The molecular geometry of the PF3 molecule is __________, and this molecule is __________.

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Step 1: Before diving into the solution, let's recall the relevant concept and formula:. - VSEPR Theory (Valence Shell Electron Pair Repulsion): This theory helps us predict molecular geometry based on the repulsion of electron pairs in the valence shell of the central atom. Now, let's solve the problem step-by-step: Step 2: . Identify the central atom and the number of electron pairs around it. - The central atom in PF3 is Phosphorus (P). - Phosphorus has 5 electrons in its outer shell, and each Fluorine atom contributes 1 electron, resulting in a total of 6 electron pairs. 	ext{Central atom: } \mathrm{P}, 	ext{ Total electron pairs: } 6 Step 3: . Apply the VSEPR theory to determine the molecular geometry. - With 6 electron pairs, the molecular geometry is trigonal bipyramidal. - However, since there are only 3 ligands (Fluorine atoms) attached to the central atom, the actual molecular geometry is a distorted tetrahedral shape, where one position is occupied by a lone pair. - This geometry is called "T-shaped." 	ext{Molecular geometry: } \mathrm{T}	ext{-shaped} Step 4: . Determine the molecule's polarity based on the molecular geometry and electronegativity differences. - Fluorine is more electronegative than Phosphorus, so the P-F bonds are polar. - However, the lone pair on Phosphorus creates a significant distortion in the T-shape, which cancels out the dipoles from the P-F bonds, resulting in a nonpolar molecule. 	ext{Molecule polarity: } 	ext{Nonpolar} Final Answer: The molecular geometry of the PF3 molecule is T-shaped, and this molecule is nonpolar.

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