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CCEA GCSE Chemistry > Structures > Flashcards

Structures Flashcards

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1
Q

Ionic bonding holds ions together in a…?

2 marks

A

Giant Ionic lattice.

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2
Q

What do Covalent Bonds create?

2 marks

A

Simple Molecules or giant Covalent Structures.

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3
Q

Different types of bonding give a substance different properties.
Give 4 Examples.

(4 marks)

A
  • Different melting + boiling points
  • Different electrical conductivity
  • Different solubility in water
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4
Q

What is a giant Ionic Lattice?

2 marks

A

An Ionic Lattice is a three-dimensional structure of oppositely charged Ions held together by Ionic Bonding.

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5
Q

Explain the following Physical Property of Ionic Compounds.
High melting + boiling points:

(3 marks)

A

Ionic solids have a high melting/boiling point because it takes a substantial amount of energy to break the strong Ionic Bonding that hold the Ions together.

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6
Q

What is the Sodium Chloride (NaCl) melting point?

1 mark

A

801°C

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7
Q

What is the Magnesium (Mg) melting point?

1 mark

A

2,852°C

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8
Q

What is the Sodium Chloride (NaCl) boiling point?

1 mark

A

1,413°C

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9
Q

What is the Sodium Chloride (NaCl) boiling point?

1 mark

A

3,600°C

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10
Q

The Ionic Bonding between Mg2+ and O2- Ions is stronger than between…?

(2 marks)

A

Na+ and Cl- Ions.

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11
Q

Explain the following Physical Property of Ionic Compounds.

Electrical Conductivity:

(3 marks)

A

Ionic Compounds conduct electricity when molten or dissolved in water because the Ions can move and carry charge.

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12
Q

Explain the following Physical Property of Ionic Compounds.

Water Solubility:

(2 marks)

A

Most Ionic Compounds are soluble in water and form Aqueous Solutions.

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13
Q

Covalent bonding forms substances with two types of structures.

Name these structures.

(6 marks)

A

Molecular Covalent Structures:
Simple molecules held together by weak forces of attraction.

Giant Covalent Structures:
Many atoms joined together by strong covalent bonds.

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14
Q

What are Molecular Covalent Structures?

2 marks

A

Simple molecules held together by weak forces of attraction.

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15
Q

Give 3 Examples of Molecular Covalent Structures?

3 marks

A

Iodine, Methane and Carbon Dioxide.

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16
Q

What are Giant Covalent Structures?

2 marks

A

Many atoms joined together by strong covalent bonds.

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17
Q

Give 2 Examples of Giant Covalent Structures.

2 marks

A

Diamond and graphite.

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18
Q

What are the atoms in Molecular Covalent Molecules held together by?

(1 mark)

A

Strong Covalent Bonds.

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19
Q

Although Strong Covalent Bonds (the Bonds) are strong, there are only…?

(2 marks)

A

Weak forces of attraction between molecules.

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20
Q

Describe Strong Covalent Bonds.

3 marks

A

Strong bonds with weak forces of attraction.

- They are called ‘van der Waals’ forces and can be broken with little energy.

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21
Q

Give the Physical properties of Molecular Covalent Structures.

(3 marks)

A
  • Low melting and boiling points.
  • Do not conduct electricity.
  • Insoluble in water.
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22
Q

Explain the following Physical property of Molecular Covalent Structures.

Low melting and boiling points:

(3 marks)

A

Little energy is needed to break the weak van der Waals’ forces between the molecules, so Covalent Molecular Structures have low melting and boiling points.

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23
Q

Explain the following Physical property of Molecular Covalent Structures.

Do not conduct electricity:

(4 marks)

A

Covalent Molecular Structures do not conduct electricity because the molecules are Neutral and there are No Charged Particles (no Ions or Electrons) to move and carry charge.

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24
Q

Explain the following Physical property of Molecular Covalent Structures.

Insoluble in water:

(4 marks)

A

Most Covalent Compounds are insoluble in water. Hydrogen Chloride and Ammonia are exceptions, because they react with water.

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25
Q

In Simple terms what is a Giant Covalent Structure?

2 marks

A

Three-dimensional structure of atoms that are joined by covalent bonds.

