Question

What is the difference between electronegativity and ionization energy

Answer 1

Ionization energy is the reverse of electronegativity. Ionization energy tells you how easily or how attracted you are to your own electrons so how hard is for somebody to steal them so it's about how much you hold on to your electrons.

Electronegativity is a chemical property and it's about how much can I steal somebody else's electrons. They are like two sides of the same coin. Electronegativity is affected by both its atomic number (number of protons in the core of an atom) and how far the valence electrons (the outermost electrons) are from the core.

Answer 2

These properties are basically the inverse of each other.

Step-by-step explanation:

• Electronegativity is the tendency of an atom to attract an electron and make it a part of its orbital.

Ionization enthalpy, is the energy required to remove an electron from an atom.

• More electronegative atoms have high ionization enthalpies If the energy required to remove an electron is less, i.e. the atom has more tendency to give electron, it would thus have less tendency to take electron.
• Values and tendency of electronegativity in the periodic table: In general, the electronegativity of a non‐metal is larger than that of metal. For the elements of one period the electronegativities increase from left to right across the periodic table. For the elements of one main group the electronegativities decrease from top to bottom across the periodic table. To the subgroup elements, there’s no regular rule.
• Values and tendency of ionization potential in the periodic table: The first ionization energy is the energy which is required when a gaseous atom/ion loses an electron to form a gaseous +1 valence ion. The energy which is required for a gaseous +1 valence ion to loose an electron to form a gaseous +2 valence ion, is called the second ionization energy of an element. In general, the second ionization energy is higher than the first ionization energy of an element. The first ionization energies of the elements of one period increase from the left to the right across the periodic table. According to the elements of main group, the first ionization energies generally decreases from top to bottom across the periodic table.