Which of the following arrangements shows the | vedclass

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(B) To determine the paramagnetism,we look at the number of unpaired electrons in the ground state of each atom:$1. 	ext{Oxygen } (O): 1s^2 2s^2 2p^4

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$N > O > Al > Ca$

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(B) To determine the paramagnetism,we look at the number of unpaired electrons in the ground state of each atom:$1. 	ext{Oxygen } (O): 1s^2 2s^2 2p^4$. The $2p$ subshell has $2$ unpaired electrons.$2. 	ext{Nitrogen } (N): 1s^2 2s^2 2p^3$. The $2p$ subshell has $3$ unpaired electrons.$3. 	ext{Aluminum } (Al): [Ne] 3s^2 3p^1$. The $3p$ subshell has $1$ unpaired electron.$4. 	ext{Calcium } (Ca): [Ar] 4s^2$. All electrons are paired,so it is diamagnetic ($0$ unpaired electrons).Comparing the number of unpaired electrons: $N (3) > O (2) > Al (1) > Ca (0)$.Therefore,the correct order of decreasing paramagnetism is $N > O > Al > Ca$.

Column-$I$	Column-$II$
$(a)$ $4s$	$(p)$ Circular orbit around nucleus
$(b)$ $4p$	$(q)$ Non-directional orbital
$(c)$ $1s$	$(r)$ Angular momentum $= 2h/\pi$
$(d)$ $3d$	$(s)$ Radial node is zero

Which of the following arrangements shows the correct order of decreasing paramagnetism?

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Match the columns and choose the correct option:

Column-$I$ Column-$II$

$(a)$ $4s$ $(p)$ Circular orbit around nucleus

$(b)$ $4p$ $(q)$ Non-directional orbital

$(c)$ $1s$ $(r)$ Angular momentum $= 2h/\pi$

$(d)$ $3d$ $(s)$ Radial node is zero

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