Answer:
Bonds that are formed from orbitals lying in the same plane and overlapping end-to-end are known as sigma bonds. These bonds occur along the internuclear axis, which is the line connecting the two atoms involved in the bond. 1. Sigma bonds: Sigma (σ) bonds are formed by the overlap of atomic orbitals along the internuclear axis. The orbitals involved can be s orbitals, p orbitals, or hybridized orbitals. Sigma bonds are the strongest type of covalent bonds and are present in various molecules and compounds.
Step-by-step explanation:
2. Overlap in the same plane: When orbitals lie in the same plane and overlap end-to-end, they form sigma bonds. This means that the electron density between the two atoms is concentrated along the internuclear axis. 3. Examples: - In a simple diatomic molecule like hydrogen (H2), each hydrogen atom has one 1s atomic orbital. When the two hydrogen atoms come together, their 1s orbitals overlap end-to-end along the internuclear axis, forming a sigma bond. - In ethene (C2H4), each carbon atom has three sp2 hybrid orbitals and one unhybridized p orbital. The sp2 hybrid orbitals overlap with the hydrogen atoms to form sigma bonds, while the unhybridized p orbitals overlap end-to-end to form a sigma bond between the two carbon atoms. In summary, sigma bonds are formed by the overlap of orbitals lying in the same plane and end-to-end along the internuclear axis. They are strong covalent bonds and can be found in various molecules and compounds. Examples include the sigma bonds in hydrogen (H2) and the carbon-carbon sigma bond in ethene (C2H4).