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Inorganic chemistry B.Sc III

Inorganic chemistry B.Sc III. Hard acid and soft acid and bases. Hard and Soft Acids and Bases. 1965- Ralph Pearson introduced the hard-soft-acid-base (HSAB ) principle. Hard acids prefer to coordinate the hard bases and soft acids to soft bases”

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Inorganic chemistry B.Sc III

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  1. Inorganic chemistryB.Sc III Hard acid and soft acid and bases

  2. Hard and Soft Acids and Bases • 1965- Ralph Pearson introduced the hard-soft-acid-base (HSAB) principle. • Hard acids prefer to coordinate the hard bases and soft acids to soft bases” • This very simple concept was used by Pearson to rationalize a variety of chemical information. • 1983 – the qualitative definition of HSAB was converted to a quantitative one by using the idea of polarizability. • A less polarizable atom or ion is “hard” and a more easily polarized atom or ion is “soft”

  3. Hard acid: • High positive charge • Small size • Not easily polarizable • Hard base: • Low polarizability • High electronegativity • Not easily oxidized

  4. Soft acid: • Low positive charge • Large size; easily oxidized • Highly polarizable • Soft base: • High polarizability • Diffuse donor orbital • Low electronegativity • Easily oxidized

  5. Hard and soft acids and bases Hard acids or bases are small and non-polarizable Soft acids and bases are larger and more polarizable Halide ions increase in softness: fluoride < chloride<bromide<iodide Hard-hard or soft-soft interactions are stronger (with less soluble salts) than hard-soft interactions (which tend to be more soluble).

  6. Most metals are classified as Hard (Class a) acids or acceptors. Exceptions shown below: acceptors metals in red box are always soft (Class b). Other metals are soft in low oxidation states and are indicated by symbol. Solubilities: AgF > AgCl > AgBr >AgI But…… LiBr > LiCl > LiI > LiF Class (b) or soft always

  7. Chatt’s explanationClass (b) soft metals have d electrons available for p-bonding Model: Base donates electron density to metal acceptor. Back donation, from acid to base, may occur from the d electrons of the acid metal into vacant orbitals on the base. Higher oxidation states of elements to the right of transition metals have more class b character since there are electrons outside the d shell. Ex. (Tl(III) > Tl(I), has two 6s electrons outside the 5d making them less available for π-bonding) For transition metals: high oxidation states and position to the left of periodic table are hard low oxidation states and position to the rightof periodic table are soft Soft donor molecules or ions that are readily polarizable and have vacant d or π* orbitals available for π-bonding react best with class (b) soft metals

  8. Hard acids tend to react better with hard bases and soft acids with soft bases, in order to produce hard-hard or soft-soft combinations In general, hard-hard combinations are energetically more favorable than soft-soft An acid or a base may be hard or soft and at the same time it may be strong or weak Both characteristics must always be taken into account e.g. If two bases equally soft compete for the same acid, the one with greater basicity will be preferred but if they are not equally soft, the preference may be inverted

  9. Fajans’ rules • For a given cation, covalent character increases • with increasing anion size. • For a given anion, covalent character increases • with decreasing cation size. • The covalent character increases • with increasing charge on either ion. • Covalent character is greater for cations with non-noble gas • electronic configurations. A greater covalent character resulting from a soft-soft interaction is related With lower solubility, color and short interionic distances, whereas hard-hard interactions result in colorless and highly soluble compounds

  10. Application of HSAB principle

  11. Quantitative measurements Absolute hardness (Pearson) Mulliken’s absolute electronegativity (Pearson) EHOMO = -I ELUMO = -A Softness

  12. Electronic Factors HSAB Concepts • Using HSAB guidelines, reactions between acids and bases can be often be predicted successfully (though not always) Q: Is OH- or S2- more likely to form an insoluble salt with a +3 transition metal ion? A: The harder species will bind more strongly. Between OH- or S2-, OH- is the harder species.

  13. Electronic Factors STABILITY OF COMPLEX Q: Why is AgI(s) very water-insoluble, but LiI very water-soluble? A: AgI is a soft acid-soft base combination, while LiI is hard-soft. The interaction between Li+ and I- ions is not strong. AgI(s) + H2O(l)  essentially no reaction LiI(s) + H2O(l)  Li+(aq) + I-(aq)

  14. Qualitative Analysis • In the separation of the group cations carried out this year, HSAB rules were used to separate classes of ions based on different hard and soft interactions • Group II: Hg2+, Cd2+, Cu2+, Sn2+, Sb3+, Bi3+ • Group III: Mn2+, Fe2+, Cu2+, Ni2+, Zn2+, Al3+, Cr2+ • Group IV: Ca2+, Sr2+, Ba2+, K+, NH4+ soft and borderline acids borderline hard acids

  15. Separation of Cations • The soft and borderline cations are separated through reaction with the soft base sulfide, S2-. Group II sulfides are less soluble than group III, so in order to selectively remove group II ions, a low pH is used: H2S(g)D 2H+(aq) + S2-(aq) • Even at low S2- concentrations, the group II ions precipitate (stronger interactions with the soft base, S2-) • Raising the pH increases the S2- concentration, which allows the precipitation of group III ions • The group IV are then precipitated as hydroxides. These cations are harder and prefer the hard base OH-.

  16. Ambidentate Bases • SCN- (thiocyanate) can interact through either its S or N atom with Lewis acids. It can donate an electron pair through more than one atom. • Interaction will be through the S-atom with a soft acid, or through the N-atom when interacting with hard acids. • Cr(III) interacts as Cr-NCS, while Pt(II) does so as Pt-SCN

  17. Electronic Factors Inductive Effects • Electron donating substituents enhance base strength and electron-withdrawing groups enhance electron acceptor (acid) strength PMe3 stronger base than PH3 gas-phase base strengths NMe3 > NHMe2 > NH2Me > NH3 strongest base weakest base This plays a role in bond lengths also Me = methyl; alkyl, aryl groups are electron donating; F, CF3, CN, etc. are e- withdrawing

  18. Structural Factors Structural Rearrangement • In some cases, a center must adjust its hybridization in order to accommodate the formation of a new bond • Order of Lewis acid strength for BX3 (X = halides) is BF3 < BCl3 < BBr3 • This is due to better p-orbital overlap in BF3 than in BCl3, which is better than BBr3 (B-F bonds are shortest). Thus more energy is needed to change from the sp2-hybridized form of BF3. opposite order to what is expected for inductive effect sp2 sp3

  19. Predict which way the following reactions will go. • HI + NaF HF + NaI R • AlI3 + 3NaF AlF3 + 3NaI R • CaS + H2O CaO + H2S R • TiF4 + 2TiI2 TiI4 + 2TiF2 L • CoF2 + HgBr2 CoBr2 + HgF2 L • HgO + H2S HgS + H2O R

  20. Predict which way the following reactions will go. HI + NaF ----------- HF + NaI R AlI3 + 3NaF AlF3 + 3NaI R CaS + H2O CaO + H2S R TiF4 + 2TiI2 TiI4 + 2TiF2 L CoF2 + HgBr2 CoBr2 + HgF2 L HgO + H2S HgS + H2O R

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