7 Written questions
6 Multiple choice questions
- Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
- 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.
- Non-conductive (insulators): ions are pinned by the rigid lattice.
- density is usually between that of the component metals; alloy remains malleable and ductile
- Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
- formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms
6 True/False questions
Non-polar solubility of an ionic solid → Soluble: the charged ions interact with the dipoles on the water molecules.
Water 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.
Surface chemistry of an alloy → Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.
Malleability and ductility of a metallic solid → Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
Alloys → Metallic mixtures
Substitutional Alloy (definition) → density is usually between that of the component metals; alloy remains malleable and ductile