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26
Q

What are Allotropes?

2 marks

A

Allotropes are different forms of the same Element, in the same state.

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27
Q

Give an Examples of Allotropes.

8 marks

A

Graphite, Graphene and Diamond are Allotropes of the same Element (Carbon) in the same State (Solid).

Carbon can form up to four covalent bonds.

28
Q

Describe Diamond.

5 marks

A

Diamond is a Giant Covalent Structure in which each Carbon atom is Covalently Bonded to 4 other Carbon atoms in a Tetrahedral, 3D structure.

29
Q

List Diamond’s properties.

3 marks

A
  • High melting and boiling points.
  • Does not conduct electricity.
  • Hardness.
30
Q

Describe the following physical property of Diamond.

High melting and boiling points:

(2 marks)

A

Diamond’s many Covalent bonds are strong and substantial energy is needed to break them.

31
Q

Describe the following physical property of Diamond.

Does not conduct electricity:

(3 marks)

A

Diamond has no free Ions or delocalised Electrons to move and carry the charge.

32
Q

Describe the following physical property of Diamond.

Hardness:

(2 marks)

A

Diamond’s 3D Tetrahedral structure with Strong Covalent Bonds makes it very hard.

33
Q

What are Diamond-tipped tools are used for?

3 marks

A

Diamond-tipped tools are used to cut through hard rock, metals and glass.

34
Q

What do the Carbon Atoms in a diamond form?

2 marks

A

The Carbon Atoms in a Diamond form a Regular Tetrahedral structure.

35
Q

What kind of Structure does Ammonia (NH3) have?

2 marks

A

Molecular Covalent Structure.

36
Q

Describe Graphite’s Giant Covalent Structure?

7 marks

A
  • Each Carbon atom forms 3 Covalent bonds with other Carbon atoms.
  • The Carbon atoms form layers of Hexagonal rings, with weak forces of attraction between each layer.
  • There is 1, Non-Bonded – or Delocalised – Electron for each Atom.
37
Q

Give 3 Graphite properties.

3 marks

A
  • High Melting and Boiling point.
  • Good Electrical conductivity.
  • Softness
38
Q

Describe the following Graphite Property.

High melting and boiling points:

(2 marks)

A

Graphite’s many Covalent bonds are strong and substantial energy is needed to break them.

39
Q

Describe the following Graphite Property.

Good electrical conductivity:

(3 marks)

A

Each Carbon atom has an Unbonded Electron. Which are Delocalised electrons that are free to move and carry charge.

40
Q

Describe the following Graphite Property.

Softness:

(2 marks)

A

The weak forces between graphite’s layers allow them to slide.

41
Q

What is Graphite used for?

2 marks

A

Graphite is used as a lubricant and in pencils.

42
Q

What is Graphene?

4 marks

A

Graphene is a Single-atom thick layer of Graphite with Strong Covalent Bonds between each Carbon atom.The atoms are arranged in hexagons.

43
Q

Give 3 properties of Graphene.

3 marks

A
  • High Melting and Boiling point.
  • Good Electrical conductivity.
  • Very Strong
44
Q

Explain the following physical property of Graphene.

High melting and boiling points:

(2 marks)

A

Graphene’s many Covalent bonds are strong and substantial energy is needed to break them.

45
Q

Explain the following physical property of Graphene.

Good Electrical Conductivity:

(3 marks)

A

Each Carbon atom has an Unbonded Electron, which are Delocalised electrons that are free to move and carry charge.

46
Q

Explain the following physical property of Graphene.

Very Strong:

(5 marks)

A

Graphene’s Strong Covalent Bonds makes it 100x stronger than Steel.
It is also the thinnest material possible (1 atom thick) and very lightweight and transparent.

47
Q

Give a brief description of Graphene and what it’s used in/will be used in.

(3 marks)

A

Graphene is a strong, light and relatively inexpensive Electrical Conductor and will be used in Solar cells and batteries.

48
Q

What are Metals?

4 marks

A

Metals are Giant Lattices of positive Ions arranged in regular layers, with Delocalised Electrons free to move throughout the structure.

49
Q

Give 3 Physical Properties of Metallic Structures.

