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Lattice energies are graphed for three series of compounds in which the ion charges are
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Chemistry
- 8) Arrange affinity (less negative Na,S, and CI the following inorder of increasiing electron tomore negative).arrow_forwardin ne taist ME He Pa Example 4. Why do the transition elements exhibit higher enthalpies of atomisation? ( DA Try percet HOarrow_forwardNitrogen ions tend to have a charge of 3-; explain the reason for this pattern/trend.arrow_forward
- 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) Euarrow_forward5. Which of the following alkali metal halides has the larger lattice energy, and which has the smaller lattice energy? Explain. (a) (b)arrow_forward11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).arrow_forward
- Predict the best choice in each of the following. You may wish to review the chapter on electronic structure for relevant examples.(a) the most metallic of the elements Al, Be, and Ba(b) the most covalent of the compounds NaCl, CaCl2, and BeCl2(c) the lowest first ionization energy among the elements Rb, K, and Li(d) the smallest among Al, Al+, and Al3+(e) the largest among Cs+, Ba2+, and Xearrow_forwardGroup the electronic configurations of neutral elements in sets according to those you would expect to show similar chemical properties. Note that as long as the configurations are grouped correctly with regard to each other, it does not matter which set you assign to each group. Set A Set B Answer Bank 1s2s? 1s°2s²2p°3s²3p°4s² Is²25²2p°3s°3p² 1s? 1s²25²2p 655²4d105p°6s²4f\45dl®6p² about us careers privacy policy terms of use contact us helparrow_forwardCalculate the electron affinity of Cl from the followingdata for NaCl, and compare your result with thevalue in Appendix B-1 : Cl2 bond energy = 239 kJ/mol;Hf (NaCl) = -413 kJ/mol; Hsub(Na) = 109 kJ/mol;IE(Na) = 5.14 eV; and r+ + r- = 281 pm.arrow_forward
- Draw Lewis structures for the following species: Br2Se, NCCN, GeO4 4- , HO2 - , NBr4 + . Write down the condensed electron configuration of the following ions: a) Fe+ b) Zn c) Ga2+ d) Cu3+arrow_forwardWrite the charge and full ground-state electron configuration of the monatomic ion most likely to be formed from each atom: (a) CI (b) Na (c) Ca Which of the formed ions will be least stable? -- --arrow_forwardRank the bonds in each set in order of decreasing bond length and decreasing bond strength: (a) Si-F, Si-C, Si-O; (b) N=N, N-N, N=N.arrow_forward
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