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Chem11-Review-Chpt 1,2 Note: this sample test does not reflect length, weight and necessarily
every topic and type of question that will be on the unit test. It should not be your only study tool,
but rather used in conjunction with class notes, textbook and other resources.
Multiple Choice Identify the choice that best completes the statement or answers the question.
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1. The particle that has the smallest mass is the
a. electron
d. nucleus
b. proton
e. ion
c. neutron
2. The atomic number of an element is defined as the
a. number of neutrons in the nucleus
b. number of protons in the nucleus
c. number of electrons in the nucleus
d. number of protons and neutrons in the nucleus
e. electron to proton ratio
3. Electron affinity increases as you go from left to right on the periodic table because
a. atomic radius decreases
d. all of the above
b. ionization energy decreases
e. none of the above
c. of the periodic law
4. Two atoms are isotopes if they have
a. different atomic numbers
b. the same mass number, but different atomic numbers
c. the same number of protons and neutrons
d. the same number of electrons, but a different number of neutrons
e. the same atomic number, but a different mass number
5. The element found in the periodic table in Group 6 and Period 4 is
a. hafnium, Hf
d. gadolinium, Gd
b. selenium, Se
e. chromium, Cr
c. lithium, Li
6. Which of the following matches of group number and common name is incorrect?
a. Group 7 - transition metals
d. Group 2 - actinides
b. Group 2 - alkali earth metals
e. Group 18 - noble gases
c. Group 17 - halogens
7. An atomic mass unit (amu) is defined as the
a. mass of a hydrogen atom
b. mass of 12 hydrogen atoms
c. mass of a carbon atom
d. one-twelfth the mass of a hydrogen atom
e. one-twelfth the mass of a carbon atom
8. The chemical family known as the halogens are the elements in Group
a. 1
d. 17
b. 2
e. 18
c. 5
9. Electronegativity is derived from
a. ionization energies
d. all of the above
b. electron affinity
e. none of the above
c. reactivity
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____ 10. According to the Lewis model of the atom, the number of bonding electrons in a nitrogen atom is
a. 1
d. 5
b. 2
e. 7
c. 3
____ 11. The empirical formulas of ionic compounds are explained using
a. equal numbers of positive and negative ions
b. a net electrical charge of zero
c. double bonds
d. neutral molecular entities
e. IUPAC prefixes
____ 12. The substance NH3 is a very important industrial chemical. It is used directly as a fertilizer and is also used to
produce many other useful chemicals. The IUPAC name of this substance is
a. hydrogen nitride
d. octane
b. ammonia
e. ammonium
c. hydrogen peroxide
____ 13. The correct formula for nitrous acid is
a. HNO3(aq)
d. N2H4(aq)
b. HNO2(aq)
e. NH4+
c. NH3(aq)
____ 14. Hydroselenic acid is a very toxic substance. Its chemical formula is
a. HSe(aq)
d. H2SeO3(aq)
b. H2SeO2(aq)
e. H2SeO4(aq)
c. H2Se(aq)
____ 15. The formula for carbon tetrachloride is
a. C1Cl4(l)
d. CCl4(l)
b. C4Cl4(l)
e. C4Cl1(l)
c. C1Cl(l)
____ 16. What is the formula for aqueous hydrogen fluoride?
a. HFl(aq)
d. HF
b. HFO3(aq)
e. H2F(aq)
c. HF(aq)
____ 17. Which one of the following formulas is incorrect?
a. Cu2O
d. Ba(HCO3)2
b. NaOH
e. ZnCl3
c. CO
____ 18. If the name of a chemical compound ends in "ide", the compound is
a. acidic
d. an oxide
b. binary
e. none of the above
c. basic
____ 19. If the classical name of an acidic substance has the ending "...ic acid", then the formula for the "per....ic acid"
of the same family is obtained by
a. removing two oxygen atoms
d. adding one oxygen atom
b. removing all of the oxygen atoms
e. subtracting one oxygen atom
c. subtracting one hydrogen atom
____ 20. A metallic element M reacts with oxygen to form an oxide with the formula M2O3. The formula of the
corresponding chloride of the metal will be
a. MCl3
d. M2Cl
b. MCl
e. M2Cl2
c. MCl2
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Short Answer
21. What is the group number of the alkaline earth metals?
22. What is the family name for Group 17?
23. If nuclear energy is so clean, why is its use controversial?
24. Why does ionization energy increase from left to right in a period on the periodic table?
25. Elements A, B, and C are in the same chemical family. Element A bursts into pink flames when it dissolves in
water. Element B sizzles slightly when it dissolves in water. Element C sizzles and sometimes burns when it
dissolves in water. How would A, B, and C be arranged in the periodic table? Of the three, which would most
likely be highest in the group? Which would most likely be lowest?
26. Explain negative electron affinities in terms of attractive and repulsive forces within the atom.
27. Examine the following 1st, 2nd, and 3rd ionization energies and state which element is most likely a noble
gas.
Element X
Element Y
Element Z
1st
(eV)
5.139
7.646
21.564
2nd
(eV)
47.286
15.035
40.962
3rd
(eV)
71.64
80.143
63.45
28. Examine the following 1st, 2nd, and 3rd ionization energies and state which element is most likely in Group
1.
Element X
Element Y
Element Z
1st
(eV)
5.139
7.646
21.564
2nd
(eV)
47.286
15.035
40.962
3rd
(eV)
71.64
80.143
63.45
29. The electronegativity of magnesium, Mg, is 1.2. Would you expect aluminum's electronegativity to be higher
or lower?
30. Explain why, in general, ionization energy and electron affinity follow the same trends throughout the
periodic table.
