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Lattice energies are graphed for three series of compounds in which the ion charges are
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Chemistry
- Nitrogen ions tend to have a charge of 3-; explain the reason for this pattern/trend.arrow_forwardin ne taist ME He Pa Example 4. Why do the transition elements exhibit higher enthalpies of atomisation? ( DA Try percet HOarrow_forwardEnergy is required to remove two electrons from Ca to formCa2+, and energy is required to add two electrons to O toform O2 - . Yet CaO is stable relative to the free elements.Which statement is the best explanation? (a) The latticeenergy of CaO is large enough to overcome these processes.(b) CaO is a covalent compound, and these processes areirrelevant. (c) CaO has a higher molar mass than either Ca orO. (d) The enthalpy of formation of CaO is small. (e) CaO isstable to atmospheric conditions.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_forwardEstimate the change in enthalpy (delta H) for the dissociation for HCl(g) into H+(g) and Cl-(g) Ionization energy for H 1312 kJ/mol Electron affinity for H (-72.8 kJ/mol) Ionization energy for Cl 1251.2 kJ/mol Electron affinity for Cl (-349 kJ/mol)arrow_forwardPredict 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_forward
- 11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).arrow_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_forwardDraw 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_forward
- Calculate the second ionization energy of the metal M (AHion2 in kJ/mol) using the following data: Lattice enthalpy of MO(s), AH = -2278 kJ/mol Bond dissociation enthalpy of O2(g) = +498 kJ/mol First electron affinity of O = -141 kJ/mol Second electron affinity of O = +744 kJ/mol Enthalpy of sublimation of M = + 125 kJ/mol First ionization energy of M = + 309 kJ/mol Standard enthalpy of formation of MO(s), AH = -341 kJ/molarrow_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_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_forward
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