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GCSE Chemistry > Paper 1 > Flashcards

Paper 1 Flashcards

1
Q

What is an ion?

A

An atom that has either gained or lost one or more electrons.

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2
Q

What types of elements do ionic bonds occur between?

A

Metals and non-metals

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3
Q

How are ionic bonds formed?

A

When a metal atom loses electrons to make a positive metal ion and a non-metal atoms gains electrons to form a negative non-metal ion.

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4
Q

What is the formula for ammonium?

A

(NH4)+

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5
Q

What is the formula for hydroxide?

A

(OH)-

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6
Q

What is the formula for nitrate?

A

(NO3)-

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7
Q

What is the formula for carbonate?

A

(CO3)2-

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8
Q

What is the formula for sulphate?

A

(SO4)2-

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9
Q

What types of elements do covalent bonds form between?

A

Non-metals only

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10
Q

How are covalent bonds formed?

A

Two elements react together making a compound and some atoms react by sharing electrons.

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11
Q

What types of elements do metallic bonds form between?

A

Metals only

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12
Q

How do metallic bonds form?

A

Electrostatic attractions between the ions and the free electrons.

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13
Q

Ionic and metallic bonding have ______ electrostatic forces of attraction so consequently have ________ melting and boiling points.

A

Strong
High

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14
Q

Covalent bonding has _______ intermolecular forces

A

Weak

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15
Q

How are giant ionic structures arranged?

A

In a lattice of ions with alternating charges.

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16
Q

How are giant ionic structures held together?

A

By strong electrostatic forces - cannot move as a solid.

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17
Q

Describe a giant ionic structure dissolving in water.

A

The ions separate to form a solution, and the ions can now freely move.

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18
Q

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

A

The ionic bonds are strong and take a lot of energy to break.

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19
Q

Can ionic substances conduct electricity? Why/why not?

A

Yes, when melted or in solution. Because the ions move through the solution, carrying the charge.

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20
Q

Why don’t covalent/simple molecules conduct electricity?

A

They don’t have any charged particles.

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21
Q

Describe the intermolecular forces between polymer molecules.

A

Relatively strong so they’re solids at room temperature.

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22
Q

How does carbon form diamond?

A

Each carbon atom forms 4 covalent bonds with other carbon atoms.

23
Q

Describe the structure and properties of diamond.

A

Very rigid structure
High melting point
Doesn’t conduct electricity - no free electrons or ions

24
Q

How does carbon form graphite?

A

Each carbon atom forms 3 covalent bonds.

25
Q

Describe the structure and properties of graphite.

A

Sheets of carbon arranged in hexagons.
Layers are held together by weak intermolecular forces so are free to move over each other.
High melting point.
One delocalised electron as only 3 of 4 outer electrons are used in bonds.
Conducts electricity and thermal energy.

26
Q

How does carbon form graphene?

A

One sheet of carbon atoms joined together in hexagons.
Only one atom thick.

27
Q

Describe the structure and properties of graphene.

A

Network of covalent bonds so very strong.
Very light.
Delocalised electrons.

28
Q

How does carbon form fullerenes?

A

Hollow molecules of carbon shaped like tubes or balls.
Mainly made up of carbon atoms arranged in hexagons (can contain pentagons or heptagons).

29
Q

What are nanotubes?

A

Fullerenes that are tiny carbon cylinders.
The ratio between the length and diameter of nanotubes is very high.
Good conductors of heat and electricity.

30
Q

What are some uses of fullerenes?

A

Medicine
Catalyst
Lubricant
Strengthening materials
Good electrical conductors

31
Q

metal + acid -> salt + ________

A

Hydrogen

32
Q

What is oxidation?

A

Loss of electrons

33
Q

What is reduction?

A

Gain of electrons

34
Q

Are metals oxidised or reduced?

A

Oxidised

35
Q

Are non-metals oxidised or reduced?

A

Reduced

36
Q

alkali + acid -> salt + ________

A

Water

37
Q

What is a base?

A

Something that will neutralise an acid.

38
Q

What will acids form when added to water?

A

H+

39
Q

What will alkalis form when added to water?

A

OH-

40
Q

H+(aq) + OH-(aq) -> ______

A

H2O(l)

41
Q

acid + base -> salt + ______

A

Water

42
Q

acid + carbonate -> salt + _______ ________ + ________

A

carbon dioxide
water

43
Q

What is a strong acid in terms of dissociation?

A

Almost all of the acid molecules dissociate (fully dissociated)

44
Q

What is a weak acid in terms of dissociation?

A

Hardly any of the acid molecules dissociate (partially dissociated)

45
Q

What is a concentrated solution?

A

Not much water added, have a high molarity value.

46
Q

What is a diluted solution?

A

Lots of water added, low molarity value.

47
Q

What is the molarity of a solution?

A

It tells us how concentrated the solution is.

48
Q

What is a mole/Avogadro’s number?

A

6.02x10^23

49
Q

What are the units of moles?

A

Mol

50
Q

What is the equation that links moles, mass and relative atomic mass?

A

Moles = mass/Mr

51
Q

What is a limiting reagent?

A

The substance in a chemical reaction that is totally used up when the chemical reaction is complete.

52
Q

What is limited by the reagent due to the reaction not continuing once it’s been used up?

A

The amount of product formed.

53
Q

What is the equation that links concentration, moles and volume?

A

Concentration = moles/volume

54
Q

How do we measure volume?

A

dm^3

GCSE Chemistry (4 decks)

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