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Chemistry > AQA Combined Chemistry 5.2 > Flashcards

AQA Combined Chemistry 5.2 Flashcards

Revision for Paper 1

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1
Q

What is the chemical formula of Buckminsterfullerene?

A

C(60)

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2
Q

What element are all fullerenes made from?

A

Carbon

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3
Q

Describe the structure of fullerenes

A

Mostly hexagonal rings of carbon. Can be spherical or cylindrical in shape

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4
Q

Give three examples of giant covalent structures

A

Diamond, graphite, silicon dioxide

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5
Q

What do the following symbols represent?

a) s
b) l
c) g
d) aq

A

a) solid
b) liquid
c) gas
d) aqueous

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6
Q

Do metals have high or low melting points and boiling points?

A

High melting and boiling points

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7
Q

Diamond and graphite are made out of a single element. Name this element.

A

Carbon

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8
Q

Can molecules conduct electricit? Give a reason for your answer

A

No, because they have no overall electric charge

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9
Q

What type of bond exists between metals and non-metals in a compound?

A

Ionic Bond

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10
Q

What is the name for the forces that exist between ions in an ionic bond?

A

Electrostatic forces

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11
Q

What type of bonding exists in metallic elements and alloys?

A

Metallic bonding

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12
Q

In which type of bond are electrons shared?

A

Covalent bond

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13
Q

In which type of bond are electrons transferred?

A

Ionic bond

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14
Q

What type of bond exists in non-metal elements and compounds?

A

Covalent Bond

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15
Q

What is the name for the electrons that are free to flow in metallic bonding?

A

Delocalised electrons

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16
Q

When atoms gain or lose electrons to become ions, they will have the electron structure of what group of elements?

A

Noble gases

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17
Q

Describe how sodium and chloride bond to form sodium chloride

A

1) The sodium atom loses one electron to become a sodium ion
2) The chlorine atom gains one electron to become a chloride ion
3) The positive sodium ion is attracted to the negative chloride ion to form sodium chloride

18
Q

What charge do metal ions have?

A

Metal ions are positive

19
Q

What charge do non-metal ions have?

A

Non-metal ions are negative

20
Q

Small molecules contain what type of bonds?

A

Covalent bonds

21
Q

Describe the structure and bonding of an ionic compound

A

a) ionic bonding
b) giant structure of ions
c) lattice structure
d) oppositely charge ions held together by electrostatic forces acting in all directions

22
Q

Why do small molecules usually have relatively low melting and boiling points?

A

a) they have weak forces between molecules (intermolecular forces)
b) it is the intermolecular forces that are overcome, not the covalent bonds, when the substance boils.

23
Q

What is the relationship between the forces between particles and a substance’s melting and boiling points?

A

The stronger the forces between particles, the higher the melting and boiling points

24
Q

What charge do the ions of elements in the following groups have?:

a) Group 1
b) Group 2
c) Group 6
d) Group 7

A

a) +
b) 2+
c) 2-
d) -

25
Q

Describe the structure and bonding in a metal

A

a) metallic bonding
b) strong metallic bonds
c) giant structure of metal atoms in regular pattern
d) outer shell electrons are delocalised

26
Q

Why do molten or aqueous solutions of ionc compounds conduct electricity?

A

Ions are free to move so charge can flow

27
Q

What are the limitations of the following diagrams to represent ionic structures?

a) dot and cross
b) ball and stick

A

a) dot and cross - doesn’t show the structure of the ionic compound, the size or arrangement of ions
b) ball and stick - suggests gap between ions which aren’t in fact there

28
Q

Why do ionic compounds have high melting and boiling points?

A

Because a lot of energy is needed to break the many strong bonds

29
Q

What type of bonds exist in large molecules, such as plymers?

A

Covalent bonds

30
Q

Describe how the arrangement of atoms makes pure metals soft

A

a) atoms arranged in layers

b) layers slide easily over each other

31
Q

What are the limitations of using the particle models below to represent solids, liquids and gases?

A

a) no forces between the particles are shown in the diagram
b) all particles are represented by spheres
c) all the spheres are solid and inelastic

32
Q

What state are most polymers at room temperature? Why?

A

a) solid

b) because they are large molecules, with strong intermolecular forces, hence relatively high melting and boiling points

33
Q

What bonds must be overcome in order to melt or boil giant covalent structures?

A

The strong covalent bonds between the atoms

34
Q

Descrobe the structure and bonding of Diamond

A

a) giant covalent structure

b) each crbon forms four covalent bonds with other carbon atoms

35
Q

Describe the properties of Diamond

A

a) hard
b) very high melting point
c) doesn’t conduct electricity

36
Q

What happens to the size of intermolecular forces as the size of molecules increase?

A

The size of intermolecular forces increase (hence higher melting and boiling points for larger molecules)

37
Q

Why are metals good conductors of heat and electricity?

A

They have delocalised electrons that can carry the charge or transfer energy

38
Q

What are cylindrical fullerenes called and why are they useful?

A

a) nanotubes

b) they have a high length to diameter ratio making them useful for nanotechnology, electronics and materials

39
Q

Describe how the arrangement of atoms in an alloy makes alloys harder than pure metal

A

a) different sized atoms
b) layers disorted
c) atoms can’t easily slide over each other

40
Q

Describe the structure and bonding of Graphite

A

a) giant covalent structure
b) each carbon forms three covalent bonds with other carbon atoms
c) forms layers of hexagonal rings
d) no covalent bonds between layers
e) one electron from each carbon atom is delocalised

41
Q

What is graphene?

A

A single layer of graphite

42
Q

Name two uses of graphene

A

Used in electronics and composites

Chemistry (5 decks)

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