The atomic structure diagram shown opposite should be familiar to you. The model of the atom shown is often called the nuclear atom or the Bohr atom and it is based on the work of Ernest Rutherford who discovered the nucleus in his famous gold foil experiment and on the work of Niels Bohr who suggested that the electrons orbit the nucleus in circular orbits or shells.
Atoms have no charge, they are neutral. Atoms
contain positively charged protons in their nucleus and
negatively charged electron in the electron shells or rings. The number
of positively charged protons and
negatively charged electrons is always the same in an atom,
so atoms are always neutral and have no charge.
The atomic number of an element
will tell you the number of protons present in the nucleus; it will also
tell you the number of electrons
present in the electron shells.
Common elements
The table below gives some examples of the number of protons and electrons in atoms using elements that you are likely to meet in your school work in chemistry:
atom
atomic number
number of positively charged protons
number of negatively charged electrons
overall charge
Lithium (Li)
3
3
3
0
Sodium (Na)
11
11
11
0
Magnesium (Mg)
12
12
12
0
Oxygen (O)
8
8
8
0
Chlorine (Cl)
17
17
17
0
Ion formation- cations and anions
However when different elements react with each other it may no longer be true
that the number of proton and electrons
will be the same. For example
when metals react with non-metal elements
they lose electrons. This means that they will have more positively charged protons than negatively charged
electrons; so the atom will have a
positive charge. We call charged atoms ions. Positively chargedions are often called cations.
Just as metals lose electrons
when they react non-metals gain electrons when they react with metals.
This means that the non-metal will have more
negatively charged electrons than positively charged protons.
So the non-metal atoms will form ions with a negative charge. Negatively charged ions are often called anions.
The Octet rule
To work out the number of electrons lost by a metalatom when it reacts or the number of electrons
gained by a non-metal atom when it reacts;
let's start with elements that do not react; the noble gases in group 0 of the periodic table.
The noble gases in group 0 are helium (He), neon (Ne), argon (Ar),
krypton (Kr), xenon (Xe) and radon (Rn). These gases are almost totally inert
and will only react under the most severe conditions and only with a few
very reactive elements such as fluorine. So why are
the noble gases so unreactive?
Well if you
work out the electron arrangement for all the noble gases
you will quickly realise that they all
consist of atoms with full outer electron
shells. It is these full electron shells which give the noble gases
their chemical stability and it is these full outer electron
shells which makes them almost totally unreactive. This leads to a rule in chemistry which is very helpful in
determining how elements react; the octet rule. The
octet rule simply states that elements will only react if they can
achieve full outer electron shells - similar to those
found in the noble gases.
Valency electrons and the periodic table
You may recall that it is possible to work out the number of electrons an
element has in its last electron shell simply by
finding the element in the periodic table.
The group in which an element is found in the
periodic table tells you the number of electrons in the last shell, so
for
example the alkali metals in group 1 of the periodic table
have 1 electron in their last shell, the
alkaline earth metals in group 2 of the periodic table have 2 electrons in
their last shell, the halogens in group 7 have 7 electrons in their last shell. This is outlined in the table below:
The metals are found in the left-hand side of the periodic table in groups 1, 2 and 3. We will for the moment ignore the transition
metals in the middle block in the periodic table. The table below gives the electron arrangement
for several different metals. If you study the table carefully
you will notice that the charge on the
metal ion formed is the same as the number of electrons
in the last shell of the metal or the group in
which the metal is found in the periodic table.
metal
atomic number
Group where the element is found in the periodic table
electron arrangement
number of electrons in last shell
number of electrons lost to obtain a full last shell
charge on ion
Sodium (Na)
11
1
2,8,1
1
1
+1
potassium (K)
19
1
2,8,8,1
1
1
+1
magnesium (Mg)
12
2
2,8,2
2
2
+2
aluminium (Al)
13
3
2,8,3
3
3
+3
Cation formation
The pattern found in the table above is fairly obvious:
group 1 metal lose 1 electron and form an ion
with a +1 charge
group 2 metals lose 2 electron and form an ion with a +2 charge
group 3 metals lose 3 electron and form an ion with a +3 charge
As an example consider the alkali metal potassium; symbol K. Its atomic number
is 19; so it contains 19 protons in its nucleus and 19 electrons
in its
electron shells. The electron arrangement is 2,8,8,1. When potassium metal
reacts with say a non-metal element it can achieve a full last shell in 2 ways:
It can gain 7 electrons to fill the last shell
or
It can lose its outer shell electron.
