NEET Exam > NEET Videos > Chemistry Class 12 > Boron Family: Trends & Properties
Boron Family: Trends & Properties Video Lecture | Chemistry Class 12 - NEET
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FAQs on Boron Family: Trends & Properties Video Lecture - Chemistry Class 12 - NEET
| 1. What are some key properties of the Boron family? |  |
Ans. The Boron family, also known as Group 13 elements, includes boron, aluminum, gallium, indium, and thallium. Some key properties of this family include having three valence electrons, forming compounds with a +3 oxidation state, and exhibiting metallic and non-metallic characteristics.
| 2. What is the trend in atomic size within the Boron family? | |
Ans. As we move down the Boron family, the atomic size generally increases. This trend is due to the addition of new energy levels (shells) as we move from boron to thallium. Thallium, being the largest element in the family, has the largest atomic size.
| 3. How does the reactivity of the Boron family change as we move down the group? | |
Ans. The reactivity of the Boron family generally increases as we move down the group. Boron is the least reactive element in the family, while thallium is the most reactive one. This trend can be attributed to the decrease in ionization energy and increase in atomic size as we move down the group.
| 4. What are some common applications of the Boron family elements? | |
Ans. The Boron family elements have various applications. Boron, for example, is used in the production of borosilicate glass, as a neutron absorber in nuclear reactors, and as a component in detergents. Aluminum is widely used in the manufacturing of aircraft, packaging materials, and construction. Gallium finds applications in semiconductors and LEDs.
| 5. How does the melting and boiling points change within the Boron family? | |
Ans. The melting and boiling points of the Boron family elements generally decrease as we move down the group. Boron has a relatively high melting and boiling point, while thallium has the lowest among the family members. This trend can be attributed to the weakening metallic bonding and the increase in atomic size as we move down the group.
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