Medium
Which one of the following sets of quantum numbers represents an impossible arrangement?
- A$n = 3, l = 2, m_l = -2, m_s = +1/2$
- B$n = 4, l = 0, m_l = 0, m_s = +1/2$
- C$n = 3, l = 2, m_l = -3, m_s = +1/2$
- D$n = 5, l = 3, m_l = 0, m_s = -1/2$
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Similar Questions
The maximum number of orbitals present in $n=4$ energy level of an atom and the maximum number of electrons with spin value $+\frac{1}{2}$ in the same orbitals are, respectively.
Which of the following represents the correct set of four quantum numbers for a $4d$ electron?
Easy
View SolutionWhich of the following are correct?
$(1)$ Electron density in $XY$ plane for $d_{x^2-y^2}$ orbital is zero.
$(2)$ The energy of $3p$-orbital is higher than the energy of $2p$-orbital.
$(3)$ $3p_z$-orbital has one angular node.
$(4)$ $4f$-orbital has no radial node.
$(1)$ Electron density in $XY$ plane for $d_{x^2-y^2}$ orbital is zero.
$(2)$ The energy of $3p$-orbital is higher than the energy of $2p$-orbital.
$(3)$ $3p_z$-orbital has one angular node.
$(4)$ $4f$-orbital has no radial node.
Explain $(n + l)$ rules for the energy of an orbital with an example.
Medium
View SolutionHow is the angular node determined? State the number of angular nodes for $s, p, d,$ and $f$ orbitals.
Easy
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