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7 Written questions

6 Multiple choice questions

  1. Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
  2. Soluble: the charged ions interact with the dipoles on the water molecules.
  3. Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.
  4. 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.
  5. Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
  6. 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.

6 True/False questions

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


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


  3. AlloysMetallic mixtures


  4. Substitutional Alloy (definition)formed between atoms of comparable radius, where one atom substitutes for the other in the lattice


  5. 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.


  6. Interstitial Alloy (properties)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