electron

Electron Affinity is the negative of the Energy Charge accompanying electron gain.

Electron Affinity refers to an isolated atom’s attraction for an additional electron, where as electronegativity is the attraction of an atom for shared electrons when it is chemically bonded to another atom . The electron affinity is experimentally measurable while electronegativity is a relative number.

Electron is a …

The amount of energy released when an Electron is added to an isolated gaseous atom is called Electron Affinity.

The amount of energy required to remove the most loosely bound Electron from an isolate gaseous atom is known as Ionisation Potential, also called Ionisation Energy. It may be represented as Atom (g) + I.E→ Positive Ion (g) + Electron (g) It is expressed in terms of eV/atom or kcal/mol or kJ/mol (1 eV per atom = 23.06 kcal/mol)

The electron that comes last in an atoms is called the differentiation electron. Based on the differentiation electron, the electron are classified into s, p, d and f blocks.

The Electronegative, x is the ability of an atom of an elements to attract electrons towards itself in a shared pair of electrons.

The lowest energy structure is the one with the smallest formal charge on the atoms. The formal charge is a factor based on a pure covalent view of bonding in which electron pairs are shared equally by neighboring atoms.

Variation in a Period In general, Atomic Radius decreases with increase in atomic numbers (going from left to right) in a Period. This is because of increase in nuclear charge due to Electrons in the same shell.

What is Electron?

Subjects

Tags