Coordination Compounds

The given question states that when 1 mol of CrCl3.6H2O is treated with excess AgNO3, 3 mol of AgCl is obtained. This implies that each CrCl3.6H2O unit reacts with 3 AgNO3 units to form 3 AgCl units. From this information, we can deduce that the complex must contain one Cr atom, as 1 mol of CrCl3.6H2O reacts to form 1 mol of Cr-containing complex. Additionally, since each CrCl3.6H2O unit contains 6 H2O molecules, the complex must also contain 6 H2O ligands. Therefore, the correct formula is [Cr(H2O)6]Cl3.

Diamagnetic substances are those that do not have any unpaired electrons and are not attracted to a magnetic field. In octahedral complexes, strong field ligands cause pairing of electrons in the d-orbitals, resulting in all electrons being paired and making the complex diamagnetic. Therefore, Co3+ in an octahedral complex with a strong field ligand is diamagnetic.

The given structure represents a carbonyl compound, with CO groups attached to a central metal atom Co. The number of CO groups on each side of the metal atom is represented by the value of n. In this case, the structure shows that there are 4 CO groups on each side of the metal atom, resulting in a value of n equal to 4.

The complex ion [Cr(H2O)4Cl2]+ shows geometrical isomerism. This is because the two chloride ligands can be either cis (on the same side) or trans (on opposite sides) to each other. This results in two possible isomers, cis-[Cr(H2O)4Cl2]+ and trans-[Cr(H2O)4Cl2]+, which have different spatial arrangements.

The complex compound [CuII(NH3)4][PtIICl4] consists of two parts: the copper complex [CuII(NH3)4] and the platinum complex [PtIICl4]. The copper complex contains a central copper ion surrounded by four ammonia ligands, while the platinum complex contains a central platinum ion surrounded by four chloride ligands. The number of possible isomers for each complex can be determined using the coordination number and geometries of the ligands. For the copper complex, the coordination number is 4 and the ligands are all the same, resulting in only one possible isomer. For the platinum complex, the coordination number is also 4, but the ligands are different, allowing for different possible arrangements. Therefore, the total number of possible isomers for the complex compound is 1 * number of isomers for the platinum complex, which is 4.

The compound [PtCl2P(C2H5)3]2 can exhibit geometrical isomerism because it contains a square planar coordination geometry around the platinum atom. In this compound, the two ethyl groups (C2H5) can be arranged either cis or trans to each other. This results in two different isomers with distinct spatial arrangements. The other compounds listed do not have the necessary structural features to exhibit geometrical isomerism.

The compounds [Co(SO4)(NH3)5]Br and [Co(SO4)(NH3)5]Cl do not represent any form of isomerism. Isomerism refers to the existence of different compounds with the same molecular formula but different structural arrangements or bonding patterns. In this case, both compounds have the same molecular formula and the same coordination sphere around the central cobalt ion. The only difference is the counterion, which is Br- in one compound and Cl- in the other. Since the coordination sphere and the overall structure of the compounds remain unchanged, there is no isomerism present.

The hybridization and shape of K3[Co(CO3)3] is sp3d2 and Octahedral. In this compound, the central cobalt atom is bonded to six ligands, three of which are carbonate ions (CO3) and three are potassium ions (K). The cobalt atom undergoes hybridization to form six hybrid orbitals, consisting of one s orbital, three p orbitals, and two d orbitals. These hybrid orbitals then overlap with the ligand orbitals to form six sigma bonds, resulting in an octahedral shape.

Square planar complexes have a square planar geometry, meaning that there are four ligands arranged around the central metal atom in a flat plane. In this case, the complex is MABXL, where A, B, X, and L are unidentate ligands. The two cis isomers refer to the arrangement of the ligands where two of them are located on the same side of the square plane, while the other two are on the opposite side. The trans isomer refers to the arrangement where two ligands are located opposite to each other across the square plane. Therefore, the correct answer is two cis and one trans isomer.

According to IUPAC nomenclature, the compound sodium nitroprusside is named as Sodium pentacyano nitrosylferrate (III). This name indicates the composition and oxidation state of the compound. "Sodium" refers to the presence of sodium ions, "pentacyano" indicates the presence of five cyanide ligands, "nitrosyl" indicates the presence of a nitrosyl ligand, and "ferrate (III)" indicates the oxidation state of iron in the compound.

The correct answer is "Good π-donor properties of Cl." In the spectrochemical series, the position of a ligand is determined by its ability to donate electron density to the metal center. Chlorine has good π-donor properties, meaning it can donate electron density to the metal through its p-orbitals. This makes it a strong ligand and places it above water in the spectrochemical series.

Monodentate ligands are ligands that can form only one bond with a metal ion. In the case of 2,4-Dinitrophenyl hydrazine, it can form a single bond with a metal ion through one of its functional groups. Therefore, it is classified as a monodentate ligand.

An octahedral complex refers to a coordination compound with six ligands surrounding the central metal ion, forming an octahedral shape. In the given options, the d8 (high spin) configuration is the only one that can form an octahedral complex. This is because d8 refers to a metal ion with eight d-electrons, which allows for the formation of six coordination bonds with ligands. The high spin configuration indicates that the electrons will occupy the available d-orbitals in a way that maximizes their spin, resulting in a high spin complex. Therefore, d8 (high spin) is the correct answer.

The correct answer is 1.15 Ǻ. In Fe(CO)5, the CO bond length will be slightly longer than the CO bond length in carbon monoxide alone. This is because the presence of the iron atom in Fe(CO)5 can slightly weaken the CO bond, causing it to stretch and increase in length. Therefore, the CO bond length in Fe(CO)5 is slightly longer than 1.128 Ǻ, but not as long as 1.72 Ǻ or 1.118 Ǻ. The closest option is 1.15 Ǻ, which is the correct answer.