## How many electrons in an atom could have these sets of quantum numbers?

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1. What number of electrons in an atom could have these arrangements of quantum numbers?

(a) n= 2

(b) n= 4 l= 1

(c) n= 6 l= 3 ml= – 1

Quantum Numbers:

The quantum quantities of an electron speak to its shell, subshell, orbital, and turn in a particle.

Just certain estimations of the quantum numbers are conceivable, and the estimations of one quantum number are reliant on the estimation of the other one.

(a) n=2n speaks to the second shell of the iota which has two subshells; s− and p-subshells.

The ss-subshell has just a single orbital while the p-subshell has three orbitals.

In this manner, an aggregate of four orbitals are available which can contain a limit of 4×2 = 8 electrons. So eight electrons can have this quantum number.

(b)n=4, l=1designate the pp-subshell of the fourth shell which contains three 4p-orbitals. Accordingly, 3×2= 6 electrons can have this arrangement of quantum numbers.

(c) n=6,l=3,ml=−1 speaks to the ff-orbital of the 6f-subshell in the 6th shell.

Accordingly, there must be two electrons having this arrangement of quantum numbers.