31. Write an empirical definition of ionic compounds.
32. For a science fair project, a student wants to design a simple device for removing certain gases from polluted
air. He knows that polar molecules dissolve well in water, so he bubbles polluted air through a jug of water to
remove unwanted gases. For his project, the student uses air containing the following gases:
1. N2(g)
5. CH4(g)
2. O2(g)
6. OCl2(g)
3. HF(g)
7. C3H8(g)
4. NH3(g)
8. CH3OCH3(g)
List the gases that will dissolve by writing down their corresponding numbers.
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33. For a science fair project, a student wants to design a simple device for removing certain gases from polluted
air. He knows that polar molecules dissolve well in water, so he bubbles polluted air through a jug of water to
remove unwanted gases. For his project, the student uses air containing the following gases:
1. N2(g)
5. CH4(g)
2. O2(g)
6. OCl2(g)
3. HF(g)
7. C3H8(g)
4. NH3(g)
8. CH3OCH3(g)
List the gases that will form hydrogen bonds with water by writing down their corresponding numbers.
34. A student records the following evidence in a lab book.
Unknown substance
Pure state
Solubility in water
Solution conductivity
I
solid
high
low
II
solid
low
low
III
solid
high
none
IV
solid
high
high
Which of the substances in the table above is most likely an ionic compound? Explain your answer.
35. Explain, in your own words, how and why ionic bonding occurs.
36. Use an electron dot diagram to explain why Lewis theory predicts that sulfur dioxide has one double bond.
37. Use an electron dot diagram to explain why the cyanide ion contains a triple bond.
38. Use an electron dot diagram to explain why ammonia is a polar molecule.
Essay
39. Explain, in your own words, how the modern periodic table was developed. How did the empty spaces appear
in the earlier versions?
40. Producing electricity with nuclear power is still debatable. In a brief essay, give two reasons why we should
continue to use nuclear power and two reasons why we should not.
41. The names of pharmaceutical drugs are generally given trade names. Should pharmaceutical companies be
required to state the IUPAC name for the active ingredient? Why or why not?
42. Explain, in your own words, why ionic compounds are brittle, have extremely high melting points, and are
solid at SATP.
Chem11-Review-Chpt 1,2
Answer Section
MULTIPLE CHOICE
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
A
B
A
E
E
D
E
D
D
C
B
B
B
C
D
C
E
B
D
A
SHORT ANSWER
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
2
halogens
The waste produced is quite dangerous and difficult to dispose of permanently and safely.
Ionization energy increases because atomic radius decreases. This happens because the nuclear charge
increases, but the number of energy levels does not. Therefore, the nucleus has a stronger hold on the
electrons as the nuclear charge increases.
Element B would be highest and element A would be lowest. Element C would lie in between.
When an electron is added to an atom it is repelled by the electrons already there, but is attracted by the
nucleus. When the repulsion outweighs the attraction, energy is absorbed.
element Z
element X
higher
They are both dependent on the same thing, atomic radius. When the atomic radius is small, it is more
difficult to remove an electron, so ionization energy is high. At the same time, it is easier for the atom to
accept another electron, so it releases energy when an electron is added and electron affinity is high.
Ionic compounds are hard solids at SATP, have high melting and boiling points, and are good conductors of
electricity in liquid and aqueous states.
3, 4, 6, and 8
3 and 4
Substance IV is most likely to be an ionic compound because its high solution conductivity indicates that ions
are present in the solution.
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35. Atoms are more stable when they have eight valence electrons. Nonmetals will try to gain electrons to form
a stable octet and metals will try to give away electrons to form a stable octet. Thus, metals give electrons to
nonmetals. Subsequently, the two oppositely charged ions are attracted to one another.
36. Between the one sulfur atom and two oxygen atoms, there are 18 valence electrons. The only way for three
atoms to attain stable octets is to arrange themselves as shown in the following diagram.
37. A carbon atom and a nitrogen atom have nine valence electrons. The negative charge means that there are
altogether ten electrons with which the atoms can attain stable octets. The only way to do this is with a triple
bond as shown in the following diagram.
38. The following diagram shows the electron dot diagram for ammonia. The high electronegativity of nitrogen
compared to hydrogen causes the electrons to spend more time with the nitrogen, thus causing a partial
negative charge at the nitrogen atom and a partial positive charge at the hydrogen atoms.
ESSAY
39. -Observations and experiments were done on all of the known elements.
-Elements were arranged left to right from lightest to heaviest.
-Elements with similar physical and chemical properties were arranged in columns.
-The property arrangement superseded the mass arrangement.
-Empty spaces occurred when placing an element in a specific chemical family meant leaving a "hole" behind
it in a row.
40. Pros
-Amounts of radioactive waste are small compared to waste produced by combustion reactions.
-No greenhouse gases are produced.
-Very little fuel is necessary to produce large amounts of electricity.
Cons
-There is a risk of leakage of radioactive tritium.
-Waste with extremely long half-lives are produced.
-There is a risk of a nuclear accident.
41. Pros
-It is easier for consumers to do their own research on the chemicals used in the drugs.
-It is easier for pharmacists to determine the contents of the drugs and advise the consumer or doctor.
Cons
-It might be very easy for other companies or organizations to copy the drugs.
42. -Brittle: if lattice is shifted by an impact, like charges are forced next to each other and repel.
-Relatively strong attraction between ions: the ionic bonds must be overcome to a large degree to break down
the crystal lattice and allow the substance to melt.
-Ions arrange themselves so that there is maximum proximity to ions of opposite charge, but maximum
distance from ions of same charge. A crystal lattice is formed and ordered particles result in a solid.