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(A): NH(3) is a liquid while the other h...

(A): `NH_(3)` is a liquid while the other hydrides of V-A Group elements are gases at room temp.
(R) : `NH_(3)` possess inter molecular hydrogen bonds in liquid state

A

Both A & R are true, R is the correct explanation of A

B

Both A & R are true, R is not correct explanation of A

C

A is true, R is false

D

A is false, R is true

Text Solution

AI Generated Solution

The correct Answer is:
To solve the question, we need to analyze both the assertion and the reason provided. ### Step 1: Analyze the Assertion The assertion states that `NH3` (ammonia) is a liquid while the other hydrides of V-A group elements are gases at room temperature. - **Fact Check**: - Ammonia (`NH3`) is indeed a liquid at room temperature (specifically, it has a boiling point of -33.34 °C, so it can exist as a liquid under certain conditions). - However, the statement that "other hydrides of V-A group elements are gases" is not entirely accurate. While most hydrides of group 15 elements (like PH3, AsH3, and SbH3) are gases at room temperature, bismuth hydride (BiH3) can also exist as a gas. Therefore, the assertion is misleading because it implies that all other hydrides are gases without exception, which is not true. ### Conclusion for Assertion: The assertion is **false** because it generalizes the state of all hydrides of V-A group elements incorrectly. ### Step 2: Analyze the Reason The reason states that `NH3` possesses intermolecular hydrogen bonds in the liquid state. - **Fact Check**: - Ammonia does indeed exhibit hydrogen bonding due to the presence of nitrogen, which is highly electronegative. This leads to strong intermolecular forces that are responsible for its liquid state at room temperature. ### Conclusion for Reason: The reason is **true** because it accurately describes the presence of hydrogen bonds in ammonia. ### Final Evaluation: - **Assertion (A)**: False - **Reason (R)**: True Thus, the correct relationship is that the assertion is false while the reason is true. ### Final Answer: The assertion is false, and the reason is true. ---
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Fifth group elements form hydrides to type AH_(3) . The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides . The H-M-H bond angle of V group hydrides decrease from 107^(circ) to 90^(circ) for NH_(3) to SbH_(3) , this is due to:

Fifth group elements form hydrides to type AH_(3) . The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides . The boiling points of the hydrides of V-group elements are in the order :

Fifth group elements form hydrides to type AH_(3) . The hydrides have a lone pair of electrons. The hydries are reducing in nature and the reducing power is related to the stability of A-H bonds. The hydrides are covalent and low boiling. Their boiling points depends on their ability to from hydrogen bond and their molecular size which decide the intermolcular forces in the hydrides . Reducing power of V-group hydrides are in order :

All the boron trihalides except BI_(3) may be prepared by direction between the elements. Boron trihalides consist of trigonal-planar BX_(3) molecules. Unlike the halides of the other elements in the group they are monomeric in the gas, liquid and solid states, BF_(3) and BCl_(3) are gases, BBr_(3) is a volatile liquid and BI_(3) is a solid. Boron trihalides are Lewis acids because they form simple Lewis complexes with suitable bases, as in the reaction: BF_(3)(g)+NH_(3)(g)toF_(3)B-NH_(3)(s) However, boron chlorides, bromides and iodides are susceptible (sensitive) to protolysis by mild proton sources such as water, alcohols and even amines, for example BCl_(3) undergoes rapid hydrolysis: BCl_(3)(g)+3H_(2)O(l)toB(OH)_(3)(aq)+3HCl (aq) It is supposed that the first step in the above reaction is the formation of the complex Cl_(3)B larr OH_(2) which then eliminates HCl and reacts with water. Which of the following is the correct prediction about observed B-X bond length, in BX_(3) molecules?

All the boron trihalides except BI_(3) may be prepared by direction between the elements. Boron trihalides consist of trigonal-planar BX_(3) molecules. Unlike the halides of the other elements in the group they are monomeric in the gas, liquid and solid states, BF_(3) and BCl_(3) are gases, BBr_(3) is a volatile liquid and BI_(3) is a solid. Boron trihalides are Lewis acids because they form simple Lewis complexes with suitable bases, as in the reaction: BF_(3)(g)+NH_(3)(g)toF_(3)B-NH_(3)(s) However, boron chlorides, bromides and iodides are susceptible (sensitive) to protolysis by mild proton sources such as water, alcohols and even amines, for example BCl_(3) undergoes rapid hydrolysis: BCl_(3)(g)+3H_(2)O(l)toB(OH)_(3)(aq)+3HCl (aq) It is supposed that the first step in the above reaction is the formation of the complex Cl_(3)B larr OH_(2) which then eliminates HCl and reacts with water. Which of the follwoing is the best order of Lewis acid strength of BF_(3),BCl_(3) and BBr_(3) ?

All the boron trihalides except BI_(3) may be prepared by direction between the elements. Boron trihalides consist of trigonal-planar BX_(3) molecules. Unlike the halides of the other elements in the group they are monomeric in the gas, liquid and solid states, BF_(3) and BCl_(3) are gases, BBr_(3) is a volatile liquid and BI_(3) is a solid. Boron trihalides are Lewis acids because they form simple Lewis complexes with suitable bases, as in the reaction: BF_(3)(g)+NH_(3)(g)toF_(3)B-NH_(3)(s) However, boron chlorides, bromides and iodides are susceptible (sensitive) to protolysis by mild proton sources such as water, alcohols and even amines, for example BCl_(3) undergoes rapid hydrolysis: BCl_(3)(g)+3H_(2)O(l)toB(OH)_(3)(aq)+3HCl (aq) It is supposed that the first step in the above reaction is the formation of the complex Cl_(3)B larr OH_(2) which then eliminates HCl and reacts with water. Which of the following reactions is incorrect ?