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Yr 10 Chemistry
The Atom
Starter
 Pick the odd one out……..
PROTON
NEUTRON
ELECTRON
Objectives
 TO KNOW the meaning of terms
atomic number and atomic mass
 TO BE ABLE to draw the electron
configuration of elements
 TO UNDERSTAND how the periodic
table is arranged according to this
configuration.
Revision
The 3 sub-atomic particles all have different properties.
You need to learn these properties.
Name of
Particle
Mass
Charge
Position
Proton
1
Positive (+)
nucleus
Neutron
1
Neutral (0)
nucleus
Electron
1/1840
Negative (-)
outside
nucleus
Revision
An atom is made of 3 types of particle.
In the
nucleus
of the
atom
PROTONS
(negatively
Charged)
NEUTRONS
(no charge)
ELECTRONS
(Moving around
outside the nucleus.
Negatively charged)
Periodic Table
The elements in the Periodic table are arranged in
order of their atomic number.
Atomic Number
The Atomic Number is the number of PROTONS
in an atom.
24
Mg
It is shown in the Periodic table.
12
(always the smaller number)
Each different element has a different number of
protons in its nucleus.
Mg
24
12
Al
27
13
Si
28
14
The structure of the atom
Particle
Proton
Relative Mass
1
Relative Charge
1
Neutron
Electron
1
0
0
-1
MASS NUMBER (A) = number of
protons + number of neutrons
SYMBOL
ATOMIC NUMBER (Z) = number of
protons
For a NEUTRAL ATOM, the number of electrons = the
number of protons
Electron Shells
Electrons occupy shells around the nucleus of an atom.
Each shell can hold different numbers of electrons before
it is full.
1st shell can hold 2 electrons
2nd shell can hold 8 electrons
3rd shell can hold 8 electrons
4th shell can hold 18 electrons
The shells MUST be filled up from
the centre outwards.
The Electrons in Carbon
The Electrons in Neon
The Electrons in Silicon
Electrons in Phosphorus
The Electrons in Argon
The Electrons in Sodium
The Electrons in Fluorine
The Electrons in Aluminium
The Electrons in Nitrogen
The Electrons in Sulfur