Name: 
 

Chemistry Practice Final (best guess at the types of questions on the final)



4/14/2012
Multiple Choice

Identify the choice that best completes the statement or answers the question.
 

 1. 

If matter is uniform throughout and cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is called a (an) __________.
a.
heterogeneous mixture
b.
element
c.
homogeneous mixture
d.
compound
e.
mixture of elements
 

 2. 

One side of a cube measures 1.55 m.  The volume of this cube is __________ cm3.
a.
2.40 ´ 104
b.
3.72 ´ 106
c.
2.40
d.
3.72
e.
155
 

 3. 

The symbol for the element lead is __________.
a.
Ld
b.
Pb
c.
Sn
d.
Hg
 

 4. 

Elements in Group 7A are known as the __________.
a.
chalcogens
b.
alkali metals
c.
alkaline earth metals
d.
halogens
e.
noble gases
 

 5. 

The correct name for SO is __________.
a.
sulfur oxide
b.
sulfur monoxide
c.
sulfoxide
d.
sulfate
e.
sulfite
 

 6. 

In the periodic table, the elements are arranged in __________. 
a.
alphabetical order
b.
order of increasing atomic number
c.
order of increasing metallic properties
d.
order of increasing neutron content
e.
reverse alphabetical order
 

 7. 

When the following equation is balanced, the coefficient of sulfur dioxide is __________.

PbS (s)  +  O2 (g) ® PbO (s)  +  SO2 (g)
a.
5
b.
1
c.
3
d.
2
e.
4
 

 8. 

Silver nitrate and aluminum chloride react with each other by exchanging anions:

3AgNO3 (aq)+  AlCl3 (aq) ® Al(NO3)3 (aq) +  3AgCl (s)

What mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of A1C13?
a.
17.6
b.
4.22
c.
24.9
d.
3.56
e.
11.9
 

 9. 

Of the reactions below, which one is a decomposition reaction?
a.
NH4Cl ®  NH3  +  HCl
b.
2Mg  +  O2 ® 2MgO
c.
2N2  +  3H2 ® 2NH3
d.
2CH4  +  4O2 ® 2CO2  +  4H2O
e.
Cd(NO3)2  +  Na2S ® CdS  +  2NaNO3
 

 10. 

The formula weight of lead nitrate (Pb(NO3)2) is __________ amu.
a.
269.2
b.
285.2
c.
317.2
d.
331.2
e.
538.4
 

 11. 

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?
a.
2.00
b.
0.500
c.
0.160
d.
0.0800
e.
0.0400
 

 12. 

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is __________.
a.
1.85
b.
2.12
c.
0.197
d.
3.52
e.
11.8
 

 13. 

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide:

Pb2+ (aq) + 2I- (aq) ® PbI2 (s)

Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq) must be added to a solution containing 0.700 mol of mc013-1.jpg to completely precipitate the lead?
a.
2.54 ´ 10-3
b.
394
c.
197
d.
0.197
e.
0.394
 

 14. 

Given the following reactions

H2O (l) ® H2O (g) DH = 44.01 kJ

2H2 (g)  +  O2 (g) ® 2H2O (g) DH =  -483.64 kJ

the enthalpy for the decomposition of liquid water into gaseous hydrogen and oxygen

2H2O (l) ® 2H2 (g)  +  O2 (g)

is __________ kJ.
a.
-395.62
b.
-527.65
c.
439.63
d.
571.66
e.
527.65
 

 15. 

Calculate the energy (J) change associated with an electron transition from n = 2 to n = 5 in a Bohr hydrogen atom. Bohr’s constant is 2.179x10-18 J
a.
6.5 ´ 10-19
b.
5.5 ´ 10-19
c.
8.7 ´ 10-20
d.
4.6 ´ 10-19
e.
5.8 ´ 10-53
 

 16. 

Which one of the following is the correct electron configuration for a ground-state nitrogen atom?
a.

mc016-1.jpg
b.

mc016-2.jpg
c.

mc016-3.jpg
d.

mc016-4.jpg
e.
None of the above is correct.
 

 17. 

Which one of the following elements has the largest atomic radius?
a.
Se
b.
As
c.
S
d.
Sb
e.
Te
 

 18. 

Alkali metals tend to be more reactive than alkaline earth metals because __________.
a.
alkali metals have lower densities
b.
alkali metals have lower melting points
c.
alkali metals have greater electron affinities
d.
alkali metals have lower ionization energies
e.
alkali metals are not more reactive than alkaline earth metals
 

 19. 

