7 Written Questions
6 Multiple Choice Questions
- Very Low: due to the strong Coulombic interactions of positive and negative ions arranged in a regular three-dimensional array.
- 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.
- Brittle: due to the repulsion of like charges caused when one layer slides across another layer.
- Hard: ionic lattice is strong and rigid
- Metallic mixtures
- Soluble: the charged ions interact with the dipoles on the water molecules.
6 True/False Questions
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
Optical properties of metal (explained) → 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.
Conductivity of a metallic solid → Good: electrons are delocalized and relatively free to move
Interstitial Alloy (properties) → formed between atoms of different radius, where the smaller atoms fill the interstitial spaces between the larger atoms
Malleability and ductility of an ionic solid → Malleable and ductile: deforming the solid does not change the environment immediately surrounding each metal core
Conductivity of an ionic solid → Good: electrons are delocalized and relatively free to move