In CCl3-, the -ve charge gets delocalised to the vacant d-orbital of chlorine (known as d-orbital resonance), wheareas no such phenomenon can be exhibited by fluorine in case of CF3- due to absence of any vacant orbital resonance.
In CCl3-, the -ve charge gets delocalised to the vacant d-orbital of chlorine (known as d-orbital resonance), wheareas no such phenomenon can be exhibited by fluorine in case of CF3- due to absence of any vacant orbital resonance.
Nitrogen is more electronegative than Phosphorus. Hence N-H bond is stronger than that of P-H bond. Due to the stronger bond between N and H atoms, it is less reactive as larger amount of energy is required to overcome the N-H bonds. Hence NH3 is less reactive than PH3
Nitrogen is more electronegative than Phosphorus. Hence N-H bond is stronger than that of P-H bond. Due to the stronger bond between N and H atoms, it is less reactive as larger amount of energy is required to overcome the N-H bonds. Hence NH3 is less reactive than PH3
Basicity depends on availability of electro density. If the electron density is high, it will donate the pair of electron easily, hence it acts as better base.
In NH3 and PH3, the central atom posses a lone pair. As N is smaller than P, electron density on N is high compared to P. Therefore NH3 acts as better base than PH3. It also decreases as you r moving from NH3 to BiH3. Basicity order in hydrides of 15th group is NH3>PH3>AsH3>SbH3>BiH3
Basicity depends on availability of electro density. If the electron density is high, it will donate the pair of electron easily, hence it acts as better base.
In NH3 and PH3, the central atom posses a lone pair. As N is smaller than P, electron density on N is high compared to P. Therefore NH3 acts as better base than PH3. It also decreases as you r moving from NH3 to BiH3. Basicity order in hydrides of 15th group is NH3>PH3>AsH3>SbH3>BiH3
The hybridisation concept says that only the orbitals with same orientation and less energy difference can combine to form hybridised orbitals.
Here the size of central atom is huge compared to that of Hydrogen, so the hydrogen atoms approach from the axial side hence have a bond angle close to 90 degrees (p-orbitals are axial and the orbitals are mutually perpendicular to each other).
The hybridisation concept says that only the orbitals with same orientation and less energy difference can combine to form hybridised orbitals.
Here the size of central atom is huge compared to that of Hydrogen, so the hydrogen atoms approach from the axial side hence have a bond angle close to 90 degrees (p-orbitals are axial and the orbitals are mutually perpendicular to each other).
Because conjugate base of strong acid is a weak base. Since HCl is strong acid than Acetic acid (CH3COOH) therefore, the conjugate base of HCl i.e Cl- will be weaker base than conjugate base of CH3COOH i.e. CH3OO-. Following are the reactions:
Because conjugate base of strong acid is a weak base. Since HCl is strong acid than Acetic acid (CH3COOH) therefore, the conjugate base of HCl i.e Cl- will be weaker base than conjugate base of CH3COOH i.e. CH3OO-. Following are the reactions:
The Arrhenius acid-base theory defines an acid as a hydrogen ion donor and a base as a hydroxide ion donor. But NH3 acts like a base (gives the “base” color in indicators; can be titrated with an acid, with appropriate pH changes being shown in the course of the titration).
So the Bronsted-Lowry theory changed the definition to: An acid is a hydrogen ion donor and a base is a hydrogen ion acceptor. NH3, is a base and the ammonium ion is its conjugate acid, NH4+.
But acid-base behavior is sometimes exhibited in systems where there is no transfer of hydrogen ions. The Lewis acid-base concept emphasizes electron transfer rather than hydrogen ion transfer. A Lewis acid accepts an electron pair and a Lewis base donates an electron pair.
Like ammonia, phosphine (PH3) has a lone pair on an atom (P) which is more electronegative than the other atoms (H’s) in the molecule. Thus, the phosphorus draws electron-density from the hydrogens, increasing the size of phosphorus’ lone pair and making PH3 a base because it is a good hydrogen ion acceptor (B-L) or because it can donate electrons from its large lone pair (Lewis).
On the other hand, in PF3, the phosphorus is bound to fluorine atoms and fluorine has a higher electronegativity than phosphorus does. Therefore, in PF3, electron-density is drawn away from the phosphorus, causing phosphorous’ lone pair to shrink. Thus, PF3 might attract electrons, making it a Lewis acid (it can’t function directly as an Arrhenius or Bronsted-Lowry acid because it has no hydrogen ions to donate, but, in aqueous solution, it might extract a hydroxide ion from water, thus increasing the concentration of hydrogen ions in the solution).
