Question

Number of electrons of manganese with magnetic quantum number value 0 is

Answer 1

Answer:

Explanation:

Lets start by writing the electronic configuration of Mn,

Mn: 1s2 2s2 2p6 3s2 3p6 3d5 4s2,

Given that ml(magnetic quantum number) = 0,

Each orbital is represented by 4 quantum numbers i.e of the form (n, l, ml, ms) where n = principal quantum number, l = azimuthal quantum number where l = 0(s orbital), l = 1(p orbital), l = 2(d orbital) and ms = spin quantum number, now lets look at all the orbitals individually to get the answer,

1s2

It has 2 electrons with this configuration (1, 0, 0, ±½)

n=1, l = 0 because this is an s orbital, ml = 0 because ml varies from -l to +l, ms = ±½ because we have 2 electrons,

2s2 (2, 0, 0, ±½),

2p6 (2, 1, -1, ±½), (2, 1, 0, ±½), and (2, 1, +1, ±½),

Here l = 1,

3s2 (3, 0, 0, ±½),

3p6 (3, 1, -1, ±½), (3, 1, 0, ±½), and (3, 1, +1, ±½),

3d5 (3, 2, -2, +½), (3, 2, -1, +½), (3, 2, 0, +½), (3, 2, 1, +½) and (3, 2, 2, +½),

4s2 (4, 0, 0, ±½),

So we have 2 electrons with ml = 0 from 1s2, 2 from 2s2, 2 from 2p6, 2 from 3s2, 2 from 3p6, 1 from 3d5(because 5 electrons are in different d orbitals and not paired) and 2 from 4s2,

Adding them up, there are 13 electrons with ml = 0 in Mn

Answer 2

Explanation:

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