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Chemistry 221 Practice Exam I



Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

1. 

What is the correct symbol for iron?
a.
Fe
b.
I
c.
Ir
d.
Sn
e.
Pb
 

2. 

A pure substance that is composed of two or more different elements is
a.
a chemical compound.
b.
a multi-element.
c.
an atom.
d.
a heterogeneous mixture.
e.
a homogeneous mixture.
 

3. 

All of the following are examples of physical properties EXCEPT
a.
the density of neon gas.
b.
the conductivity of copper wire.
c.
the boiling point of water.
d.
the frying of an egg.
e.
the density of mercury metal.
 

4. 

The density of acetic acid is 1.05 g/mL. What is the volume of 275 g of acetic acid?
a.
3.46 x 10-3 mL
b.
3.82 x 10-3 mL
c.
2.62 x 102 mL
d.
2.76 x 102 mL
e.
2.89 x 102 mL
 

5. 

You can identify a metal by carefully determining its density. A 23.1 g piece of an unknown metal is 1.23 cm long, 2.11 cm wide, and 1.00 cm thick. What is the identity of the element?
a.
nickel, 8.90 g/cm3
b.
aluminum, 2.70 g/cm3
c.
titanium, 4.54 g/cm3
d.
zirconium, 6.51 g/cm3
e.
chromium 7.20 g/cm3
 

6. 

The radius of a helium atom is 31 pm. What is the radius in meters?
a.
3.1 x 10-14 m
b.
3.1 x 10-12 m
c.
3.1 x 10-11 m
d.
3.1 x 10-9 m
e.
3.1 x 10-8 m
 

7. 

A rectangular box has dimensions of 20.0 cm x 15.0 cm x 8.00 cm. Calculate the volume of the box in liters.
a.
2.40 x 10-3 L
b.
4.30 x 10-3 L
c.
2.40 L
d.
43.0 L
e.
2.40 x 103 L
 

8. 

At 25 °C, the density of oxygen in air is 0.275 g/L. What volume will be occupied by 5.0 kg of oxygen?
a.
1.4 L
b.
5.5 L
c.
22 L
d.
1.4 x 103 L
e.
1.8 x 104 L
 

9. 

Express 5.00 x 10-2 m in standard notation using the correct number of significant figures.
a.
0.05 cm
b.
50 mm
c.
50.0 mm
d.
500 m
e.
500. m
 

10. 

Gamma (γ) rays are
a.
positively charged electrons.
b.
identical to electrons.
c.
helium nuclei.
d.
identical to canal rays.
e.
high energy radiation.
 

11. 

Tritium, a radioactive isotope of hydrogen, is produced
a.
by decomposition of rain water.
b.
by decomposition of deep aquifer water.
c.
by cathode rays.
d.
commercially for use in smoke detectors.
e.
naturally in the upper atmosphere by cosmic radiation.
 

12. 

Silver has an atomic mass of 107.9 amu. If 51.84% of Ag exists as Ag-107 (106.9051 amu), what is the identity and the atomic mass of the other isotope?
a.
Ag-108; 107.9 amu
b.
Ag-109; 109.0 amu
c.
Ag-109; 109.9 amu
d.
Ag-110; 109.9 amu
e.
Ag-110; 110.2 amu
 

13. 

The density of lithium is 0.546 g/cm3. What volume is occupied by 3.66 x 1023 atoms of lithium?
a.
2.30 cm3
b.
6.24 cm3
c.
6.94 cm3
d.
7.25 cm3
e.
7.73 cm3
 

14. 

Which element comprises over three quarters of the Earth's atmosphere?
a.
oxygen
b.
nitrogen
c.
helium
d.
argon
e.
hydrogen
 

15. 

Of the following elements, which two are the most abundant in the Earth's crust: iron, hydrogen, silicon, calcium, uranium, and oxygen?
a.
hydrogen and oxygen
b.
hydrogen and iron
c.
iron and calcium
d.
silicon and oxygen
e.
silicon and uranium
 

16. 

The smallest unit into which a pure substance such as sugar or water can be divided, while still retaining its composition and chemical properties is a(n) ________.
a.
atom
b.
molecule
c.
isotope
d.
mixture
e.
ion
 

17. 

A bromide ion has ________ electrons.
a.
8
b.
34
c.
35
d.
36
e.
37
 

18. 

Which formula represents the binary compound formed by strontium ions and phosphate ions?
a.
Sr2(PO4)3
b.
SrPO4
c.
Sr2P3
d.
Sr3(PO4)2
e.
SrP
 

19. 

Sodium oxalate has the chemical formula, Na2C2O4. Based on this information, the formula for iron(III) oxalate is __________.
a.
FeC2O4
b.
Fe(C2O4)2
c.
Fe(C2O4)2
d.
Fe2(C2O4)3
e.
Fe3(C2O4)2
 

20. 

What is the correct formula for aluminum sulfide?
a.
AlSO3
b.
Al2(SO4)3
c.
AlS
d.
Al3(SO3)2
e.
Al2S3
 

21. 

Predict which ionic compound has the highest melting point.
a.
NaCl
b.
AlN
c.
CsI
d.
MgBr2
e.
KF
 

22. 

The empirical formula of a hydrocarbon with a molar mass of 78.11 g/mol is CH. What is the molecular formula?
a.
C6H6
b.
C5H28
c.
C5H2O
d.
C2H4
e.
C8H18
 

23. 

How many oxygen atoms are there in 1.50 mol of O2?
a.
1.81 x 1024 atoms
b.
2.89 x 1025 atoms
c.
9.03 x 1023 atoms
d.
5.78 x 1025 atoms
e.
2.82 x 1022 atoms
 

24. 

Nitrogen and oxygen form an extensive series of oxides with the general formula NxOy. What is the empirical formula for an oxide that contains 63.65% nitrogen?
a.
N2O
b.
NO
c.
NO2
d.
N2O3
e.
N2O5
 

25. 

A 2.000 g sample of CoCl2·xH2O is dried in an oven. When the anhydrous salt is removed from the oven, its mass is 1.565 g. What is the value of x?
a.
0.5
b.
1
c.
2
d.
4
e.
6
 

Essay - note that these questions will not be graded by the computer, but answers will be provided
 

26. 

What is the difference between the accuracy of measurements and the precision of measurements?
 

27. 

Significant figures allow us to estimate uncertainty in calculated values. In some circumstances, following significant figure rules can lead to estimates of uncertainty that are too high or low. This is the case for the mathematical expression below.
99 x 1.02 = 100.98
Following the rules governing significant figures in multiplication, the answer can be rounded to 1.0 x 102. What is wrong with rounding the answer to two significant figures?
 

28. 

In which ionic compound, NaBr or KBr, is the force of attraction between anions and cations stronger?
 

29. 

The numerical quantity of a mole, 6.022 x 1023, is defined as the number of atoms in a specific mass of an element. What is the mass and the identity of the element used to define one mole?
 



 
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