7 Written questions
6 Multiple choice questions
- Non-conductive (insulators): ions are pinned by the rigid lattice.
- 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.
- 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
- Metallic mixtures
- Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
6 True/False questions
Surface chemistry of an alloy → Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.
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.
Water solubility of an ionic solid → Soluble: the charged ions interact with the dipoles on the water molecules.
Brittleness of an ionic solid → Hard: ionic lattice is strong and rigid
Malleability and ductility of an ionic solid → Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
Substitutional Alloy (properties) → formed between atoms of comparable radius, where one atom substitutes for the other in the lattice