![]() This is due to an increase in the nuclear charge and decrease in size of the atoms. the amount of energy released will be more. As we move from alkali metals to halogens in a period, generally electron affinity increases, i.e. The variation of electron affinity is not as systematic as in the case of ionisation energy. Variation of Electron Affinity in a period: Tellurium has a more negative electron affinity value than potassium and phosphorus.It is defined as the amount of energy released (required in the case noble gases) when an electron is added to the valence shell of an isolated neutral gaseous atom in its ground state to form its anion.Potassium has a more positive electron affinity value than phosphorous.Ne has the most positive electron affinity value and Br has the most negative electron affinity.Then, repulsion forces increase between the newly joined electron and the valence electrons present in the larger orbitals of the atom. In groups, electron affinity from top to bottom decreases because the number of electrons increase in an atom as we go down through a column. Therefore, VIIA group elements readily capture the electrons and release the energy. From the modern periodic table, it is clear that Ne belongs to inert gas group elements while Br in VIIA group element needs an electron to get inert gas configuration. In the same way, tellurium has a more negative electron affinity than potassium and phosphorus.Įlectron affinity values are compared for the given elements by using their behavior in period and groups in a modern periodic table. ![]() Potassium has a more positive electron affinity value than phosphorous, since electron affinity decreases from top to bottom and increases from left to right in periodic the table. Therefore, Ne has the most positive electron affinity value Br and has the most negative electron affinity value among the given elements. We know that inert gas elements have the most positive electron affinity values and the VIIA group elements have the most negative electron affinity values in the modern periodic table. Given atoms are neon, potassium, phosphorous, tellurium, and bromine In groups, electron affinity decreases from top to bottom because the number of electrons increases in the atom as we go down a column.In periods, the main group elements’ electron affinity increases from left to right while the groups’ electron affinity decreases from top to bottom.In the modern periodic table, inert gases have the most positive electron affinity values while the VIIA group elements have the most negative electron affinity values, as they achieve inert gas configuration.Inert gases have the most positive electron affinity values, since they are inert in nature. Neon,potassium,phosphorous,tellurium,bromine.Įlectron affinity is an energy that is released during the addition of an electron to the neutral atom in its gaseous state to form a negatively charged ion. To rank items as equivalent, overlap them. Rank from most positive to most negative. Rank the following elements by electron affinity, from most positive to most negative value.
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