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Which of the species NP, NP+ and NP2− would be paramagnetic? Briefly explain why (one sentence).
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- Using an MO energy-level diagram, would you expect F2 to have a lower or higher first ionization energy than atomic fluorine? Why?Write condensed electron configurations for the following: (a) Zr; (b) V3+; (c) Mo3+.1) give the electron configuration, (not condensed or orbital) for the imaginary ion Ge^-2 3) give the electron configuration, (not condensed or orbital) 7) what would the electron configuration of nickel look like if the quantum theory was the exact same as ours now except that each orbital was able to hold three electrons instead of two? What would the most stable ion of nickel look like and why would it be stable?
- Explain why N2 2+ is diamagnetic, while O2 4+, which has the same number of valence electrons, is paramagnetic.Mixing SbCl3 and GaCl3 in a 1:1 molar ratio using liquid sulfur dioxide as a solvent gives a solidionic compound with the empirical formula GaSbCl6. A controversy arose over whether this compoundis [SbCl2]+[GaCl4]− or [GaCl2]+[SbCl4]−.(a) Predict the molecular structure of the two anions from the two choices using VSEPR theory.(b) It is learned that the cation in the compound has a bent structure. Based on this fact, whichformulation is the correct one?4. Write an appropriate set of four quantum numbers (n, l, ml & ms) that could be representative of a valence electron in each of the following atoms or ions. (a) Bi (m (b) Sr (c) Mo (d) Ru2+ (e) Eu
- Iron(III) sulfate [Fe2(SO4)3] is composed of Fe3+ and SO4 2− ions. Explain why a sample of iron(III) sulfate is uncharged.1.) a.) True or false: Elements with high ionization energies tend to have lave electron affinities as well. Explain why in terms of nuclear chargeb.) The size of the transition metals decreases slightly in going from left to right across the period. Explain in terms of nuclear charge.c.) Carbon monoxide has a larger bond dissociation energy (1072 Kj/mol) than molecular nitrogen (N2, 945 Kj/mol). Suggest an explanationd.) Given that both the electronic configuration of Ca ([Ar] 4s2 and Zn ([Ar] 3d10 4s2 end with 4s2, explain the difference between the first ionization energy of Ca (IE1 = 590Kj/mol) and Zn (IE1 =906 kJ/mol) e.) In general, ionization energies increase across a period from left to right. Explain why the second ionization energy of Cr is higher, not lower, than that of Mn f.) Which of each of the following pairs of molecules has the larger bond angle? Explain your reasoning. i.) PH3 and NH3Is N2 + diamagnetic or paramagnetic?