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The ease of formation of the adduct, NH3 · BX3 (where X = F, Cl, Br) follows the order:
- a)BBr3 < BCl3 < BF3
- b)BCl3 < BF3 < BBr3
- c)BF3 < BCl3 < BBr3
- d)BBr3 < BF3 < BCl3
Correct answer is option 'C'. Can you explain this answer?
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The ease of formation of the adduct, NH3 · BX3 (where X = F, Cl, ...
Formation of Adduct NH3 BX3
The formation of adduct NH3 BX3 (where X = F, Cl, Br) is a common reaction in chemistry. This reaction involves the addition of ammonia (NH3) to a boron trihalide (BX3) to form a complex compound. The ease of formation of this adduct varies depending on the halogen present in the boron trihalide.
Order of Ease of Formation
The order of ease of formation of the adduct NH3 BX3 (where X = F, Cl, Br) is as follows:
BF3 BCl3 BBr3
This means that the adduct formed between ammonia and boron trifluoride (BF3) is the easiest to form, while the adduct formed between ammonia and boron tribromide (BBr3) is the most difficult to form.
Explanation
The ease of formation of the adduct NH3 BX3 can be explained by the following factors:
1. Electronegativity
The electronegativity of the halogen present in the boron trihalide plays a significant role in the ease of formation of the adduct. Fluorine (F) is the most electronegative element, followed by chlorine (Cl) and then bromine (Br). This means that the bond between boron and fluorine is the most polar, while the bond between boron and bromine is the least polar.
2. Size of the Halogen
The size of the halogen present in the boron trihalide also affects the ease of formation of the adduct. The larger the halogen, the more difficult it is for ammonia to approach the boron atom and form a complex. Bromine is larger than chlorine, which is larger than fluorine.
3. Bond Strength
The strength of the bond between boron and the halogen also affects the ease of formation of the adduct. The bond strength decreases as we move from fluorine to bromine.
Based on these factors, we can see that the ease of formation of the adduct NH3 BX3 follows the order BF3 BCl3 BBr3. Fluorine is the most electronegative and has the smallest size, making it the easiest to form a complex with ammonia. Chlorine is less electronegative and larger than fluorine, making it slightly more difficult to form a complex. Bromine has the lowest electronegativity and the largest size, making it the most difficult to form a complex with ammonia.
The formation of adduct NH3 BX3 (where X = F, Cl, Br) is a common reaction in chemistry. This reaction involves the addition of ammonia (NH3) to a boron trihalide (BX3) to form a complex compound. The ease of formation of this adduct varies depending on the halogen present in the boron trihalide.
Order of Ease of Formation
The order of ease of formation of the adduct NH3 BX3 (where X = F, Cl, Br) is as follows:
BF3 BCl3 BBr3
This means that the adduct formed between ammonia and boron trifluoride (BF3) is the easiest to form, while the adduct formed between ammonia and boron tribromide (BBr3) is the most difficult to form.
Explanation
The ease of formation of the adduct NH3 BX3 can be explained by the following factors:
1. Electronegativity
The electronegativity of the halogen present in the boron trihalide plays a significant role in the ease of formation of the adduct. Fluorine (F) is the most electronegative element, followed by chlorine (Cl) and then bromine (Br). This means that the bond between boron and fluorine is the most polar, while the bond between boron and bromine is the least polar.
2. Size of the Halogen
The size of the halogen present in the boron trihalide also affects the ease of formation of the adduct. The larger the halogen, the more difficult it is for ammonia to approach the boron atom and form a complex. Bromine is larger than chlorine, which is larger than fluorine.
3. Bond Strength
The strength of the bond between boron and the halogen also affects the ease of formation of the adduct. The bond strength decreases as we move from fluorine to bromine.
Based on these factors, we can see that the ease of formation of the adduct NH3 BX3 follows the order BF3 BCl3 BBr3. Fluorine is the most electronegative and has the smallest size, making it the easiest to form a complex with ammonia. Chlorine is less electronegative and larger than fluorine, making it slightly more difficult to form a complex. Bromine has the lowest electronegativity and the largest size, making it the most difficult to form a complex with ammonia.
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The ease of formation of the adduct, NH3 · BX3 (where X = F, Cl, ...
With increase size and decrease electronegativity back bonding decrease so easily form adduct
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