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Edexcel
Additional
Science
Chemistry
Topics 1+2
- The Atom
- Nucleus- in the
centre; it contains
protons and
neutrons.
- Electrons- they move
around the nucleus;
they have a negative
charge; they occupy
shells / energy levels.
The first energy
levels holds 2, every
other holds 8. A full
shell equates to 8
electrons. (the second
shell onwards)
- Electrons- they move
around the nucleus;
they have a negative
charge; they occupy
shells / energy levels.
The first energy
levels holds 2, every
other holds 8. A full
shell equates to 8
electrons. (the second
shell onwards)
- Atomic Number-
tells you the
number of protons
which is equal to
the number of
electrons.
- Mass Number- the
total number of
protons and
neutrons combined.
Mass number-
Atomic Number=
no. of neutrons
- Proton
- 1
- +1
- +1
- 1
- Neutron
- 1
- 0
- 0
- 1
- Electron
- 1/2000
- Relative
Mass
- -!
- Relative
Charge
- Relative
Charge
- Relative
Mass
- 1/2000
- Proton
- Mass Number- the
total number of
protons and
neutrons combined.
Mass number-
Atomic Number=
no. of neutrons
- Nucleus- in the
centre; it contains
protons and
neutrons.
- Isotopes
- isotopes- the different
atoms of the same
element which have the
same number of
protons but different
numbers of neutrons.
(different mass
numbers)
- e.g. isotopes include
Carbon 12/14 and
Chlorine 35/37
- Relative Atomic Mass
of Isotopes: (% of
isotope 1 × mass of
isotope 1) + (% of
isotope 2 × mass of
isotope 2) ÷ 100
- Relative Atomic Mass
of Isotopes: (% of
isotope 1 × mass of
isotope 1) + (% of
isotope 2 × mass of
isotope 2) ÷ 100
- e.g. isotopes include
Carbon 12/14 and
Chlorine 35/37
- Organ-
isation
of The
Periodic
Table
pt.1
- 1800s- scientists
didnt know about
the structure of
atoms, so ordered
them in atomic
mass
- 1800s- scientists
didnt know about
the structure of
atoms, so ordered
them in atomic
mass
- isotopes- the different
atoms of the same
element which have the
same number of
protons but different
numbers of neutrons.
(different mass
numbers)
- Organisation of the
Periodic Table pt.2
- 1869- Dmitri
Mendeleev
ordered
elements in
groups,
according to
their properties.
This left gaps;
the gaps
predicted new
elements
- Metals and non
metals are on
opposite sides of
the table; metals
-left, non metals-
right
- Periods- these run
across the periodic
table in rows; the
elements are
increasing in atomic
number. the row
number that the
element is in
corresponds to
number of energy
levels/ shells the
element has. e.g. the
elements in period 3
have 3 energy
levels/shells.
- Groups- these are
columns that run
down the periodic
table; elements in
these groups have
similar properties
because they have
the same no. of
electrons on their
outer shell. the
group no. equals the
no. of electrons on
their outer shell.
- Groups- these are
columns that run
down the periodic
table; elements in
these groups have
similar properties
because they have
the same no. of
electrons on their
outer shell. the
group no. equals the
no. of electrons on
their outer shell.
- Periods- these run
across the periodic
table in rows; the
elements are
increasing in atomic
number. the row
number that the
element is in
corresponds to
number of energy
levels/ shells the
element has. e.g. the
elements in period 3
have 3 energy
levels/shells.
- 1869- Dmitri
Mendeleev
ordered
elements in
groups,
according to
their properties.
This left gaps;
the gaps
predicted new
elements
- Ionic Bonding
- in ionic bonding electrons are
transferred to form positively or
negatively charged atoms called
ions, because of the attraction of
opposite charges + and -, the ions
are strongly attracted
- A shell with 1/2/3
electrons will be
looking forward
to lose 1 or 2. or
3 this is because
it's quicker than
trying to gain 7
or 6.
