paper 1 Flashcards
(131 cards)
1
Q
aqueous means
A
dissolved in water
2
Q
water
A
H2O
3
Q
ammonia NH3
A
4
Q
carbon dioxide
A
CO2
5
Q
hydrogen
A
H2
6
Q
Chlorine
A
Cl2
7
Q
Oxygen
A
O2
8
Q
how do ions form
A
ions form when atoms or groups of atoms gain or loose electrons to form charged particles
9
Q
formula for ammonium
A
NH4+
10
Q
nitrate formula
A
NO3-
11
Q
Hydroxide
A
OH-
12
Q
carbonate
A
CO3^2-
13
Q
sulfate
A
SO4^2-
14
Q
element definition
A
- substance made out of one kind of atom only.
15
Q
compound definition
A
a pure substance made out of two or more different elements that are chemically bonded.
16
Q
mixture definition
A
a combination of two or more substances that are NOT chemically bonded
17
Q
john daltons atom theory
A
solid spheres made up from different elements
18
Q
jj thomson atom theory (1897)
A
atoms aren’t solid spheres
discovered electrons
plum pudding model
19
Q
1909 rutherford atom theory
A
fired positively charged alpha particles at an extremely thin sheet of gold
some particles deflected more than expected some deflected backwards
plum pudding model was wrong
theory of the nuclear atom
nucleus
20
Q
bohr atom theory
A
new model where all the electrons were contained in shells
electrons can only exist in fixed orbits
each shell has a fixed energy
21
Q
relative mass and relative charge of proton
A
relative mass = 1
relative charge = +1
22
Q
relative mass and relative charge of neutron
A
relative mass = 1
relative charge = 0
23
Q
relative mass and relative charge of electrons
A
relative mass = 0.0005
relative charge = -1
24
Q
nucleus contains
A
protons and neutrons
positively charged
25
where are electrons in an atom
move around in shells
negatively charged alpha particles
small mass
26
atoms are
neutral
27
why are atoms neutral
same number of protons and electrons
28
in an ion the number of protons doesn’t equal
the number of electrons , this means it has an overall charge
29
the mass number tells you
total number of protons and neutrons
( mass is in the nucleus to remember)
30
atomic number tells you
how many protons an atom has
31
how to work out number of neutrons
atomic number - mass number
32
isotope definition
the atoms have the same number of protons but with a different number of neutrons
eg carbon 12 , carbon 13 , carbon 14 are isotopes of carbon
33
Ar means
relative atomic mass
34
Ar of an element is the
average mass of one atom compared to 1/13 of the mass of one atom
35
how to work out relative atomic mass
(_x_)+(_+_) / both abundances +
36
differences between modern day periodic table and mendeleevs periodic table
mend ordered by atomic mass
left gaps for future elements
37
group 1 elements have
1 outer shell
38
group 7 elements have
7 outer shell electrons
39
group 0 have
full outer shell of 8 electrons
or two in the case of helium
40
horizontal rows are called
periods
41
vertical rows are
groups
42
how many electrons can go on the first second and third shell
first ~ 2 electrons
second ~ 8 electrons
third ~ 8 electrons
43
electronic configuration is
amount of electrons in each shell
eg. 2.8.8
44
group number tells you
number of electrons in the outer shell
45
number of shells is the same as the
period of the element
46
negative ions are
anions and are formed when atoms gain electrons
47
positive ions are
cations and they form when atoms lose electrons
48
OILRIG
oxidation is reduction of electrons
reduction is gain of electrons
49
group 1 and two are
metals , they lose electrons to form positive ions
50
group 6,7 are
non metals , gain electrons to form negative ions
51
elements in the same group
same number of outer electrons
have to lose or gain the same number to get a full outer shell
this means that they form ions with the same charge
52
ionic compounds are make up of
positively charged part and a negatively charged part
53
the overall charge of any ionic compound is
zero
54
ions ending in -ate are
negatively charged ions containing oxygen and at least one other element
55
ions ending in -ide mean
negative ions containing only one element
except hydroxide ions which are OH-
56
ionic bonding
when a metal and non metal react together
metal atom looses electrons to form cation
non metal gains these electrons to form anion
oppositely charged ions are strongly attracted to one another by electrostatic forces
attraction is called an ionic bond
57
ionic compound structure
giant ionic lattice structure
strong electrostatic forces of attraction between oppositely charged ions
58
ionic compound properties
high melting and boiling points due to strong attraction
don’t conduct electricity when ions are fixed
dissolve easily in water r
59
covalent bond is
strong bond that forms when a pair of electrons is shared between two atoms
60
properties of simple molecular substances
held by very strong covalent bond
low boiling and melting points
don’t conduct electricity
61
polymers are
molecules made up of long chains of covalently bonded carbon atoms
62
giant covalent structure properties
high melting and boiling points
aren’t soluble in water
don’t conduct electricity (except graphite and graphene )
63
diamond structure properties
strong covalent bond
high melting point
doesn’t conduct electricity
64
graphite structure
carbon atoms arranged in hexagons
bonds held weak
high melting
conducts electricity
65
graphene structure
one layer of graphite
sheet of carbon atoms joined together in hexagons
one atom thick
66
fullerenes are
molecules of carbon shaped like closed tubes or hollow balls
67
metals have a
giant structure
68
delocalised means
feee to move around
69
electrostatic attraction hold atoms together in a regular structure and are knows as
metallic bonding
70
all metals are bonded by
metallic bonding
71
non metal characteristics
