CHEM 10113, Exam 3
November 2, 2011
Name_____________________
(please print)
All equations must be balanced and show phases for full credit. Significant figures count, and
box your answers!
1. (11 points) In each blank write >, < or = as appropriate.
Cl-Cl bond polarity
H-H bond polarity
# of valence electrons in
SeO2
EA of Ta
# of valence electrons in
NO2–
EA of Cu
electronegativity of Re
electronegativity of Ru
size of Kr
size of Rb+
IE of Sr
IE of Sr+
Bond order of O2
Bond order of F2
Wavelength of IR light
Wavelength of X-rays
Energy of blue light
Energy of orange light
2. (12 points) Briefly define the following terms.
Shielding –
Free radical –
Covalent bond –
Expanded octet –
3. (10 points) SHOW ALL WORK. Use tabulated average bond energies
(appended to exam) to estimate the enthalpy of the following reaction.
H2O2(g)  H2O(g) + ½ O2(g)
1
4. (15 pts) SHOW ALL WORK. A heat lamp produces 32.8 watts of power at a
wavelength of 6.5 m. How many photons are emitted per second? (1 watt = 1
J/s)
5. (3 points) If the value of ml for an electron in an atom is –3, what is the
smallest value of l that the electron could have?
6. (2 point) Which quantum number is related to shape of the orbital?
7. (12 points) Fill in the blanks in the following equations. For coefficients of 1,
please write “1” rather than leaving blank.
Example:
__ MgCl2(___) + __ AgNO3(___)  __ ____(s) + 1 ______(___)
Answer:
1 MgCl2(aq) + 2 AgNO3(aq)  2 AgCl(s) + 1 Mg(NO3)2(aq)
a) ___ _____ (
b) ___ H2(
)
)
+ F2(
+ _____ (
)
)
 ___ PtI2(
)
 ___ ____ (g)
8. (6 points) Name the element or ion:
a. Its valence electron configuration is ns1 and its most stable ion has the same
electron configuration as krypton.______
b. It has 7 unpaired valence electrons and is a lanthanide._____
9. (6 points) Give the complete electron configuration for a. P2– ion, and b. Be.
10. (5 points) Write the standard formation reaction for Cu(NO3)2·3H2O(s).
2
11. (6 points) Give the short-hand electron configurations for a. Co+, and b. Pb.
12. (6 points) Give the valence electron configurations of a. Ge, and b. Eu.
13. (6 points) Write the chemical equations for a. the second ionization energy of
zinc, and b. the EA of Y.
14. (6 points) Contrast three properties of alkali metals and three properties of
the noble gases.
Alkali metals
Noble gases
15. (3 points) The bond order of the N-O bond in NO2− is _________.
16. (10 points) SHOW ALL WORK. Calculate the enthalpy change for the
reaction
Ca2+(aq) + 2 OH–(aq) + CO2(g)  CaCO3(s) + H2O(l)
by manipulating the following equations.
CaCO3(s)  CaO(s) + CO2(g) H = –178.1 kJ
CaO(s) + H2O(l)  Ca(OH)2(s) H = –65.3 kJ
Ca(OH)2(s)  Ca2+(aq) + 2 OH–(aq) H = –16.2 kJ
3
17. (24 points) Write the complete Lewis electron dot formulas for each of the
molecules below. Please put the final answers in the boxes; anything outside of
the boxes will not be graded.
O22–
NF3
ClO3–
PCl4+
4
18. (7 points) SHOW ALL WORK. Use the Born-Haber cycle as shown to
determine the value of H for step 3.
-349 kJ
+122 kJ
+108 kJ
-788 kJ
-411 kJ
5
CHEM 10113, Exam 3
November 2, 2011
Name_____________________
(please print)
All equations must be balanced and show phases for full credit. Significant figures count, and
box your answers!
1. (11 points) In each blank write >, < or = as appropriate.
IE of Ca+
IE of Ca2+
# of valence electrons in
OCN–
polarity of Sb-Cl bond
# of valence electrons in
NO2–
polarity of Cl-Cl bond
Frequency of radiowaves
Frequency of UV light
Bond order of CO
Bond order of N2
Size of S
2–
ion
Size of Ar ion
EA of In
EA of Hf
electronegativity of I
electronegativity of Au
Wavelength of gamma
rays
Wavelength of X-rays
2. (12 points) Briefly define the following terms.
Diamagnetic –
Ionic bond –
Emission spectrum –
Ground state –
3. (10 points) SHOW ALL WORK. Use tabulated average bond energies
(appended to exam) to estimate the enthalpy of the following reaction.
Cl2CF2(g) + F2(g)  CF4(g) + Cl2(g)
6
4. (15 pts) SHOW ALL WORK. A heat lamp produces 34.6 watts of power at a
wavelength of 5.5 m. How many photons are emitted per second? (1 watt = 1
J/s)
5. (3 points) If the value of ml for an electron in an atom is –3, what is the
smallest value of n that the electron could have?
6. (2 point) Which quantum number is related to spatial orientation?
7. (12 points) Fill in the blanks in the following equations. For coefficients of 1,
please write “1” rather than leaving blank.
