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# Periodic Trends: Ionization Energy

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Practice Periodic Trends: Ionization Energy
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Periodic Trends: Ionization Energy

herd of sheep

Like many other animals, sheep travel in herds.  The tendency is for each individual sheep to stay with the herd. However, a sheep may sometimes wander off, depending on how strong the attraction is for a particular food or water supply.  At other times, a sheep may become frightened and run off.  Whether a sheep chooses to stay with the herd or go its own way depends on the balance between attraction to the herd and attraction to the outside influence.

There is an on-going tension between the electrons and protons in an atom.  Reactivity of the atom depends in part on how easily the electrons can be removed from the atom.  We can measure this quantity and use it to make predictions about the behaviors of atoms.

### Ionization energy

Ionization energy is the energy required to remove an electron from a specific atom. It is measured in kJ/mol, which is an energy unit, much like calories. The ionization energies associated with some elements are described below. For any given atom, the outermost valence electrons will have lower ionization energies than the inner-shell kernel electrons. As more electrons are added to a nucleus, the outer electrons become shielded from the nucleus by the inner shell electrons. This is called electron shielding .

 Element $IE_1$ $IE_2$ $IE_3$ $IE_4$ $IE_5$ $IE_6$ H 1312 He 2373 5251 Li 520 7300 11,815 Be 899 1757 14,850 21,005 B 801 2430 3660 25,000 32,820 C 1086 2350 4620 6220 38,000 47,261 N 1400 2860 4580 7500 9400 53,000 O 1314 3390 5300 7470 11,000 13,000

If we plot the first ionization energies vs. atomic number for the main group elements, we would have the following trend

ionization energy and atomic number

Moving from left to right across the periodic table, the ionization energy for an atom increases.  We can explain this by considering the nuclear charge of the atom.  The more protons in the nucleus, the stronger the attraction of the nucleus to electrons.  This stronger attraction makes it more difficult to remove electrons.

Within a group, the ionization energy decreases as the size of the atom gets larger.  On the graph, we see that the ionization energy increases as we go up the group to smaller atoms.  In this situation, the first electron removed is farther from the nucleus as the atomic number (number of protons) increases.  Being farther away from the positive attraction makes it easier for that electron to be pulled off.

#### Summary

• Ionization energy refers to the amount of energy needed to remove an electron from an atom.
• Ionization energy decreases as we go down a group
• Ionization energy increases from left to right across the periodic table.

#### Practice

Use the following link to answer the questions below:

1. What is a “gaseous atom”?
2. Why would the ionization energy for O be somewhat less than that for N?
3. Why is a third-level electron easier to remove than a first-level one?

#### Review

1. Define “ionization energy”.
2. Do valence electrons have larger or smaller ionization energies that the inner-shell kernel electrons?
3. What is electron shielding?
4. Describe the trends in ionization energy from left to right across the periodic table.
5. Describe the trends in ionization energy from top to bottom of a group in the periodic table.
6. Why is the second ionization energy for lithium so much larger than the first ionization energy?