Question

Find the values of quantum no. n,l,m,and s for 2 s electron

Answer 1

The three quantum numbers (n, l, and m) that describe an orbital are integers: 0, 1, .... The number of orbitals in a subshell is therefore 2(l) + 1. ... of these orbitals, there are two allowed values of the spin quantum ...

Answer 2

For 2s :-

Principal Quantum No. = 2

Azimuthal Quantum No. = 0

Magnetic Quantum No. = 0

Spin Quantum No. = +½ or -½

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$\huge\underline{\underline{\sf Extra\: Info:}}$

$\large\underline{\underline{\sf Principal\:Quantum\:No.(n)}}$

$\textsf{It\:is\:represented\:by\: symbol\:(n)}\\ \textsf{It\: represents\:the\:name,size,\:and\:energy\:of\:shell\:to\:which}\\ \textsf{electron\:belongs.}$

• The value of n lies between 1 to infinity .

i.e n = 1, 2, 3, 4 - - - infinity.

$\large\underline{\underline{\sf Azimuthal\: Quantum\:No.(l)}}$

$\textsf{Represented\:by\:"l"}$ $\textsf{It\:represent\:the\:shape\:of\:the\:subshell\:and\: orbital\:and\: orbital\: Angular\: Momentum}$

It's value is between 0 to (n-1)

• l = 0, 1, 2 - - - - (n - 1)

• l = 0 (s Subshell)

• l = 1 (p Subshell)

• l = 2 (d Subshell)

• l = 3 (f Subshell)

$\large\underline{\underline{\sf Magnetic\: Quantum\:No.(m)}}$

$\textsf{Represented\:by\:"m"}$ $\textsf{Value\:of\:m=all\:integral\:value\:from\:-l\:to\:+l\: including\:zero}$

i.e Value of m = - l to + l

$\large\underline{\underline{\sf Spin\: Quantum\:No.(s)}}$

$\textsf{Represented\:by\:"s"}$ $\textsf{It\: represents\:the\: direction\:of\: Electron\: spin\: around\:its\:own\:axis}$