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5 Written questions

5 Matching questions

  1. Very Polar Covalent
  2. Molecular Geometry
  3. Lewis Structure
  4. Drawing Lewis Structures
  5. EDG Octahedral
  1. a 1.0-2.0
  2. b MG Octahedral
    MG Square pyramidal
    MG Square planar
  3. c Shows the valence electrons as dots around the symbol for the element. The number of valence electrons for a representative element is the same as its group number on the periodic table.
  4. d 1) Total the valence electrons of all bonded atoms. (- means you add electrons, + means you subtract electrons)
    2) Use one pair of electrons to bond each outer atom to the central atom.
    3) Complete the octets around all of the outer atoms.
    4) Place any remaining electrons on the central atom.
    5) If there are not enough electrons to give the central atom an octet, make multiple bonds.
  5. e The arrangement of only the atoms in the molecule.

5 Multiple choice questions

  1. Orbital Hybridization dsp3
  2. MG Trigonal Bipyramidal
    MG Seesaw
    MG T-Shaped
    MG Linear
  3. Results from sharing electrons between two atoms, usually nonmetal atoms.
  4. MG Linear
  5. Orbital Hybridization sp

5 True/False questions

  1. DipoleA molecule with one end having a slight positive charge and the other end having a slight negative charge due to differences in electronegativity. Arrow points towards the more electronegative element.

          

  2. More than Octet RuleStates that representative elements tend to gain, lose, or share electrons until they are surrounded by eight valence electrons (an octet).

          

  3. Dipole MomentA quantitative measure of the magnitude of a dipole. The higher the dipole moment, the more polar is the molecule.

          

  4. Octet RuleHydrogen provides an exception to the octet rule because it requires only two electrons to attain a noble gas configuration.

          

  5. Nonpolar Covalent BondA bond in which one atom attracts the pair of electrons more strongly than the other atom.