The molecular structures are shown below:
Effective atomic number for each molecule
1). Na[Fe(CN)3(NH3)3]
Oxidation state of Fe=
X + 3(-1) + 3(0) = -1
X= +2
Atomic number of Fe. = 26
No. Of electrons in Fe2+=24
Electrons from 3 CN-. =6
Electrons from 3 NH3. =6
EAN. = 36(EAN is obeyed)
2). [Cr(H2O)2(NH3)2(en)]Cl3
Oxidation state of Cr=
X +2(0)+2(0)+0=+3
X=+3
Atomic number of Cr. = 24
No. Of electrons in Cr3+. = 21
Electrons from 2 H2O. = 4
Electrons from 2 NH3. =4
Electrons from en. =4
EAN. = 35(EAN not obeyed)
3). [Co (o-phen)2(NH3)(NCS)]Cl
Oxidation state of Co=
X+0+2(0)+(-1)=+1
X=+2
Atomic number of Co =27
No. Of electrons in Co2+=25
Electrons from 2 o- phen =8
Electrons from NH3 =2
Electrons from NCS=2
EAN. = 37(EAN not obeyed)
4).[(n3-C3H5)Co (CO)2]
Oxidation state of Co = 0
Atomic number of Co= 27
No. Of electrons in Co = 27
Electrons from n3-C3H5=3
Electrons from 2CO =4
EAN. =34(EAN not obeyed)
5). [Fe(diphos)(CO)3]-
Oxidation state of Fe=
X=-1
Atomic number of Fe=26
No. Of electrons in Fe-1= 27
Electrons from diphos=4
Electrons from 3 CO= 6
EAN. = 37(EAN not obeyed)
B). Kf is the rate of formation.
It is said that kf is higher for [Fe(OH-]2- than for [Zn(OH-)4 and
[Cr(OH-)4]-
In each oxidation state is given as:
Fe =+2 3d6
Zn=+2 3d10
Cr=+3 3d3
OH- is a strong field ligand and cause pairing of electrons.
In cause of Zn pairing is impossible high spin complex is formed.
Cr3+ has only 3 electrons on 3d and hence pairing occurs easily.
Fe2+ requires more pairing energy hence Kf is greater.
C). Rotation alon CH2-CH2 bond is possible so as to cause all the Nitrogens in same plane to bind the Co.
For each of the following complexes, draw the molecular structure and determine the effective ato...
please do answer all the questions below. thank you For each of the following complexes, draw the molecular structure and determine the effective atomic numbers. (i) Na[Fe(CN)s(NH3)3l (i) [Cr(H2O)2(NH3)2(en)]Cl (ii) [Co(o-phen)2(NHs)(NCS))CI (iv) (n3-C3Hs)Co(CO)2] (v) [Fe(diphos)(CO)sl in which diphos Ph2PCH2CH2PPh2 and Ph CsHs (10 marks) (i)/ The K for Fe(OH)4]2-is found to be higher than that found in (5 marks) Zn(OH)4]2-and [Cr(OHM. Explain . Cho and coworkers used the following ligand to react with cobalt. Predict how this ligand would bind...
For each of the following complexes draw the structure, determine the electron count at the metal centre (use the neutral ligand method) and give the oxidation state of the metal (0) [Tan-CsHs)-(CH3)3] (11) [Ni(n-C3Hs)(PPh3>(CO)2] (111) [Mn(n-CHS)(CO)3]* [Ru(PMe3)2(CHPh)C12] (v) [Co(H2-COXCO);}2 Assume a direct Co-Co bond in (v) Explain, using suitable diagrams, the Berry pseudorotation mechanism
Part A (2 marks) In the following pairs of complexes, which do you expect to have a larger ligand field splitting parameter Ao? Why? Explain? i) [Fe(NH3)612+ or [Fe(NH3). 13+ ii) (Co(CN)613- or [Rh(CN)613- Part B (3 maks) In the following pairs of complexes, which do you expect to be more labile? Why? Explain? ) [Cr(NH3)613+ or [Mn(NH3)6]3+ ii) (Co(CN)613- or [Rh(CN)613- ii) [Cr(NH3).]3+ or [V(NH3).]2+
1. Determine the number of Infrared and Raman active bands for the following compounds. В С. A B с В (a) (b) 2. a) Build the molecular orbital energy diagram for the following molecules, O 2 ,02+ and O 2 -. b) Calculate the bond order for the three molecules, and justify which one is more stable. 3. How many unpaired electrons would you expect for the following complexes: [CoCle], [Cr(NHs)e]9 and [Cr(H2O)e3? 4. KMnO4 was expected to show no...
For each of the complexes, draw the structure and determine whether or not they obey the 18- electron rule. (1) (11) (111) (CpzCo] [Fe(n-C3Hs)(PMe3)2(CO)2]* [Fe(n'-C:Hs)(PMe3)2(THF)] CpRh(u2-H)2(CO)]2 [Mnz(CO)..] (v)
1. For each of the following complexes, give the electron configurations of the d-type M Os, for tetrahedral complexes. Also ie ) (e) for octahedral complexes and (e( ch complex in units of the Bohr , Fe(CN) 3, CoCl , Ni(CO)4, Ti(H2O) +, magnet n f.в Co ( NH3) 3+, Co(FLO)r", Fe(CN) V Fa". Cu(H2O) г., CuCl? , V(CO), Cr(CO) each octahedral complex is high-spi the ligand field theory notes). ust use your judgment as to whether n or low-spin...
1. Predict the molecular geometry of the following complexes, and determine whether each will be diamagnetic or paramagnetic: (a) [Fe(CN)614- (b) [Fe(C2O4)314- (C) [Zn(NH3)4]2+ (d) [Mo(CO)6] (e) [Rh(NH3)4]+
For each of the following transition metal complexes, determine the oxidation state of the metal, its coordination number, and the number of d electrons on that metal. (a) RuO4 (b) (CO(NH3).]3+ (c) [Cr(H2O).]8+ (d) Cr(H2O)3Cl2 (e) [Fe(H2O).]3+ (1) (Co(NH3).]2+ (9) MOCI (h) (Pt(CN)4]2- () [Mn(H2O).]2+ (1) Re(CO).Br (k) (Ag(CN 2] (1) [ReH9]?
2. Determine the oxidation state of the metal in each of the following coordination complexes: (a) Mn (CO). (b) [Re:Br2] ; (c) [Fe(H20).(OH)2]; (d) (CO(NH3),C1]
For each of the following metal complexes, specify the number of ligands, the coordination number of the metal, the oxidation number of the metal, the geometry of the complex and draw the structure. Transition metal complexes with four ligands usually form tetrahedral structures unless the metal has a d8 configuration, in which case it can form either tetrahedral or square planar structures. NH4[Co(NCS)4(py)2] [RhBr(CO)5](NO3)2 K4[Fe(CN)6] [HgI4]2- [Cu(NH3)4]Cl2