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GCSE - Chemistry > Chemistry Higher 3 GCSE > Flashcards

Chemistry Higher 3 GCSE Flashcards

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1
Q

arrangement of particles in solid, liquid, gas

A

regular, random, random

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2
Q

relative distance between particles in solid, liquid, gas

A

very close, close, far apart

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3
Q

main movement of particles in solid, liquid, gas

A

vibrate in fixed positions, move around each other and move quickly in all directions

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4
Q

at what state can you not compress a substance

A

solid or liquid
Because there is no space for the particles to move into. A substance in its solid shape has a fixed shape and cannot flow, because the particles vibrate around in fixed positions and cant move from place to place.

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5
Q

what is an atom

A

a small piece of matter

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6
Q

how big is an atom

A

Helium atoms are the smallest and they are 62pm (62 *10-12 (to the power of -12))

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7
Q

what are electrostatic forces

A

forces of attraction between positive and negative charges.

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8
Q

limitations of the particle model

A

doesn’t show:
forces between the particles
the size of particles
the space between particles

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9
Q

relative mass of an electron

A

0.0005

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10
Q

isotopes

A

different number of neutrons

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11
Q

ion

A

different number of electrons

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12
Q

Atomic model

A

DaTe RnBo

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13
Q

relative atomic mass/ formula mass

A

the mean mass of an atom/ formula compared to 1/12 the mass of a 12 6 Carbon atom

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14
Q

pure

A

consists of only 1 element

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15
Q

what is an alloy

A

a mixture of a metal and one or more element

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16
Q

how do you know what a substance is impure

A

the m.p is often less than that of a pure substance

it melts over a range of temperatures

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17
Q

how can you find the m.p

A

heat slowly

stir the substance as you melt it

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18
Q

How does crystallisation work

A

You have to heat a solution, until it becomes a saturated solution. Then allow to cool, and crystallisation should form

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19
Q

stationary phases in PC

A

absorbent paper

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20
Q

mobile phases in PC

A

solvent like water or propane

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21
Q

stationary phases in TLC

A

thin layer of silica or alumina powder spread over the glass plate

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22
Q

Thin layer chromatography method

A
  1. put solvent in the chromatography tank to a depth of 1cm. (make sure there are no naked flames if it is flammable)
  2. add a small amount of the sample to the baseline
  3. let the solvent travel through the powder and take out the plate before it reaches the top
  4. analyse the pattern
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23
Q

gas chromatography stationary phase

A

silica or alumina powder in metal column

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24
Q

gas chromatography mobile phase

A

unreactive carrier as like nitrogen

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25
Q

what is the solvent front

A

how far the water/ solvent has actually reached

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26
Q

explanation for gas chromatography

A

the sample is turned into a gas and injected into the column. The carrier gas pushes the sample through the column. The different components take different times to travel through the column, depending on how strongly they bond to the stationary phase.

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27
Q

advantages of TLC

A

quicker
more sensitive- so less sample
large range of stationary phases to choose from

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28
Q

what ions do metals form

A

they form positive ions as they lose electrons

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29
Q

what ions do non-metals form

A

they form negative ions as they gain electrons

30
Q

do metals react with each other

A

no, but non-metals can react with each other

31
Q

metal oxides produce what

A

alkaline solutions

32
Q

non-metal oxides produce what

A

acidic solutions

33
Q

structure and bonding in ionic compounds

A

ions are held together by ionic bonds, which act in all directions. ionic bonds are strong electrostatic forces between the oppositely charged ions

34
Q

structure and bonding in covalent compounds

A

involve electrostatic forces, but the forces are between the nucleus of each bonded atom and the shared electrons. The covalent bonds are strong, but the IMF are weak

35
Q

2 types of polymers

A

thermosoftening - tangled chains that are easy to seperate

thermosetting- chains joined with covalent bonds- called cross linking

36
Q

metallic bonds

A

electrons leave their outer shells of the metal atoms, forming a ‘sea of delocalised electrons’ around the positively charged ions. They have strong electrostatic forces of attraction between the delocalised electron and the ions

37
Q

Why can carbon form so many compounds

A

its atoms have 4 electrons, so it can form 4 covalent bonds

38
Q

What can carbon form

A

CHAINS AND RINGS

39
Q

What is an allotrope

A

different forms of the same element in different arrangements

40
Q

Diamond

A

exists as a giant covalent structure, in which each carbon atom is joined to 4 others. Can’t transfer electricity. High melting point and very hard

41
Q

Graphite

A

Giant covalent structure where each carbon atom is joined to 3 others. Has 1 delocalised electron that can carry the charge

42
Q

why is graphite slippery

A

even though the covalent bonds between in the graphite are strong. The forces between the layers is quite weak, so the layers can easily slide over each other

43
Q

Graphene

A

A layer of graphite
Transparent
Strong
Conducts electricity

44
Q

Fullerenes

A

Large family of carbon allotropes. Nanotube: a sheet of graphene rolled into a tube.
Buckyball: Graphene closed to make a hollow ball.

45
Q

what elements are in the solid state at r.t

A

metals
ionic compounds
giant covalent

46
Q

Brittle

A

Cracks under pressure

47
Q

Malleable

A

be bent

48
Q

how big are nanoparticles

A

1nm- 100 nm

49
Q

nanoparticles uses

A

paints

cosmetics

50
Q

what is a mole

A

a unit for amount of substance

51
Q

What is Avogadro’s constant

A

6.02 * 10 (-23) / mol

The number of entities in one mol

52
Q

acid + carbonate

A

salt + water + carbon dioxide

53
Q

acid + metal

A

salt + hydrogen

54
Q

dilute acid

A

contains a low ratio of acid to volume of solution

55
Q

concentrated acid

A

contains a higher ratio of acid to volume of solution

56
Q

weak acids

A

they partially ionise

57
Q

strong acids

A

they fully ionise

58
Q

explanation behind weak and strong acids

A

acids release Hydrogen ions in aqueous solutions. As the concentration of H+ ions increases by a factor of 10, by pH decreases by 1.

59
Q

electrolysis of water anode

A

4H+(aq) + 4e- -> 2H2 (g)

60
Q

electrolysis of water cathode

A

4OH-(aq) -> 2H20(l) + O2(g) + 4e-

61
Q

when is hydrogen produced

A

at the anode, unless there is an atom of a metal less reactive than hydrogen, then it will form

62
Q

when is oxygen produced

A

at the cathode, unless there is a group 7 element there (bromine, chlorine, iodine?)

63
Q

non-inert electrodes

A

will change

64
Q

inert electrodes

A

will not change

65
Q

in electroplating, what is the cathode

A

the object you want to coat

66
Q

in electroplating, what is the anode

A

the metal you want to coat with

67
Q

in electroplating, what is the electrolyte

A

has atoms of the metal you want to coat with

68
Q

how does electroplating work

A

atoms lose electrons at the anode and then they gain electrons at the cathode, so they move and stay on the cathode.

69
Q

how is copper purified

A

both electrodes are made from copper.
The anode is the impure one and the cathode is the pure one. Copper(2) sulfate solution is usually used as the electrolyte. The cathode will gain copper atoms, and the anode will lose the electrons.

70
Q

what type of particle is present in covalent bonding

A

a molecule

71
Q

why might a covalent compound have a low melting point

A

because it still had weak intermolecular forces

GCSE - Chemistry (33 decks)

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