As you may expect it requires much less energy to simply lose one electron
than to gain 7. So it loses its outer shell electron and ends up
forming an ion, with only 18 electrons.
Its new electron arrangement will be 2,8,8 the same as the noble gas argon.
This is outlined in the
image below:
Non-metal ions- forming anions
The non-metals are found in the right-hand side of the periodic table. The non-metals in groups 5, 6 and 7 are the ones which will
form ions.
The non-metalelements in group 4 tend to share electrons when they form compounds and
will form covalent bonds, this means that they
do not tend to form compounds containing ions. So we are really only interested in the non-metalselements in
groups 5, 6 and 7. These
non-metalelements when they react with metals
will gain electrons from the metal atoms and
form ions with a negative charge, we call these negatively charged ions anions.
Like the metals these non-metalelements will
only react if they can achieve full last shells.
As an example consider the element chlorine. Chlorine has an atomic number
of 17; this means it has 17 protons in its nucleus and 17 electrons
in its shells. Chlorine's electron arrangement will be 2,8,7. To fill its
last shell it needs to gain 1 electron. It could get this one
electron by
reacting with an alkali metal such as potassium. When it gains
1 electron the chlorine atom will
form a chloride ion. It will have a -1 charge
since
it has 1 more electron than proton. This is shown below:
So the number of electrons gained by the non-metal atom will depend on the group the
non-metal is found in. The number of electrons gained will simply be the
number required for the element to end up with
full outer shells, this is shown below:
non-metal
atomic number
Group where the element is found in the periodic table
electron arrangement
number of electrons in last shell
number of electrons gained to obtain a full last shell
charge on ion
nitrogen(N)
7
5
2,5
5
3
-3
phosphorus (P)
15
5
2,8,5
5
3
-3
oxygen (O)
8
6
2,6
6
2
2-
fluorine (F)
9
7
2,7
7
1
1-
An outline of the periodic table shown below summarises the
charge formed on the ion formed by any
element in that particular group.
Remember that:
Metals always form positively chargedions by losing electrons.
Non-metal elements will form negatively charged ions by gaining electrons.
Transition metals in the central block of the periodic table do not follow the rules for other metals. They can form ions with variable charges depending on the reaction and the reaction conditions. You will learn more about the chemistry of these metals when you study A-level chemistry.
Atoms to ions self-check
Test your understanding of how ions are formed by completing the exercise below. The words in the yellow boxes below appear in the drop down menus in the paragraph below, simply select the correct word from the drop down menu.
Atoms are have no charge because they contain __________ numbers of positively charged
__________ and negatively charged
__________. However when metal atoms react with non-metals they __________ electrons to form positively charged ions called __________ while non-metal atoms gain electrons and form
__________ charged ions called __________. Atoms only react if they end up with __________ outer electrons shells, this is often called the __________ rule.
Key Points
Ions are charged particles.
Metals lose electrons to form ions with positive charges. These ions are called cations.
Non-metal elements form negatively charged ions by gaining electrons. These negatively charged ions are called anions.
The number of electrons lost or gained by an element when it reacts is related to its position in the periodic table; for example group 1 metals will lose 1 electron when they react with non-metals and form ions with a 1+ charge while group 5 non-metalelements will gain 3 electrons to form an ion with a 3- charge.
The octet rule states that elements will only react if they can achieve full outer electron shells. For metals this means that they will lose electrons and non-metals will gain electrons when they react.