Hydrogen is unique among the elements because __________.
1.  It is not really a member of any particular group.
2.  Its electron is not at all shielded from its nucleus.
3.  It is the lightest element.
4.  It is the only element to exist at room temperature as a diatomic gas.
5.  It exhibits some chemical properties similar to those of groups 1A and 7A.
a.
1, 2, 3, 5
b.
1, 2, 3, 4, 5
c.
1, 4, 5
d.
3, 4
e.
2, 3, 4, 5
 

 20. 

Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a.
decreases, increases
b.
increases, increases
c.
increases, decreases
d.
stays the same, increases
e.
increases, stays the same
 

 21. 

A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
a.
PO43-
b.
SiF4
c.
CF4
d.
SeF4
e.
NF3
 

 22. 

Of the possible bonds between carbon atoms (single, double, and triple), __________.
a.
a triple bond is longer than a single bond
b.
a double bond is stronger than a triple bond
c.
a single bond is stronger than a triple bond
d.
a double bond is longer than a triple bond
e.
a single bond is stronger than a double bond
 

 23. 

The O-C-O bond angle in the CO32- ion is approximately __________.
a.
90°
b.
109.5°
c.
120°
d.
180°
e.
60°
 

 24. 

According to VSEPR theory, if there are four electron domains on a central atom, they will be arranged such that the angles between the domains are __________.
a.
120°
b.
109.5°
c.
180°
d.
360°
e.
90°
 

 25. 

Gaseous mixtures __________.
a.
can only contain molecules
b.
are all heterogeneous
c.
can only contain isolated atoms
d.
are all homogeneous
e.
must contain both isolated atoms and molecules
 

 26. 

A fixed amount of gas at 25.0°C occupies a volume of 10.0 L when the pressure is 629 torr. Use Charles's law to calculate the volume (L) the gas will occupy when the temperature is increased to 121°C while maintaining the pressure at 629 torr.
a.
10.9
b.
13.2
c.
2.07
d.
7.56
e.
48.4
 
 
nar001-1.jpg
 

 27. 

The heating curve shown was generated by measuring the heat flow and temperature for a solid as it was heated. The slope of the __________ segment corresponds to the heat capacity of the gas.
a.
AB
b.
BC
c.
CD
d.
DE
e.
EF
 
 
nar002-1.jpg
 

 28. 

Based on the figure above, the boiling point of water under an external pressure of 0.316 atm atm is __________°C.
a.
70
b.
40
c.
60
d.
80
e.
90
 

 29. 

A sealed 1.0 L flask is charged with 0.500 mol of I2 and 0.500 mol of Br2. An equilibrium reaction ensues:

I2 (g)  +  Br2 (g)  mc029-1.jpg  2IBr (g)

When the container contents achieve equilibrium, the flask contains 0.84 mol of IBr. The value of Keq is __________.
a.
11
b.
4.0
c.
110
d.
6.1
e.
2.8
 

 30. 

Using the data in the table, which of the conjugate bases below is the weakest base?

mc030-1.jpg
a.
OAc-
b.
CHO2-
c.
ClO-
d.
F-
e.
OAc- and CHO2-
 

 31. 

Which substance is the reducing agent in the following reaction?

Fe2S3  +  12HNO3 ® 2Fe(NO3)3  +  3S  +  6NO2  +  6H2O
a.
HNO3
b.
S
c.
NO2
d.
Fe2S3
e.
H2O
 

 32. 

The half-life of a radionuclide
a.
is constant.
b.
gets shorter with passing time.
c.
gets longer with passing time.
d.
gets shorter with increased temperature.
e.
gets longer with increased temperature.
 

 33. 

Boric oxide is __________.
a.
B2O
b.
BO2
c.
BO
d.
B2O3
e.
B2O4
 

 34. 

What happens to the silicon that is a contaminant in crude iron in a converter?
a.
it is converted to the tetrafluoride that bubbles out as a gas.
b.
It is precipitated as sodium silicate.
c.
It is converted to silicon dioxide and becomes part of the slag.
d.
It is precipitated as the carbide.
e.
It is precipitated as iron silicate.
 

 35. 

Alkenes always contain a __________.
a.
Cmc035-1.jpgC bond
b.
CºC bond
c.
C-C bond
d.
Cmc035-2.jpgH bond
e.
CºH bond
 



 
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