Draw a d orbital scheme for [Fe(CN)4]3-?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Draw the d orbital electron diagrams for the following complexes. Ni(OH2), [Cr(CN))
4. Draw an MO diagram for CN- including: a. The irreducible representations describing each basis orbital. b. The relative energies of the basis orbitals. c. The relative energies of the product orbitals. d. The irreducible representations describing each product molecular orbital. e. The electron occupancy of each product molecular orbital.
3. When Clz(9) is added to aqueous Ke[Fe(CN).), [Fe(CN).]*- is oxidized to [Fe(CN).jº-and Kz[Fe(CN).] precipitates, as shown below. 2K [Fe(CN)6] (aq) +C12(g) = 2K [Fe(CN).](s) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C: [Fe(CN)6]3-(aq) + [Fe(CN)6]+-(aq) E° = 0.356 V Cl2(g) + 2e + 2Cl(aq) E° = 1.360 V Ksp of K3[Fe(CN)6] = 106.5
3. When C12(g) is added to aqueous K4[Fe(CN).), [Fe(CN)]*- is oxidized to [Fe(CN).]>- and K:[Fe(CN)] precipitates, as shown below. 2K.[Fe(CN),](aq) +Cl2(g) = 2Ks[Fe(CN)2](3) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant. (10 pts) At 25°C [Fe(CN).J” (aq) + € → [Fe(CN).]" (aq) E = 0.356 V Cl2(g) + 2e → 2Cl(aq) E* = 1.360 V Kup of Kj[Fe(CN).] = 106.5 Answer: b. When 80.0 mL of 1.00 M KCN is added to...
3. When Cl2(g) is added to aqueous K [Fe(CN)6], [Fe(CN).]*- is oxidized to [Fe(CN).]}-and K [Fe(CN)6] precipitates, as shown below. 2K [Fe(CN).] (aq) + Cl2(g) = 2K3[Fe(CN).J(8) + 2Cl(aq) a. Write the net ionic equation for the reaction and calculate its equilibrium constant (10 pts) At 25°C: [Fe(CN).]" (aq) + e[Fe(CN).]" (aq) E° = 0.356 V Cl2(9) + 2e → 2Cl(aq) E° = 1.360 V Ksp of K3 [Fe(CN)6] = 106.5 b. When 80.0 mL of 1.00 M KCN is...
6) In both [Fe(H20).]** and [Fe(CN)61* ions, the iron is present as Fe(11); however, [Fe(H20)6]** is paramagnetic, whereas [Fe(CN)6] is diamagnetic. Please write the electronic configuration of d-orbital for these two complexes and explain this difference. (8 marks) Fe2+ = 15² 25² 2p% 35² 306 45 306 act 6 = -a 30-446
How many d-electrons does the iron have in the [Fe(CN)_6]^3- complex? A. 3 B. 4 C. 5 D. 6
Give the balanced redox reaction between GLUCOSE and ferricyanide in a BASIC solution. Fe(CN)_6^(3–)+ e^-→Fe(CN)_6^(4-)
Give the balanced redox reaction between glucose and ferricyanide in a basic solution. Fe(CN)_6^(3–)+ e^-→Fe(CN)_6^(4-)
Please help Is an outersphere mechanism likely for the cross reaction of [Fe(CN)6]-3/-4 and [Mo(CN8)]-3/-4 with a k11=6.3x102 and k22=3x104 k12=3.0x104 [Fe(CN)6]-3 + [Mo(CN8)]-4 --> [Fe(CN)6]-4 + [Mo(CN8)]-3