Worksheet: Molecular, Network, Ionic, and Metallic Solids
In this worksheet, we will practice comparing the properties and examining examples of molecular, network, ionic, and metallic solids.
Which of the following quantities is larger in diamond than in graphite?
- ACovalent bond length
- BThermodynamic stability at 1 atm and 298 K
- CElectrical conductivity
- DReactivity with hydrogen
- EBond angle
Why does an amorphous solid typically melt over a wide range of temperatures?
- AThe material contains a mixture of compounds with different melting temperatures.
- BA solid–solid phase transition results in a crystalline material with a higher melting temperature.
- CThe melting temperature depends on the solvent content, which decreases slowly as the material is heated.
- DThere is a large amount of variation in the strength of intermolecular interactions throughout the material.
- EHeating causes the material to decompose, altering its melting temperature.
Which of the following statements concerning amorphous solids is false?
- AUnlike crystalline solids, amorphous solids tend to lose structural organization as their lattices extend.
- BUnlike crystalline solids, amorphous solids lack a repeating unit cell, leading to a random organization of atoms.
- CAmorphous solids are said to behave as supercooled liquids, leading to an ease in transitioning between physical states.
- DThe formation of amorphous solids is aided by the rapid cooling of a molten compound.