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5 Written questions

5 Matching questions

  1. 4 ED
  2. Dipole Moment
  3. VSEPR (Valence-shell electron-pari repulsion)
  4. Dipole
  5. EDG Linear
  1. a Orbital Hybridization sp3
  2. b A model that is based on the natural repulsive forces that electron pairs exhibit within a molecule.
  3. c MG Linear
  4. d A 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.
  5. e A quantitative measure of the magnitude of a dipole. The higher the dipole moment, the more polar is the molecule.

5 Multiple choice questions

  1. Orbital Hybridization d2sp3
  2. Two or more Lewis structures that are equally good representations of the bonding in a molecule or ion. Usually differ only in the positions of multiple bonds or single, unpaired electrons.
  3. P, S, Cl, Br, I
  4. The energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
  5. The relative ability of an atom to attract a pair of electrons. Increases from left to right and from bottom to top. Fluorine has the highest and francium has the lowest. gas>liquid>solid Determines polarity.

5 True/False questions

  1. Nonpolar Covalent0.4-1.0

          

  2. EDG TetrahedralMG Octahedral
    MG Square pyramidal
    MG Square planar

          

  3. Metallic BondResults from sharing electrons between two atoms, usually nonmetal atoms.

          

  4. Lattice EnergyA stable, ordered, solid three-dimensional array of ions associated with ionic compounds.

          

  5. 3 EDOrbital Hybridization sp3