274317
A chemist wants to determine the molecular geometry of the $\left[\mathrm{CoCl}_{4}\right]^{2-}$ ion. Which of the following gives the best suggestion for a measurement and for the interpretation of that measurement?
1 Using aborption spectroscopy, measure $\lambda_{\max }$ calculate $\Delta_{0}$ for octahedral geometry.
2 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. If this number is low, geometry is likely to be square planar; otherwise, it is likely to be tetrahedral.
3 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molcule. If this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be square planar.
4 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. if this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be octahedral.
Explanation:
(B) : The complex ion is $\left[\mathrm{CoCl}_{4}\right]^{2-}$. The oxidation state of cobalt metal is +2 . $\mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}$ The square planar complex has one unpaired electron whereas tetrahedral compound has 3 unpaired electrons. Hence, it is the best method of determining of the molecular geometry of $\left[\mathrm{CoCl}_{4}\right]^{2-}$.
AIIMS-2009
COORDINATION COMPOUNDS
274319
Which complex of $\mathrm{Co}^{2+}$ will have the weakest crystal field splitting ?
274321
Potassium ferricyanide on ionization produces
1 2 ions
2 1 ions
3 3 ions
4 4 ions
Explanation:
(D) : The chemical formula of potassium ferricyanide is $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$. The ionization of the compound is given as - $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] \rightleftharpoons 3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}$ \(\begin{aligned} & \mathrm{K}_3\left[\mathrm{Fe}(\mathrm{CN})_6\right] \rightleftharpoons \begin{array}{l}\begin{array}{c}\text { Potassium } \\ \text { ferricyanide }\end{array}\end{array} \underbrace{3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}}_{4 \text { ions }}\end{aligned}\)
BCECE-2010
COORDINATION COMPOUNDS
274323
Which one of the following will give a white precipitate with $\mathrm{AgNO}_{3}$ in aqueous medium?
(D) : If the complex ionises the $\mathrm{Cl}^{-}$ion then they form the precipitate with $\mathrm{AgCl}$. In the given option, only option (d) ionises own $\mathrm{Cl}^{-}$ion. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2} \stackrel{2 \mathrm{AgNO}_{3}}{\longrightarrow}\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{NO}_{3}+\underset{\mathrm{PPt}}{2 \mathrm{AgCl}}$
274317
A chemist wants to determine the molecular geometry of the $\left[\mathrm{CoCl}_{4}\right]^{2-}$ ion. Which of the following gives the best suggestion for a measurement and for the interpretation of that measurement?
1 Using aborption spectroscopy, measure $\lambda_{\max }$ calculate $\Delta_{0}$ for octahedral geometry.
2 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. If this number is low, geometry is likely to be square planar; otherwise, it is likely to be tetrahedral.
3 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molcule. If this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be square planar.
4 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. if this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be octahedral.
Explanation:
(B) : The complex ion is $\left[\mathrm{CoCl}_{4}\right]^{2-}$. The oxidation state of cobalt metal is +2 . $\mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}$ The square planar complex has one unpaired electron whereas tetrahedral compound has 3 unpaired electrons. Hence, it is the best method of determining of the molecular geometry of $\left[\mathrm{CoCl}_{4}\right]^{2-}$.
AIIMS-2009
COORDINATION COMPOUNDS
274319
Which complex of $\mathrm{Co}^{2+}$ will have the weakest crystal field splitting ?
274321
Potassium ferricyanide on ionization produces
1 2 ions
2 1 ions
3 3 ions
4 4 ions
Explanation:
(D) : The chemical formula of potassium ferricyanide is $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$. The ionization of the compound is given as - $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] \rightleftharpoons 3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}$ \(\begin{aligned} & \mathrm{K}_3\left[\mathrm{Fe}(\mathrm{CN})_6\right] \rightleftharpoons \begin{array}{l}\begin{array}{c}\text { Potassium } \\ \text { ferricyanide }\end{array}\end{array} \underbrace{3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}}_{4 \text { ions }}\end{aligned}\)
BCECE-2010
COORDINATION COMPOUNDS
274323
Which one of the following will give a white precipitate with $\mathrm{AgNO}_{3}$ in aqueous medium?
(D) : If the complex ionises the $\mathrm{Cl}^{-}$ion then they form the precipitate with $\mathrm{AgCl}$. In the given option, only option (d) ionises own $\mathrm{Cl}^{-}$ion. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2} \stackrel{2 \mathrm{AgNO}_{3}}{\longrightarrow}\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{NO}_{3}+\underset{\mathrm{PPt}}{2 \mathrm{AgCl}}$
274317
A chemist wants to determine the molecular geometry of the $\left[\mathrm{CoCl}_{4}\right]^{2-}$ ion. Which of the following gives the best suggestion for a measurement and for the interpretation of that measurement?
