Question

what are the possible values of m for an electron in 3d sub shell?

Answer 1

For electrons located in a

3p

orbital, the principal quantum number is equal to

n=3→the third energy level

So, you know that you have

n=3

. Next, find the value of the angular momentum quantum number,

l

, which gives you the subshell in which the electron is located.

The

p

subshell is denoted by

l=1

, so the first two quantum numbers for these two electrons are

n=3,l=1

Now, the

p

subshell can hold

3

orbitals, which are denoted by the magnetic quantum number,

ml

.

l=1⇒⎧⎪ ⎪⎨⎪ ⎪⎩ml=−1→the 3px.orbitalml=−0→the 3pz.orbitalml=+1→the 3py.orbital

Finally, the spin quantum number,

ms

, which can only take two possible values, gives you the spin of the electron.

You can form several possible sets of quantum numbers to describe two electrons located in

3p

orbitals. For example, you can have

n=3,l=1,ml=−1,ms=+1/2
This electron is located on the third energy level, in the

3p

subshell, in the

3px

orbital, and has spin-up

n=3,l=1,ml=−1,ms=−1/2
This electron is located on the third energy level, in the

3p

subshell, in the

3px

orbital, and has spin-down

These two sets describe electrons that are located in the same orbital, which is why the only differ in the value of the spin quantum number.

Similarly, you can have

n=3,l=1,ml=0,ms=+1/2
This electron is located on the third energy level, in the

3p

subshell, in the

3pz

orbital, and has spin-up

n=3,l=1,ml=1,ms=−1/2
This electron is located on the third energy level, in the

3p

subshell, in the

3py

orbital, and has spin-down

Hope this will help you..... ✌

Answer 2

Answer: m= - 2,-1,0,+1,+2

Explanation: we have to find quantum nos. for 3d subshell.

So, n=3

l=2. As we know m= - l to l.

So you get the answer