Name ______________________________________________ Date ______/______/______ Period ________
Chapter 5  Periodicity Activity
ATOMIC
RADII
Directions: Using the given data for the sizes of atoms (atomic radii) below,
1. Create a line graph (use a ruler) by graphing Period 2’s data on the graph below.
2. In a different color, create a line graph Period 3’s data on the same graph.
3. Label each axis, and include a key/legend.
4. Answer all questions.
1
H
30
Li
123
Na
157
K
203
Rb
216
Cs
235
1
2
3
4
5
6
2
13
14
15
16
17
O
66
S
104
Se
117
Te
137
Po
153
F
64
Cl
99
Br
114
I
133
At
-----
18
He
----Ne
----Ar
----Kr
----Xe
----Rn
-----
Atomic Radii
Be
89
Mg
136
Ca
174
Sr
192
Ba
198
B
88
Al
125
Ga
125
In
150
Tl
155
C
77
Si
117
Ge
122
Sn
140
Pb
154
N
70
P
110
As
121
Sb
141
Bi
152
Note: Mark the vertical axis from 0 – 160 (by 20’s)
Trend in Atomic Size Across the Periodic Table
Li
Na
Be
Mg
B
Al
C
Si
N
P
O
S
F
Cl
Horizontal Trend Questions
1. What is the trend in atomic size as you go across the periodic table? _______________________________
2. This is true because there are more _____________________ (protons / electrons / layers of electrons)
pulling the electron cloud in toward the nucleus.
Vertical Trend Questions
3. Examine the sizes of the Group 1 elements (H, Li, Na, K, Rb, Cs). What is the trend in atomic size as you go
down a column of the periodic table? ________________________________________
4. This is true because there are more ______________________ (protons / electrons / layers of electrons)
making the electron cloud larger.
5  Periodicity Activity
IONIZATON
ENERGY
Directions: Using the given data for the ionization energy below,
1. Create a line graph (use ruler) on GRAPH PAPER by plotting the ionization energies of given elements.
2. Plot the ionization energy (I) of each element (y axis) against the element’s atomic number, Z (x axis).
3. Plot the atomic numbers consecutively as they are listed. For example, plot 2 after 1, element 18 after
17, and element 31 after 20, and so on.
4. Label each data point with the symbol of the element it represents (H for hydrogen, Li for lithium, etc.)
5. Label each axis, and include a meaningful title for your graph.
6. Answer all questions.
Note: To make the numbers easier to graph, the ionization energies have been made relative to that of
hydrogen, so that IH = 1.00)
Note: This graph has
already been done for
you on the next page.
Use the graph to answer
the following questions.
Questions
1. What is ionization energy?
(Use the graph you have just made to answer the following questions)
2. As you progress across a row of the periodic table, what general pattern in Ionization Energy do you see?
3. What do the elements in the first column of the periodic table have in common?
4. What do the elements in the last column of the periodic table have in common?
5. From which family of elements on the periodic table would it be easiest to remove an electron? Why?
6. From which family of elements would it be most difficult to remove an electron? Why?
7. Explain why your graph has “dips” as you go across a row.
Sample Graph
Chemistry Class – Extra Credit Activity
South Pasadena  AP Chemistry
Name ___________________________________
Due Date: __Monday, March 16th, 2015________
8  Electron Configurations & Chemical Periodicity
BUILDING THE PERIODIC TABLE
The following elements belong together in families as grouped below. The elements listed are not necessarily
in order. The letters are not the symbols for the elements.
ZRD, SIFP, JXBE, LHT, QKA, WOV, YMC, GUN
The assignment is to arrange 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 your periodic table for
assistance if necessary.
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
U has a total of six electrons.
(Used as an example below – U is carbon, therefore G and N are either silicon or germanium.)
A is the second most common element in the atmosphere.
E is a noble gas.
S is an alkali metal.
O is a halogen.
O has an atomic number larger than V but smaller than W.
The charge on an L ion is 2+.
C has five electrons in its outer energy level.
The atomic mass of T is more than that of H but less than that of L.
M has an atomic number one less than that of A.
The electrons of atom N are distributed in three energy levels.
R has the largest atomic mass of its group.
F is a gas at room temperature.
Atom B contains 10 protons.
Q has an atomic mass less than that of K.
Y is more metallic than either M or C.
X has an atomic number one higher than F.
D has the smallest atomic mass in its group.
P is the most reactive element in its family.
J has the greatest density of the elements in its group as listed.
Atoms of I are larger than those of S.
I
VIII
II
III
IV
U
the dotted lines provide
a workspace for listing
the families
GUN
V
VI
VII