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Eleanor Rowe Chemistry GCSE > Bonding, Structure and Properties of Matter > Flashcards

Bonding, Structure and Properties of Matter Flashcards

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1
Q

Why does an atom lose or gain electrons?

A

To get a full outer shell and be stable

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2
Q

What happens to a metal when it forms an ion?

A

They lose electrons to form positive ions

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3
Q

What happens to non metals when they form an ion

A

They gain electrons to form negative ions

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4
Q

If an atom lost 2 electrons to form an ion what would the charge be?

A

2+

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5
Q

If an atom gains 3 electrons when turning to an ion what would the charge be?

A

3-

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6
Q

What type of bonding occurs when a metal and non metal react together?

A

Ionic bonding

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7
Q

What is ionic bonding?

A

When non metals and metals react together
The metal atom loses electrons to form positively charged ion
The non metal atom gains these electrons to form negatively charged ion

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8
Q

What is the force called where oppositely charged ions are strongly attracted to each other?

A

Electrostatic forces

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9
Q

What charge will group 1 element ions have?

A

1+

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10
Q

What charge will group 2 element ions have?

A

2+

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11
Q

What charge will group 6 element ions have?

A

2-

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12
Q

What charge will group 7 element ions have?

A

1-

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13
Q

What diagrams show ionic bonding or ions?

A

Dot and cross diagrams

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14
Q

What must you always do when drawing an ion?

A

Use square brackets and state the charge

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15
Q

What is the structure of ionic compounds?

A

Giant ionic lattice

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16
Q

What are the properties of the ionic compound structure (giant regular lattice)?

A

Very strong electrostatic forces of attraction in all directions between oppositely charged ions

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17
Q

Properties of ionic compounds

A

High melting and high boiling points due to many strong bonds between ions.
When solid can’t conduct electricity as ions are held in place
When liquid will conduct electricity as ions are free to move
Dissolve easily in water- ions superstar and are free to move

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18
Q

What method do you use to write the empirical formula of an ionic compound?

A

Swap and drop

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19
Q

What is covalent bonding?

A

When two non metals react together and share electron pairs to make covalent bonds

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20
Q

How can you draw covalent bonds?

A

Dot and cross diagram
In shells
Line diagrams

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21
Q

What is a simple molecular substance?

A

A substance made up of molecules containing a few atoms joined together by covalent bonds.
Eg/ hydrogen ( needs two atoms of hydrogen in order to both have full outer shell through covalent bonds)

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22
Q

What are the properties of simple molecular substances?

A

Forces of attraction between molecules are very weak
Melting and boiling points are very low as molecules are easily parted from each other
Gases or liquids at room temperature
Don’t conduct electricity as there are no free electrons

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23
Q

What is a covalent bond?

A

A chemical bond made by the sharing of a pair of electrons between two atoms

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24
Q

In what states are most simple molecular substances at room temperature?

A

Gas or liquid

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25
Q

What forces are stronger in simple molecular substances? Covalent bonds or intermolecular forces?

A

Covalent bonds

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26
Q

What forces need to be overcome to boil a simple molecular compound?

A

Intermolecular forces

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27
Q

Why may hydrogen chloride have poor electrical conductivity?

A

It doesn’t contain any ions or delocalised electrons to carry a charge

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28
Q

Explain how the atoms are held together in a molecule of hydrogen chloride

A

A pair of electrons (one from hydrogen and one from chlorine) is shared between the two atoms.
The atoms the held together by the strong attraction between this shared pair of negatively charged electrons and the positively charged nuclei of the atoms.

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29
Q

Why may a substance have a higher boiling point than another substance?

A

They could be a larger molecule so the intermolecular forces are stronger between the bonds so it takes more energy to boil it, therefore the temperature is higher.

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30
Q

What is a polymer?

A

A long chain of repeating units

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31
Q

How do you draw a polymer?

A

Draw the shortest repeating section

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32
Q

How do you find the molecular formula of a polymer?

A

Write down the molecular formula in brackets and put an n outside of it

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33
Q

What state are polymers at room temperature?

A

Solid

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34
Q

What has larger intermolecular forces, polymer molecules or simple covalent molecules and what does this mean?

A

Polymer molecules have larger intermolecular forces as they are bigger so more energy is needed to break them.

35
Q

Are the intermolecular forces weaker in polymer molecules than ionic or giant molecular compounds?

A

Yes

They have lower boiling points

36
Q

What are the bonds like in giant covalent structures?

A

All the atoms are bonded to each other by strong covalent bonds

37
Q

What are the melting and boiling points of giant covalent structures?

A

Very high as lots of energy is needed to break the covalent bonds between the atoms

38
Q

Do giant covalent structures conduct electricity?

A

No, they don’t contain charged particles so don’t conduct electricity.

