Book edition 10th Edition

Author(s) David Halliday

Pages 1328 pages

ISBN 9781118230718

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Short Answer

Label these statements as true or false:
(a) One (and only one) of these sub shells cannot exist: 2p,4f,3d,1p
(b) The number of values of $m_{l}$ that are allowed depends on l and not on n.
(c) There are four sub shells for n = 4 .
(d) The smallest value of for a given value of l is l + 1 .
(e) All states with l = 0 also have $m_{l} = 0$ .
(f) There are n sub shells for each value of n .

The given statement is true.
The given statement is true.
The given statement is true.
The given statement is true.
The given statement is true.
The given statement is true.

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Step by Step Solution

TABLE OF CONTENTS :

TABLE OF CONTENTS

Step 1: The given data

There are different electronic configuration statements that need to be verified.

Step 2: Understanding the concept of the electronic configuration

The electronic configuration with the principal quantum number, n, has an orbital angular quantum number in the range of 0 to n-1 integer values.

In contrast, the range of magnetic angular quantum number ranges from -l to +l. The number of sub-shells is equal to the principal quantum number.

Step 3: a) Calculation of not possible state configuration

From any principal quantum number, we can get the number of the sub-shells in that electronic configuration that is s, p, d, and f.

So, here the state is not possible as the orbital quantum number of this state is l = 1(for p) . This is equal to the principal quantum number (n = 1), which is impossible.

Hence, this statement is true.

Step 4: b) Calculation of the dependence of the magnetic quantum number

The value of magnetic quantum number $m_{l}$ ranges from -l to +l . Thus, it depends on the value of l , not on the value of n .

Hence, this statement is true

Step 5: c) Calculation of the number of sub shells for n = 4

The number of sub-shells of an orbital is equal to the principal number.

Thus, the number of sub shells for n = 4 is 4.

Hence, this statement is true.

Step 6: d) Calculation of the smallest value of n

We know that the values of orbital quantum numbers l range from 0 to (n-1).

Thus, here the smallest value of for any value of is given by:

l = n -1

n = l + 1

Hence, this statement is true.

Step 7: e) Calculation of the values of magnetic quantum number for l = 0

We know that the values of magnetic quantum number for any value of range from -l to +l . Thus, for the value l = 0 , the only value of $m_{l}$ is $m_{l} = 0$ .

Hence, this statement is true.

Step 8: f) Calculation of the number of sub shells for n

From the concept, we can say that the number of sub-shells of an orbital is equal to its principal quantum number n .

Hence, this statement is true.

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Fundamentals Of Physics

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Short Answer

Step by Step Solution

Step 1: The given data

Step 2: Understanding the concept of the electronic configuration

Step 3: a) Calculation of not possible state configuration

Step 4: b) Calculation of the dependence of the magnetic quantum number

Step 5: c) Calculation of the number of sub shells for n = 4

Step 6: d) Calculation of the smallest value of n

Step 7: e) Calculation of the values of magnetic quantum number for l = 0

Step 8: f) Calculation of the number of sub shells for n

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Fundamentals Of Physics

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Short Answer

Step by Step Solution

Step 1: The given data

Step 2: Understanding the concept of the electronic configuration

Step 3: a) Calculation of not possible state configuration

Step 4: b) Calculation of the dependence of the magnetic quantum number

Step 5: c) Calculation of the number of sub shells for n = 4

Step 6: d) Calculation of the smallest value of n

Step 7: e) Calculation of the values of magnetic quantum number for l = 0

Step 8: f) Calculation of the number of sub shells for n

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