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5 Written questions

5 Matching questions

  1. EDG Tetrahedral
  2. 5 ED
  3. Lattice
  4. Duet Rule Elements
  5. Metallic Bond
  1. a Orbital Hybridization dsp3
  2. b Occurs when the nuclei of a collection of metal atoms simultaneously attract their collective electrons.
  3. c MG Tetrahedral
    MG Trigonal pyramidal
    MG Nonlinear
  4. d A stable, ordered, solid three-dimensional array of ions associated with ionic compounds.
  5. e H

5 Multiple choice questions

  1. 1.0-2.0
  2. 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.
  3. An attractive force between ions of opposite charges, often a metal cation and a nonmetal anion.
  4. 0-0.4
  5. A bond in which one atom attracts the pair of electrons more strongly than the other atom.

5 True/False questions

  1. Lattice EnergyA stable, ordered, solid three-dimensional array of ions associated with ionic compounds.

          

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

          

  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. Ionization Energy(∆ 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. Electronegativity and PolarityThe 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.