39
Q

What are examples of giant covalent structures?

A

Diamond
Graphite
Silicon dioxide

40
Q

What is an allotrope?

A

Different structural forms of the same element in the same physical state.

41
Q

What are the properties of diamond?

A

Really hard
Giant covalent structure
Very high melting point
Doesn’t conduct electricity as it has no free electrons or ions

42
Q

What are the allotropes of carbon?

A

Diamond
Graphite
Graphene
Fullerenes

43
Q

What is the structure of diamond?

A

Each carbon atom has four covalent bonds

Tetrahedral

44
Q

What are the properties of Graphite?

A

Soft
Slippery as no bonds between layers
High melting and boiling points
Conducts electricity as one delocalised electron

45
Q

What are the uses of diamond?

A

Drills and saw tops

46
Q

What are the uses of graphite?

A

Pencils

Lubricant

47
Q

What are the properties of graphene?

A 
Hard
Very strong 
High melting and boiling points 
Light 
Conducts electricity
48
Q

Uses of graphene

A

Electronics

Carbon fibres

49
Q

What is the structure of graphene

A 
One layer of graphite 
Sheet of carbon atoms 
Joined in hexagons 
2D compound 
One atom thick
50
Q

Structure of graphite

A

Sheets of hexagons

51
Q

Properties of Fullerenes

A

High melting and boiling points
Hard
Conducts electricity

52
Q

Structure of fullerenes

A

60 carbon atoms joined together to form a ball
Can also form nanotubes
Or a cage in form of ball
Hollow centre

53
Q

Uses of fullerenes

A

Anti cancer drug transportation

54
Q

What is a nanotube

A

A tiny carbon cylinder

55
Q

What are the properties of nanotubes?

A

Conduct heat and electricity

High tensile strength

56
Q

True/false: metals have layers

A

True

57
Q

Do metals consist of a giant structure?

A

Yes

58
Q

How does metallic bonding work?

A

Metal atoms lose outer electrons to form positive ions.
They are arranges in a lattice structure and the lost delocalised electrons move around between the metal ions.
The positive ions and negative electrons have electrostatic force of attraction which is strong in metals and holds the ions together.

59
Q

What structure of metal causes it to conduct electricity and heat?

A

Having delocalised electrons

60
Q

What structure causes metals to be malleable and ductile?

A

Layers of metal ions that can slip over each other

61
Q

What structure of metal will cause it to have high melting and boiling points, be strong and hard and solid?

A

A strong force of attraction between metal ions and delocalised electrons

62
Q

What is an alloy?

A

A mixture of metals or of metals and carbon

63
Q

True/false: alloys are harder than pure metals

A

True

64
Q

How are the repeating units in a polymer bonded together?

A

Covalent bonding

65
Q

Explain why most metals are malleable

A

The layers of atoms in metals are able to slide over each other

66
Q

What are the three states of matter

A

Solid
Liquid
Gas

67
Q

Properties of solids

A 
Strong forces of attraction between particles 
Close together in fixed positions 
Regular arrangement 
Defined shale and volume 
Particles vibrate and expand when heated
68
Q

Properties of liquids

A 
Weak force of attraction 
Randomly arranged but stick close together 
Definite volume but don’t keep shale 
Constantly moving particles 
Move faster when hot 
Expands when heated
69
Q

Properties of gas

A 
Very weak force of attraction 
Free to move far apart 
Travel in straight lines 
Don’t keep definite shape or volume 
Move constantly with random motion 
Either expand or increase pressure when heated
70
Q

When a solid is heated/cooled, its particles gain more energy

A

Heated

71
Q

What does aqueous mean

A

Dissolved in water

72
Q

If the temperature of a substance is below the melting point, what state is it?

A

Solid

73
Q

If the temperature of a substance is above the boiling point, what state will it be?

A

Gas

74
Q

If the temperature of the substance is between the melting and boiling points, what state will it be?

A

Liquid

75
Q

How do you work out the surface area to volume ratio?

A

Surface area/volume

76
Q

True/false as particles decrease in size, the size of their surface area increases in relation to their volume.

A

True

77
Q

Do nano particles have a high or low surface area to volume ratio?

A

High

78
Q

What are the uses of nanoparticles?

A 
Catalysts 
Electric circuits 
Deodorants 
Surgical masks 
Wound dressings 
Cosmetics
79
Q

Is it known to doctors if nanoparticles can get into your body through suncream and damage cells?

A

No

80
Q

Sulphate ionic formula

A

SO4

81
Q

Nitrate ionic formula

A

NO3

82
Q

Hydroxide ionic formula

A

OH

83
Q

Carbonate ionic formula

A

CO3

84
Q

Ammonia ionic formula

A

NH4

Eleanor Rowe Chemistry GCSE (9 decks)

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