Question

How many electrons can be held in a sublevel l = 3?

Answer 1

Answer : The number of electrons held in sub-level l = 3 can be, 14 electrons

Explanation :

Azimuthal Quantum Number : It describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3... the orbitals are s, p, d, f...

Magnetic Quantum Number : It describes the orientation of the orbitals. It is represented as $m_l$. The value of this quantum number ranges from $(-l\text{ to }+l)$. When l = 2, the value of $m_l$ will be -2, -1, 0, +1, +2.

Spin Quantum number : It describes the direction of electron spin. This is represented as $m_s$ The value of this is $+\frac{1}{2}$ for upward spin and $-\frac{1}{2}$ for downward spin.

As we are given that,

$l=3$

$m_l=-3,-2,-1,0,1,2,3$

$m_s=+\frac{1}{2}\text{ and }-\frac{1}{2}$  (For each sub-shell)

From this we conclude that, there are 7 orbitals and each orbital contains 2 electrons. So, the number of electrons held in sub-level l = 3 are, $7\times 2=14$ electrons.

Hence, the number of electrons held in sub-level l = 3 can be, 14 electrons

Answer 2

There can be two electrons in one orbital maximum. The s sublevel has just one orbital, so can contain 2 electrons max. The p sublevel has 3 orbitals, so can contain 6 electrons max. The d sublevel has 5 orbitals, so can contain 10 electrons max.

Hope this helped
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