Total number of electrons in Cu atom having m | vedclass

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(B) The electronic configuration of $Cu$ $(Z=29)$ is $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \ 4s^1 \ 3d^{10}$.For $s$-orbitals $(l=0)$,$m_l$ is always $0$.

Vedclass · Accepted Answer

$13$

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(B) The electronic configuration of $Cu$ $(Z=29)$ is $1s^2 \ 2s^2 \ 2p^6 \ 3s^2 \ 3p^6 \ 4s^1 \ 3d^{10}$.For $s$-orbitals $(l=0)$,$m_l$ is always $0$. There are $2$ electrons in $1s$,$2$ in $2s$,$2$ in $3s$,and $1$ in $4s$.For $p$-orbitals $(l=1)$,$m_l$ values are $-1, 0, +1$. Each $p$-subshell has $6$ electrons,so $2$ electrons have $m_l=0$ in each ($2p$ and $3p$).For $d$-orbitals $(l=2)$,$m_l$ values are $-2, -1, 0, +1, +2$. In a filled $3d^{10}$ subshell,$2$ electrons have $m_l=0$.Total electrons with $m_l = 0$ are: $2 (1s) + 2 (2s) + 2 (2p) + 2 (3s) + 2 (3p) + 1 (4s) + 2 (3d) = 13$.

List-$A$	List-$B$
$(1)$ Principal quantum number	$(A)$ Shape of the orbital
$(2)$ Azimuthal quantum number	$(B)$ Spin of the electron
$(3)$ Magnetic quantum number	$(C)$ Orientation of the orbital in space
$(4)$ Spin quantum number	$(D)$ Size of the orbital

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

Total number of electrons in $Cu$ atom having $m_l = 0$.

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