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Metallic Bonding -Chemistry
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States of matter
Metallic Bonding -Chemistry
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Ionic Bonding -Chemistry
Metallic Bonding -Chemistry
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Covalent Bonding -Chemistry
Metallic Bonding -Chemistry
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Cards (44)
Properties of metals
They conduct
heat
: let's
heat
flow through them easily
They conduct
electricity
: let's
electricity
flow through them easily
They have
high
melting points
They are strong and
tough
but
bendable
They will
shine
when freshly cut or scratched
They have
higher
densities than non metals
Alloy
A
mixture
of a
metal
plus other
metals
or
non metals
, eg
carbon
Pure metals are too
soft
for many uses, so they can be made
harder
by adding another
element
to the pure metal forming an
alloy
Metals are
good
conductors of
heat
and electricity
Because they have free
delocalised electrons
that are free to
move
throughout the structure
Metals have
high
melting points
Because a lot of
energy
is needed to overcome the
attraction
between metal ions and delocalised electrons
Elements
All of the
atoms
are the
same
Compounds
Contain
two
or more different elements chemically combined in
fixed
proportions
Mixtures
Different
elements
or
compounds
, but they are not chemically combined
Filtration
Used to separate a
soluble
solid from a
liquid
Crystallisation
1. Used to separate a
soluble
solid from a
liquid
2. Can happen
faster
for the water to evaporate by gently
heating
the solution
Simple distillation
Used to separate a
soluble
solid from a liquid, but you save the
water
Fractional distillation
Used to separate
two
or more liquids with
different
boiling points
Paper chromatography
Used to separate
dissolved substances
from another based on their different
solubilities
, e.g. ink and food colouring
Plum pudding model
An atom is a ball of
positive
charge with
negative
electrons embedded in it
Alpha scattering experiment
1. Scientists fired tiny, positive
alpha
particles at a piece of
gold foil
2. Some particles
deflected
(changed direction) as they passed through
3. Some bounced back
4. This tells us the centre of the atom must have a
positive
charge as some atoms were
deflected
John Newlands
Arranged elements in increasing
atomic weight
, invented "
Law of Octaves
"
Dmitri Mendeleev
Arranged elements in increasing
atomic weight
, switched some elements so they would fit into the
same group
with similar patterns
Left gaps in areas he thought an element was missing, predicted the
properties
of undiscovered elements with elements in the
same group
Atomic mass number
The centre part of the atom is the
nucleus
Electrons have a
negative
charge (-1)
Protons have a
positive
charge (+1)
Neutrons have a
neutral
charge (0)
Isotopes
Atoms of the same element with a different amount of
neutrons
, but the same amount of
protons
Ions
Atoms that have an overall charge, because they have
lost
or
gained
electrons
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