In an earlier paper1 the stability constants of Oo(II), Ni(II), Zn(II), Cd(II)
and Pb(II) formato, acetato, propionato, butyrato, glycolato and chloroacetato complexes, determined by potentiometric1, polarographic~ , 3 and spectrophotometric4 methods, were summarfaed. Good agreement between stability constants determined by different methods were obtained, except for the complexes specified ~n the title, which were examined spectrophotometrically and polarographically

B. Grabarić

I. Filipović

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CROATICA CHEMICA ACTA CCA-909 CCACAA 48 (1) 17-18 (1976) YU ISSN 0011-1643 541.126 Note On the Stability Constants of Copper(II) Formato, Acetato, Propionato, Butyrato and Glycolato Complexes Determined by the Spectrophotometric Method B. Grabaric and I. Filipovic Laboratory of Inorganic Chemistry, Facuity of Technology, University of Zagreb, POB 179, 41001 Zagreb, Croatia, Yugoslavia R eceiv ed M ay 13, 1975 In an earlier paper1 the stability constants of Oo(II), Ni(II), Zn(II), Cd(II) and Pb(II) formato, acetato, propionato, butyrato, glycolato and chloroacetato complexes, determined by potentiometric1, polarographic~ , 3 and spectrophoto-metric4 methods, were summarfaed. Good agreement between stability con-stants determined by different methods were obtained, except for the complexes specified ~n the title, which were examined spectrophotometrically and polaro-gra phically. In the meantime we published an improved technique and numerical treatment in determining stability constants by the spectrophotometric method of corresponding solutions5, so we investigate these systems more rigorously. The measurements were carried out at 25.0 .± 0.2 °C in buffer solutions of constant acid to salt ratio, being 1 : 2 for formate and glycolate, 5 : 1 for ace;tate and 6 : 1 for propionate and butyrate. Ionic strength of all solutions was kept at a constant value of 2 mol dm-3 by adding sodium perchlorate. Measurements of absorption were performed at 760 nm. The change of pH between 3 to 5 had no influence on absonption. The stability constants obtained under these e~perimental conditions and with the apparatus, which were same as previously4, but with the new technique and numerical treatment, are given in Table, together with their 95 per cent confidence intervals. It must be emphasized, however, that the polarngraphic method is prefered over the spectrophotometric one, because the experimental conditions re.quired for the former allow very low metal ion concentrations to be used. This is advantaigeous when precipitate can be formed. E. g. in the spectrophotometric investigation ,of the specified complexes (except for Cu(II) formato complexes), the required exiperimental conditions do not allow investigation at ligand concentrations higher than 0.1 mol dm-3 due to the preci<pitation ·of a slightly soluble Cu(II) complex. The present results confirm all conclusions in the earlier papers1-4, but are in much better agreement with those obtained by polarogrnphic2•3•6 and potentiometric7 method, than the earlier ones4. This was e:x:pected because of the imprO'vements in technique and numerical treatment. 1S :B. GRABARIC AND I. FILIPOVIC TABLE Stability constants of Cu(II) complex es Ligand log 131 log (34 Formate 1.59 ± 0.08 2.48± 0.11 2.92±0.22 3.58±0.12 Acetate 1.91 ±0.01 2.46± 0.01 Propionate 1.94±0.01 2.76±0.08 Butyrate 1.89 :i: 0.02 4.13±0.02 Glycolate 2.46±0.04 REFERENCES 1. I. Filip o vi c, T . M a tus i n o vi c, B. Mayer, I. Pi l j a c, B. B a ch - D r a-g u tin o vi c, and A. Bu j a k, Croat. Chem. Acta, 42 (1970) 541. 2. I. Filipovic, I. Pi l j a c, A. Med v e d, J. S av i c, A. Bu j a k, B. B a ch-- D rag u tin o vi c, and B. Mayer, Croat. Chem. Acta 40 {1968) 131. 3. I. Filipovic, A Bu j a k, and V. Vu k i c e vi c, Croat. Chem. Acta, 42 (1970) 493. 4. B. Grab a r i c and I. Filipovic, Croat. Chem. Acta, 42 (1970) 479. 5. B. Grab a r i c, I. Pi l j a c, and I. Filip o vi c, Anal. Chem., 45 (1973) 1932. 6. B. G r a b a r i c, M. T k a l c e c, I. P i l j a c, I. F i l i p o vi c, and V 1. S i m e o n Anal. Chim. Acta 74 (1975) 147. 