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The ionization potential, ionization energy or E_{I} of an atom or molecule is the energy required to remove an electron from the isolated atom or ion. More generally, the nth ionization energy is the energy required to strip it of the nth electron after the first $n-1$ electrons have been removed. It is considered a measure of the "reluctance" of an atom or ion to surrender an electron, or the "strength" by which the electron is bound; the greater the ionization energy, the more difficult it is to remove an electron. The ionization potential is an indicator of the reactivity of an element. Elements with a low ionization energy tend to be reducing agents and to form salts.

- Main article: Ionization energies of the elements

Some values for elements of the third period are given in the following table:

Element | First | Second | Third | Fourth | Fifth | Sixth | Seventh |
---|---|---|---|---|---|---|---|

Na | 496 | 4,560 | |||||

Mg | 736 | 1,450 | 7,730 | ||||

Al | 577 | 1,816 | 2,881 | 11,600 | |||

Si | 786 | 1,577 | 3,228 | 4,354 | 16,100 | ||

P | 1,060 | 1,890 | 2,905 | 4,950 | 6,270 | 21,200 | |

S | 999.6 | 2,260 | 3,375 | 4,565 | 6,950 | 8,490 | 27,107 |

Cl | 1,256 | 2,295 | 3,850 | 5,160 | 6,560 | 9,360 | 11,000 |

Ar | 1,520 | 2,665 | 3,945 | 5,770 | 7,230 | 8,780 | 12,000 |

Large jumps in the successive ionization energies occur when passing noble gas configurations. For example, as can be seen in the table above, the first two ionization energies of magnesium (stripping the two 3s electrons from a magnesium atom) are much smaller than the third, which requires stripping off a 2p electron from the very stable neon configuration of Mg^{2+}.

Consider an electron of charge -e, and an ion with charge +ne, where n is the number of electrons missing from the ion. According to the Bohr model, if the electron were to approach and bind with the atom, it would come to rest at a certain radius a. The electrostatic potential V at distance a from the ionic nucleus, referenced to a point infinitely far away, is:

$V\; =\; frac\{1\}\{4piepsilon\_0\}\; frac\{ne\}\{a\}\; ,!$

Since the electron is negatively charged, it is drawn to this positive potential. (The value of this potential is called the ionization potential). The energy required for it to "climb out" and leave the atom is:

$E\; =\; eV\; =\; frac\{1\}\{4piepsilon\_0\}\; frac\{ne^2\}\{a\}\; ,!$

This analysis is incomplete, as it leaves the distance a as an unknown variable. It can be made more rigorous by assigning to each electron of every chemical element a characteristic distance, chosen so that this relation agrees with experimental data.

It is possible to expand this model considerably by taking a semi-classical approach, in which momentum is quantized. This approach works very well for the hydrogen atom, which only has one electron. The magnitude of the angular momentum for a circular orbit is:

$L\; =\; |mathbf\; r\; times\; mathbf\; p|\; =\; rmv\; =\; nhbar$

The total energy of the atom is the sum of the kinetic and potential energies, that is:

$E\; =\; T\; +\; U\; =\; frac\{p^2\}\{2m\_e\}\; -\; frac\{ke^2\}\{r\}\; =\; frac\{m\_e\; v^2\}\{2\}\; -\; frac\{ke^2\}\{r\}$

Velocity can be eliminated from the kinetic energy term by setting the Coulomb attraction equal to the centripetal force, giving:

$T\; =\; frac\{ke^2\}\{2r\}$

Now the energy can be found in terms of k, e, and r. Using the new value for the kinetic energy in the total energy equation above, it is found that:

$E\; =\; -\; frac\{ke^2\}\{2r\}$

Solving the angular momentum for v and substituting this into the expression for kinetic energy, we have:

$frac\{n^2\; hbar^2\}\{rm\_e\}\; =\; ke^2$

This establishes the dependence of the radius on n. That is:

$r(n)\; =\; frac\{n^2\; hbar^2\}\{km\_e\; e^2\}$

At its smallest value, n is equal to 1 and r is the Bohr radius a_{0}. Now, the equation for the energy can be established in terms of the Bohr radius. Doing so gives the result:

$E\; =\; -\; frac\{1\}\{n^2\}\; frac\{ke^2\}\{2a\_0\}\; =\; -\; frac\{13.6eV\}\{n^2\}$

This can be expanded to larger nuclei by incorporating the atomic number into the equation.

$E\; =\; -\; frac\{Z^2\}\{n^2\}\; frac\{ke^2\}\{2a\_0\}\; =\; -\; frac\{13.6\; Z^2\}\{n^2\}eV$

According to the more complete theory of quantum mechanics, the location of an electron is best described as a "cloud" of likely locations that ranges near and far from the nucleus, or in other words a probability distribution. The energy can be calculated by integrating over this cloud. The cloud's underlying mathematical representation is the wavefunction which is built from Slater determinants consisting of molecular spin orbitals. These are related by Pauli's exclusion principle to the antisymmetrized products of the atomic or molecular orbitals. This linear combination is called a configuration interaction expansion of the electronic wavefunction.

In general, calculating the nth ionization energy requires calculating the energies of $Z-n+1$ and $Z-n$ electron systems. Calculating these energies is not simple, but is a well-studied problem and is routinely done in computational chemistry. At the lowest level of approximation, the ionization energy is provided by Koopmans' theorem.

- Bragg-Gray Cavity Theory
- Electronegativity
- Ionization
- The ionization potential is equal to the ionization energy divided by the charge of an electron.
- The work function is the energy required to strip an electron from a solid.
- Ion
- Koopmans' theorem
- Di-tungsten tetra(hpp) has the lowest recorded ionization energy for a stable chemical compound.
- Electron affinity

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Last updated on Saturday October 11, 2008 at 05:10:30 PDT (GMT -0700)

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This article is licensed under the GNU Free Documentation License.

Last updated on Saturday October 11, 2008 at 05:10:30 PDT (GMT -0700)

View this article at Wikipedia.org - Edit this article at Wikipedia.org - Donate to the Wikimedia Foundation

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