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Chemical Bonding

85 cards · 🇺🇸 English

Ionic, covalent, metallic bonds and intermolecular forces.

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Chemical bond

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  1. 1Chemical bond
    The association of atoms or ions to form molecules, crystals, and other structures through electrostatic forces or electron sharing
  2. 2Three types of 'strong bonds' or 'primary bonds'
    Covalent, ionic, and metallic bonds
  3. 3Examples of 'weak bonds' or 'secondary bonds'
    Dipole-dipole interactions, London dispersion force, and hydrogen bonding
  4. 4Why do chemical bonds form?
    Electrons shared between two nuclei are attracted to both; constructive quantum mechanical wavefunction interference stabilizes the paired nuclei
  5. 5Bond distance
    The optimal distance bonded nuclei maintain, balancing attractive and repulsive effects explained by quantum theory
  6. 6What theories allow chemists to predict bond properties?
    Simplified rules like the octet rule and VSEPR theory, plus more sophisticated theories like valence bond and molecular orbital theory
  7. 7Octet rule
    A simplified rule used to predict chemical bonding behavior (atoms tend to combine to achieve eight valence electrons)
  8. 8VSEPR theory
    Valence Shell Electron Pair Repulsion theory, used to predict molecular geometry
  9. 9Valence bond theory
    A theory that includes orbital hybridization and resonance to explain chemical bonding
  10. 10Molecular orbital theory
    A theory that includes linear combination of atomic orbitals and ligand field theory to explain bonding
  11. 11In a covalent bond, where are electrons drawn?
    Into the space between the two atomic nuclei
  12. 12Why does bond formation release energy?
    The reduction in kinetic energy as electrons occupy a more spatially distributed orbital (longer de Broglie wavelength) compared to being confined closer to their respective nuclei
  13. 13Polar covalent bond
    A covalent bond where one or more electrons are unequally shared between two nuclei
  14. 14What happens to molecules with weak intermolecular bonds?
    They have soft bulk character and low melting points, as in waxes and oils
  15. 15What happens when covalent bonds extend in networks?
    The structures may be both strong and tough (e.g., diamond, quartz, silicate minerals), with greatly increased melting points
  16. 16In an ionic bond, what happens to the bonding electron?
    It is not shared at all, but transferred from one atom to another
  17. 17Why are ionic bonds formed?
    One nucleus offers a more tightly bound position to an electron, causing an electron to transfer and creating oppositely charged ions that attract electrostatically
  18. 18Characteristic of ionic bond orientation
    Often no particular orientation in space, since they result from equal electrostatic attraction of each ion to all ions around them
  19. 19Why are ionic substances brittle?
    Forces between ions are short-range and do not easily bridge cracks and fractures
  20. 20Metallic bonding
    Bonding where each atom donates one or more electrons to a 'sea' of electrons that reside between many metal atoms
  21. 21Why are metals malleable?
    Metallic bonding is more collective in nature, allowing atoms to be attracted to each other without particularly-oriented bonds, enabling easier deformation
  22. 22What causes good electrical and thermal conductivity in metals?
    The cloud of electrons in metallic bonding, which also causes their shiny lustre
  23. 23What did Lavoisier prove about water?
    That water can be decomposed into hydrogen and oxygen, which cannot be decomposed further, thereby proving they are elements
  24. 24Law of conservation of mass
    In a chemical reaction, matter does not appear or disappear; the total mass remains the same even if substances are transformed
  25. 25Law of definite proportions
    If a compound is broken down, the masses of constituent elements always have the same proportions by weight, regardless of quantity or source
  26. 26Valency originally called
    'Combining power', describing how compounds were joined owing to attraction of positive and negative poles
  27. 27Abegg's rule
    Proposed in 1904 by Richard Abegg: the difference between the maximum and minimum valencies of an element is often eight
  28. 28Planetary model of the atom
    Proposed by Hantaro Nagaoka in 1904: a positively charged center surrounded by revolving electrons, like Saturn and its rings
  29. 29What did Max Planck say about energy regulation between atoms?
    At the 1911 Solvay Conference: 'The intermediaries could be the electrons.'
  30. 30Lewis structure
    A diagram showing electrons shared between atoms in chemical bonds, developed by Gilbert N. Lewis in 1916

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