Which of the following is the correct order of ionization enthalpies of elements of 14th group?

Which of the following is the correct order of ionization enthalpies of elements of 14th group?

  1. A

    C > Si > Ge > Sn

  2. B

    C > Si > Ge > Sn < Pb

  3. C

    C < Si < Ge < Sn < Pb

  4. D

    C < Si > Ge > Sn < Pb

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    Solution:

    As we move down the group, the ionization energy decreases, due to increase in atomic size, thereby, increasing the distance of the electrons from the nucleus. The first ionization energy of lead is slightly higher than that of tin. The reason is due to lanthanide contraction. The atomic size of tin and lead are very close, and hence, the charge density is more in case of lead, due to more charge. Due to higher charge density, the outer electrons are attracted more by the nucleus in lead and hence, the ionization energy is more in the case of lead.

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