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CHAPTER 6
Review and Reinforcement of the Periodic Table
_______ 1. Which of the following metals is not an alkali metal?
a) Sodium
b) Potassium
c) Iron
d) Francium
_______2. Alkali metals must be stored under oil because of their extreme
a) Radioactivity
b) Reactivity
c) Softness
d) Brilliance
________3. Magnesium reacts with _____________ which makes magnesium fires hard to fight
a) Carbon dioxide
b) Foam
c) Water
d) Air
________4. Alkali metals are malleable, ductile, and good conductors. Why are they not used in
construction practices?
a) Too expensive
b) Too hard
c) Too brittle
d) Too soft
_________5. All of the halogens exist in elemental form as _____________ molecules.
a) Monatomic
b) Diatomic
c) Triatomic
d) Ionic
_________6. The most reactive element is
a) Bromine
b) Iodine
c) Fluorine
d) Chlorine
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_________7. Natural gas wells are a major source of today’s
a) Helium
b) Hydrogen
c) Argon
d) Xenon
________ 8. There are no known compounds of
a) Xenon
b) Krypton
c) Helium, neon, and argon
d) Any of the noble gases
________ 9. The formation of nitrogen compounds from nitrogen gas is called
a) Nitrogenation
b) Purification
c) Oxidation
d) Nitrogen fixation
_________ 10. The majority of a multi-vitamin, by mass, is made up of
a) Carbon family compounds
b) Nitrogen family compounds
c) Transition metal compounds
d) Alkaline earth metal compounds
11. Explain how Charles Hall contributed to today’s large-scale production of aluminum.
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12. Why is carbon considered to be “unique” among the elements?
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13. Compare the two forms of elemental oxygen.
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14. Why are gold alloys more commonly used for jewelry than pure gold?
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15. Why is iron such a significant metal? What is one of the disadvantages of iron?
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16. What is an alloy? Explain with an example.
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17. Why is beryllium a better choice than iron to use in an alloy for making planes?
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18. What properties distinguish metals from nonmetals?
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BUILDING THE PERIODIC TABLE
The following elements belong together in families as grouped below. The elements as listed are not
necessarily in order. The letters are NOT the normal symbols for the elements.
ZRD, SIFP, JXBE, LHT, QKA, WOV, YMC, GUN
The assignment is to rearrange these elements in the proper periodic form, according to the information
given below. Fill in the answers in the periodic table provided at the bottom of this page. Use the
ALCHEM periodic table for assistance if necessary.
1. U has a total of six electrons. (Used as an example below – U is carbon, therefore G and N are either silicon or germanium)
2. A is the second most common element in the atmosphere.
3. E is a noble gas.
4. S is an alkali metal.
5. O is a halogen.
6. O has an atomic number larder than V but smaller than W.
7. The charge on an L ion is 2+.
8. C has 5 electrons in its outer energy level.
9. The atomic mass of T is more than that of H but less than that of L.
10. M has an atomic number one less than A.
11. The electrons of atom N are distributed in 3 energy levels.
12. R has the largest atomic mass of its group.
13. F is a gas at room temperature.
14. Atom B contains 10 protons.
15. Q has an atomic mass less than K.
16. Y is more metallic than either M or C.
17. X has an atomic number one higher than F.
18. D has the smallest mass in its group.
19. P is the most reactive element in its family.
20. J has the greatest density of the elements in its group as listed.
21. Atoms of I are larger than those of S.
I
II
III
IV
U
Dotted
lines
provide
workspace
for families
GUN
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V
VI
VII
VIII
Review and Reinforcement
Reading the Periodic Table
On the line at the left, write the number of the appropriate location of each group of elements on the
periodic table below. Some letters will be used more than once.
____
____
____
____
____
____
____
1. Carbon family
2. Alkaline earth metals
3. Inner transition metals
4. Halogens
5. d-block elements
6. Oxygen group
7. Alkali metals
____
____
____
____
____
____
____
8. f-block elements
9. Noble gases
10. p-block elements
11. Nitrogen family
12. p-block elements
13. Transition metals
14. Group of 1 semi-metal & 4 metals
m
a
k
b
c
d
e
f
g
h
i
j
Use your skills to answer the following questions. Below is the abbreviated electron configuration for
sodium. Explain each part of this configuration in the space provided.
