The basic character of hydrides of the 15 group elements decreases in the order

Question

The maximum covalency of a non-metallic group 15 element 'E' with the weakest E-E bond is:

Answer 1

The question asks about the decreasing order of basic character for hydrides of Group 15 elements. Let's understand the concept to arrive at the correct answer:

Group 15 elements include nitrogen (N), phosphorus (P), arsenic (As), and antimony (Sb). The basic nature of their hydrides depends on the capacity of the element to donate a lone pair of electrons. This ability decreases down the group due to increased atomic size and decreased electronegativity.

Nitrogen (NH₃): Ammonia is the most basic among these hydrides due to the small size of nitrogen and high electronegativity, allowing effective donation of its lone pair.
Phosphorus (PH₃): Phosphine is less basic than ammonia. Compared to nitrogen, phosphorus is larger and less electronegative, resulting in reduced ability to donate electrons.
Arsenic (AsH₃): Arsenic hydride has even lesser basic character than phosphine due to increased atomic size and further reduced electronegativity.
Antimony (SbH₃): Stibine is the least basic among them. This is due to its large atomic size and minimal electronegativity, making it the least capable of donating a lone pair.

Thus, the basic character decreases in the order:

NH_3 > PH_3 > AsH_3 > SbH_3

This reasoning aligns perfectly with the given correct option:

NH_3 > PH_3 > AsH_3 > SbH_3

Therefore, the correct answer is the option that states this order.

Answer 2

The question asks about the decreasing order of basic character for hydrides of Group 15 elements. Let's understand the concept to arrive at the correct answer:

Group 15 elements include nitrogen (N), phosphorus (P), arsenic (As), and antimony (Sb). The basic nature of their hydrides depends on the capacity of the element to donate a lone pair of electrons. This ability decreases down the group due to increased atomic size and decreased electronegativity.

Nitrogen (NH₃): Ammonia is the most basic among these hydrides due to the small size of nitrogen and high electronegativity, allowing effective donation of its lone pair.
Phosphorus (PH₃): Phosphine is less basic than ammonia. Compared to nitrogen, phosphorus is larger and less electronegative, resulting in reduced ability to donate electrons.
Arsenic (AsH₃): Arsenic hydride has even lesser basic character than phosphine due to increased atomic size and further reduced electronegativity.
Antimony (SbH₃): Stibine is the least basic among them. This is due to its large atomic size and minimal electronegativity, making it the least capable of donating a lone pair.

Thus, the basic character decreases in the order:

NH_3 > PH_3 > AsH_3 > SbH_3

This reasoning aligns perfectly with the given correct option:

NH_3 > PH_3 > AsH_3 > SbH_3

Therefore, the correct answer is the option that states this order.

The basic character of hydrides of the 15 group elements decreases in the order

The Correct Option is C

Solution and Explanation

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