7. B. Grab a r i c, B. Mayer, I. Pi l j a c, and I. Filipovic, Electrochim. Acta 20 (1975) 799. SAZETAK Odredivanje konstanti stabilnosti formijato-, acetato-, propionato-, butirato-glikolato-kompleksa bakra(II) spektrofotometrijskom metodom B. Grabaric i I. Filipovic Konstante stabilnosti kompleksa navedenih u naslovu odredene su usavrsenom spektrofotometrijskom metodom korespondiraju6ih otopina obzirom na tehniku mje-renja i numericko-statisticku obradu. Dobivene konstante stabilnosti mnogo se bolje slazu sa konstantama stabilnosti dobivenim polarografskom i potenciometrijskom metodom od ranije navedenih. ZA VOD ZA ANORGANSKU KEMIJU TEHNOLOSK'I FAKULTET SVEUCILISTA U ZAGREBU Prispj elo 13. svibnja 1975. CROATICA CHEMICA ACTA CCACAA 48 (1) 19-24 (1976) CCA-910 YU ISSN 0011-1643 539.19:516 Original Scientific Paper Graph Theory and Molecular Orbitals. XVI. on n:-Electron Charge Distribution1 I. Gutman and N. Trinajstic The Rugjer Boskovic Institute, P .O.B. 1016, 41001 Zagreb, Croatia, Yugoslavia R eceived M a y 16, 1975 An integral formula is derived exhibiting the dependence of the n-electron charge density (in the framework of HU.eke! theory) on the coefficients of the characteristic polynomial of the molecular graph and o.ne of its subgraphs. Several simple consequences of this formula are demostrated. The n:-electron charge density is cine of the most important pieces of infor:mation about a conjugated molecule which can be obtained from simple Ruckel MO calculations2• This quantity was first intrnduced by Coulson3 and was later successfully correlated with a number of e:xiperimental findings (e . g., reactivity towards electrophilic and nucleophilic reagents in aromatic substitution reactions4, proton NMR shifts5, etc.). Besides, there is a close relationship between the n:-electron charge distribution and the d i.pole moment of a conjugated molecule6• A well-known result is a uniform charge distribution in artemant hydro-carbons regardless any detail in their structure.7 No analog,ous regularity exists for non-alternant hydrncarbons. The above results were also quite recently obtained using graph-theoretical considerations and proof-1echniques8,9 • In this work we would like to present some additional results leading to the further understanding of the dependence of n:-electron charge density on structural features of the molecule. We use here the formalism of graph theory as it was developed in earlier papers of this series10• Thus, in case the molecular graph G possesses N vertices, A= A (G), its adjacency matrix will be de-fined as A = { 1 if vertices p and q are adjacent pq 0 otherwd.se (1) The characteristic polynomial of G is P (x) = det I x 1 - A I (2) Its roots (i.e. graph spectrum) are denoted as x 1 , x 2, ••• , XN· For graphs without self-loops, as are the molecular graphs corresponding to conjugated hydro-carbons, N ~xi= O j = l (3) 20 I. GUTMAN AND N. TRINAJSTIC Let G, be a subgraph of G obtained after removal of the vertex r and all incident edges to it from the graph G. Let further Gh be a graph obtained by introducing a self-loop with a weight h on the vertex r of the graph 0 11- 13• The weight h is to• be understood as a variable parameter. In matrix notation this means that A pq (Gh) = A pq (G) for all p and q, except for p = q = r, when A rr (Gh) = h and A,, (G) = 0 Therefore, for a graph with a self-loop with weight h, Of course., N L xi= h j = l Gh = G for h = 0 (4) (5) (6) (7) We denote the characteristic polynomial of G, and G h by P , and Ph, respectively. The following relation was proved elsewhere12,1a. The characteristic polynomial P may be written in the form N p = p (x) = L an x N-n n = O This enables us to define another polynomial, H, where i = v - 1. Then H = H (x ) = (i x)N P (1/ix) H = L i" a11 x" n which can be also presented as where H=U+iV U = U (x) = L (--)" a 2 n x 2" n V = V (x) = L (- )" aw+i x2n+1 n In an analogous way we define the. polynomials Hn U ,, V ,, and H1,, U1,, V 1,, Hr= (ixt· 1 P, (1/ix) = U, + i V, Hh = (ix) N Ph (1/ix) = u,, + i vh