3. Which one of each of the following pairs has the higher electron affinity? Explain in detail for each case. (a) C or F (b) For I (c) Te or I (d) О or S (e) S or Se
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- Which element in each of the following sets would you expect to have the lowest third ionization energy, IE3? (a) O Na O Al O Mg (b) O Ga ок O Mg (c) O Ca O Sc OK оооChoose the option in each that has the desired characteristic. Briefly explain each of your choices. (a) Larger Size? Si or Cl (b) Lower IE1? P or Po (c) Better Electron Affinity? O or F (d) Smaller Size? Br or Te2-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 Xe
- Hydrogen is an unusual element because it behaves in someways like the alkali metal elements and in other ways likenonmetals. Its properties can be explained in part by its electronconfiguration and by the values for its ionization energyand electron affinity. (a) Explain why the electron affinity ofhydrogen is much closer to the values for the alkali elementsthan for the halogens. (b) Is the following statement true?“Hydrogen has the smallest bonding atomic radius of anyelement that forms chemical compounds.” If not, correct it.If it is, explain in terms of electron configurations. (c) Explainwhy the ionization energy of hydrogen is closer to the valuesfor the halogens than for the alkali metals. (d) The hydrideion is H-. Write out the process corresponding to the firstionization energy of the hydride ion. (e) How does the processin part (d) compare to the process for the electron affinityof a neutral hydrogen atom?For each of the following pairs of atoms, state which youexpect to have the higher first ionization energy: (a) Bi orXe; (b) Se or Te; (c) Rb or Y; (d) K or Ne.11)Explain the given ionization energy for each pair using electron configurations. (12(Be)l1(B), I1(N)>l1(O) ).
- For each of the following pairs of atoms, state which youexpect to have the greater electron affinity: (a) Xe or Cs;(b) Pm or F; (c) Ca or K; (d) Po or At.Valence electrons in an atom of phosphorus are closer to the nucleus than the valence electrons ofaluminum because: (A) P has a greater effective nuclear charge and a greater shielding than Al.(B) P has a greater effective nuclear charge with the same shielding as Al.(C) P has the same effective nuclear charge with greater shielding than Al.(D) P has the same effective nuclear charge and the same shielding as Al.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
- 7. Which element has the smallest first ionization energy? (a) Cs (b) Ga (c) K (d) Bi (e) As 8. Which element has the smallest second ionization energy? (a) Mg (b) Li (c) S (d) O (e) Ca 9. Which of the following sets contain all linear molecules? (a) H2S, HCN, CO2. (b) HCN, O2, CO2 (c) H2O, CO, Cl2. (d) H2S, CO, CO2. (e) BF3, Cl2, O2 10. The molecular geometry of SnCl3-ion is: (a) trigonal planar (b) T-shaped. (c) trigonal pyramidal. (d) Tetrahedral (e) see-saw 11. The geometry of the molecule SPC13 is best described as: (a) square planar (b) trigonal pyramidal (c) trigonal bipyramidal. (d) octahedral (e) tetrahedral 12. The O-S-Cl bond angles in O2SCl2 are expected to be approximately: (a) 90° (b) 109.5° (c) 120° (d)180 ° (e) 90° and 120°5. Which of the following alkali metal halides has the larger lattice energy, and which has the smaller lattice energy? Explain. (a) (b)(a) Account for formation of the following series of oxidesin terms of the electron configurations of the elementsand the discussion of ionic K2O, CaO, Sc2O3, TiO2, V2O5, CrO3. (b) Name these oxides.(c) Consider the metal oxides whose enthalpies of formation(in kJ mol -1) are listed here. Calculate the enthalpy changes in the following general reactionfor each case:MnOm(s) + H2(g)----->nM(s) + mH2O(g)(You will need to write the balanced equation for each caseand then compute ΔH°.) (d) Based on the data given, estimatea value of ΔHf° for Sc2O3(s).