300 Chemistry Problem Set
Periodic Table/Trends
1. Fill in the table below
Description/Beginning of Sentence
1. As one goes down the vertical
column in a given family in the
Periodic Table, the radius of the
atom
2. As one goes from left to right in the
same period of the Periodic Table,
the radius of the atom
3. The size of the atom gets bigger as
one goes down a column of a given
group in the Periodic Table because
the number of principal energy
levels
4. The size of the atom gets bigger as
one goes down a column of a given
group in the Periodic Table because
the number of inner electrons
5. The size of the atom gets bigger as
one goes down the column of a
group on the Periodic Table because
the attraction of the outer electrons
to the nucleus is reduced by the
6. The reduction of the attractive force
between the outer electrons and the
nucleus due to the inner electrons is
called the
7. Within a given period, as the atomic
number increases, the size of the
atom
8. As one goes from left to right on the
Periodic Table, the atomic number
increases because of an increase in
the number of
9. As one goes from left to right across
a period, the atomic radius decreases
because of the increased attraction
of the electrons by an increased
number of
10. This describes the attraction of
electrons toward the nucleus,
drawing them closer to the nucleus
11. The energy needed to remove an
Answer/End of Sentence
electron from an atom is called
12. As one moves down a group, the
ionization energy needed to remove
an electron to form an ion
13. As one moves down a group, the
reason that the ionization energy
decreases, making it easier to
remove an electron is that the
electrons are farther from the
14. As one moves down a group, the
reason the ionization energy
decreases, making it easier to
remove an electron is that there is an
increase in
15. As one moves left to right across a
period, the ionization energy needed
to remove an electron tends to
16. As one moves left to right across a
period, the ionization energy needed
to remove an electron increases
because there is an increase in
17. The tendency of an atom to attract
other electrons to itself is referred to
as
18. As one moves down a group, the
electronegativity
19. As one moves left to right across a
period, the electronegativity
20. These elements are an exception to
the increase of electronegativity
from left to right across the Periodic
Table
21. These 2 things tend to increase as
one moves down a group on the
Periodic Table
22. These 2 things tend to decrease as
one moves down a group on the
Periodic Table
23. These 3 things tend to increase as
one moves left to right across a
period on the Periodic Table
24. This tends to decrease as one moves
left to right across a period on the
Periodic Table
25. These 2 things tend to remain
constant as one moves left to right
across the Periodic Table
2. Respond to the questions below:
a. Where are the most active metals located?
b. Where are the most active nonmetals located?
c. As you go left to right across a period, what does atomic size do and why?
d. As you travel down a group, what does atomic size do and why?
e. As you go from left to right across a period, what does ionization energy
do and why?
f. As you go down a group, what does ionization energy do and why?
g. Where is the highest electronegativity found?
h. Where is the lowest electronegativity found?
i. Elements of Group 1 are called…
j. Elements of Group 2 are called…
k. Elements of Groups 3 to 12 are called…
l. Where are the metals located? Nonmetals?
m. Elements of Group 17 are called…
n. The most active element in Group 17 is…
o. Elements of Group 18 are called…
p. What sublevels are filling across the transition elements?
q. What sublevels are filling in the first two groups of representative
elements?
r. What sublevels are filling across the last 6 groups of representative
elements?
s. Elements within a group have a similar number of …
t. Elements across a period have a similar number of …
u. A colored ion generally indicates a …
v. As you go down a group, what happens to the metallic character of
elements and why?
w. What is an element with both metallic and nonmetallic properties called
and where would one be located on the Periodic Table?
3. Respond to the following questions:
a. Rank the following elements by increasing atomic radius: carbon,
aluminum, oxygen, potassium.
b. Rank the following elements by increasing electronegativity: sulfur,
oxygen, neon, aluminum.
c. Why does fluorine have a higher ionization energy than iodine?
d. Why do elements in the same group tend to behave similarly in chemical
reactions?
e. Rank in order of increasing atomic radius: K, Na, Rb.
f. Rank in order of increasing atomic radius: Br, I, F.
g. Rank in order of increasing atomic radius: N, O, F.
h. Rank in order of increasing atomic radius: Zr, Ru, Ag.
i. Explain the trend for atomic radius going across the periods of the
Periodic Table.
j. Explain the trend for atomic radius going down the groups of the Periodic
Table.
k. Rank in order of increasing ionization energy: Ca, Mg, Ra.
l. Rank in order of increasing ionization energy: Cr, W, Mo.
m. Rank in order of increasing ionization energy: Al, P, Si.
n. Rank in order of increasing ionization energy: Xe, Te, Sn.
o. Explain the trend for ionization energy going across the periods.
p. Explain the trend for ionization energy going down the groups.
q. Rank in order of decreasing electronegativity: Li, Na, Cs.
r. Rank in order of decreasing electronegativity: Si, Cl, P.
s. Rank in order of decreasing electronegativity: Se, Br, Kr.
t. Rank in order of decreasing electronegativity: F, B, C.
u. Explain the trend for electronegativity going across the periods.
v. Explain the trend for electronegativity going down the groups.
w. Rank in order of decreasing ionic radius: Be, Sr, Mg.
x. Rank in order of decreasing ionic radius: Cl, F, I.
y. Explain the trend for ionic size going across the periods.
z. Explain the trend for ionic size going down the groups.
For additional practice:
Relevant sections in book is 11.11
Additional practice problems can be found on p. 356 (48-57) and p. 357 (68, 69, 71-74)