Because ·of the relation (8), and therefore, H h =H-ihxH, U h =U+h xV, Vh= V-hxU, (8) (9) (10) (11) (12) (13) (14) (15) (16) (17) (18) (19) GRAPH THEORY AND MOLECULAR ORBITALS. XVI. 21 which finally gives [ H :, [ = [(U + h X Vr) 2 + (V - h X U,.)2]'/• (20) We note that the dependence of the coefficients an on the molecular graiph structure is nowadays completely elucidated14- 18• Therefore, the topological pro-perties of the polynomials H, U, V, etc., are also well understood1. For later discussion it will be important that the polynomials U and U r are positive for all values of x. This is a consequence of the relation (21) which holds for an arbitrary graph1• A Topological Formula for rt-Electron Charge Density In Hiickel theory the rt-electron charge density (Qr) ·on the atom r is related to the rt-electron energy19 as follows oE" Qr = - -0 a, (22) where ar is the Coulomb integral2 •4•6 corresponding to the atom (vertex) r, and E" is the total rt-electron energy. When the corresponding graph-theoretical terminology is used10, the Eq. (22) is given by, oE"(G) Qr= - --0 A ,, (23) The above equation may be further transformed by taking into account Eqs. (4), (5), and (7): = [ o E" (Gh)] Q, oh h = o (24) In1 it is shown that the following equation is valid for graphs having no self-loops (that is, for graphs whose spectra fulfill Eq. (3)): += E" (G) = (1/rt) J ln ~~I dx (25) Using Eq. (6) the above formula may be easily extended to include graphs possessing self-loops. Namely, +oo E,, (Gh) = h + (1/rt) J ln ~~h I dx (26) A detailed analysis shows that += a E .. (G,,l = 1 + (l/rc) J a ln [ Hh [ dx ah ah x 2 (27) -co 22 I. GUTMAN AND N . TRINAJSTIC which combined with Eq. (20) and substituted iback into Eq. (23) yields a topo-logical formula for :n:-electron charge density: +co f UV -VU Q, = 1 + (1/:rt) r r u2 + v2 dx (28) x E:xipression (28) exhibits the exact analytical form of the dependence of Q, on the coefficients of the characteristic polynomials P and P,. Another form of Eq. (28) is +co Q, = 1 + (1/rr.) f P, (ix) dx P (ix) (29) This elegant formula was first obtained by Coulson and Longuet-Higgins19, but using a very different way of reasoning. It can be shown that Eqs. (28) and (29) are completely equivalent. However, the form of Eq. (28) is more convenient for the following discussion. It results from Eqs. (28) and (29) that Q, is uniquely determined with (and that it can be calculated from) the spectra of graph G and G,. It is interesting to compare this conclusion with the original definition of charige density3, which is based solely on the coefficients of MO's (i. e. eigenvectors o.f the graph G). DISCUSSION The form of Eq. (28) indicates that the dependence of Q, on the molecular topology is rather complicated. This is inded the cases,9,20 • However, in the present discussion we wish to show some properties of the charge distribution which follow straightforwardly from our formula and the topological behaviour of the polynomials H and H,. First, for all alternant systems it is always17,18, and therefore it follows from Eq. (13), V(x)=V,(x)=O This leads, then, to Q, = 1 (30) (31) (32) Thus, the charge distribution in all alternant hydrocarbons (including free radicals) is uniform. In non-alternants the charge density of a :n:-cerrtre oibviously depends both on the hydrocarbon itself and the :n:-centre position in the molecule. This fact is well reflected in formula (28). Namely, Eq. (28) may be also written as Q, = 1 +A,+ B, (33) where + co A, = - (1/rr.) f vu, dx (34) u2 + v2 x GRAPH THEORY AND MOLECULAR ORBITALS. XVI. 23 + oo J UV, dx B, = (l/rr.) _ u2+v2 x (35) -00 Since the polynomials U, U, (and of course, U2 + V2) are positive for all values of x, the sigru of the integral A, is determined with V (x) only; that is to say solely from the molecular graph G. By analogy, the sign of the term B, depends on the graph G, only. Hence, A, may be understood as being the »molecular« and B, as being the »positional« contribution tQ the charge density. The actual numerical vaiue of the re-electron charge density results from the