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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","bond energies",{"label":268,"url":269,"covers":270},"CRC Handbook of Chemistry and Physics, 2007, and Olmsted & Williams, Chemistry, 5th ed. (2011), via Chempendix","https://sites.google.com/site/chempendix/bond-lengths","bond lengths",[272,273,274,275,276],"These are AVERAGE values over many compounds, so bond-energy estimates of ΔH are approximations; enthalpies of formation give more accurate 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 (1.33 Å) → C≡C 837 (1.20 Å).","Bond lengths (Å) are average values; a dash means the length source does not tabulate that bond (mostly interhalogen pairs and some Si/N/P/O combinations).","This table is a general reference; averaged bond energies vary somewhat from one compound to another.",[278,279,280],"chemical-bonding-and-lewis-structures","molecular-geometry-and-bonding-theories","thermochemistry",[282,283,284,285,286,287,288,289,290,291,292],"H","C","N","O","F","Cl","Br","I","Si","P","S",[294,295,296,297,298,299,300],"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",[302],"standard-enthalpies-of-formation","Average Bond Energies and Bond Lengths","Estimate a reaction enthalpy as ΔH ≈ Σ(bonds broken) − Σ(bonds formed) using these averaged values.",[306],{"key":18,"label":307},"Bond order",1787246032876]