October 23

Hi Class,

We are using the same PowerPoint from last class (see October 19). We learned about the first 4 quantum numbers, and how to determine what they are:



1st Quantum Number: Principle Quantum number (n)- Energy Level, Whole number integer ranging from 1 to infinity



2nd Quantum number (L) ranges from zero to (n-1): Each numerical value corresponds to a letter, a shape and a maximum number of electrons



0 = s : 2 electrons maximum- This subshell is spherical

1 = p: 6 electrons maximum- This subshell is dumbbell shaped

2 = d: 10 electrons maximum- This subshell has 4 cloverleaf shaped orientations, and one that resembles a dumbbell with a doughnut.

3= f: 14 electrons maximum - This subshell has a shape that is not easy to depict in pictures.



3rd Quantum number (m l) -ranges from -l to +l



4th Quantum number (m s) - is either -1/2 or +1/2



Homework:

1. Give the values of n, ℓ, mℓ and ms for every orbital with n = 6.
2. Indicate whether the set of quantum numbers (n, ℓ, mℓ) exits or not.
a. 1, 1, 0
b. 5, 4, –3
c. 3, 2, –3
d. 6, 7, +7
e. 8, 1, 0
f. –2, 1, +1
g. 4, 2, –1
h. 7, 3, +4

3. Draw the shapes (including the orientation) of all the s, p and d orbitals.

4. Which orbital in each of the following pairs is higher in energy?
a. 5s or 5d
b. 4s or 3p
c. 6s or 4d

5. What is the maximum number of electrons in an atom that can have these quantum numbers?
a) n = 2
b) n = 3,
c) n = 3, l = 1
d) n = 4, l = 2
e) n = 5, l= 3, ml=3