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Electronegativity refers to the tendency of an atom to attract e-, while ionization energy refers to the amount of energy it takes to remove an e- in the gas phase. Both follow similar trends in the periodic table, increasing from left to right across a period as effective nuclear charge increases and decreasing from top to bottom down a period as the distance between e- and the nucleus increases. However, there are important exceptions (like oxygen, which has a lower ionization energy than nitrogen despite having a higher electronegativity). Generally, elements with low ionization energies tend to also have less electronegativity. This makes sense because lower ionization energies indicate a greater tendency to donate e- (since it takes less energy to remove one), so elements with low IE would be less likely to accept/attract e-.
The trends for both electronegativity and ionization energy are the same. Electronegativity is the the tendency for an atom to attract an electron. With a higher electronegativity, there is usually a higher ionization energy.
Electronegativity is the tendency for an atom to attract an electron in a shared bond, while the ionization energy is the energy needed to remove an electron from an atom in its gas phase. The trends for both are the same on the periodic table, increasing the further one goes to the right and upwards. Fluorine is the most electronegative element because it only needs one more electron for ideal electron configuration, which is why it holds its electrons to tightly to the nucleus. This trend occurs for ionization energy because the tighter electrons are held to the nucleus, the more energy is needed to remove them, which is also why the ionization energy for fluorine is so high.
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