Easy
Which of the following sets of quantum numbers is impossible for an electron?
- A$n = 1, l = 0, m_l = 0, m_s = +\frac{1}{2}$
- B$n = 9, l = 7, m_l = -6, m_s = -\frac{1}{2}$
- C$n = 2, l = 1, m_l = 0, m_s = +\frac{1}{2}$
- D$n = 3, l = 2, m_l = -3, m_s = +\frac{1}{2}$
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The following sets of quantum numbers represent four electrons in an atom:
$(i)$ $n = 4, l = 1$ $(ii)$ $n = 4, l = 0$
$(iii)$ $n = 3, l = 2$ $(iv)$ $n = 3, l = 1$
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$(i)$ $n = 4, l = 1$ $(ii)$ $n = 4, l = 0$
$(iii)$ $n = 3, l = 2$ $(iv)$ $n = 3, l = 1$
The sequence representing the increasing order of energy is:
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