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7 Written Questions

6 Multiple Choice Questions

  1. Very Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.
  2. Insoluble: ionic compounds tend not to dissolve in nonpolar solvents because the attractions between ions are much more favorable than the attractions among the separated ions and nonpolar solvent molecules.
  3. Brittle: due to the repulsion of like charges caused when one layer slides across another layer.
  4. Hard: ionic lattice is strong and rigid
  5. Metallic mixtures
  6. Soluble: the charged ions interact with the dipoles on the water molecules.

6 True/False Questions

  1. Interstitial Alloy (definition)interstitial atoms do not appreciably expand the lattice and so density is often substantially increased; interstitial atoms make the lattice more rigid reducing ductility and malleability

          

  2. Optical properties of metal (explained)When light falls on a metal it is almost totally absorbed since the bonding electrons can jump up to a broad band of energy levels allowing energy changes corresponding to the full range of frequencies in the visible region of the spectrum.

    These currents immediately re-emit the light out of the metal thus providing a strong reflection if the metal surface is smooth.

          

  3. Conductivity of a metallic solidGood: electrons are delocalized and relatively free to move

          

  4. Interstitial Alloy (properties)formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms

          

  5. Malleability and ductility of an ionic solidMalleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core

          

  6. Conductivity of an ionic solidGood: electrons are delocalized and relatively free to move

          

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