Question

Which is a correct set of values of m for one of the subshells of n = 2?

Answer 1

Answer: The correct answer is -1, 0, 1.

Explanation:

The Quantum numbers are:

1. Principle Quantum Number: This number describes the size of the orbital. It is represented by "n". The value of n = 1,2,3,4....

2. Azimuthal Quantum Number: This number describes the shape of the orbital. It is denoted as "l". The value of l ranges from 0 to (n-1).

3. Magnetic Quantum Number: This number describes the orientation of the orbitals in space. It is denoted as $m_l$. The value of $m_l$ ranges from $(-l\text{ to }+l)$.

We are given:

n = 2 which means,

Value of l = 0 to (2 - 1) = 0, 1

Value of $m_l=-l\text{ to }+l=-1\text{ to }+1=-1,0,+1$

Hence, the correct answer is -1, 0, 1.

Answer 2

Answer:

The correct set of values of m for one of the subshells is -1,0,1.

Explanation:

The "Principal quantum number" (n) represents the number of shells (levels) that an atom has where the electrons has the higher probability to be find.

The "Magnetic quantum number" (m) represents the orientation of the electrons in a subshell (s, p, d, f). The number it takes depends on the location of the electron in that subshell.

Remeber that each shell (level) has specific subshells and a specific number of electrons to be placed. For example, shell number 1 has only s subshell, shell number 2 has s subshell and p subshell, shell number 3 has s, p and d subshells and so on (you can check this in a Moeller's Diagram).

In this case, the principal quantum number n is 2, so it has the s subshell and the p subshell. You can see this in the attachment.

S subshell has only 1 orbital (space for two electrons), that means that the electrons on it have only one type of orientation, that's why the magnetic quantum number can be equal 0.

P subshell has 3 orbitals (space for six electrons), that means that the electrons on it could have 3 types of orientation and that's why the magnetic quantum number could be -1, 0 or 1 depending on where orbital the electrons are placed.

So, for n=2, the magnetic quantum number has the value 0 for the s subshell, and it has the set of values -1,0,1 for the p subshell.