Explain the trend of the first ionization energies of these three elements.the 30th: 9.394 eVthe 48th:8.993 eVthe 80th: 10.437 eV
First of all, in periodic table the position of 30th, 48th and 80th element has to be described.
The 30th element is zinc:
(Zn)= period 4, group= 12, d-block, 1st ionization energy = 9.394 eV (given)
The 48th element is cadmium:
(Cd)= period 5, group =12, d-block, 1st ionization energy = 8.993 eV (given)
The 80th element is mercury:
(Hg)= period 6, group =12, d-block, 1st ionization energy = 10.437 eV (given)
Hence, all the three elements, Zn, Cd and Hg are in same group, in descending order form Zn> Cd> Hg.
In general, the ionization energy is explained as the amount of energy required to remove an electron from the isolated gaseous atom.
In periodic table, the first ionization energy increases along a period from left to right as the nuclear charge increases and so removal of electron becomes difficult.
While, in a group, the first ionization energy decreases from top to bottom as size of atom increases and nuclear charge decreases.
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