actual gcse spec points (paper one) Flashcards
1
Q
solid –> liquid?
A
melting
2
Q
liquid –> gas?
A
evaporation
3
Q
gas –> liquid?
A
condensation
4
Q
liquid –> solid?
A
freezing
5
Q
solid –> gas?
A
sublimation
6
Q
gas –> solid?
A
deposition
7
Q
what are elements in the periodic table arranged by?
A
in order of atomic number
8
Q
which ones are the groups?
A
vertical
9
Q
which ones are periods?
A
horizontal
10
Q
what does the group an atom is in determine?
A
the number of outer shell electrons
11
Q
what does the period an atom is in determine?
A
the number of electron shells
12
Q
do metals conduct electricity?
A
yes
13
Q
do non-metals conduct electricity?
A
no
14
Q
what kind of oxides to metals form?
A
basic oxides (which react with acids to form a salt and water)
15
Q
what kind of oxides do non-metals form?
A
acidic or neutral
16
Q
what happens when magnesium is combusted in oxygen?
A
bright white flame
17
Q
what happens when hydrogen is combusted in oxygen?
A
explosive reaction - think squeaky pop test
18
Q
what happens when sulphur is combusted in oxygen?
A
blue flame
19
Q
what is thermal decomposition?
A
breaking down using heat
20
Q
what is the observation for the decomposition of copper carbonate?
A
green powder –> black powder
21
Q
how do metal carbonates decompose? as in what do they form
A
metal oxides and carbon dioxide
22
Q
what is a solvent?
A
the liquid in which a substance is going to be dissolved
23
Q
what is a solute?
A
the substance that is going to be dissolved
24
Q
what is a solution?
A
it is the mixture of a solvent and dissolved solute
25
what is a saturated solution?
a solution where no more solute can be dissolved
26
what is the definitions of an element?
a substance containing only one type of atom
27
what is the definition of a compound?
a substance containing more than one type of atom chemically bonded together
28
what is the definition of a mixture?
two or more substances that are not chemically bonded
29
what percentage of nitrogen is in dry air?
78%
30
what percentage of oxygen is there in dry air?
21%
31
what percentage of argon is there in dry air?
0.9%
32
what percentage of carbon dioxide is there in dry air?
0.035%
33
what is the pH of a strongly acidic substance?
0-3
34
what is the pH of a weakly acidic substance?
4-6
35
what is the pH of a neutral substance?
7
36
what is the pH of a weakly alkaline substance?
8-10
37
what is the pH of a strongly alkaline substance?
11-14
38
where are the neutrons and protons?
nucleus
39
where are the electrons?
the electron shells
40
what is the relative mass of the sub-atomic particles?
neutron: 1
proton: 1
electron: 1/2000
41
what is the relative charges of the sub-atomic particles?
protons: 1
neutrons: 0
electrons: -1
42
what is the atomic number?
the number of protons
43
what is the mass number?
the number of protons and neutrons
44
what is an isotope?
atoms with the same number of protons but a different number of electrons
45
what is the relative atomic mass?
average atomic mass (mass number)
46
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
47
how are elements arranged in the periodic table?
by increasing atomic number
48
what does the period an atom is in mean?
number of electron shells
49
what does the group an atom is in mean?
number of outer shell electrons
50
what is oxidation?
loss of electrons or gain of oxygen
51
what is reduction?
gain of electrons or loss of oxygen
52
what is an oxidising agent?
something that gives up oxygen or takes electrons (gets reduced)
53
what is a reducing agent?
something that takes oxygen or gives up electrons (gets oxidised)
54
how are ions formed?
by electron loss or gain
55
is a cation positive or negative?
positive
56
is an anion positive or negative?
negative
57
what charge does silver get?
+1
58
what charge does copper get?
+2
59
what charge does iron (ii) get?
+2
60
what charge does iron (iii) get?
+3
61
what charge does lead get?
+2
62
what charge does zinc get?
+2
63
what charge does hydrogen get?
+1
64
what charge does hydroxide have?
-1
65
what charge does ammonium have?
+1
66
what charge does carbonate have?
-2
67
what charge does nitrate have?
-1
68
what charge does sulphate have?
-2
69
what is the formula of a hydroxide ion?
OH-
70
what is the formula of an ammonium ion?
NH4+
71
what is the formula of a carbonate ion?
CO3-2
72
what is the formula of a nitrate ion?
NO3-
73
what is the formula of a sulphate ion?
SO4-2
74
what is ionic bonding in terms of electrostatic attraction?
strong electrostatic attraction between positive and negative ions
75
why do compounds that form giant ionic lattices have high melting and boiling points?
strong electrostatic attraction between oppositely charged ions requires lots of energy to overcome
76
when can/can't ionic compounds conduct electricity?
they can only conduct electricity when molten or aqueous, they can't conduct when solid
77
why can't ionic compounds conduct electricity when solid?
there are no ions free to move
78
what is the reactivity series of the metals that are more reactive than carbon?
potassium
sodium
lithium
calcium
magnesium
aluminium
79
what is the reactivity series of the metals that are less reactive than carbon (but more reactive than hydrogen)?
zinc
iron
lead
80
what is the reactivity series of the metals that are less reactive than hydrogen (and carbon obviously)?
