Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN: 9781337399074
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 7, Problem 79SCQ

The energies of the orbitals in many elements have been determined. For the first two periods they have the following values:

Chapter 7, Problem 79SCQ, The energies of the orbitals in many elements have been determined. For the first two periods they

  1. (a) Why do the orbital energies generally become more negative on proceeding across the second period?
  2. (b) How are these values related to the ionization energy and electron attachment enthalpy of the elements?
  3. (c) Use these energy values to explain the observa­tion that the ionization energies of the first four second-period elements are in the order Li < Be > B < C.

(Data from J. B. Mann, T. L Meek, and L C. Allen: Journal of the American Chemical Society, Vol. 122, p. 2780. 2000.)

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Chapter 7 Solutions

Chemistry & Chemical Reactivity

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  • A. A main group element with the valence electron configuration 3s1 is in periodic group?It forms a monatomic ion with a charge of my ?B. A main group element with the valence electron configuration 2s22p4 is in periodic group?It forms a monatomic ion with a charge of?
    Boron, atomic number 5, occurs naturally as two isotopes, 10B and 11B, with natural abundances of 19.9% and 80.1%, respectively. (a) In what ways do the two isotopes differ from each other? Does the electronic configuration of 10B differ from that of 11B? (b) Draw the orbital diagram for an atom of 11B. Which electrons are the valence electrons? (c) Indicate three ways in which the 1s electrons in boron differ from its 2s electrons. (d) Elemental boron reacts with fluorine to form BF3, a gas. Write a balanced chemical equation for the reaction of solid boron with fluorine gas. (e) ­ΔHf° for BF3(g) is  -1135.6 kj/mol. Calculate the standard enthalpy change in the reaction of boron with fluorine. (f) Will the mass percentage of F be the same in 10BF3 and 11BF3? If not, why is that the case?
    In Section 8.6, we estimated the effective nuclear charge on beryllium’s valence electrons to be slightly greater than 2+. What would a similar process predict for the effective nuclear charge on boron’s valence electrons? Would you expect the effective nuclear charge to be different for boron’s 2s electrons compared to its 2p electron? In what way? (Hint: Consider the shape of the 2p orbital compared to that of the 2s orbital.)
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