MCQ
Quantum No. $l = 2$ and $m = 0$ represent which orbital :
- A$d_{xy}$
- B$d_x^2 - y^2$
- ✓$d_z^2$
- D$d_{zx}$
✓
Answer
Correct option: C.
$d_z^2$
c
Quantum numbers $1=2$ and $m =0$ represent $d _{z^2}$ orbital.
Quantum numbers $1=2$ and $m =0$ represent $d _{z^2}$ orbital.
Note: For $s,p,d$ and $f$ orbitals, the value of the azmithual quantum number $'l'$ is $0,1,2,3$
When $l=2$, $m$ can have values $-2,-1,0,+1,+2$.
A $d$-subshell can have five different orientations and orbitals corresponding to these orientations are $d _{ xy }, d _{ xz }, d _{ yz }, d _{ x ^2- y ^2} d _{ z ^2}$
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