Peridic Table
Name________________________________
Period_______Date_____________________
1. Write down the atomic masses for lithium and potassium below. Calculate the average mass for
sodium using the atomic masses of lithium and potassium. Record this value, and the actual atomic
mass from the periodic table.
Li
Lithium:
Na
Sodium:
K
Potassium:
Rb
Cs
Actual
______________ amu
?
amu
______________ amu
Average (Na) ______________ amu
How does the average atomic mass compare
to the actual mass on the periodic table?
Fr
(Na)
______________ amu
__________________________________
______ 3. carbon family
______ 10. f-block elements
______ 4. alkaline earth metals
______11. noble gases
______ 5. inner transition metals
______ 12. p-block elements
______ 6. halogens
______ 13. nitrogen family
______ 7. d-block elements
______ 14. s-block elements
______ 8. oxygen family
______ 15. transition metals
______ 9. alkali metals
______ 16. group of one metalloid & four metals
M
A
K
B
C
D
E
F
J
G
H
I
On the line at the left, write the letter of the contribution that each chemist made to the periodic table. Each
letter will only be used once.
______ 17. Dmitri Mendeleev
A. arranged elements by atomic number
______ 18. H.G.J. Moseley
B. grouped elements into sets of three
______ 19. J.W. Dobereiner
C. predicted the existence and properties of three undiscovered
elements
D. organized elements into repeating groups of eight, which he
termed octaves.
______ 20. J.A.R Newlands
Explain the abbreviated electron configuration
for sodium:
Write the abbreviated electron configuration
for strontium:
a. ______________________
e. _________________________________
b. ______________________
Write the abbreviated electron configuration
[Ne] 3s1
for sulfur:
c. ______________________
d. ______________________
f. _________________________________
Identify each of the following elements as a metal (M), nonmetal, (NM), or semimetal (metalloid) (SM).
________ 21. sodium
________ 22. silicon
________ 23. neon
________ 24. calcium
________ 25 nitrogen
________ 26. hydrogen
Write the family names that have been given for each of the following groups:
27. Group IA (1)
____________________________________________
28. Group IIA (2)
____________________________________________
29. Group VIIA (17) ____________________________________________
30. Group VIIIA (18) ____________________________________________
32. What properties distinguish metal from nonmetals?
_______________________________________________________________________________
_______________________________________________________________________________
33. Use the periodic table to decide which atom in each pair has the larger atomic radius?
_____ a. Li or K
_____ b. Ca or Ni
_____ c. Ga or B
_____ d. O or C
_____ e. Cl or Br
_____ f. Be or Ba
_____ g. Si or S
_____ h. Fe or Au
34. Use the periodic table to decide which ion has the smaller atomic radius?
_____ a. K+ or O2_____ b. Ba2+ or I_____ c. Al3+ or P3_____ d. K+ or Cs+
_____ e. Fe2+ or Fe3+
_____ f. F- or S235. Use the periodic table to decide which atom or ion has the larger ionization energy?
_____ a. Na or O
_____ b. Be or Ba
_____ c. Ar or F
_____ d. Cu or Ra
_____ e. I or Ne
_____ f. K or V
_____ g. Ca or Fr
_____ h. W or Se
36. Write the charge that each atom will acquire when it has a complete set of valence electrons.
_____ a. O
_____ b. Na
_____ c. F
_____ d. N
_____ e. Ca
_____ f. Ar
37. Define atomic radius: ________________________________________________________________
_______________________________________________________________________________
38. Why do atoms get smaller as you move across a period? ____________________________________
_______________________________________________________________________________
39. Explain the relationship between the relative size of an ion to its atom and the charge on the ion.
_______________________________________________________________________________
_______________________________________________________________________________
40. Explain why noble gases are inert and do not form ions. ____________________________________
41. Chlorine, selenium and bromine are located near each other on the periodic table. Which of these
elements a) is the smallest? b) has the highest ionization energy?
42. Phosphorus, sulfur and selenium are located near each other on the periodic table. Which of these
elements a) is larger? b) has the highest ionization energy?
43. Scandium, yttrium and lanthanum are located near each other on the periodic table. Which of these
elements a) is larger? b) has the smaller ionization energy?
44. a) Which of the following atoms is smallest: vanadium, chromium or tungsten? b) Which has the
highest ionization energy?
45. a) Which of the following atoms is smallest: nitrogen, phosphorus or arsenic? b) Which of these atoms
has the smallest ionization energy?
46. Which of the following is the largest: a potassium atom, a potassium ion with a +1 charge, or a rubidium
atom?
47. Circle the largest:
Cl
Cl-1
Br
48. Circle the smallest:
Li
Li+1
Na
49. Circle the largest:
Te-2
I-1
Xe
50. Aluminum, silicon and phosphorus are located near each other on the periodic table. Which of these
elements a) is the largest? b) has the highest ionization energy?
