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AQA Paper 1 Chemistry > Structure and Bonding > Flashcards

Structure and 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 charge will an ion of oxygen take?

A

2- (6 electrons in outer shell so needs to gain two)

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9
Q

What charge will an ion of Selenium take?

A

2- (group 6, so has 6 electrons in the outer shell and needs to gain two)

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10
Q

Explain in terms of electrons what occurs when lithium bonds with chlorine

A

One electron transferred from lithium to chlorine

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11
Q

Why do atoms transfer electrons in ionic bonding?

A

So that they can have full outer shells

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12
Q

Explain in terms of electrons what occurs when lithium bonds with fluorine

A

One electron transferred from lithium to fluorine

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13
Q

Explain in terms of electrons what occurs when magnesium bonds with oxygen

A

Two electrons transferred from magnesium to oxygen

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14
Q

Explain in terms of electrons what occurs when beryllium bonds with oxygen (3 marks)

A

Two electrons transferred from beryllium to oxygen

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15
Q

Explain in terms of electrons what occurs when magnesium bonds with chlorine

A

One electron transferred from magnesium to two different chlorine atoms

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16
Q

Explain in terms of electrons what occurs when sodium bonds with oxygen

A

Two electrons transferred to an oxygen atom from two different sodium atoms

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17
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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18
Q

Why don’t sulphur ions and oxygen ions form ionic bonds with each other?

A

Both have negative charges so would repel

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19
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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20
Q

Define giant ionic lattice

A

A huge 3D network of ions

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21
Q

State the melting points of ionic substances

A

High

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22
Q

Explain why ionic substances have high melting points.

A

Strong bonds between oppositely charged ions are hard to break

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23
Q

Will NaCl(s) conduct electricity?

A

No

24
Q

Will NaCl (aq) conduct electricity?

A

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

25
Q

Will NaCl (l) conduct electricity?

A

Yes

26
Q

What does molten mean?

A

Melted

27
Q

Explain why ionic compounds do not conduct electricity when solid

A

Because the ions are not free to move

28
Q

Explain why ionic compounds conduct electricity in solution

A

Because the ions are free to move

29
Q

Explain why ionic compounds conduct electricity when molten

A

Because the ions are free to move

30
Q

What does soluble mean?

A

Dissolves in water

31
Q

What does insoluble mean?

A

Does not dissolve in water

32
Q

Magnesium carbonate is insoluble. What do you need to do before it will conduct electricity?

A

Melt it

33
Q

Sodium fluoride is soluble. Explain what the easiest way for it to conduct electricity is

A

Dissolve it in water because this does not require high temperatures

34
Q

Explain why chlorine and fluorine form covalent bonds

A

They are both non-metals

35
Q

Complete the sentence: In covalent bonds, electrons are _______________________

A

Shared

36
Q

In ionic bonds, electrons are ___________________

A

Transferred

37
Q

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

A

Giant covalent

38
Q

How many bonds does each carbon have in diamond?

A

4

39
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

40
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

41
Q

Explain why graphite conducts electricity

A

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

42
Q

Explain why graphite can act as a lubricant

A

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

43
Q

What is graphene?

A

One layer of graphite

44
Q

What is a fullerene?

A

Substance made of carbon atoms arranged in a cage

45
Q

What type of substance are methane and water?

A

Simple molecular (or simple molecules)

46
Q

What is a molecule?

A

A group of atoms chemically bonded together

47
Q

Describe the structure of simple covalent molecules

A

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

48
Q

What are intermolecular forces?

A

Weak forces between molecules which hold them together

49
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)

50
Q

What is a polymer?

A

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

51
Q

Describe the main features of metals in terms of their structure

A

Positive metal ions arranged in layers with delocalised electrons

52
Q

Explain why metals can conduct electricity

A

Delocalised electrons are free to carry charge

53
Q

Explain why pure metals are soft

A

Layers of metal ions are free to slide over each other

54
Q

What is an alloy?

A

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

55
Q

Give a reason for alloying a metal

A

To make it harder, to make it less reactive

56
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

AQA Paper 1 Chemistry (7 decks)

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