- A shell with
6,5 or 7
electrons
will be
looking to
gain 1 or 2
electrons
because it's
quicker and
easier than
losing 5/6/7.
- PROPERTIES
- ionic bonds
produce
compounds with
similar
structures; the
ions form a
closely packed
regular lattice
arrangement
- They have high
melting points,
due to the very
strong bonds
between the ions
and electrostatic
forces of
attraction; it
takes a lot of
energy to break
these bonds
- They
conduct
electricity
when
aqueous of
molten.
when
dissolved
the ions
separate
and are all
free to
move so
they'll carry
electric
current..
- They
conduct
electricity
when
aqueous of
molten.
when
dissolved
the ions
separate
and are all
free to
move so
they'll carry
electric
current..
- They have high
melting points,
due to the very
strong bonds
between the ions
and electrostatic
forces of
attraction; it
takes a lot of
energy to break
these bonds
- ionic bonds
produce
compounds with
similar
structures; the
ions form a
closely packed
regular lattice
arrangement
- PROPERTIES
- A shell with
6,5 or 7
electrons
will be
looking to
gain 1 or 2
electrons
because it's
quicker and
easier than
losing 5/6/7.
- A shell with 1/2/3
electrons will be
looking forward
to lose 1 or 2. or
3 this is because
it's quicker than
trying to gain 7
or 6.
- in ionic bonding electrons are
transferred to form positively or
negatively charged atoms called
ions, because of the attraction of
opposite charges + and -, the ions
are strongly attracted
- Dot and Cross Diagrams
- Dot and Cross diagrams show
where electrons have moved
during ionic bonding and the
charges that elements have as a
result.
- if elements
lose electrons
they gain a
positive
charge, the
number of
electrons they
lose will go
after the
charge sign.
e.g calcium
has 2
electrons on
its last energy
level, it
ionically bonds
and loses 2. so
it has a charge
of +2
- if elements
gains
electrons they
gain a
negative
charge, the
number of
electrons they
gaim will go
after the
charge sign. e.g
chlorine has 7
electrons on
its last energy
level, it
ionically bonds
and gains 1. so
it has a charge
of +1
- if elements
gains
electrons they
gain a
negative
charge, the
number of
electrons they
gaim will go
after the
charge sign. e.g
chlorine has 7
electrons on
its last energy
level, it
ionically bonds
and gains 1. so
it has a charge
of +1
- Arrows show
where the
electron
moves
- the new
electron
configurations
are drawn
with their
charges
- the new
electron
configurations
are drawn
with their
charges
- if elements
lose electrons
they gain a
positive
charge, the
number of
electrons they
lose will go
after the
charge sign.
e.g calcium
has 2
electrons on
its last energy
level, it
ionically bonds
and loses 2. so
it has a charge
of +2
- Dot and Cross diagrams show
where electrons have moved
during ionic bonding and the
charges that elements have as a
result.
- Insoluble
Salts
- All
nitrates
are
soluble
- All
chlorides
are
soluble
expect
silver
and lead
- All
sulfates
are
soluble
expect
barium,
calcium
and lead
- All
carbonates
and
hydroxides
are
INSOLUBLE
except
SODIUM,
AMMONIUM
and
POTASSIUM
- All
carbonates
and
hydroxides
are
INSOLUBLE
except
SODIUM,
AMMONIUM
and
POTASSIUM
- All
sulfates
are
soluble
expect
barium,
calcium
and lead
- All
chlorides
are
soluble
expect
silver
and lead
- All
nitrates
are
soluble
- Precipitation
Reactions
- 1. add 1
spatula of
compound to
a test tube,
fill with
distilled
water and
shake
thoroughly. do
the same
with the
other
compound
- 2. tip the 2
solutions
into a beaker
and give it a
stir to
ensure it's all
mixed
together. the
precipitate
will appear
as the 2
solutions
react.
