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5 Written questions

5 Matching questions

  1. Electron Affinity
  2. Isoelectric
  3. Sextet Rule Elements
  4. Drawing Lewis Structures
  5. Ions
  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 Al, B
  3. c 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. 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. 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.
  2. 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.
  3. A model that is based on the natural repulsive forces that electron pairs exhibit within a molecule.
  4. An attractive force between ions of opposite charges, often a metal cation and a nonmetal anion.
  5. Hydrogen provides an exception to the octet rule because it requires only two electrons to attain a noble gas configuration.

5 True/False questions

  1. Nonpolar Covalent BondA bond in which the electrons are shared equally between two atoms.

          

  2. 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.

          

  3. 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.

          

  4. Electronegativity and PolarityThe greater the electronegativity difference between two atoms the more polar the bond.

          

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

          

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