Chemistry Covalent Bonding

Covalent Bonding definition

Covalent bonding is the strong electrostatic attraction between a shared pair of electrons and the nuclei of the atoms in the bond

Why do the MP and BP of simple molecular structures increase with relative molecular mass

The larger a molecule is, the stronger inter-molecular forces of attraction are, and stronger IMF require more thermal energy to overcome

Why are the MP and BP of simple molecular structures low?

MP and BP of simple molecular structures are low as the weak inter-molecular forces of attraction require little thermal energy to overcome

Explanation for the high BP and Mp of giant covalent latices and why they are solid

A great deal of thermal energy is required to overcome the many strong covalent bonds to go from a solid to a liquid

Why is diamond so hard?

Diamond is extremely hard as many strong covalent bonds extend in all directions, and each carbon atom is bonded with 4 others.

Why can’t diamond conduct electricity?

Diamond can’t conduct electricity as all outer shells electrons are fixed in covalent bonds, and are unable to move

Why is graphite weak?

Graphite is weak as the weak inter-molecular forces of attraction which hold the layer of graphite together are easily broken, and layers can slide over one another

Why can graphite conduct electricity?

Graphite can conduct electricity as each carbon is bonded to three others, which means there is a free electron that is able to move, which means that a current is able to flow

Why is C60 (Buckminster Fullerene) weak?

C60 is weak as it is a simple molecular structure held together by weak inter-molecular forces of attraction

Why can’t C60 conduct electricity?

C60 can’t conduct electricity as even though there is a free electron, it can not move beyond the molecule.