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Chapter 6: Problem 21

What type of electron orbital (i.e., \(\mathrm{s}, \mathrm{p}, \mathrm{d}\), or \(\mathrm{f}\) ) is designated by (a) \(\mathbf{n}=3, \ell=2, \mathbf{m}_{\ell}=-1\) ? (b) \(\mathbf{n}=6, \ell=3, \mathbf{m}_{\ell}=2 ?\) (c) \(\mathbf{n}=4, \ell=3, \mathbf{m}_{\ell}=3\) ?

Short Answer

Expert verified
Question: Identify the type of electron orbital for the given quantum numbers: (a) n=3, l=2, m_l=-1 (b) n=6, l=3, m_l=2 (c) n=4, l=3, m_l=3 Answer: (a) d orbital (b) f orbital (c) f orbital

Step by step solution

01

(a) Identify the orbital with n=3, l=2, m_l=-1

Given the quantum numbers n=3, l=2, m_l=-1, we will focus on the value of l, which is 2. Since l=2, it corresponds to the d orbital.
02

(b) Identify the orbital with n=6, l=3, m_l=2

Given the quantum numbers n=6, l=3, m_l=2, we will focus on the value of l, which is 3. Since l=3, it corresponds to the f orbital.
03

(c) Identify the orbital with n=4, l=3, m_l=3

Given the quantum numbers n=4, l=3, m_l=3, we will focus on the value of l, which is 3. Since l=3, it corresponds to the f orbital.

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Most popular questions from this chapter

Give the symbols of (a) all the elements in period 5 that have at least two half-filled \(5 \mathrm{p}\) orbitals. (b) all the elements in Group 1 that have full \(3 \mathrm{p}\) orbitals. (c) all the metalloids that have paired \(3 p\) electrons. (d) all the nonmetals that have full \(3 \mathrm{~d}\) orbitals and 3 half- filled \(3 \mathrm{p}\) orbitals.

Give the symbol of the element of lowest atomic number whose ground state has (a) a completed \(\mathrm{f}\) subshell. (b) \(20 \mathrm{p}\) electrons. (c) two \(4 \mathrm{~d}\) electrons. (d) five 5p electrons.

In what main group(s) of the periodic table do element(s) have the following number of filled p orbitals in the outermost principal level? (a) 0 (b) 1 (c) 2 (d) 3

Which of the following electron configurations are for atoms in the ground state? In the excited state? Which are impossible? (a) \(1 s^{2} 2 s^{2} 2 p^{1}\) (b) \(1 s^{2} 1 p^{1} 2 s^{1}\) (c) \(1 s^{2} 2 s^{2} 2 p^{3} 3 s^{1}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 d^{10}\) (e) \(1 s^{2} 2 s^{2} 2 p^{5} 3 s^{1}\)

Given the following sets of electron quantum numbers, indicate those that could not occur, and explain your answer. (a) \(3,0,0,-\frac{1}{2}\) (b) \(2,2,1,-\frac{1}{2}\) (c) \(3,2,1,+\frac{1}{2}\) (d) \(3,1,1,+\frac{1}{2}\) (e) \(4,2,-2,0\)
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