Why is Graphite an electrical conductor while Diamond is an electrical insulator?
Answer and explanation
Correct answer: C. graphite possesses metallic close-packed planes while diamond forms weak van der Waals sheets
- Step 1: In graphite, each carbon is sp^2 hybridized, leaving one unhybridized 2p electron per atom delocalized across graphene planes to conduct electricity. Step 2. In diamond, all four valence electrons are tightly bound in localized sp^3 sigma bonds with a huge band gap (~5.5 eV). Answer: Graphite has delocalized pi electrons across its sp^2 sheets, whereas Diamond has all electrons localized in sp^3 sigma bonds. Why not the others: Graphite contains no metal ions; diamond is covalent, not ionic; density does not determine electrical conductivity.
Practise more Qualitative Analysis, Chemical Bonding and Periodic Trends.
Free questions with an explanation for every one, and full timed Medical College Admission Test (Bangladesh) mock tests.
More Qualitative Analysis, Chemical Bonding and Periodic Trends questions
- What characteristic flame color is produced by Sodium salts during a flame test?
- What characteristic flame color is observed for Potassium salts viewed through blue cobalt glass?
- Which reagent is used as a sensitive wet test to detect Ammonium ions (NH4+) through the formation of a brown precipitate?
- What is the chemical formula of the brown coordination complex formed in the confirmatory ring test for Nitrate ions (NO3-)? (Hard)
- Which precipitating reagent is added to test for the presence of Sulfate ions (SO4 2-) forming a white precipitate insoluble in dilute HCl?
- Why are transition metal complexes generally colored in aqueous solution? (Hard)