brittle
dull
low boiling points
don’t conduct electricity
72
non metals gain
electrons to gain full outer shell
73
metals loose
electrons to gain full outer shells
74
avogadros constant / mole is equal to
6.02 x 10^23
75
moles =
mass / relative atomic mass
76
concentration =
mass of solute / volume of solution
77
reactions stop when
one reactant is used up
78
three states of matter
solid, liquid, gas
79
properties of a solid
strong forces of attraction between particles
fixed position
particles don’t move
can vibrate in fixed position
80
properties of a liquid
some force of attraction between particles
don’t keep a definite shape
particles constantly moving
81
properties of a gas
no force of attraction between particles
free to move
hotter the gas gets the faster particles move
82
physical changes are
reversible
83
chemical changes aren’t
easily reversible
84
liquid to gas is
evaporation
85
gas to liquid is
condensing
86
solid to gas is
subliming
87
solid to liquid is
melting
88
liquid to solid is
freezing
89
a pure substance is
a substance that is completely made up of a single element or compound
90
distillation practical to separate solutions
pure water from sea water
thermometer
distillation flask
heat source eg bunsen burner
pour seawater into a distillation flask
connected the bottom end of the condenser to a cold tap using rubber tubing
run cold water through the condenser to keep it cool
gradually heat the distillation flask
the water vapour passes into the condenser where it cools and condenses
flows into beaker where it is collected
eventually salt will be left in the flask
91
fractional distillation
separating mixture of liquids
crude oil substitute ??
put mixture in a flask
fractionating column attach
gradually heat flask, different liquids will have different boiling points so evaporate at different temps
when the first liquid has been collected, raise the temperature until the next one reaches the top
92
filtration
filter paper
funnel
beaker
93
crystallisation
bunsen burner
evaporation dish
pour solution onto evaporating dish and gently heat solution
some water will evaporate and the solution will get more concentrated
once some water have evaporated/ crystals start to form , remove the dish from heat and leave solution to cool
salt should start to form crystals as it becomes insoluble in the cold, highly concentrated solution
filter the crystals out of the solution and leave them in a warm place to dry
94
chromatography
filter paper
ink
solvent
beaker
watch glass
draw a line near the bottom of the paper (baseline) USE A PENCIL
put a spot of mixture to be separated on the line
put solvent into a beaker
dip the bottom of the paper into solvent BUT NOT THE SPOT OF INK
put a watch glass ontop of the beaker to stop any solvent from evaporating
remove the paper before solvent reaches top of paper
mark the distance w a pencil
95
rf value =
distance travelled by solute / distanced travelled by solvent
96
steps of water purification
filtration - wire mesh screens out large twigs and then the gravel and sand beds filter out any other solid bits
sedimentation - iron ingrate or aluminium sulfate is added to water which makes fine particles clump together and settle at the bottom
chlorination - chlorine gas is bubbled through to kill harmful bacteria
97
litmus is
red in acidic solutions
purple in neutral
blue in alkali
98
methyl orange is
red in acidic
yellow in neutral and alkali
99
phenolphthalein
colourless in acidic or neutral solution
pink in alkaline
100
acids and bases
neutralise eachother
produce a salt and water
101
102
acids produce ______ in water
hydrogen ions
103
strong acids
ionise almost completely in water
104
weak acids
do not fully ionise in solution
105
acid + metal oxide —->
salt + water
106
acid + metal hydroxide ——>
salt + water
107
acid + metal ——>
salt + hydrogen
108
test for hydrogen
lit split
squeaky pop
109
test for oxygen
lit splint blow out
glow
reignited in tube
110
text for carbon dixodide
bubbling gas through limewater
if gas is co2 , limewater will turn cloudy
111
acid + metal carbonate —->
salt + water + carbon dioxide
112
electrolysis is
the breaking down of a substance using electricity
an electric current is passed through an electrolyte causing it to decompose
113
electrolyte is
a molten or dissolved ionic compound
114
the positive ions ( cations ) in the electrolyte moves toward the cathode and are
reduced ( gain electrons )
115
the negative ions (anions ) in the electrolyte moves toward the anode and are
oxidised ( lose electrons )
116
if something gains oxygen it’s
oxidised
117
the more reactive something is the
easily it is to oxidise
118
test for zinc
quiet sqeaky pop
119
test for iron
very quiet squeaky pop
120
metal + water ——>
metal hydroxide + hydrogen
121
reduction and oxidation can happen simultaneously this is called a
redox reaction
122
displacement reactions are examples of
redox reactions
123
if you put a less reactive metal into a solution of a more reactive metal salt ,
nothing will happen
124
how can a metal be extracted from its ore
chemically by reduction using carbon
when an ore is reduced oxygen is removed from
125
what is the haber process
nitrogen and hydrogen react to form ammonia
N2 +3H2 ===>< 2NH3
126
what is equilibrium
when the forward reaction will be going the same rate as backward one
127
at equilibrium both reactions are taking place but
there’s no overall affect
128
closed system means
none of the reactants or products can escape
129
equilibrium can only be reached if the reversible reaction takes place …
in a closed system
130
what can change the position of equilibrium
temperature , pressure and concentrations
131
exothermic vs endothermic
exo - heat given out
endo - heat given in
