QUESTION 12 When an electron goes from a ground state to an excited state, it: O Always absorbs energy O Always emits energy O Either absorbs or releases energy depending on the state of the electron and the identity of the element QUESTION 13 True or False? Two electrons in an atom can have the exact same set of quantum numbers, (n. I, mj, m-). O True False

QUESTION 12 When an electron goes from a ground state to an excited state, it: O Always absorbs energy O Always emits energy O Either absorbs or releases energy depending on the state of the electron and the identity of the element QUESTION 13 True or False? Two electrons in an atom can have the exact same set of quantum numbers, (n. I, mj, m-). O True False

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter11: Modern Atomic Theory

Section: Chapter Questions

Problem 12ALQ

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Similar questions

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, = 2, m = 0, ms = +1/2 (b) n = 2, = 1, m = 1, ms = 0 (c) n = 3, = 1, m = 2, ms = +1/2
6.27 Refer w the data and energy-Ievel diagram shown in Problem 6.26, and find the wavelength of light that would be emitted when a hydrogen atom undergoes the transition from the state labeled as n = 4 to the state labeled as n = 2. Express your answer in nm.
Suppose you live in a different universe where a different set of quantum numbers is required to describe the atoms of that universe. These quantum numbers have the following rules: N, principal 1, 2, 3,, L, orbital = N M, magnetic -1, 0, +1 How many orbitals are there altogether in the first three electron shells?
Give the symbol of the element of lowest atomic number whose ground state has (a) a completed f subshell. (b) twenty p electrons. (c) two 4d electrons. (d) five 5p electrons.
Explain why each of the following sets of quantum numbers would not be permissible for an electron, according to the rules for quantum numbers. a n = 1, I = 0, mi = 0, ms = +1 b n = 1, I = 3, mi = +3, ms=+12 c n = 3, I = 2, mi = +3, ms=12 d n = 0, I = 1, mi = 0, ms=+12 e n = 2, I = 0, mi = 1, ms=+32
Write a complete set of quantum numbers (n, , m) that quantum theory allows for each of the following orbitals: (a) 2p, (b) 3d, and (c) 4f.
What are the allowed values for each of the four quantum numbers: n, l, ml, and ms?
What is the maximum number of orbitals that can be identified by each of the following sets of quantum numbers? When none is the correct answer, explain your reasoning. (a) n = 3, = 0, m = +1 (b) n = 5, = 1, (c) n = 7, = 5, (d) n = 4, = 2, m = 2
Answer the following questions. (a) What characteristic of an atomic orbital does the quantum number ms describe? (b) Does a photon with a frequency of 35.8 Hz have more or less energy than one with a frequency of 125 Hz? (c) How many orbitals can be associated with the following set of quantum numbers:n=3, l=2? (d) Is a sample of ZnCl2 containing the Zn2+ ion diamagnetic?
Which of the following statements is (are) true? I. The product of wavelength and frequency of light is a constant. II. As the energy of electromagnetic radiation increases, its frequency decreases. III. As the wavelength of light increases, its frequency increases. a I only b II only c III only d I and III only e II and III only
Tbe relative orbital levels for the hydrogen atom can be represented as Draw the relative orbital energy levels for atoms with more than one electron and explain your answer. Also explain bow the following radial probability distributions support your answer.
Using complete subshell notation (not abbreviations, 1s22s22p6, and so forth), predict the electron configuration of each of the following atoms: (a)C (b)P (c)V (d) Sb (e) Sm

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