i only have one submission for these and i dont' really know how to tell which one has the higher boiling point. can you help?
Of each pair of solids, which one has the higher melting point?
Kr(s) or Cu(s)
and..
CCl4(s) or SiCl4(s)
nvm i got it wrong:(
Kr is a gas. Right? Cu is a solid. Right? So which do you think boils (melts, even) higher.
To determine which solid has the higher melting point, you need to consider the nature of the compounds involved. The melting point of a substance is influenced by factors such as the strength of the intermolecular forces between its particles.
For the first pair, Kr(s) and Cu(s), we have krypton (Kr) and copper (Cu). Krypton is a noble gas and exists as individual atoms in its solid state. These atoms are held together by weak London dispersion forces, which arise due to temporary imbalances in electron distribution. Copper, on the other hand, is a metal that forms a regular lattice structure held together by metallic bonding, which consists of a sea of delocalized electrons surrounding positively charged metal ions. Metallic bonding is generally stronger than London dispersion forces.
Based on this information, we can deduce that Cu(s) has a higher melting point than Kr(s) because metallic bonding is stronger than London dispersion forces.
For the second pair, CCl4(s) and SiCl4(s), we have carbon tetrachloride (CCl4) and silicon tetrachloride (SiCl4). Carbon tetrachloride is a covalent compound consisting of carbon and chlorine atoms bonded together by covalent bonds. Silicon tetrachloride is also a covalent compound with silicon and chlorine atoms bonded together. Both compounds have molecular structures and are held together by intermolecular forces like London dispersion forces and dipole-dipole interactions.
Comparing the two compounds, silicon tetrachloride (SiCl4) is larger and has a higher molar mass compared to carbon tetrachloride (CCl4). This suggests that SiCl4 has stronger London dispersion forces, resulting in a higher melting point compared to CCl4.
In summary:
- Cu(s) has a higher melting point than Kr(s) due to stronger metallic bonding compared to London dispersion forces.
- SiCl4(s) has a higher melting point than CCl4(s) due to stronger London dispersion forces caused by its larger size.