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chemistry: atomic structure
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Cards (36)
Chromatography
To
separate
out
mixtures
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Evaporation
To separate a
soluble salt
from a solution; a
quick
way of separating out the salt
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Filtration
To separate
solids
from
liquids
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Crystallisation
To separate a
soluble salt
from a solution; a
slower
method of separating out salt
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Distillation
To
separate
out mixtures of
liquids
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Simple distillation
Separating a
liquid
from a
solution
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Fractional distillation
Separating out a mixture of liquids. Fractional distillation can be used to
separate
out crude oil into
fractions
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Atoms
Contained in the nucleus are the
protons
and
neutrons
Moving around the nucleus are the
electron
shells
They are
negatively
charged
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Overall, atoms have
no
charge; they have the same number of
protons
as electrons
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Ion
A
charged
particle - it does not have an equal number of
protons
to electrons
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Atomic
Number
The number of
protons
in the
nucleus
of an atom
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Mass
Number
The total number of
protons
and
neutrons
in the nucleus of an atom
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To calculate the relative atomic mass
Equation:
relative atomic mass
(
Ar
) = sum of (isotope abundance × isotope mass number) / sum of abundances of all isotopes
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Balancing Symbol Equations
There must be the
same
number of
atoms
on both sides of the equation
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Balanced equation
CH4 + 2O2 ->
2H2O
+
CO2
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Elements
Made of
atoms
with the
same
atomic number
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Isotopes
Elements with the same number of
protons
but different numbers of
neutrons
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Compounds
When two or more elements are chemically joined, held together by
chemical bonds
and
difficult
to separate
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Compound formulas
CO2
NaCl
HCl
H2O
Na2SO4
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Chemical Reaction
Can be shown by a
word
equation or a
symbol
equation
Reactants on the
left
, products on the
right
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Equations need to be
balanced
, so the same number of
atoms
are on each side
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To balance equations,
numbers
are put in
front
of the compounds
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Metals
Strong,
malleable
, good conductors of electricity and
heat
, bond metallically
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Non-Metals
Dull,
brittle
, not always
solids
at room temperature
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Metals
are found at the
left
part of the periodic table, non-metals are at the right
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Alkali
Metals
Group 1 elements,
soft
, very reactive metals with one
electron
in their outer shell
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Alkali metal reactions
1. Reaction with
water
to produce
hydrogen
2. Reaction with
chlorine
to produce a
metal salt
3. Reaction with
oxygen
to form
metal oxides
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Halogens
Group
7 non-metal
elements (fluorine, chlorine, bromine, iodine) that become
less
reactive going down the group
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Noble Gases
Group
0
elements (helium, neon, argon) that are
unreactive
due to full outer shells
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Electronic Structure
Electrons are found in shells, with a maximum of
2
in the innermost shell, then
8
in the 2nd and 3rd shells
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The inner shell is filled first, then the
2nd
then the
3rd
shell
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History of the Atom
John Dalton
- atoms described as
solid spheres
JJ Thomson
-
plum pudding
model
Ernest Rutherford
-
alpha scattering
experiment
Niels Bohr
- electrons in
shells
orbiting nucleus
James Chadwick
- discovered
neutrons
in nucleus
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The periodic table was not complete in the early
1800s
as some
elements
had not been found
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Mendeleev
left gaps in the periodic table, believing there were
undiscovered
elements which were later found to fit the pattern
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Modern Periodic Table
Elements in order of
atomic mass
/
proton number
Shows where
metals
and
non-metals
are
Columns
are groups, showing number of
outer shell electrons
Rows
are periods, showing
full electron shells
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The
periodic table
can be used to predict the
reactivity
of elements
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