Question

which of the following are possible values of N L and M for an atom having maximum value of m=+2​

Answer 1

Answer: The possible value of n will be 3, l will be 0, 1, 2 and m will be -2, -1, 0, +1, +2.

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.

If maximum value of m is +2, the possible values will be m will be -2, -1, 0, +1, +2. and l = 2, 1 and 0, The possible value of n will be 3.

Answer 2

Answer:

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Explanation:

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