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7 Written questions

6 Multiple choice questions

  1. Soluble: the charged ions interact with the dipoles on the water molecules.
  2. Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
  3. Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
  4. Good: electrons are delocalized and relatively free to move
  5. 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. 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. Optical properties of metal (explained)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.

          

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

          

  3. Vapor pressure an of ionic solidVery Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.

          

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

          

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

          

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

          

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