The two electrons in the K shell will differ | vedclass

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(D) The $K$ shell corresponds to the principal quantum number $n = 1$.For $n = 1$,the only possible value for the azimuthal quantum number $l$ is $0$

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Spin quantum number

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(D) The $K$ shell corresponds to the principal quantum number $n = 1$.For $n = 1$,the only possible value for the azimuthal quantum number $l$ is $0$ ($s$-orbital).For $l = 0$,the only possible value for the magnetic quantum number $m_l$ is $0$.According to the Pauli exclusion principle,no two electrons in an atom can have the same set of all four quantum numbers.Therefore,the two electrons in the $1s$ orbital must differ in their spin quantum number ($m_s = +1/2$ and $m_s = -1/2$).

Quantum Number	Information
$(1)$ Principal quantum number	$(A)$ Spatial orientation of the orbital
$(2)$ Azimuthal quantum number	$(B)$ Energy and size of the orbital
$(3)$ Magnetic quantum number	$(C)$ Electron spin
$(4)$ Spin quantum number	$(D)$ Shape of the orbital

The two electrons in the $K$ shell will differ in which of the following quantum numbers?

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