SF2 polar or non polar
The Correct Answer and Explanation is :
SF2 (sulfur difluoride) is a polar molecule. To understand why, we need to look at the molecular structure, electronegativity differences, and the distribution of electron density.
Molecular Geometry:
SF2 has a bent or V-shaped molecular geometry. This is because sulfur (S) is the central atom, and it forms two bonds with fluorine (F) atoms. The sulfur atom has two lone pairs of electrons, which create a repulsion that pushes the fluorine atoms closer together, resulting in the bent shape. The bond angle between the two fluorine atoms is approximately 98°, which is smaller than the ideal 120° for a trigonal planar structure.
Electronegativity:
Fluorine is much more electronegative than sulfur (F = 3.98, S = 2.58 on the Pauling scale). This means that the fluorine atoms attract the shared electrons in the S-F bonds more strongly than sulfur does. As a result, the electron density is skewed toward the fluorine atoms, creating partial negative charges (δ-) on the fluorines and a partial positive charge (δ+) on the sulfur atom.
Dipole Moment:
Due to the difference in electronegativity between sulfur and fluorine, and the bent shape of the molecule, the individual bond dipoles do not cancel out. The overall dipole moment points from the sulfur atom (positive charge) toward the fluorine atoms (negative charge). This creates an overall dipole moment in the molecule, which confirms its polarity.
Conclusion:
SF2 is polar because it has a bent molecular geometry, a significant difference in electronegativity between sulfur and fluorine, and a resultant dipole moment. These factors cause the molecule to have an uneven distribution of charge, making it polar.