274271
Which of the following carbonyls will have the strongest $\mathrm{C}-\mathrm{O}$ bond?
1 $\mathrm{Mn}(\mathrm{CO})_{6}^{+}$
2 $\mathrm{Cr}(\mathrm{CO})_{6}$
3 $\mathrm{V}(\mathrm{CO})_{6}^{-}$
4 $\mathrm{Fe}(\mathrm{CO})_{5}$
Explanation:
(A) : When electron density on metal is high then tendency of back bonding is also high. Due to backbonding lone pair of electron from filled metal orbital is donated to empty antibonding $\left(\pi^{*}\right)$ orbital of $\mathrm{CO}$ lignad. So, bond strength of $\mathrm{C}-\mathrm{O}$ decrease and bond length increase. Hence, $\left[\mathrm{Mn}(\mathrm{CO})_{6}\right]^{+}$has strength $\mathrm{C}-\mathrm{O}$ bond because metal has low electron density due to which backbonding tendency decreases.
AIPMT -2011)
COORDINATION COMPOUNDS
274275
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the d orbits that undergo increase in energy are
(C) : In octahedral symmetry the -orbitals split into two sets with an energy difference, where the $\mathrm{d}_{\mathrm{xy}}, \mathrm{d}_{\mathrm{yz}}$, dzx orbitals will be lower in energy than the $d_{x^{2}-y^{2}}, d_{z^{2}}$ which will have higher energy because the former group is farther from the ligands than the latter therefore experience less repletion.
AP EAPCET-12.07.2022
COORDINATION COMPOUNDS
274281
The correct order for wavelengths of light absorbed in the complex ions $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}$, $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ and $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$ is
(A) : The absorption of light in the complex ions depends upon the nature of metal, oxidation number and ligand (spectrochemical series). The compounds have the same metal as well as same oxidation state but different in ligands. Weak field ligands (WFL) have the lower energy gap between $t_{2 g}$ and $e_{g}$ orbital. So, low amount of energy required and high wavelength of light used for absorption. Hence the correct order of wavelength of light absorbed are that $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}>\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}>\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$
Kerala-CEE-29.08.2021]**
COORDINATION COMPOUNDS
274283
Accordingly to the crystal field theory, for an octahedral field, the energy of two $e_{g}$ ordinals will be increased by
1 $\left(\frac{1}{5}\right) \Delta_{0}$
2 $\left(\frac{2}{5}\right) \Delta_{0}$
3 $\left(\frac{3}{5}\right) \Delta_{0}$
4 $\left(\frac{4}{5}\right) \Delta_{0}$
Explanation:
(C) : According to the crystal field theory for octahedral field the energy levels of $\mathrm{e}_{\mathrm{g}}$ are higher, $0.6 \Delta_{\mathrm{o}}$ or $\left(\frac{3}{5}\right) \Delta_{\mathrm{o}}$ while $\mathrm{t}_{2 \mathrm{~g}}$ is lower $0.4 \Delta_{\mathrm{o}}$. or $\left(\frac{2}{5}\right) \Delta_{\mathrm{o}}$
TS EAMCET 10.08.2021
COORDINATION COMPOUNDS
274291
The theory that can completely/properly explain the nature of bonding in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is:
1 Werner's theory
2 Crystal field theory
3 Valence bond theory
4 Molecular orbital theory
Explanation:
(D) : $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is a tetrahedral complex in which bonding in complex properly explain by the 'Molecular orbital theory' (MOT).
274271
Which of the following carbonyls will have the strongest $\mathrm{C}-\mathrm{O}$ bond?
1 $\mathrm{Mn}(\mathrm{CO})_{6}^{+}$
2 $\mathrm{Cr}(\mathrm{CO})_{6}$
3 $\mathrm{V}(\mathrm{CO})_{6}^{-}$
4 $\mathrm{Fe}(\mathrm{CO})_{5}$
Explanation:
(A) : When electron density on metal is high then tendency of back bonding is also high. Due to backbonding lone pair of electron from filled metal orbital is donated to empty antibonding $\left(\pi^{*}\right)$ orbital of $\mathrm{CO}$ lignad. So, bond strength of $\mathrm{C}-\mathrm{O}$ decrease and bond length increase. Hence, $\left[\mathrm{Mn}(\mathrm{CO})_{6}\right]^{+}$has strength $\mathrm{C}-\mathrm{O}$ bond because metal has low electron density due to which backbonding tendency decreases.
