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Chemistry > Unit 2 Structure and Bonding Core questions > Flashcards

Unit 2 Structure and Bonding Core questions Flashcards

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1
Q

When does ionic bonding occur?

A

When a metal and non-metal react

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2
Q

When does covalent bonding occur?

A

When non-metals react

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3
Q

When does metallic bonding occur?

A

When metals react

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4
Q

What is an ionic bond?

A

The electrostatic attraction between oppositely charged ions

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5
Q

What is a covalent bond?

A

The electrostatic attraction between the positive nuclei of atoms and the shared, negative electrons between them

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6
Q

What is a metallic bond?

A

The electrostatic attraction between positive metal ions and the delocalised electrons

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7
Q

What charge will an ion of lithium have?

A

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

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8
Q

What charge will an ion of beryllium have?

A

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

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9
Q

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

A

Negative

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10
Q

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

A

Positive (because they have lost a negative!)

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11
Q

What charge will an ion of oxygen have?

A

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

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12
Q

What charge will an ion of Selenium have?

A

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

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13
Q

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

A

One electron lost from lithium and it is gained by chlorine

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14
Q

Why do atoms transfer electrons in ionic bonding?

A

So that they can have full outer shells

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15
Q

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

A

One electron lost from lithium and it is gained by fluorine

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16
Q

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

A

Two electrons lost from magnesium and they are both gained by oxygen

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17
Q

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

A

Two electrons lost from beryllium and they are both gained by oxygen

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18
Q

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

A

Two electrons are lost from magnesium and two different chlorine atoms each gain 1 electron

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19
Q

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

A

two different sodium atoms lose one electron and an oxygen atom gains both

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20
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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21
Q

What is the name for the structure of a solid ionic compound?

A

Giant ionic lattice

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22
Q

Define giant ionic lattice

A

A huge 3D network of ions

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23
Q

State the melting points of ionic substances

A

High

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24
Q

State the melting points of ionic substances

A

High

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25
Q

Explain why ionic substances have high melting points

A

Strong ionic bonds between oppositely charged ions require lots of energy to break

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26
Q

Will a solid ionic compound conduct electricity and why?

A

No, because the ions are held firmly in place

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27
Q

Will a molten ionic compound conduct electricity?

A

Yes, as the ions are free to move so can carry a charge

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28
Q

What does molten mean?

A

Melted

29
Q

What does (aq) stand for?

A

Aqueous, which means dissolved in water

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

What happens in covalent bonding?

A

Atoms share a pair of electrons

36
Q

How many covalent bonds will a group 7 element make?

A

1 as they need one more electron for a full outer shell

37
Q

How many covalent bonds will a group 6 element make?

A

2 as they need two more electrons for a full outer shell

38
Q

How many covalent bonds will a group 5 element make?

A

3 as they need three more electrons for a full outer shell

39
Q

How many electrons does hydrogen have when it has a full outer shell?

A

2 as the first shell only holds 2 electrons

40
Q

How many covalent bonds does hydrogen make?

A

1 as it only needs one more electron for a full outer shell. It also only has 1 electron to share!

41
Q

In ionic bonds, electrons are ___________________

A

Transferred from a metal atom to a non-metal

42
Q

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

A

Giant covalent

43
Q

How many bonds does each carbon have in diamond?

A

4

44
Q

Explain why diamond has a high melting point

A

It has a giant covalent structure. The strong covalent bonds between the atoms require a lot of energy to break

45
Q

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

A

There are no mobile electrons/ions to carry a charge

46
Q

Explain why graphite conducts electricity

A

Carbon only makes 3 bonds, each carbon has a delocalised electron that can move through the graphite

47
Q

Explain why graphite can act as a lubricant

A

Layers of atoms can slide over each other

48
Q

What is graphene?

A

One layer of graphite

49
Q

What is a fullerene?

A

Substance made of carbon atoms arranged in a cage

50
Q

What type of substance are methane and water?

A

Simple molecular (or simple covalent molecules)

51
Q

What is a molecule?

A

A group of atoms chemically bonded together

52
Q

Describe the structure of simple covalent molecules

A

Strong covalent bonds between atoms, weak intermolecular forces between the molecules

53
Q

What are intermolecular forces?

A

Weak forces between molecules which hold them together

54
Q

Explain why molecular substances have a low melting point?

A

Weak intermolecular forces between the molecules which require little energy to break

55
Q

What is a polymer?

A

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

56
Q

Describe the structure of metals

A

Positive metal ions arranged in layers with delocalised electrons

57
Q

Explain why metals can conduct electricity

A

Have a delocalised electrons can carry a charge

58
Q

Explain why pure metals are soft

A

Layers of metal ions can slide over each other

59
Q

What is an alloy?

A

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

60
Q

Give a reason for alloying a metal

A

To make it harder

To make it less reactive

61
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

62
Q

Why do metals conduct heat?

A

Delocalised electrons can move and transfer energy

63
Q

What happens at the melting point?

A

A substance goes from solid to liquid or from liquid to solid

64
Q

What happens at the boiling point?

A

A substance goes from liquid to gas or from gas to liquid

65
Q

What is a nanoparticle?

A

A particle between 1 and 100 nm in size

66
Q

Why are nanoparticles useful?

A

They have a high surface area to volume ratio. This means they have unique properties and smaller quantities are needed to be effective

67
Q

What are some uses of nanoparticles?

A

They are used in medicine, electronics, cosmetics, sun creams, deodorants and as catalysts.

68
Q

What are some risks of nanoparticles?

A

They are still new so haven’t been studied in detail yet and they may cause harmful effects to the human body

Chemistry (5 decks)

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