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Ever heard of Electronegativity?
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- Trend Across a Period
- As you go across a period, electronegativity increases. For example, Oxygen has an electronegativity of 3.44. Nitrogen, which is to the left, has an electronegativity of 3.04. Fluorine, which is to the right, has an electronegativity of 3.98.
- Trend Down a Group
- As you go down a group, electronegativity decreases. For example, Sulfur has an electronegativity of 2.58. Oxygen, which is above Sulfur, has an electronegativity 3.44. Selenium, which is below Sulfur, has an electronegativity of 2.5
- How the Shielding Effect affects Electronegativity
- The more shielding an atom has, the lower the electronegativity. Let's use Fluorine as an example. It has the highest electronegativity at 4.0. This is because its nucleus has a very powerful effective nuclear charge force towards its electrons. Since all of the electrons are pulled very close to the nucleus, there is very little shielding. Francium, which is at the bottom of the periodic table, has much more shielding, however, because of all the energy levels it contains.
- Connection Between the Coulombic Attraction and Electronegativity
- Coulombic Attraction and Electronegativity. There is a connection, so I will explain it. As the atomic number increases, the nuclear attraction for electrons will also increase. This pulls the electrons closer to the nucleus. The Coulombic attraction of the nucleus of an atom for its electrons is referred to as the electronegativity.
- Why is this the Trend? (Period)
- As you go across a period, electronegativity increases. The reason behind this is simple. As more protons are added, there is more pull from the protons in the nucleus. Since no more energy levels are added, this allows for the nucleus to attract a stronger bond to the electrons, thus increasing electronegativity.
- Why is this the Trend? (Group)
- As you go down a group, electronegativity decreases. There's a simple reason behind this. As you move down a group, the atom gets larger. Because of this, more energy shells are added. As a result. the attractive force of the nucleus will get weaker the further an electron is from the nucleus. It's like a fireplace. The closer I am, the warmer I am. But the further away I get, the colder I become.
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