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7 Written questions

6 Multiple choice questions

  1. Good: electrons are delocalized and relatively free to move
  2. Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
  3. Brittle: due to the repulsion of like charges caused when one layer slides across another layer.
  4. formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms
  5. 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.
  6. 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.

6 True/False questions

  1. Identification of an ionic solidNon-conductive (insulators): ions are pinned by the rigid lattice.

          

  2. Hardness of an ionic solidBrittle: due to the repulsion of like charges caused when one layer slides across another layer.

          

  3. Optical properties of metals (list and reason)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.

          

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

          

  5. Surface chemistry of an alloyAlloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.

          

  6. Conductivity of alloysGood: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)

          

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