year 10 eoy exam Flashcards
1
Q
describe solids in terms of the arrangement, movement, and energy of the particles
A
they are arranged in regular rows and columns, and they are very tightly packed together, they have very little energy and do not move very much (vibrate)
2
Q
describe liquids in terms of the arrangement, movement, and energy of the particles
A
they are arranged randomly, and are still touching with some spaces between them. they have more energy than solids and the particles can move around and over each other
3
Q
describe gasses in terms of the arrangement, movement, and energy of the particles
A
they have a lot of energy, and are randomly and widely spaced out. they can move freely
4
Q
what is the name of the change from solid to liquid?
A
melting
5
Q
what is the name for the change from a liquid to a gas?
A
evaporation
6
Q
what is the name of the change from gas to solid?
A
deposition
7
Q
what is the name of the change from a solid to a gas?
A
sublimation
8
Q
what is the name of the change from a liquid to a solid?
A
freezing
9
Q
what is the name for the change from a gas to a liquid?
A
condensation
10
Q
what is a solvent?
A
the liquid in which a substance is going to be dissolved
11
Q
what is a solute?
A
the substance that is going to be dissolved
12
Q
what is a solution?
A
it is the mixture of a solvent and dissolved solute
13
Q
what is a saturated solution?
A
a solution where no more solute can be dissolved
14
Q
what is the definition of an element?
A
a substance containing only one type of atom
15
Q
what is the definition of a compound?
A
a substance containing more than one type of atom chemically bonded together
16
Q
what is the definition of a mixture?
A
two or more substances that are not chemically bonded
17
Q
what is simple distillation?
A
it is a method to separate a a solvent from a solution
the solution is heated, and the solvent evaporates, and moves away and is then cooled
simple distillation works because the solvent will have a lower boiling point than the solute
18
Q
how can you figure out if a substance is pure or not?
A
if it has a fixed boiling point, it is pure
mixtures may melt/boil over a range of temperatures
19
Q
what is fractional distillation?
A
it is used to separation of a mixture of liquids by their boiling points
it works when the liquids have different boiling points
the liquids are vaporised and are put in the fractionating column, where they then condense at different heights/temperatures, so they can be easily separated into fractions
20
Q
what is filtration?
A
it separates an insoluble salt (precipitation) from the salt solution
you would filter out the precipitate from the solution using filter paper
21
Q
what is crystallisation?
A
it is used to separate a soluble salt from the solution
you heat the solution in an open container to let the solvent evaporate out, then leave it to cool. then the solid would begin to come out of the solution and crystallise.
22
Q
what is an atom?
A
the smallest/simplest part of an element
23
Q
what is a molecule?
A
two or more atoms that are chemically bonded
24
Q
what is the nucleus of an atom made up of?
A
protons and neutrons
25
where are the electrons in an atom?
they are in the electron shells
26
what is the relative charge of sub-atomic particles?
proton: +1
neutron: 0
electron: -1
27
what is the relative mass of the sub-atomic particles
neutron: 1
proton: 1
electron: 1/2000
28
what is the atomic number?
the number of protons (the bottom one)
29
what is the mass number?
the number of protons and neutrons added together (the top one)
30
what is the number of electrons equal to?
the number of protons/the atomic number
31
what is an isotope?
atoms with the same number of protons (therefore the same element) but a different number of neutrons
32
how do you calculate the relative atomic mass from abundances?
eg. atom 1 has y neutrons 60% abundance
atom 2 has n neutrons, 40% abundance
(y x 60) + (n x 40)
/
100
33
how are atoms ordered in the periodic table?
by atomic number
34
what does the group an element is in mean?
the number of outer electrons
35
what does the period an element is in mean?
the number of electron shells
36
an atom, y has 8 electrons, what group and period is it in, and what electric configuration would it have?
group 6, period 2
2, 6
37
are metals able to conduct electricity?
yes
38
can non-metals conduct electricity?
no
39
what kind of oxides do metals have?
basic oxides
40
what kind of oxides do non-metals have?
acidic or neutral oxides
41
why do elements in the same group have similar chemical properties?
they have the same number of outer electrons so they will react and bond similarly
42
why do noble gases not react easily?
because they have a full outer shell so they are stable and don't need to gain or loose any electrons
43
how do you calculate the relative formula mass (Mr) from the relative atomic mass (Ar)?
