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Chemistry > C2 > Flashcards

C2 Flashcards

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1
Q

3 states of matter

A

Solid, liquid, gas

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2
Q

Forces of attraction, shape/volume and movement of solid

A

Strong - holds particles together, definite shape and volume, vibrate about their spot.

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3
Q

Forces of attraction, shape/volume and movement of liquid

A

Weak - randomly arranged and free to move past each other, define volume but do not have a definite shape, contantly move with random motion.

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4
Q

Forces of attraction, shape/volume and movement of gas

A

Very weak - free to move and far apart, no definite shape or volume, constantly move with random motion.

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5
Q

3 limitations of the simple particle model

A

Assumes all particles are spheres, assumes all particles are solids, does not show forces between the particles.

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6
Q

What elements react in ionic bonding?

A

A metal and a non-metal

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7
Q

What happens in an ionic bonding reaction?

A

A number of electrons passes from an atom to another atom so that they both achieve a full outer energy level.

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8
Q

2 properties of ionic compounds (giant ionic lattices)

A

Very high melting and boiling point - strong electrostatic forces require a lot of energy to break, cannot conduct electricity when solid - ions cannot move because of the forces.

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9
Q

What elements react in covalent bonding?

A

Non-metals

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10
Q

Define covalent bond

A

Shared pair of electrons.

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11
Q

2 properties of small covalent molecules (simple molecular substances)

A

Low MP and BP (gases and liquids at room temp.) - weak intermolecular forces between molecules, do not conduct electricity - molecules do not have an overall electric charge.

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12
Q

1 property of giant covalent molecules

A

High MP and BP (solid at room temp.) - have millions of strong covalent bonds

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13
Q

Why does diamond have a high MP and BP?

A

Each carbon atom forms 4 strong covalent bonds, which have to be broken when diamonds are melted.

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14
Q

Why cannot diamond conduct electricity?

A

There are no free electrons to carry electrical charge.

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15
Q

What atoms are silicon dioxide made from and what property does it have?

A

Oxygen and silicon atoms, high MP and BP.

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16
Q

3 properties of graphite

A

High MP and BP, soft and slippery, conducter of both electricity and heat

17
Q

Why does graphite have a high MP and BP?

A

Each carbon atom forms 3 covalent bonds - forms hexagonal rings. It takes a great deal of energy to break these bonds.

18
Q

Why is graphite soft and slippery?

A

Hexagonal rings are in layers - no covalent bonds between the layers so they can slide.

19
Q

Why does graphite conduct electricity and heat?

A

Each carbon atom has a single electron that is not in a covalent bond - released from the atom (delocalised). These can conduct thermal energy and electricity.

20
Q

Define graphene

A

Single layer of graphite - one atom thick.

21
Q

2 properties of graphene

A

Excellent conducter of electricity - delocalised electrons like graphite, extremely strong.

22
Q

Define fullerenes

A

Molecules of carbon atoms with hollow shapes, have hexagonal rings (can also have rings of 5 or 7 carbon atoms).

23
Q

3 uses of fullerenes

A

Deliver a drug by caging other molecules, lubricants, catalysts.

24
Q

2 properties of carbon nanotubes

A

High tensile strength (able to stretch without breaking), excellent conducters of heat and electricity

25
Q

Use of carbon nanotubes

A

Reinforce materials without adding too much weight (e.g. tennis rackets).

26
Q

Define polymers

A

Made up by joining together thousands of small, identical molecules (monomers).

27
Q

1 property of polymers

A

Have a high MP and BP (solids at room temp.) - strong intermolecular forces of attraction.

28
Q

What elements react in metallic bonding?

A

Metals

29
Q

How are metals structured?

A

Consist of giant structure of atoms arranged in regular layers. Electrons in the outer energy level of each atom are delocalised. There is a strong electrostatic attraction (metallic bond) between the sea of delocalised negative electrons and the positive metal ions.

30
Q

Why can metals conduct electricity?

A

Delocalised electrons can move and are charged so can carry an electric current and thermal energy.

31
Q

Why do metals have a high MP and BP?

A

A great deal of energy is required to break the strong metallic bonds.

32
Q

Why can metals be bent and shaped (malleable)?

A

The layers of atoms are able to slide over each other.

33
Q

Define alloy

A

A mixture of metals

34
Q

Why are alloys harder than pure metals?

A

The different sized of atoms distorts the layers, making it more difficult for them to slide over each other.

Chemistry (5 decks)

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