Explain why FeSO4 is a high spin compound, whereas K4[Fe(CN)6] and K3[Fe(CN)6] are low spin.
Explain why FeSO4 is a high spin compound, whereas K4[Fe(CN)6] and K3[Fe(CN)6] are low spin.
A solution is prepared by adding 0.075 mole of K3 [Fe(CN)6] to 0.72 L of 2.2 M NaCN. Assuming no volume change, calculate the concentrations of Fe(CN)63- and Fe3+ in this solution. The K (overall) for the formation of Fe(CN)63- is 1.0 x 1042. [Fe(CN)6*] = [Fe3+] = Submit Answer Try Another Version 2 item attempts remaining
A solution is prepared by adding 0.063 mole of K3 [Fe(CN)6] to 0.59 L of 2.1 M NaCN. Assuming no volume change, calculate the concentrations of Fe(CN)63- and Fe3+ in this solution. The K (overall) for the formation of Fe(CN)63- is 1.0 x 1042. M [Fe(CN)6*] = C [Fe3+]= C M Submit Anchor Another Voreion 2 itom attomnte romaining
Consider the coordination compound Caz[Co(CN)6]: i. ii. Give the systematic name of the compound. What is the magnetic property of the complex (diamagnetic, strong or weakly paramagnetic)? (Use the appropriate d-orbital splitting diagram from the formula sheet to explain your answer) iii. Will the complex be a high-spin or low-spin complex?
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...
for each metal, indicate the high spin, low spin, or doesn't matter, and give the number of unpaired electrons. a). [Mn(CN)6]4- b). [FeCl4]2- c). [Co(OH2)6]3+ d). [ReO4]- e). [Ti(OH2)6]3+
Name the coordination compounds 1. [CO(NH3)6]C12 2. [CO(NH3)5Cl]012 3. [Co(H20).]Br3 4. K3[Fe(CN)6] 5. K3[CoF6]. 6. Na4[PtClo]
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
Calculate the ionic strength of a solution that is 0.040 mol kg-1 in K3[Fe(CN)6] (aq), 0.030 mol kg-1 in KCl (aq), and 0.050 mol kg-1 in NaBr (aq)
Question 2 5 pts The octahedral complex hexacyanoferrate(III) ion, [Fe(CN).l, is a low-spin complex. How many unpaired electrons does the complex have? OS OO 03 04 O1
The E? values for two low-spin iron complexes in acidic solution are as follows: [Fe(o?phen)3]3+(aq)+e? ?[Fe(o?phen)3]2+(aq) E?=1.12V [Fe(CN)6]3?(aq)+e? ?[Fe(CN)6]4?(aq) E?=0.36V Part A Which complex is more difficult to reduce? [Fe(o-phen)3]3+ [Fe(CN)6]3? PArt B Is it thermodynamically favorable to reduce both Fe(III) complexes to their Fe(II) analogs? yes no