A. The complex exhibits geometrical isomerism.
B. The complex is white in colour.
C. The calculated spin-only magnetic moment of the complex is 2.84 BM.
D. The calculated CFSE (Crystal Field Stabilization Energy) of Ni in this complex is $-0.8 \, \Delta_0$.
E. The geometrical arrangement of ligands in this complex is similar to that in $\text{Ni(CO)}_4$.
Choose the correct answer from the options given below :
To identify the incorrect statements about the complex $[\text{Ni}(\text{PPh}_3)_2\text{Cl}_2]$, we need to understand the properties and characteristics of the complex.
- Paramagnetic Nature: The given complex is paramagnetic, indicating the presence of unpaired electrons.
- Electronic Configuration of Ni: For Ni (Nickel), the outer electronic configuration in the +2 oxidation state is \(3d^8 \, 4s^0\). The two electrons are removed from the 4s and one 3d, leading to eight 3d electrons.
- Geometrical Isomerism (Statement A): The complex can exhibit geometrical isomerism due to the different arrangements of ligands (two triphenylphosphine \((\text{PPh}_3)\) and two chloride ions (Cl−)) around the central metal ion.
- Colour of the Complex (Statement B): Coordination complexes of Ni2+ usually are colored. However, the related phosphine complexes are less intensely colored, often appearing pale yellow or off-white.
- Spin-only Magnetic Moment (Statement C): The spin-only magnetic moment can be calculated using the formula \(\mu_s = \sqrt{n(n+2)} \, \text{BM}\), where \(n\) is the number of unpaired electrons. In this case, having two unpaired electrons would lead to: \(\mu_s = \sqrt{2(2+2)} = 2.83 \, \text{BM}\).
- Crystal Field Stabilization Energy (Statement D): CFSE for a d8 system in an octahedral field is usually different from the given value of \(-0.8 \Delta_0\).
- Geometrical Arrangement (Statement E): $[\text{Ni}(\text{PPh}_3)_2\text{Cl}_2]$ is a square planar complex, whereas $\text{Ni(CO)}_4$ is tetrahedral. Therefore, their geometrical arrangements differ.
Based on this analysis, the incorrect statements are C, D, and E.
Similar Questions
- A 'p'-block element (E) and hydrogen form a binary cation $(\text{EH}_x)^+$, while $\text{EH}_3$ on treatment with $\text{K}_2\text{HgI}_4$ in alkaline medium gives a precipitate of basic mercury(II)amido-iodine. Given below are first ionisation enthalpy values ($\text{kJ mol}^{-1}$) for first element each from group 13, 14, 15 and 16. Identify the correct first ionisation enthalpy value for element E.
- Given below are two statements :
Statement I : The first ionization enthalpy of Cr is lower than that of Mn.
Statement II : The second and third ionization enthalpies of Cr are higher than those of Mn.
In the light of the above statements, choose the correct answer from the options given below : - Among $\text{H}_2\text{S, H}_2\text{O, NF}_3, \text{NH}_3 \text{ and CHCl}_3$, identify the molecule (X) with lowest dipole moment value. The number of lone pairs of electrons present on the central atom of the molecule (X) is :
- Given below are two statements :
Statement I : Elements 'X' and 'Y' are the most and least electronegative elements, respectively among N, As, Sb and P. The nature of the oxides $\text{X}_2\text{O}_3$ and $\text{Y}_2\text{O}_3$ is acidic and amphoteric, respectively.
Statement II : $\text{BCl}_3$ is covalent in nature and gets hydrolysed in water. It produces $[\text{B(OH)}_4]^-$ and $[\text{B(H}_2\text{O)}_6]^{3+}$ in aqueous medium.
In the light of the above statements, choose the correct answer from the options given below : Given below are two statements :
Statement I : $\text{C} < \text{O} < \text{N} < \text{F}$ is the correct order in terms of first ionization enthalpy values.
Statement II : $\text{S} > \text{Se} > \text{Te} > \text{Po} > \text{O}$ is the correct order in terms of the magnitude of electron gain enthalpy values.
In the light of the above statements, choose the correct answer from the options given below :- If the enthalpy of sublimation of Li is $155 \text{ kJ mol}^{-1}$, enthalpy of dissociation of $\text{F}_2$ is $150 \text{ kJ mol}^{-1}$, ionization enthalpy of Li is $520 \text{ kJ mol}^{-1}$, electron gain enthalpy of F is $-313 \text{ kJ mol}^{-1}$, standard enthalpy of formation of LiF is $-594 \text{ kJ mol}^{-1}$. The magnitude of lattice enthalpy of LiF is _________ $\text{kJ mol}^{-1}$. (Nearest Integer)
- Among the following oxides of 3d elements, the number of mixed oxides are _________.
$\text{Ti}_2\text{O}_3, \text{V}_2\text{O}_4, \text{Cr}_2\text{O}_3, \text{Mn}_3\text{O}_4, \text{Fe}_3\text{O}_4, \text{Fe}_2\text{O}_3, \text{Co}_3\text{O}_4$ - Consider three metal chlorides x, y and z, where x is water soluble at room temperature, y is sparingly soluble in water at room temperature and z is soluble in hot water. x, y and z are respectively
- In the Group analysis of cations, $\text{Ba}^{2+}$ & $\text{Ca}^{2+}$ are precipitated respectively as
- "X" is an oxoanion of the lightest element of group 7 (in the periodic table). The metal is in +6 oxidation state in "X". The color of the potassium salt of X is
Important Questions from Inorganic Chemistry
- A 'p'-block element (E) and hydrogen form a binary cation $(\text{EH}_x)^+$, while $\text{EH}_3$ on treatment with $\text{K}_2\text{HgI}_4$ in alkaline medium gives a precipitate of basic mercury(II)amido-iodine. Given below are first ionisation enthalpy values ($\text{kJ mol}^{-1}$) for first element each from group 13, 14, 15 and 16. Identify the correct first ionisation enthalpy value for element E.
- Given below are two statements :
Statement I : The first ionization enthalpy of Cr is lower than that of Mn.
Statement II : The second and third ionization enthalpies of Cr are higher than those of Mn.
In the light of the above statements, choose the correct answer from the options given below : - Among $\text{H}_2\text{S, H}_2\text{O, NF}_3, \text{NH}_3 \text{ and CHCl}_3$, identify the molecule (X) with lowest dipole moment value. The number of lone pairs of electrons present on the central atom of the molecule (X) is :
- Given below are two statements :
Statement I : Elements 'X' and 'Y' are the most and least electronegative elements, respectively among N, As, Sb and P. The nature of the oxides $\text{X}_2\text{O}_3$ and $\text{Y}_2\text{O}_3$ is acidic and amphoteric, respectively.
Statement II : $\text{BCl}_3$ is covalent in nature and gets hydrolysed in water. It produces $[\text{B(OH)}_4]^-$ and $[\text{B(H}_2\text{O)}_6]^{3+}$ in aqueous medium.
In the light of the above statements, choose the correct answer from the options given below : Given below are two statements :
Statement I : $\text{C} < \text{O} < \text{N} < \text{F}$ is the correct order in terms of first ionization enthalpy values.
Statement II : $\text{S} > \text{Se} > \text{Te} > \text{Po} > \text{O}$ is the correct order in terms of the magnitude of electron gain enthalpy values.
In the light of the above statements, choose the correct answer from the options given below :
