Solution Found!
How many electrons in an atom can have each of the
Chapter 8, Problem 11P(choose chapter or problem)
How many electrons in an atom can have each of the following quantum number or sublevel designations?
(a) n = 2, l= 1, ml = 0
(b) 5p
(c) n = 4,l = 3
Questions & Answers
QUESTION: Problem 11P
How many electrons in an atom can have each of the following quantum number or sublevel designations?
(a) n = 2, l= 1, ml = 0
(b) 5p
(c) n = 4,l = 3
ANSWER:
Solution 11P:
Here, we are going to find out the total number of electrons in each orbital.
Step 1:
There are four quantum numbers.
The Principal Quantum Number (n):
The principal quantum number determines the overall size and energy of an orbital. It is an integer.
The possible values are n = 1, 2, 3,..
The Angular Momentum Quantum Number (l): The angular momentum quantum
determines the shape of the orbital. The possible values of l are 0, 1, 2,...., (n - 1).
The Magnetic Quantum Number (ml): The magnetic quantum number specifies the orientation of the orbital. The values of ml will be -l to +l.
The Spin Quantum Number (ms): The spin quantum number specifies the orientation of
the spin of the electron. For an electron the ms =+½ or -½
Therefore,
Value of l |
orbital |
0 |
s |
1 |
p |
2 |
d |
3 |
f |