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chemistry > eoy exams yr 9 > Flashcards

eoy exams yr 9 Flashcards

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1
Q

what is the definition of a solvent?

A

liquid that dissolves the solid

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2
Q

what is the definition of soluble?

A

can be dissolved (in the solvent)

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3
Q

what is the definition of saturated?

A

no more solid will dissolve

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4
Q

what is the definition of a solute?

A

the solid that will be dissolved in a solvent

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5
Q

what is the definition of a solution?

A

the mixture of a solvent and a solute

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6
Q

what is the definition of insoluble?

A

cannot be dissolved

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7
Q

what is the definition of suspension

A

solid spread out in a solution

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8
Q

what is solubility usually measured in?

A

g per 100g (of water/other solvent)

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9
Q

how would you separate dissolved salt and water?

A

through evaporation or crystalisation

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10
Q

how would you separate a mixture of inks?

A

chromatography

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11
Q

how would you separate ethanol and water?

A

distillation

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12
Q

how would you separate sand and water?

A

filtration

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13
Q

what is the chemical test for water?

A

anhydrous copper sulphate (white —> blue) hydrous copper sulphate

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14
Q

what is the physical test for pure water?

A

boiling/melting point

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15
Q

explain the energy and movement of:
- a solid
- a liquid
- a gas

A

solid: low energy + vibrating
liquid: medium energy + more movement than a solid, atoms can slide over each other
gas: high energy + can move freely

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16
Q

what is the name of the process of a solid –> liquid?

A

melting

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17
Q

what is the name of the process of a liquid –> gas

A

evaporation

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18
Q

what is the name of the process of a gas –> liquid

A

condensing

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19
Q

what is the name of the process of a liquid –> solid

A

freezing

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20
Q

what is the name of the process of a solid –> gas

A

sublimation

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21
Q

what is the name of the process of a gas –> solid

A

deposition/desublimation

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22
Q

if you put ammonia and hydrogen chloride in a tube, why does the ammonium chloride (white powder) form closer to the hydrogen chloride

A

the hydrogen chloride is heavier so it diffuses slower

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23
Q

what is the definition of an atom?

A

an atom is the smallest part of a chemical element that can exist

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24
Q

what is the definition of a molecule?

A

two or more atoms that are chemically bound together

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25
Q

what is the relative mass of neutrons, protons, and electrons?

A

neutrons - 1
protons - 1
electrons - 1/2000

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26
Q

what is the relative charge of neutrons, protons, and electrons

A

neutron: 0
proton: +1
electron: -1

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27
Q

what is the definition of an isotope?

A

atoms with the same number of protons (therefore the same element) but a different number of neutrons

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28
Q

how would you calculate the relative atomic mass if the atoms were:
Cl^35 - 75.8%
Cl^37 - 24.2%
(both have 17 atomic number)

A

[(35 x 75.8) + (37.24.2)] /100
= 3548.4/100
=35.5 (3sf)

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29
Q

how are element arranged in the periodic table?

A

ascending atomic number

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30
Q

what does the group the element is in tell you about the atomic structure of it?

A

number of electrons on the outer shell

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31
Q

what does the period the element is in tell you about the atomic structure of it?

A

the number of electron shells

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32
Q

why are noble gasses unreactive?

A

they are already stable, do not need to loose/gain any electrons

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33
Q

what is the definition of an ionic bond?

A

ionic bond is the strong electrostatic attraction between positive and negative ions

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34
Q

what is the definition of oxidation (in terms of electrons)?

A

loss of eletrons

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35
Q

what is the definition of reduction (in terms of electrons)?

A

gain of electrons

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36
Q

what structure do ionic compounds form?

A

giant ionic lattices

37
Q

why do ionic compounds have high melting points?

A

the strong electrostatic attraction requires a lot of energy to break/overcome

38
Q

why are ionic compounds not conductive as a solid, but are as molten/aqueous

A

solid - ions cant move
aqueous/molten - ions are free to move and carry charges

39
Q

definition of an element?

A

a substance of only 1 type of atom

40
Q

definition of a compound?

A

two or more different elements chemically bonded

41
Q

definition of a mixture?

A

two or more substances not chemically bonded

42
Q

what are the characteristics of metals?

A
  • good conductors
  • high melting point
  • malleable
  • can be made to be shiny
43
Q

composition of air (+%’s)

A

nitrogen - 78%
oxygen - 21%
argon - 0.9%
carbon dioxide - 0.035 or 0.04

44
Q

what is the test for oxygen?

A

the glowing splint method - place a ‘glowing’ splint into the gas, if it relights, oxygen is present

45
Q

what happens when carbon is combusted in oxygen

A

orange sparks - slightly acidic

46
Q

what happens when iron is combusted in oxygen

A

orange flame

47
Q

what happens when magnesium combusts with oxygen?

