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Why cycloheptatrienyl cation is more stable than cycloheptatriene?
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Kevin Wilkinson
Why cycloheptatrienyl cation is more stable than cycloheptatriene?
PF3 is more stable than NF3 because P-F bond energy is more than N-F bond energy.
Why P-F bond is more stronger than N-F bond?
1) phosphorus has empty 3d orbitals which can accept electron pair from flourine forming a backbond(though not very strong as phosphorus is large backbonding becomes difficult but still it can be considered) .
2) Nitrogen and flourine are small atoms so their nuclei repel more effectively than in case of phosphorus(as P atom is large) hence decreasing the bond strength( just as Cl-Cl BE being more than F-F BE)
PF3 is more stable than NF3 because P-F bond energy is more than N-F bond energy.
Why P-F bond is more stronger than N-F bond?
1) phosphorus has empty 3d orbitals which can accept electron pair from flourine forming a backbond(though not very strong as phosphorus is large backbonding becomes difficult but still it can be considered) .
2) Nitrogen and flourine are small atoms so their nuclei repel more effectively than in case of phosphorus(as P atom is large) hence decreasing the bond strength( just as Cl-Cl BE being more than F-F BE)
An ion carrying higher charge and smaller size is associates with greater lattice energy and hydration energy. That is why Cu+2 is more stable than Cu+1. It is expected on the basis of electronic configuration that Cu+ should be more stable because it has completely filled orbitals, but the lattice and hydration energy factors dominate as a result Cu+2 is more stable
An ion carrying higher charge and smaller size is associates with greater lattice energy and hydration energy. That is why Cu+2 is more stable than Cu+1. It is expected on the basis of electronic configuration that Cu+ should be more stable because it has completely filled orbitals, but the lattice and hydration energy factors dominate as a result Cu+2 is more stable
The cyclohexyl cation is more stable due to the hyperconjugation of the electrons from the C-H double bond where that carbocation is located.
Benzene howeve is sp2 hybridized throughout the entire ring. If we deprotonate any of the carbons on benzene, it becomes sp hybridized. As sp hybridized, it wants to be linear but can’t due to the double bond. Unlike the cyclohexyl cation, there are no hydrogens close enough to stablize it’s positive charge.
The cyclohexyl cation is more stable due to the hyperconjugation of the electrons from the C-H double bond where that carbocation is located.
Benzene howeve is sp2 hybridized throughout the entire ring. If we deprotonate any of the carbons on benzene, it becomes sp hybridized. As sp hybridized, it wants to be linear but can’t due to the double bond. Unlike the cyclohexyl cation, there are no hydrogens close enough to stablize it’s positive charge.
Bond order of He2 is 0 which directly suggests that He-He bond is extremely unstable and easily splits into individual atoms. Now since in case of He, which is an individual atom, the concept of bond order doesn't actually make any real sense as there are no actual chemical bonds involved, molecular orbital theory fails to explain the stability of He has.
Bond order of He2 is 0 which directly suggests that He-He bond is extremely unstable and easily splits into individual atoms. Now since in case of He, which is an individual atom, the concept of bond order doesn't actually make any real sense as there are no actual chemical bonds involved, molecular orbital theory fails to explain the stability of He has.
PF3 is more stable than NF3 because P-F bond energy is more than N-F bond energy.
Why P-F bond is more stronger than N-F bond?
1) phosphorus has empty 3d orbitals which can accept electron pair from flourine forming a backbond(though not very strong as phosphorus is large backbonding becomes difficult but still it can be considered) .
2) Nitrogen and flourine are small atoms so their nuclei repel more effectively than in case of phosphorus(as P atom is large) hence decreasing the bond strength( just as Cl-Cl BE being more than F-F BE)
PF3 is more stable than NF3 because P-F bond energy is more than N-F bond energy.
Why P-F bond is more stronger than N-F bond?
1) phosphorus has empty 3d orbitals which can accept electron pair from flourine forming a backbond(though not very strong as phosphorus is large backbonding becomes difficult but still it can be considered) .
2) Nitrogen and flourine are small atoms so their nuclei repel more effectively than in case of phosphorus(as P atom is large) hence decreasing the bond strength( just as Cl-Cl BE being more than F-F BE)
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An ion carrying higher charge and smaller size is associates with greater lattice energy and hydration energy. That is why Cu+2 is more stable than Cu+1. It is expected on the basis of electronic configuration that Cu+ should be more stable because it has completely filled orbitals, but the lattice and hydration energy factors dominate as a result Cu+2 is more stable
An ion carrying higher charge and smaller size is associates with greater lattice energy and hydration energy. That is why Cu+2 is more stable than Cu+1. It is expected on the basis of electronic configuration that Cu+ should be more stable because it has completely filled orbitals, but the lattice and hydration energy factors dominate as a result Cu+2 is more stable
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The cyclohexyl cation is more stable due to the hyperconjugation of the electrons from the C-H double bond where that carbocation is located.
Benzene howeve is sp2 hybridized throughout the entire ring. If we deprotonate any of the carbons on benzene, it becomes sp hybridized. As sp hybridized, it wants to be linear but can’t due to the double bond. Unlike the cyclohexyl cation, there are no hydrogens close enough to stablize it’s positive charge.
The cyclohexyl cation is more stable due to the hyperconjugation of the electrons from the C-H double bond where that carbocation is located.
Benzene howeve is sp2 hybridized throughout the entire ring. If we deprotonate any of the carbons on benzene, it becomes sp hybridized. As sp hybridized, it wants to be linear but can’t due to the double bond. Unlike the cyclohexyl cation, there are no hydrogens close enough to stablize it’s positive charge.
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Regards
Shivin Diwakar
Regards
Shivin Diwakar
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Why this structure is stable ??
Why this structure is stable ??
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Q. Why is CO more stable than CO2?
Never ask why until you ask IF.
CO is NOT more stable than CO2.
The heat of formation of CO is -110 kJ/mol.
The heat of formation of CO2 is -393 kJ/mol.
That means that CO2 is more stable than CO, by almost 300 kJ/mol.
NIST Chemistry WebBook
In brief, CO2 is more stable than CO because it is fully oxidized: carbon has a +4 oxidation state, while in CO it has a +2 oxidation state.
Q. Why is CO more stable than CO2?
Never ask why until you ask IF.
CO is NOT more stable than CO2.
The heat of formation of CO is -110 kJ/mol.
The heat of formation of CO2 is -393 kJ/mol.
That means that CO2 is more stable than CO, by almost 300 kJ/mol.
NIST Chemistry WebBook
In brief, CO2 is more stable than CO because it is fully oxidized: carbon has a +4 oxidation state, while in CO it has a +2 oxidation state.
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Bond order of He2 is 0 which directly suggests that He-He bond is extremely unstable and easily splits into individual atoms. Now since in case of He, which is an individual atom, the concept of bond order doesn't actually make any real sense as there are no actual chemical bonds involved, molecular orbital theory fails to explain the stability of He has.
Bond order of He2 is 0 which directly suggests that He-He bond is extremely unstable and easily splits into individual atoms. Now since in case of He, which is an individual atom, the concept of bond order doesn't actually make any real sense as there are no actual chemical bonds involved, molecular orbital theory fails to explain the stability of He has.
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