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7 Written questions

6 Multiple choice questions

  1. Good: electrons are delocalized and relatively free to move
  2. Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.
  3. Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
  4. Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
  5. Metallic mixtures
  6. Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)

6 True/False questions

  1. 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.

          

  2. Non-polar solubility of an ionic solidInsoluble: 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.

          

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

          

  4. Substitutional Alloy (properties)density is usually between that of the component metals; alloy remains malleable and ductile

          

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

          

  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.