### Quantum Number Orbital Identification**Question 6.62:**For the table that follows, determine which orbital corresponds to the given quantum numbers. Do not be concerned with \(x\), \(y\), and \(z\) subscripts. If the quantum numbers are not allowed, specify "not allowed."| n | l | m\_l | Orbital ||---|---|------|----------|| 2 | 1 | 1 | 2p (example) || 1 | 0 | 0 | || 3 | -3| 2 | || 3 | 2 | -2 | || 2 | 0 | 1 | || 0 | 0 | 0 | || 4 | 2 | 1 | || 5 | 3 | 0 | |#### Instructions:- **n** represents the principal quantum number.- **l** denotes the azimuthal (angular momentum) quantum number.- **m\_l** is the magnetic quantum number.#### Explanation:Each combination of quantum numbers gives rise to a specific atomic orbital, with allowed values governed by quantum mechanics principles. Unallowed combinations should be marked as "not allowed."Note: The table provides examples of quantum number sets, such as \(n = 2\), \(l = 1\), \(m\_l = 1\), corresponding to a 2p orbital, which is the given example.

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6.62 For the table that follows, write which orbital goes with the quantum numbers. Don't worry about x, y, z subscripts. If the quantum numbers are not allowed, writel "not allowed." I n 2 1 3 3 204 5 1 0 WNOON WO -3 2 0 2 3 E-O ~~ m 0 2 2 1 0 1 0 Orbital 2p (example)

6.62 For the table that follows, write which orbital goes with the quantum numbers. Don't worry about x, y, z subscripts. If the quantum numbers are not allowed, writel "not allowed." I n 2 1 3 3 204 5 1 0 WNOON WO -3 2 0 2 3 E-O ~~ m 0 2 2 1 0 1 0 Orbital 2p (example)

Chemistry

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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

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