Search for notes by fellow students, in your own course and all over the country.
Browse our notes for titles which look like what you need, you can preview any of the notes via a sample of the contents. After you're happy these are the notes you're after simply pop them into your shopping cart.
Document Preview
Extracts from the notes are below, to see the PDF you'll receive please use the links above
4
5
6
7
Li Be
B
C
N
O
F Ne
Na Mg
Al Si
P
S
Cl Ar
Rb Sr
Y
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt ?
?
?
Metals to the left of this line, non
metals to the right
To the right of
the Periodic
table
Form negative ions
...
Halogens
Consist of molecules made of a pair
of atoms
Have seven electrons in their
outer shell
...
Increasing atomic mass number
...
g
...
g
...
Knowledge of isotopes
explained why order based on atomic
weights was not always correct
...
g
...
g
...
g
...
Conductors, high melting and
boiling points, ductile,
malleable
...
Increasing
atomic
number
...
Form +1 ions
...
With
oxygen
Forms a metal
oxide
Metal + oxygen →
metal oxide
e
...
4Na + O2 →
2Na2O
With
water
Forms a metal
hydroxide and
hydrogen
Metal + water →
metal hydroxide +
hydrogen
e
...
2Na + 2H2O →
2NaOH + H2
With
chlorine
Forms a metal
chloride
Metal + chlorine →
metal chloride
e
...
2Na + Cl2 →
2NaCl
Compared
to group 1
Boiling
points
increase
down the
group
Elements in the same group have the
same number of outer shell electrons and
elements in the same period (row) have
the same number of electron shells
...
Alkali metals
K Ca Sc Ti
The Periodic
table
Mendeleev
Transition metals
0
He
Elements with similar
properties are in columns
called groups
Before discovery
of protons,
neutrons and
electrons
3
Elements
arranged in
order of atomic
number
Group 1
1 2
H
Noble gases
Halogens
Development
of the Periodic
table
Alkali metals
Typical
properties
• Less reactive
• Harder
• Denser
• Higher melting points
• Many have different ion
possibilities with different
charges
• Used as catalysts
• Form coloured compounds
• Cu2+ is blue
• Ni2+ is pale green, used in the
manufacture of margarine
• Fe2+ is green, used in the
Haber process
• Fe3+ is reddish-brown
• Mn2+ is pale pink
1 2
H
3
4
5
6
7
Li Be
B
C
N
O
F Ne
Na Mg
Al Si
P
S
Cl Ar
Y
The Periodic
table
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt ?
?
?
Metals to the left of this line, non
metals to the right
To the right of
the Periodic
table
Form positive ions
...
Form negative ions
...
Consist of molecules made of a pair
of atoms
Metals and
non metals
Group
7
To the left of
the Periodic
table
Have seven electrons in their
outer shell
...
Melting and boiling points increase
down the group (gas → liquid →
solid)
Increasing atomic mass number
...
g
...
g
...
g
...
e
...
Cl2 + H2 → 2HCl
e
...
Cl2 +2KBr →2KCl
+ Br2
Boiling
points
increase
down the
group
Increasing
atomic
number
...
Elements arranged in order
of atomic weight
Early periodic tables were incomplete,
some elements were placed in
inappropriate groups if the strict order
atomic weights was followed
...
Knowledge of isotopes
explained why order based on atomic
weights was not always correct
...
Form +1 ions
...
Forms a metal
oxide
Metal + oxygen →
metal oxide
e
...
4Na + O2 →
2Na2O
Forms a metal
hydroxide and
hydrogen
Metal + water →
metal hydroxide +
hydrogen
e
...
2Na + 2H2O →
2NaOH + H2
Forms a metal
chloride
Metal + chlorine →
metal chloride
e
...
2Na + Cl2 →
2NaCl
• Less reactive
• Harder
• Denser
• Higher melting points
• Many have different ion
possibilities with different
charges
• Used as catalysts
• Form coloured compounds
• Cu2+ is blue
• Ni2+ is pale green, used in the
manufacture of margarine
• Fe2+ is green, used in the
Haber process
• Fe3+ is reddish-brown
• Mn2+ is pale pink
1 2
H
3
4
5
6
7
Li Be
B
C
N
O
F Ne
Na Mg
Al Si
P
S
Cl Ar
Y
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
Fr Ra Ac Rf Db Sg Bh Hs Mt ?
?
?
Metals to the left of this line, non
metals to the right
Form positive ions
...
Have seven electrons in their
outer shell
...
Increasing atomic mass number
...
g
...
g
...
