1) Before naming the complex compound we have to go through following instructions.
A) Cation should be named before anion.
B) Ligand should be named before metal ion in alphabetical order.
C) for anionic ligands which ends with ite, ate etc then replace it with ito,ato respectively.
D) number of each type of ligand is representated by mono, di , tri , etc or bis, tris, etc.
E) after naming of ligand is completed, naming of central metal atom starts. For cationic complex ion , name of central metal will be same as the element. Ex- Ni is known as nickel.
For anionic complex ion, name of the central metal ends with suffix ate. Ex - Cu is Known as cuperate.
For determination of oxidation number some rules should be kept in mind-
1) an element which is free in state has a 0 oxidation number
2) oxidation state of group 1 is +1 whereas group 2 has +2 oxidation state. Group 17 has -1 oxidation state if the element is in binary compound.
Let's take an example of Ni(Co) 4
Let Ni be x
We know that oxidation state of CO is 0
Therefore x+4× 0 = 0
Keeping in mind the above given rules :::
1a)[Ni(CN)4] -2
Name of the compound is tetracyanonickelate (II) and oxidation state is --> let Ni be x
Since oxidation number of -CN is -1
x + 4 × -1 = -2==>> x= +2
1)b) [ Co(Cl4)] -2
Name of the compound is tetrachlorocobaltate (II) and oxidation number is - let Co be x
Oxidation number of Cl is -1
x + 4 × -1 = -2
x = 2
1)c) [Mn(NH3)6] +2
Name of the compound is hexaamminemanganese (II)
Since NH3 has neutral oxidation state therefore
Oxidation state = x+0= 2
Therefore oxidation state of Mn is +2
# as per HomeworkLib guidelines I am supposed to answer only first question so plz post them separately
(1) Name the following complexes and determine the oxidation number of central metal atoms (9 points)...
(1) Name the following complexes and determine the oxidation number of central metal atoms (9 points) (a) [Ni(CN).] (b) [Co(Cl)] (c) [Mn(NH)]
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]?
Calculate the (a) oxidation state of the metal and (b) the coordination number. Which of the following complexes has the highest value of the sum, a +b. The spectrochemical series is i <Br" <CI <F <OH <H20 < NH; <en< NO, <CN Select one: A. Two of complexes have the same highest value of the sum, a +b. B. Na[Cr(NH3),C13] C. [Ni(H20),(NO2)2] D. [Co(en) CICI E.K_[Cu(CN),
6 Identify the coordination number (C.N.), metal oxidation state(O.S.) and the number of metal d electrons for each of the following complexes. (a) [Ni(CN):) C.N. = _ ; O.S. = __, d-electrons = d-electrons = (b) [Pd(Cl)]2 C.N. = _ ; O.S. = ___, d-electrons = (c) [Cr(CN)]C.N. =__; O.S. = —, (d) [Fe(CO).]? C.N. = __; O.S. = ___, d-electrons =- (e) [Cr(CI):]& C.N. = ___; O.S. = __, d-electrons = (1) [Ag(CN)2] C.N. = ___; O.S. = ___,...
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]
6 Identify the coordination number (C.N.), metal oxidation state(O.S.) and the number of metal d electrons for each of the following complexes. (a) [Ni(CN)s] C.N. = __;0.S. = ___, d-electrons = (b) (Pd(C1).]C.N. = ____; O.S. - ___, d-electrons = (c) (Cr(CN)] C.N. - ___.O.S. = ___, d-electrons = (d) [Fe(CO).)? C.N. = ___; O.S. = ___, d-electrons = (e) (Cr(Cl)s) C.N. = ____ ; O.S. = ____ d-electrons =_ (1) (Ag(CN)2] C.N. = _ ; O.S. = _ ,...
What is the coordination number for each of the following complexes or compounds? [Co(NH3)4Cl2]+ [Ca(EDTA)]2− [Pt(NH3)4]2+ Na[Ag(CN)2] Enter the coordination numbers, in the order that the complexes are listed, as four integers separated by commas (e.g., 1,2,3,4). What is the charge on each of the following complex ions? hexaaquairon(II), [Fe(H2O)6]? tris(carbonato)aluminate(III), [Al(CO3)3]? amminepentachloroplatinate(IV), [Pt(NH3)Cl5]? Express the charges numerically, in the order that the complexes are listed, separated by commas. For a nonzero charge, be sure to include the sign (e.g.,...
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
can anyone confirm my answers for all of 2 and all of 4? 1. Name following coordination complexes. (a) K][PdC1] (b) [Co(H2O),(NH3)4]2+ (b) [Mn(NH3),(En)]2+ (c) [CrCl,(NH3)4]CI, 2. State the coordination number and oxidation state of the following catalysts. (a) [Pt(CO) PPhz] (b) [Ni(C1).]2- (c) [Ir(Cl) (CO)En(PPhz)2]3+ (d)Liz[AuClo] 3. Define the following. (a) Ligand (b) Coordination number (c) Polydentate ligand (d) Primary valency 4. Write the formula of following coordination complexes. (a) Tris(ethylenediammine)cobalt(III) nitrate (b) Hexacyanomolybdate(II) (c) Tetrahydroxocuprate(II) (d) Sodium dibromidodichloridonickelate
Enter the coordination number for the transition metal in each compound. Note: Due to requirements to build this question, the complex ion is enclosed in { } rather than square brackets. K{Fe(H2O)2(ox)2} {Co(H2O)4(CN)2}Cl {Mn(NH3)4}Br2 {Ni(acac)2} {Cu(NH3)2}2SO4 Ca{MnEDTA}