Open 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. (6.6, 6.8, 6.9)1. 2. 3. a. PBr₃
10. Chemical Bonding
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.
Determine the number of valence electrons for each atom. Selenium has 6 valence electrons, and each fluorine has 7 valence electrons.
Draw the Lewis structure for F2Se. Place selenium in the center with a single bond to each fluorine atom, and distribute the remaining electrons to satisfy the octet rule.
Analyze the molecular shape using VSEPR theory. With two bonding pairs and two lone pairs on the central selenium atom, the shape is bent or angular.
Evaluate the electronegativity difference between selenium and fluorine. Since fluorine is more electronegative, the bonds are polar. The bent shape means the dipoles do not cancel, resulting in a polar molecule.
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