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Periodic Trends Lab - Honors
In this graphing lab, you’ll graph 3 different atomic properties to discover trends within a family
and period on the periodic table.
Procedure 1:
1. Graph on graph paper, 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. Label element symbols at the
peaks and valleys.
2. Answer the questions below about this graph and what conclusions you would draw.
Questions - Ionization Energy (potential)
a. Define ionization energy.
b.
c.
d.
e.
f.
What is the trend as you move down a group (column)?
What is the trend as you move across a period (row)?
Which family of elements tend to be at the top of the peaks?
Which family of elements tend to be at the bottom of the “valleys”?
Arrange the following atoms in order of increasing ionization energy: lithium, oxygen,
magnesium, strontium, and chlorine. Explain your order.
Procedure 2:
1. On a new graph, graph the trend of electronegativity. The graph should have the atomic
number on the x-axis and electronegativity on the y-axis. Label element symbols at the peaks and
valleys.
2. Answer the questions below about this graph and what conclusions you would draw.
Questions - Electronegativity
a. Define electronegativity.
b. What is the trend as you move down a group (column)?
c. What is the trend as you move across a period (row)?
d. Make a simple representation of the periodic table, draw arrows to represent increasing
electronegativity.
Procedure 3:
1. Creating a third graph, graph the trend of atomic radius. The graph should have the atomic
number on the x-axis and atomic radius on the y-axis. Label element symbols at the peaks and
valleys.
2. Answer the questions below about this graph and what conclusions you would draw.
Questions - Atomic Radius
a. Define atomic radius.
b. What is the trend as you move down a group (column)?
c. What is the trend as you move across a period (row)?
d. Make a simple representation of the periodic table, draw arrows to represent an
increasing atomic radius.
e. When an atom loses an electron, what is its charge? What do you think happens to the
size of the atom?
f.
When an atom gains an electron, what is its charge? What do you think happens to the
size of the atom?
g. Arrange the following atoms in order of increasing atomic radius: potassium, carbon,
rubidium, iodine, fluorine, and lithium. Explain your order.
Properties of Elements
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