november mocks Flashcards
1
Q
how are solids arranged?
A
close together and tightly packed in regular rows
2
Q
how do solids move?
A
vibrate about a fixed point
3
Q
how much energy do solids have?
A
little energy
4
Q
what kind of oxides to metals have?
A
basic oxides, which reacts with acids to give a salt and water
5
Q
what kind of oxides to non-metals have?
A
acidic or neutral
6
Q
what happens when oxygen combusts in magnesium?
A
a bright white light given off, white powder produced
7
Q
what happens when hydrogen combusts?
A
theres an explosive reaction (think squeaky pop)
8
Q
what happens when sulphur combusts?
A
blue flame
9
Q
what does solvent mean?
A
the liquid in which the solute dissolves in
10
Q
what does solute mean?
A
the substance that is dissolved
11
Q
what does solution mean?
A
the liquid formed between the solute and the solution
12
Q
what does saturated solution mean?
A
no more solute can dissolve in the solvent
13
Q
what is the relative mass of an electron?
A
1/2000
14
Q
what is the charge on Ag (silver)?
A
+1
15
Q
what is the charge of Cu (copper)?
A
+2
16
Q
what is the charge on Fe (iron (II))?
A
+2
17
Q
what is the charge on Fe (iron (III))
A
+3
18
Q
what is the charge on Pb (lead)?
A
+2
19
Q
what is the charge on Zn (zinc)?
A
+2
20
Q
what is the charge of OH (hydroxide)?
A
-1
21
Q
what is the charge of ammonium?
A
+1
22
Q
what is the charge of carbonate?
A
-2
23
Q
what is the charge of nitrate?
A
-1
24
Q
what is the charge of sulphate?
A
-2
25
what is the formula of hydroxide (including charge)?
OH-
26
what is the formula of ammonium (including charge)?
NH4+
27
what is the formula of carbonate (including charge)?
CO3-2
28
what is the formula of nitrate (including charge)?
NO3-
29
what is the formula for sulphur (inluding charge)?
SO4-2
30
what is ionic bonding?
the strong electrostatic attraction between oppositely charged ions
31
why do ionic compounds have high melting points and boiling points?
the strong electrostatic attraction requires a lot of energy to overcome
32
when can ionic compounds conduct electricity?
when molten or aqueous
33
why can ionic compounds only conduct electricity when molten or aqueous?
the ions are free to move
34
what is the percentage of nitrogen in the air?
78%
35
what is the percentage of oxygen in the air?
21%
36
what is the percentage of argon in the air?
0.9%
37
what percentage of carbon is in the air?
0.035%
38
what pH value means strongly acidic?
0-3
39
what pH value is weakly acidic?
4-6
40
what pH value is neutral?
7
41
what pH value is weak alkaline?
8-10
42
what pH value is strongly alkaline?
11-14
43
what are acids in an aqueous solution sources of?
hydrogen ions
44
what are alkalis in an aqueous solution a source of?
hydroxide ions
45
what are alkalis?
soluble bases
proton receivers
46
what are bases?
proton receivers
47
what are acids?
proton donors
48
can alkalis can neutralise acids?
yes
49
is sodium (Na+) soluble?
yes
50
is potassium (K+) soluble?
yes
51
is ammonium soluble?
yes
52
are nitrates soluble, and are there any exceptions?
yes, there are no exceptions
53
are chlorides soluble, and are there any exceptions?
they are soluble except for silver chloride and lead (II) chloride
54
is silver chloride soluble?
no
55
is lead (II) chloride soluble?
no
56
are sulphates soluble and are there any exceptions?
yes they are, except for barium sulphate, calcium sulphate, and lead (II) sulphate
57
are carbonates soluble and are there any exceptions?
no they aren't, except for sodium carbonate, potassium carbonate, and ammonium carbonate
58
are hydroxides soluble?
no, except for sodium hydroxide, potassium hydroxide, and calcium hydroxide (though it is slightly soluble)
59
what is the reaction between an alkali and an acid?
alkali + acid -> water + salt
60
what is the reaction between bases ad acids?
base + acid -> water + salt
61
what is the reaction between a carbonate, acid?
carbonate + acid -> water + salt + carbon dioxide
62
what is the reaction between a metal and an acid?
metal + acid -> salt + hydrogen
63
how do you get an insoluble salt from two soluble reactants?
precipitate method:
mix them
filter
64
what is metallic bonding?
the strong electrostatic attraction between positive metal ions and a sea of delocalised negative electrons
65
what are the uses of aluminium?