15. __________________________________________________________________
16. __________________________________________________________________
[Ne] 3 s 1
17. __________________________________________________________________
18. __________________________________________________________________
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Practice Problems
1. Chlorine, selenium, and bromine are located
near each other on the periodic table. Which of
these elements is (a) the smallest atom? (b) the
atom with the highest ionization energy?
6. Which of the following is the largest: a
potassium atom, a potassium ion with a charge
of +1, or a rubidium atom?
2. Phosphorous, sulfur, and selenium are located
near each other on the periodic table. Which of
these elements is the (a) largest atom? (b) the
atom with the highest ionization energy?
7. Which of the following is the largest: a
chlorine atom, a chlorine ion with a charge of 1-,
or a bromine atom?
3. Scandium, yttrium, and lanthanum are
located near each other in the periodic table.
Which of these elements is (a) the largest atom?
(b) the atom with the smallest ionization energy?
8. Which of the following is the smallest: a
lithium atom, a lithium ion with a charge of 1+,
or a sodium atom?
4. (a) Which of the following atoms is smallest:
vanadium, chromium, or tungsten? (b) Which of
these atoms has the highest ionization energy?
9. Which of the following is the largest: a
tellurium ion with a charge of 2-, an iodine ion
with a charge of 1-, or a xenon atom?
5. (a) Which of the following atoms is smallest:
nitrogen, phosphorus, or arsenic? (b) Which of
these atoms has the smallest ionization energy?
10. Aluminum, silicon, and phosphorous are
located near each other in the periodic table.
Which of these elements is (a) the largest atom?
(b) the atom with the highest ionization energy?
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APPLY – Two Trendy Elements
You can compare the sizes and chemical
reactivity of two atoms by looking at their
location on the periodic table. The two
diagrams at the right show the relative sizes
of a sodium atom and a chlorine atom. Use
your knowledge of periodic trends to
answer the following questions.
Sodium atom
Chlorine atom
1. Both sodium and chlorine are in the same period on the periodic table. Explain the difference in their
sizes.
2. Predict the charge that an ion of each element would have. Explain your answer.
3. Compare the amount of ionization energy required to remove the first electron from each of these
atoms.
4. Compare the electron affinities of these atoms.
5. Draw the ion for each atom. Be sure to accurately represent their sizes relative to the original atoms.
6. Explain the ions you have drawn. How do these two elements compare in size now?
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Review and Reinforcement
Periodic Trends
Use the periodic table and your knowledge of periodic trends to answer the following questions.
Which atom in each pair has the larger atomic radius?
_____ 1.
Li or K
_____ 2.
Ca or Na
_____ 3.
Ga or B
_____ 4.
O or C
_____ 5.
Cl or Br
_____ 6.
Be or Ba
_____ 7.
Si or S
_____ 8.
Fe or Au
Which ion in each pair has the smaller atomic radius?
_____ 9.
Na+ or O2-
_____ 10.
Ba2+ or I-
_____ 11.
Al3+ or P3-
_____ 12.
K+ or Cs+
_____ 13.
Fe2+ or Fe3+
_____ 14.
F- or S2-
Which atom or ion in each pair has the larger ionization energy?
_____ 15.
Na or O
_____ 16.
Be or Ba
_____ 17.
Ar or F
_____ 18.
Cu or Ra
_____ 19.
I or Ne
_____ 20.
K or V
_____ 21.
Ca or Fr
_____ 22.
W or Se
Write the charge that each of the following atoms will acquire when it has a complete set of valence e-.
_____ 23.
O
_____ 24.
Na
_____ 25.
F
_____ 26.
N
_____ 27.
Ca
_____ 28.
Ar
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Review and Reinforcement: Periodic Trends – CONTINUED
29. Define atomic radius.
30. Why do atoms get smaller as you move across a period?
31. Explain the relationship between the relative size of an ion to its atom and the charge on the ion.
32. Contrast ionization energy and electron affinity in general. In general, what can you say about these
values for metals and non-metals?
33. Why is there such a large jump in ionization energy between the second and third ionization energies
for magnesium?
34. Explain why noble gases are inert and do not form ions.
35. Define the term electronegativity. What is the periodic trend for electronegativity?
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