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GCSE Chemistry > C3 - Structure And Bonding > Flashcards

C3 - Structure And Bonding Flashcards

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1
Q

What are some of the properties of solids?

A
  • The particels are very close together
  • They have a regular pattern
  • They vibrate around a fixed position
  • They have low energy
  • They cannot be compressed
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2
Q

What are some of the properties of liquids?

A
  • The particels are close together
  • The particels are randomly arranged
  • The particles can move around each other
  • They have some energy
  • They cannot be compressed
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3
Q

What are some of the properties of gases?

A
  • The particles are far apart
  • The particles are randomly arranged
  • the particles move quicklyy in all directions
  • They have the highest energy
  • They can be compressed
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4
Q

What is the change that occurs when a sold turns directly into a gas?

A

Sublimation

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5
Q

What is the energy, transferred by heating, used for when substances change state?

A

It is used to brak the bonds between particles and/or to overcome forces of attraction.

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6
Q

What determines the melting and boiling point of a substance?

A

The strength of the bonds or forces of attration.

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7
Q

What happens to the forces of attraction when a substance freezes?

A

They get stronger because energy is transferred from the substance to the surroundings.

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8
Q

When do ions form?

A

When a metal and non-metal react with one another as the opposite charged ions are strongly attracted to one another.

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9
Q

What happens to metals electrons when they form ions

A

They lose electrons (forming a positive charge)

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10
Q

What happens to non-metals electrons when they form ions?

A

They gain electrons (forming a negative charge)

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11
Q

When is an ionic compound formed?

A

When a negative ion joins with a posive ion.

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12
Q

What is the structure of ionic compounds?

A

A giant ionic lattice

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13
Q

What is the giant ionic lattice structure held together by?

A

Very strong electrostatic forces of attraction.

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14
Q

Because ionic compounds have strong forces of attraction what does this mean?

A

They have high melting and boiling points (so are sloid at room temp)

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15
Q

When can ionic conpounds conduct electricity?

A

When they are in liquid form or dissolved in water.

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16
Q

When is a covalent bond formed?

A

When two atoms share a pair of electrons.

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17
Q

What does covalent bonds usually occur between?

A

Non-metals

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18
Q

What is a molecule?

A

A collection of two or more atoms held together by chemical bonds.

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19
Q

What are the molecules held together by?

A

Strong covalent bonds

20
Q

What holds together the molecules with their neighbouring molecules?

A

Weak intermolecular forces

21
Q

Because of the weak intermolecular forces, what do subsatnces with small molecules have?

A

Low melting and boiling points

22
Q

Can small molecules conduct electricity?

A

No

23
Q

What happens when a small molecule melts or boils?

A

Its weak intermolecular forces are overcome, not its strong covalent bonds.

24
Q

How may electrons are shared in a double bond?

A

4 (2 pairs)

25
Q

What are allotropes?

A

Different structural forms of the same element

26
Q

What structure does diamond have?

A

Giant covalent structure made up of carbon atoms that form 4 covalent bonds, making it very hard/strong.

27
Q

Because of the strong covalent bonds diamond has a…

A

High melting a boiling point

28
Q

Why does diamond not conduct electricity?

A

Because it doesnt have any free electrons

29
Q

What structure does graphite have?

A

It is arranged in hexagonal layers as each carbon atom only forms 3 covalent bonds. As there are no covalent bonds between the layers this makes the layers free to slide over eachother.

30
Q

Does graphite have a high melting point?

A

Yes, to overcome the covalent bonds

31
Q

Can graphite conduct electicity?

A

Yes because only 3 out of the 4 of carbons outer electrons are being used. Meaning there are delocalised electrons between the layers.

32
Q

What is graphene?

A

It is one layer of graphite. It is a sheet of carbon atoms joined together in hexagons. The sheet is one atom thick

33
Q

What are the properties of graphene?

A

It is strong (due to the covalent bonds) and it is light

34
Q

Can graphene conduct electricity?

A

Like graphite it contains delocalised electrons so it can conduct electricity.

35
Q

What are fullerenes?

A

Molecules of carbon shaped like tubes or balls.

36
Q

What are the carbon atom arrainged in in fullerenes?

A

They are arrainged in hexagons, pentagons or heptagons

37
Q

What are the uses of fullerenes?

A
  • they can help make catalysts (because of their great surface area calatlyst molecules can be attached to the fullerenes)
  • they also make great lubricants
  • They can be used to cage other molecules (e.g. to deliver drugs into the body)
38
Q

What are some examples of fullerenes?

A

Buckminster fullerene and nanotubes

39
Q

What are nanotubes?

A

Tiny carbon cylindes that have a high length to diameter ratio (they are long and thin).

40
Q

What are some of the properties of nanotubes?

A
  • They can conduct heat and electricity (because they have delocalised electrons)
  • they have a high tensile strength so can resist being stretched
41
Q

What are nanotubes used in?

A
  • electronics

- to strengthan materials without adding weight (e.g. a tennis racket)

42
Q

Why is metallic bonding so strong?

A

Because of the strong electrostatic attraction between the ions

43
Q

Can metallic bonding conduct electricity?

A

Yes because they contain delocalised elecrons that are free to move between the layers.

44
Q

What are the properties of metals?

A
  • They are solid at room temp, meaning tthey have a high melting and boiling point
  • they can conduct electricity and heat due to the delocalised electrons
  • their layers can side over one another making metals malleable
45
Q

What is the difference between metals and alloys?

A

Alloys are harder and more useful than pure metals. Alloys are harder due to the different sized atoms present in the metal, this means that the layers cant slide over one another.

GCSE Chemistry (3 decks)

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