Knowledge of isotopes
explained why order based on atomic
weights was not always correct
...
Insulators,
low melting and boiling points
...
The Periodic
table
e
...
NaCl
metal atom loses
outer shell electrons
and halogen gains an
outer shell electron
AQA GCSE
Atomic structure
and periodic
table part 2
Group 0
Group 1
Rb Sr
0
He
Development
of the Periodic
table
K Ca Sc Ti
Elements in the same group have the
same number of outer shell electrons and
elements in the same period (row) have
the same number of electron shells
...
Negative outer electron is further
away from the positive nucleus so is
more easily lost
...
g
...
g
...
g
...
g
...
g
...
Form +1 ions
...
• Fe2+ is green, used in the
Haber process
• Fe3+ is reddish-brown
• Mn2+ is pale pink
better hope – brighter future
1 2
H
3
4
5
6
7
Li Be
B
C
N
O
F Ne
Na Mg
Al Si
P
S
Cl Ar
Y
Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te
I
Xe
Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn
?
?
Metals to the left of this line, non
metals to the right
Metals and
non metals
Group
7
Fr Ra Ac Rf Db Sg Bh Hs Mt ?
AQA GCSE
Atomic structure
and periodic
table part 2
Group 0
Group 1
Rb Sr
The Periodic
table
V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr
Development
of the Periodic
table
K Ca Sc Ti
0
He
Transition metals
(Chemistry only)
This is due
to having
full outer
shells of
electrons
...
better hope – brighter future
The smallest part of an
element that can exist
Have a radius of around 0
...
Element
Contains only one type of
atom
Around 100 different elements each
one is represented by a symbol e
...
O,
Na, Br
...
Contains electrons
Electronic
shell
Max number of
electrons
1
2
Name of
Particle
Relative
Charge
Relative
Mass
Proton
+1
1
2
8
Neutron
0
1
3
8
Electron
-1
Very small
4
2
Relative electrical charges of subatomic particles
Mass
number
7
Li
3
Atomic
number
Mixtures
The sum of the protons and neutrons in the
nucleus
The number of
protons in the atom
A ball of positive charge
with negative electrons
embedded in it
JJ Thompson ‘s experiments
showed that showed that an atom
must contain small negative
charges (discovery of electrons)
...
Electrons
orbit the nucleus at
specific distances
Niels Bohr proposed that electrons
orbited in fixed shells; this was
supported by experimental
observations
...
Example
Filtration
Separating an insoluble solid
from a liquid
To get sand from a mixture of
sand, salt and water
...
Simple distillation
To separate a solvent from a
solution
To get pure water from salt water
...
Separating substances that move
at different rates through a
medium
+
-
-
Chemical
equations
Description
To separate out the dyes in food
colouring
...
Rutherford's scattering
experiment
Central nucleus
Pre 1900
Tiny solid spheres that
could not be divided
Word
equations
Symbol
equations
Relative
atomic mass
Compound
Electronic
structures
Atoms,
elements and
compounds
Atom
Isotopes
better hope – brighter future
James
Chadwick
Provided the evidence to
show the existence of neutrons within the nucleus
A beam of alpha particles are
directed at a very thin gold foil
-
-
-
+
-
Most of the alpha particles
passed right through
...
A tiny number of particles
reflected back from the
nucleus
...
Uses words to show reaction
reactants → products
magnesium + oxygen → magnesium oxide
Uses symbols to show reaction
Shows the number of atoms and
molecules in the reaction, these
need to be balanced
...
35Cl
(75%) and 37Cl (25%)
Relative abundance =
(% isotope 1 x mass isotope 1) + (% isotope
2 x mass isotope 2) ÷ 100
e
...
(25 x 37) + (75x 35) ÷ 100 = 35
...
1
nanometres and have no charge (0)
...
g
...
Two or more elements
chemically combined
Compounds can only be separated
into elements by chemical reactions
...
A ball of positive charge
with negative electrons
embedded in it
JJ Thompson ‘s experiments
showed that showed that an atom
must contain small negative
charges (discovery of electrons)
...
Electrons
orbit the nucleus at
specific distances
Niels Bohr proposed that electrons
orbited in fixed shells; this was
supported by experimental
observations
...
Most of the alpha particles
passed right through
...
A tiny number of particles
reflected back from the
nucleus
...
To separate a solid from a
solution
To obtain pure crystals of sodium
chloride from salt water
...
2Mg + O2 → 2MgO
Separating a mixture of liquids
each with different boiling points
To separate the different
compounds in crude oil
...
Law of conservation of mass states
the total mass of products = the
total mass of reactants
...
