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GCSE Chemistry > C2.3 - Properties Of Materials > Flashcards

C2.3 - Properties Of Materials Flashcards

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1
Q

why does carbon have 4 electrons in its outer shell

A

carbon has 4 electrons in its outer shell because carbon is in Group 4

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2
Q

what is carbon

A

carbon is the 6th element in the periodic table

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3
Q

what is the atomic mass of carbon

A

the atomic mass of carbon is 12

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4
Q

how many covalent bonds can carbon make with other atoms

A

carbon can make up to 4 covalent bonds with other atoms

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5
Q

what are organic compounds

A

organic compounds are naturally occuring synthetic carbon based compounds

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6
Q

can carbon bond with other carbons

A

yes - carbon can bond with other carbons

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7
Q

what are allotropes

A

allotropes are different forms of an element in the same state (e.g. a solid) but with different atomic arrangements

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8
Q

what are the 4 allotropes of carbon

A

diamond, graphit, graphine and fullerenes

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9
Q

how is graphite formed

A

graphite is formed when each carbon atom bonds with 3 other carbon atoms

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10
Q

why can graphite conduct electricity

A

graphite can conduct electricity because it has free electrons

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11
Q

how are the layers in graphite held together

A

the layers are held together by weak bonds, so they can break off easily

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12
Q

what is graphene

A

graphene is a single layer of graphite

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13
Q

why can graphene conduct electricity

A

graphene can conduct electricity because it has free electrons

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14
Q

what is graphene used in

A

graphene is used in electronics and solar panels

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15
Q

how is diamond formed

A

diamond is formed when each carbon atom bonds with 4 other carbon atoms

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16
Q

why can’t diamond conduct electricity

A

diamond can’t conduct electricity because all of its outermost electrons are involved in bonding

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17
Q

what are some properties of diamond

A

diamond cannot conduct electricity. diamonds are very hard. dimond is extremely strong

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18
Q

what are diamonds used in

A

diamonds are used in drill bits, and polished diamonds are used in jewellery

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19
Q

why is diamond very strong

A

diamond is extremely strong because each atom forms the full number of covalent bonds

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20
Q

what are fullerenes

A

fullerenes are tubes and spherical structures formed using only carbon atoms

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21
Q

what are fullerenes used as

A

fullerenes are used as superconductor, for reinforcing carbon fibre structures, and as containers for drugs being used introduced into the body

22
Q

what is diamond an example of

A

dimaond is an example of a gian covalent structure

23
Q

what is graphite an example of

A

giant covalent structure

24
Q

how many C-C bonds does diamond have

A

diamond has 4 C-C bonds

25
Q

how many C-C bonds does graphite have

A

graphite has 3 C-C bonds

26
Q

how many C-C bonds does Buckminster fullerene have

A

Buckminster fullerene has 3 C-C bonds

27
Q

what is an example of a metallic structure

A

steel

28
Q

what is an example of a giant covalent structure

A

carbon fibre

29
Q

what is an example of ionic compounds

A

sodium chloride

30
Q

what is an example of a simple covalent structure

A

iodine

31
Q

what is an example of polymers

A

wax

32
Q

is a metallic structure brittle or flexible

A

a metallic structure is flexible

33
Q

is a giant covalent structure brittle or flexible

A

a giant covalent structure is brittle (it shatters)

34
Q

are ionic compounds brittle or flexible

A

ionic compounds are brittle

35
Q

is a simple covalent structure brittle or flexible

A

a simple covalent structure is brittle

36
Q

are polymers brittle or flexible

A

polymer are flexible

37
Q

what is the arrangement of structures in a metallic structure

A

the particles are closely packed in layers but the layers can slide over each other

38
Q

what is the arrangement of structures in a giant covalent structure

A

the particles are closley packed in layers but the layers can’t slide over each other

39
Q

what is the arrangement of structures in ionic compounds

A

the particles are in a uniform lattice

40
Q

what is the arrangement of structures in simple covalent structures

A

the particles are in a lattice of simple molecules, held together by intermolecular forces

41
Q

what is the arrangement of structures in polymers

A

the particles aren’t in a lattice, but held together by intermolecular forces (which are relatively weak)

42
Q

what are bulk properties

A

bulk properties are how atons/molecules interact in big groups

43
Q

what are some examples of bulk properties

A

density, hardness, malleability, conductivity, melting/boiling points

44
Q

what is malleability

A

malleability is how easily you can change the shape

45
Q

what do atomic/molecular properties rely on

A

atomic/molecular properties rely on the atomic structure of the atoms

46
Q

what are some examples of atomic/molecular properties

A

electronic structure, atomic radius, bonding, intermolecular structure

47
Q

what are nanoparticles

A

nanoparticles are particles with a size between 1 and 100nm

48
Q

what are some properties of nanoparticles

A

nanoparticles are very small, and have a very large surface area to volume ratio

49
Q

what can nanoparticles be used for

A

nanoparticles can be used in suncream. nanoparticles can be used for catalysts, windows, ovens and clothes (self cleaning)

50
Q

why are nanoparticles used in suncream

A

extra small size of nanoparticles makes the cream colourless (instead of white). the nanopoarticles block UV (they don’t sctter visible light)

51
Q

why are nanoparticles used in catalysts, windows, ovens and clothes (self cleaning)

A

nanoparticles have a large surface area to volume ratio so more of the substance comes into contact with the surrounding material e.g. catalysts speed up reactions but they aren’t catalysts. a nanoparticle coating on glass will keep the glass clean

52
Q

what are some risks of nanoparticles

A

they are so small that they can be breathed in and absorbed into tissues. they can take a long time to be broken down once released into the environment. they are so new thst not all the risks have been identified. the risks are difficult to predict

GCSE Chemistry (12 decks)

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