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7 Written questions

6 Multiple choice questions

  1. Good: electrons are delocalized and relatively free to move
  2. Soluble: the charged ions interact with the dipoles on the water molecules.
  3. 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.
  4. Hard: ionic lattice is strong and rigid
  5. Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
  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. Substitutional Alloy (definition)density is usually between that of the component metals; alloy remains malleable and ductile

          

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

          

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

          

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

          

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

          

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