
(a)
Interpretation: The electron sublevel starts to fill after the completion of 3s 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
The relative energy of orbitals is represented as follows:
(b)
Interpretation: The electron sublevel starts to fill after the completion of 4p 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
The relative energy of orbitals is represented as follows:
(c)
Interpretation: The electron sublevel starts to fill after the completion of 3d 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
The relative energy of orbitals is represented as follows:
(d)
Interpretation: The electron sublevel starts to fill after the completion of 3p 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
The relative energy of orbitals is represented as follows:

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Chapter 5 Solutions
EBK BASIC CHEMISTRY
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