Question

Why do network solids typically have higher melting temperatures than molecular solids?

A. Network and molecular solids typically have the same melting temperatures.
B. Network solids have covalent bonds between all atoms of the crystal.
C. All covalent substances do not have strong attractive forces between them.
D. All covalent substances have strong attractive forces between them.

Answer 1

@Hoslos

Answer 2

@dtan5457

Answer 3

Network solids have covalent bonds instead of intermolecular bonds. Covalent bonds are alot stronger, making it a lot harder to melt.

Answer 4

So is it D?

Answer 5

Whereas molecular solids are generally of low boiling point and made of Hydrogen bonds and London Dispersion forces. As well as dipole-dipole attractions.

Answer 6

So what is the answer?

Answer 7

I'm debating between B and D.

Answer 8

Me too.

Answer 9

But @dtan5457 , if we compare CO2 with NH4 for instance, which one seems to be stronger?

Answer 10

I will go for D.
Differently from network solids that have a chemical bond called covalent bond, the molecular solids do not have a chemical bond. Their bonds are of electrostatic or coulumbic nature, meaning it is due to the attraction of opposite charges among the ions. There are also hydrogen bonding in molecular solids. They are also of low boiling and melting point as well as soft in durability, compared to the network solids.
CO2 is a molecular solid, in which dipole-dipole attraction occurs between C and O, making a relatively soft structure than a covalent one like graphite.

Answer 11

Oh it was B....

Answer 12

Ouch, sorry. Tricky question.