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7 Written questions

6 Multiple choice questions

  1. Very Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.
  2. Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
  3. 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
  4. Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
  5. Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
  6. Non-conductive (insulators): ions are pinned by the rigid lattice.

6 True/False questions

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


  2. Non-polar solubility of an ionic solidSoluble: the charged ions interact with the dipoles on the water molecules.


  3. Brittleness of an ionic solidHard: ionic lattice is strong and rigid


  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. Optical properties of metals (list and reason)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. Water 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.