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Chemical Bonding and Intermolecular Forces

Chemistry cards on ionic/covalent/metallic bonds, polarity, and IMFs for gen-chem exams.

12 cards· by GuruOwl

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  1. 01
    What is an ionic bond?
    Electrostatic attraction between cations and anions after electron transfer (often metal + nonmetal).
    bonding
  2. 02
    What is a covalent bond?
    Sharing of electron pairs between atoms (often nonmetals).
    bonding
  3. 03
    What makes a molecule polar?
    Polar bonds arranged so bond dipoles don’t cancel (asymmetric shape) → net dipole moment.
    polarity
  4. 04
    List intermolecular forces from generally weakest to strongest (typical exam order)?
    London dispersion < dipole–dipole < hydrogen bonding (stronger still: ion–dipole).
    imf
  5. 05
    What is hydrogen bonding (requirements)?
    H bonded to N, O, or F interacting with a lone pair on N/O/F of another molecule (or nearby group).
    imf
  6. 06
    Why does water have a high boiling point for its molar mass?
    Extensive hydrogen bonding between molecules.
    imf
  7. 07
    What are London dispersion forces?
    Temporary induced dipoles in all molecules; stronger with larger, more polarizable electron clouds.
    imf
  8. 08
    Metallic bonding description?
    Metal cations in a “sea” of delocalized valence electrons — explains conductivity and malleability.
    bonding
  9. 09
    What is electronegativity?
    An atom’s ability to attract shared electrons in a bond; large ΔEN → more ionic character.
    polarity
  10. 10
    VSEPR purpose in one line?
    Predict molecular geometry from electron domains around a central atom (minimize repulsion).
    geometry
  11. 11
    Bond angle in a tetrahedral molecule like CH₄?
    ≈ 109.5°.
    geometry
  12. 12
    Why is CO₂ nonpolar while H₂O is polar?
    CO₂ is linear — bond dipoles cancel. H₂O is bent — bond dipoles add to a net dipole.
    polarity