Textbook Question
Match each of the formulas (a to c) with the correct diagram (1 to 3) of its shape, and name the shape; indicate if each molecule is polar or nonpolar.
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a. PBr3
4. Molecular Compounds
Molecular Polarity (Simplified)
Multiple Choice
Determine if difluorine selenide, F2Se, is polar or nonpolar.
A
polar
B
nonpolar
Verified step by step guidance1
Identify the molecular geometry of difluorine selenide (F2Se). Selenium (Se) is the central atom, and it is bonded to two fluorine (F) atoms. Consider the electron pair geometry around the selenium atom.
Determine the number of valence electrons for selenium and fluorine. Selenium has 6 valence electrons, and each fluorine has 7 valence electrons. Calculate the total number of valence electrons in the molecule.
Use the VSEPR (Valence Shell Electron Pair Repulsion) theory to predict the shape of the molecule. Selenium has two bonding pairs and two lone pairs of electrons, leading to a bent or angular shape.
Assess the electronegativity of the atoms. Fluorine is more electronegative than selenium, which means the F-Se bonds are polar, with a partial negative charge on the fluorine atoms.
Evaluate the symmetry of the molecule. Due to the bent shape, the dipole moments do not cancel out, resulting in a net dipole moment. Therefore, F2Se is a polar molecule.
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