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What is Bond Dissociation Energy (BDE)?
The energy required to break a specific bond in the gas phase.
Define 'endothermic' in the context of bond energetics.
A process that requires energy input, such as breaking a bond.
Define 'exothermic' in the context of bond energetics.
A process that releases energy, such as forming a bond.
What is the relationship between bond order and bond dissociation energy?
Higher bond order (e.g., triple bond) generally corresponds to higher bond dissociation energy.
Define enthalpy of reaction ($\Delta H$) using bond dissociation energies.
The difference between the sum of the energies required to break bonds in reactants and the sum of the energies released by forming bonds in products: $\Delta H = \Sigma H(broken) - \Sigma H(formed)$.
Compare the energy changes in breaking vs. forming bonds.
Breaking bonds: requires energy (endothermic). Forming bonds: releases energy (exothermic).
How do bond length and bond strength relate to BDE?
Shorter bonds: stronger, higher BDE. Longer bonds: weaker, lower BDE.
Differentiate between single, double, and triple bonds in terms of BDE.
Single bonds: lowest BDE. Double bonds: intermediate BDE. Triple bonds: highest BDE.
What is the effect of increasing bond order on bond strength?
Increasing bond order (single to double to triple) increases bond strength.
What is the effect of a negative $\Delta H$ value?
The reaction is exothermic, meaning it releases heat.
What is the effect of a positive $\Delta H$ value?
The reaction is endothermic, meaning it requires heat.