Question

List the values of n, l, and ml for each of the orbitals in a 4d subshell​

Answer 1

Answer:

Each electron has its unique set of quantum numbers, which means that two electrons can share one, two, or even three quantum numbers, but never all four.

Now, you are given a

4

d

orbital and asked to find how many sets of quantum numbers can describe an electron located in such an orbital, or, in other words, how many electrons can occupy a

4

d

orbital.

So, the principal quantum number,

n

, describes the energy level on which the electron is located. In this case, you have

n

=

4

→

the electron is located on the fourth energy level

The subshell in which the electron is located is described by the angular magnetic quantum number,

l

, which for the fourth energy level takes the following values

l

=

0

→

the s-subshell

l

=

1

→

the p-subshell

l

=

2

→

the d-subshell

l

=

3

→

the f-subshell

Since you're looking for the d-subshell, you will need

l

=

2

.

The specific orbital in which the electron is located is given by the magnetic quantum number,

m

l

. For any d-subshell, the magnetic quantum number can take the values

m

l

=

{

−

2

,

−

1

,

−

0

,

+

1

,

+

2

}

Each of these five values describes one of the five d-orbitals available in a d-subshell.

Answer 2

The values of n, l and ml for each orbits in 4d subshell is listed.

Explanation:

• n denotes the principle of quantum number, l denotes angular momentum quantum number and ml denotes magnetic $(m_1)$ and spin $(m_2)$ quantum number.
• In n=4 the orbital has 4 energy levels. They are s, p, d and f subshell.
• Considering 4d subshell, the value of n is 4, the value of l is 2 and the value of ml is 5 (-2, -1, 0, 1, 2).
• 4d Subshell takes 10 electrons.
• 5 electrons will be shared with spin. So, the value of $m_{s} =1/2$ or $-1/2$.