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electron affinity is the atoms affinity or how much an atom wants an electron and the energy it gives off when it obtains an electron. Ionization energy is the energy it takes to take away an electron from an atom. Usually, these trends follow a similar pathway on the periodic table as atoms who have a high electron affinity have a high ionization energy and vice versa.
We will not need to know how to calculate the exact values in ionization energy or electronegativity; however, we will need to know what they mean and their respective periodic trends. We'll also need to know how they apply to bonding (i.e. the atom with the highest electronegativity prefers a negative formal charge, and the atom with the lowest IE or highest electronegativity is usually the central atom in a Lewis diagram).
Ionization energy is the energy required to remove an electron from an ion or gaseous atom, whereas electron affinity is the amount of energy released when an electron is added to an atom to form an anion. Both periodic trends, however, are the same.
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