Ionization potential

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 "n"th 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.

Values and trends

:"Main article:" Ionization energies of the elementsGenerally the "n"-1st ionization energy is larger than the "n"th ionization energy. The next ionization energy (the "n"-1st) involves removing an electron from an orbital closer to the nucleus. Electrons in the closer orbital experience greater forces of electrostatic attraction, and thus, require more energy to be removed.

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

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 Mg²⁺.

Electrostatic explanation

Atomic ionization energy can be predicted by an analysis using electrostatic potential and the Bohr model of the atom, as follows.

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:

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

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 "a₀". 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.

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

Quantum-mechanical explanation

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 "n"th 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.

ee also

*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

External links

* [http://equipcoservices.com/support/reference/ionization-potentials-of-common-chemicals/ Ionization Potentials of Common Chemicals]