The electron sublevel starts to fill after the completion of 5s sublevel should be determined. Concept Introduction: The rules for the allowed quantum numbers combinations are as follows: All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers. The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on. The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2. The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2 For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell. Here, for s orbital value of l = 0 , for p orbital it is l = 1 , for d orbital it is l = 2 and for f it is 3. The relative energy of orbitals is represented as follows:

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Answer 1

Question

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

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4:45 PM Tue Apr 1 K 77% Problem 9 of 10 Submit Curved arrows are used to illustrate the flow of electrons. Using the provided starting structure, draw the curved electron-pushing arrows for the following reaction or mechanistic step(s). Be sure to account for all bond-breaking and bond-making steps. Then draw any missing organic intermediates or products for this reaction. Include all lone pairs in the structures. Ignore inorganic byproducts, counterions, and solvents. :0: H Select to Add Arrows HI CH3OH H+ ·HO CH3OH, H+ 0:0 H H Select to Add Arrows tion Versirate CH3OH, H* Select to Draw Product

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Answer 2

Question

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

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Answer 3

Question

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 4

Question

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Expert Solution & Answer

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Check out a sample textbook solution

See solution

Answer 5

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 6

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 7

Chapter 5, Problem 92APP

(a)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5s sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 8

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 9

(b)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4d sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.

The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.

The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 10

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 11

(c)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 4f sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.

The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

For same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 12

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 13

(d)

Interpretation Introduction

Interpretation: The electron sublevel starts to fill after the completion of 5p sublevel should be determined.

Concept Introduction:

The rules for the allowed quantum numbers combinations are as follows:

All the three quantum numbers ( n, l and m ) describes the orbital of an atom and they are integers.
The principal quantum number, n value cannot be zero. Thus, the values allowed for the principal quantum number are 1, 2, 3, 4, and so on.
The value of angular quantum number, l can be between 0 to n-1. Thus, if value of n is equal to 3 the value of l can be 0, 1 or 2.
The value of magnetic quantum number, m can be between − l to +l . Thus, if value of l is equal to 2, m can be wither -2, -1, 0, +1, or +2

lFor same number of principal quantum number, an orbital form a shell. The first character denotes the shell and the second identifies the sub-shell.

Here, for s orbital value of l=0 , for p orbital it is l=1 , for d orbital it is l=2 and for f it is 3.

The relative energy of orbitals is represented as follows:

Answer 14

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Answer 15

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Answer 17

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Solution Summary: The author explains the rules for the allowed quantum numbers combinations: n, l, and m describe the orbital of an atom and they are integers.

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