- it is used for cables, some cars (because it's light), planes, pots, and pans
- it is useful because of it's lack of corrosion, it's low density, it's strength when alloyed, and it is a good conductor of heat and electricity
- it doesn't corrode because it forms aluminium oxide on the surface
66
what are the uses of copper?
- it is used in electrical wires, pots and pans, surfaces in hospitals, and water pipes
- it is a good conductor of heat and electricity, it is unreactive, malleable, and has anti-microbial properties
67
what is mild steel made out of?
iron and up to 0.25% carbon
68
what are the uses of mild steel?
- nails, car bodies, ships, and bridges
- mild carbon is strong, hard, malleable, and ductile
- it rusts when exposed to oxygen and water
69
what is high carbon steel made out of?
iron, 0.6-1.2% carbon, and usually small amounts of manganese
70
what are the uses of high carbon steel?
- it is used for cutting tools and masonry nails
- it is harder and more than resistant than mild steel, but also more brittle
71
what is stainless steel made up of?
iron, chromium, and often nickel
72
what are the uses of stainless steel?
- it is used in kitchen sinks, sauce pans, knives and forks, and gardening tools
- it is also used in brewing, dairy, and chemical industries
- it is resistant to corrosion
73
what is an alloy?
a mixture of a metal and one or more elements (usually other metals or carbon)
74
why are alloys harder than normal metals?
different sized atoms so the layers cant slide over each other as easily
75
what is the order of reactivity?
potassium
sodium
lithium
calcium
magnesium
aluminium
zinc
iron
copper
silver
gold
76
what is a covalent bond?
the strong electrostatic attraction between positive nuclei and shared pairs of electrons
77
why do simple molecular substances have low melting and boiling points?
the weak intermolecular forces require little energy to overcome
78
why do structures with giant covalent structures have high melting and boiling points?
the many strong covalent bonds require a lot of energy to overcome
79
what effect does increased surface area have on rates of reactions?
increasing surface area increases rate of reaction, because more reactant particles are exposed so there are more frequent collisions, and so more successful collisions per unit time
80
what is the effect of increasing the concentration of a solution on rates of reaction?
increasing the concentration increases the rate of reaction because there are more particles in the same volume so there are more frequent collisions, so there are more successful collisions per unit time
81
what effect does increasing pressure on a gas have on rate of reaction?
increasing pressure increases rate of reaction because there are the same number of particles in a smaller volume so there are more frequent collisions so there are more successful collisions per unit time
82
what effect does increasing temperature have on rate of reaction?
increasing temperature increases rate of reaction because the particles have more kinetic energy so there are more frequent collisions at the activation energy, so there are more successful collisions per unit time
83
what effect does a catalyst have on rate of reaction?
catalysts increase rate of reaction by providing an alternative route at a lower activation energy so there are more successful collisions per unit time
84
what is a catalyst
a substance that increases the rate of reaction but remains unchanged at the end of the reaction
85
how does a catalyst work?
they provide an alternative pathway with a lower activation energy
86
what is the empirical formula?
smallest whole number ratio between atoms in a compound
87
what is a molecular formula?
the actual ratio between atoms in a compound
88
what is the relationship between moles, mass, and Mr?
mass = Mr x moles
89
what is the relationship between moles, volume, and concentration?
moles = concentration x volume
90
what is the relationship between moles and volume of a gas?
moles = volume/24
91
what is a hydrocarbon?
a compound of hydrogen and carbon only
92
what is a homologous series?
a group of molecules which have:
- similar chemical reactions
- similar trend in physical properties
- same general formula
93
what is isomerism?
molecules with the same molecular formula but a different structural formula
94
what does the meth prefix mean?
one carbon atom
95
what does the eth prefix mean?
two carbon atoms
96
what does the prop prefix mean?
three carbon atoms
97
what does the but prefix mean?
four carbon atoms
98
what does the pent prefix mean?
five carbon atoms
99
what does the hex prefix mean?
six carbon atoms
100
what is a substitution reaction?
when a group of atoms is replaced by one atom or a group of atoms (eg alkanes and halogens)
101
what is an addition reaction?
when a group of atoms is added to one atom or a group of atoms (eg alkenes with bromine water)
102
what kind of reaction is alkanes and halogens?
substitution
103
what kind of reaction is alkenes and bromine water?
addition
104
what is crude oil?
