NEET Exam > NEET Videos > Chemistry Class 11 > Octet Rule & its Limitations
Octet Rule & its Limitations Video Lecture | Chemistry Class 11 - NEET
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FAQs on Octet Rule & its Limitations Video Lecture - Chemistry Class 11 - NEET
| 1. What is the octet rule? |  |
Ans. The octet rule is a principle in chemistry that states that atoms tend to gain, lose, or share electrons in order to achieve a stable electron configuration with eight valence electrons, similar to the noble gases.
| 2. What are valence electrons? | |
Ans. Valence electrons are the electrons located in the outermost energy level of an atom. They are involved in chemical bonding and determine the reactivity of an element.
| 3. What are the limitations of the octet rule? | |
Ans. While the octet rule is useful in explaining the formation of many compounds, there are exceptions and limitations to its application. Some elements, such as hydrogen and helium, can achieve stability with just two electrons. Elements beyond the second period of the periodic table can have expanded octets, meaning they can have more than eight valence electrons. Additionally, compounds involving transition metals often do not follow the octet rule.
| 4. How does the octet rule apply to ionic compounds? | |
Ans. In ionic compounds, atoms transfer electrons to achieve a complete outer shell and form ions with a full octet. For example, sodium (Na) donates an electron to chlorine (Cl) to form sodium chloride (NaCl), where sodium becomes a positively charged ion (Na+) and chlorine becomes a negatively charged ion (Cl-).
| 5. Is the octet rule always followed in covalent compounds? | |
Ans. While the octet rule is generally followed in covalent compounds, there are exceptions. Some elements, such as boron and beryllium, can form stable compounds with fewer than eight valence electrons. Additionally, elements beyond the second period of the periodic table can have expanded octets and accommodate more than eight electrons in their valence shells.
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Oct 23, 2024 Last updated |
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