![]() ![]() Although affinity varies greatly across the periodic table, some patterns emerge. The greater the negative value, the more stable the anion is. This affinity is known as the second electron affinity and these energies are positive.Įlectron affinity can be either positive or negative value. However, more energy is required to add an electron to a negative ion which overwhelms any the release of energy from the electron attachment process. By convention, the negative sign shows a release of energy. This affinity is known as the first electron affinity and these energies are negative. When an electron is added to a neutral atom, energy is released. ![]() To use electron affinities properly, it is essential to keep track of sign. Electron affinities are more difficult to measure than ionization energies.Īn atom of Nitrogen in the gas phase, for example, gives off energy when it gains an electron to form an ion of Nitrogen. Note that, ionization energies measure the tendency of a neutral atom to resist the loss of electrons. In other words, it can be expressed as the neutral atom’s likelihood of gaining an electron. The change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion. In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as: ![]() Electron affinity of Nitrogen is 7 kJ/mol. ![]()
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