add the Ar of each of the elements and multiply each Ar by how many atoms of it are needed
eg. H2O= (Hx2) + (Ox1)
= (1x2) + (16x1)
= 2 + 16
= 18
so the Mr of water is 18
44
what is the unit for the amount of a substance?
mol
45
what is the relationship between mass, relative formula mass, number of moles?
mass = Mr x moles
46
how do you calculate percentage yield?
amount that you got divided by the total amount you could have gotten multiplied by 100
47
what is meant by the term empirical formula?
the simplest whole-number ratio between atoms/ions in a compound
48
what is meant by the term molecular formula?
the actual number of each type of element in a molecule
49
describe the method to find out the formula of a metal oxide by combustion
1. measure the mass of the empty crucible and lid
2. add a sample of magnesium into the crucible and measure the mass of it (with the lid)
3. work out the mass of the magnesium by subtracting the mass of the empty crucible from the mass of the crucible and the magnesium
4. put the crucible and magnesium on a tripod and gauze over a Bunsen burner and heat on a blue flame for several minutes
5. make sure to lift the lid of the crucible while you heat it every 30 seconds/frequently to make sure the magnesium is fully oxidised
6. after several minutes, weigh the crucible, and then heat for another minute and weigh again. if the mass has stayed the same, the magnesium has been fully oxidised, if not, continue weighing and heating until the mass stays constant
7. measure the mass of the crucible and it's contents. subtract the mass of the empty crucible from it to find the mass of the metal oxide formed
50
why must the lid be on when heating magnesium, to form magnesium oxide to find the formula?
to prevent the magnesium escaping, but the lid must be lifted frequently to let oxygen in to react with magnesium
51
how do you find the formula of magnesium oxide from the practical of combusting metal oxides to find the formula
find the number of moles of magnesium and oxygen:
say the mass of Mg is x and the Mr is 24, x/24=a
say the mass of O is y and the Mr is 16, y/16=b
so the ratio is a:b, Mg(a)O(b)
52
how are ions formed?
by electron loss or gain
53
what is the charge of metals in group 1?
+1 (because they loose one electron so it gets less negative/more positive)
54
what is the charge of metals in group 2?
+2 (because they loose 2 electrons so it gets less negative/more positive)
55
what is the charge of metals in group 3?
+3 (because they loose 3` electrons so it gets less negative/more positive)
56
what is the charge of non-metals in group 5?
-3 (because they gain 3 electrons so they get more negative/less positive)
57
what is the charge of non-metals in group 6?
-2 (because they gain 2 electrons so they get more negative/less positive)
58
what is the charge of non-metals in group 7?
-1 (because they gain 1 electrons so they get more negative/less positive)
59
what is the charge of Ag (silver)?
+1
60
what is the charge of Cu (copper)?
+2
61
what is the charge of Fe (iron)?
+2 or +3
62
what is the charge of Pb (lead)?
+2
63
what is the charge of Zn (zinc)?
+2
64
what is the charge of hydrogen?
+1
65
what is the charge of hydroxide?
-1
66
what is the charge of ammonium?
+1
67
what is the charge of carbonate?
-2
68
what is the charge of nitrate?
-1
69
what is the charge of sulphate?
-2
70
what is the formula of hydroxide?
OH-1
71
what is the formula of ammonium?
NH4+1
72
what is the formula of carbonate?
CO₃-2
73
what is the formula for nitrate?
NO₃-1
74
what is the formula for sulphate?
SO4-2
75
what is the charge of ammonia?
nothing, it is not an ion and therefore has no charge
76
what is the formula for ammonia?
NH3
77
what is an ionic bond in terms of electrostatic bond?
strong electrostatic attraction between positive and negative ions
78
why do compounds with giant ionic lattices have high melting points?
the strong electrostatic attraction requires a lot of energy to overcome
79
can ionic compounds conduct electricity as a solid, and why?
no, because the ions are not free to move
80
can ionic compounds conduct electricity when aqueous or molten, and why?
yes, because the ions are free to move
81
what is a covalent bond?
strong electrostatic attraction between a pair of shared electrons and the positive nuclei
82
why do simple covalent structures have low melting/boiling points?
because the weak intermolecular forces require little energy to overcome
83
why does the melting/boiling point of simple molecular forces increase with increasing relative molecular mass (generally)?
because the bigger the molecule, the stronger the intermolecular forces
84
describe how you would represent metallic lattices with a 2d diagram
when metal atoms join together, the outer electrons become delocalised
metals have a giant regular arrangement of layers of positive ions surrounded by a sea of delocalised electrons
85
what is metallic bonding?