AIPMT -2011)
COORDINATION COMPOUNDS
274275
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the d orbits that undergo increase in energy are
(C) : In octahedral symmetry the -orbitals split into two sets with an energy difference, where the $\mathrm{d}_{\mathrm{xy}}, \mathrm{d}_{\mathrm{yz}}$, dzx orbitals will be lower in energy than the $d_{x^{2}-y^{2}}, d_{z^{2}}$ which will have higher energy because the former group is farther from the ligands than the latter therefore experience less repletion.
AP EAPCET-12.07.2022
COORDINATION COMPOUNDS
274281
The correct order for wavelengths of light absorbed in the complex ions $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}$, $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ and $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$ is
(A) : The absorption of light in the complex ions depends upon the nature of metal, oxidation number and ligand (spectrochemical series). The compounds have the same metal as well as same oxidation state but different in ligands. Weak field ligands (WFL) have the lower energy gap between $t_{2 g}$ and $e_{g}$ orbital. So, low amount of energy required and high wavelength of light used for absorption. Hence the correct order of wavelength of light absorbed are that $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}>\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}>\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$
Kerala-CEE-29.08.2021]**
COORDINATION COMPOUNDS
274283
Accordingly to the crystal field theory, for an octahedral field, the energy of two $e_{g}$ ordinals will be increased by
1 $\left(\frac{1}{5}\right) \Delta_{0}$
2 $\left(\frac{2}{5}\right) \Delta_{0}$
3 $\left(\frac{3}{5}\right) \Delta_{0}$
4 $\left(\frac{4}{5}\right) \Delta_{0}$
Explanation:
(C) : According to the crystal field theory for octahedral field the energy levels of $\mathrm{e}_{\mathrm{g}}$ are higher, $0.6 \Delta_{\mathrm{o}}$ or $\left(\frac{3}{5}\right) \Delta_{\mathrm{o}}$ while $\mathrm{t}_{2 \mathrm{~g}}$ is lower $0.4 \Delta_{\mathrm{o}}$. or $\left(\frac{2}{5}\right) \Delta_{\mathrm{o}}$
TS EAMCET 10.08.2021
COORDINATION COMPOUNDS
274291
The theory that can completely/properly explain the nature of bonding in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is:
1 Werner's theory
2 Crystal field theory
3 Valence bond theory
4 Molecular orbital theory
Explanation:
(D) : $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is a tetrahedral complex in which bonding in complex properly explain by the 'Molecular orbital theory' (MOT).
274271
Which of the following carbonyls will have the strongest $\mathrm{C}-\mathrm{O}$ bond?
1 $\mathrm{Mn}(\mathrm{CO})_{6}^{+}$
2 $\mathrm{Cr}(\mathrm{CO})_{6}$
3 $\mathrm{V}(\mathrm{CO})_{6}^{-}$
4 $\mathrm{Fe}(\mathrm{CO})_{5}$
Explanation:
(A) : When electron density on metal is high then tendency of back bonding is also high. Due to backbonding lone pair of electron from filled metal orbital is donated to empty antibonding $\left(\pi^{*}\right)$ orbital of $\mathrm{CO}$ lignad. So, bond strength of $\mathrm{C}-\mathrm{O}$ decrease and bond length increase. Hence, $\left[\mathrm{Mn}(\mathrm{CO})_{6}\right]^{+}$has strength $\mathrm{C}-\mathrm{O}$ bond because metal has low electron density due to which backbonding tendency decreases.
AIPMT -2011)
COORDINATION COMPOUNDS
274275
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the d orbits that undergo increase in energy are
(C) : In octahedral symmetry the -orbitals split into two sets with an energy difference, where the $\mathrm{d}_{\mathrm{xy}}, \mathrm{d}_{\mathrm{yz}}$, dzx orbitals will be lower in energy than the $d_{x^{2}-y^{2}}, d_{z^{2}}$ which will have higher energy because the former group is farther from the ligands than the latter therefore experience less repletion.
