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Postby WYacob_2C » Fri Oct 25, 2019 11:06 pm

Can someone explain electronegativity and its relationship to ionization energy, if there is one.

Hannah Lee 2F
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Re: Electronegativity

Postby Hannah Lee 2F » Fri Oct 25, 2019 11:21 pm

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-.

Karina Kong 2H
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Re: Electronegativity

Postby Karina Kong 2H » Sat Oct 26, 2019 12:36 pm

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.

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Re: Electronegativity

Postby 805373590 » Sat Oct 26, 2019 12:53 pm

Electronegativity: tendency of an atom to attract an electron
Ionization energy: required energy to remove an electron from an atom

Rhea Shah 2F
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Re: Electronegativity

Postby Rhea Shah 2F » Sat Oct 26, 2019 5:14 pm

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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