the strong electrostatic attraction between positive metal ions and delocalised electrons
86
what are the typical physical properties of metals?
they are good conductors of heat and electricity
they are malleable
they have a high melting point
87
what is the trend in physical properties in group 1 metals?
they get lighter and softer, get dull more quickly (going down the group)
88
what happens when lithium reacts with water?
fizzing, moves about, gas produced
89
what happens when sodium reacts with water?
it turns into a sphere, exothermic reaction, moves quicker than lithium, fizzes more than lithium
90
what happens when potassium reacts with water?
burns with a lilac flame, reacts quicker than sodium, bangs at the end
91
what happens when rubidium reacts with water?
explodes as soon as it touches the water
92
what happens when caesium reacts with water?
breaks tub of water due to explosion
93
what happens to the reactivity going down the group 1 metals?
the reactivity increases
94
why does the reactivity increase going down group 1 metals?
- they all need to lose one electron
- number of electron shells increases going down the group
- outer electron gets further away from nucleus
- attraction between nucleus and electron decrease
- therefore it is easier to remove
95
what is the colour and state of fluorine at room temperature?
pale yellow gas
96
what colour and state is chlorine at room temperature?
pale green gas
97
what is the colour and state of bromine at room temperature?
red/brown liquid
98
what is the colour and state of iodine at room temperature?
grey solid
99
what colour and state is astatine at room temperature?
black solid
100
what happens when fluorine is reacted with iron wool?
too reactive to find out
101
what happens when chlorine is reacted with iron wool?
slight heating causes a violent reaction
102
what happens when bromine is reacted with iron wool?
strong heating causes a visible reaction
103
what happens when iodine is reacted with iron wool?
very strong heating for a few minutes causes a slight reaction
104
what happens when astatine is reacted with iron wool?
even less reaction than iodine
105
what is the trend in reactivity going down group seven?
the reactivity decreases
106
why does the reactivity decrease going down group seven?
- they all need to gain one electron
- number of shells increases going down the group
- incoming electron is further away from the nucleus
- weaker attraction between electron and nucleus
- harder to gain electrons
107
what percentage of nitrogen is in dry air?
78%
108
what percentage of oxygen is in dry air?
21%
109
what percentage of argon is in dry air?
0.8%
110
what percentage of carbon dioxide is in dry air?
0.04%
111
what happens when magnesium reacts with oxygen?
bright white light + white powder formed
112
what happens when hydrogen reacts with oxygen?
causes explosive reaction (squeaky pop test)
113
what happens when sulphur reacts with oxygen?
produces a blue flame
114
what happens when copper carbonate is heated (thermal decomposition)
copper carbonate --> carbon dioxide + copper oxide
(CuCO3 --> CuO + CO2)
115
what is the order of reactivity for metals (most reactive -> least reactive)?
potassium
sodium
lithium
calcium
magnesium
aluminium
carbon
zinc
iron
lead
hydrogen
copper
mercury
silver
gold
platinum
116
under which conditions does iron rust?
when both water and oxygen are present
117
what is the barrier method?
preventing oxygen and water from reaching the iron by covering the iron in something else (eg. plastic, oil)
118
what is galvanising?
it is when iron is covered in zinc to prevent rusting. the zinc acts as a barrier and prevents oxygen and water reaching the iron but even if it is broken, zinc is more reactive than iron so it still wont rust
119
what is sacrificial protection?
it is when the iron is coated in something more reactive as the oxygen will react with that first and not the iron
120
what is oxidation?
the loss of electrons or the gain of oxygen
121
what is reduction?
the gain of electrons or the loss of oxygen
122
what is an oxidising agent?
something that gives oxygen, or takes electrons (something that has been reduced)
123
what is a reducing agent?
something that takes oxygen or gives electrons (something that has been oxidised)
124
how are metals more reactive than carbon extracted?
electrolysis (breaking down compound using electricity)
125
how are metals less reactive than carbon extracted?
reacted with carbon - displacement reaction
126
what metals do not need extraction?
mercury and silver (might need purifying though)
gold and platinum
127
what is the use 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
128
what is mild steel made of?
iron and up to 0.25% carbon
129
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
130
what is high-carbon steel made up of?
iron, 0.6-1.2% carbon, and small amounts of manganese
131
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
132
what is stainless steel made of?
iron, chromium, and usually nickel
133
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
134
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
135
what is an alloy?
