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Lewis approach to chemical bond - Chemical Bonding & Molecular Structure Video Lecture - Class 11

FAQs on Lewis approach to chemical bond - Chemical Bonding & Molecular Structure Video Lecture - Class 11

1. What is Lewis approach to chemical bond?
Ans. The Lewis approach to chemical bonding, developed by American chemist Gilbert N. Lewis, describes the formation of chemical bonds in terms of the sharing or transfer of electrons between atoms. According to Lewis, atoms tend to gain, lose, or share electrons to acquire a stable electron configuration similar to that of noble gases.
2. How does the Lewis approach explain the formation of chemical bonds?
Ans. According to the Lewis approach, the formation of chemical bonds occurs through the sharing of electrons between atoms. Atoms can either share electrons equally in covalent bonds or transfer electrons from one atom to another in ionic bonds. The sharing or transfer of electrons allows atoms to achieve a stable electron configuration and increases the stability of the overall system.
3. What are Lewis structures and how do they represent chemical bonds?
Ans. Lewis structures, also known as Lewis dot structures, are diagrams that represent the arrangement of atoms and valence electrons in a molecule or ion. In Lewis structures, the valence electrons of each atom are represented by dots or lines. Dots represent electrons, while lines represent chemical bonds. By counting the valence electrons and arranging them around the atoms, Lewis structures provide a visual representation of how atoms are bonded in a molecule or ion.
4. How does the Lewis approach explain the concept of lone pairs?
Ans. In the Lewis approach, lone pairs are represented as unshared pairs of electrons. These are electrons that are not involved in bonding and are localized on a specific atom. Lone pairs play a crucial role in determining the shape and reactivity of molecules. They can influence the polarity of bonds, participate in hydrogen bonding, and affect the overall stability of a molecule.
5. What are the limitations of the Lewis approach to chemical bonding?
Ans. While the Lewis approach provides a useful framework for understanding chemical bonding, it has certain limitations. It does not account for the concept of molecular orbitals, which is essential for explaining the bonding in complex molecules. The Lewis approach also assumes that electrons are localized around specific atoms, ignoring the delocalization of electrons in some molecules. Additionally, it does not account for the directional nature of bonds in molecules, which is important for understanding molecular shapes and properties.
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