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5 Written questions

5 Matching questions

  1. Isoelectric
  2. Electron Affinity
  3. Electron Domain
  4. Drawing Lewis Structures
  5. Lewis Structure
  1. a 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.
  2. b 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.
  3. c 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.
  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 When an atom gains or loses electrons to attain an octet of valence electrons, it does not become a noble gas. Chloride ion, Cl-, has the same electron configuration as argon, but it is not argon. Chloride ion has the same number of electrons (term) with argon but chloride has one fewer proton.

5 Multiple choice questions

  1. 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.
  2. Orbital Hybridization sp2
  3. A quantitative measure of the magnitude of a dipole. The higher the dipole moment, the more polar is the molecule.
  4. (∆ H lattice) is the energy required to completely separate a mole of a solid ionic compound into its gaseous ions. Ionic compounds tend to have high lattice energies, which tend to make ionic compounds hard and brittle with relatively high melting points.
  5. A bond in which one atom attracts the pair of electrons more strongly than the other atom.

5 True/False questions

  1. Electron Domain GeometryThe arrangement of electron domains around the central atom of a molecule.


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


  3. IonsForm 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. 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.


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