Chemistry
posted by Anonymous on .
The principal quantum number, n, describes the energy level of a particular orbital as a function of the distance from the center of the nucleus. Additional quantum numbers exist to quantify the other characteristics of the electron. The angular momentum quantum number (§¤), the magnetic quantum number (m§¤), and the spin quantum number (ms) have strict rules which govern the possible values. Identify allowable combinations of quantum numbers for an electron. Select all that apply.
n=3 l=1 ml=0 ms=+1/2
n=4 l=2 ml=3 ms=1/2
n=3 l=0 ml=0 ms=+1/2
n=2 l=1 ml=0 ms=1
n=4 l=4 ml=0 ms=+1/2
n=5 l=1 ml=1 ms=1/2

Here are the rules.
n can be any whole number over zero; i.e., 1, 2, 3, 4, etc.
l ("ell") can be any whole number beginning with zero, 1, 2, 3, etc with a maximum of n1.
m_{l} =  ell to + ell in whole numbers;i.e., if ell is 2 then m_{l} can be 2,1,0,+1,+2.
m_{s} may have two values only; i.e., +1/2 or 1/2
Your job is to take these rules and apply them to each of the above and find those that are allowed. To give you a fast start
#1 is allowed.
#2 is not allowed. Why not? If N is 4, then l CAN be 2 (l can have values in this case of 0,1,2,3) so 2 is allowed. However, m_{l} CANNOT be 3 because m_{l} may take values from l to +l (in whole numbers) which will allow 2,1,0,+1,and +2 but not +3. 
4 and 5

hjgtgy