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5 Written Questions

5 Matching Questions

  1. Sextet Rule Elements
  2. Electronegativity
  3. Metallic Bond
  4. 5 ED
  5. Lewis Structure
  1. a Orbital Hybridization dsp3
  2. b Al, B
  3. c For covalent molecules often show shared pairs of electrons (bonding pairs) as lines and unshared electron pairs (nonbonding pairs) as lines or dots.
  4. d 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. e Occurs when the nuclei of a collection of metal atoms simultaneously attract their collective electrons.

5 Multiple Choice Questions

  1. A quantitative measure of the magnitude of a dipole. The higher the dipole moment, the more polar is the molecule.
  2. A stable, ordered, solid three-dimensional array of ions associated with ionic compounds.
  3. 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.
  4. Results from sharing electrons between two atoms, usually nonmetal atoms.
  5. Orbital Hybridization d2sp3

5 True/False Questions

  1. 2 EDOrbital Hybridization sp3


  2. Lewis StructureTwo 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. Ions>2.0


  4. Molecular GeometryRefers to the arrangement of a molecule's atoms in three-dimensional space.


  5. VSEPR (Valence-shell electron-pari repulsion)A region around an atom in which electrons will most likely be found. Produced by a nonbonding pair, a single bond, a double bond, or a triple bond.


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