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Periodic Trends - Coggle Diagram
Periodic Trends
Ionization Energy
Ionization Energy is merely the minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule.
Trend
Increase moving from left to right across an element period. (Atomic radius decreases and electrons are more attracted to Nucleus).
Conversely, as one progresses down a group on the periodic table, the ionization energy will likely decrease since the valence electrons are farther away from the nucleus and experience greater shielding.
The higher the Ionization Energy, the more difficult it is to remove an electron. Therefore, ionization energy is an indicator of reactivity.
Electron Affinity
Is the energy released when an electron is added to an atom.The change in energy
(in kJ/mole) of a neutral atom (in the gaseous phase) when an electron is added to the atom to form a negative ion. In other words, the neutral atom's likelihood of gaining an electron.
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Electronegativity
Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound
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