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7 Written questions

6 Multiple choice questions

  1. Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
  2. Non-conductive (insulators): ions are pinned by the rigid lattice.
  3. 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. Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
  5. density is usually between that of the component metals; alloy remains malleable and ductile
  6. formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms

6 True/False questions

  1. Hardness of an ionic solidHard: ionic lattice is strong and rigid


  2. Surface chemistry of an alloyGood: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)


  3. Identification of an ionic solidUnable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity


  4. Non-polar solubility of an ionic solidSoluble: the charged ions interact with the dipoles on the water molecules.


  5. Vapor pressure an of ionic solidHard: ionic lattice is strong and rigid


  6. Optical properties of metals (list and reason)Shiny, reflective, lustrous: because electrons move freely throughout the metal. Metals are shiny because of the very strong absorption of light by the delocalised bonding electrons.


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