Medium
If an electron has a spin quantum number of $+ \frac{1}{2}$ and a magnetic quantum number of $- 1$,it cannot be present in an
- A$d$-orbital
- B$f$-orbital
- C$p$-orbital
- D$s$-orbital
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Similar Questions
Find the exact orbital from the following for which $n=4$ and $l=1$.
Using $s, p, d, f$ notations,describe the orbital with the following quantum numbers:
$(a) n=2, l=1$
$(b) n=4, l=0$
$(c) n=5, l=3$
$(d) n=3, l=2$
$(a) n=2, l=1$
$(b) n=4, l=0$
$(c) n=5, l=3$
$(d) n=3, l=2$
Medium
View SolutionThe sum of electrons present in all subshells of an atom with $m_s$ value of $+\frac{1}{2}$ for $n=4$ and $m_s$ value of $-\frac{1}{2}$ for $n=3$ is
The magnetic quantum number for an electron when the value of principal quantum number is $2$ can have ............ values.
Medium
View SolutionThe number of orbitals with $n = 5, m_{l} = +2$ is $......$ . (Round off to the Nearest Integer)
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