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Polar Covalent Bonds

This guide explores polar and nonpolar covalent bonds, highlighting how electronegativity differences between atoms result in charge imbalances, leading to the formation of polar covalent bonds. Key terms like delta (δ) notation for partial charges, the characteristics of diatomic molecules, and the influence of molecular geometry on overall polarity are outlined. Additionally, guidelines to determine whether a molecule is polar, nonpolar, or ionic based on electronegativity values are provided, alongside practical exercises for applying these concepts.

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Polar Covalent Bonds

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  1. Polar Covalent Bonds

  2. In some covalent bonds, one of the two atoms holds electrons more tightly ⇒ polar covalent bond results between two atoms

  3. Delta (δ) Notation for polar bonds • Electrons concentrate around the more EN atom in a molecule ⇒ Atom gains a partial negative charge, indicated with δ– • Since electrons spend less time around the other atom ⇒ Other atom gains a partial positive charge, indicated with δ+

  4. For you to try… • For each of the bonds to the right: • i. Use delta notation (δ+ and δ–) to indicate which atom in each bond is more electronegative, and • ii. Use an arrow to point from the less electronegative atom to the more electronegative atom.

  5. POLARITY OF MOLECULES • For diatomic molecules: • – nonpolar molecules: when the 2 atoms have equal EN values • – polar molecules: when the 2 atoms have different EN values – have dipole (+ and – ends)

  6. For molecules of three or more atoms • – polarity depend on the individual bonds and geometry around central atom • – Polar molecules have an overall dipole (positive end and negative end) • – In nonpolar molecules, there may be individual dipoles that cancel → no overall dipole

  7. Guidelines for Determining if a Molecule is Polar or Nonpolar or Ionic • Use the electronegativity (EN) chart and compare the change in EN. • 0-.4 nonpolar covalent • .4 -1.7 polar covalent • Above 1.7 ionic

  8. You try it… • Draw the covalent molecules on the right. Label the following: • δ– and δ+ • Arrows toward δ– • Change in EN • Nonpolar covalent, polar covalent, or ionic

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