Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
9th Edition
ISBN: 9781285462530
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Textbook Question
Chapter 6, Problem 38PS
Explain briefly why each of the following is not a possible set of quantum numbers for an electron in an atom. In each case, change the incorrect value (or values) to make the set valid.
- (a) n = 2, ℓ = 2, mℓ = 0, ms = +1/2
- (b) n = 2, ℓ = 1, mℓ = 1, ms = 0
- (c) n = 3, ℓ = 1, mℓ = 2, ms = +1/2
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Give the notation (using letter designations for l) for the subshells denoted by the following quantum number. (Enter your answer in the format of 5p for 5p.)
(a) n = 4, l = 0(b) n = 1, l = 0(c) n = 5, l = 3(d) n = 5, l = 2
2. An electron in a hydrogen atom is excited from the ground state to the n=4 state. Comment
on the correctness of the following statements (true or false and why?).
%3D
(a) n = 4 is the first excited state.
(b) It takes more energy to ionize (remove) the electron from n = 4 than from the ground
state.
(c) The electron is farther from the nucleus (on average) in n = 4 than in the ground state.
(d) The wavelength of light emitted when the electron drops from n = 4 to n = 1 is longer
than that from n =4 to n =2.
(e) The wavelength the atom absorbs in going from n= 1 to n=4 is the same as that emitted
as it goes from n =4 to n = 1.
Which of the following represent valid sets of quantum numbers? For a set is invalid, explain briefly why it is not correct.(a) n = 3, ℓ = 3, mℓ = 0(b) n = 2, ℓ = 1, mℓ = 0(c) n = 6, ℓ = 5, mℓ = ‒1(d) n = 4, ℓ = 3, mℓ = ‒4
Chapter 6 Solutions
Chemistry & Chemical Reactivity, Hybrid Edition (with OWLv2 24-Months Printed Access Card)
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