Shows the number of atoms and
molecules in the reaction, these
need to be balanced
...
g
...
5
Before the discovery of the
electron, John Dalton said the
solid sphere made up the different
elements
...
1
nanometres and have no charge (0)
...
g
...
JJ Thompson ‘s experiments
showed that showed that an atom
must contain small negative
charges (discovery of electrons)
...
-
Contains protons and neutrons
+
-
-
Relative
Charge
Relative
Mass
+1
1
2
0
1
3
-1
Very small
4
Max number of
electrons
1
7
Li
3
The number of
protons in the atom
Number of electrons =
number of protons
Two or more elements or compounds
not chemically combined together
Method
Description
The development of
the model of the atom
AQA GCSE
Atomic structure
and periodic
table part 1
Relative electrical charges of subatomic particles
-
Ernest Rutherford's alpha particle
scattering experiment showed
that the mass was concentrated at
the centre of the atom
...
Provided the evidence to
show the existence of neutrons within the nucleus
-
-
Most of the alpha particles
passed right through
...
A tiny number of particles
reflected back from the
nucleus
...
Can be separated by
physical processes
...
To get sand from a mixture of
sand, salt and water
...
Shows the number of atoms and
molecules in the reaction, these
need to be balanced
...
To separate the different
compounds in crude oil
...
Relative
atomic mass
Name of
Particle
Electronic
shell
Electronic
structures
Contains electrons
-
better hope – brighter future
35Cl
(75%) and 37Cl (25%)
Relative abundance =
(% isotope 1 x mass isotope 1) + (% isotope
2 x mass isotope 2) ÷ 100
e
...
(25 x 37) + (75x 35) ÷ 100 = 35
...
Do not conduct electricity
when solid
Ions are held in a fixed position in
the lattice and cannot move
...
Ionic bonding
Electrons are transferred so
that all atoms have a noble
gas configuration (full outer
shells)
...
Metals as conductors
Group 1 metals form +1 ions
Group 2 metals form +2 ions
Group 6 non metals form -2 ions
Group 7 non metals form -1 ions
Delocalised electrons
carry electrical charge
through the metal
...
Pure metals
can be bent
and shaped
Atoms are arranged
in layers that can
slide over each
other
...
Alloy
Ionic compounds
x x
(2, 8)
Giant
structure
(2, 8, 8)
Structure
Na+
The three
states of matter
Large amounts of energy needed to
break the bonds
...
The amount of energy needed
for a state change depends on
the strength of forces between
particles in the substance
...
Properties of
metals and alloys
Occurs in compounds formed
from metals combined with
non metals
...
This sharing of
electrons leads to strong
metallic bonds
...
Particles are atoms that
share pairs of electrons
Occurs in most non metallic
elements and in compounds of
non metals
...
Do conduct electricity
when molten or dissolved
Lattice breaks apart and the ions
are free to move
...
x
x
Cl
x x
(2, 8, 1)
(2, 8, 7)
Na+
Non metals atoms gain electrons to
become negatively charged ions
+
x
Na
Metal atoms lose electrons and
become positively charged ions
x
x
[ ][ ]
Na
x
x
x
Cl
x
x
-
The three
states of matter
Do not conduct electricity
when solid
Properties of ionic
compounds
Large amounts of energy needed to
break the bonds
...
The amount of energy needed
for a state change depends on
the strength of forces between
particles in the substance
...
Energy is transferred by
the delocalised
electrons
...
Pure metals
can be bent
and shaped
Atoms are arranged
in layers that can
slide over each
other
...
Group 1 metals form +1 ions
Group 2 metals form +2 ions
Group 6 non metals form -2 ions
Group 7 non metals form -1 ions
Metallic
bonding
Particles are atoms which
share delocalised
electrons
Melting and
freezing happen at
melting point,
boiling and
condensing happen
at boiling point
...
This sharing of
electrons leads to strong
metallic bonds
...
Occurs in most non metallic
elements and in compounds of
non metals
...
Lattice breaks apart and the ions
are free to move
...
Atoms are arranged
in layers that can
slide over each
other
...
Metallic
bonding
Non metals atoms gain electrons to
become negatively charged ions
Energy is transferred by
the delocalised
electrons
...
Chemical
bonds
Large amounts of energy needed to
break the bonds
...
The three
states of matter
Occurs in metallic elements
and alloys
...
This sharing of
electrons leads to strong
metallic bonds
...
Larger molecules
Intermolecular
have higher
forces increase with
melting and
the size of the
boiling points
...
Excellent
conductor
...
