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GCSE Science AQA 2016 Onwards > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

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1
Q

Definition of a compound

A

Two or more elements which are chemically combined

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2
Q

Definition of Covalent Bonding

A

Shared pair of electrons

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3
Q

Definition of Ionic Bonding

A

(electrostatic) attraction between oppositely charged ions

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4
Q

Describe the structure of NaCl

A

Giant ionic lattic (structure) electrostatic attraction Between Na+ and Cl-

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5
Q

Type of bonding in graphite

A

Covalent

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6
Q

Describe the structure of diamond

A

Giant covalent structure where each carbon has 4 bonds

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7
Q

Describe the structure of graphite

A

Giant covalent structure where each carbon has 3 bonds. It is arranged in layers.

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8
Q

Definition of Metallic Bonding

A

(electrostatic) attraction between positive metal ions and the delocalised electrons

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9
Q

Type of bonding in CO2

A

Covalent

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10
Q

Describe the structure of CO2

A

Simple molecular

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11
Q

Identify the bonding in H2O and describe its structure

A

Covalent Simple molecular

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12
Q

Identify the type of bonding in copper and describe its structure

A

Metallic Giant metallic lattice

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13
Q

Identify the type of bonding in sodium and describe its structure

A

Ionic Giant ionic lattice

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14
Q

Identify the type of bonding in Ca(OH)2 and describe its structure

A

Ionic Giant ionic lattice

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15
Q

Identify the type of bonding in SiO2 and describe its structure

A

Covalent Giant covalent lattice/structure (giant molecular)

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16
Q

Graphite, diamond, nanotubes and fullerenes are all _________________ of carbon

A

allotropes

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17
Q

Explain why NaCl is a solid at room temperature

A

It has a giant ionic lattice It is held together by ionic bonds which are very strong Therefore it has a high melting point

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18
Q

Explain why oxygen is a gas at room temperature

A

It has a simple molecular structure It is held together by weak intermolecular forces Therefore it has a low melting point

19
Q

Explain why iron is a solid at room temperature

A

It has a giant metallic structure It is held together by strong metallic bonds Therefore it has a high melting point

20
Q

Explain why iron conducts electricity as a solid and liquid

A

It has delocalised electrons which are free to move throughout the metal structure

21
Q

Explain why graphite conducts electricity

A

Each carbon has only 3 bonds. This leaves one delocalised electron Which is free to move throughout the structure

22
Q

Explain why diamond doesn’t conduct electricity

A

Each carbon has 4 bonds. It has no free electrons

23
Q

Explain why sodium chloride doesn’t conduct electricity as a solid

A

The ions can’t move and carry the charge

24
Q

Explain why sodium chloride conducts electricity when dissolved

A

The ions are free to move and carry the charge

25
Q

Explain why carbon dioxide doesn’t conduct electricity

A

Its electrons aren’t free to move and carry the charge

26
Q

Explain why molten magnesium chloride can conduct electricity

A

The ions are free to move and carry the charge

27
Q

Explain why methane is a gas at room temperature

A

It is a simple molecular substance It is held together by weak intermolecular forces Therefore it has a low melting point

28
Q

Explain why graphite has a very high melting point

A

It has a giant covalent structure which is held together by strong covalent bonds which require a lot of energy to break

29
Q

What property makes diamond useful for sharpening knives

A

It is very hard

30
Q

Explain why diamond is so hard

A

It is arranged in a giant lattice Each carbon has 4 bonds The lattice is rigid

31
Q

Explain why thermosetting polymers have high melting points

A

They have crosslinks between the chains made with covalent bonds which are strong

32
Q

What conditions can be changed to make high density polyethene instead of low density polyethene?

A

Temperature

Pressure

33
Q

What is a nanoparticle

A

a particle between 1nm and 100nm in size

34
Q

Why do nanoparticles have different properties?

A

Because they have a much bigger surface area

35
Q

What are the risks of nanoparticles?

A

Their large surface area makes them very reactive/explosive (nano aluminium) Nanoparticles are easily absorbed by the lungs and there is little research into the long term health risks.

36
Q

Explain why copper is used to make wires rather than graphite

A

Copper and graphite both conduct electricity

Copper and graphite both have a high melting point

Graphite is soft and brittle

Copper is strong and ductile

37
Q
A
38
Q

Name properties you would expect of an ionic compound?

A

High melting point

Doesn’t conduct electricity when solid

Conducts electricity when molten or in solution

39
Q

Name properties you’d expect of a simple covalent solid

A

Low melting point

Brittle

Dull

Soft

40
Q

Name properties you’d expect of a metal

A

High melting point

Conducts heat and electricity

Hard

Lustrous (shiny)

Malleable (can be hammered into shape)

Ductile ( can be drawn into wires)

41
Q

What is meant by the term diatomic?

A

molecule containing two atoms

42
Q

Name the diatomic elements

A

Hydrogen, nitrogen, oxygen, fluorine, chlorine, bromine, iodine

(I Bring Clay For Our New House)

(Have NO Fear Ice Cold Beer)

43
Q
A

GCSE Science AQA 2016 Onwards (12 decks)

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