Name:_________________________Lab #:______Date:__________
Periodic Trends Lab
Background:
In this activity, you are going to discover some of the trends of the properties that exist on
the modern periodic table. To do this, you are going to graph these properties.
Objective:



To define some of the properties of the element
To graph the properties of the elements (use atomic numbers 1 through 36 only)
To determine the general trends found on the periodic table
Materials: graph paper, reference table, pencils
Procedure:
1. On a piece of graph paper, graph the trend of first ionization energy (potential). The
graph should have the atomic number on the x-axis and ionization energy on the y-axis.
2. Answer the questions about this graph and what conclusions you would draw.
3. On a piece of graph paper, graph the trend of electronegativity. The graph should have
the atomic number on the x-axis and electronegativity on the y-axis.
4. Answer the questions about this graph and what conclusions you would draw.
5. On a piece of graph paper, graph the trend of atomic radius. The graph should have the
atomic number on the x-axis and atomic radius on the y-axis.
6. Answer the questions about this graph and what conclusions you would draw.
Analysis:
Ionization Energy (Use graph on pg 174 to help answer questions)
Create the graph as described in the procedure.
1. Define ionization energy.
2. What is the trend as you move down a group (column), increase or decrease?
3. What is the trend as you move across a period (row), increase or decrease?
4. On the representation of the periodic table below, draw arrows to represent increasing
first ionization energy (potential).
Electronegativity
Create the graph as described in the procedure.
1. Define electronegativity.
2. What is the trend as you move down a group (column),
increase or decrease?
3. What is the trend as you move across a period (row), increase or decrease?
4. On the representation of the periodic table above, draw arrows to represent an increasing
electronegativity.
Atomic Radius (Use graph on page 171 to help answer questions)
Create the graph as described in the procedure.
1. Define atomic radius.
2. What is the trend as you move down a group (column), increase or decrease?
3. What is the trend as you move across a period (row), increase or decrease?
4. On the representation of the periodic table above, draw arrows to represent an increasing
atomic radius.
Summary:
1. Arrange the following atoms in order of increasing atomic radius: potassium, carbon,
rubidium, iodine, fluorine, and lithium.
2. Explain why the atomic radius decreases across a period?
3. Arrange the following atoms in order of increasing ionization energy: lithium, oxygen,
magnesium, strontium, chlorine, and tellurium.
4. Explain why ionization energy and electronegativity increases across a period?
Properties of Elements (Data)
Element
Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
Sodium
Magnesium
Aluminum
Silicon
Phosphorous
Sulfur
Chlorine
Argon
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
Ionization
Energy
(kJ/mole)
1312
2373
513
899
801
1086
1402
1314
1681
2081
496
738
577
789
1012
1000
1251
1520
419
590
633
659
651
653
717
762
760
737
746
906
579
762
947
941
1140
1351
Atomic
Radius
(pm)
Electronegativity
37
32
134
125
90
77
75
73
71
69
154
145
130
118
110
102
99
97
196
174
144
132
122
118
139
125
126
118
117
120
120
122
122
117
114
110
2.2
1
1.6
2
2.6
3
3.4
4
0.9
1.3
1.6
1.9
2.2
2.6
3.2
0.8
1
1.4
1.5
1.6
1.7
1.6
1.9
1.9
1.9
2
1.7
1.8
2
2.2
2.5
3