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Nicole Garrido 2I
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Postby Nicole Garrido 2I » Sun Nov 11, 2018 7:10 pm

How does electronegativity affect the radius of an atom? The process not just the trend.

Blake Salfer 1B
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Joined: Thu Sep 27, 2018 11:18 pm

Re: Radius

Postby Blake Salfer 1B » Sun Nov 11, 2018 7:17 pm

as atomic radius increases electronegativity decreases because there is less attraction between the nucleus and shared electrons as atomic radius increases

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Re: Radius

Postby becca_vandyke_4b » Sun Nov 11, 2018 7:25 pm

In terms of coulombs law, as the radius increases, the attraction between the negative electrons and the positive protons inside the nucleus decreases. Therefore, the electrons are more easily removed from the atom. In an element like F, the atomic radius is smaller because the zeff is higher for this element. Therefore the atom is more likely to gain electrons than lose them.

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Re: Radius

Postby 705170809 » Sun Nov 11, 2018 8:32 pm

Electronegativity is the attractive force between the protons and the electrons. As the atomic radius increases, the protons in the nucleus have a less attractive force to the electrons which is why the electrons are further from the nucleus, expanding the atom, and thus electronegativity decreases. This is why electronegativity and atomic radius have opposite periodic trends.

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Re: Radius

Postby yuetao4k » Sun Nov 25, 2018 9:59 pm

As electronegativity increases, the pull on the electrons is greater. This means that the electrons are closer to the nucleus, thus giving the molecule a smaller atomic radius.

Liset Rivera 3A
Posts: 31
Joined: Thu Sep 27, 2018 11:23 pm

Re: Radius

Postby Liset Rivera 3A » Sun Nov 25, 2018 10:10 pm

The higher the electronegativity, the smaller the atomic radius. This is due to the electrons being closer to the nucleus, thus causing the atomic radius to be higher.

Ahmed Mahmood 4D
Posts: 50
Joined: Thu Sep 27, 2018 11:28 pm

Re: Radius

Postby Ahmed Mahmood 4D » Fri Dec 07, 2018 10:05 pm

As you move down a column, more energy levels are added to an atom, causing increased distance between the nucleus and valence electrons. Due to electron shielding (the interference of inner energy shells in the interactions between outer energy shells and the nucleus), electronegativity decreases as the attraction between the nucleus and outer electrons is lowered. Across a row, the atom is more prone to accepting electrons due to the fact that it gets closer and closer to filling its valence shell, causing electronegativity to increase. This relates to radius because, as you move down a column, additional energy shells cause greater radius, while moving across a row causes a tighter pull on the valence shell from the nucleus and thus a smaller nucleus.

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