3.4 Ionisation energy and the periodic table  (Page 3/4)

The characteristics of each group are mostly determined by the electron configuration of the atoms of the element.

• Group 1: These elements are known as the alkali metals and they are very reactive.

  

• Group 2: These elements are known as the alkali earth metals . Each element only has two valence electrons and so in chemical reactions, the group 2 elements tend to lose these electrons so that the energy shells are complete. These elements are less reactive than those in group 1 because it is more difficult to lose two electrons than it is to lose one.
• Group 3 elements have three valence electrons.
  The number of valence electrons of an element corresponds to its group number on the periodic table.
• Group 7: These elements are known as the halogens . Each element is missing just one electron from its outer energy shell. These elements tend to gain electrons to fill this shell, rather than losing them. These elements are also very reactive.
• Group 8: These elements are the noble gases . All of the energy shells of the halogens are full and so these elements are very unreactive.

  

• Transition metals: The differences between groups in the transition metals are not usually dramatic.

Investigation : the properties of elements

Refer to [link] .

1. Use a periodic table to help you to complete the last two diagrams for sodium (Na) and potassium (K).
2. What do you notice about the number of electrons in the valence energy level in each case?
3. Explain why elements from group 1 are more reactive than elements from group 2 on the periodic table (Hint: Think back to 'ionisation energy').

It is worth noting that in each of the groups described above, the atomic diameter of the elements increases as you move down the group. This is because, while the number of valence electrons is the same in each element, the number of core electrons increases as one moves down the group.

Periods in the periodic table

A period is a horizontal row in the periodic table of the elements. Some of the trends that can be observed within a period are highlighted below:

• As you move from one group to the next within a period, the number of valence electrons increases by one each time.
• Within a single period, all the valence electrons occur in the same energy shell. If the period increases, so does the energy shell in which the valence electrons occur.
• In general, the diameter of atoms decreases as one moves from left to right across a period. Consider the attractive force between the positively charged nucleus and the negatively charged electrons in an atom. As you move across a period, the number of protons in each atom increases. The number of electrons also increases, but these electrons will still be in the same energy shell. As the number of protons increases, the force of attraction between the nucleus and the electrons will increase and the atomic diameter will decrease.
• Ionisation energy increases as one moves from left to right across a period. As the valence electron shell moves closer to being full, it becomes more difficult to remove electrons. The opposite is true when you move down a group in the table because more energy shells are being added. The electrons that are closer to the nucleus 'shield' the outer electrons from the attractive force of the positive nucleus. Because these electrons are not being held to the nucleus as strongly, it is easier for them to be removed and the ionisation energy decreases.
• In general, the reactivity of the elements decreases from left to right across a period.