a mixture of a metal and one or more elements
136
why are alloys harder than pure metals?
in an alloy, the elements have slightly differently sized elements, which breaks up the normal lattice arrangement and prevents the layers sliding over eachother
137
what is the test for hydrogen/
the squeaky pop test; put a lit splint in the gas, and if it makes a squeaky pop, hydrogen is present
138
what is the test for oxygen?
put a glowing splint in the gas, if it relights, oxygen is present
139
what is the tests for carbon dioxide?
bubble the gas into lime water, if it goes cloudy, carbon dioxide is present
140
what is the test for chlorine?
use damp blue litmus paper, if chlorine is present it will go white
141
what is the test for chloride ions?
add nitric acid to remove impurities, then add silver nitrate solution. if chloride ions are present, it will form a white precipitate of silver chloride
142
what is the test for bromide ions?
add nitric acid to remove impurities, then add silver nitrate solution. if bromide is present, it will form a cream precipitate of silver bromide
143
what is the test for iodide ions?
add nitric acid to remove impurities, then add silver nitrate solution. if iodide ions are present, it will form a yellow precipitate of silver iodide
144
how do you test for sulphate ions?
add hydrochloric acid to remove impurities, then add barium chloride solution. if sulphate ions are present, a white precipitate of barium sulphate will form
145
how do you test for carbonate ions?
use hydrochloric acid, if it fizzes, carbonate ions are present
146
what is a chemical test for water?
use anhydrous copper sulphate. if it turns from white to blue, water is present
147
what is a physical test for pure water?
it will boil at 100 degrees celcius
148
what can be used to distinguish acidic and alkaline solutions?
universal indicator, red and blue litmus paper, methyl orange, phenolphthalein
149
what colour is methyl orange in acids?
red
150
what colour is methyl orange in neutrals?
yellow
151
what colour is methyl orange in alkalis?
yellow
152
what colour is phenolphthalein in acids?
colourless
153
what colour is phenolphthalein in neutrals?
colourless
154
what colour is phenolphthalein in alkalis?
pink
155
what colour is universal indicator in acids?
red
156
what colour is universal indicator in neutrals?
green
157
what colour is universal indicator in alkalis?
blue/purple
158
what colour is blue litmus in acids?
red
159
what colour is blue litmus in neutrals?
blue
160
what colour is blue litmus in alkalis?
blue
161
what colour is red litmus in acids?
red
162
what colour is red litmus in neutrals?
red
163
what colour is red litmus in acids?
red
164
what is the pH of a strongly acidic substance?
0-3
165
what is the pH of a weakly acidic substance?
4-6
166
what is the pH of a neutral substance?
7
167
what is the pH of a weakly alkaline solution?
8-10
168
what is the pH of a strongly alkaline solution?
11-14
169
what are acids in an aqueous solution a source of?
hydrogen ions
170
what are alkalis in an aqueous solution a source of?
hydroxide ions
171
can alkalis neutralise acids?
yes
172
are common sodium, potassium, and ammonium compounds soluble?
yes
173
are nitrates soluble?
yes
174
are common chlorides soluble (except from silver and lead II)?
yes
175
are silver chlorides soluble?
no
176
are lead (II) chlorides soluble?
no
177
are common carbonates soluble (except for those of sodium, potassium and aluminium)?
no
178
is sodium carbonate soluble?
yes
179
is potassium carbonate soluble?
yes
180
is aluminium carbonate soluble?
yes
181
are common sulphates soluble (except for those of barium, calcium, and lead (II))?
yes
182
is barium sulphate soluble?
no
183
is calcium sulphate soluble?
no
184
is lead (II) sulphate soluble?
no
185
are common hydroxides soluble (other than those of sodium, potassium, and calcium)?
no
186
is sodium hydroxide soluble?
yes
187
is potassium hydroxide soluble?
yes
188
is calcium hydroxide soluble?
slightly
189
what is an acid in terms of proton transfer?
acids are proton (H+) donors
190
what are bases in terms of proton transfer?
bases are proton (H+) acceptors
191
what happens when an alkali is reacted with an acid?
alkali + acid --> water + salt
192
what happens when a base is reacted with an acid?
base + acid --> water + salt
193
what happens when a carbonate is reacted with an acid?
carbonate + acid --> water + salt + carbon dioxide
194
what happens when a metal is reacted with an acid (excluding nitric acid)?
metal + acid --> salt + hydrogen
195
what are alkalis in terms of bases?
soluble bases
196
what can act as bases?