The Arrhenius acid-base theory defines an acid as a hydrogen ion donor and a base as a hydroxide ion donor. But NH3 acts like a base (gives the “base” color in indicators; can be titrated with an acid, with appropriate pH changes being shown in the course of the titration).
So the Bronsted-Lowry theory changed the definition to: An acid is a hydrogen ion donor and a base is a hydrogen ion acceptor. NH3, is a base and the ammonium ion is its conjugate acid, NH4+.
But acid-base behavior is sometimes exhibited in systems where there is no transfer of hydrogen ions. The Lewis acid-base concept emphasizes electron transfer rather than hydrogen ion transfer. A Lewis acid accepts an electron pair and a Lewis base donates an electron pair.
Like ammonia, phosphine (PH3) has a lone pair on an atom (P) which is more electronegative than the other atoms (H’s) in the molecule. Thus, the phosphorus draws electron-density from the hydrogens, increasing the size of phosphorus’ lone pair and making PH3 a base because it is a good hydrogen ion acceptor (B-L) or because it can donate electrons from its large lone pair (Lewis).
On the other hand, in PF3, the phosphorus is bound to fluorine atoms and fluorine has a higher electronegativity than phosphorus does. Therefore, in PF3, electron-density is drawn away from the phosphorus, causing phosphorous’ lone pair to shrink. Thus, PF3 might attract electrons, making it a Lewis acid (it can’t function directly as an Arrhenius or Bronsted-Lowry acid because it has no hydrogen ions to donate, but, in aqueous solution, it might extract a hydroxide ion from water, thus increasing the concentration of hydrogen ions in the solution).
In CCl3-, the -ve charge gets delocalised to the vacant d-orbital of chlorine (known as d-orbital resonance), wheareas no such phenomenon can be exhibited by fluorine in case of CF3- due to absence of any vacant orbital resonance.
Hence, CCl3(-) more stable than CF3(-).
In CCl3-, the -ve charge gets delocalised to the vacant d-orbital of chlorine (known as d-orbital resonance), wheareas no such phenomenon can be exhibited by fluorine in case of CF3- due to absence of any vacant orbital resonance.
Hence, CCl3(-) more stable than CF3(-).
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Nitrogen is more electronegative than Phosphorus. Hence N-H bond is stronger than that of P-H bond. Due to the stronger bond between N and H atoms, it is less reactive as larger amount of energy is required to overcome the N-H bonds. Hence NH3 is less reactive than PH3
Nitrogen is more electronegative than Phosphorus. Hence N-H bond is stronger than that of P-H bond. Due to the stronger bond between N and H atoms, it is less reactive as larger amount of energy is required to overcome the N-H bonds. Hence NH3 is less reactive than PH3
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Basicity depends on availability of electro density. If the electron density is high, it will donate the pair of electron easily, hence it acts as better base.
In NH3 and PH3, the central atom posses a lone pair. As N is smaller than P, electron density on N is high compared to P. Therefore NH3 acts as better base than PH3. It also decreases as you r moving from NH3 to BiH3. Basicity order in hydrides of 15th group is NH3>PH3>AsH3>SbH3>BiH3
Hope this helps
Basicity depends on availability of electro density. If the electron density is high, it will donate the pair of electron easily, hence it acts as better base.
In NH3 and PH3, the central atom posses a lone pair. As N is smaller than P, electron density on N is high compared to P. Therefore NH3 acts as better base than PH3. It also decreases as you r moving from NH3 to BiH3. Basicity order in hydrides of 15th group is NH3>PH3>AsH3>SbH3>BiH3
Hope this helps
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Flourine being most electronegative element pulls the lone pair of electrons towards itself and make this lone pair less available.
Flourine being most electronegative element pulls the lone pair of electrons towards itself and make this lone pair less available.
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The hybridisation concept says that only the orbitals with same orientation and less energy difference can combine to form hybridised orbitals.
Here the size of central atom is huge compared to that of Hydrogen, so the hydrogen atoms approach from the axial side hence have a bond angle close to 90 degrees (p-orbitals are axial and the orbitals are mutually perpendicular to each other).
regards.
