CompoundCis - [Co(NH,),CI,JTrans - [Co(NH),CI]Fac - [Co(NH),CI]Mer - [Co(NH,),Cl,Cis-[Co(en) Cl]+ (Remember,because en is a bidentate ligand itcounts as two ligands each)Trans-[Co(en),C₁₂]*Cis-SCI₂FTrans-SCIFFac-[RhCI,(pyr),]Mer - [RhCI, (pyr),]Fac - [Co(NH,),(H,O),Mer - [Co(NH,),(H,O),Drawing

Step 1:Cis-[Co(NH3)4Cl2] Step 2:Trans-[Co(NH3)4Cl2] Step 3:Fac-[Co(NH3)3Cl3]Step…

Answered: Compound Cis - [Co(NH,),CI,J Trans -…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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What is the transition metal-containing product for the following reaction, where [Rh(CO)Br3]2- is a square-planar complex? [Rh(CO)Br3]2- + CO(g) --> ? Group of answer choices [RhBr4]3- an equal mixture of cis- and trans-[Rh(CO)2Br2]- trans-[Rh(CO)2Br2]- cis-[Rh(CO)2Br2]-
The complex trans-[Co(en)2Cl2]+ undergoes substitution of Cl- by H2O slower than the complex trans-[Co(en)2Cl2]. explain the reason for the difference
Possible geometry of complex (Co(NH3) Cl(en) 2)Cl2
4. For each of the following transition metal complex ions (a) [FeBr2(OH)(NO3)]¹- (b) [RhF3(SCN)3]4- (c) [TiBr4]³- (i) Draw the structure of the transition metal complex ion. Show the charge on the complex in your structure. Give the oxidation state of the metal. State whether the complex is high spin or low spin or not applicable. Provide reasons for your answer. (iv) Draw the arrangement of d-electrons in the ground state. Label the orbital sets. (v) Calculate the LFSE (in units of Ao or AT) for each complex. (ii) (iii)
Answer the following questions about the following coordination complex: [Co(en)2Cl2]Cl a) Provide the charge and electron configuration for the central metal ion and explicitly state its d-electron count. b) What is the coordination number of the complex ion in this coordination complex? c) What is the geometry of the complex ion? d) If this were a high-spin complex, how many unpaired electrons would be present? What if this complex were low-spin? Which (if any) of these two configurations would be paramagnetic?
Drawing an isomer of a metal complex Here is an isomer of the [FeBr₂Cl₂ (OH)]³ complex: OH Cl Cl 3- Br Fe Cl Br Draw another isomer below. []¯ ☑
Considering Br as a weak field ligand , the number of unpaired electrons in [Co(Br))6]2- will be (Atomic number Co= 27)
For the following complex, give the electron count and oxidation state for the metal, include all the steps (MLIXxZz, VN, LBN, EN, dh, OS). H- H COI CO Cr CO CO
The complex (Fe(H,O)]* is paramagnetic. Is the H,0 ligand inducing a strong or weak field?
COBALT COMPLEX: [CoCl4]2-(aq) + 6H2O(l) « [Co(H2O)6]2+(aq) + 4Cl-(aq) + Heat Blue Pink STEPS #- Solutions Observations 1-DISSOLVE COBALT COMPLEX PINK SOLUTION 2-SOLUTION PLUS HCl BLUE SOLUTION 3-ADD WATER PINK SOLUTION 4-HEAT SOLUTION BLUE SOLUTION According to the equilibrium equation, which ion(s) do you have when the solution dissolved? Explain how you know the identity of the ion(s) present. 2. Explain what happened when the HCl was added to the solution. 3. Explain what happened when the H2O was added to the solution. 4. Explain what happened when the solution was heated. Was the reaction exothermic or endothermic?
The DOTA ligand is a cyclic octadentate ligand with four N- donors and four O-donors. * True O False
1. Determine whether the following complexes are low spin or high spin complex (i) (ii) [Co(CN)G]* [CoF6]3- To support you answer, draw the electrons arrangement at t2g and eg sub-orbitals. Explain further why the complexes exhibit different electron arrangements.

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