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AQA GCSE Chemistry > C2: Structure and Bonding > Flashcards

C2: Structure and Bonding Flashcards

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1
Q

Describe ionic bonding.

A

Metals transfer their electrons to non-metals, creating a positive metal ion and negative non-metal ion. (LIP/GIN) Strong electrostatic attraction holds the two oppositely charged ions together.

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2
Q

Describe covalent bonding.

A

Two non-metals share pairs of electrons to form strong covalent bonds.

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3
Q

Describe metallic bonding.

A

Two metals bond through sharing a sea of delocalised electrons, creating strong electrostatic attraction between the electrons and the ions.

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4
Q

How do you work out the charge of an element’s ion?

A

By looking at the group number, which shows the number of outer shell electrons, and determining how many electrons should be lost/gained to make a full outer shell. Loss is Positive, Gain is Negative.

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5
Q

What does LIP/GIN stand for?

A

Loss is positive, gain is negative. (of electrons)

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6
Q

What should you always remember when drawing an ionic bonding diagram?

A
  • Representing electrons, one ion has dots, the other has crosses.
  • Both have brackets and charges around the outside.
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7
Q

Describe 2 limitations of using dot and cross diagrams to represent ionic structure.

A
  1. They don’t show the 3D arrangements of the atoms and electron shells.
  2. They don’t show the relative sizes of the atoms.
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8
Q

What is an ionic compound?

A

A giant structure of ions, held together by strong electrostatic forces between oppositely charged ions. These forces act in all directions in the lattice.

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9
Q

Why can ionic substances only conduct electricity when molten or dissolved?

A

Because when molten or dissolved, the ions and electrons are free to move and carry charge.

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10
Q

Why do ionic compounds have high melting and boiling points?

A

They have a high boiling point because much energy is needed to overcome the strong electrostatic attraction.

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11
Q

Describe the properties of ionic compounds.

A

They only conduct electricity when molten or dissolved and they have high melting and boiling points.

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12
Q

Describe the properties of giant covalent structures.

A

They have high melting and boiling points and cannot conduct electricity.

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13
Q

Why do giant covalent structures have high melting and boiling points?

A

They have a high boiling point because much energy is needed to overcome the strong covalent bonds.

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14
Q

Why can’t giant covalent structures conduct electricity?

A

Because they have no electrons that are free to move and carry charge.

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15
Q

Why are metals good at conducting electricity?

A

Because they are metallically bonded, so contain a sea of delocalised electrons that are free to move and carry charge.

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16
Q

What are the limitations of the particle model of the states of matter?

A

They don’t show forces, and all particles are represented as solid spheres, which isn’t accurate.

17
Q

What should you remember when writing ionic equations?

A

State symbols.

18
Q

What are the 4 state symbols?

A

(s) - solid
(l) - liquid
(aq) - aqueous
(g) - gas

19
Q

What is an aqueous solution?

A

A type of solution in which water is the solvent.

20
Q

What is a simple molecule?

A

Usually a gas or liquid, bonded by weak intermolecular forces.

21
Q

What are the properties of simple molecules?

A

Relatively low melting and boiling points. (M/B point increases as simple molecules get bigger). They don’t conduct electricity.

22
Q

Why do simple molecules have low melting and boiling points?

A

Because less energy is needed to overcome the weak intermolecular forces.

23
Q

Why don’t simple molecules conduct electricity?

A

Because the molecules do not have an electric charge.

24
Q

What is a polymer?

A

Very large molecules linked by covalent bonds, with strong intermolecular forces between molecules, so they are solid at room temperature.

25
Q

Why might a substance be a solid at room temperature?

A

Because it has a high melting and boiling point.

26
Q

Why might a substance be a gas at room temperature?

A

Because it has a low melting and boiling point.

27
Q

Describe the structure and properties of Diamond.

A
  • Carbon allotrope.
  • Each carbon atom forms 4 covalent bonds with other carbon atoms.
  • It has a giant covalent structure.
  • So diamond is very hard, has a very high melting point and does not conduct electricity.
28
Q

Describe the structure and properties of Graphite.

A

-Carbon allotrope.
- Each carbon atom forms 3 covalent bonds with three other carbon atoms.
- It has layers of hexagonal rings which have no covalent bonds between the layers.
- 1 electron from each carbon atom is delocalised.
-So graphite is

29
Q

Describe the structure and properties of Graphene.

A
30
Q

What is an allotrope?

A
31
Q

Name the 3 main allotropes of carbon.

A

Diamond, Graphite and Graphene.

32
Q

Describe the properties of metals.

A

High melting and boiling points, and good conductors of electricity.

33
Q

Why do metals have high melting and boiling points?

A

Because they have many strong electrostatic forces which take much energy to overcome.

34
Q

Why are metals good conductors of thermal energy?

A

Because energy is transferred by the delocalised electrons.

35
Q

What is an alloy?

A

A mixture of 2+ elements, where at least 1 is a metal.

36
Q

What are nanoparticles?

A
37
Q

What are the 6 uses of nanoparticles?

A
  • Medicine.
  • Cosmetics.
  • Sun creams.
  • Deodorants.
  • Catalysts.
  • Electronics.
38
Q

What are the risks of using nanoparticles?

A
39
Q

Name 3 nanoparticle structures.

A

Buckminsterfullrene, Graphene, Nanotubes.

AQA GCSE Chemistry (11 decks)

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