The hybridisation concept says that only the orbitals with same orientation and less energy difference can combine to form hybridised orbitals.
Here the size of central atom is huge compared to that of Hydrogen, so the hydrogen atoms approach from the axial side hence have a bond angle close to 90 degrees (p-orbitals are axial and the orbitals are mutually perpendicular to each other).
regards.
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Because conjugate base of strong acid is a weak base. Since HCl is strong acid than Acetic acid (CH3COOH) therefore, the conjugate base of HCl i.e Cl- will be weaker base than conjugate base of CH3COOH i.e. CH3OO-. Following are the reactions:
HCl (Strong acid) -> H+ + Cl-(weak base)
CH3COOH (weak acid) ->H+ + CH3COO- (strong base)
Because conjugate base of strong acid is a weak base. Since HCl is strong acid than Acetic acid (CH3COOH) therefore, the conjugate base of HCl i.e Cl- will be weaker base than conjugate base of CH3COOH i.e. CH3OO-. Following are the reactions:
HCl (Strong acid) -> H+ + Cl-(weak base)
CH3COOH (weak acid) ->H+ + CH3COO- (strong base)
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The Arrhenius acid-base theory defines an acid as a hydrogen ion donor and a base as a hydroxide ion donor. But NH3 acts like a base (gives the “base” color in indicators; can be titrated with an acid, with appropriate pH changes being shown in the course of the titration).
So the Bronsted-Lowry theory changed the definition to: An acid is a hydrogen ion donor and a base is a hydrogen ion acceptor. NH3, is a base and the ammonium ion is its conjugate acid, NH4+.
But acid-base behavior is sometimes exhibited in systems where there is no transfer of hydrogen ions. The Lewis acid-base concept emphasizes electron transfer rather than hydrogen ion transfer. A Lewis acid accepts an electron pair and a Lewis base donates an electron pair.
Like ammonia, phosphine (PH3) has a lone pair on an atom (P) which is more electronegative than the other atoms (H’s) in the molecule. Thus, the phosphorus draws electron-density from the hydrogens, increasing the size of phosphorus’ lone pair and making PH3 a base because it is a good hydrogen ion acceptor (B-L) or because it can donate electrons from its large lone pair (Lewis).
On the other hand, in PF3, the phosphorus is bound to fluorine atoms and fluorine has a higher electronegativity than phosphorus does. Therefore, in PF3, electron-density is drawn away from the phosphorus, causing phosphorous’ lone pair to shrink. Thus, PF3 might attract electrons, making it a Lewis acid (it can’t function directly as an Arrhenius or Bronsted-Lowry acid because it has no hydrogen ions to donate, but, in aqueous solution, it might extract a hydroxide ion from water, thus increasing the concentration of hydrogen ions in the solution).
The Arrhenius acid-base theory defines an acid as a hydrogen ion donor and a base as a hydroxide ion donor. But NH3 acts like a base (gives the “base” color in indicators; can be titrated with an acid, with appropriate pH changes being shown in the course of the titration).
So the Bronsted-Lowry theory changed the definition to: An acid is a hydrogen ion donor and a base is a hydrogen ion acceptor. NH3, is a base and the ammonium ion is its conjugate acid, NH4+.
But acid-base behavior is sometimes exhibited in systems where there is no transfer of hydrogen ions. The Lewis acid-base concept emphasizes electron transfer rather than hydrogen ion transfer. A Lewis acid accepts an electron pair and a Lewis base donates an electron pair.
Like ammonia, phosphine (PH3) has a lone pair on an atom (P) which is more electronegative than the other atoms (H’s) in the molecule. Thus, the phosphorus draws electron-density from the hydrogens, increasing the size of phosphorus’ lone pair and making PH3 a base because it is a good hydrogen ion acceptor (B-L) or because it can donate electrons from its large lone pair (Lewis).
On the other hand, in PF3, the phosphorus is bound to fluorine atoms and fluorine has a higher electronegativity than phosphorus does. Therefore, in PF3, electron-density is drawn away from the phosphorus, causing phosphorous’ lone pair to shrink. Thus, PF3 might attract electrons, making it a Lewis acid (it can’t function directly as an Arrhenius or Bronsted-Lowry acid because it has no hydrogen ions to donate, but, in aqueous solution, it might extract a hydroxide ion from water, thus increasing the concentration of hydrogen ions in the solution).
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