Atoms and Molecules
- History of the Atom
- Models for the Atom
- Subatomic Particles
- Periodic Table
- Periodic Trends
- Polyatomic Ions
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|Atoms and Molecules - Periodic Trends|
Electronegativity increases as you move across the periodic table from left to right. This occurs due to a greater charge on the nucleus, causing the electron bonding pairs to be very attracted to atoms placed further right on the periodic table. Fluorine is the most electronegative element. Electronegativity decreases as you move down the periodic table. This is caused by an increased amount of shielding, or screening, by the innermost electrons. As you move down the table more electrons are added between the nucleus and the bonding pair, causing the effective nuclear charge to be less. The increase in distance between the nucleus and the bonding pair decreases the attraction between the two.
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Electronegativity was originally proposed by Linus Carl Pauling. Pauling was born on February 28, 1901, in Lake Oswego, Oregon. Throughout his childhood he excelled academically. At the age of 15, he was only two credits short of graduating high school. When denied the opportunity to take these credits while enrolled in college, he decided to leave high school and obtain a job. He used his earnings from his early jobs to save money for college. Pauling was accepted to Oregon State University in September of 1917, where he received a degree in chemical engineering. During his undergraduate studies, Pauling taught courses in quantitative analysis and chemistry for home economics majors. After graduation from OSU, Pauling attended the California Institute of Technology and received his Ph. D. in physical chemistry and mathematical physics. In 1926, Pauling received the Guggenheim Fellowship, which allowed him to travel to Europe and study under Sommerfeld, Bohr, and Schrödinger. This led to his interest in the electronic structure of atoms and molecules. In 1932, Pauling introduced the concept of electronegativity. He introduced this concept based on the energy required to break bonds and dipole moments. He established the Pauling Electronegativity Scale, which is used to predict the nature of bonds between molecules and atoms. This scale gives values of electronegativity in Pauling Units.
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Electronegativity is how strongly electrons are pulled or attracted to one of the atoms in a covalent bond.
When two unlike atoms are covalently bonded, the shared electrons will be more strongly attracted to the atom of greater electronegativity.
The equation used in determining differences in Pauling electronegativity between atoms A and B.
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This video serves as a graphic representation of the trends in electronegativity as one moves down and across the periodic table.
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