Zinc loses electrons: Zn → Zn²⁺ + 2e⁻, thus it is oxidized (increase in oxidation state from 0 to +2). Copper ions gain electrons: Cu²⁺ + 2e⁻ → Cu, thus copper is reduced. Zn acts as the reducing agent, CuSO₄ as the oxidizing agent. This is a single displacement redox reaction. Zn is more reactive than Cu.
Explanation:
Unsaturated hydrocarbons contain at least one double or triple bond between carbon atoms. Benzene (C6H6) has a ring structure with alternating double bonds (delocalized pi electrons), making it highly unsaturated. Cyclohexane, propane, and methane contain only single bonds and are saturated hydrocarbons.
Explanation:
Half-life (t₁/₂) is the time taken for half of the radioactive nuclei in a sample to decay. It is constant for a given isotope and independent of initial amount (first-order kinetics). After one half-life, 50% remains; after two, 25%. It is a measure of stability. Short half-life = more radioactive.
Explanation:
Aluminium oxide: Al³⁺ and O²⁻. To balance charges, 2 Al³⁺ (total +6) combine with 3 O²⁻ (total -6). Thus valency of Al is 3. It loses three electrons. Formula determined by criss-cross method.
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