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- At 580 nm, which is the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00 I03L cm-1 mol-1.Calculate (a) the absorbance of a 4.47 10-5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of a solution in a 2.50-cm cell in which the concentration of the complex is one half that in(a). (c) the percent transmittance of the solutions described in (a) and (b). (d) the absorbance of a solution that has half the transmittance of that described in (a).Zinc(II) and the ligand L form a 1:1 complex that absorbs strongly at 600 nm. As long as the molar concentration of L exceeds that of zinc(II) by a factor of 5, the absorbance depends only on the cation concentration. Neither zinc(II) nor L absorbs at 600 nm. A solution that is 1.59 10-4 M in zinc(II) and 1.00 10-3 M in L has an absorbance of 0.352 in a 1.00-cm cell at 600 nm. Calculate (a) the percent transmittance of this solution. (b) the percent transmittance of this solution in a 2.50-cm cell. (c) the molar absorptivity of the complex..A. w: Mn= 25, Co= 27, Ni= 28, Zn= 30 ------------ Complex K3[Mn(C204)3] Highly distorted. O Low distorted. O not distorted. O The magnetic moment of the -------------- complex [Ni(en)3]CI2 is * 0Bm 2.8 BM 1.8 BM O OO0O0 3.8 BM
- The molar absorptivity (ε) of the FeSCN2+ complex ion is 4700 M-1 · cm-1 at a wavelength of 450 nm. Using a 1-cm sample tube, you measure the absorbance as (2.0x10-1). What is the concentration of FeSCN2+?The molar absorptivity (ε) of the FeSCN2+ complex ion is 4700 M-1 · cm-1 at a wavelength of 450 nm. Using a 1-cm sample tube, you measure the absorbance as (2.0x10-1). What is the concentration of FeSCN2+? What is your answer? _____________x10^_____Consider the octahedral complex [FeBr6] 4−. In water solution it has an absorption peak at 864 nm with a molar absorptivity (ε) of 3.6 L mol-1 cm-1 . (I have a, b, and c, I need help with d, e, and f.) (a) What is the energy (in wavenumbers, cm-1 ) of the absorption peak? Show all work. (b) How many valence d electrons does the metal center have? Justify your answer. (c) How many unpaired electrons per molecule would a magnetic susceptibility experiment predict? What would the S number be for this transition metal center? Justify your answers. (d) What electronic transition results from absorption of 864-nm light? (e) Calculate the ligand stabilization energy (in units of ∆o) and units of coulombic (Πc) energy. (f) How would the ligand field strengths (∆o) of [Fe(NH3)6] 2+ and [Fe(bipy)3] 2+ differ from that of [FeBr6] 4−? Why?
- The absorption coefficient of a glycogen-iodine complex is 0.20 at light of 450 nm. What is the concentration when the transmission is 40 % in a cuvette of 2 cm?8. a. The value of molar absorptivity constant (e) for a colored substance is 35,000 M -1 cm-1 at 473 nm and the curvette is 1.00 cm. Determine the range of concentration possible if absorbance can be measured from 0.050 to 0.95. b. Calculate the concentration for the following values of absorbance for the colored substance above. A= 0.27 A=0.54The experimental magnetic moment of Na2CoCl4 is 4.59 BM. The difference of theexperimental and the spin only magnetic moment values can be explained by(a) Jahn-Teller distortion(b) Mixing of tetrahedral and square planar complexes(c) Mixing of ground state with first excited state(d) Mixing of tetrahedral and octahedral complexes
- calculat dlta E for each complex Trans complex : G= 355 microsiemens λ= 450 nm Cis complex : G=250 microsiemens λ=500 nm.A student is working with a metal thiocyanate complex, M(SCN)+, with a molar absorptivity constant, ε, of 6500 cm−1M−1 at 500 nm. If the student is using a 1.00 cm cuvette for absorbance measurements at 500 nm, what concentration of M(SCN)+ will give an absorbance value of 0.120? [M(SCN)+]=Describe the IR active symmetric and asymmetric Pt-Cl stretching vibrations for cis-[Pt(NH3)2Cl2] ans trans-[Pt(NH3)2Cl2]complexes. ???
