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TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
What is ionization energy?
The energy required to remove an electron from an atom
is called ionization energy.
• This energy is measured when an element is in its
gaseous state.
• The energy required to remove the first electron
from an atom is called the first ionization energy.
• The energy required to remove the second electron
from an atom is called the second ionization energy
and so on and so forth. ☺
TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
Trends in ionization energy
Looking at the data for alkali metals and noble gases, first ionization energy generally
decreases from top to bottom within a group.
Looking at the data from sodium to argon, first ionization energy generally increases
across a period.
TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
Explanation for trends in ionization energy
Down a Group
As the distance from nucleus to electrons increases within a group:
• Nuclear charge has a smaller effect on the electrons in the
highest occupied energy level due to shielding effects (Zeff
is constant) and this means less energy is required to
remove an electron from this energy level—first ionization
energy is lower
Across a Period
In general, the first ionization energy of representative elements
tends to increase from left to right across a period. This trend can
be explained by the nuclear charge and the shielding effect.
• The nuclear charge increases across the period, but the
shielding effect remains constant (Zeff increases across a
group.)
• As a result, there is an increase in the attraction of the
nucleus for an electron. Thus, it takes more energy to
remove an electron from an atom.
TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
What is electronegativity?
Electronegativity is the ability of an atom of an element to attract
electrons when the atom is in a compound.
• Scientists use factors such as ionization energy to calculate values
for electronegativity.
• In your own words, describe the difference between ionization
energy and electronegativity?
TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
Electronegativity Values for Selected
Elements (Pauling Units)
H
2.1
Li
1.0
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Be
1.5
Mg
1.2
Ca
1.0
Sr
1.0
Ba
0.9
B
2.0
Al
1.5
Ga
1.6
In
1.7
Tl
1.8
C
2.5
Si
1.8
Ge
1.8
Sn
1.8
Pb
1.9
N
3.0
P
2.1
As
2.0
Sb
1.9
Bi
1.9
O
3.5
S
2.5
Se
2.4
Te
2.1
F
4.0
Cl
3.0
Br
2.8
I
2.5
TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
Trends in electronegativity
In general, electronegativity values decrease from top to bottom within a group.
For representative elements, the values tend to increase from left to right across a
period.
• Metals at the far left of the periodic table have low values.
• Nonmetals at the far right (excluding noble gases) have high values.
• The values among the transition metals are not as regular.
In your own words, explain these
trends in electronegativity
TEKS 5C: Use the Periodic Table to identify and explain periodic trends, including atomic and
ionic radii, electronegativity, and ionization energy.
Summary: periodic trends