AP EAPCET-12.07.2022
COORDINATION COMPOUNDS
274281
The correct order for wavelengths of light absorbed in the complex ions $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}$, $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ and $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$ is
(A) : The absorption of light in the complex ions depends upon the nature of metal, oxidation number and ligand (spectrochemical series). The compounds have the same metal as well as same oxidation state but different in ligands. Weak field ligands (WFL) have the lower energy gap between $t_{2 g}$ and $e_{g}$ orbital. So, low amount of energy required and high wavelength of light used for absorption. Hence the correct order of wavelength of light absorbed are that $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}>\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}>\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$
Kerala-CEE-29.08.2021]**
COORDINATION COMPOUNDS
274283
Accordingly to the crystal field theory, for an octahedral field, the energy of two $e_{g}$ ordinals will be increased by
1 $\left(\frac{1}{5}\right) \Delta_{0}$
2 $\left(\frac{2}{5}\right) \Delta_{0}$
3 $\left(\frac{3}{5}\right) \Delta_{0}$
4 $\left(\frac{4}{5}\right) \Delta_{0}$
Explanation:
(C) : According to the crystal field theory for octahedral field the energy levels of $\mathrm{e}_{\mathrm{g}}$ are higher, $0.6 \Delta_{\mathrm{o}}$ or $\left(\frac{3}{5}\right) \Delta_{\mathrm{o}}$ while $\mathrm{t}_{2 \mathrm{~g}}$ is lower $0.4 \Delta_{\mathrm{o}}$. or $\left(\frac{2}{5}\right) \Delta_{\mathrm{o}}$
TS EAMCET 10.08.2021
COORDINATION COMPOUNDS
274291
The theory that can completely/properly explain the nature of bonding in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is:
1 Werner's theory
2 Crystal field theory
3 Valence bond theory
4 Molecular orbital theory
Explanation:
(D) : $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is a tetrahedral complex in which bonding in complex properly explain by the 'Molecular orbital theory' (MOT).
274271
Which of the following carbonyls will have the strongest $\mathrm{C}-\mathrm{O}$ bond?
1 $\mathrm{Mn}(\mathrm{CO})_{6}^{+}$
2 $\mathrm{Cr}(\mathrm{CO})_{6}$
3 $\mathrm{V}(\mathrm{CO})_{6}^{-}$
4 $\mathrm{Fe}(\mathrm{CO})_{5}$
Explanation:
(A) : When electron density on metal is high then tendency of back bonding is also high. Due to backbonding lone pair of electron from filled metal orbital is donated to empty antibonding $\left(\pi^{*}\right)$ orbital of $\mathrm{CO}$ lignad. So, bond strength of $\mathrm{C}-\mathrm{O}$ decrease and bond length increase. Hence, $\left[\mathrm{Mn}(\mathrm{CO})_{6}\right]^{+}$has strength $\mathrm{C}-\mathrm{O}$ bond because metal has low electron density due to which backbonding tendency decreases.
AIPMT -2011)
COORDINATION COMPOUNDS
274275
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the d orbits that undergo increase in energy are
(C) : In octahedral symmetry the -orbitals split into two sets with an energy difference, where the $\mathrm{d}_{\mathrm{xy}}, \mathrm{d}_{\mathrm{yz}}$, dzx orbitals will be lower in energy than the $d_{x^{2}-y^{2}}, d_{z^{2}}$ which will have higher energy because the former group is farther from the ligands than the latter therefore experience less repletion.
AP EAPCET-12.07.2022
COORDINATION COMPOUNDS
274281
The correct order for wavelengths of light absorbed in the complex ions $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}$, $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ and $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$ is
(A) : The absorption of light in the complex ions depends upon the nature of metal, oxidation number and ligand (spectrochemical series). The compounds have the same metal as well as same oxidation state but different in ligands. Weak field ligands (WFL) have the lower energy gap between $t_{2 g}$ and $e_{g}$ orbital. So, low amount of energy required and high wavelength of light used for absorption. Hence the correct order of wavelength of light absorbed are that $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}>\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}>\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$
Kerala-CEE-29.08.2021]**
COORDINATION COMPOUNDS
274283
Accordingly to the crystal field theory, for an octahedral field, the energy of two $e_{g}$ ordinals will be increased by
1 $\left(\frac{1}{5}\right) \Delta_{0}$
2 $\left(\frac{2}{5}\right) \Delta_{0}$
3 $\left(\frac{3}{5}\right) \Delta_{0}$
4 $\left(\frac{4}{5}\right) \Delta_{0}$
Explanation:
(C) : According to the crystal field theory for octahedral field the energy levels of $\mathrm{e}_{\mathrm{g}}$ are higher, $0.6 \Delta_{\mathrm{o}}$ or $\left(\frac{3}{5}\right) \Delta_{\mathrm{o}}$ while $\mathrm{t}_{2 \mathrm{~g}}$ is lower $0.4 \Delta_{\mathrm{o}}$. or $\left(\frac{2}{5}\right) \Delta_{\mathrm{o}}$
TS EAMCET 10.08.2021
COORDINATION COMPOUNDS
274291
The theory that can completely/properly explain the nature of bonding in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is:
1 Werner's theory
2 Crystal field theory
3 Valence bond theory
4 Molecular orbital theory
Explanation:
(D) : $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is a tetrahedral complex in which bonding in complex properly explain by the 'Molecular orbital theory' (MOT).
