Molecular Geometry

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Author:
Gymnastxoxo17
ID:
234007
Filename:
Molecular Geometry
Updated:
2014-03-23 21:19:11
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Folders:
AP Chem
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d
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  1. 2 bonding domains, 0 non-bonding domains
    linear
  2. 3 bonding domains, 0 non-bonding domains
    trigonal planar
  3. 2 bonding domains, 1 non-bonding domain
    bent
  4. 4 bonding domains, 0 non-bonding domains
    tetrahedral
  5. 3 bonding domains, 1 non-bonding domain
    trigonal pyramidal
  6. 2 bonding domains, 2 non-bonding domains
    bent
  7. 5 bonding domains, 0 non-bonding domains
    trigonal bipyramidal
  8. 4 bonding domains, 1 non-bonding domain
    seesaw
  9. 3 bonding domains, 2 non-bonding domains
    t-shaped
  10. 2 bonding domains, 3 non-bonding domains
    linear
  11. 6 bonding domains, 0 non-bonding domains
    octahedral
  12. 5 bonding domains, 1 non-bonding domain
    square pyramidal
  13. 4 bonding domains, 2 non-bonding domains
    square planar
  14. intramolecular bonds
    bonds between atoms, within molecules
  15. covalent bonds
    shared electrons
  16. non-polar covalent bonds
    electronegativity difference equals zero
  17. polar covalent bonds
    unequal sharing of electrons between atoms, electronegativity difference is .1 to 1.7
  18. ionic bonds
    losing or gaining of electrons, electronegativity difference is greater than 1.7
  19. things that would make a molecule polar
    • surrounded by different elements
    • non-bonding domains
  20. how to determine the central atom in lewis structure
    • element that has only one atom
    • atom with the most valence openings
  21. electronegativity trends
    • increase in atomic number, increase in number of protons, nucleus size increases and becomes stronger, stronger attraction for electrons
    • elements with electrons close to nucleus experience less shielding and the effective nuclear charge is greater
  22. hybridization
    blended orbitals
  23. deficient
    does not require octet, stable because all available electrons are shared (e.g. B or Be)
  24. single bonds
    sigma (include one of the bonds in a double bond)
  25. double bonds
    pi (in a double bond, one is sigma and one is pi)
  26. formal charge (formula and use)
    • Cf= x - (y + z/2)
    • x=number of valence electrons in free atom; y=number of unshared electrons of atom in lewis structure; z=number of bonding electrons of atom in lewis structure
    • more likely lewis structure will have a formal charge closer to zero
  27. molecules are deficient when
    they have an odd number of total valence electrons

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