The absence of 2 d subshell using quantum numbers is to be explained. Concept introduction: Principal Quantum Number ( n ) refers to the size of an atom’s orbital. The larger the value of ( n ) , the greater is the size of orbital. Angular Momentum Quantum Number ( l ) describes the shape of an atom’s orbital. The values of ( l ) are integers. Its values range from 0 to ( n − 1 ) . Magnetic Quantum Number ( m l ) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of ( l ) . For a value of ( l ) , there will be ( 2 l + 1 ) number of integral values of ( m l ) .

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Answer 1

Question

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

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Answer 2

Question

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

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Answer 3

Question

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

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Answer 4

Question

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

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Answer 5

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

Answer 6

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

Answer 7

Chapter 6.8, Problem 1PPB

Interpretation Introduction

Interpretation:

The absence of 2d subshell using quantum numbers is to be explained.

Concept introduction:

Principal Quantum Number (n) refers to the size of an atom’s orbital. The larger the value of (n), the greater is the size of orbital.

Angular Momentum Quantum Number (l) describes the shape of an atom’s orbital. The values of (l) are integers. Its values range from 0 to (n−1).

Magnetic Quantum Number (ml) describes the orientation of orbital in space with the help of integral values, and so, it depends on the value of (l). For a value of (l), there will be (2l+1) number of integral values of (ml).

Answer 8

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Answer 9

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Answer 10

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Answer 11

Ch. 6.1 - Practice ProblemATTEMPT What is the frequency (in...Ch. 6.1 - Prob. 1PPB Ch. 6.1 - Practice Problem CONCEPTUALIZE Which of the...Ch. 6.1 - Prob. 1CP Ch. 6.1 - Calculate the frequency of light with wavelength...Ch. 6.1 - Prob. 3CP Ch. 6.1 - Prob. 4CP Ch. 6.2 - Practice Problem ATTEMPT Calculate the difference...Ch. 6.2 - Prob. 1PPB Ch. 6.2 - Prob. 1PPC

Solution Summary: The author explains the absence of 2d subshell using quantum numbers. Principal quantum number (n) refers to the size of an atom's orbital.

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