22541-76-0

Basic information

• Product Name: VANADIUMION
• Synonyms: vanadium(4+)
• CAS NO: 22541-76-0
• Molecular Formula: V+4
• Molecular Weight: 50.9415
• Mol File: 22541-76-0.mol

Chemical Properties

• Boiling Point: °Cat760mmHg
• Flash Point: °C
• Appearance: /
• Density: g/cm³
• CAS DataBase Reference: VANADIUMION(CAS DataBase Reference)
• NIST Chemistry Reference: VANADIUMION(22541-76-0)
• EPA Substance Registry System: VANADIUMION(22541-76-0)

Safety Data

• Hazardous Substances Data: 22541-76-0(Hazardous Substances Data)

Usage

InChI:InChI=1/V/q+4

Upstream product

• 7440-62-2 vanadium 
• 12436-25-8 sodium metavanadate 
• 12035-98-2 vanadium(II) oxide 
• 7647-01-0 hydrogenchloride 
• 22541-77-1 vanadium(III) 
• 22537-31-1 vanadium⁽⁵⁺⁾ 
• 15121-26-3 vanadium ⁽²⁺⁾ 
• 15092-81-6 peroxodisulfate ion 
• 69-09-0 chlorpromazine hydrochloride 
• 22541-54-4 arsenic(III) 

Downstream Products

• 16522-06-8 oxo citrato vanadate (IV) (1-) 
• 22537-31-1 vanadium⁽⁵⁺⁾ 

Relevant articles and documents

Kinetics of oxidation of iodide by vanadium (V): Catalysis by the water pools of CTAB reverse micelles

The kinetic study of the oxidation of iodide ion by V(V) has been carried out in the water pools of cetyl trimethyl ammonium bromide(CTAB) reverse micelles in a mixture of chloroform-hexane (3 : 2). The study of the effect of concentration of V(V) and I- on rate show that the reaction obeys first order kinetics with each of the reactants. A plot of k′ (pseudo first order rate constant) versus [H+] is linear with a positive intercept at constant concentrations of iodide and bromide. The rate of the reaction is markedly increased in the reverse micellar medium compared to conventional aqueous medium under identical conditions. The pronounced acceleration in reverse micelles has been accounted for by the concentration effect in the water pool which have an effect on kinetics.

Reactions of molybdenum(vi) with metal ion reductants

The reactions of aqueous H2MoO4 at low pH with titanium(ii), titanium(iii), europium(ii), vanadium(ii), and germanium(ii), as monitored at 430 nm, give biphasic profiles featuring a sharp rise in absorbance followed by a marked decrease (Fig. 1). The final product is the dimeric Mo(v) cation, [Mo2O4]2+, and the strongly absorbing intermediate is taken as a monomeric Mo(v) species. The molar absorbances of the transients from different reductants are not the same, nor are the rate laws governing the fadings. None of the decay curves exhibits evidence of a second order dependence on the transient. The kinetic behaviors of these systems are consistent with the intervention of successor complexes of the type, (formed by inner sphere reductions of Mo(vi)), which decompose, via first-order processes, to a monomeric Mo(v) species. The latter then experiences rapid dimerization, which is kinetically silent. The possibility that Ge(ii) bypasses the unstable tripositive state by reducing Mo(vi) to Mo(iv) (which then undergoes rapid Mo(vi)-Mo(iv) comproportionation) is considered. The Royal Society of Chemistry 2006.

Oxidation kinetics of acetophenone oximes with vanadium(v)

Oxidation kinetics of acetophenone oxime (APO) and p-hydroxyacetophenone oxime (HAPO) by vanadium(V) in aqueous acetic acid medium is reported. The reactions are totally second order, first order with respect to each reactant under second order conditions and negative order with respect to substrate under pseudo-first order conditions. The proposed mechanism involves a two-electron oxidation to the carbocation, which ultimately forms the corresponding keto compound.

Kinetics of oxidation of iodide by vanadium (V)

Kinetics of oxidation of iodide ion by VV under uncatalysed and RuIII catalysed conditions in aqueous perchloric acid medium have been studied. The reaction is first order in [VV] and first order in [I-]. With [H+], the reaction shows a complex behavior of 1.5 order till [H+] is 0.5 M and second order beyond that concentration. In the case of RuIII catalyzed oxidation, the reaction exhibits a dual character of first order and zero order in [VV]. The first order component shows 1.5 order in [I-] first order in III> and 1.5 order in [H+]. The zero order component shows first order in [I-], first order in [RuIII] and independent of [H+]. No catalysis has been observed with OsVIII. Suitable rate laws have been postulated based on the observations.

Mechanism of vanadium(V) oxidation of thallium(I) in aqueous acetic acid medium: A kinetic study

The vanadium(V) oxidation of thallium(I) in aqueous acetic acid containing hydrochloric acid is considerably accelerated both by the hydrogen and chloride ions as well as by increasing acetic acid content of the medium. The experimental results obey the rate law: d[V(V)] k K1 β3 [V(V)]T [Tl(I)]T [H-]T2 [Cl-]T3 dt {1 + β1[Cl-] + β2[Cl-]2 + β3[Cl-]3} {1 + 2K1[V(V)][H-] + K1[H-]2 + 2K12[V(V)][H-]3} where β1, β2 and β3 are cumulative stability constants of the species TlCl, TlCl2-, TlCl32- respectively, k is the rate constant of the slow step and K1 is the equilibrium constant for, H4VO4+ + 2H+ ? V(OH)23+ + 2 H2O The main active species of vanadium(V) and thallium(I) are V(OH)23+ and TlCl32- respectively. The reaction constants involved in the mechanism are derived.

Osmium(VIII) mediated vanadium(V) oxidation of arsenic(III) in aqueous sulphuric acid

Osmium(VIII) mediated oxidation of As(III) by V(V) in aqueous sulphuric acid involves formation of an Os(VIII)-As(III) complex which intercts withV(V) resulting in a termolecular complex.The latter then yields As(V).The probable active species are discussed.