The element with quantum numbers n=2, l=1, m=1, s=-1/2 has the following position in the periodic table

Options

A. Group VII-A, period II
B. Group 0, period II
C. Group VII-A, period III
D. Group 0, period III

Answer

A

Explanation

Quantum numbers n = 2 & l = 1 means the last electron is in 2p orbital. So the element belongs to period 2. Magnetic quantum number `m=+1` means that the electron can be in `p_(x)orp_(y)` orbital. Also any electron can take the value of spin quantum number as `+1//2or-1//2`.
Hence possible electronic configurations are :
`underset("Group IIIA")(1s^(2),2s^(2),2p^(1))," "underset("Group IVA")(1s^(2),2s^(2),2p^(2))," "underset("Group VIA")(1s^(2),2s^(2),2p^(4)),orunderset("Group VIIA")(1s^(2),2s^(2),2p^(5))`
From the given options only option (a) is possible.