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Chemsitry
Inorganic Chemistry
Group 2
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Ashling Asirifi
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Cards (29)
Atomic radius
Increases
down the group
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Atomic radius
Atoms have
more
shells of electrons making the atom
bigger
as you go down the group
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1st Ionisation Energy
The
outermost
electrons are held more
weakly
because they are successively further from the nucleus in additional shells
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1st Ionisation Energy
The outer shell electrons become more
shielded
from the attraction of the
nucleus
by the repulsive force of inner shell electrons
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Melting points of Group 2 metals
Decrease
down the group
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Melting points of Group 2
metals
The metallic bonding
weakens
as the atomic size
increases.
The distance between the positive ions and delocalized electrons increases. Therefore the electrostatic attractive forces between the positive ions and the delocalized electrons weaken
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Reactivity of Group 2 metals
Increases
down the group
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Reaction of Mg with oxygen
1. Mg
burns
with a bright
white
flame
2. MgO appears as a
white
powder
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Reaction of Mg with steam
1. Mg reacts to produce
magnesium oxide
and
hydrogen
2. Mg would
burn
with a bright
white
flame
3. MgO appears as a
white
powder
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Reaction of Group 2 metals with cold water
1. Increasing
vigour
down the group to form
hydroxides
2.
Fizzing
(more vigorous down group)
3. Metal
dissolving
(faster down group)
4. Solution
heating
up (more down group)
5. White
precipitate
forming (less precipitate forms down group)
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Reaction of Mg with warm water
1.
Mg
+ 2 H2O Mg(OH)2 +
H2
2.
Slower
reaction than with
steam
3. No
flame
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Titanium
Abundant
Low
density
Corrosion
resistant
Used for making
strong
, light alloys for use in
aircraft
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Extracting titanium
1.
TiO2
converted to
TiCl4
at 900C
2.
TiCl4
purified by fractional distillation in
argon
atmosphere
3. Ti extracted by
Mg
in
argon
atmosphere at 500C
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Reason titanium is expensive
Expensive cost of the
magnesium
Batch process is
slow
and requires more
labour
and energy
Need for
argon
and to remove
moisture
High
temperatures required
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Calcium oxide
can be used to remove SO2 from waste gases by
flue gas desulfurisation
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Removing SO2 from waste gases
1.
Gases
pass through a scrubber containing basic
calcium oxide
2.
Calcium oxide
reacts with
acidic sulfur dioxide
in a neutralisation reaction
3. Calcium sulfite formed can be used to make
calcium sulfate
for
plasterboard
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Group
II
sulfates
Become
less
soluble down the group, with
BaSO4
being the least soluble
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Testing for presence of sulfate ion
1.
Acidified BaCl2
solution is added
2. White precipitate of
BaSO4
forms if
sulfate
ions present
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Barium sulfate
is used in medicine as a
'Barium meal'
given to patients who need x-rays of their intestines
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Barium sulfate
is safe to use because its low solubility means it is not absorbed into the
blood
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If barium metal is reacted with sulfuric acid
It will only react
slowly
, as the
insoluble barium sulfate
produced will cover the surface of the metal and act as a barrier to further attack
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Group
II hydroxides
Become more
soluble
down the group
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Calcium hydroxide
Partially soluble
in water
Appears as a
white precipitate
Used in
agriculture
to
neutralise acidic soils
Aqueous solution (
limewater
) can be used to test for
carbon dioxide
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Barium hydroxide
Easily
dissolves
in
water
Makes the solution strongly
alkaline
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Magnesium hydroxide
Insoluble
in water
Slightly
alkaline
suspension in water (
pH 9
)
Used in medicine to
neutralise
excess acid in the stomach and treat
constipation
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Making insoluble salts by precipitation
1. Mix appropriate
solutions
of ions so that a
precipitate
is formed
2. Precipitate is removed by
filtration
,
washed
and dried
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Ionic equations for precipitation
reactions
Show only the ions that are reacting and leave out
spectator
ions
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Common rules for
solubility
of
salts
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Filtration
Gravitational
filtration used for
small
amounts of solid
Vacuum
filtration used for
larger
amounts of solid
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