Question

Indicate which of the following sets of three quantum numbers are wrong and explain why they are wrong:
(a) 4, 1, 0
(b) 3, 3, +2
(c) 2, 1, 0
(d) 2, 1, +2
(e) 1, 0, 0

Answer 1

(b) 3, 3, +2  

Explanation:

Of all the given options, B is wrong. A set of quantum numbers cannot be given as  3, 3, +2. The given numbers are for:

1. Prinicipal quantum number(n)
2. Azimuthal quantum number(l) which is l = n-1
3. Magnetic quantum number

• According to Pauli's exclusion principle "no two electrons in an atom can have the same set of the four quantum numbers". This principle indicates that no two electrons in the same orbital can spin in the same direction.
• The value 3, 3, +2 is a violation of this rule. Here the principal quantum number and the azimuthal quantum numbers are the same.

Learn more:

Gold foil experiment https://brainly.com/question/1542931

atomic orbitals https://brainly.com/question/9288609

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