1 Using aborption spectroscopy, measure $\lambda_{\max }$ calculate $\Delta_{0}$ for octahedral geometry.
2 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. If this number is low, geometry is likely to be square planar; otherwise, it is likely to be tetrahedral.
3 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molcule. If this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be square planar.
4 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. if this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be octahedral.
Explanation:
(B) : The complex ion is $\left[\mathrm{CoCl}_{4}\right]^{2-}$. The oxidation state of cobalt metal is +2 . $\mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}$ The square planar complex has one unpaired electron whereas tetrahedral compound has 3 unpaired electrons. Hence, it is the best method of determining of the molecular geometry of $\left[\mathrm{CoCl}_{4}\right]^{2-}$.
AIIMS-2009
COORDINATION COMPOUNDS
274319
Which complex of $\mathrm{Co}^{2+}$ will have the weakest crystal field splitting ?
274321
Potassium ferricyanide on ionization produces
1 2 ions
2 1 ions
3 3 ions
4 4 ions
Explanation:
(D) : The chemical formula of potassium ferricyanide is $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$. The ionization of the compound is given as - $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] \rightleftharpoons 3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}$ \(\begin{aligned} & \mathrm{K}_3\left[\mathrm{Fe}(\mathrm{CN})_6\right] \rightleftharpoons \begin{array}{l}\begin{array}{c}\text { Potassium } \\ \text { ferricyanide }\end{array}\end{array} \underbrace{3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}}_{4 \text { ions }}\end{aligned}\)
BCECE-2010
COORDINATION COMPOUNDS
274323
Which one of the following will give a white precipitate with $\mathrm{AgNO}_{3}$ in aqueous medium?
(D) : If the complex ionises the $\mathrm{Cl}^{-}$ion then they form the precipitate with $\mathrm{AgCl}$. In the given option, only option (d) ionises own $\mathrm{Cl}^{-}$ion. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2} \stackrel{2 \mathrm{AgNO}_{3}}{\longrightarrow}\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{NO}_{3}+\underset{\mathrm{PPt}}{2 \mathrm{AgCl}}$
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
COORDINATION COMPOUNDS
274317
A chemist wants to determine the molecular geometry of the $\left[\mathrm{CoCl}_{4}\right]^{2-}$ ion. Which of the following gives the best suggestion for a measurement and for the interpretation of that measurement?
1 Using aborption spectroscopy, measure $\lambda_{\max }$ calculate $\Delta_{0}$ for octahedral geometry.
2 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. If this number is low, geometry is likely to be square planar; otherwise, it is likely to be tetrahedral.
3 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molcule. If this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be square planar.
4 Measure the molecule's magnetic moment and use the result to estimate the number of unpaired spins in the molecule. if this number is low, the geometry is likely to be tetrahedral; otherwise, it is likely to be octahedral.
Explanation:
(B) : The complex ion is $\left[\mathrm{CoCl}_{4}\right]^{2-}$. The oxidation state of cobalt metal is +2 . $\mathrm{Co}^{2+}=[\mathrm{Ar}] 3 \mathrm{~d}^{7}$ The square planar complex has one unpaired electron whereas tetrahedral compound has 3 unpaired electrons. Hence, it is the best method of determining of the molecular geometry of $\left[\mathrm{CoCl}_{4}\right]^{2-}$.
AIIMS-2009
COORDINATION COMPOUNDS
274319
Which complex of $\mathrm{Co}^{2+}$ will have the weakest crystal field splitting ?
274321
Potassium ferricyanide on ionization produces
1 2 ions
2 1 ions
3 3 ions
4 4 ions
Explanation:
(D) : The chemical formula of potassium ferricyanide is $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]$. The ionization of the compound is given as - $\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right] \rightleftharpoons 3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}$ \(\begin{aligned} & \mathrm{K}_3\left[\mathrm{Fe}(\mathrm{CN})_6\right] \rightleftharpoons \begin{array}{l}\begin{array}{c}\text { Potassium } \\ \text { ferricyanide }\end{array}\end{array} \underbrace{3 \mathrm{~K}^{+}+\left[\mathrm{Fe}(\mathrm{CN})_6\right]^{3-}}_{4 \text { ions }}\end{aligned}\)
BCECE-2010
COORDINATION COMPOUNDS
274323
Which one of the following will give a white precipitate with $\mathrm{AgNO}_{3}$ in aqueous medium?
(D) : If the complex ionises the $\mathrm{Cl}^{-}$ion then they form the precipitate with $\mathrm{AgCl}$. In the given option, only option (d) ionises own $\mathrm{Cl}^{-}$ion. $\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2} \stackrel{2 \mathrm{AgNO}_{3}}{\longrightarrow}\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{NO}_{3}+\underset{\mathrm{PPt}}{2 \mathrm{AgCl}}$
