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GCSE CHEMISTRY > Structure and Bonding > Flashcards

Structure and Bonding Flashcards

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1
Q

What are the three types of chemical bonds?

A

Ionic, covalent and metallic bonds.

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2
Q

What is an ionic bond?

A

A bond between a metal and non-metal in which electrons have been exchanged.

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3
Q

What is a covalent bond?

A

A bond between two non-metals in which electrons are shared.

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4
Q

What is a metallic bond?

A

A bond between metal atoms in which electrons are delocalised.

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5
Q

How does an ionic compound form?

A

The metal loses electrons to get a full outer shell becoming a positively charged ion while the non-metal gains electrons becoming a negatively charged ion. The oppositely charged ions are electrostatically attracted to each other.

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6
Q

What is the charge of an ion from group 1?

A

1

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7
Q

What is the charge of an ion from group 2?

A

2

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8
Q

What is the charge of an ion from group 6?

A

-2

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9
Q

What is the charge of an ion from group 7?

A

-1

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10
Q

.What is an ionic compound?

A

.A giant structure of ions which are held together by strong electrostatic forces of attraction between oppositely charged ions.

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11
Q

.What are simple molecules?

A

.Small molecules such as oxygen and water that contain atoms joined together by covalent bonds.

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12
Q

.What is the state symbol for a solid?

A

.(s)

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13
Q

.What is the state symbol for a liquid?

A

.(l)

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14
Q

.What is the state symbol for a gas?

A

.(g)

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15
Q

.What is the state symbol for a solution?

A

.(aq)

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16
Q

.What are the properties of ionic compounds?

A

.High melting and boiling point. Don?t conduct electricity when solid but do when molten or dissolved.

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17
Q

.Why do ionic compounds have high melting and boiling points?

A

.Strong bonds between molecules which takes lots of energy to overcome.

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18
Q

.Why can?t ionic compounds conduct electricity when solid?

A

.Ions are unable to move freely.

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19
Q

.Why can ionic compounds conduct electricity when molten or dissolved?

A

.Ions are free and so are able to move.

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20
Q

.What are the properties of simple molecules?

A

.Low melting and boiling point. Poor conductors.

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21
Q

.Why do simple molecules have low melting and boiling points?

A

They have have intermolecular forces which are require less energy to overcome than bonds?

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22
Q

Explain why chlorine and fluorine form covalent bonds

A

They are both non-metals

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23
Q

Complete the sentence: In covalent bonds, electrons are _______________________

A

Shared

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24
Q

In ionic bonds, electrons are ___________________

A

Transferred

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25
Q

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

A

Giant covalent

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26
Q

How many bonds does each carbon have in diamond?

A

4

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27
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

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28
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

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29
Q

Explain why graphite conducts electricity

A

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

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30
Q

Explain why graphite can act as a lubricant

A

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

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31
Q

What is graphene?

A

One layer of graphite

32
Q

What is a fullerene?

A

Substance made of carbon atoms arranged in a cage

33
Q

What type of substance are methane and water?

A

Simple molecular (or simple molecules)

34
Q

What is a molecule?

A

A group of atoms chemically bonded together

35
Q

Describe the structure of simple covalent molecules

A

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

36
Q

What are intermolecular forces?

A

Weak forces between molecules which hold them together

37
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)

38
Q

What is a polymer?

A

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

39
Q

Describe the main features of metals in terms of their structure

A

Positive metal ions arranged in layers with delocalised electrons

40
Q

Explain why metals can conduct electricity

A

Delocalised electrons are free to carry charge

41
Q

Explain why pure metals are soft

A

Layers of metal ions are free to slide over each other

42
Q

What is an alloy?

A

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

43
Q

Give a reason for alloying a metal

A

To make it harder, to make it less reactive

44
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

45
Q

What charge do electrons have?

A

-1

46
Q

What charge will an ion of lithium take?

A

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

47
Q

What charge will an ion of beryllium take?

A

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

48
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)

49
Q

What charge will an ion of fluorine take?

A

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

50
Q

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

A

Negative

51
Q

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

A

Positive (because they have lost a negative!)

52
Q

What charge will an ion of oxygen take?

A

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

53
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)

54
Q

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

A

One electron transferred from lithium to chlorine

55
Q

Why do atoms transfer electrons in ionic bonding?

A

So that they can have full outer shells

56
Q

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

A

One electron transferred from lithium to fluorine

57
Q

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

A

Two electrons transferred from magnesium to oxygen

58
Q

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

A

Two electrons transferred from beryllium to oxygen

59
Q

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

A

One electron transferred from magnesium to two different chlorine atoms

60
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

61
Q

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

A

There is an electrostatic force of attraction between oppositely charged ions

62
Q

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

A

Both have negative charges so would repel

63
Q

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

A

Giant ionic lattice

64
Q

Define giant ionic lattice

A

A huge 3D network of ions

65
Q

State the melting points of ionic substances

A

High

66
Q

Explain why ionic substances have high melting points.

A

Strong bonds between oppositely charged ions are hard to break

67
Q

Will NaCl(s) conduct electricity?

A

No

68
Q

Will NaCl (aq) conduct electricity?

A

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

69
Q

Will NaCl (l) conduct electricity?

A

Yes

70
Q

What does molten mean?

A

Melted

71
Q

Explain why ionic compounds do not conduct electricity when solid

A

Because the ions are not free to move

72
Q

Explain why ionic compounds conduct electricity in solution

A

Because the ions are free to move

73
Q

Explain why ionic compounds conduct electricity when molten

A

Because the ions are free to move

74
Q

What does soluble mean?

A

Dissolves in water

75
Q

What does insoluble mean?

A

Does not dissolve in water

76
Q

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

A

Melt it

77
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

GCSE CHEMISTRY (4 decks)

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