274271
Which of the following carbonyls will have the strongest $\mathrm{C}-\mathrm{O}$ bond?
1 $\mathrm{Mn}(\mathrm{CO})_{6}^{+}$
2 $\mathrm{Cr}(\mathrm{CO})_{6}$
3 $\mathrm{V}(\mathrm{CO})_{6}^{-}$
4 $\mathrm{Fe}(\mathrm{CO})_{5}$
Explanation:
(A) : When electron density on metal is high then tendency of back bonding is also high. Due to backbonding lone pair of electron from filled metal orbital is donated to empty antibonding $\left(\pi^{*}\right)$ orbital of $\mathrm{CO}$ lignad. So, bond strength of $\mathrm{C}-\mathrm{O}$ decrease and bond length increase. Hence, $\left[\mathrm{Mn}(\mathrm{CO})_{6}\right]^{+}$has strength $\mathrm{C}-\mathrm{O}$ bond because metal has low electron density due to which backbonding tendency decreases.
AIPMT -2011)
COORDINATION COMPOUNDS
274275
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the d orbits that undergo increase in energy are
(C) : In octahedral symmetry the -orbitals split into two sets with an energy difference, where the $\mathrm{d}_{\mathrm{xy}}, \mathrm{d}_{\mathrm{yz}}$, dzx orbitals will be lower in energy than the $d_{x^{2}-y^{2}}, d_{z^{2}}$ which will have higher energy because the former group is farther from the ligands than the latter therefore experience less repletion.
AP EAPCET-12.07.2022
COORDINATION COMPOUNDS
274281
The correct order for wavelengths of light absorbed in the complex ions $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}$, $\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}$ and $\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$ is
(A) : The absorption of light in the complex ions depends upon the nature of metal, oxidation number and ligand (spectrochemical series). The compounds have the same metal as well as same oxidation state but different in ligands. Weak field ligands (WFL) have the lower energy gap between $t_{2 g}$ and $e_{g}$ orbital. So, low amount of energy required and high wavelength of light used for absorption. Hence the correct order of wavelength of light absorbed are that $\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+}>\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}>\left[\mathrm{Co}(\mathrm{CN})_{6}\right]^{3+}$
Kerala-CEE-29.08.2021]**
COORDINATION COMPOUNDS
274283
Accordingly to the crystal field theory, for an octahedral field, the energy of two $e_{g}$ ordinals will be increased by
1 $\left(\frac{1}{5}\right) \Delta_{0}$
2 $\left(\frac{2}{5}\right) \Delta_{0}$
3 $\left(\frac{3}{5}\right) \Delta_{0}$
4 $\left(\frac{4}{5}\right) \Delta_{0}$
Explanation:
(C) : According to the crystal field theory for octahedral field the energy levels of $\mathrm{e}_{\mathrm{g}}$ are higher, $0.6 \Delta_{\mathrm{o}}$ or $\left(\frac{3}{5}\right) \Delta_{\mathrm{o}}$ while $\mathrm{t}_{2 \mathrm{~g}}$ is lower $0.4 \Delta_{\mathrm{o}}$. or $\left(\frac{2}{5}\right) \Delta_{\mathrm{o}}$
TS EAMCET 10.08.2021
COORDINATION COMPOUNDS
274291
The theory that can completely/properly explain the nature of bonding in $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is:
1 Werner's theory
2 Crystal field theory
3 Valence bond theory
4 Molecular orbital theory
Explanation:
(D) : $\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]$ is a tetrahedral complex in which bonding in complex properly explain by the 'Molecular orbital theory' (MOT).