Example:
__ MgCl2(___) + __ AgNO3(___)  __ ____(s) + 1 ______(___)
Answer:
1 MgCl2(aq) + 2 AgNO3(aq)  2 AgCl(s) + 1 Mg(NO3)2(aq)
a) ___ _____ (
b) ___ I2(
)
+ F2(
)
+ _____ (
)
)
 ___ ZnCl2(
)
 ___ ____ (g)
8. (6 points) Name the element or ion:
a. Its electron configuration is 1s22s22p1 and it has a +1 charge._____
b. It has 5 unpaired valence electrons and its highest principle level is 6.______
9. (6 points) Give the complete electron configurations for a. Si+ ion, and b. C.
10. (5 points) Write the standard formation reaction for MgSO4·7H2O(s).
7
11. (6 points) Give the short-hand electron configurations for a. Os+, and b. Te.
12. (6 points) Give the valence electron configurations of a. Sn, and b. Nd.
13. (6 points) Write the chemical equations for a. the second ionization energy of
cadmium, and b. the EA of Db.
14. (6 points) Contrast three properties of alkali metals and three properties of
the halogens.
Alkali metals
halogens
15. (3 points) The bond order of the P-O bond in PO43− is _________.
16. (10 points) SHOW ALL WORK. Calculate the enthalpy change for the
reaction
C(s) + 2 H2(g)  CH4(g)
by manipulating the following equations.
C(s) + O2(g)  CO2(g) H = –393.5 kJ
H2(g) + ½ O2(g)  H2O(l) H = –285.8 kJ
CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(l) H = –890.3 kJ
8
17. (24 points) Write the complete Lewis electron dot formulas for each of the
molecules below. Please put the final answers in the boxes; anything outside of
the boxes will not be graded.
NO–
IF4–
NO3–
CCl4
9
18. (7 points) SHOW ALL WORK. Use the Born-Haber cycle as shown to
determine the value of H for step 4.
+496 kJ
+122 kJ
+108 kJ
-788 kJ
-411 kJ
10
CHEM 10113, Exam 3
November 2, 2011
Name_____________________
(please print)
All equations must be balanced and show phases for full credit. Significant figures count, and
box your answers!
1. (11 points) In each blank write >, < or = as appropriate.
bond order of F2
bond order of N2
EA of V
EA of Zn
 of microwaves
electronegativity of P
 of yellow light
electronegativity of Mg
size of Br–
size of Kr
–
IE of Ar
IE of Ar
Energy of radiowaves
Energy of microwaves
C=O bond polarity
H-H bond polarity
# of valence electrons in
H2CO2
# of valence electrons in
Cl2CO
2. (12 points) Briefly define the following terms.
Effective nuclear charge –
Electron sea model –
degenerate –
Paramagnetic –
3. (10 points) SHOW ALL WORK. Use tabulated average bond energies
(appended to exam) to estimate the enthalpy of the following reaction.
H2C=CH2(g) + Br2(g)  BrH2C-CH2Br(g)
11
4. (15 pts) SHOW ALL WORK. A heat lamp produces 40.0 watts of power at a
wavelength of 6.1 m. How many photons are emitted per second? (1 watt = 1
J/s)
5. (3 points) If the value of ml for an electron in an atom is –4, what is the
smallest value of n that the electron could have?
6. (2 point) Which quantum number is related to energy?
7. (12 points) Fill in the blanks in the following equations. For coefficients of 1,
please write “1” rather than leaving blank.
Example:
__ MgCl2(___) + __ AgNO3(___)  __ ____(s) + 1 ______(___)
Answer:
1 MgCl2(aq) + 2 AgNO3(aq)  2 AgCl(s) + 1 Mg(NO3)2(aq)
a) ___ Li (
)
b) ___ ____ (
+ ___ H2O(l)  _____(g) + ___ _____(s)
)
+ Br2(
)
 ___ CsBr(
)
8. (6 points) Name the element or ion:
a. Its electron configuration is 1s22s22p5 and it has a -1 charge. _____
b. It has 4 unpaired valence electrons and its highest principle level is 4.______
9. (6 points) Give the complete electron configurations for a. Cl+ ion, and b. F.
10. (5 points) Write the standard formation reaction for CuSO4·5H2O(s).
12
11. (6 points) Give the short-hand electron configurations for a. Au+, and b. Po.
12. (6 points) Give the valence electron configurations of a. Pb, and b. Ce.
13. (6 points) Write the chemical equations for a. the second ionization energy of
mercury, and b. the EA of Re.
14. (6 points) Contrast three properties of halogens and three properties of the
noble gases.
halogens
Noble gases
15. (3 points) The bond order of the C-O bond in HCO2− is _________.
16. (10 points) SHOW ALL WORK. Calculate the enthalpy change for the
reaction
2 HCl(g) + F2(g)  2 HF(l) + Cl2(g)
by manipulating the following equations.
4 HCl(g) + O2(g)  2 H2O(l) + 2 Cl2(g) H = –202.4 kJ
½ H2(g) + ½ F2(g)  HF(l) H = –600.0 kJ
H2(g) + ½ O2(g)  H2O(l) H = –285.8 kJ
13
17. (24 points) Write the complete Lewis electron dot formulas for each of the
molecules below. Please put the final answers in the boxes; anything outside of
the boxes will not be graded.
BrO–
ClO4–
SBr2
AsCl4+
14
18. (7 points) SHOW ALL WORK. Use the Born-Haber cycle as shown to
determine the value of H for step 2.
-349 kJ
+496 kJ
+108 kJ
-788 kJ
-411 kJ
15