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Concepts of Chemical Bonding Test

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5 Written Questions

5 Matching Questions

  1. EDG Tetrahedral
  2. Sextet Rule Elements
  3. EDG Octahedral
  4. Metallic Bond
  5. Drawing Lewis Structures
  1. a MG Octahedral
    MG Square pyramidal
    MG Square planar
  2. b Occurs when the nuclei of a collection of metal atoms simultaneously attract their collective electrons.
  3. c 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.
  4. d Al, B
  5. e MG Tetrahedral
    MG Trigonal pyramidal
    MG Nonlinear

5 Multiple Choice Questions

  1. 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.
  2. The energy required to remove an electron from an atom or ion in the gaseous state. Increases from left to right and from bottom to top on the Periodic Table.
  3. Form when electrons transfer from an atom of low ionization energy (usually a metal) to an atom of high electron affinity (usually a nonmetal). The electrostatic attraction between two oppositely charged ions constitutes this bond.
  4. A bond in which the electrons are shared equally between two atoms.
  5. H

5 True/False Questions

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

          

  2. LatticeA stable, ordered, solid three-dimensional array of ions associated with ionic compounds.

          

  3. 4 EDOrbital Hybridization dsp3

          

  4. EDG LinearMG Linear

          

  5. Electron DomainThe 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.

          

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