7 Written questions
6 Multiple choice questions
- Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
- Non-conductive (insulators): ions are pinned by the rigid lattice.
- 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.
- 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.
- 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
- Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.
6 True/False questions
Substitutional Alloy (properties) → formed between atoms of comparable radius, where one atom substitutes for the other in the lattice
Conductivity of a metallic solid → Non-conductive (insulators): ions are pinned by the rigid lattice.
Non-polar solubility of an ionic solid → 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.
Conductivity of alloys → Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
Vapor pressure an of ionic solid → Hard: ionic lattice is strong and rigid
Alloys → Metallic mixtures