In many of their compounds the transition metals have covalence 9, forming nine bonds with use of nine hybrid spd bond orbitals. A set of maximum-valence single-bond radii is formulated for use in these compounds. These have now found that the structures of many compounds of transition metals can be discussed in a satisfying way on the basis of covalence 9 (or 8 in some cases) and have formulated a corresponding set of maximum-valence single-bond radii, given in Table 1. These radii may be used in interpreting the experimental values of bond lengths.It was recognized long ago that the formulas of the carbonyls Cr(CO)6, Fe(CO)5, and Ni(CO)4 correspond to completion of the argon structure (9 outer electron pairs, shared or unshared) by the metal atom. In Ni(CO)4, for example, the nickel atom might form sp3 single bonds (a shared electron pair) with each of the four carbon atoms and have five unshared pairs in its 3d orbitals. This structure is not acceptable, however, because it gives the nickel atom the formal charge -4, which cannot be overcome by the partial ionic character of the bonds. The structure in which the nickel atom has one unshared pair and forms double bonds with each of the carbon atoms, giving nickel the covalence 8 and zero formal charge, was suggested in 1921 by Langmuir (5) and verified in 1935 by the determination of the nickel-carbon bond length as 182 + 3 pm by Brockway and Cross (6). In Fe(CO)5 we assign double bonds from the iron atom to four carbon atoms and a single bond (with transfer of an electron to the iron atom) to the fifth, and in Cr(CO)6 three double bonds and three single bonds to carbon atoms, giving valence 9 to iron and chromium. The amount of ionic character of the metal-carbon bonds is large enough to make these structures compatible with the electroneutrality principle.The structure for Co2(CO)8 with cobalt-carbon double bonds and a cobalt-cobalt single bond corresponds to valence 9 and the argon structure for cobalt. The observed cobaltcobalt bond length 252.4 i 0.2 pm (7) leads directly to 126.2 pm for the single-bond covalent radius for cobalt with valence 9. Similar values are reported for R1 (v = 9) in other molecules with cobalt-cobalt bonds: 123.5 pm in dicobalthexacarbonyl diphenylacetylene (8), 123.5 pm in ethylidene tri(cobalttricarbonyl) (9), 123.5 pm in bis(tricobaltenneacarbonyl)acetone (10), 122.4 to 124.3 pm in Cos(CO)1sC3H (11), and 124.4 pm in hexacarbonyl- 3,4,5,5,6,6-hexafluorocyclohexa-1-yne-3-enedicobalt (12). Values of R1 (v = 9) for iron are given by observed iron-iron bond lengths as, for example, 123 pm in Fe2(CO)9 (13), 132 pm in Fe5(CO)15C (14) Table 1, are from 8 to 12 pm larger than the single-bond metallic radii, which for these metals correspond to the valence 6.The following equation (17) is to be used in calculating the bond length for a bond with bond number n (less than 1) between atoms A and B: Bond length = R1(A) + R1(B) -60 pm log n -CIXA -XBI [1] In this equation XA is the electronegativity of atom A and c is the Schomaker-...