Review Questions and Problems
Origin and Arrangement
51. The first periodic law and table was proposed by the Russian scientist _________________________.
52. How was the early periodic law different from the modern law?
_______________________________________________________________________________________
___________________________________________________________________________________
53. The horizontal rows in the periodic table are called __________________. The number of a period is
the same as the number of the ___________________ principle energy level containing electrons.
54. The vertical columns of the periodic table are called __________________ or ___________________.
55. Why do members of a group exhibit similar chemical properties?
____________________________________________________________________________________
________________________________________________________________________________
Metals
56. Where are the metals located on the periodic table? ______________________
57. What names are given to these groups of metals? Group 1 ________________ Group 2
___________________________________________
58. What groups contain the most reactive metals?
_________________________________________________________________________________
59. What are some of the general physical and chemical properties of metals?
____________________________________________________________________________________
________________________________________________________________________________
Nonmetals
60. Where are the nonmetals found in the periodic table? ____________________
61. Which groups contain the most reactive nonmetals? _____________________
62. What is the name given to group 17? ____________________
63. What are some of the general physical and chemical properties of nonmetals?
____________________________________________________________________________________
________________________________________________________________________________
Other categories
64. What is a metalloid (semimetal)?
____________________________________________________________________________________
________________________________________________________________________________
65. List the seven metalloids:
__________________________________________________________________________________
66. Where are the transition metals located on the table? _______________________________________
67. What characteristic of atomic structure distinguishes the transition elements from the representative
elements?
____________________________________________________________________________________
________________________________________________________________________________
68. Why are the elements in group 18 called inert?
____________________________________________________________________________________
________________________________________________________________________________
Part II: Using Elements 1-14 shown below, answer the following questions.
1
3
6
9
8
2
7
5
13
4
14
10
11
12
69. Element ______ is an alkaline earth metal.
76. Element ______ is a nonreactive gas.
70. Element ______ is in the oxygen family.
77. Element ______ 4 valence electrons.
71. Element ______ is an alkali metal.
78. Element ______ is in the lanthanide series.
72. Element ______ is a metalloid.
79. Element ______ is a halogen.
73. Element ______ is a gas with 1 valence electron.
80. Element ______ is the only liquid metal.
74. Element ______ is in Period 5.
81. Element ______ is man-made.
75. Element ______ is the alkaline earth
metal with the smallest atomic radius.
82. Element ______ has the highest melting point,
and its abbreviated configuration is: [Xe]6s24f145d4
Review Trends: Summarize the following trends across and down the Periodic Table radius, (AR), ionization energy, (IE), electron affinity, (EA), and electronegativity, (EN)
atomic
Part III: Practice Problems
83. Circle the atom in each pair that has a larger radius.
a. Sn, Sr
b. Cl, I
c. Na, Rb
d. Mg, Be
e. S,P
f. Pa, U
g. B, Al
h. Au, Ba
i. Mg, Na
j. K, Ca
k. Al, B
l. Br, Cl
i. Fe, Fe3+
j. S2-, S
k. Se2-, Kr
l. Br-, Se2-
m. F, N
n. Ne, Ar
84. Circle the particle in each pair that has a larger radius.
a. Ca, Ca2+
b. F-, Cl-
c. As3-, P3d. Pb4+, Pb
e. Mg2+, Be2+ g. C, C4f. Te2+, Te
h. Ag, Ag+
85. Predict the oxidation number (charge after the atom gains or loses electrons) for these elements:
a. Al
b. N
c. Cl
d. Ca
e. Mg
f. S
g. Na
h. C
i. Ar
j. Be
k. K
l. Rn
86. How many electrons were gained or lost to produce the following ions?
a. K+
b. O2-
c. Ga3+
d. P3-
e. Sn4+
f. Br-
g. Ca2+
h. Sc3+
87. Circle the atom in each pair that has a lower first ionization energy.
a. N, O
b. Te, Sn
c. Ne, F
d. C, Ge
e. Br, I
f. Mg, Ca
g. I, Sb
h. Al, N
i. F, S
88. Circle the element would have the highest 1st ionization energy? Na, Mg, Al
Circle the element would have the highest 2nd ionization energy? K, Ca, Ga
Circle the element would have the highest 3rd ionization energy?
Periodic Table
Be, B, C
Periodic Table Puzzle
1
18
2
13
14
15
16
The following sets of elements belong together in
groups:
ZRD, PSIF, JXBE, LHT, QKA, WOV, GUN, YMC
J has an atomic number three times that of T
U has a total of six electrons
I2A is the simple formula of an oxide
P is less dense thanS
S is an alkali metal
E is a noble gas
W is a liquid
Z has the smallest atomic mass in its group
B has ten protons
O has an atomic number larger than V
D has the largest atomic mass of its group
C has five electrons in its outer energy level
F is a gas
X has an atomic number one higher than F
L is an alkaline earth metal with atomic mass of 40
Y is a metalloid
O is a halogen
The atomic mass of T is more than that of H
Q has an atomic mass 2 times that of A
Atoms of I are larger than those of S
M has an atomic number one less than that of A
The electrons of atom N are distributed over three energy levels
The atomic radius of K is the largest of the group
17