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GOB Chemistry: Electronegativity, Bond Polarity, Molecular Polarity & Intermolecular Forces

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Termini in questo insieme (20)

  • What is electronegativity?

    Electronegativity is the ability of an atom to attract and share electron pairs in a chemical bond.

  • How does electronegativity trend across the periodic table?

    Electronegativity increases from left to right across a period and from bottom to top in a group.

  • What is the electronegativity of fluorine and why is it significant?

    Fluorine has the highest electronegativity value of \(4.0\), making it the strongest atom at attracting electrons.

  • Define nonpolar covalent bond.

    Atoms share electrons equally with a ΔEN between 0 and 0.4, e.g., Cl–Cl or C–H bonds.

  • Define polar covalent bond.

    Electrons are shared unequally due to a ΔEN between 0.5 and 1.8, causing partial charges (δ+ and δ−) on atoms.

  • Define ionic bond.

    Electrons are essentially transferred between atoms with a ΔEN greater than 1.8, forming ions.

  • How to determine bond polarity using electronegativity?

    Calculate ΔEN by subtracting smaller EN from larger EN; classify bond type based on ΔEN ranges.

  • What determines molecular polarity?

    Molecular polarity depends on bond polarity and molecular shape; dipoles must not cancel for molecule to be polar.

  • What is the molecular shape and polarity of CO2?

    CO2 is linear with polar bonds, but dipoles cancel, making it a nonpolar molecule.

  • What is the molecular shape and polarity of H2O?

    H2O is bent with polar O–H bonds; dipoles do not cancel, so it is polar.

  • What are hydrogen bonds?

    Strong dipole–dipole attractions between H bonded to N, O, or F and lone pairs on N, O, or F of another molecule.

  • Why does water have a high boiling point compared to H2S?

    Water forms hydrogen bonds requiring more energy to break, while H2S lacks hydrogen bonding.

  • List the intermolecular forces from strongest to weakest.

    Ionic bonds > Hydrogen bonds > Dipole–dipole attractions > Dispersion forces.

  • What type of intermolecular force exists in nonpolar molecules?

    Dispersion forces, caused by temporary induced dipoles, are the only forces in nonpolar molecules.

  • Explain 'like dissolves like' in terms of polarity.

    Polar and ionic substances dissolve in polar solvents; nonpolar substances dissolve in nonpolar solvents.

  • How do lone pairs affect molecular polarity?

    Lone pairs can create asymmetry in shape, preventing dipole cancellation and making molecules polar.

  • What is the role of electronegativity in bond polarity?

    Electronegativity differences cause unequal sharing of electrons, creating bond dipoles.

  • How to identify the polarity of a molecule with multiple bonds?

    Draw Lewis structure, determine shape, check bond polarities, and see if dipoles cancel or add up.

  • What is the strongest intermolecular force in ionic compounds?

    Strong ionic bonds between oppositely charged ions in a crystal lattice.

  • Why can methane (CH4) not form hydrogen bonds?

    Hydrogen in CH4 is bonded to carbon, not N, O, or F, so no hydrogen bonding occurs.