1. Lewis Dot Structure
The Lewis dot structure for selenium tetrafluoride (SeF4) shows the central selenium atom surrounded by four fluorine atoms. Selenium has 6 valence electrons and each fluorine contributes 7 valence electrons. The structure has the selenium atom in the center with single bonds to each of the four fluorine atoms. Additionally, there are two lone pairs of electrons on the selenium atom.
2. Hybridization
The hybridization of selenium in SeF4 is sp3d. This means that one s orbital, three p orbitals, and one d orbital from selenium combine to form five sp3d hybrid orbitals. Four of these orbitals are used to form the Se-F bonds, while the remaining orbital contains a lone pair.
3. Electron Geometry
The electron geometry of SeF4 is trigonal bipyramidal. This geometry takes into account all electron pairs, including the lone pairs on the selenium atom. In this arrangement, the areas of electron density (the bonds and lone pairs) form a structure that resembles a triangle with a point above and below the center atom.
4. Molecular Geometry
The molecular geometry of SeF4 is see-saw. This is derived from the trigonal bipyramidal shape after accounting for the presence of the two lone pairs on the selenium atom, which influence the overall shape by pushing the fluorine atoms closer together.
5. Polarity
SeF4 is polar. This is due to the presence of the lone pairs on the selenium atom and the differences in electronegativity between selenium and fluorine. The asymmetrical shape of the molecule results in an uneven distribution of electron density, leading to a dipole moment. Thus, SeF4 is overall a polar molecule.