Fall CHEM 110
-----------------------------------------------------------------------------------------------------------1. What is the maximum number of electrons that can have n = 3 and ms = + ½ ?
-----------------------------------------------------------------------------------------------------------2. Consider the highest energy electron in the ground state of Mg. Which of the following
orbitals would this electron be in? Give the subshell designation (e.g., 2p, 1s, 3d, etc.).
-----------------------------------------------------------------------------------------------------------3. Which of the following could not be an orbital diagram for an atom in its ground state?
1s
A. (⇅)
B. (⇅)
2s
(⇅)
2p
(⇅) (↑) (↑)
3s
(⇅)
(⇅) (⇅) (⇅)
(↑)
C. (⇅)
D. (⇅)
(⇅)
(⇅)
(⇅) (⇅) ( )
(⇅) (⇅) (⇅)
(⇅)
E. (⇅)
(⇅)
(↑) (↑) (↑)
-----------------------------------------------------------------------------------------------------------4. The following represent electron excited states (What is the difference between excited and
ground states?). Determine the element and write the ground-state condensed electron
configurations for the following:
(a) 1s22s23p24p1
(b) [Kr] 4d65s25p1.
-----------------------------------------------------------------------------------------------------------5. Which of the following would have to lose two electrons in order to achieve a noble gas
electron configuration?
O
Sr
Na
Se
Br
A.
O, Se
B.
Sr
C.
Na
D.
Br
E.
Sr, O, Se
-----------------------------------------------------------------------------------------------------------6. How many unpaired electrons on there in the ground state electron configuration of Fe+3
------------------------------------------------------------------------------------------------------------
Recitation 4
Fall CHEM 110
-----------------------------------------------------------------------------------------------------------7. Consider the following statements as they apply to Na+, O2− and F−. Determine if it is true or
false and explain why.
A. Na+, O2− and F− are an isoelectronic series.
B. When Na+ forms Na2+, it has a greater ionization energy than when O2− forms O− and
F− forms F.
C. Comparing valence electrons of all three, a valence electron in O2− experiences the
least effective nuclear charge.
D. All three species have a filled quantum level n = 2.
E. F− has the smallest radius.
-----------------------------------------------------------------------------------------------------------8. What is electron affinity? Which of the following reactions shows the electron affinity process?
A. Cl (g) → Cl+ (g) + e−
B. Cl−(g) → Cl (g) + e−
−
−
C. Cl (g) + e → Cl (g)
D. Cl (g) + e− → C+ (g)
-----------------------------------------------------------------------------------------------------------9. Which one of the following ions has the smallest radius?
A. Mg2+
C. Be2+
B. N3−
D. Li+
----------------------------------------------------------------------------------------------------------10. The sequential ionization energies of an element are plotted in the figure. Which of the
following is MOST likely to be the element?
A.
B.
C.
D.
E.
Li
Be
B
C
N
------------------------------------------------------------------------11. Which of these compounds is not ionic?
A.
NaCl
B.
BaCl2 C.
CsF D.
SF6
----------------------------------------------------------------------------------12. Which of these are molecular?
i.
H 2O
ii.
HCl
iii.
HNO3
iv.
Na2SO4
----------------------------------------------------------------------------------------------------------13. Rank the following compounds from smallest to largest lattice energy? (Lowest to highest
melting point?)
CaO, CsI, BaS, NaF, NaCl
-----------------------------------------------------------------------------------------------------------
Recitation 4