Polar Bonds: Covalent bonds with unequal sharing of electrons due to significant differences in electronegativity (>0.4).
Non-Polar Bonds: Covalent bonds with equal sharing of electrons, either due to equal electronegativity or minimal differences (<0.4).
Electronegativity: A measure of an atom's ability to attract and bond with electrons. Increases across periods and up groups on the periodic table. Measured using the Pauling scale.
Dipole Moment: Occurs when there is a separation of charges within a molecule, resulting in partially positive and negative ends.
Bonds
Polar Bonds
Caused by significant electronegativity differences.
Example: Water (H2O) with an electronegativity difference of 1.4 between hydrogen and oxygen.
Non-Polar Bonds
Characterized by equal sharing of electrons.
Example: Chlorine (Cl2) with no electronegativity difference.
Molecules
Polar Molecules
Molecules with an uneven distribution of charge, leading to partially positive and negative ends.
Asymmetrical, causing a dipole.
Polar molecules dissolve in polar solvents.
Examples: HF, water, acetone, sulfur dioxide.
Nonpolar Molecules
Symmetrical molecules with evenly distributed charges.
Do not form positive or negative poles.
Nonpolar molecules dissolve in nonpolar solvents.
Examples: Carbon dioxide, benzene, methane.
Examples
Polar Molecules
HF: Polar due to large electronegativity difference.
Water: Bent shape causes asymmetry.
Acetone: Somewhat polar due to its carbonyl group.
Nonpolar Molecules
Carbon Dioxide (CO2): Linear symmetry cancels out polar bonds.
Benzene (C6H6): Symmetrical molecule.
Additional Resources
Explore more on ionic vs covalent bonds, molecule vs compound, acid-base chemistry, and polar-covalent bonds.
Check out the interactive periodic table for more element properties and trends.
Fun Chemistry Video
An unrelated but entertaining chemistry experiments video is available on the channel mentioned in the article.