1. Find the electron configuration and ground state term symbol for a) Cu; b) Ni2+; c) Al3+; d) Ce+. Use the rare gas notation for closed shells.
2. Write the Lewis dot structure showing the formal charges, predict the structure including an estimate of all bond angles, and indicate the likely hybrid orbital on the central atom for the following: a) SO3; b) XeO44–; c) IF3.
3. Several of the highest occupied molecular orbitals for Cr2 are shown below. Label the type of orbital and explain how you reached that conclusion. Predict the energy ordering of these orbitals and explain your reasoning.
4. The Pauling electronegativity for Xe is estimated to be 2.60, about the same as S, which has χ = 2.58. Based on this, make a predictive comparison of the chemical reactivity of the two elements. Explain your reasoning. Possible useful information: IP1(S) = 10.360 eV; IP1(Xe) = 12.130 eV.