How many integer values of magnetic quantum numbers does exist for certain value of l?
Answers
Explanation:
There are 4 quantum numbers which describe an electron in an atom.
These are:
n
the principal quantum number. This tells you which energy level the electron is in.
n
can take integral values 1, 2, 3, 4, etc
l
the angular momentum quantum number. This tells you the type of sub - shell or orbital the electron is in. It takes integral values ranging from 0, 1, 2, up to
(
n
−
1
)
.
If
l
= 0 you have an s orbital.
l
=
1
gives the p orbitals
l
=
2
gives the d orbitals
m
is the magnetic quantum number. For directional orbitals such as p and d it tells you how they are arranged in space.
m
can take integral values of
−
l
...
...
...
...
.
0
...
...
...
...
.
+
l
.
s
is the spin quantum number. Put simply the electron can be considered to be spinning on its axis. For clockwise spin
s
= +1/2. For anticlockwise
s
= -1/2. This is often shown as
↑
and
↓
.
In your question
n
=
3
. Let's use those rules to see what values the other quantum numbers can take:
l
=
0
,
1
and
2
, but not 3.This gives us s, p and d orbitals.
If
l
= 0
m
= 0. This is an s orbital
If
l
= 1,
m
= -1, 0, +1. This gives the three p orbitals. So
m
= 0 is ok.
If
l
= 2
m
= -2, -1, 0, 1, 2. This gives the five d orbitals.
s
can be +1/2 or -1/2.
These are all the allowed values for
n
=
3
Note that in an atom, no electron can have all 4 quantum numbers the same. This is how atoms are built up and is known as The Pauli Exclusion Principle.
Answer:
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