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Chemistry GCSE > Structures > Flashcards

Structures Flashcards

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1
Q

What is a giant ionic lattice

A

Regular arrangement of alternating positive and negative ions

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2
Q

Examples of giant ionic lattice

A

Sodium chloride

Magnesium oxide

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3
Q

Properties of a giant ionic lattice

A

Crystalline

High melting points

Conducts electricity when liquid

Doesn’t conduct electricity when solid

Soluble in water

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4
Q

Why is a giant ionic lattice got high melting points

A

Ionic bonds are strong and require a lot of energy to break therefore it has a high melting point.

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5
Q

Why does a giant ionic lattice conduct electricity when a liquid but not when a solid

A

It doesn’t conduct electricity when a solid because ions are not free to move and carry charge, the ions are free to move and carry charge when liquid therefore able to conduct electricity.

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6
Q

What properties does a covalent molecular have

A

Low melting and boiling points

Doesn’t conduct electricity,

Not soluble in water

Soft when solid

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7
Q

Why does a covalent molecular have low melting and boiling points

A

Due to weak bonds between molecules breaking easily as requires little energy to break

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8
Q

Why does a covalent molecular not conduct electricity

A

No charged particles that are free to move and carry charge

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9
Q

Why is a covalent molecular soft when solid

A

Due to the weak bond between molecules breaking easily

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10
Q

What is the name of the forces between the molecules in simple covalent structures

A

Van Der Waals

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11
Q

Examples of a covalent molecular

A

Iodine
Carbon dioxide
Water
Ammonia
Methane

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12
Q

What is Giant covalent DIAMOND

A

Extensive covalent bonding in all directions with each carbon bonded to 4 others in a tetrahedral arrangement

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13
Q

What might the giant covalent DIAMOND be used for

A

Used in drill bits

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14
Q

Features of the giant covalent bond DIAMOND

A

Very high melting and boiling points

Diamond doesn’t conduct electricity

Insoluble in water

Diamond is extremely hard

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15
Q

Why does the giant covalent DIAMOND have very high melting and boiling points

A

Due to strong covalent bonds requiring large amounts of energy to break

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16
Q

Why does the giant covalent DIAMOND not conduct electricity

A

No charged particles free to move and carry charge

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17
Q

Why is the giant covalent DIAMOND very hard

A

Due to the extensive strong covalent bonds

18
Q

What is the giant covalent GRAPHITE

A

Layered structure with each carbon bonded to 3 others in the layer

19
Q

What might the giant covalent GRAPHITE be used in

A

Lubricant and pencil led

20
Q

There is ….. free electron per each carbon atom which becomes delocalised in the giant covalent

A

One

21
Q

The giant covalent GRAPHITE has weak ….

A

Van der waals between layers

22
Q

Describe the giant covalent graphite

A

A slippery soft solid as weak van der waals between layers allows the layers to slide over each other

23
Q

Properties of the giant covalents graphite and graphene

A

Conducts electricity as they have delocalised electrons free to move and carry charge

24
Q

Giant covalent Graphene properties

A

Conducts heat and electricity efficiently

Nearly transparent

100x stronger then steel

Very thin

Light

Inexpensive

25
Q

What is might the giant covalent Graphene be used for

A

Solar cells, light emitting diodes, touch panels, smart windows or phones

26
Q

Describe the giant covalent GRAPHENE

A

It is a single atom thick layer of graphite with strong covalent bonds between each carbon atom. The atoms are arranged in hexagons / two dimensional

27
Q

What is a giant metallic structure

A

Regular arrangement of closed packed metal ions in a sea of delocalised electrons

28
Q

Properties of a giant metallic structure

A

High melting points

Dense and strong

Conducts electricity

Conducts heat

Ductile

Malleable

29
Q

Why does a giant metallic structure have a high melting point and is strong and dense

A

Strong metallic bonds require a lot of energy to break

30
Q

How can a giant metallic structure conduct electricity

A

Free delocalised electrons are free to move and carry charge

31
Q

Why is a giant metallic structure ductile and malleable

A

Can be reshaped without falling apart as metal ions slide over each other and are still held in place by delocalised electrons

32
Q

Why does a giant metallic structure conduct heat

A

Free elections with high kinetic energy can move around and transfer particles.

33
Q

What is an alloy

A

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

34
Q

Example of alloys

A

Steel is a alloy of IRON + CARBON

white gold is a alloy of SILVER + GOLD

rose gold is a alloy of GOLD + COPPER

brass is a alloy of ZINC + COPPER

35
Q

What unit is used to measure the percentage of gold in alloys

A

Carats

36
Q

How to find the percentage of gold in a alloy

A

Number of carats ➗ 24 ✖️ 100

37
Q

What are allotropes

A

Different forms of the same element in the same physical state

38
Q

Ductile meaning

A

Can be drawn into wires

39
Q

Malleable

A

Can be hammered into shape

40
Q

Metallic bonding Meaning

A

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

Chemistry GCSE (7 decks)

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