Comment on the molecular hybridization in each of the two carbons in ethane. What is the bond angle in each of the carbon atom?
In ethane (C2H6), each carbon atom is sp3 hybridized. This means that in each carbon atom, one S orbital and three P orbitals combine to form four hybridized orbitals called sp3 orbitals. These orbitals are arranged in a tetrahedral geometry around each carbon atom.
The bond angle in each carbon atom in ethane is approximately 109.5 degrees. This is because the four sp3 orbitals are arranged as far apart from each other as possible in three-dimensional space, resulting in a tetrahedral arrangement with bond angles of 109.5 degrees.
In ethane (C2H6), each carbon atom forms four covalent bonds, resulting in a tetrahedral arrangement of its electron pairs. The hybridization of each carbon atom in ethane is sp3.
To understand the hybridization, let's look at the electronic configuration of carbon. The atomic number of carbon is 6, and its electronic configuration is 1s2 2s2 2p2. In the process of hybridization, one 2s orbital and three 2p orbitals mix to form four sp3 hybrid orbitals.
Each sp3 hybrid orbital overlaps with a hydrogen 1s orbital to form a sigma (σ) bond. Thus, each carbon atom in ethane is sp3 hybridized, with four sigma bonds.
The bond angle between the carbon atom and any two of its attached hydrogen atoms in ethane is approximately 109.5 degrees. This angle reflects the tetrahedral arrangement of electron pairs around the carbon atom due to its sp3 hybridization.