Successive ionisation energies Question
The first eight successive ionisation energies of an element are 1310, 3390, 5320, 7450, 11000, 13300, 71300, 84100kJ/mol. Deduce which group in the Periodic Table does this element belong to? Explain your decision.
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- From the first ionisation energy to the sixth ionisation energy ( 1310, 3390, 5320, 7450, 11000, 13300) there is gradual increase showing that these electrons are in the same shell.
- Between the sixth ionisation energy and the seventh (13300 and 71300) there is a big gap showing a transition into another shell closer to the nucleus.
- Since the first six electrons are in the same shell, the element has six electrons in the outer shell. Therefore the element is in Group VI of the periodic table.