electricity when molten or in a solution but not as a solid

A

Ions can only move when molten or in a solution to conduct. As a solid they are held in a strong lattice

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8
Q

Covalent molecular examples

A

Iodine, carbon dioxide, water

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9
Q

Properties of covalent molecular

A

1) low melting and boiling points
2) most not soluble in water but some are
3) don’t conduct electricity
4) soft when solid

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10
Q

Why does covalent molecular have low melting and boiling points

A

Only the Van der Waal forces between molecules need to be broken and these are weak so only a small amount of energy is needed

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11
Q

Why doesn’t covalent molecular conduct electricity

A

No charged particles like ions or free electrons present so there is no attraction to electrodes

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12
Q

Why is covalent molecular soft when solid

A

Weak Van der Waal forces are easy to shift around

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13
Q

Allotropes of carbon

A

Diamond, graphite and Graphene

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14
Q

Properties of diamond

A

1) Very high melting point
2) insoluble in water
3) doesn’t conduct electricity
4) very hard substance

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15
Q

Why does diamond have a very high melting point (3500°C)

A

Many strong covalent bonds must be broken

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16
Q

Why doesn’t diamond conduct electricity

A

There is no free electrons or ions

17
Q

Why is diamond a very hard substance

A

It has a highly regular structure

18
Q

Properties of graphite

A

1) High melting point
2) insoluble in water
3) conducts electricity
4) soft and slippery

19
Q

Why does graphite have a high melting point

A

Many strong covalent bonds must be broken which requires a lot of energy

20
Q

Why does graphite conduct electricity

A

Has a layer of free electrons that can flow as a current

21
Q

Why is graphite soft and slippery

A

The layers slide over each other easily. It’s used in pencils and lubricants

22
Q

Properties of Graphene

A

1) Very light and thin
2) transparent
3) 100 times stronger than steel
4)very good conductor
5) used in batteries and solar cells

23
Q

Properties of a giant metallic structure

A

1) High melting points
2) malleable and ductile
3) conducts heat and electricity
4) insoluble in water (many react)

24
Q

Why do giant metallic structures have high melting points

A

The bond between the free electrons and the positive metal ions is very strong and requires a lot of energy to break

25
Q

Why are giant metallic structures malleable and ductile

A

The metal ions are arranged in layers and slip over each other easily

26
Q

Why do giant metallic structures conduct heat and electricity

A

Delocalised electrons are free to move so they can carry an electrical current

27
Q

Allotrope

A

Different forms of the same element in the same physical state

28
Q

Ductile

A

Can be drawn out into wires

29
Q

Malleable

A

Can be hammered into shape

30
Q

What is metallic bonding

A

The attraction between delocalised electrons and positive ions in a regular lattice

31
Q

What is an alloy

A

A mixture of two or more elements, at least one of which is a metal, and the resulting mixture has metallic properties

32
Q

Examples of alloys

A

Brass = copper + zinc (5-45%)
bronze = 60% copper + 40% tin
gold = gold + silver
steel = iron + carbon

33
Q

Properties of alloys

A

Harder than pure metals
still conducts electricity

34
Q

Why is an alloy is harder than pure metal

A

The different sizes disrupts regular layers making it harder for layers to slide over each other

35
Q

Why can an alloy still conduct electricity

A

Free electrons can still move in the structure

GCSE Chemistry (7 decks)

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