- 3. put a folded
piece of filter
paper into a
filter funnel.
put the
funnel on a
conical flask
- 4. pour the
content of
the beaker
into the
middle of the
filter paper
- 5. swill out
the beaker
with more
distilled
water and tip
it onto the
paper
- 6. rinse the
content of
the filter
paper with
distilled
water to
make sure
all of the
soluble
product
from the
reaction has
washed
away and all
that
remains is
the
precipitate
- 7.scrape of
the
precipitate
and put it
on fresh
filter paper
and leave to
dry
- 7.scrape of
the
precipitate
and put it
on fresh
filter paper
and leave to
dry
- 6. rinse the
content of
the filter
paper with
distilled
water to
make sure
all of the
soluble
product
from the
reaction has
washed
away and all
that
remains is
the
precipitate
- 5. swill out
the beaker
with more
distilled
water and tip
it onto the
paper
- 4. pour the
content of
the beaker
into the
middle of the
filter paper
- 3. put a folded
piece of filter
paper into a
filter funnel.
put the
funnel on a
conical flask
- 2. tip the 2
solutions
into a beaker
and give it a
stir to
ensure it's all
mixed
together. the
precipitate
will appear
as the 2
solutions
react.
- how to get a
pure dry
precipiate
- 1. add 1
spatula of
compound to
a test tube,
fill with
distilled
water and
shake
thoroughly. do
the same
with the
other
compound
- Barium
Sulfate
- Barium
sulfate is
an
insoluble
salt used
in x-rays.
- normally only bones show up on x-rays,
BaSO4 is opaque so when drunk it
shows up in the gut and any problems
like blockages can be seen
- BaSO4 salts are toxic but can be safely
drunk because they're insoluble; they
wont pass into the bloodstream. it just
passes through the body.
- BaSO4 salts are toxic but can be safely
drunk because they're insoluble; they
wont pass into the bloodstream. it just
passes through the body.
- normally only bones show up on x-rays,
BaSO4 is opaque so when drunk it
shows up in the gut and any problems
like blockages can be seen
- Barium
sulfate is
an
insoluble
salt used
in x-rays.
- FLAME
TEST
- Sodium-
Yellow/ Orange
- Potassium-
Lilac
- Calcium- Red
- Copper- Blue/Green
- Copper- Blue/Green
- Calcium- Red
- Potassium-
Lilac
- 1. dip a wire loop into HCL
and rinse it off with
water to ensure it is clean
- 2. dip the wire loop into the
compound sample and put
it into the blue flame of a
bunsen burner
- this method can be used for
both solution and solid
forms of compounds. if
doing solids, dip in HCL
before to make sure the
compound sticks.
- this method can be used for
both solution and solid
forms of compounds. if
doing solids, dip in HCL
before to make sure the
compound sticks.
- 2. dip the wire loop into the
compound sample and put
it into the blue flame of a
bunsen burner
- Sodium-
Yellow/ Orange
- Testing for Ions
- Carbonates- add the suspected ions to
dilute HCL. carbonates react with acid
to make CO2. Pipe the gas created from
the reaction into a test tube full of
limewater. if carbonate ions are
present it will go cloudy because of the
CO2.
- Sulfates- to test for sulfate ions
add dilute HCL followed by a barium
chloride solution. if there are sulfate
ions a white precipitate will appear:
barium sulfate
- Chloride- to test for chloride ions add
dilute nitric acid followed by a silver
nitrate solution. if chloride ions are
present, a white precipitate will
form: silver chloride
- Chloride- to test for chloride ions add
dilute nitric acid followed by a silver
nitrate solution. if chloride ions are
present, a white precipitate will
form: silver chloride
- Sulfates- to test for sulfate ions
add dilute HCL followed by a barium
chloride solution. if there are sulfate
ions a white precipitate will appear:
barium sulfate
- Carbonates- add the suspected ions to
dilute HCL. carbonates react with acid
to make CO2. Pipe the gas created from
the reaction into a test tube full of
limewater. if carbonate ions are
present it will go cloudy because of the
CO2.
- Spectro-
scopy
- using light emitted by
elements in a heated sample
to identify elements
- using light emitted by
elements in a heated sample
to identify elements
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