Easy
The $p_x$ orbital can accommodate:
- A$4$ electrons
- B$6$ electrons
- C$2$ electrons with parallel spins
- D$2$ electrons with opposite spins
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Similar Questions
Describe the orbitals with the following quantum numbers using $s, p, d, f$ notations:
$(a) \ n = 2, l = 1$
$(b) \ n = 4, l = 0$
$(c) \ n = 5, l = 3$
$(d) \ n = 3, l = 2$
$(a) \ n = 2, l = 1$
$(b) \ n = 4, l = 0$
$(c) \ n = 5, l = 3$
$(d) \ n = 3, l = 2$
Medium
View SolutionValues of the four quantum numbers for the last electron in the atom are $n = 4, l = 1, m = +1$ and $s = -1/2$. Atomic number of the atom will be
Medium
View SolutionWhat are the electronic configurations of elements with atomic numbers $Z = 117$ and $Z = 120$?
Easy
View SolutionIn $Sr$ $(Z=38)$, the number of electrons with $l=0$ is $x$, and the number of electrons with $l=2$ is $y$. The value of $(x-y)$ is equal to:
($l=$ Azimuthal quantum number)
($l=$ Azimuthal quantum number)
The number of angular and radial nodes of $4d$ orbital respectively are
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