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Electronegativity, Polarity & Intermolecular Forces in Chemistry

Learn about electronegativity and polarity, types of covalent bonds, intermolecular forces, and solubility of polar molecules. Explore the concepts with examples and understand the impact on molecular properties.

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Electronegativity, Polarity & Intermolecular Forces in Chemistry

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  1. Electronegativity and Polarity

  2. Elecronegativity • Relative ability of an atom to attract electrons in a chemical bond • Fluorine has the highest electronegativity value • Trend: • Increases across (left to right) a period • Decreases down a group

  3. Types of covalent bonds • Non-polar covalent: equal sharing of electrons • Polar covalent: unequal sharing of electrons

  4. Non-polar covalent • Sharing of electrons equally • Usually occurs when two identical atoms are bonded together. • Examples: H2, O2, N2, Cl2, Br2, I2, F2

  5. Polar covalent • Unequal sharing of electrons • Unequal sharing caused by 2 elements with different electronegativities (different abilities to attract electrons). • The bond is called a dipole (two poles) • Creates molecule with partial charges

  6. Partial charges symbolized by (delta) + and - • The more electronegative atom is located at the partially negative end • Example: + - H-Cl and H-Cl

  7. Polar molecule or not? • The shape of a molecule usually tells if a molecule is polar or not • If the VSEPR shape is symmetric it is usually non-polar • If the molecule is asymmetric it is polar

  8. Youtube polar vs nonpolar

  9. Intermolecular Forces • The force that exists between separate molecules. • This force attracts molecules to each other.

  10. 3 Types • London Dispersion force or induced dipole moment between molecules; only force in non-polar molecules; weakest force (caused by the motion of electrons) (ex: CH4) Induced dipole moment

  11. Dipole-dipole the force between two polar molecules; stronger force (ex: HCl)

  12. Hydrogen bond forms between the hydrogen end of one dipole and fluorine, oxygen, or nitrogen (that have at least one lone pair) end of another dipole; strongest force (ex: H2O) Hydrogen bond

  13. IMF’s • ALL molecules have dispersion forces • All polar molecules have dipole-dipole forces and dispersion forces • Molecules that hydrogen bond have all 3

  14. Solubility of polar molecules • Properties are due to intermolecular forces • Like dissolves like • Polar substances will dissolve polar molecules (and ionic compounds) • Non-polar substances will dissolve non-polar molecules

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