The electron affinities of five elements are given below. Which statement best e

Question

The electron affinities of five elements are given below. Which statement best explains why the electron affinity at phosphorus does not follow the general trend. _13Al 12 kcal/mole _14Si 32 kcal/mole _15P 17 kcal/mole _16S 48 kcal/mole _17Cl 87 kcal/mole a. The 4^th p electron in sulfur is spin paired b. The valence orbitals in silicon exists at higher energy than the valence orbitals in phosphorus. c. The valence electrons in phosphorus are held less tightly by the nucleus than the valence electrons in silicon. d. Gaining an electron in phosphorus will increase electron-electron repulsions in half-filled orbitals. e. None of the above provides an adequate explanation for the discontinuity that is observed at phosphorus.

Explanation / Answer

Option D is the correct answer

Explanation: When an atom gains an electron, it releases the energy which is known as the electron affinity. The configuration of Phosphorus is - 1s2 2s2 2p6 3s2 3p3 , where 3p orbital is half filled, and the half filled orbitals and full orbitals are more stable than partially filled orbitals. When adding an electron on phosphorus- that electron is pair up with the originally unpaired electron - which will cause forcing of electron -electron repulsion which would make it unstable. Thus the larger the electron affinity, easier it is for an electron to be added.

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.