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Compare the expected values for first, second, and third ionization energies of Mg.
B) MgCl2 a stable complex and MgCl has never been observed. Considering part a, explain why
MgCl2 is preferred. Hint: think about the source of stability for ionic compounds.
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- Describe any patterns observed in ΔH for the chloride salts. Is there a periodic trend in DH for the Group I chloride salts? Describe the trend.What is the trend observed what is the trend observed for ions energy going down a group? Explain why this trend occursOnly typed explanation of both subparts otherwise leave it
- For the structure of ZnS as shown on image: Please identify the nearest neighbors to one Zn ion; what are the nextneighbors to that Zn ion.Compare the energetic favorability of Fe2+, Cu2+, and Zn2+ to their metallic states by H2.In which compound does Cr exhibit greater metallic behav-ior, CrF₂ or CrF₆? Explain
- (a) The ionization energy of potassium (K) is 4.34 eV and the electron affinity of chlorine (Cl) is -3.61 eV. The Madelung constant for the KCl structure is 1.748 and the distance between ions of opposite sign is 0.314 nm. On the basis of these data only, compute the cohesive energy of KCl per ion pair. (b) The observed cohesive energy of KCl is 6.42 eV per ion pair. On theassumption that the difference between this figure and that obtained in (a) is due to the exclusion principle repulsion, find the exponent n in the formula Br^-n for the potential energy arising from this source.Identify the stable e-configurations in the formation of the following ions: K+, Mg2+, S2-, Zn2+, Pb2+, Pb4+, Mn2+, Fe3+ by writing the ionization processe.The dipole moment of gaseous Ag – Cl is ? = 6.08 D, and the bond distance is r(Ag − Cl) = 228. 1 pm. Calculate the percent ionic character for this bond in the gas phase. In solid form it is however, found the following values for the two silver halides Ag − CL and Ag − F: See image Explain why solid silver chloride is sparingly soluble in water, while solid silver fluoride is moderately soluble B) Explain why solid silver chloride is sparingly soluble in water, while solid silver fluoride is moderately soluble Given extra information: Formal charge: ?? = ??? – (??? + ???); where ??? = valence electrons in free atom, ???= free-pair electrons, ??? = number of bonds to the atom. The elementary charge: ? = 1.6022 × 10−19 C.1 Debye (?)= 3.3356 × 10−30 C × m. The dipole moment has definition: ? = ? × ?, where ? is partialcharge in Coulomb (?), ? is the bond distance (?). Picometer: 1 ?? = 1 × 10−12
- Which is the strongest reductant: Al, Cu, I-, Al3+, Cu2+, or I2? Explain.How Explain the trends /patterns IN REACTIVITY with reference to the ELECTRONIC arrangement of the elements ?Draw a Lewis structure of the thiocyanate ion that contains a triple carbon-nitrogen bond. When thiocyanate binds to a metal through the sulfur atom, studies show that the M-S-C bond angle is approximately 108-109 degrees, but when it binds through the nitrogen atom, the M-N-C bond angle is 180 degrees. On the basis of your Lewis structure for SCN-, briefly rationalize this diffrence.