The sublevel designation, the allowable ml values, and the number of orbitals are,
For ,n = 2, l = 0 ⇒ sublevel s, ⇒ ml = 0, number of orbitals = 1
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How to calculate electron quantum numbers? </h3>
The rules for electron quantum numbers are:
1. Shell number, 1 ≤ n,
2. Subshell number, 0 ≤ l ≤ n − 1, from s, p, d, f, g, h...
3. Orbital energy shift, -l ≤ ml ≤ l
4. Spin, either -1/2 or +1/2
- So,(a) n = 2, l = 0 ⇒ sublevel s
-l ≤ ml ≤ l ⇒ ml = 0
number of orbitals = 1
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What are quantum numbers?</h3>
Quantum numbers describe the location of a specific electron within a nucleus. One of four quantum numbers can be used to define each electron in an atom. M S, N, L, M 1, and L A set of rules determines the possible values that can be assigned to each integer.
The position and energy of an electron in an atom are expressed using a set of numbers known as quantum numbers. The four classifications of quantum numbers are: fundamental, azimuthal, magnetic, and spin kinds. Quantum numbers are used to indicate the values of the conserved quantities in a quantum system.
To know more about quantum numbers, refer:
brainly.com/question/5927165
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