What quantum numbers specify these subshells: 1s 4p 5d⋯ n=? l=?

Question

What quantum numbers specify these subshells: 1s 4p 5d⋯ n=? l=?

coffentw · Accepted Answer

Step 1
The principal quantum number (n) for 1s is 1 and the azimuthal quantum number (l) for 1s is 0.
Calculate the range of azimuthal quantum number (l) as follows:

l = n - 1

Substitute 1 for n in the above equation for the calculation of l as follows:

l = 1 - 1

= 0

The value of n is 1 and l is 0 for the 1s orbital.
The principal quantum number (n) defines the shell of the orbital. For 1s, the shell is 1.
The azimuthal quantum number (l) defines the subshell of the orbital. It is calculated as the difference between the n and 1. For 1s, the subshell is 0.
Step 2
The principal quantum number (n) for 4p is 4. Calculate the range of azimuthal quantum number (l) as follows:

l = n - 1

Substitute 4 for n in the above equation for the calculation of l as follows:

l = 4 - 1

= 3

The value of l for 4p lies between 0, 1, 2, 3 . For p orbital, the value of l is 1. Therefore, the azimuthal quantum number (l) for 4p is 1.
The value of n is 4 and l is 1 for the 4p orbital.
The principal quantum number (n) defines the shell of the orbital. For 4p, the shell is 4. The azimuthal quantum number (l) defines the subshell of the orbital. It is calculated as the difference between the n and 1. For 4p orbital, the value of l can be 0, 1, 2, 3. The orbital is p. For p orbital, the azimuthal quantum number is 1. Therefore, for 4p orbital, l is 1.
Step 3
The principal quantum number (n) for 5d is 5. Calculate the range of azimuthal quantum number (l) as follows:

l = n - 1

Substitute 5 for n in the above equation for the calculation of l as follows:

l = 5 - 1

= 4

The value of l for 5d lies between 0,1,2,3,4. For d orbital, the value of l is 2. Therefore, the azimuthal quantum number (l) for 5d is 2.
The value of n is 5 and l is 2 for the 5d orbital.
The principal quantum number (n) defines the shell of the orbital. For 5d, the shell is 5.
The azimuthal quantum number (l) defines the subshell of the orbital. It is calculated as the difference between the n and 1.
For 5d orbital, the value of l can be 0, 1, 2, 3, 4. The orbital is d. For d orbital, the azimuthal quantum number is 2. Therefore, for 5d orbital, l is 2.

RizerMix · Accepted Answer

The subshell notation used in chemistry and physics indicates the values of the quantum numbers that specify a particular electron orbital. In this case, we are asked to determine the quantum numbers for the subshells 1s, 4p, and 5d.
The first quantum number,

n

, represents the energy level of the electron and can have any positive integer value. The second quantum number,

l

, indicates the shape of the electron orbital and can have integer values ranging from 0 to

n - 1

. The third quantum number,

m_{l}

, specifies the orientation of the orbital in space and can have integer values ranging from

- l

to

+ l

.
For the subshell 1s, we have

n = 1

and

l = 0

. This subshell contains a single spherical orbital that can hold up to two electrons.
For the subshell 4p, we have

n = 4

and

l = 1

. This subshell contains three dumbbell-shaped orbitals oriented along the x, y, and z axes, each of which can hold up to two electrons.
For the subshell 5d, we have

n = 5

and

l = 2

. This subshell contains five cloverleaf-shaped orbitals oriented along the x, y, and z axes, each of which can hold up to two electrons.
In summary, the quantum numbers for the subshells 1s, 4p, and 5d are:
- 1s:

n = 1

,

l = 0

- 4p:

n = 4

,

l = 1

- 5d:

n = 5

,

l = 2

Vasquez · Accepted Answer

To specify the subshells in an atom, we use a notation that includes the principal quantum number (

n

) and the azimuthal quantum number (

l

).
The principal quantum number (

n

) determines the energy level of an electron, and it can take on any positive integer value. The azimuthal quantum number (

l

) determines the shape of the orbital and can take on integer values ranging from 0 to

n - 1

.
For the subshell 1s, we have

n = 1

and

l = 0

. The subshell 1s consists of a single s orbital, which is spherical in shape.
For the subshell 4p, we have

n = 4

and

l = 1

. The subshell 4p consists of three p orbitals, which are dumbbell-shaped and oriented along the x, y, and z axes.
For the subshell 5d, we have

n = 5

and

l = 2

. The subshell 5d consists of five d orbitals, which are cloverleaf-shaped and oriented along the x, y, and z axes.
In summary, the subshells 1s, 4p, and 5d have the following values for

n

and

l

:
- 1s:

n = 1

,

l = 0

- 4p:

n = 4

,

l = 1

- 5d:

n = 5

,

l = 2

Jeffrey Jordon · Accepted Answer

The subshells 1s, 4p, and 5d can be specified by their quantum numbers, which are represented by the principal quantum number

n

and the azimuthal quantum number

l

.
For the subshell 1s,

n = 1

and

l = 0

.

n = 1

and

l = 0

for 1s subshell.
For the subshell 4p,

n = 4

and

l = 1

.

n = 4

and

l = 1

for 4p subshell.
For the subshell 5d,

n = 5

and

l = 2

.

n = 5

and

l = 2

for 5d subshell.

What quantum numbers specify these subshells: 1s\ 4p\ 5d\cdots\ n=?\ l=?

Answered question

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