Name
Classification of Elements
The Periodic Table
H
He
Be
B
C
N
0
F
Ne
Na Mg
Al
Si
P
S
Cl
Ar
Cu Zn Ga Ge As Se
Br
Kr
1
Xe
Li
K
Ca Sc
Ti
V
Rb
Sr
Y
Zr
Nb Mo Tc
Ru Rh Pd
Ag
Cd
Cs
Ba La
Hf
Ta
W
Ir
Pt
Au
Hg TI Pb Bi Po At Rn
Fr
Ra Ac
Rf
Ha
Sg Uns Uno Une
Ce
Pr
Nd Pm Sm Eu Gd Tb Dy Ho
Th Pa
Cr Mn Fe Co
U
Re Os
Ni
Np Pu Am Cm Bk
Cf
In
Sn Sb Te
Er Tm Yb
Lu
Es Fm Md No
Lr
1. The elements in periods 2 through 7 that are to the left of the zigzagged line are metals.
List five metals.
2. The elements in periods 1 through 6 that are to the right of the zigzagged line are
nonmetals. List five nonmetals.
3. The elements that border either side of the zigzagged line are metalloids. Metalloids have
properties of both metals and nonmetals. Name two metalloids.
4. The alkali metals are in group 1. They have only one electron in their outer shell. They
are very reactive and have a low melting point. Shade the alkali metals blue.
5. The nobel gases are found in group 18. Their outer energy level is filled, and they are
very nonreactive, colorless gases. Shade the nobel gases red.
6. Halogens have seven electrons in the outer shell. They are located in group 17 on the
periodic table. Halogens react with metals to form salts. Shade the halogens green.
7. The transition elements are found in groups 3 through 12 and periods 4 through 7. These
elements have either one or two electrons in the outer energy level. They are often used
to form alloys because they are hard and have high melting points. Shade the transition
elements orange.
8. Alkaline earth metals are located in group 2. They have two electrons in their outer
energy level. Shade the alkaline metals purple.
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11
BASIC CHEMISTRY
PERIODIC TABLE WORKSHEET
Name
1. Where are the most active metals located?
2. Where are the most active nonmetals located?
3. As you go from left to right across a period, the atomic size ( decreases / increases ).
Why?
4. As you travel down a group, the atomic size (decreases / increases). Why?
5. A negative ion is (larger / smaller) than its parent atom.
6. A positive ion is (larger / smaller) than its parent atom.
7. As you go from left to right across a period, the first ionization energy generally
( decreases / increases). Why?
8. As you go down a group, the first ionization energy generally ( decreases / increases).
Why?
9. Where is the highest electronegativity found?
10. Where is the lowest electronegativity found?
11. Elements of Group 1 are called
.
12. Elements of Group 2 are called
.
13. Elements of Group 3-12 are called.
14. As you go from left to right across the periodic table, the elements go from
( metals / nonmetals) to ( metals / nonmetals ).
15. Group 17 elements are called
16. The most active element in Group 17 is
17. Group 18 elements are called
18. What sublevels are filling across the Transition Elements?.
19, Elements within a group have a similar number of
20. Elements across a series have the same number of.
21. A colored ion generally indicates a
22. As you go down a group, the elements generally become ( more / less) metallic.
23. The majority of elements in the periodic table are (metals / nonmetals ).
24. Elements in the periodic table are arranged according to their
25. An element with both metallic and nonmetallic properties is called a
Chemistry IF8766
36
©Instructional Fair, Inc.
Name
__^_ Date
Periodic Trends Worksheet
Directions: Use your notes to answer the following questions.
1. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen,
potassium.
2. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
3. Why does fluorine have a higher ionization energy than iodine?
4. Why do elements in the same family generally have similar properties?
5. Indicate whether the following properties increase or decrease from left to right across the
periodic table.
a. atomic radius (excluding noble gases)
b. first ionization energy
c. electronegativity
6. What trend in atomic radius occurs down a group on the periodic table? What causes this
trend?
7. What trend in ionization energy occurs across a period on the periodic table? What causes
this trend?
8. Circle the atom in each pair that has the largest atomic radius.
a. Al or B
b. Na or Al
c. S or O
d. O or F
e. Br or Cl
f. Mg or Ca
9.
Circle the atom in each pair that has the greater ionization energy.
a. Li or Be
b. Ca or Ba
c. Na or K
d. P or Ar
e. Cl or Si
f. Li or K
10. Define electronegativity.
11. Circle the atom in each pair that has the greater electronegativity.
a. Ca or Ga
b. Br or As
c. Li or 0
d. Ba or Sr
e. Cl or S
f. O or S
PERIODIC TABLE WORKSHEET
Name
1, Where are the most active metals located?
2. Where are the most active nonmetals located?
3. As you go from left to right across a period, the atomic size ( decreases / increases).
Why?
4. As you travel down a group, the atomic size (decreases / increases). Why?
5. A negative ion is (larger / smaller) than its parent atom.
6. A positive ion is (larger / smaller) than its parent atom.
7. As you go from left to right across a period, the first ionization energy generally
( decreases / increases). Why?
8. As you go down a group, the first ionization energy generally (decreases / increases).
Why?
9. Where is the highest electronegativity found?
10. Where is the lowest electronegativity found?
11. Elements of Group 1 are called
.
12. Elements of Group 2 are called
.
13. Elements of Group 3-12 are called.
14, As you go from left to right across the periodic table, the elements go from
( metals / nonmetals ) to ( metals / nonmetals).
15. Group 17 elements are called
16. The most active element in Group 17 is
17. Group 18 elements are called
18. What sublevels are filling across the Transition Elements?.
19. Elements within a group have a similar number of
20. Elements across a series have the same number of.
21. A colored ion generally indicates a
22. As you go down a group, the elements generally become ( more / less) metallic.
23. The majority of elements in the periodic table are (metals / nonmetals).
24. Elements in the periodic table are arranged according to their
25. An element with both metallic and nonmetallic properties is called a
Chemistry IF8766
36
©Instructional Fair, Inc.