Very strong
...
Buckminsterfullerene,
C60
First fullerene to be
discovered
...
Can also
have rings of five
(pentagonal) or
seven
(heptagonal)
carbon atoms
...
000 000 001m or a
billionth of a metre)
...
Nanoparticles may be toxic to
people
...
Rigid structure
...
Strong covalent bonds
...
No delocalised electrons
...
Dot and cross :
+ Show which atom the
electrons in the bonds come
from
- All electrons are identical
Atoms share pairs of electrons
Usually gases or liquids
Graphene
Fullerenes
Single layer of
graphite one
atom thick
Do not conduct
electricity
...
Properties of small molecules
Low melting and
boiling points
...
Covalent
bonding
Solids at
room
temperature
Nanoparticles
Very large
molecules
Each carbon
atom is bonded
to four others
Very hard
...
g
...
5°
Can be giant
covalent
structures
e
...
polymers
Graphite
Very conductive
...
High tensile strength
...
Large surface area to
volume ratio
...
Each carbon atom is
bonded to three
others forming
layers of hexagonal
rings with no
covalent bonds
between the layers
better hope – brighter future
Slippery
...
Very high melting
point
...
Does conduct
electricity
...
Due to them
molecules not
having an overall
electrical charge
...
molecules
...
Contains
delocalised
electrons
...
Contains
strong
covalent
bonds
...
Very thin and
long
cylindrical
fullerenes
Graphene and
fullerenes
Single layer of
graphite one
atom thick
Do not conduct
electricity
...
Can also
have rings of five
(pentagonal) or
seven
(heptagonal)
carbon atoms
...
Very high melting point
...
Does not conduct
electricity
...
Very high melting
points
1 nanometre (1 nm)
= 1 x 10-9 metres
(0
...
Can be small
molecules
e
...
ammonia
Nanoparticles may be toxic to
people
...
2D with bonds:
+ Show which atoms are bonded
together
- It shows the H-C-H bond
incorrectly at 90°
3D ball and stick model:
+ Attempts to show the H-C-H
bond angle is 109
...
Lots of energy needed to break
strong, covalent bonds
...
Properties of small molecules
Low melting and
boiling points
...
Nanoparticles
Solids at
room
temperature
Very hard
...
g
...
Used in electronics
industry
...
Reinforcing
composite materials
...
Catalysts and
lubricants
...
Strong covalent bonds
...
Larger molecules
Intermolecular
have higher
forces increase with
melting and
the size of the
boiling points
...
Contains
delocalised
electrons
...
Contains
strong
covalent
bonds
...
AQA
BONDING, STRUCTURE
AND THE PROPERTIES
OF MATTER 2
Size of particles and their
properties (Chemistry only)
Covalent
bonding
Due to them
molecules not
having an overall
electrical charge
...
Due to having weak
intermolecular
forces that easily
broken
...
Giant covalent
structures
Solids at
room
temperature
1 nanometre (1 nm)
= 1 x 10-9 metres
(0
...
Use of nanoparticles
Hexagonal rings
of carbon atoms
with hollow
shapes
...
Very hard
...
Very high melting point
...
Does not conduct
electricity
...
Lots of energy needed to break
strong, covalent bonds
...
5°
Nanoparticles may be toxic to
people
...
Graphite
Layers can slide over each
other
...
Used in electronics
industry
...
Reinforcing
composite materials
...
Large surface area to
volume ratio
...
Delocalised electrons
between layers
...
Graphite
better hope – brighter future
The sum of the Mr of the
reactants in the quantities
shown equals the sum of
the Mr of the products in
the quantities shown
...
Normal script numbers show the number of
molecules
...
Number of moles = mass (g) or mass (g)
Ar
Mr
One mole of H2O = 18g (1 + 1 + 16)
One mole of Mg = 24g
6
...
02 x 1023 molecules
One mole of NaCl will contain 6
...
7g of sulfuric acid (H2SO4)?
Give your answer to 1 significant figure
...
7 = 0
...
Conservation of mass
and balanced symbol
equations
Represent
chemical
reactions and
have the same
number of
atoms of each
element on both
sides of the
equation
Chemical measurements
Mass appears to
decrease during a
reaction
Limiting reactants
(HT only)
Magnesium + oxygen → magnesium oxide
Relative formula
mass (Mr)
One of the reactants
is a gas
No atoms are lost or
made during a
chemical reaction
Less moles of product
are made
...
Mean value is 46
...
Range of results is 44s to 49s = 5s
3
...
5s ±2
...
Calculate the mean
2
...
