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Estimate a reaction enthalpy from bond energies: ΔH ≈ Σ D(bonds broken) − Σ D(bonds formed).","Average bond energy table in kJ/mol — H, C, N, O, halogen, Si, P, and S bonds, single through triple — with bond lengths, for estimating reaction enthalpies from bonds broken and formed.",[13,17,20,23],{"key":14,"label":15,"type":16},"bond","Bond","text",{"key":18,"label":19,"type":16},"type","Bond Order",{"key":21,"label":22,"type":16},"energy","Bond Energy (kJ/mol)",{"key":24,"label":25,"type":16},"length","Bond Length 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Chemistry 2e, §7.5 Strengths of Ionic and Covalent Bonds (Tables 7.2 and 7.3)","https://openstax.org/books/chemistry-2e/pages/7-5-strengths-of-ionic-and-covalent-bonds","CC BY 4.0",[233,234,235,236,237],"These are AVERAGE values over many compounds — bond-energy estimates of ΔH are approximations; enthalpies of formation give exact values when available.","ΔH ≈ Σ D(bonds broken) − Σ D(bonds formed). Breaking bonds costs energy (positive); forming bonds releases it.","For the same pair of atoms, more bonds = stronger and shorter: C–C 345 kJ/mol (1.54 Å) → C=C 611 (1.34 Å) → C≡C 837 (1.20 Å).","Bond lengths are tabulated for the carbon single/double/triple ladders (C–C, C–N, C–O); a dash means the source does not tabulate a length for that bond.","ChemWhiz problems that need bond energies supply them in the problem statement; this table is the general reference.",[239,240,241],"chemical-bonding-and-lewis-structures","molecular-geometry-and-bonding-theories","thermochemistry",[243,244,245,246,247,248,249,250,251,252,253],"H","C","N","O","F","Cl","Br","I","Si","P","S",[255,256,257,258,259,260,261],"bond energy table","average bond energies kJ/mol","bond enthalpy table","bond energy calculation delta H","C-H bond energy","bond length table","single double triple bond strength",1785108608492]