Question

For l = 2, value of m cannot be​

Answer 1

Answer:

Possible

m

l

values are

−

2

,

−

1

,

0

,

1

,

2

. See below.

Explanation:

There are four quantum numbers: the principle quantum number,

n

, the angular momentum quantum number,

l

, the magnetic quantum number,

m

l

, and the electron spin quantum number,

m

s

. For this question we are concerned with

l

and

m

l

.

The angular momentum quantum number,

l

, describes the shape of the subshell and its orbitals, where

l

=

0

,

1

,

2

,

3

...

corresponds to

s

,

p

,

d

,

and

f

subshells (containing

s

,

p

,

d

,

f

orbitals), respectively. Each shell has up to

n

−

1

types of subshells/orbitals.

An angular momentum quantum number of

l

=

2

describes a

d

subshell.

I HOPE MY ANSWER WILL HELP YOU...

Answer 2

Answer:

l=2

so the value of m can be -2,-1,0,1,2

You haven't given the options so choose the who has not value from 2,-1,0,1,2

Thank You

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