Electron Affinity and Metallic Character - Edubirdie

University:
University of Arkansas
Course:
CHEM 1103 | University Chemistry I
Academic year:

2019
Views:

55

Pages:

1
Author:

BobN

Electron affinity is the energy released when an electron is added to a gaseous atom or ion. Electron affinities are generally negative - that is, exothermic - because energy is generally released when an electron is added. We can represent this process using the equation shown, where the electron is a reactant being added to a chlorine gas atom. For group 1A metals, electron affinity becomes less exothermic as we move down the column. Across a row, electron affinity generally increases. However, noble gases have electron affinities greater than zero because they are already stable. The process of adding an electron to a noble gas does not release energy. Metallic character is how much an element acts like a characteristic metal. Metallic character increases to the left and down in the periodic table. This makes sense given that our nonmetals are in the top right of the periodic table. We can see this trend if we move down a column from nitrogen to bismuth. Nitrogen is a nonmetal and a gas at room temperature. Bismuth is a metal, acting as a better conductor of heat and electricity. It's a solid at room temperature and shiny. We can also see this trend if we move to the left across a row from chlorine to sodium. Chlorine is also a nonmetal and a gas at room temperature. However, sodium is an alkali metal with very characteristic metallic properties.

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