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Chemistry > Unit 5, 6 & 7 - Ionic Bonding/ Covalent Bonding/ Types Of Substance > Flashcards

Unit 5, 6 & 7 - Ionic Bonding/ Covalent Bonding/ Types Of Substance Flashcards

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1
Q

What are bonds?

A

Forces of attraction that hold atoms together.

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2
Q

What does more stable mean?

A

Less reactive

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3
Q

What is a noble gas atom?

A

An atom with a full outer shell.

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4
Q

What are ions?

A

Electrically charged particles formed when atoms lose or gain electrons.

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5
Q

What is a cation?

A

An ion that is formed from metals losing electrons and has a positive charge. (Losing electron)

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6
Q

What is an anion?

A

An ion that is formed from non-metals and has a negative charge. (Gaining electron)

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7
Q

What does the name change to when non-,metals form negative ions?

A

-ide

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8
Q

What are electrostatic forces?

A

The forces of attraction between all positively and negatively charged objects.

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9
Q

What is an ionic bond?

A

A bond between oppositely charged ions formed by the attraction between them.

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10
Q

What is an ionic bond formed from?

A

Metals and non-metals?

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11
Q

How is the group related to the number of electrons in the outer shell?

A

The group number is the same as the number of electrons in the outer shell.

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12
Q

What is a lattice structure?

A

The structure formed when billions of ions are closely packed together in a regular pattern.

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13
Q

What do ionic compounds form and why?

A

Crystals when solid because of their regular lattice structure.

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14
Q

Give 3 properties of crystals.

A

Particular regular shape
Flat surface
Sharp edges

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15
Q

Do ionic compounds have electrical charge?

A

No

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16
Q

What is a polyatomic ion?

A

A group of two or more atoms that have become charged.

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17
Q

What do all ionic compound contain?

A

Charged particles called ions

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18
Q

What are the ionic bonds?

A

The electrostatic force that holds the opposite charged ions

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19
Q

What do ionic compounds not contain?

A

Atoms or molecules

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20
Q

Are the electrostatic forces strong or weak?

A

Strong

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21
Q

What causes the substance to melt?

A

A lot of energy which separates the ions

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22
Q

If the forces holding ionic compounds is strong then…

A

They have high melting and boiling points.

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23
Q

Why would more energy be needed to separate ions?

A

If the charge is more than one

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24
Q

Do ionic compounds conduct electricity when solid?

A

No

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25
Q

Why do ionic compounds conduct electricity when they are molten or dissolved in water?

A

Because the charged particles are free to move

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26
Q

What is an aqueous solution?

A

When ionic compounds are dissolved in water to form the solution.

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27
Q

What are the anions attracted to?

A

The positive electrode called anode

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28
Q

What are the cations attracted to?

A

The negative electrodes called cathode

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29
Q

What enables ionic compounds to conduct electricity?

A

The ions being able to move, not the electrons

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30
Q

What bonds are in molecular substances?

A

String covalent bonds

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31
Q

What does the molecular formula show?

A

The number of atoms of each element bonded together in a simple molecule

32
Q

What are covalent bonds formed between?

A

Non-metals

33
Q

What happens in a covalent bond?

A

The atoms share electrons to make their outer shells full

34
Q

What is a double covalent bond?

A

When more than one electron is shared

35
Q

What is the valency of an element?

A

The number of covalent bonds formed to make full outer shells

36
Q

What influences the properties of a compound?

A

The atoms and the type of bonding

37
Q

What are the forces between the molecules called?

A

Intermolecular forces that are weak

38
Q

Why does water have low boiling and melting points?

A

Because it doesn’t take much energy to over come the force.

39
Q

What is an electric current

A

A flow of charged particles

40
Q

Why can the electrons not flow in simple molecules?

A

The force between the electrons and the protons holds them in place

41
Q

What are monomers?

A

Small, simple molecules

42
Q

What is a polymer?

A

Monomers that are joined together in a chain.

43
Q

Why do longer polymers have higher melting and boiling points?

A

They have more intermolecular forces and the long chain tends to get tangled up.

44
Q

What are compounds and elements both examples of?

A

Molecules

45
Q

What is an allotrope?

A

Different forms of the same element

46
Q

How is fullerene formed?

A

Each carbon atom is covalently bonded to three other carbon atoms

47
Q

What shape is fullerene?

A

Either spherical or tubular

48
Q

Why is fullerene soft and slippery?

A

Because the intermolecular forces are weak

49
Q

What is the formation of graphene?

A

A sheet of carbon atoms which are bonded to three other carbon atoms and can be rolled up.

50
Q

Why is graphene the lightest material?

A

It is only one atom thick

51
Q

Why is graphene a good electrical conductor?

A

It allows free electrons to move across the surface.

52
Q

Give two example of giant structures of carbon

A

Diamond and graphite

53
Q

What is different about giant structures?

A

They have huge three-dimensional networks of carbon.

54
Q

Why does graphite and diamond have high melting and boiling points?

A

Many strong covalent bonds need to be broken

55
Q

Why is there delocalised electrons in graphite

A

Because it has a layered structure so not all electrons are held in covalent bonds

56
Q

Is graphite an electrical conductor?

A

Yes

57
Q

Why is diamond no an electrical conductor?

A

All of the electrons are used in the covalent bonding

58
Q

Why is graphite a good lubricant and soft

A

The forces between the layers are weak so the layers can slide.

59
Q

Why is diamond an electrical insulator?

A

There are no free electrons to carry charge

60
Q

Why is diamond very hard and rigid?

A

The structure arrangement is very rigid and the covalent bonds between each atom is very strong.

61
Q

Give two general properties of metals

A

Any of: high melting points, shiny when polished, malleable, high density, good conductors of electricity

62
Q

Give two properties of non metals

A

Any of: low melting points, not usually shiny, brittle, low density, poor conductors of electricity

63
Q

How are atoms arranged in metallic bonding?

A

Same size, closely packed and in layers

64
Q

In metallic bonding, why is there a ‘sea’ of electrons?

A

The outer shell electrons are lost from the atoms and are free to move anywhere throughout the metal

65
Q

What is metallic bonding?

A

The electrostatic attraction between the positive ions and the negative delocalised electrons.

66
Q

Is the attraction in metallic bonding strong or weak?

A

Strong

67
Q

What does malleable mean?

A

They can be hammered into shape without shattering.

68
Q

Why are metals malleable?

A

The layers of ions slide over each other and the sea of electrons holds the ions together so it doesn’t break

69
Q

How do metals conduct electricity?

A

When a voltage is applied to either end of a metal, the electrons flow to one end causing an electrical current

70
Q

What makes the electrical conductivity increase?

A

When the amount of delocalised electrons increase.

71
Q

Are all electrons involved in the sea of electrons?

A

No, only from the outer shell

72
Q

Give a weakness of dot cross diagram

A

It suggests that the electrons are different (dots and crosses)

73
Q

Give a weakness of metallic model

A

Doesn’t show the ions will always be vibrating

74
Q

Give weakness of 3D ball and stick model

A

It’s not sticks holding the atoms together

75
Q

Give strength of dot cross diagram

A

Shows how electrons are shared

76
Q

Give strength of metallic model

A

Shows how metal ions are held in a lattice structure

77
Q

Give strength of 3D ball and stick model

A

Shows shape of structure

Chemistry (12 decks)

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