4. CHEMICAL BONDING AND MOLECULAR STRUCTURE
This chapter delves into the principles of chemical bonding, exploring the Kössel-Lewis approach, the octet rule, covalent bonding, VSEPR theory, valence bond theory, and molecular orbital theory. Important concepts such as hybridization, resonance, and hydrogen bonding are also discussed, providing a comprehensive understanding of how atoms combine to form molecules and the resulting molecular geometries.
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4.3.1Bond Length
Bond length is the equilibrium distance between the nuclei of bonded atoms,...
What we have learnt
- Chemical bonding is essential for the formation of stable molecules and compounds.
- The octet rule serves as a guideline for predicting how atoms combine based on achieving a stable electronic configuration.
- Various theories like VSEPR, valence bond, and molecular orbital theory provide frameworks for understanding molecular geometry and bonding.
Key Concepts
- -- KösselLewis Approach
- A method for explaining chemical bonding based on electron transfer and the stable octet configuration of noble gases.
- -- Octet Rule
- A postulate that suggests atoms tend to combine in a way that gives them eight electrons in their valence shell, achieving stability.
- -- Hybridization
- The process of combining atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons in chemical bonding.
- -- VSEPR Theory
- A theory used to predict the geometry of individual molecules based on the repulsion between electron pairs.
- -- Resonance
- The concept that certain molecules cannot be adequately described by a single Lewis structure and instead are represented by multiple structures.
- -- Hydrogen Bonding
- An attractive interaction between a hydrogen atom bonded to an electronegative atom and another electronegative atom.
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