Easy
Which of the following sets of quantum numbers is not possible for an electron?
- A$n=3, l=1, m=0, s=+\frac{1}{2}$
- B$n=4, l=0, m=0, s=-\frac{1}{2}$
- C$n=3, l=3, m=-3, s=+\frac{1}{2}$
- D$n=1, l=0, m=0, s=-\frac{1}{2}$
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View SolutionGiven below are two statements. One is labelled as Assertion $A$ and the other is labelled as Reason $R$.
Assertion $A$ : Energy of $2s$ orbital of hydrogen atom is greater than that of $2s$ orbital of lithium.
Reason $R$ : Energies of the orbitals in the same subshell decrease with increase in the atomic number.
In the light of the above statements,choose the correct answer from the options given below.
Assertion $A$ : Energy of $2s$ orbital of hydrogen atom is greater than that of $2s$ orbital of lithium.
Reason $R$ : Energies of the orbitals in the same subshell decrease with increase in the atomic number.
In the light of the above statements,choose the correct answer from the options given below.
The correct order of decreasing energy for the electrons whose quantum numbers $n$ and $l$ are given below,is
$A$. $n=5, l=2$
$B$. $n=5, l=0$
$C$. $n=4, l=3$
$D$. $n=4, l=1$
$A$. $n=5, l=2$
$B$. $n=5, l=0$
$C$. $n=4, l=3$
$D$. $n=4, l=1$
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