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7 Written questions

6 Multiple choice questions

  1. Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
  2. density is usually between that of the component metals; alloy remains malleable and ductile
  3. Soluble: the charged ions interact with the dipoles on the water molecules.
  4. formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms
  5. Non-conductive (insulators): ions are pinned by the rigid lattice.
  6. 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 True/False questions

  1. Conductivity of a metallic solidNon-conductive (insulators): ions are pinned by the rigid lattice.

          

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

          

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

          

  4. 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.

          

  5. Malleability and ductility of an ionic solidPoor: ionic lattices are rigid and once broken tend to cleave along an entire plane.

          

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