7 Written questions
6 Multiple choice questions
- Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
- density is usually between that of the component metals; alloy remains malleable and ductile
- Soluble: the charged ions interact with the dipoles on the water molecules.
- formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms
- 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.
6 True/False questions
Conductivity of a metallic solid → Non-conductive (insulators): ions are pinned by the rigid lattice.
Hardness of an ionic solid → Hard: ionic lattice is strong and rigid
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.
Malleability and ductility of an ionic solid → Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
Interstitial Alloy (properties) → formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms