Question

An electron is present in 4f subshell. Find the possible values of n,l and m

Answer 1

Here is your Answer:

n- Principal Quantum no.(n=1,2,3....)

l - Azimuthal Quantum no.(s=0, P=1,d=2, f=3)

m- magnetic Quantum no.(-l,0+l)

So in 4f

n=4

l=3

m= -3,-2,-1,0,+1,+2,+3

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Answer 2

The values of all the quantum numbers for 4f subshell is, n = 4, l = 3, $m_l=-3,-2,-1,0+1,+2,+3$

Explanation :

Principle Quantum Numbers : It describes the size of the orbital. It is represented by n. n = 1,2,3,4....

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

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.

Now we have to calculate the values of all the quantum numbers for 4f subshell.

For 4f :

n = 4       (Because it is in 4th shell)

l = 3         (Because it is in 'f' orbital)

$m_l=-3,-2,-1,0+1,+2,+3$     (Because l = 3)

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