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Group 15 Properties (Nitrogen Family) Video Lecture - JEE

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FAQs on Group 15 Properties (Nitrogen Family) Video Lecture - JEE

1. What are the properties of the Nitrogen family?

Ans. The Nitrogen family, also known as Group 15 elements, consists of nitrogen (N), phosphorus (P), arsenic (As), antimony (Sb), and bismuth (Bi). These elements share certain common properties. They have five valence electrons in their outermost shell, which allows them to form covalent compounds with other elements. They have relatively high electronegativity and tend to gain or share electrons to achieve a stable electron configuration. They exhibit multiple oxidation states and can form compounds with various elements.

2. How does the reactivity of the Nitrogen family change as you move down the group?

Ans. The reactivity of the Nitrogen family elements generally decreases as you move down the group. Nitrogen (N) is the most reactive element in the group due to its high electronegativity and small atomic size. It readily forms covalent compounds with other elements. However, as you move down the group, the atomic size increases, and the electronegativity decreases. This results in decreased reactivity. For example, bismuth (Bi) is the least reactive element in the group and forms compounds with difficulty.

3. What are the common uses of the Nitrogen family elements?

Ans. The elements of the Nitrogen family have various practical applications. Nitrogen (N) is extensively used in the production of ammonia, which is crucial for the production of fertilizers and explosives. Phosphorus (P) is an essential nutrient for plants and is used in the manufacturing of fertilizers, detergents, and matches. Arsenic (As), despite its toxicity, has applications in the semiconductor industry and wood preservation. Antimony (Sb) finds use in flame retardants, batteries, and alloys. Bismuth (Bi) is used in cosmetics, pharmaceuticals, and as an alloying agent.

4. How do the melting and boiling points of the Nitrogen family elements change down the group?

Ans. Generally, the melting and boiling points of the Nitrogen family elements increase as you move down the group. Nitrogen (N) has a low boiling point (-195.8°C) and melting point (-210.0°C) due to the presence of weak van der Waals forces between its molecules. However, as you move down the group, the atomic size increases, resulting in stronger metallic bonding or van der Waals forces. This leads to higher melting and boiling points. For example, bismuth (Bi) has a melting point of 271.4°C and a boiling point of 1560°C.

5. How do the oxidation states of the Nitrogen family elements vary?

Ans. The Nitrogen family elements can exhibit multiple oxidation states. Nitrogen (N) commonly exhibits oxidation states of -3, +3, and +5. Phosphorus (P) can have oxidation states of -3, +3, and +5 as well. Arsenic (As) can show oxidation states ranging from -3 to +5, with +3 and +5 being the most common. Antimony (Sb) can have oxidation states of -3, +3, and +5. Bismuth (Bi) mainly exhibits the +3 oxidation state. The ability to exhibit multiple oxidation states allows these elements to form a wide range of compounds with different properties.

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	Nov 16, 2024 Last updated

Group 15 Properties (Nitrogen Family) for JEE2024 is part of JEE preparation. The notes and questions for Group 15 Properties (Nitrogen Family) have been prepared according to the JEE exam syllabus. Information about Group 15 Properties (Nitrogen Family) covers all important topics for JEE2024 Exam. Find important definitions, questions, notes, meanings, examples, exercises and tests below for Group 15 Properties (Nitrogen Family).

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