1. Jason Qian Jaemo Lee John Seo
Electronegativity
Jason Qian
Jaemo Lee
John Seo

2. Definition
Electronegativity is a measure of the ability of an atom in a chemical compound to attract an electron from another atom in the compound.

3. Quick Facts
Electronegativity cannot be directly measured; it must be calculated from other atomic or molecular properties.
Most common scale of measurement for electronegativity is the Pauling scale.
The Pauling scale ranges from 0.7 to 4.0
Hydrogen is approximately 2.2 Pauling units

4. The Periodic Trends
In general, electronegativity increases from bottom to top in a column and left to right across a group.
So the most bottom left element, Cesium, is the least electronegative.
The most top right element, Fluorine, is the most electronegative.

5. The Shielding Effect Electronegativity depends on the Shielding Effect
As more energy levels are added, the electrons of that level are repelled by the electrons between the protons and the electrons of the highest energy level.
As you move towards the right of the periodic table, the number of protons increases while keeping the energy levels constant, so a larger attractive force reduces shielding
As you move down a group, more energy levels are added, thus strengthening the shielding effect, which decreases the attraction between the outer electrons and the nucleus

6. Exceptions
Does not include noble gases because they all have 8 valence electrons, causing them to be very stable. They are neither electronegative or electropositive.
Gallium and germanium have higher electronegativities than aluminum and silicon because of the missing d-block electrons.
Elements of the fourth period have very small atomic radii. This is because the electrons in the 3d orbital are not effective at “shielding” the increased positive charge. Smaller atomic size usually indicates a higher electronegativity.