Diamond is a poor conductor of electricity because:
A. All four valence electrons are involved in covalent bonding, no free electrons
B. It has a layered structure
C. It has free electrons
D. It is made of carbon
Answer: Option A
Solution (By JKSSB Mock Tests)
In diamond, each carbon is sp³ hybridized and forms four covalent bonds, using all valence electrons. There are no delocalized electrons; thus it cannot conduct electricity. Graphite, with sp² hybridization, has one delocalized electron per carbon, making it a conductor. Diamond is an electrical insulator but excellent thermal conductor.
Explanation:
SO₂ from burning coal and NOₓ from vehicles form H₂SO₄ and HNO₃ in rain. CO₂ forms weak carbonic acid (normal rain pH ~5.6). Ammonia is basic and neutralizes acidity.
Explanation:
C₂H₅OH + CH₃COOH ⇌ CH₃COOC₂H₅ + H₂O (esterification). Conc. H₂SO₄ acts as catalyst and dehydrating agent. Ethyl ethanoate is an ester with fruity smell.
Explanation:
Sulfur dioxide (SO₂) from burning of fossil fuels (coal, oil) reacts with water vapor to form sulfurous and sulfuric acids, causing acid rain. Nitrogen oxides (NOx) also contribute. CO is a toxic gas but does not form strong acid; O₂ and N₂ are normal atmospheric gases. Acid rain damages ecosystems, buildings, and soil.
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