Graded Assignment 6-Chapters 7, 8; Due Tuesday November 27, 2012
1.For a principle quantum number, n=4 ,what is the total
number of orbitals permitted?
2. How many electrons can be placed in n=1 shell?
3. How many electrons can be placed in the n=3 shell?
4.How many orbitals are there in a 5d subshell?
5.How many orbitals are there in a 7s subshell?
6. How many electrons can be placed in the 5f subshell?
7. How many electrons can be placed in a 3p subshell?
8.What is the maximum number of orbitals with n=3, l=2
9. What is the maximum number of electrons with n=4, l=3
10. What is the maximum number of orbitals with n=5, l=1
11. What is the maximum number of electrons with n=2, l=0
12. Which orbitals cannot exist?
a. 2p
b. 3p
c. 4d
d. 3f
e. 6s f. 2d
13.Circle the set of quantum numbers that is allowed?
a. n = 6, l=0, ml=0, ms=1
b. n= 5, l=3, ml = -3, ms = -1/2
c. n=2, l=2, ml = 0, ms = ½
d. n = 3, l=1, ml = -2, ms = 1/2
14. Which of the following quantum numbers represents a 6p electron?
a. n = 6, l=0, ml=0, ms=-1/2
b. n= 6, l=5, ml = -3, ms = -1/2
c. n=6, l=1, ml = 0, ms = ½
d. n = 6, l=2, ml = -2, ms = 1/2
15. How many electrons can have the quantum numbers n=5, l=3, ml = 0?
Graded Assignment 6-Chapters 7, 8; Due Tuesday November 27, 2012
16. How many electrons can have the quantum numbers n=5, l=3, ml = 0, ms = 1/2?
17. Pick the smallest atom of the set: Te-2, Ba+2, I-, Cs+, Sr+2, Se-2?
18. Which of the following atoms would you expect to have the highest first ionization energy:
Te, Br, Sb, Se, Cl?
19. (12 points)Name the orbitals defined by the following quantum numbers:
a. n =6, l= 2, ml = 0
b. n = 2, l=1, ml = 1
c. n = 4, l = 3, ml = -1
d. n = 5, l = 0, ml = 0
20. ( 24 points) Write the condensed electron configurations for the following:
b. Cr+3
a. Cr
c. Cs+
d. Ga
e. Se-2
h. Te
21. (10 points) Write all the quantum numbers for a 5d electron?
f. Ga+3
g. Sr