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GCSE AQA Chemistry Important > C2 Bonding > Flashcards

C2 Bonding Flashcards

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1
Q

Which electrons are used in bonding?

A

Outer electrons

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2
Q

Group 1 metals react with what to form an ionic compound?

A

Non-metal

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3
Q

What group in the periodic table has the same electronic configuration as ions?

A

0 Noble Gases

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4
Q

Describe how a calcium ion is formed.

A

Loses 2 outer electrons

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5
Q

What is the charge on a potassium ion?

A

+1

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6
Q

How is a chloride ion formed?

A

Gains 1 outer shell electron

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7
Q

What do group 7 elements react with to form an ionic compound?

A

Metals

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8
Q

What is the charge on an oxide ion?

A

O2-

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9
Q

What is an ion?

A

A charged particle

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10
Q

What is an ionic compound?

A

Metal & Non-metal chemically bonded

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11
Q

What charge will group 1 elements form?

A

+1

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12
Q

What charge will the halogens form?

A

-1

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13
Q

What is ionic bonding?

A

Electrostatic attraction between ion formed by the transfer of electrons

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14
Q

Ionic compounds have what type of boiling and melting points? Why?

A

High, because they are lattice structure so ionic bonds would have to be broken

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15
Q

When melted or dissolved in water ionic compounds conduct electricity, why?

A

Ions are free to move

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16
Q

What is the formula of methane?

A

CH4

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17
Q

What are represented by ?

A

Shared pair of electrons – covalent bond

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18
Q

What type of bonding is found in methane?

A

Covalent

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19
Q

Why do simple molecules evaporate easily?

A

Weak intermolecular forces don’t need a lot of energy to break

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20
Q

What group of elements don’t often bond because they are unreactive?

A

0 – Noble Gases

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21
Q

What type of bonding is found in compounds with metals and non-metals?

A

Ionic

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22
Q

What type of bonding is found in C2H6?

A

Covalent

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23
Q

What type of bonding is found in potassium bromide?

A

Ionic

24
Q

What is the formula of potassium bromide?

A

KBr

25
Q

Explain in terms of electron transfer how potassium bromide is bonded?

A

1 outer electron is transferred from potassium to the bromine to form ions which attract

26
Q

Draw a hydrogen molecule.

A
27
Q

Draw a chlorine molecule

A
28
Q

Give a dot and cross diagram for water

A
29
Q

Draw an ammonia molecule

A
30
Q

Give a dot and cross diagram for methane

A
31
Q

Draw a hydrogen chloride molecule

A
32
Q

Give a dot and cross molecule for an oxygen molecule

A
33
Q

Is methane a simple molecular or giant covalent structure?

A

Simple Molecular

34
Q

Is diamond a simple molecular or giant covalent structure?

A

Giant Covalent

35
Q

In covalent compounds what happens to the electrons?

A

Shared

36
Q

What is a covalent bond?

A

A pair of shared electrons

37
Q

What is a double covalent bond?

A

2 pairs of shared electrons

38
Q

Why does methane have low melting and boiling points?

A

The low melting point is because it only has weak intermolecular forces that need to be broken

39
Q

Why do simple molecular substances not conduct electricity?

A

There are no free ions or electrons to move

40
Q

What type of bonding is in diamond?

A

Giant Covalent

41
Q

How many bonds does carbon make in a diamond?

A

4

42
Q

Why does diamond have a high melting point?

A

Each carbon atom has 4 strong bonds to other carbons in a giant structure so a lot of energy is needed to break them.

43
Q

Why is diamond hard?

A

Each carbon has 4 strong bonds in a giant structure

44
Q

In graphite how many bonds does carbon make?

A

3

45
Q

Why is graphite in pencils soft and slippery?

A

Layers are held together with weak forces so slide over each other

46
Q

Why does graphite conduct electricity in electrodes?

A

1 electron from each carbon is free to move

47
Q

Draw a labelled diagram for the bonding in metals

A
48
Q

What is the name of the bonding in metals?

A

Metallic

49
Q

Describe the bonding found in metals

A

Positive ions attracted to a sea of electrons

50
Q

Why do metals conduct electricity?

A

Delocalised outer electrons can move

51
Q

Why can metals be hammered and bent?

A

Layers slide over each other

52
Q

What are shape memory alloys?

A

Alloys that change shape at different temperatures

53
Q

What is the difference between a thermosoftening polymers and a thermosetting polymer?

A

Thermosoftening can be heated and reshaped but thermosetting would char

54
Q

What size are nanoparticles?

A

Very small 1-100nm

55
Q

Do nanoparticles have the same properties as the material in bulk?

A

No because of the large surface area for their volume

56
Q

Give 3 uses or nanoparticles.

A

Sun protection

Socks with silver or tennis balls

Catalysts

GCSE AQA Chemistry Important (18 decks)

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