copper
silver
gold
81
which metals in the reactivity series react with water?
potassium, sodium, lithium, calcium
82
which metals in the reactivity series react with acid?
those above copper (as in copper can't)
83
what happens when magnesium reacts with hydrochloric acid? (i think this happens with sulphuric acids and other metals too, but more reactive metals will react more vigorously)
- fizzing
- colourless gas (hydrogen)
- reaction becomes warm (exothermic)
- magnesium disappears to leave a colourless solution of magnesium chloride
84
what is the equation for the reaction between an acid and an alkali?
alkali + acid --> water + salt
(AAWS)
85
what is the equation for the reaction between an acid and a base?
base + acid --> water + salt
(BAWS)
86
what is the equation for the reaction between an acid and a carbonate?
carbonate + acid --> water + salt + carbon dioxide
(CAWS COD)
87
what is the equation for the reaction between an acid and a metal?
metal + acid --> salt + hydrogen
(MASH)
88
what is the test for hydrogen gas?
place a lit splint into the gas, makes a squeaky pop
89
how are most metals extracted?
from ores found in the earth's crust
90
how are unreactive metals often found?
as an uncombined element
91
which extraction method is used for metals below carbon in the reactivity series?
extracted with carbon in a displacement reaction
92
which extraction method is used for metals above carbon in the reactivity series?
electrolysis
93
in what conditions does iron rust?
when oxygen and water are present
94
how does the barrier method prevent rusting?
prevents the oxygen and water from reaching the iron
95
how does galvanising 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 won't rust because the oxygen (or water) will react with the zinc before reacting with the iron
96
how does sacrificial protection prevent rusting?
the oxygen will react with the substance that has been used to coat the iron before reacting with the iron
97
what are acids in an aqueous solution a source of?
a source of hydrogen ions
98
what are alkalis in an aqueous solution a source of?
hydroxide ions
99
what is an acid?
a proton donor
100
what is a base?
a proton acceptor
101
what are alkalis?
bases that are soluble in water
102
what can act as bases?
metal oxides, metal hydroxides, and ammonia
103
is sodium soluble in water?
yes
104
is potassium soluble in water?
yes
105
is ammonium soluble in water?
yes
106
are group one soluble?
yes
107
are nitrates soluble?
yes
108
are halides soluble?
yes, except for silver halides and lead halides
109
are chlorides soluble?
yes, except for silver and lead chlorides
110
are sulphates soluble?
yes, except for calcium, barium, and lead sulphates
111
are carbonates soluble?
no except for sodium, potassium, and ammonium carbonates
112
are hydroxides soluble?
no except for sodium and potassium hydroxides (calcium hydroxide is slightly soluble)
113
is barium hydroxide soluble?
yes
114
what is the experiment to prepare a pure, dry sample of a soluble salt, starting from an insoluble reagent?
insoluble base and acid method:
- heat acid up
- add base until no more disappears while stirring with a glass rod
- filter out excess base
- gently heat filtered solution until crystals start to form
- allow solution to cool and leave to crystallise
- filter out the crystals
- pat dry with filter paper
115
what method is used to prepare a pure, dry hydrated copper (II) sulphate crystals starting from copper (II) oxide?
insoluble base and acid method
116
how is a covalent bond formed between atoms?
by the sharing of a pair of electrons
117
what is a covalent bond?
strong electrostatic attraction between nuclei and shared pairs of electrons
118
why do simple molecular structures have low melting and boiling points?
the weak intermolecular forces require little energy to overcome
119
why do the melting and boiling points of simple molecular substances increase with increasing relative molecular mass?
molecules with larger masses have more intermolecular forces, so larger molecules have more intermolecular forces which must be overcome
120
do covalent compounds usually conduct electricity?
no
121
why do giant covalent structures have high melting and boiling points?
they have many strong covalent bonds which require a lot of energy to overcome
122
why is diamond hard?
doesn't have layers and has many strong covalent bonds in the giant lattice which require a lot of energy to overcome
123
can diamond conduct electricity?
no
124
why can't diamond conduct electricity?
because there are no free moving charged particles
125
why is graphite soft?
made of layers which can easily slide over eachother
126
can graphite conduct electricity?
yes
127
why can graphite conduct electricity?
has delocalised electrons which are free to move
128
why is the C60 fullerene soft?
the molecules can roll over each other easily
129
why does the C60 fullerene have a higher BP compared to other simple molecular structures?
it has a higher molecular mass (although its BP is still low)
130
can the C60 fullerene conduct electricity?
no
131
what is produced when group one metals react with water?
metal hydroxide and hydrogen
132
what are the observations of the reaction between water and sodium/potassium/lithium?
- fizzing (hydrogen is produced)
- metal floats and moves around on the water
- metal disappears
133
what is the trend of reactivity of group one?
get more reactive as you go down the group
134
what does fluorine look like at room temperature?
very pale yellow gas
135
what does chlorine look like at room temperature?
pale green gas
136
what does bromine look like at room temperature?
red/brown liquid
137
what does iodine look like at room temperature?
grey solid
138
what does astatine look like at room temperature?
black solid
139
how does reactivity change in group 7?
become less reactive down group 7
140
what is the effect of changing concentration on