delicate balance of these two contributions. As a simple illustration let us consider a non-alternant hydrocarbon molecule having only one odd-membered cycle r, while all other structural details are arbitrary. Let the size of r be y. The coef-ficients a2 n+ 1 of the characteristic polynomial of such graphs have the property ] { O for 2n+l < y sign[(-)" aw+i = (-)«r + l)/ 2 for 2n + 1 ;;;,, y Therefore, from Eq. (13), sign [ V ~x) ] = (-) Cr+ 1)/2 and finally from Eq. (34), sign [A,]=(-) <r-1) /2 = { + 1 if y = 4m + 1 -1 if y = 4m + 3 it is seen that the sign of A, is not depending on r . (36) (37) (38) Let us now consider an atom r belonging to the cycle r . Graph G, then contains no odd cycles and therefore17,ts V, (x) = 0. Consequently, B, = 0, and the only contribution to Q, stems from A,. The following rule follows, therefore, immediately from Eq. (38). Rule In a conjugated hydrocarbon containing only one odd-membered cycle all atoms belonging to this cycle are negatively charged (Q, > 1) if the size of the cycle is 4m + 1 and positively charged (Q, < 1) if the size of the cycle is 4m + 3. · This result is independent of any other detail in the molecular structure. The case when the considered re-centre does not belong to r may be treated by analogy. However, G, contains now the cycle r and therefore, sign [V,~x)] = (-)<r+l)/2 which combined with Eq. (35) yields, sign [B,] = { - 1 if y = 4 m + 1 + 1 if y = 4m + 3 (39) (40) a result which is expected since the total charge of the neutral hydrocarbon is zero. 24 I. GUTMAN AND N. TRINAJSTIC REFERENCES l.PartXV:I. Gutman andN. Trin a jstic, J . Chem. Phys., inpress. 2. K. H i g a s i, H . B a b a , A . Rem b au m, Quantum Organi c Chemistry, Wiley, New York 1965, Chapter V. 3. C. A. Co u 1 son, Proc. Roy. Soc. (London) A 169 (1939) 413. 4. L . Sa 1 em. The MoLecular Orbital Theory of Con jugated Systems, B enj amin, New Yor.k 1966, Chapter 6. 5. R. B. Herman, Int. J. Quantum Chem. 2 (1968) 165. 6. A. Streit w i es er, Jr., Molecular Orbital Theory for Organic Chemists, Wiley, New York 1961, Chapter 6. 7. C. A. Co u 1 son and G . S. Rush brook e, Proc. Cambridge Phil. Soc. 36 (1940) 193; G. G. Ha 11, Proc. Roy. Soc. (London) A 191 (1955) 251. 8. Part V: I. Gut ma 11 and N. Tri 11 a j st i c, Chem. Phys. Lett. 20 (1973) 25. 9. Part VI: I. Gutman, N. Trina j st i c, and T. Ziv k o vi c, Tetrahedron 29 (1973) 3449. 10. For review see: I. Gutm a n and N. T ri n a j st i {;, Topics Curr. Chem. 42 (1973) 49 ; Croat. Chem. Acta 45 (1975). 11. R. B. Ma 11 ion, A. J. Schwenk, and N. Trina j st i c, Croat. Chem. Acta 46 (1974) 171. 12. R. B. Ma 11 ion, N. Trin a j st i c, and A. J . Schwenk, Z. Naturf orsch. 29a (1974) 1481. 13. R. B. Mallion, A. J . Schwenk, and N. Trinaj s tic, in M. Fiedler (Ed.), Recent Advances in Graph Theory, Academia, Prague, 1975, p . 345. 14. C. A. C o u 1 son, Proc. Cambridge Phil. Soc. 46 (1950) 202. 15. H . Sachs, Pub!. Math. Debrecen 11 (1963) 119. 16. H. H o soy a, Theoret. Chim. Acta 25 (1972) 215. 17. Part I: A. Graovac, I. Gutman, N. Trinajstic, and T. Zivkovic, Theoret . Chim. Acta 26 (1972) 67. 18. Part II : D. C ve t k o vi c, I. Gutman, and N. Trina j st i c, Croat. Chem. Acta 44 (1972) 365. 19. C. A . Co u 1 son and H. C. Long u et - Higgins, Proc. Roy. Soc. (London) A 192 (1947) 39 ; ibid. A 192 (1947) 16. 20. I. Gutman, Ph. D. Thesis, University of Zagreb 1973. SAZETAK Teorija graJ'ova i molekularne orbitale. XVI. 0 raspodjeli it-elektronskog naboja I. Gutman i N . Trinajstic Izvedena je integralna formula koja ukazuje na vezu izmedu raspodjele n-elek-tronskog naboja u ko.njugiranom ugljikovodiku i koeficijenata karakteristienog poli-noma .pripadnog molekularnog grafa i jednog njegovog podgrafa. Prikazano je takoder i nekoliko jednostavnih posljedica ove topoloske formule. INSTITUT » R U D ER BOSKOVIC«, 41001 ZAGREB, HRVATSKA P r ispjelo 16. svibnja 1970. 

On the Stability Constants of Copper(II) Formato, Acetato, Propionato, Butyrato and Glycolato Complexes Determined by the Spectrophotometric Method

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