7 Written questions
6 Multiple choice questions
- Unable to conduct electricity as a solid; soluble in water; aqueous solution conducts electricity
- Very Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.
- Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
- Poor: ionic lattices are rigid and once broken tend to cleave along an entire plane.
- Metallic mixtures
- Alloy formation sometimes alters the chemistry such as the formation of a chemically inert oxide layer in stainless steel.
6 True/False questions
Optical properties of metal (explained) → 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.
Water solubility of an ionic solid → Soluble: the charged ions interact with the dipoles on the water molecules.
Brittleness of an ionic solid → Brittle: due to the repulsion of like charges caused when one layer slides across another layer.
Substitutional Alloy (definition) → density is usually between that of the component metals; alloy remains malleable and ductile
Conductivity of alloys → Good: alloys usually retain a sea of mobile electrons (delocalized covalent bonds) and so remain conducting (for both HEAT and ELECTRICITY)
Interstitial Alloy (definition) → interstitial atoms do not appreciably expand the lattice and so density is often substantially increased; interstitial atoms make the lattice more rigid reducing ductility and malleability