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chemistry > eoy exams yr 9 > Flashcards

eoy exams yr 9 Flashcards

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
what is the relative mass of neutrons, protons, and electrons?
neutrons - 1 protons - 1 electrons - 1/2000
26
what is the relative charge of neutrons, protons, and electrons
neutron: 0 proton: +1 electron: -1
27
what is the definition of an isotope?
atoms with the same number of protons (therefore the same element) but a different number of neutrons
28
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)
[(35 x 75.8) + (37.24.2)] /100 = 3548.4/100 =35.5 (3sf)
29
how are element arranged in the periodic table?
ascending atomic number
30
what does the group the element is in tell you about the atomic structure of it?
number of electrons on the outer shell
31
what does the period the element is in tell you about the atomic structure of it?
the number of electron shells
32
why are noble gasses unreactive?
they are already stable, do not need to loose/gain any electrons
33
what is the definition of an ionic bond?
ionic bond is the strong electrostatic attraction between positive and negative ions
34
what is the definition of oxidation (in terms of electrons)?
loss of eletrons
35
what is the definition of reduction (in terms of electrons)?
gain of electrons
36
what structure do ionic compounds form?
giant ionic lattices
37
why do ionic compounds have high melting points?
the strong electrostatic attraction requires a lot of energy to break/overcome
38
why are ionic compounds not conductive as a solid, but are as molten/aqueous
solid - ions cant move aqueous/molten - ions are free to move and carry charges
39
definition of an element?
a substance of only 1 type of atom
40
definition of a compound?
two or more different elements chemically bonded
41
definition of a mixture?
two or more substances not chemically bonded
42
what are the characteristics of metals?
- good conductors - high melting point - malleable - can be made to be shiny
43
composition of air (+%'s)
nitrogen - 78% oxygen - 21% argon - 0.9% carbon dioxide - 0.035 or 0.04
44
what is the test for oxygen?
the glowing splint method - place a 'glowing' splint into the gas, if it relights, oxygen is present
45
what happens when carbon is combusted in oxygen
orange sparks - slightly acidic
46
what happens when iron is combusted in oxygen
orange flame
47
what happens when magnesium combusts with oxygen?
bright white light - white solid formed very slightly alkaline
48
what happens when sulphur is combusted with oxygen
blue flame
49
thermal decomposition of a metal carbonate
meta carbonate --> metal oxide + carbon dioxide
50
copper (III) carbonate --> ______ + ______
copper oxide + carbon dioxide
51
what is the chemical test for carbon dioxide?
limewater (clear --> cloudy)
52
what colours does methyl orange go in acids, alkaline, and neutral substances
acid - red neutral - yellow alkaline - yellow
53
what colours does phenolphthalein go in acids, neutral, and alkaline substances
acids - colourless neutral - colourless alkaline - pink
54
what colours does blue litmus go in acids, neutral, and alkaline substances
acids - red neutral - blue (stay the same) alkaline - blue (stay the same)
55
what colours does red litmus go in acids, neutral, and alkaline substances
acids - red (stays the same) neutral - red (stays the same) alkaline - blue (stay the same
56
what are the pH's for strong acids, weak aids, neutral, weak alkalis, strong alkalis
strong acid: 0-3 weak acid: 4-6 neutral: 7 weak alkaline: 8-10 strong alkaline: 11-14
57
what is the reaction between metals and acids
metal + acid --> salt + hydrogen
58
properties of ionic compounds
- 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
what is the test for hydrogen?
squeaky pop test - place a lit splint into the gas, if hydrogen is present it will make a pop
60
definition of an acid
proton donor (H+)
61
definition of a base
proton acceptor (h+)
62
definition of an alkali
OH- donors (bases that are soluble in water)
63
describe a test for making soluble salts (using insoluble base + acid)
- 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
acid + base --> ____ + ____
water + salt
65
what is the equation for metal carbonates reacting with acids
acid + metal carbonate ---> salt + water + carbon dioxide
66
what happens to the metal carbonate in acids
disappears
67
how do you know carbon dioxide is released in a metal carbonate + acid reaction?
it fizzes
68
what is precipitation?
an insoluble solid being produced in a solution
69
what do metals form
giant metallic lattice
70
definition of metallic bonding
strong electrostatic attraction between positive metal ions and delocalised eletrons
71
describe the reactivity of group 1 metals with water
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
how do the reactions of group 1 metals and air change?
as you go down the periods, the metal turns dull quicker (reacts faster)
73
why does the reactivity of group 1 metals increase as you go down the periods?
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
definition of redox reaction
a reaction where reduction and oxidation occurs
75
definition of reducing agent
gets oxidised - they give the electrons to the substance being reduced
76
what is an ore
a rock containing a metal
77
how do you extract mercury or silver
dont need to be extracted - maybe purified
78
how do you extract something less reactive than carbon?
displacement using carbon
79
how do you extract something more reactive than carbon?
electrolysis - breaking down a compound using eectricity
80
what are the uses of aluminium?
cables, planes, and pots and pans
81
what are the uses of copper?
electrical pipes, pots and pans, water pipes
82
what are the uses of high carbon steel
cutting tools, masonry nails
83
what are the uses of low carbon steel
nails, car bodies, ships
84
what are the uses of stainless steel
kitchen sinks, saucepans, knives and forks
85
what are alloys
mixture of a metal and one or more elements
86
what is rust
iron --> iron (III) oxide ---> hydrated iron (III) oxide
87
how do barrier methods prevent rust
stops oxygen and water from reaching the iron has to be replaced
88
how do sacrificial methods prevent rust
add a more reactive metal to the iron - that metal will react instead has to be replaced + expensive
89
galvanising method for preventing rust
zinc coating -> is a barrier and will react before iron

chemistry (6 decks)

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