Question

Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary. Orbital Quantum numbers not allowed n = 1, ? = 1, m? = 0 4d n = 4, ? = 2, m? = 2 2p n = 2, ? = 1, m? = -1 not allowed n = 3, ? = 2, m? = -3 5f n = 5, ? = 3, m? = 1 Answer Bank 4d 4f 5d 5p 3s 3d 2s not allowed 5s 5f 2p 3p 1p 4s 3f 2d 4p 1s

          Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary.

Orbital Quantum numbers
not allowed n = 1, ? = 1, m? = 0
4d n = 4, ? = 2, m? = 2
2p n = 2, ? = 1, m? = -1
not allowed n = 3, ? = 2, m? = -3
5f n = 5, ? = 3, m? = 1

Answer Bank
4d 4f 5d 5p 3s
3d 2s not allowed 5s
5f 2p 3p 1p 4s
3f 2d 4p 1s

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Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary.

Orbital Quantum numbers
not allowed n = 1, ? = 1, m? = 0
4d n = 4, ? = 2, m? = 2
2p n = 2, ? = 1, m? = -1
not allowed n = 3, ? = 2, m? = -3
5f n = 5, ? = 3, m? = 1

Answer Bank
4d 4f 5d 5p 3s
3d 2s not allowed 5s
5f 2p 3p 1p 4s
3f 2d 4p 1s

Added by Carolyn O.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Jennifer Hudspeth

11/27/2022

Step 1

n = 1, ℓ = 1, mℓ = 0: This set of quantum numbers is not allowed. The quantum number ℓ can range from 0 to n-1. Since n is 1 in this case, ℓ can only be 0. Therefore, ℓ = 1 is not allowed. Show more…

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Complete the table by pairing each set of quantum numbers with the orbital it describes. If the set of quantum numbers is not possible, label it as not allowed. Use each orbital description as many times as necessary: Orbital Quantum numbers not allowed: n = 1, l = 1, ml = 0 4d: n = 4, l = 2, ml = 2 2p: n = 2, l = 1, ml = -1 not allowed: n = 3, l = 2, ml = -3 5f: n = 5, l = 3, ml = 1

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Transcript

00:02 Hi there.

00:03 To answer this question, let's talk about quantum numbers first and the possible values for those.

00:08 So the first quantum number, the principal quantum number n, that of course tells us the energy level.

00:18 And it can be any positive integer.

00:25 The lower the integer, the closer the energy level is to the nucleus.

00:30 All right, the next quantum number l, the angular momentum quantum number, tells us the subshell.

00:38 An l is an integer ranging from 0 to n minus 1.

00:52 In other words, if n were 2, l could be 0 or 1, because 2 minus 1 is 1.

00:59 Furthermore, when l equals 0, it's an s orbital.

01:03 When l equals 1, that describes the p orbitals.

01:06 When l equals 2, it's the d orbitals.

01:09 And when l equals 3, that would be the f orbitals.

01:12 The third quantum number, this is the last quantum number that actually describes the orbital, that's the magnetic quantum number.

01:22 It also must be an integer.

01:24 It's going to describe the orbital's orientation in space, and it ranges from, so its values can be anything between negative l to positive l.

01:41 So if l were 2, ms of l could be negative 2, negative 1, 0, or 2.

01:47 The fourth and final quantum number is the spin quantum number.

01:52 And we don't see that in this question, but that refers to the electrons themselves.

01:57 And whether they have a positive spin, in which case the value is positive one -half, or a negative spin, in which case the value is negative one -half.

02:06 Okay, so let's analyze what we have here for our first one.

02:10 So i'm just going to do this as a little table.

02:19 For the first one, we have n equals one, l -equals one.

02:22 M sub l equals 0.

02:24 Well, if n is 1 and l ranges from 0 to n minus 1, l could only be 0.

02:32 So we have an issue with l here.

02:34 It cannot be 1.

02:36 So this set is not allowed.

02:42 All right...

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