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7 Written questions

6 Multiple choice questions

  1. Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
  2. Very Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.
  3. Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
  4. Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
  5. Metallic mixtures
  6. Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.

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. Water solubility of an ionic solidSoluble: the charged ions interact with the dipoles on the water molecules.

          

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

          

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

          

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

          

  6. Interstitial Alloy (definition)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