Structure and Bonding [carbon] - Chemistry Paper 1 Flashcards

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1
Q

What are allotropes?

A

Different structural forms of the same element

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2
Q

How many bonds does diamond make?

A

4

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3
Q

Why can’t diamond conduct electricity?

A

because all 4 electrons are used in bonding

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4
Q

Why is diamond hard/can’t be stractched?

A

Because in order to scratch diamond the strong covalent bonds need to be overcome and this requires a lot of energy

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5
Q

Why does diamond have a high melting point?

A

Because it takes a lot of energy to overcome the strong covalent bonds

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6
Q

How many bonds does graphite make?

A

3

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7
Q

Why can graphite conduct electricity?

A

Because there’s one free electron that can move between graphite’ layers and carry a charge

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8
Q

Why is graphite soft and slippery?

A

Because it contains layers which are held together by weak intermolecular forces. This allows for the layers of graphite to move over each other

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9
Q

Why does graphite have a high melting point?

A

Because the covalent bonds in the layers need a lot of energy to break

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10
Q

What is graphene?

A

A sheet of carbon atoms joined together in hexagons/or, a single layer of graphite

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11
Q

How thick is graphene?

A

Just one atom thick, meaning graphene is 2D

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12
Q

What are the properties of graphene?

A

very strong, very light, conductor of heat and electricity

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13
Q

What are the potential uses of graphene?

A

Composite materials, electroncs

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14
Q

What are fullerenes?

A

Hollow molecules of carbon, shaped like tubes or balls

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15
Q

What are fullerenes made up of?

A

Carbon atoms arranged in hexagons , pentagons, or heptagons

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16
Q

What was the first fullerene to be discovered?

A

Buckminster fullerene

17
Q

What’s the molecular formula of buckminster fullerene?

A

C60

18
Q

What are nanotubes?

A

Fullerenes which are tiny carbon cylinders

19
Q

What are fullerenes used in?

A

Medicine, catalysts, lubricants, strengthening materials, in electronics