Problem 1
The photoelectric effect demonstrates that radiation energy is quantized into "packets" or photons. Explain how and why this observation is of significance in under standing the structure of atoms.
Problem 2
Explain how we can know that higher fre quency light contains higher energy photons.
Problem 3
Electron affinity is the energy released when an electron is attached to an atom. If an atom has a positive electron affinity, the added electron is attracted to the nucleus to form a stable negative ion. Why doesn't a Beryllium atom have a positive electron affinity? Explain how this demonstrates that the energy of a 2 s orbital is less than the energy of a \(2 \mathrm{p}\) orbital.
Problem 4
Why does an inert gas atom have a high ionization energy but a low electron affinity? Why do these properties combine to make the atoms of inert gases unreactive?
Problem 5
Consider electrons from two different subshells in the same atom. In photoelectron spectroscopy, the lower energy electron has a higher ionization energy but is observed to have lower kinetic energy after ionization. Reconcile the lower energy with the higher ionization energy with the lower kinetic energy.
Problem 6
Chlorine atoms have 5 distinct ionization energies. Explain why. Predict the number of ionization energies for Bromine atoms, and explain your answer. (Hint: examine the structure of the periodic table.)
Problem 7
Why does a Bromine atom have a much smaller radius than a Potassium atom, even though a Br atom has 16 more electrons than does a \(\mathrm{K}\) atom?
Problem 8
Explain why electrons confined to smaller orbitals are expected to have higher kinetic energies.
Problem 9
Define "shielding" in the context of electron-electron repulsion. What is the significan oe of shielding in determining the energy of an electron? How is the affected by core penetration?