a mixture of hydrocarbons
105
what are the fractions of crude oil (in order of low to high boiling point)?
refinery gasses
gasoline
kerosene
diesel
fuel oil
bitumen
106
what is the trend in colour of crude oil (low to high bp)?
light to dark
107
what is the use of refinery gases?
fuel for cooking
108
what is the use of gasoline?
fuel for cars
109
what is the use of kerosene?
fuel for aircrafts
110
what is the use for diesel?
fuel for trains
111
what is the use for fuel oil?
fuel for ships
112
what is the use of bitumen?
used to make roads
113
what is fuel?
a substance that, when burned, releases energy
114
what are the possible products of complete combustion of hydrocarbons?
carbon dioxide + water
115
what are the possible products of incomplete combustion in hydrocarbons?
carbon monoxide + water
116
what is the general formula for alkanes?
CnH2n+2
117
why are alkanes considered saturated hydrocarbons?
they have no carbon = carbon double bond
118
what is necessary for alkanes to react with halogen?
uv light
119
what happens to bromine water when it reacts with alkanes?
without uv: stays orange (no reaction happens)
with uv: turn colourless (reaction happens)
120
what do alkenes contain that alkanes dont?
c=c double bond
121
what is the general formula for alkenes?
CnH2n
122
why are alkenes unsaturated?
they have a c=c double bond
123
what happens when alkenes react with bromine water?
- turns colourless
- forms dibromoalkanes
124
how is an addition polymer formed?
joining up many small molecules called monomers
125
how could you dispose of an addition polymer?
- recycle
- incineration
- landfill
126
what are the cons of recycling?
uses energy
127
what are the pros and cons of incineration?
pro: produces energy
cons: produces carbon dioxide (green house gas --> global warming
there are toxic products (eg carbon monoxide and hydrogen chloride)
128
what are the cons of landfill?
takes up a lot of space
produces methane (a greenhouse gas)
129
what is simple distilation?
separates a liquid from a solution by heating
130
what is fractional distilation?
separates fraction (crude oil)
131
what is crystalisation?
obtain a salt from a solution
132
how do you measure Rf values?
distance moved by dot/distance moved by solvent
133
what is the test for hydrogen?
squeaky pop test
put a lit splint into gas and it will make a squeaky pop
134
what is the test for oxygen?
glowing splint test
put a glowing splint into the gas, it will relight if oxygen is present
135
what is the test for carbon dioxide?
limewater
bubble gas into limewater, it will go cloudy
136
what is the test for ammonia?
place damp red litmus paper into gas, it will go blue
137
what is the test for chlorine?
place a damp blue litmus paper into gas, it will go white
138
what kind of wire is used to carry out a flame test?
nichrome or platinum
139
what acid is the wire dipped in during a flame test?
hydrochloric acid
140
how do you test for lithium ions?
flame test
goes red
141
how do you test for sodium ions?
flame test
goes yellow
142
how do you test for potassium ions?
flame test
goes lilac
143
how do you test for calcium ions?
flame test
goes orange-red
144
what is the test for copper ions (that doesn't use sodium hydroxide)?
flame test
blue-green
145
how do you test for ammonium?
dissolve in water
add to sodium hydroxide solution
heat it
test the gas produced using damn red litmus paper (should go blue)
146
how do you test for copper ions (without a flame test)?
dissolve in water and add a few drops of sodium hydroxide
blue precipitate formed (copper hydroxide)
147
how do you test for iron (II) ions?
dissolve in water and add a few drops of sodium hydroxide
forms green precipitate
148
how do you test for iron (III) ions?
dissolve in water and add a few drops of sodium hydroxide
brown precipitate formed
149
how do you test for chloride ions?
- dissolve in water
- add nitric acid
- add silver nitrate
- forms white precipitate
150
how do you test for bromide ions?
- dissolve in water
- add nitric acid
- add silver nitrate
- forms cream precipitate
151
how do you test for iodide ions?
- dissolve in water
- add nitric acid
- add silver nitrate
- forms yellow precipitate
152
how do you test for sulphate ions?
- add hydrochloric acid and look for fizzing
- if there's no fizzing, add barium chloride
- forms white precipitate
153
how do you test for carbonates?
- add hydrochloric acid, look for fizzing
- if there is fizzing, bubble through limewater
- should go cloudy
154
how do you test for the presence of water?
add anhydrous copper (II) sulphate
goes white -> blue
