Question

What is the only possible value of mℓ for an electron in an s orbital?Express your answer numerically.

2.

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

Check all that apply.

	-1, 0, 0, -1/2
	3, 2, 2, -1/2
	3, 1, 0, -1/2
	4, 3, -4, -1/2
	3, 2, 0, -1/2
	2, 1, 3, 1/2
	2, 1, 0, -1
	3, 3, 1, -1/2

Answer 1

Answer: According to the question , Here the

1] The azimuthal or angular momentum quantum number l corresponds to the subshell in which the electron is located. s subshells are coded as 0, p subshells as 1, d as 2, and f as 3.

Hence , For the S orbotal Ml value is = 0 .

2] According to the given information here first we have to understand the definations of the 4 quantum numbers :

n = 1, 2, 3, ..., n

l = 0 to n − 1 >> This includes all possible values up to n-1.

ml = all values from -l to +l >> example if l = 2 them ml = -2, -1, 0, +1, +2

ms = +1/2 and -1/2

Now analysing the given data

1] -1, 0, 0, -1/2 Not possible because n can not be negative

2] 3, 2, 2, -1/2 This is a possible configuration

3] 3, 1, 0, -1/2 this is a possible configuration

4] 4, 3, -4, -1/2 Not possible configuration

5] 3, 2, 0, -1/2 this is possible

6] 2, 1, 3, 1/2 not possible ml can not be greater than n

7] 2, 1, 0, -1 not possible because ms is not greater than 1/2 or -1/2

8] 3, 3, 1, -1/2 not possible

Hence it is all about the given question . Thank you :)