A

bright white light - white solid formed
very slightly alkaline

48
Q

what happens when sulphur is combusted with oxygen

A

blue flame

49
Q

thermal decomposition of a metal carbonate

A

meta carbonate –> metal oxide + carbon dioxide

50
Q

copper (III) carbonate –> ______ + ______

A

copper oxide + carbon dioxide

51
Q

what is the chemical test for carbon dioxide?

A

limewater (clear –> cloudy)

52
Q

what colours does methyl orange go in acids, alkaline, and neutral substances

A

acid - red
neutral - yellow
alkaline - yellow

53
Q

what colours does phenolphthalein go in acids, neutral, and alkaline substances

A

acids - colourless
neutral - colourless
alkaline - pink

54
Q

what colours does blue litmus go in acids, neutral, and alkaline substances

A

acids - red
neutral - blue (stay the same)
alkaline - blue (stay the same)

55
Q

what colours does red litmus go in acids, neutral, and alkaline substances

A

acids - red (stays the same)
neutral - red (stays the same)
alkaline - blue (stay the same

56
Q

what are the pH’s for strong acids, weak aids, neutral, weak alkalis, strong alkalis

A

strong acid: 0-3
weak acid: 4-6
neutral: 7
weak alkaline: 8-10
strong alkaline: 11-14

57
Q

what is the reaction between metals and acids

A

metal + acid –> salt + hydrogen

58
Q

properties of ionic compounds

A
  • high melting point
  • hard
  • not conductive as a solid; conductive as a liquid/aqueous/molten
  • brittle
  • usually soluble in water
  • usually not soluble in other solvents
59
Q

what is the test for hydrogen?

A

squeaky pop test - place a lit splint into the gas, if hydrogen is present it will make a pop

60
Q

definition of an acid

A

proton donor (H+)

61
Q

definition of a base

A

proton acceptor (h+)

62
Q

definition of an alkali

A

OH- donors (bases that are soluble in water)

63
Q

describe a test for making soluble salts (using insoluble base + acid)

A
  • heat the acid until bubbles start to appear
  • slowly add the base until no more disappears, all the acid has reacted
  • filter out the excess base
  • pour the filtrate into an evaporating basin
  • heat until crystals begin to form
  • leave to crystallise for a few days
  • pick out crystals
  • dry with filter paper
64
Q

acid + base –> ____ + ____

A

water + salt

65
Q

what is the equation for metal carbonates reacting with acids

A

acid + metal carbonate —> salt + water + carbon dioxide

66
Q

what happens to the metal carbonate in acids

A

disappears

67
Q

how do you know carbon dioxide is released in a metal carbonate + acid reaction?

A

it fizzes

68
Q

what is precipitation?

A

an insoluble solid being produced in a solution

69
Q

what do metals form

A

giant metallic lattice

70
Q

definition of metallic bonding

A

strong electrostatic attraction between positive metal ions and delocalised eletrons

71
Q

describe the reactivity of group 1 metals with water

A

lithium: fizzes, moves about, produces gas
sodium: turns into a sphere, releases heat, fizzes and moves more than lithium - more reactive than lithium
potassium: burns with a lilac flame, reacts quicker than sodium - more reactive with sodium
rubidium: explodes as soon as it touches the water - more reactive than potassium
caesium: breaks the tub of water due to the explosion - more reactive than rubidium

72
Q

how do the reactions of group 1 metals and air change?

A

as you go down the periods, the metal turns dull quicker (reacts faster)

73
Q

why does the reactivity of group 1 metals increase as you go down the periods?

A

the lower the period, the more electron shells it has, so the last electron is further away from the nucleus - so the attraction is weaker and the electron is more easily lost

74
Q

definition of redox reaction

A

a reaction where reduction and oxidation occurs

75
Q

definition of reducing agent

A

gets oxidised - they give the electrons to the substance being reduced

76
Q

what is an ore

A

a rock containing a metal

77
Q

how do you extract mercury or silver

A

dont need to be extracted - maybe purified

78
Q

how do you extract something less reactive than carbon?

A

displacement using carbon

79
Q

how do you extract something more reactive than carbon?

A

electrolysis - breaking down a compound using eectricity

80
Q

what are the uses of aluminium?

A

cables, planes, and pots and pans

81
Q

what are the uses of copper?

A

electrical pipes, pots and pans, water pipes

82
Q

what are the uses of high carbon steel

A

cutting tools, masonry nails

83
Q

what are the uses of low carbon steel

A

nails, car bodies, ships

84
Q

what are the uses of stainless steel

A

kitchen sinks, saucepans, knives and forks

85
Q

what are alloys

A

mixture of a metal and one or more elements

86
Q

what is rust

A

iron –> iron (III) oxide —> hydrated iron (III) oxide

87
Q

how do barrier methods prevent rust

A

stops oxygen and water from reaching the iron
has to be replaced

88
Q

how do sacrificial methods prevent rust

A

add a more reactive metal to the iron - that metal will react instead
has to be replaced + expensive

89
Q

galvanising method for preventing rust

A

zinc coating -> is a barrier and will react before iron

chemistry (4 decks)

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