7 Written questions
6 Multiple choice questions
- Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
- 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.
- Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
- density is usually between that of the component metals; alloy remains malleable and ductile
- formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms
6 True/False questions
Hardness of an ionic solid → Hard: ionic lattice is strong and rigid
Surface chemistry of an alloy → Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
Identification of an ionic solid → Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
Non-polar solubility of an ionic solid → Soluble: the charged ions interact with the dipoles on the water molecules.
Vapor pressure an of ionic solid → Hard: ionic lattice is strong and rigid
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.