Covaent Bonding Flashcards
Definition of covalent bonding
The electrostatic attraction between protons in two nuclei and a shared pair of electrons between them
how strong are covalent bonds
covalent bonding is a very strong attraction
properties of simple molecular substances like c60 fullerene
low boiling point
don’t conduct electricity
why do simple molecular substances have low boiling points
- although simple molecules contain very strong covalent bonds there are also weak IMFs between the molecules
- when simple molecular substances boil its the weak IMFS which break
as molecular mass increases, what happens to the boiling point of simple molecular substances
as molecular mass increases so does the strength of the weak IMFs resulting in the boiling point increasing
why dont simple molecular substances conduct electricity
- electrical conductivity require charged particles that can move freely
- but in simple molecular substances there aren’t any charged particles
- simple molecular substances never conduct electricity because molecules are neutral
what is C60 fullerene
- c60 fullerene is a unique simple molecule composed of 60 carbon atoms in a ball
what is c60 fullerene boiling point like
its boiling point is low, but not as low as other molecules because of its high molecular mass
why is c60 fullerene soft and slippery
because the molecules can role over eachother easily
why is c60 fullerene an electrical insulator
because the molecules are neutral
give 3 examples of giant covalent substances
diamond
graphite
silicon dioxide
what is diamond
a form of pure carbon arranged in a giant lattice
descibe the stricture of diamond
- every carbon makes 4 covalentbonds
- tetrahedal shape
- ## strong grid like arrangement
why does diamond sublime at very high temperatures
- covalent bonds are very string
- there are lots of bonds in a giant lattice
- lots of energy is required to break all the bonds
what is diamond used for
cutting
