Chem 1711
Name _____________________________________
Quiz 7 (25 points)
1.
2.
3.
Match each equation given below to the appropriate energy term (I – VI). Then indicate whether the sign of the energy
term will be + or − .
energy term
+ or −
a.
Sn+ (g)  Sn2+ (g) + e–
________
________
I.
electron affinity
IV. ΔH°f
b.
MgF2 (s)  Mg2+ (g) + 2 F– (g)
________
________
II.
1st ionization energy
V. lattice energy
c.
F (g) + e–  F– (g)
________
________
III.
2nd ionization energy
VI. bond energy
a.
How many valence electrons does a sulfur atom have?
____________________
b.
Draw the Lewis symbol for an element, X, if it has 3 valence electrons.
____________________
Consider the Pauling electronegativity values (χ) given for the following elements:
Zn (χ=1.6)
Br (χ=2.8)
C (χ=2.5)
S (χ=2.5)
a
Which one of the following bonds is the most polar?
Zn–Br
b.
Zn–S
a.
Zn–S
Br
Ar
B
Ca
Kr
Rb
Ne
Al3+
K+
Rb
Cr
Ar
Ca
S
Which one of the following is the most electronegative?
K
g.
Fe3+
Which one of the following has the largest atomic radius?
I
f.
Ti2+
Cl
Which one of the following species is isoelectric with P3–?
N3–
e.
C–Br
Which one of the following elements has the smallest 1st ionization energy?
O
d.
C–S
Which one of the following has the least favorable electron affinity value?
S
c.
C–Br
Which one of the following is diamagnetic?
S2–
b.
C–S
Which one of the following bonds is nonpolar?
Zn–Br
4.
November 19, 2013
Ga
Which one of the following compounds should have the greatest lattice energy?
SrCl2
Li3N
KBr
5.
a.
Using the noble gas core symbolism, write the electron configuration of In+.
b.
Circle the species in the following list that have noble gas configurations:
c.
Put the following species in order of decreasing radius: Te2–, Ca2+, Br–, Se2–
_____________________________
Zn2+
Al3+
P3–
Zr
Y3+
Ne
_________ > _________ > _________ > _________
6.
7.
a.
How many electrons can have the following set of quantum numbers? n = 3,  = 2, m = 0, ms = –1/2
_________
b.
How many electrons can have the following combination of quantum numbers? n = 10,  = 8, m = 3
_________
Consider the ground-state orbital diagram shown below:
↑↓
1s
↑↓
2s
↑↓ ↑↓ ↑↓
2p
↑↓
3s
↑↓ ↑↓ ↑↓
3p
↑↓
4s
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
3d
↑↓ ↑↓ ↑
4p
Circle 1 core electron in the diagram above. Put an X over 1 valence electron in the diagram above.
8.
Circle the one best answer below. Why is the 2nd ionization energy of Ca less than the 2nd ionization energy of K?
a. Ca has a noble gas configuraiton and therefore does not want to ionized.
b. The 2nd ionization energy corresponds to removal of a 4s electron from K, but a 4p electron from Ca.
c. The 2nd ionization energy corresponds to forming an anion of K, and that is an energetcally unfavorable process.
d. The 2nd ionization energy corresponds to the removal of a core electron from K vs. a valence from Ca.
e. It’s not; the 2nd ionization energy of Ca is greater than the 2nd ionization energy of K.
9.
Circle the one best answer below. Why is the 1st ionization energy of O less than the 1st ionization energy of N?
a. It’s not; the 1st ionization energy of O is greater than the 1st ionization energy of N.
b. The 1st ionization energy of O corresponds to the removal of a spin-paired 2p electron, which is a lower energy cost
than the removal of an unpaired 2p electron in N.
c. The 1st ionization energy of N requires that a core electron be removed.
d. The removal of an electron from O results in a noble gas configuration, and is therefore energetically favorable.
e. All of these are true.
