**Question 2:** Which of the following sets of quantum numbers is allowed?a. \( n = 2, \, \ell = 1, \, m_{\ell} = +1/2, \, m_s = -1/2 \)b. \( n = 3, \, \ell = 2, \, m_{\ell} = +1, \, m_s = +1 \)c. \( n = 4, \, \ell = 1, \, m_{\ell} = 0, \, m_s = -1/2 \)d. \( n = 4, \, \ell = 3, \, m_{\ell} = -1, \, m_s = 0 \)e. \( n = 5, \, \ell = 2, \, m_{\ell} = +2, \, m_s = -1 \)

Answered: 2) Which of the following sets of…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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According to quantum mechanics, there are four types of quantum numbers. The electrons are filled in atomic orbitals. The details of atomic orbital can be got by the following four quantum numbers:

Principal quantum number(n): It defines the number of shells in an atom. The energy and size of the orbital depend on the principal quantum number. Its values are 1,2,3,4...etc.
Azimuthal quantum number(l) or angular momentum quantum number(l): It defines the number of subshells in a particular shell. The shape of the orbital depends on the angular momentum quantum number. Its values are 0 to (n-1).

for l = 0 the subshell is = s

for l = 1 the subshell is = p

for l = 2 the subshell is = d

for l = 3 the subshell is = f