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Chemistry 130 (Lecture VII-VIII)
Answer
1. Which of the following statements is not consistent with a quantum mechanical
view of nature?
a. Matter can be thought of as waves
b. Excited atoms can emit all possible energies
c. Knowing the exact speed of an electron means we do not know anything
about its location in an atom
d. Atomic orbitals correspond to the probability of finding an electron in a
given region of space around the nucleus
2. What is the correct ranking for the energy of the following orbitals from
smallest to largest?
a. 6s < 4f < 5d < 6p
b. 6s < 5d < 4f < 6p
c. 6s < 5f < 5d < 6p
d. 4f < 5d < 6s < 6p
3. Which region of the periodic table would you expect the (yetundiscovered) element #119?
a. s-block
b. p-block
c. d-block
d. f-block
4. Order the following orbitals—3s, 3p, 3d—by increasing shielding ability.
a. 3s < 3p < 3d
b. 3p < 3d < 3s
c. 3s < 3d < 3p
d. 3d < 3p < 3s
5. Identify the orbitals below (i.e., “1s” or “5f”. You may ignore the orientation). Also state
the number and type of nodes present.
i)
ii)
Name:
Name:
Nodes:
Nodes:
6. Answer the following questions with both the atomic symbol and the correct spelling of the
name of the element:
i)
The element in the second period with properties similar to iodine:
Symbol:
ii)
Name:
The alkaline earth metal in the fourth period:
Symbol:
iii)
Name:
The noble gas in the third period:
Symbol:
iv)
Name:
The halogen with the average atomic mass closest to that of arsenic:
Symbol:
Name:
7. State whether each of the following sets of electron quantum numbers are valid. If not, explain
why.
i)
n=3, ℓ= 3, mℓ=0
Circle one:
Valid
Not Valid
Explanation (if necessary):
ii)
n=2, ℓ= 1, mℓ=1
Circle one:
Valid
Not Valid
Circle one:
Valid
Not Valid
Explanation (if necessary):
iii)
n=4, ℓ= 1, mℓ=-2
Explanation (if necessary):
8. What type or orbitals have an angular momentum quantum number of ℓ=2? For a given
principal quantum number, how many orbitals have the quantum number ℓ=2? Using the axes
provided below, draw one example of an orbital with ℓ=2.