1.
A coffee cup calorimeter containing 100.0 mL of concentrated HCl at 20.3 °C. When 1.82 g Zn(s) is added, the temperature rises to 30.5 °C. What is the heat of reaction per mol of reacted Zn? Assume the resultant solution has a specific heat of solution = 4.184 J/g. °C and density = 1.00 g/mL.
                   
A.
-198 kJ/mol
B.
-300. kJ/mol
C.
-272 kJ/mol
D.
-156 kJ/mol
E.
-122 kJ/mol


2.
When NaOH(s) is added to water, it releases -44.5 kJ/mol heat. Find the maximum temperature of the water, when 500. mL of 7.0 M NaOH solution is prepared. The initial temperature of water is 21°C. The solution has a density of 1.08 g/mL and specific heat of 4.00 J/ g·°C
.
A.
83 °C
B.
74 °C
C.
53 °C
D.
93 °C
E.
69 °C


3.
The change in the internal energy of a system that absorbs 2,500 J of heat and that does 7,655 J of work on the surrounding is:
A.
5,155 J
B.
-5,155 J
C.
+10,155 J
D.
-10,155 J
E.
1.91 x 107


4.
Use the given data to calculate ΔHo for the following reaction:

       2C(graphite) + 3CO2 (g) + 8 H2O (g) + 2H2(g) ◊5CH4 (g) + 7O2(g)

Given:

H2(g)   + ½ O2(g)   ◊ H2O (g)           ΔHo = -285.8 kJ

C(graphite) + 2H2(g)   ◊ CH4 (g)           ΔHo = -74.81 kJ

CH4 (g) + 2O2(g)   ◊   CO2 (g) +2 H2O (g)     ΔHo = -890.3 kJ
A.
2788 kJ
B.
2943 kJ
C.
3155 kJ
D.
3515 kJ
E.
3093 kJ


5.
For which one of the following reactions is the value of ΔHorxn equal to ΔHof for the product?
A.
Xe (g) + 2F2 (g) ◊ XeF4 (g)
B.
CH4 (g) + 2Cl2 (g) ◊ CH2Cl2 (l) + 2HCl (g)
C.
N2 (g) + O3 (g) ◊ N2O3 (g)
D.
2CO (g) + O2 (g) ◊ 2CO2 (g)
E.
2C (graphite) + O2 (g) ◊ 2CO (g)


6.
The Bohr theory explains that an emission spectral line is:
A.
due to an interaction between electrons in two different principal orbits.
B.
due to an electron losing energy and changing orbits.
C.
due to an electron gaining energy and changing orbits..
D.
due to an increase in the principal quantum number n of an electron.
E.
due to an electron losing energy but keeping the same values of its all four quantum numbers.


7.
What is the magnitude of the partial positive and partial negative charges in the HF molecule? (1 D = 3.36 × 10–30 C m; 1e– = 1.6022 × 10–19 C; bond length HF = 0.92 angstroms; Dipole Moment HF = 1.82 D; 1 angstroms = 1 x 10-10 m)
A.
-0.41 and +0.41
B.
-0.92 and +0.92
C.
-0.65 and +0.65
D.
-0.33 and +0.33
E.
-0.17 and +0.17


8.
Which one of the following sets of quantum numbers can correctly represent a 3p orbital?
i.
ii.
iii.
iv.
v.
n = 3
n = 1
n = 3
n = 3
n = 3
l = 1
l = 3
l = 2
l = 1
l = 0
ml = 2
ml = 3
ml = 1
ml = –1
ml = 1
 
A.
v
B.
i
C.
ii
D.
iii
E.
iv


9.
The ground–state electron configuration for an atom of indium (In) is
A.
[Kr]5s24d105p1.
B.
[Ar]4s24p63d5.
C.
[Ar]4s23d104p1.
D.
[Kr]5s24p64d5.
E.
[Kr]5s25p64d5.