Estimate of
uncertainty in mean
would be half the
range
Conc
...
volume (dm3)
The balancing numbers in a
symbol equation can be
calculated from the masses of
reactants and products
HT only
Greater mass = higher
concentration
...
Convert the masses in grams to
amounts in moles and convert
the number of moles to simple
whole number ratios
...
5) so mass of 1 mole of
HCl = 36
...
5 moles
Balanced symbol equation tells us that
for every one mole of Mg, you need
two moles of HCl to react with it
...
5x2 = 5 moles of HCl
You will need 5 x 36
...
5g
The sum of the Mr of the
reactants in the quantities
shown equals the sum of
the Mr of the products in
the quantities shown
...
Subscript
Normal script
Subscript numbers show the number of
atoms of the element to its left
...
Mass of one mole of a substance in grams
= relative formula mass
One mole of any substance will
contain the same number of particles,
atoms, molecules or ions
...
= mass (g)
...
02 x 1023 molecules
One mole of NaCl will contain 6
...
7g of sulfuric acid (H2SO4)?
Give your answer to 1 significant figure
...
Greater volume = lower
concentration
...
If you have a 60g of Mg, what mass of
HCl do you need to convert it to MgCl2?
One mole of Mg = 24g
6
...
Calculate the mean
2
...
Estimate of
uncertainty in mean
would be half the
range
Example:
1
...
5s
2
...
Time taken was 46
...
5s
Concentration of
solutions
One mole of H2O = 18g (1 + 1 + 16)
4
...
05 mol
98
Less moles of product
are made
...
5) so mass of 1 mole of
HCl = 36
...
5 moles
Balanced symbol equation tells us that
for every one mole of Mg, you need
two moles of HCl to react with it
...
5x2 = 5 moles of HCl
You will need 5 x 36
...
5g
(Mr of H2SO4)
better hope – brighter future
The sum of the Mr of the
reactants in the quantities
shown equals the sum of
the Mr of the products in
the quantities shown
...
48g + 32g = 80g
80g = 80g
Mass changes when a reactant or product is a gas
AQA GCSE
QUANTITATIVE CHEMISTRY 1
Subscript numbers show the number of
atoms of the element to its left
...
Amounts of
substances in
equations (HT only)
Normal script
Moles (HT only)
Conservation of mass
and balanced symbol
equations
H2 + Cl2 → 2HCl
Concentration of
solutions
1
...
3
...
If you have a 60g of Mg, what mass of
HCl do you need to convert it to MgCl2?
One mole of H2O = 18g (1 + 1 + 16)
One mole of Mg = 24g
6
...
02 x 1023 molecules
One mole of NaCl will contain 6
...
7g of sulfuric acid (H2SO4)?
Give your answer to 1 significant figure
...
7 = 0
...
5s
of results is 44s to 49s = 5s
was 46
...
5s
Conc
...
volume (dm3)
Using moles to
balance equations
(HT only)
Mass of the products equals
the mass of the reactants
...
Calculate the mean
2
...
Estimate of
uncertainty in mean
would be half the
range
Mg + 2HCl → MgCl2 + H2
One mole of magnesium reacts
with two moles of hydrochloric
acid to make one mole of
magnesium chloride and one
mole of hydrogen
Ar : Mg =24 so mass of 1 mole of Mg =
24g
Mr : HCl (1 + 35
...
5g
So 60g of Mg is 60/24 =
Balanced symbol equation tells us that
for every one mole of Mg, you need
two moles of HCl to react with it
...
5g
2Mg + O2 → 2MgO
48g + 32g = 80g
80g = 80g
...
Chemical measurements
Calcium carbonate →
Limiting reactants
(HT only)
...
2
...
Concentration of
solutions
AQA GCSE
QUANTITATIVE CHEMISTRY 1
1
...
3
...
5s
of results is 44s to 49s = 5s
was 46
...
5s
HT
Amounts of
substances in
equations (HT only)
Normal script
Moles (HT only)
Subscript
Conservation of mass
and balanced symbol
equations
H2 + Cl2 → 2HCl
Using moles to
balance equations
(HT only)
Equation
Convert the masses in grams to
amounts in moles and convert
the number of moles to simple
whole number ratios
...
02 x 1023 per mole
Mg + 2HCl → MgCl2 + H2
One mole of magnesium reacts
with two moles of hydrochloric
acid to make one mole of
magnesium chloride and one
mole of hydrogen
One mole of H2O will contain
One mole of NaCl will contain
How many moles of sulfuric acid molecules are there in
4
...
better hope – brighter future