metal oxides, metal hydroxides, ammonia
197
describe an experiment to prepare a pure dry sample of a soluble salt from an insoluble reactant
- add excess insoluble base to the acid
- filter to react the unreacted base
- heat the solution so water evaporates and crystals remain
198
describe an experiment to prepare a pure dry sample of a soluble salt from an acid and an alkali
- use titration to find the exact volume of alkali that reacts with the acid
- mix the exact volumes of the acid and base
- warm solution so water evaporates and crystals remain
199
describe an experiment to prepare a pure, dry sample of an insoluble salt from two soluble reactants
- mix solutions of two soluble reactants
- filter mixture (insoluble salt will remain on the paper)
- wash salt with distilled water
- leave salt to dry
200
how do you prepare pure dry copper sulphate crystals from copper (II) oxide?
1. heat the sulphuric acid
2. add copper oxide until no more disappears (while stirring continuously)
3. filter out the excess base
4. transfer solution into evaporating dish
5. heat until crystals start to form
6. leave to crystallise for a few days
7. filter or pick out crystals
8. pat dry with filter paper
201
how do you prepare pure, dry lead (II) sulphate crystals?
1. mix the aqueous lead (II) nitrate solution and the aqueous potassium sulphate solution together
2. filter out sat precipitate
3. rinse with distilled water
4. dry salt by patting with filter paper
202
how does temperature effect the rate of reaction?
rate of reaction increases with increasing temperature. the particles have more kinetic energy so the collide at the required activation energy more often, so there are more successful collisions per unit time
203
how does surface area effect rate of reaction?
increasing surface area increases the rate of reaction. more of the reactant is exposed, so there are more frequent collisions, so there are more successful collisions per unit time
204
how does concentration effect the rate of reaction?
increasing concentration increases the rate of reaction. there are more particles in the same volume, so there are more frequent collisions, so there are more successful collisions per unit time
205
how does pressure effect 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
206
how do catalysts effect the rate of reaction?
catalysts increase the rate of reaction by providing an alternative route with a lower activation energy, so there are more successful collisions per unit time
207
what are catalysts?
they are substances that increases the rate of reaction, but remain chemically unchanged at the end of the reaction
208
what is the method to investigate how surface area of a solid effects the rate of reaction?
1. measure out 3g of marble chips into a conical flask
2. set up a delivery tube and inverted 50cm3 measuring cylinder full of water in a trough
3. measure out 20m3 of hydrochloric acid with a measuring cylinder
4. add the hydrochloric acid to the conical flask, fit the bung, and start the timer
5. measure and record the volume of carbon dioxide in the measuring cylinder every 5 seconds
6. stop either when the measuring cylinder is full or after 60 seconds (whichever is sooner)
7. repeat with two different sizes of marble chips
209
what is the method to investigate the effects of different catalysts on the decomposition of hydrogen peroxide?
1. using a measuring cylinder, measure out 50cm3 of hydrogen peroxide into a conical flask
2. connect the gas syringe to the bung using a delivery tube. make sure the syringe is close (its on zero)
3. measure out 0.5g of the first catalyst being tested eg. manganese (IV) oxide
4. add the manganese (IV) oxide to the conical flask and immediately attach the bung to it. start the timer
5. measure the amount of gas in the syringe every 10 seconds. stop timing after 60 seconds
6. repeat 1-5 for platinum, iron (V) oxide, and vanadium (V) oxide
210
what is a hydrocarbon?
a compound containing hydrogen and carbon only
211
what is crude oil?
a mixture of hydrocarbons
212
how is crude oil separated into fractions?
it is vaporised then it enters the fractioning column, where it rises and the temperature falls. different fractions condense at different times, so they are separated
213
what are the names of the fractions of crude oil in order of increasing boiling point?
refinery gasses, gasoline, kerosene, diesel, fuel oil, bitumen
214
what is the trend in colour of the fractions of crude oil?
gets darker going down
215
what is the trend in viscosity in the fractions of crude oil?
increases going down
216
what is a fuel?
a substance that, when burned, releases heat energy
217
what are the uses of refinery gasses?
fuel for heating and cooking
218
what are the uses of gasoline?
fuel for cars (NOT VANS)
219
what are the uses of kerosene?
fuel for planes
220
what are the uses of diesel?
fuel for lorries/trains (NOT VANS)
221
what are the uses of fuel oil?
fuel for boats (NOT SHIPS)
222
what is the use for bitumen?
making roads
