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Paper 1 GCSE Chemistry EC > Unit 2: Bonding > Flashcards

Unit 2: Bonding Flashcards

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1
Q

What charge do electrons have?

A

-1

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2
Q

What charge will an ion of lithium take?

A

1+ (one electron in the outer shell, needs to lose it)

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3
Q

What charge will an ion of beryllium take?

A

2+ (two electrons in the outer shell, needs to lose them both)

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4
Q

What charge will an ion of barium take?

A

2+ (group 2 so two electrons in the outer shell, needs to lose them both)

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5
Q

What charge will an ion of fluorine take?

A

1- (7 electrons in the outer shell, needs to gain one)

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6
Q

If something has gained electrons, what charge will it have?

A

Negative

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7
Q

If something has lost electrons, what charge will it have?

A

Positive (because they have lost a negative!)

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8
Q

What is reduction in terms of electrons?

A

Reduction is gain of electrons

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9
Q

What is oxidation in terms of electrons?

A

Oxidation is lossof electrons

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10
Q

Why do atoms transfer electrons in ionic bonding?

A

So that they can have full outer shells

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11
Q

Why do sodium ions and chlorine ions form an ionic bond?

A

There is an electrostatic force of attraction between oppositely charged ions

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12
Q

What is the name for a substance made of billions of oppositely charged ions joined together?

A

Giant ionic lattice

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13
Q

Define giant ionic lattice

A

A huge 3D network of ions

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14
Q

State the melting points of ionic substances

A

High

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15
Q

What is an ionic bond?

A

Strong electrostatic attraction between oppositely charged ions

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16
Q

Explain why ionic substances have high melting points.

A

Strong bonds between oppositely charged ions are hard to break

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17
Q

Will NaCl(s) conduct electricity?

A

No- (s) is solid

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18
Q

Will NaCl (aq) conduct electricity?

A

Yes (aq stands for aqueous which means it is dissolved in water)

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19
Q

Will NaCl (l) conduct electricity?

A

Yes- (l) is liquid or molten

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20
Q

Explain why ionic compounds do not conduct electricity when solid

A

Because the ions are not free to move

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21
Q

Explain why ionic compounds conduct electricity in solution

A

Because the ions are free to move

22
Q

When do ionic bonds form?

A

Between a metal and a non-metal

23
Q

Explain why ionic compounds conduct electricity when molten

A

Because the ions are free to move

24
Q

What does soluble mean?

A

Dissolves in water

25
Q

What does insoluble mean?

A

Does not dissolve in water

26
Q

Explain why chlorine and fluorine form covalent bonds

A

They are both non-metals

27
Q

Complete the sentence: In covalent bonds, electrons are _______________________

A

Shared

28
Q

In ionic bonds, electrons are ___________________

A

Transferred

29
Q

What is the name given to the structure of diamond, graphite and silicon dioxide?

A

Giant covalent

30
Q

How many bonds does each carbon have in diamond?

A

4

31
Q

Explain why diamond has a high melting point

A

Giant structure, Strong covalent bonds between the atoms, requires a lot of energy to break

32
Q

Explain why most giant covalent substances do not conduct electricity (3 marks)

A

There are no electrons/ions/charged particles that are free to move

33
Q

Explain why graphite conducts electricity

A

Has delocalised electrons between the layers that can move through the graphite

34
Q

Explain why graphite can act as a lubricant

A

Weak forces between layers which are free to slide over each other

35
Q

What is graphene?

A

One layer of graphite

36
Q

What type of substance are methane and water?

A

Simple molecular (or simple molecules)

37
Q

What is a molecule?

A

A group of atoms chemically bonded together

38
Q

Describe the structure of simple covalent molecules

A

Strong covalent bonds between atoms, weak forces holding the molecules together

39
Q

What are intermolecular forces?

A

Weak forces between molecules which hold them together

40
Q

Explain why methane has a low melting point

A

It is a simple molecular substance with weak forces between the molecules (which are easy to break)

41
Q

What is a polymer?

A

Millions of small molecules joined together in a chain to form a large molecule

42
Q

Describe the main features of metals in terms of their structure

A

Positive metal ions arranged in layers with delocalised electrons

43
Q

Explain why metals can conduct electricity

A

Delocalised electrons are free to carry charge

44
Q

Explain why pure metals are soft

A

Layers of metal ions are free to slide over each other

45
Q

What is an alloy?

A

A mixture of two or more elements, at least one of which is a metal

46
Q

Give a reason for alloying a metal

A

To make it harder, to make it less reactive

47
Q

Explain why alloys can be harder than pure metals

A

Different size of atoms disturb the layers to stop them sliding over each other

48
Q

What is the reactivity series?

A

A list of elements ordered by their reactivity

49
Q

What type of ion do metals from?

A

Positive Ion

50
Q

What type of ion do non-metals form?

A

Negative ion

Paper 1 GCSE Chemistry EC (7 decks)

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