Fluorine atoms have a higher electron affinity than Oxygen atoms, but O ions hav

Question

Fluorine atoms have a higher electron affinity than Oxygen atoms, but O ions have no electron affinity even though they have the same number of electrons as F atoms. What's up with that?"(degree, degree)" squareroot In your answer, provide the electron configuration of each atom/ion. b) Which is higher: the third ionization energy of Li, or the energy required to eject a is electron from a Li atom in a photoelectron spectroscopy experiment? Briefly explain your reasoning. c) A phosphorous atom is introduced to a light source and electrons are emitted. The emitted electrons with the lowest kinetic energy came from which orbital (circle one): 3p 3s 2p 2s Is d) For your answer in part c), why do these electrons have the lowest kinetic energy {circle one)? a. A half-filled shell is broken, and half-filled shells are unusually stable. b. The electrons nearest the nucleus have the lowest kinetic energy. c. Electron-electron repulsion is greatest in this orbital. d. The ionization energy is high for this orbital.

Explanation / Answer

9.

A) Anion is negative so it is difficult to add electron.

B) third ionisation energy

C) 1s

D) answer:- d

Due to higher ionisation energy

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