Graphite fluoride and graphite oxide are electrically conducting compounds.
A) True
B) False

Hint: Graphite oxide and graphite fluoride are covalent compounds of graphite. Conduction of electricity is due to the availability of delocalised or free electrons in a compound.

Complete answer:
We know that graphite is an allotrope of carbon. It has a large covalent structure forming layers of hexagonal rings in which each carbon atom forms three covalent bonds with other carbon atoms. There is a nonbonded electron from each carbon atom which is free to move between the layers of graphite. It is also called a delocalised electron as seen in metal. So, graphite is a good conductor of electricity.
When graphite makes bond with oxygen atom, graphite oxide is formed and when graphite makes bond with fluorine, graphite fluoride is formed. After making covalent bonds with oxygen (in graphite oxide) and fluorine (in graphite fluoride), there are no delocalised electrons present in both the compounds. We can say that they have very negligible electrical conductivity. So, they are bad conductors of electricity.
In the above question, it is written that graphite fluoride and graphite oxide are electrically conducting compounds, which is not a correct statement.

Hence, the correct answer is (B) false.

Note: Due to the presence of carbonyl and hydroxyl group in graphite oxide, it shows hydrophilic nature, whereas, due to the absence of hydroxyl group in graphite fluoride, it shows hydrophobic nature.
Graphite can be used as electrodes in batteries and for electrolysis due to its high conductivity.