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A ion hg 2 xe4f 14 5d 10 or xe 6s 2 4f 14 5d 8 b cl

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a) ion Hg2+?[Xe]4f145d10or [Xe] 6s24f145d8b) Cl[Ne]3s23p5Or you can give me the full (withoutnoble gas shorthand notation)c) W (element 74)[Xe]6s24f145d4Or you can give me the full (withoutnoble gas shorthand notation)
5. Which of the following electron configurations correspond to an excited state?i) Identify the atoms and write the ground-state electron configuration where appropriate.ii) How many unpaired electrons are present in each of these species (indicate forboththe ground state and excited state, as applicable)?
CHM 111
6. In each of the following sets, circle the atom or ion has thesmallestradius?
7. In each of the following sets, circle the atom or ion has thehighestionization energy?
8. Rank the following ionic compounds from lowest to highest values of lattice energy:a) NaF, KF, LiFLiF > NaF > KFb) NaCl, NaBr, NaINaCl > NaBr > NaIc) AlCl3, MgCl2, NaClAlCl3> MgCl2> NaCl9. Arrange the ions N3-, O2-, Mg2+, Na+, and F-in order of increasing radius, starting withthe smallest first.All have same number of electrons. Smallest will be Mg2+with most protons pullingon same number of electrons. Largest will be N3-with fewest protons pulling onsame number of electrons.
CHM 11110. Calculate the energy change (indicating +/- sign) for the formation of NaH (s) fromits elements in their standard states and the following tabulated information:Na (s) + ½ H2(g) → NaH (s)???H (g) + e-→ H-(g)-70.1 kJ/mol½ H2(g) → H (g)+217.9kJ/molNa (s) → Na (g)+107.3 kJ/molNa (g) → Na+(g) + e-+495.8 kJ/molNa+(g) + H-(g) → NaH (s)-810.9 kJ/mol-60.1 kJ/molAll steps are given in the correct direction leading to formation of the ioniccompound – as given in table in text.11. Consider the following reaction:CH4(g) + 2 O2(g) →CO2(g) + 2 H2O (g)

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