0.3 The periodic table  (Page 4/5)

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A change in the number of electrons of an atom does not change the type of atom that it is. However, the charge of the atom will change. If electrons are added, then the atom will become more negative . If electrons are taken away, then the atom will become more positive . The atom that is formed in either of these cases is called an ion . Put simply, an ion is a charged atom.

Ion

An ion is a charged atom. A positively charged ion is called a cation e.g. ${\mathrm{Na}}^{+}$ , and a negatively charged ion is called an anion e.g. ${\mathrm{F}}^{-}$ . The charge on an ion depends on the number of electrons that have been lost or gained.

But how do we know how many electrons an atom will gain or lose? Remember what we said about stability? We said that all atoms are trying to get a full outer shell. For the elements on the left hand side of the periodic table the easiest way to do this is to lose electrons and for the elements on the right of the periodic table the easiest way to do this is to gain electrons. So the elements on the left of the periodic table will form cations and the elements on the right hand side of the periodic table will form anions. By doing this the elements can be in the most stable electronic configuration and so be as stable as the noble gases.

Look at the following examples. Notice the number of valence electrons in the neutral atom, the number of electrons that are lost or gained and the final charge of the ion that is formed.

Lithium

A lithium atom loses one electron to form a positive ion: In this example, the lithium atom loses an electron to form the cation ${\mathrm{Li}}^{+}$ .

Fluorine

A fluorine atom gains one electron to form a negative ion:

You should have noticed in both these examples that each element lost or gained electrons to make a full outer shell.

Investigation : the formation of ions

1. Use the diagram for lithium as a guide and draw similar diagrams to show how each of the following ions is formed:
1. ${\mathrm{Mg}}^{2+}$
2. ${\mathrm{Na}}^{+}$
3. ${\mathrm{Cl}}^{-}$
4. ${\mathrm{O}}^{2+}$
2. Do you notice anything interesting about the charge on each of these ions? Hint: Look at the number of valence electrons in the neutral atom and the charge on the final ion.

Observations:

Once you have completed the activity, you should notice that:
• In each case the number of electrons that is either gained or lost, is the same as the number of electrons that are needed for the atoms to achieve a full outer energy level.
• If you look at an energy level diagram for sodium ( $\mathrm{Na}$ ), you will see that in a neutral atom, there is only one valence electron. In order to achieve a full outer energy level, and therefore a more stable state for the atom, this electron will be lost .
• In the case of oxygen ( $\mathrm{O}$ ), there are six valence electrons. To achieve a full energy level, it makes more sense for this atom to gain two electrons. A negative ion is formed.

Exercise: the formation of ions

Match the information in column A with the information in column B by writing only the letter (A to I) next to the question number (1 to 7)

 1. A positive ion that has 3 less electrons than its neutral atom A. ${\mathrm{Mg}}^{2+}$ 2. An ion that has 1 more electron than its neutral atom B. ${\mathrm{Cl}}^{-}$ 3. The anion that is formed when bromine gains an electron C. ${\mathrm{CO}}_{3}^{2-}$ 4. The cation that is formed from a magnesium atom D. ${\mathrm{Al}}^{3+}$ 5. An example of a compound ion E. ${\mathrm{Br}}^{2-}$ 6. A positive ion with the electron configuration of argon F. ${\mathrm{K}}^{+}$ 7. A negative ion with the electron configuration of neon G. ${\mathrm{Mg}}^{+}$ H. ${\mathrm{O}}^{2-}$ I. ${\mathrm{Br}}^{-}$

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