Understanding what controls the strength of bonding of adsorbed intermediates to transition-metal surfaces is of central importance in many technologies,e specially catalysis and electrocatalysis.Our recently measured bond enthalpies of À OH, À OCH 3 , À O(O)CH and À CH 3 to Pt(111) and Ni (111) surfaces are fit well (standardd eviation of 7.2 kJ mol À1 )b y ap redictive equation involving only knownp arameters (gasphase ligand-hydrogen bond enthalpies,b ond enthalpies of adsorbed Ha toms to that surface,e lectronegativities of the elements,a nd group electronegativities of the ligands). This equation is based upon Paulingsequation, with improvements introduced by Matcha, derived here following manipulations of Matchase quation similar to (but going beyond) those introduced by Schock and Marks to explain ligand-metal bond enthalpytrends in organometallic complexes.Understanding the energetics of chemical reactions on transition-metal surfaces is crucial for many technologies, including the development of better catalysts,c hemical sensors,s urface organo-functionalization, microelectronics and optical device fabrication, bioengineered materials,a nd nanomaterials synthesis.H ere,w es how how trends in the experimentally measured bond enthalpies of adsorbed molecular fragments to late-transition-metal surfaces can be understood though simple properties of the metal and the adsorbed molecular fragment. We will refer to these adsorbed fragments as ligands herein, since we will follow pioneering work describing metal-ligand bond enthalpies in organometallic complexes. [1][2][3] Thus,w ec orrelate bond enthalpies with the electronegativity of the metal, the group electronegativity of the ligand, and the bond enthalpies of the ligand to an H atom. Specifically,w et reat four molecular fragments that bind to the metal via their OorCatom, and their adsorption enthalpies to Pt(111) and Ni(111) surfaces,which are the only systems for which the bond enthalpies have been experimentally measured for such molecular fragments.Herein, we derive an equation based on Paulings equation, electronegativies,a nd known bond enthalpies that is able to accurately reproduce these bond enthalpies with as tandard deviation of only 7.2 kJ mol À1 relative to experimental values for the limited systems for which data are available (ÀOH, ÀOCH 3 , ÀO(O)CH, and ÀCH 3 on Pt (111) and Ni (111)). Our derivation starts with Matchasb ond enthalpy equation, [1] itself an improvement on Paulings equation. We follow the approach of Schock and Marks, [2] who subtracted two of Matchase quations to establish ar elationship between D(LÀM(111)), the ligand-metal surface bond enthalpy,a nd D(LÀH), the gas-phase ligandhydrogen bond enthalpy,b ut instead we combine three of Matchase quations to the same end. Our derivation eliminates the gas-phase M À Md imer bond enthalpy, D(M À M), from Schocksa nd Marks equation, which we show is less appropriate for metal surfaces than the revised equation. This term is replaced with D(HÀM(111)), the bond enthalpy of ahydrog...