Explain why the ionization energy of S slightly lower than P when we would expec

Question

Explain why the ionization energy of S slightly lower than P when we would expect it to be higher based on the general trend d. o. Explain why there is a decrease in ionization energy form Zn to Ga. 22. Answer the questions below using plots of electron affinity for groups IA, A, and VIIA. a. Define electron affinity. b. Explain why the electron affinities for groups IIA and VIIIA are-0 kJ/mol. Explain why the magnitudes of the electron affinities for group VIIA is so high com- pared to the other groups c. d. Explain why the magnitude of the electron affinity for F is less than for Cl

Explanation / Answer

22. A) Electron affinity: It can be defined as a measure of the energy change when an electron is added to a neutral atom to form a negative ion.

b) Electron affinities for group IIA i.e., Alkali earth elements and group IIA noble gases are 0 kJ/mol because they do not form stable negative ions. Hence, an electron is not addedto these groups.

c) Group VIIA has high electron affinity compared to other groups because they have more valence electrons and their valence electron shell is closer to the nucleus. hence, they take up electrons very easily compared to other groups.

d) Magnitude for electron affinity is less for F than Cl because of its small size. The electron is being added to smaller 2p orbital of fluorine and requires more electron coupling energy than while adding to larger 3p orbital of chlorine. Hence, Cl takes up electron more easily than F.

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