Difficulty: Easy
Correct Answer: Diamagnetic under normal conditions
Explanation:
Introduction / Context:Knowing whether a material is diamagnetic, paramagnetic, or ferromagnetic is essential in materials science and device engineering. Carbon in the diamond structure provides a classic case study of closed-shell bonding and magnetic response.
Given Data / Assumptions:
Concept / Approach:Diamagnetism arises when all electrons are paired; an applied field induces a small magnetic moment that opposes the field, giving a negative magnetic susceptibility. Diamond’s covalent network has paired electrons and no unpaired spin carriers, so it is diamagnetic. Paramagnetism requires unpaired electrons; ferromagnetism needs exchange-coupled ordering and domains.
Step-by-Step Solution:
Identify electronic structure of diamond: fully paired electrons in strong covalent bonds.Conclude absence of permanent dipoles; only induced moments occur.Therefore, classify as diamagnetic.Verification / Alternative check:
Magnetic susceptibility measurements show small negative χ for diamond, consistent with diamagnetism.Why Other Options Are Wrong:
Paramagnetism requires unpaired spins; ferromagnetism and antiferromagnetism require magnetic sublattices and ordering not present in diamond.Common Pitfalls:
Confusing graphite's conduction behavior with magnetic ordering; graphite is also diamagnetic.Final Answer:
Diamagnetic under normal conditions
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