the atomic number of coblt is 27 and find the outer most shell
Answers
Answer:
The number of electrons each energy level can hold increases as you add more and more energy levels to an atom.
The relationship that exists between the energy level,
n
, and the number of electrons it can hold can be written like this
∣
∣
∣
∣
¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯
a
a
no. of e
−
=
2
n
2
a
a
∣
∣
−−−−−−−−−−−−−−−−−−
You can use this equation to find the maximum number of electrons that can be added to each energy level. You will have
the first energy level,
n
=
1
no. of e
−
=
2
⋅
1
2
=
2 e
−
the second energy level
n
=
2
no. of e
−
=
2
⋅
2
2
=
8 e
−
the third energy level,
n
=
3
no. of e
−
=
2
⋅
3
2
=
18 e
−
the fourth energy level,
n
=
4
no. of e
−
1
=
2
⋅
4
2
=
32 e
−
and so on.
In your case, cobalt,
Co
, is said to have a total of
27
electrons surrounding its nucleus. These electrons will be placed in orbitals in order of increasing energy in accordance to the Aufbau Principle.
http://www.chemguide.co.uk/atoms/properties/atomorbs.html
http://www.chemguide.co.uk/atoms/properties/atomorbs.html
Now, it's very important to remember that when you're adding electrons to an atom, the 3d-orbitals, which are located on the third energy level, are higher in energy than the 4s-orbital.
This means that you must fill the 4s-orbital first, then distribute the rest of the electrons to the 3d-orbitals.
So, a neutral cobalt atom will have
n
=
1
→
2 e
−
in the
1
s
subshell
n
=
2
→
8 e
−
in the
2
s
and
2
p
subshells
Now, these two energy levels will hold
2 e
−
+
8 e
−
=
10 e
−
Now comes the tricky part. The third energy level can hold
18 e
−
, so in theory it can hold the remaining
27 e
−
−
10 e
−
=
17 e
−
that the neutral cobalt atom has. You could thus say that
n
=
3
→
17 e
−
in the
3
s
,
3
p
, and
3
d
subshells
and conclude that the electrons that surround the nucleus of a cobalt atom are spread out on
3
energy levels. You would be wrong.
Taking it one subshell at a time, you will have
2 e
−
→
in the
3
s
subshell
6 e
−
→
in the
3
p
subshell
You now have
17 e
−
−
(
2 e
−
+
6 e
−
)
=
9 e
−
to distribute. Because the 4s orbital is filled before the 3d-orbitals, the next two electrons are going to be distributed on the fourth energy level
n
=
4
→
2 e
−
in the
4
s
subshell
The remaining
7 e
−
will now be distributed in the 3d-subshell.
Therefore, a neutral cobalt atom will have
n
=
1
→
2 e
−
in the
1
s
subshell
n
=
2
→
8 e
−
in the
2
s
and
2
p
subshells
n
=
3
→
15 e
−
in the
3
s
,
3
p
, and
3
d
subshells
n
=
4
→
2 e
−
in the
4
s
subshell
Explanation:
Hope this helps you
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Answer:
The number of electrons each energy level can hold increases as you add more and more energy levels to an atom.
The relationship that exists between the energy level,
n
, and the number of electrons it can hold can be written like this
∣
∣
∣
∣
¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯¯
a
a
no. of e
−
=
2
n
2
a
a
∣
∣
−−−−−−−−−−−−−−−−−−
You can use this equation to find the maximum number of electrons that can be added to each energy level. You will have
the first energy level,
n
=
1
no. of e
−
=
2
⋅
1
2
=
2 e
−
the second energy level
n
=
2
no. of e
−
=
2
⋅
2
2
=
8 e
−
the third energy level,
n
=
3
no. of e
−
=
2
⋅
3
2
=
18 e
−
the fourth energy level,
n
=
4
no. of e
−
1
=
2
⋅
4
2
=
32 e
−
and so on.
In your case, cobalt,
Co
, is said to have a total of
27
electrons surrounding its nucleus. These electrons will be placed in orbitals in order of increasing energy in accordance to the Aufbau Principle.
Explanation:
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