Electronic, Molecular shape and bond angles of C2H6, C2H4, C2H2, H2O, NH3, CCL4, C6H6, CO2, CH3OH, CH3NH2,CH3OCH3, CH3COCH3, CHOOH, CHOOCH3, CH2O, CHONH2.
The Correct Answer and Explanation is :
To answer your question, let’s break down the molecular shapes, electronic configurations, and bond angles of each molecule in your list. I’ll explain how to determine these based on their VSEPR (Valence Shell Electron Pair Repulsion) theory and molecular structures.
- C2H6 (Ethane)
- Electronic Shape: Tetrahedral (due to sp³ hybridization on both carbon atoms)
- Bond Angles: 109.5° (for each C-H bond and between the two C-H bonds)
- C2H4 (Ethene)
- Electronic Shape: Trigonal Planar (due to sp² hybridization)
- Bond Angles: 120° (C=C bond angle)
- C2H2 (Ethyne)
- Electronic Shape: Linear (due to sp hybridization)
- Bond Angles: 180° (C≡C bond angle)
- H2O (Water)
- Electronic Shape: Tetrahedral (due to sp³ hybridization of oxygen)
- Bond Angles: 104.5° (due to lone pairs on oxygen pushing the H atoms closer)
- NH3 (Ammonia)
- Electronic Shape: Tetrahedral (sp³ hybridized nitrogen)
- Bond Angles: 107.3° (due to lone pair on nitrogen)
- CCl4 (Carbon Tetrachloride)
- Electronic Shape: Tetrahedral (sp³ hybridized carbon)
- Bond Angles: 109.5° (Cl-C-Cl bond angle)
- C6H6 (Benzene)
- Electronic Shape: Trigonal Planar (due to sp² hybridization of carbon atoms)
- Bond Angles: 120° (C-C-C bond angle)
- CO2 (Carbon Dioxide)
- Electronic Shape: Linear (sp hybridized carbon)
- Bond Angles: 180° (O=C=O bond angle)
- CH3OH (Methanol)
- Electronic Shape: Tetrahedral (sp³ hybridized carbon and oxygen)
- Bond Angles: 109.5° (H-C-H bond angle)
- CH3NH2 (Methylamine)
- Electronic Shape: Tetrahedral (sp³ hybridized carbon and nitrogen)
- Bond Angles: 107.3° (H-N-H bond angle)
- CH3OCH3 (Dimethyl Ether)
- Electronic Shape: Tetrahedral (sp³ hybridized carbon and oxygen)
- Bond Angles: 109.5° (C-O-C bond angle)
- CH3COCH3 (Acetone)
- Electronic Shape: Trigonal Planar (sp² hybridized carbonyl carbon)
- Bond Angles: 120° (C-C-C bond angle)
- CHOOH (Formic Acid)
- Electronic Shape: Trigonal Planar (sp² hybridized carbon)
- Bond Angles: 120° (C=O and C-O-H bond angles)
- CHOOCH3 (Methyl Formate)
- Electronic Shape: Trigonal Planar (sp² hybridized carbonyl carbon)
- Bond Angles: 120° (C=O bond angles)
- CH2O (Formaldehyde)
- Electronic Shape: Trigonal Planar (sp² hybridized carbon)
- Bond Angles: 120° (C=O bond angle)
- CHONH2 (Glycine)
- Electronic Shape: Tetrahedral (sp³ hybridized carbon and nitrogen)
- Bond Angles: 109.5° (H-C-H bond angle)
Explanation:
The molecular shape and bond angles depend on the hybridization of atoms involved in bonding and the number of bonding pairs and lone pairs around the central atoms. The general trend follows the VSEPR theory, which states that electron pairs (bonding and lone pairs) repel each other and arrange themselves to minimize repulsion. For example, in methane (CH4), the electron pairs are arranged in a tetrahedral shape around the central carbon atom to achieve the lowest energy configuration. Similarly, molecules like CO2, which have linear bonds, and H2O, which is bent due to lone pairs on oxygen, exhibit different angles based on the number of electron pairs surrounding the atoms.