Electron Affinity – Definition, Factors Affecting and Electronic Configuration

What is Electron Affinity?

Electron Affinity – Definition: Electron affinity is the measure of how much an atom or molecule attracts electrons to itself. The higher the electron affinity of an atom or molecule, the more it will pull electrons away from other atoms or molecules. Electron affinity is usually measured in units of kilojoules per mole (kJ/mol).

Factors Affecting Electron Affinity

• The electron affinity of an atom (A) is a measure of how strongly it attracts an electron to itself. The higher the electron affinity of an atom, the more likely it is to gain an electron, and the more stable the atom becomes.
• The electron affinity of an atom is affected by a number of factors, including its atomic number (Z), the number of electrons in its outer shell, and the presence of electron-attracting elements in its vicinity.
• The electron affinity of an atom also increases as the distance between the atom and the electron decreases.

Studying Electron Affinity with Infinity Learn

• Electron affinity is a measure of how much a atom or molecule will gain an electron. It is measured in units of kilojoules per mole (kJ/mol). The higher the electron affinity, the more likely the atom or molecule is to gain an electron.
• The electron affinity of an atom can be affected by its position on the periodic table. For example, atoms in the third row of the table (such as sulfur) have a lower electron affinity than atoms in the fourth row (such as carbon). This is because the third row elements have more stable electron configurations than the fourth row elements.
• The electron affinity of an atom can also be affected by its chemical environment. For example, the electron affinity of fluorine is much higher in the gas phase than it is in aqueous solution. This is because the electron affinity of fluorine is Lewis acidic in the gas phase, but it is Lewis basic in aqueous solution.