Group Activity- 4 Quantum numbers and electron configurations
Name _______________________
Group Members: _________________________________
1. State the number of electrons described by the following quantum numbers
a. n = 3, l = 0
b. n = 3, l = 1
c. n = 3, l = 2, ml = -1
d. n = 5, l = 0, ml -2, ms -1/2
2. Give the n and l values for the following orbitals:
a. 1s
b. 2d
c. 3d
d. 6d
e. 5p
3. How many possible orbitals are there
a. n = 4
b. n = 2
c. n = 3
d. n = 5
4. Write the complete set of quantum numbers that represent the valence electrons for the following elements:
a. Sodium
b. Bromine
5. Fill in the blanks
a. The subshell with the quantum numbers n=4, l=2 is _____________________.
b. The ml values for a d orbital are ____________________________.
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d. The allowed values of l for the shell with n=2 are ________________________________.
e. The allowed values of l for the shell with n=4 are ____________________________.
f. The number of orbitals in a shell with n=3 is _______________________________
g. The number of orbitals with n=3 and l=1 is _________________________________.
h. The maximum number of electrons with quantum numbers with n=3 and l=2 is __________________.
i. When n=2, l can be _______________________________________________.
j. When n=2, the possible values for ml are ________________________________________.
k. The number of electrons with n=4, l=1 is _________________________________.
l. The subshell with n=3 and l=1 is designated as the ________________________ subshell.
m. The lowest value of n for which a d subshell can occur is n=______________________________.
Write the ground state noble gas electron configuration for each neutral atom. Indicate the outer
electrons and the core electrons.
1.
Na
2. Pb
3. Sr
4. U
5. N
6. Ag
7. Ti
8. Ce
9. Cl
10. Hg
Write a noble gas electron configuration with equations for each ion’s formation. State whether they
are diamagnetic or paramagnetic
1.
Na+
2. Pb2+
2
3. In3+
4. In+
5.
Mn+4
Rank the following in terms of increasing atomic radii
P, N, Sr, Al, Cr, Mn, K, O
Rank the following in terms of decreasing ionization energy
P, N, Sr, Al, Cr, Mn, K, O
Rank the following in terms of increasing ionic radii
K+
O2- F-
I-
Rb
Rb+
Rank the following in terms of increasing ionic radii
Fe+
O2- Fe+2
Fe +3
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