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Verdich [7]
3 years ago
10

Which of the following is not a valid set of quantum numbers

Chemistry
2 answers:
zhuklara [117]3 years ago
7 0

Answer:  C. n = 3, l = 3, m = 3

Explanation:

1. Principle Quantum Numbers: This quantum number describes the size of the orbital. It is represented by n. n = 1,2,3,4....

2. Azimuthal Quantum Number: This quantum number describes the shape of the orbital. It is represented as 'l'. The value of l ranges from 0 to (n-1). For l = 0,1,2,3... the orbitals are s, p, d, f...

3. Magnetic Quantum Number: This quantum number describes the orientation of the orbitals. It is represented as m_l. The value of this quantum number ranges from (-l\text{ to }+l). When l = 2, the value of m_l will be -2, -1, 0, +1, +2.

A.  n = 2, l = 1 , m = 0 is possible.

B. n = 1, l = 0, m = 0   is possible.

C. n = 3, l = 3, m = 3 is not possible as for n = 3, l = 0, 1 and 2 and m = 0,+1, +2, -1 and -2.

ASHA 777 [7]3 years ago
3 0
I believe the answer is C, n = 3, l = 3, m = 3. The magnetic quantum number, or 

<span>ml</span>, can only take values that range from <span>−l</span> to <span>+l</span>, as you can see in the table above.

For option C), the angular momentum quantum number of equal to ++2<span>, which means that <span>ml</span> can have a maximum value of </span>+2<span>. Since it is given as having a value of </span>+3**, this set of quantum numbers is not a valid one.

The other three sets are valid and can correctly describe an electron.

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