7 Written questions
6 Multiple choice questions
- Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
- formed between atoms of comparable radius, where one atom substitutes for the other in the 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.
- 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
- Brittle: due to the repulsion of like charges caused when one layer slides across another layer.
6 True/False questions
Vapor pressure an of ionic solid → Very Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.
Alloys → Metallic mixtures
Conductivity of alloys → Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
Substitutional Alloy (properties) → formed between atoms of comparable radius, where one atom substitutes for the other in the lattice
Malleability and ductility of a metallic solid → Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
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.