Concept explainers
(a)
Interpretation:
The energy required to break all of the bonds in one mole of
Concept Introduction:
The
The equation that describes the bond dissociation for
Bond energies are always endothermic and have a positive sign. It takes energy to break a bond.
The enthalpy of reaction can be determined by the sum of the bond dissociation energies of all the reactants minus the sum of the bond dissociation energies of all products present in
The equation to calculate enthalpy of reaction is as follows:
Negative sign in the equation depicts that bonds will form in the products. It is an exothermic process, so the energy charge is the negative of bond energy.
(b)
Interpretation:
The energy required to break all of the bonds in one mole of
Concept Introduction:
Refer to part (a).
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Chemistry: Principles and Practice
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- Which is the strongest bond energy? Cl(g) ΔH°f, = +121.3 kJ mol–1 CCl4(g) ΔH°f, = –95.98 kJ mol–1 HCl(g) ΔH°f, = –92.3 kJ mol–1 Question 8 options: Cl–Cl in Cl2 H–Cl in HCl C–Cl in CCl4arrow_forwardUsing the VSEPR Theory, draw the following compounds; represent them as covalent bonds. a) CH3OH b) CO2arrow_forwardWhich of these molecules has the highest bond energy. (A) F2 (B) Cl2 (C) Br2 (D) I2arrow_forward
- State whether each of these statements is true or false. (a)A carbon–carbon triple bond is shorter than a carbon–carbonsingle bond. (b) There are exactly six bonding electrons inthe O2 molecule. (c) The C—O bond in carbon monoxide islonger than the C—O bond in carbon dioxide. (d) The O—Obond in ozone is shorter than the O—O bond in O2. (e) Themore electronegative the atom, the more bonds it makes toother atoms.arrow_forwardJudging from their relative positions in the Periodic Table, which atom in each set is more electronegative? (a) Carbon or nitrogen (b) Chlorine or bromine (c) Oxygen or sulfurarrow_forwardDraw all possible resonance structures for each of these compounds. Determine the formal charge on each atom in each of the resonance structures:(a) O3(b) SO2(c) NO2 −(d) NO3−arrow_forward
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