# Chemistry

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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

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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 n-1.

ml = - ell to + ell in whole numbers;i.e., if ell is 2 then ml can be -2,-1,0,+1,+2.

ms 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, ml CANNOT be 3 because ml may take values from -l to +l (in whole numbers) which will allow -2,-1,0,+1,and +2 but not +3.

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4 and 5

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