Chem 1711
Name _____________________________________
Quiz 7 (25 points)
1.
2.
November 19, 2013
a.
How many electrons can have the following set of quantum numbers? n = 3,  = 2, m = 0, ms = –1/2
_________
b.
How many electrons can have the following combination of quantum numbers? n = 10,  = 8, m = 3
_________
Consider the ground-state orbital diagram shown below:
↑↓
1s
↑↓
2s
↑↓ ↑↓ ↑↓
2p
↑↓
3s
↑↓ ↑↓ ↑↓
3p
↑↓
4s
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
3d
↑↓ ↑↓ ↑
4p
Circle 1 core electron in the diagram above. Put an X over 1 valence electron in the diagram above.
3.
a.
Using the noble gas core symbolism, write the electron configuration of In+.
b.
Circle the species in the following list that have noble gas configurations:
c.
Put the following species in order of decreasing radius: Te2–, Ca2+, Br–, Se2–
_____________________________
Zn2+
Al3+
P3–
Zr
Y3+
Ne
_________ > _________ > _________ > _________
4.
5.
Match each equation given below to the appropriate energy term (I – VI). Then indicate whether the sign of the energy
term will be + or − .
energy term
+ or −
a.
Sn+ (g)  Sn2+ (g) + e–
________
________
I.
electron affinity
IV. ΔH°f
b.
MgF2 (s)  Mg2+ (g) + 2 F– (g)
________
________
II.
1st ionization energy
V. lattice energy
c.
F (g) + e–  F– (g)
________
________
III.
2nd ionization energy
VI. bond energy
Circle the one best answer below. Why is the 1st ionization energy of O less than the 1st ionization energy of N?
a. It’s not; the 1st ionization energy of O is greater than the 1st ionization energy of N.
b. The 1st ionization energy of O corresponds to the removal of a spin-paired 2p electron, which is a lower energy cost
than the removal of an unpaired 2p electron in N.
c. The 1st ionization energy of N requires that a core electron be removed.
d. The removal of an electron from O results in a noble gas configuration, and is therefore energetically favorable.
e. All of these are true.
6.
Consider the Pauling electronegativity values (χ) given for the following elements:
Zn (χ=1.6)
Br (χ=2.8)
C (χ=2.5)
S (χ=2.5)
a
Which one of the following bonds is the most polar?
Zn–Br
b.
Zn–S
C–S
C–Br
C–S
C–Br
Which one of the following bonds is nonpolar?
Zn–Br
Zn–S
7.
8.
a.
How many valence electrons does a phosphorus atom have?
____________________
b.
Draw the Lewis symbol for an element, X, if it has 4 valence electrons.
____________________
a.
Which one of the following species is isoelectric with P3–?
N3–
b.
Rb
Ga
S
Li3N
KBr
Cl
Ti2+
Fe3+
Br
Ar
B
Which one of the following elements has the smallest 1st ionization energy?
O
9.
Ca
Which one of the following has the least favorable electron affinity value?
S
g.
Ar
Which one of the following is diamagnetic?
S2–
f.
Cr
Which one of the following compounds should have the greatest lattice energy?
SrCl2
e.
K+
Which one of the following is the most electronegative?
K
d.
Al3+
Which one of the following has the largest atomic radius?
I
c.
Ne
Ca
Kr
Rb
Circle the one best answer below. Why is the 2nd ionization energy of Ca less than the 2nd ionization energy of K?
a. Ca has a noble gas configuraiton and therefore does not want to ionized.
b. The 2nd ionization energy corresponds to removal of a 4s electron from K, but a 4p electron from Ca.
c. The 2nd ionization energy corresponds to forming an anion of K, and that is an energetcally unfavorable process.
d. The 2nd ionization energy corresponds to the removal of a core electron from K vs. a valence from Ca.
e. It’s not; the 2nd ionization energy of Ca is greater than the 2nd ionization energy of K.