4 marks

A
  • High melting and boiling point.
  • Good Electrical conductivity.
  • Malleable and ductile.
50
Q

Explain the following Physical Properties of Metal.

High melting and boiling points:

(2 marks)

A

High temperatures are required to break strong metallic bonds.

51
Q

Explain the following Physical Property of Metal.

Good Electrical Conductivity:

(2 marks)

A

Metal’s Delocalised Electrons can move and carry charge.

52
Q

Explain the following Physical Property of Metal.

Malleable and ductile:

(6 marks)

A

Metal’s layers of Ions can slide over each other, but are still held together by the Delocalised Electrons.

This means metal is malleable (can be hammered into shape) and ductile(it can be drawn out into wires).

53
Q

What does ‘Malleable’ Structure mean?

1 mark

A

It can be hammered into shape.

54
Q

What does ‘Ductile’ mean?

1 mark

A

It can be drawn out into wires.

55
Q

What is an Alloy?

2 marks

A

An Alloy is a mixture of 2 or more Elements, at least one of which is a Metal.

56
Q

Describe an Alloy’s Structure.

6 marks

A
  • The mixture of (2/+ Elements - 1 being Metal) has metallic properties allowing for a Metallic Structure.
  • different sized Atoms of the different Elements distort this structure making it more difficult for the layers to slide over one another. Making them harder than Pure Metals.
57
Q

What is the Gold used for jewellery alloyed with?

2 marks

A

Other metals, often Silver, Copper or Zinc. This strengthens the jewellery while maintaining its shine.

58
Q

What is the proportion of Gold in an Alloy measured in? Describe this.

(5 marks)

A

The proportion of Gold in an Alloy is measured in Carats.

  • 24 carat Gold = Pure Gold,
  • 18 carat Gold = 75% Pure Gold
59
Q

Describe the Melting point of the following structures.

Giant Ionic Lattice, Molecular Covalent, Metallic Lattice, Giant Covalent (Diamond), Giant Covalent (Graphite and Graphene)

(10 marks)

A

Giant Ionic Lattice - High

Molecular Covalent - Low

Metallic Lattice - Usually High

Giant Covalent (Diamond) - High

Giant Covalent (Graphite and Graphene) - High

60
Q

Describe the Water Solubility of the following Structures.

Giant Ionic Lattice, Molecular Covalent, Metallic Lattice, Giant Covalent (Diamond), Giant Covalent (Graphite and Graphene)

(10 marks)

A

Giant Ionic Lattice - Soluble

Molecular Covalent - Insoluble

Metallic Lattice - Insoluble

Giant Covalent (Diamond) - Insoluble

Giant Covalent (Graphite and Graphene) - Insoluble

61
Q

Describe the Electrical Conductivity of the following Structures.

Giant Ionic Lattice, Molecular Covalent, Metallic Lattice, Giant Covalent (Diamond), Giant Covalent (Graphite and Graphene)

(11 marks)

A

Giant Ionic Lattice - Conductive when molten or dissolved

Molecular Covalent - Not conductive

Metallic Lattice - Conductive

Giant Covalent (Diamond) - Not conductive

Giant Covalent (Graphite and Graphene) - Conductive

62
Q

List the structures with a High Melting Point.

7 marks

A
  • Giant Ionic Lattice,
  • Giant Covalent (Diamond),
  • Giant Covalent (Graphite and Graphene),
  • Metallic Lattice (Usually High)
63
Q

Give the structure with a Low Melting Point.

1 mark

A

Molecular Covalent

64
Q

Give a Soluble structure.

1 mark

A

Giant Ionic Lattice

65
Q

List the Insoluble structures.

5 marks

A
  • Molecular Covalent,
  • Metallic Lattice,
  • Giant Covalent (Diamond),
  • Giant Covalent (Graphite and Graphene)
66
Q

List the Conductive structures.

5 marks

A
  • Giant Ionic Lattice; Conductive when molten or dissolved
  • Metallic Lattice
  • Giant Covalent (Graphite and Graphene)
67
Q

List the structures which are Not Conductive.

3 marks

A
  • Molecular Covalent

- Giant Covalent (Diamond)

CCEA GCSE Chemistry (7 decks)

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