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5 Written questions

5 Matching questions

  1. EDG Octahedral
  2. Drawing Lewis Structures
  3. VSEPR (Valence-shell electron-pari repulsion)
  4. Duet Rule Elements
  5. Very Polar Covalent
  1. a 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.
  2. b A model that is based on the natural repulsive forces that electron pairs exhibit within a molecule.
  3. c MG Octahedral
    MG Square pyramidal
    MG Square planar
  4. d 1.0-2.0
  5. e H

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. 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.
  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. Al, B
  5. Orbital Hybridization d2sp3

5 True/False questions

  1. Ions>2.0


  2. Nonpolar Covalent0-0.4


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


  4. Molecular GeometryThe arrangement of only the atoms in the molecule.


  5. IonicForm 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.


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