Quantum Guide 4th
Quantum Guide 4th
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Chemistry Orbital Help!?
Having trouble with chemistry orbitals on my study guide. Please help points to most helpful.
1. How many orbitals (if any) are defined by each of the following sets of quantum numbers?
a. n=6
b. n=4, l=0
c. n=3, l=2, ml=0
d. n=4, l=1, ml=-2
and
2. What is the maximum number of electrons (if any) that can be defined by each of the following sets of quantum numbers?
a. n=6
b. n=4, l=0
c. n=3, l=0, ml=0
d. n=4, l=2, ml=3
e. n=2, l=1, ml=-1, ms=-1/2
Thanks
1a If you have energy level n, then you can have n-squared orbitals for that principal quantum number. if n=6, then you have 36 possible orbitals.
If l = 0 it's an s orbital
If l=1 it's a p orbital (Thee are 3 types of p)
If l = 2 it's a d orbital (There are 5 types of d)
If l=3 it's an f orbital (There are 7 types of f)
1b If n=4 and l=0, you can only have one orbital. It is called the 4s orbital.
1c If n=3 and l=2 and ml = 0, you can only have one orbital. This is referring specifically to ONE of the five 3d orbitals.
1d If n=4 and l=1, this should be a 4p orbital. But the rules for ml say that ml should fall between + or - the value of l. Therefore this set of quantum numbers is not allowed because ml = -2, which falls outside the range of -1, 0, +1. There is NO orbital possible for this set of quantum numbers.
The maximum number of electrons that can fit in an orbital is 2. One of them will have ms = +1/2 and the other electrons will have ms = -1/2
2a Maximum # of electrons = 72 (2 x n-squared)
2b Maximum # of electrons = 2 (in a 4s orbital)
2c Maximum # of electrons = 2 (in a 3 s orbital)
2d Maximum # of electrons = zero (This set of numbers is wrong)
2e Maximum # of electrons = 1 (in a 2p orbital. The other electron would have ms = +1/2)