S=O bonds have inefficient orbital overlap making the sulfur atom electron-poor and electrophilic.Select answer from the options belowTrueFalse

Analyzing the Statement

1. Understanding S=O Bonds:

   • Sulfur (S) can form multiple bonds, including double bonds with oxygen (O). In a double bond such as S=O, the overlap of orbitals is crucial in determining the electronic properties of the molecule.

2. Orbital Overlap Efficiency:

   • The efficiency of orbital overlap affects the electron density around the atoms involved in the bond. Poor overlap typically leads to a lower density of electrons around the less electronegative atom.

3. Characterization of Sulfur:

   • Sulfur is less electronegative than oxygen, leading to a partial positive charge on sulfur when bonded to oxygen. This behavior indicates that the sulfur atom can act as an electrophile, attracting nucleophiles.

Conclusion

Given that S=O bonds indeed have inefficient orbital overlap, resulting in sulfur being electron-poor and electrophilic, the statement is:

Final Answer

True