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GCSE Chemistry > C3 > Flashcards

C3 Flashcards

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1
Q

What is graphene?

A

A single layer of graphite and has properties that make it useful in electronics and conmposites a

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2
Q

What are the properties of graphene?

A
  • excellent conductor of electricity and thermal energy
  • very low density
  • most reactive form of carbon
  • pieces of it are incredible strong for its mass
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3
Q

What are fullerenes?

A

Molecules made of carbon atoms with hllow shapes . The structure of fullerenes is based on hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms.

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4
Q

What was the first fullerene to be discovered?

A

Buckminsisterfullerene c60 which had a speherical shape

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5
Q

What are carbon nanotubes?

A

Cylindrical fullerenes with very high length to dimater ratios. Their properties make them useful for nanotechnology, electronics and materials.

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6
Q

What are the molecular forces like between buckministerfullerene?

A

Weak intermolecular forces between molecules

-slippery and low melting point

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7
Q

What are the states of matter?

A
  • solids
  • liquid
  • gases
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8
Q

What is the difference between the volume and shape of the three states of matter?

A
  • solids have fixed shape and volume
  • liquids have a fixed volume but can change their shape
  • gases have no fixed shape or volume , they can be compressed easily
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9
Q

What does particle theory describe?

A
  • movment of particles

- average distance between particles

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10
Q

How close are the state of matters particles together?

A
  • solids particles touch
  • liquids particles touch but move around aswell
  • gas particles do not touch
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11
Q

What is needed for a solid to become a base?

A

Heat which will break bonds between atoms and increase the energy making particles move around faster and increase collisions between particles making them move around rapidly

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12
Q

What takes place at the maelting point?

A

Melting and freezing

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13
Q

What takes place at the boiling point?

A

Boiling and condensing

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14
Q

What is the reason for a substance having a high boiling or melting point?

A

Strong forces between particles.

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15
Q

What are the three types of bonding?

A

Ionic , covalent and metallic

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16
Q

What compounds does ionic bonding occur in?

A

Metal and non metal

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17
Q

What compound does covalent bonding occur in?

A

Non metal and non metal

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18
Q

What does metallic bonding occur in?

A

Metallic elements and alloys

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19
Q

How do atoms gain a stable valence shell?

A
  • ionic bonding

- covalent bonding

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20
Q

What happens during ionic bonding?

A

Metal atom loses electron to become positively charge ion or a non metal gains an electron to become a negatively charged ipn

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21
Q

What is an ionic compound?

A

A giant structure of ions

22
Q

What holds ionic compounds toegther?

A

Strong electrostatic forces between oppositkey charged ions. These forces act in all directions in a lattice structure, this is ionic bonding.

23
Q

What is covalent bonding?

A

When atoms shair pairs of electrons , froming bonds that are strong

24
Q

What may covalently bonded substances consist off?

A

Small molcules

25
Q

What covalently bonded substances have very large molecules?

A

Polymers

26
Q

What are examples of giant covalent structures?

A

Diamond

Silicon dixoide

27
Q

What is metallic bonding?

A

Two metals reacting , forming bonds

28
Q

What do metals atoms consist off?

A

A giant structure of atoms in a regular repeating pattern

29
Q

What is the electrons configuration for metallic bonding?

A

Electrons in the outer shell are delocalised and so are free to move through the structure.

30
Q

What are the properties of ionic compounds?

A
  • high melting points

- high boiling points, because large amount of energy needed to break bonds

31
Q

How do you make ionic compounds conduct electricity ?

A

Melt it or dissolve it in water. This frees up the so ions charge can flow .

32
Q

What state are small Covalent molecules usually found in?

A

Gases or liquids

33
Q

What are the melting points of small covalent molecules?

A

Low melting and boiling points

34
Q

How strong are small Covalent molecules intermolecular forces?

A
  • weak intermolecular forces

- overcome when melted or boiled

35
Q

What happens as molecules get bigger?

A

Intermolecular forces increase so larger molecules have high melting and boiling points

36
Q

Do small Covalent molecules conduct electricity ?

A

No because they have no overall electric charge

37
Q

Properties of polymers?

A
  • very large molecules
  • atoms in polymer molecules are linked to other atoms by strong covalent bonds
  • intermolecular forces are strong
  • solids at room temperature
38
Q

What are giant covalent structures?

A

Substances that are solids with very high melting points, covalently bonded.

39
Q

What is bonding like in giant covalent structures?

A

All atoms linked by strong covalent bonds

40
Q

How to melt or boil a giant covalent strcutre?

A

Overcome the strong covlent bonds .

41
Q

Properties of metals and alloys?

A

Metals have a giant structure of atoms with strong metallic bonding. Means most metals have high melting and boiling points

42
Q

What is the structure and properties of a pure metal?

A
  • atoms are arranged in layers
  • can be bent and shaped
  • soft
43
Q

What are alloys?

A

Metals mixed together . They are harder than just a pure metal

44
Q

Are metals good conductors of electricity?

A

Yes, because delocalised electrons carry electrical charge through the metal. Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons.

45
Q

What are the properties of diamond?

A
  • formed from carbon
  • each carbon atoms forms four covalent bonds with other carbon atoms in a giant covalent structure
  • diamond is very hard
  • has a very high melting point
  • does not conduct electricity
46
Q

Properties of graphite?

A
  • made of carbon
  • each carbon atom forms three covalent bonds with three other atoms, forming layers of hexagonal rings which have no covalent bonds between layers
47
Q

Are graphite electrons delocalised?

A

Graphite has 1 delocalised electrons

48
Q

Why can metals be bent and shaped?

A

Metal ions can slide over each other

49
Q

How are metals structured?

A

-strong electrostatic attraction between sea of delocalised negative electrons and positive metal ions

50
Q

Why can delocalised electrons carry a current?

A

Because they are charged

51
Q

Why are alloys harder?

A

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

GCSE Chemistry (14 decks)

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