First ionization energy | Wikipedia audio article
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Date: 19/10/2018

This is an audio version of the Wikipedia Article:
First ionization energy

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SUMMARY
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The ionization energy (ionisation energy) (Ei) is qualitatively defined as the minimum amount of energy required to remove the most loosely bound electron, the valence electron, of an isolated neutral gaseous atom to form a cation. It is quantitatively expressed in symbols as 

X + energy →  X+ + e−where X is any atom or molecule capable of being ionized, X+ is that atom or molecule with an electron removed, and e− is the removed electron. This is an endothermic process.
Generally, the closer the electrons are to the nucleus of the atom, the higher the atom's ionization energy.
The units for ionization energy are different in physics and chemistry. In physics, the unit is the amount of energy required to remove a single electron from a single atom or molecule: expressed as an electron volt. In chemistry, the units are  the amount of energy it takes for all of the atoms in a mole of substance to lose one electron each: molar ionization energy or enthalpy, expressed as kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).Comparison of Ei of atoms in the periodic table reveals two patterns:

Ei generally increases as one moves from left to right within a given period.
Ei generally decreases as one moves down a given group.(The latter is due to the outer electron shell being progressively further away from the nucleus with the addition of one inner shell per row as one moves down the column.)
The nth ionization energy refers to the amount of energy required to remove an electron from the species with a charge of (n-1). For example, the first three ionization energies are defined as follows:

1st ionization energy
X →  X+ + e−2nd ionization energy
X+ →  X2+ + e−3rd ionization energy
X2+ →  X3+ + e−The term ionization potential is an older name for ionization energy, because the oldest method of measuring ionization energies was based on ionizing a sample and accelerating the electron removed using an electrostatic potential. However this term is now considered obsolete.
Some factors affecting the ionization energy include:

Nuclear charge: the greater the magnitude of nuclear charge the more tightly the electrons are held by the nucleus and hence more will be ionization energy.
Number of electron shells: the greater the size of the atom less tightly the electrons are held by the nucleus and ionization energy will be less
Effective nuclear charge (Zeff): the greater the magnitude of electron shielding and penetration the less tightly the electrons are held by the nucleus, the lower the Zeff of the electron, and hence less will be the ionization energy.
Type of orbital ionized: the atom having a more stable electronic configuration has less tendency to lose electrons and consequently has high ionization energy.
Occupancy of the orbital matters: if the orbital is half or completely filled then it is harder to remove electrons