Explanation
Ni(CO)4 is diamagnetic, all others are paramagnetic.
[Ag(NH3)2] Cl contains Ag+ in d10 configuration which is diamagnetic, all others are paramagnetic.
In [Fe(H2O)6]2+ ,Fe2+ with 3d6 configuration having 4 unpaired electrons shows maximum paramagnetism.
By mixing equimolar amounts of CuSO4 and (NH4)2SO4.[Cu(NH3)4]SO4 is formed
IUPAC name is potassium trioxalatoaluminate (III)
It is optically active when two Cl atoms are in cis position.
[Cu(NH3)4]2+
Na2[Fe(CN)5NO] is sodium nitroprusside.
K3[Cr(C2O4)3] contains Cr in + 3 oxidation state and its C.N. is 6.
Mn2+ will have half filled more stable d5 configuration and without disturbing it an outer orbital complex can be formed.
It is called potassiumhexacyanoferrate (II)
No. of sigma bonds is 19 and pi bonds is 11. Each CN contains 1 sigma and two pi bonds, so also each CO group.
[NiCl4]2- is paramagnetic due to two unpaired electrons.
Dichlorobis (urea) copper (II) is [CuCl2{O = C (NH2)2}2].
[Ni(CN)4]2- is square planar
In [Fe(CN)6]4- EAN of Fe = 26 - 2 + 6 ×2 = 36
In Na2[CdCl4],Cd2+ contains 4d10 configuration and is colourless.
Magnetic moment corresponding to Fe2+ ion 3d6 with d2sp3 hybridization will be zero and it will be diamagnetic.
[Cr(H2O)6]3+ contains 3 unpaired electrons wheras [Fe(CN)6]4- contains zero unpaired electron. All other complexes have one unpaired electron each.
This is the correct IUPAC name.
AgCl + 2 NH4OH →[Ag(NH3)2]Cl+ 2H2O.
[Ni(CN)4]2- shows dsp2 hybridization.
Both Ni(CO)4 and Ni(PPh3)2 Cl2 will be tetrahedral.
In Fe (CO)5, Fe is in zero oxidation state.
In Fe(CO)5, Fe atom is dsp3 hybridized giving a trigonal bipyramidal structure.
The complex compound [Co(en)2Cl2] Br shows ionization isomerism, cis-and trans-isomerism and optical isomerism.
According to Werner’s theory of complexes, primary valency is ionizable.
Brown ring test for nitrate is due to the complex [Fe(H2O)5NO]2+.
When an octahedral complex contains all the three bidentate ligands, it shows optical isomerism.
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