10.
The binding energy for Lithium is 279.7 kJ/mol. Calculate the minimum wavelength of light that can remove an electron from an atom on the surface of Lithium metal.
A.
1.28 x 10-7 m
B.
428 m
C.
4.28 x 10-7 m
D.
1.40 x 10-12 m
E.
2.14 10-3 m


11.
Which statement best describes relationships in a modern periodic table?
A.
Nonmetallic properties tend to predominate for elements at the far right portion of the table.
B.
Elements are always arranged in order of decreasing atomic weights.
C.
Metalloids usually are the cations in ionic compounds.
D.
The fourteen elements in the "lanthanide" series form a new independent group.
E.
Each transition element is placed in the column of the main group element that it most closely resembles.


12.
Which comparison of ionization energies is correct?
A.
Ca > Mg
B.
Ar > He
C.
Ca+ > Ca
D.
Na > Mg
E.
Mg+ > Mg2+


13.
List in order of increasing atomic size: Sr, Se, As, Ga, In.
A.
Se < As < Ga < In < Sr
B.
Ga < In < Se < As < Sr
C.
Sr < In < Ga < Se < As
D.
In < Ga < As < Se < Sr
E.
As < Ga < Se < Sr < In


14.
Which of the following statements is/are CORRECT for an oxygen atom?
 
I.
The effective nuclear charge felt by a 2s electron is greater than that felt by a 1s electron.
 
II.
The effective nuclear charges felt by 2s and 2p electrons are identical.
 
III.
The effective nuclear charge felt by a 2p electron is less than that felt by a 2s electron.
 
A.
II only
B.
I only
C.
III only
D.
I and II only
E.
I and III only


15.
Use the following data to calculate the 2nd ionization energy for the Metal (M):

M(s)   → M(g)                              ΔH°    = 148.0 kJ
X2(g)   → 2X(g)                           ΔH°    = 159.0 kJ
M(g)   → M+(g)   +    e-                ΔH°    = 738.0 kJ
M+(g)   → M2+(g) +   e-               ΔH°    =   ?
X(g)    +   e-     → X -(g)                ΔH°    = -328.0 kJ
M(s) +    X2(g)   → MX2(s)         ΔHf°    = -1123 kJ
MX2(s)    →     M2+(g) + 2X -(g)    ΔH°    = 2962 kJ          
A.
1589 kJ
B.
794.0 kJ
C.
1642 kJ
D.
1450. kJ
E.
159.8 kJ


16.
The number of lone pairs of ClO3- (where all atoms are satisfied with octet) is
A.
20
B.
27
C.
10
D.
24
E.
9


17.
Calculate the bond energy of C-F in kJ/mol from the given data:

   CH4 (g) + 2Cl2(g) +2F2(g) → CF2Cl2(g) +2HF +2HCl (g)   ΔH° = -1194 kJ/mol

Bond      bond energy

C-H       413 kJ/mol

F-F      154 kJ/mol

C-Cl      339 kJ/mol

H-F      565 kJ/mol

H-Cl      427 kJ/mol

Cl-Cl      243 kJ/mol
A.
478
B.
970.
C.
709
D.
489
E.
355


18.
All of the following structures obey the Lewis octet rule EXCEPT
 
A.
N2O5
B.
N2O
C.
N2O4
D.
N2O3
E.
All of the above are correct structures.


19.
Which one of the following bonds is the most polar?
A.
O-Cl
B.
O-Br
C.
O-I
D.
Br-Cl
E.
I-Br


20.
Choose the groups of molecules below in which all the molecules have no net dipole moment.
A.
CO2, Cl2C=CCl2, NH4+
B.
HF, H2O, N2
C.
NH3, Cl2C=CCl2, O2
D.
SiBrCl3, N2, Cl2C=CCl2
E.
BeCl2, CH3Br , H2O


STOP This is the end of the test. When you have completed all the questions and reviewed your answers, press the button below to grade the test.