Question

Which of the following set of quantum numbers (ordered n,l,ml,ms) are possible for an electron in an atom?

Quantum Number Rules Learning Goal: To learn the restrictions on each quantum number. Quantum numbers can be thought of as labels for an electron. Every electron in an atom has a unique set of four quantum numbers. The principal quantum number n corresponds to the shell in which the electron is located. Thus n can therefore be any integer. For example, an electron in the 2p subshell has a principal quantum number of n = 2 because 2p is in the second shell. The azimuthal or angular momentum quantum number corresponds to the subshell in which the electron is located. s subshells are coded as 0, p subshells as 1, das 2, and fas 3. For example, an electron in the 2p subshell has l = 1. As a rule, l can have integer values ranging from 0 to n - 1. The magnetic quantum number me corresponds to the orbital in which the electron is located. Instead of 2pz., 2py, and 2pz, the three 2p orbitals can be labeled -1,0, and 1, but not necessarily respectively. As a rule, my can have integer values ranging from l to +l. The spin quantum number m, corresponds to the spin of the electron in the orbital. A value of 1/2 means an "up" spin, whereas 1/2 means a "down" spin.

Answer 1

C)

for option 1:

n must be a positive number

n can't be -1

Hence, this is not valid

for option 2:

Value of l is 2

So, valid values of ml are [-2, -1, 0, 1, 2]

so, ml can't be 3

Hence, this is not valid

for option 3:

This is valid

for option 4:

Value of l is 2

So, valid values of ml are [-2, -1, 0, 1, 2]

so, ml can't be 3

Hence, this is not valid

for option 5:

This is valid

for option 6:

ms can be -1/2 or 1/2.

It can’t be -2

Hence, this is not valid

for option 7:

This is valid

for option 8:

l must be less than n

Here value of n is 2

But value of l is 4

so, l can't be 4

Hence, this is not valid

Answer: option 3, 5, 7

Answer 2

The answer is option 3,5,7. I don't know why the answer above has a dislike if it's right.