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Evaluate the following statements regarding carbon compounds: Statement-I: Carbon compounds are generally good conductors of electricity. Statement-II: They possess strong forces of attraction between their molecules.
Both I and II are correct
Only I is correct
Only II is correct
Both I and II are incorrect
Both I and II are incorrect
Most carbon compounds are poor conductors of electricity because they are covalent in nature and do not contain free ions or electrons to carry charge. Furthermore, these compounds possess weak intermolecular forces of attraction, which accounts for their relatively low melting and boiling points.
Most carbon compounds are poor conductors of electricity because they are covalent in nature and do not contain free ions or electrons to carry charge. Furthermore, these compounds possess weak intermolecular forces of attraction, which accounts for their relatively low melting and boiling points.
Think of carbon compounds like a box of individually wrapped chocolates; each chocolate is a self-contained unit (molecule) with very little pull between them, unlike a giant block of salt where every piece is tightly locked to its neighbor by strong electrical grips.
COvalent compounds are COnductors of nothing (Poor Conductors).
CH4тАЛ тАФ Methane, a classic example of a covalent carbon compound with weak intermolecular forces.
CnтАЛH2n+2тАЛ тАФ General formula for alkanes, illustrating the covalent nature of hydrocarbons.
Carbon atoms achieve stability by sharing electrons to form covalent bonds with other atoms. Unlike ionic compounds which dissociate into charged ions in solution, covalent molecules remain neutral, preventing the flow of electricity. Additionally, the weak van der Waals forces between these discrete molecules allow them to be easily separated by heat.
Carbon compounds are predominantly covalent.
Covalent bonds do not produce mobile charged particles.
Intermolecular forces in covalent compounds are van der Waals forces, which are significantly weaker than ionic electrostatic bonds.
Exceptions exist, such as Graphite, which is a good conductor due to delocalized electrons.
Low melting points allow for easy processing in manufacturing.
Diverse structural capability due to catenation.
Poor electrical conductivity limits their use in electronic circuitry unless specifically modified (like conductive polymers).
Fuels (e.g., LPG, Petrol)
Plastics and Polymers
Biological molecules (Proteins, Lipids)
Statement I is false because covalent bonding does not generate ions.
Statement II is false because the forces between carbon molecules (van der Waals) are weak, not strong.
Graphite is a notable exception to the conductivity rule due to its hexagonal layer structure and free electrons.
D is correct тАФ Both statements are incorrect because carbon compounds are typically poor conductors and held together by weak intermolecular forces.
Always remember that 'Ionic' implies high melting points and conductivity in liquid/aqueous state, while 'Covalent' implies low melting points and electrical insulation.