QQuestionChemistry
QuestionChemistry
"Consider a molecule of PBr^3, and determine if each of the following statements is True or False.
1) In the best Lewis structure, the central atom has an expanded octet. [ Select ] [""True"", ""False""]
2) The molecular geometry and the electron geometry are the same. [ Select ] [""False"", ""True""]
3) The Br−P−Br bond angle is equal to 120°. [ Select ] [""True"", ""False""]
4) It is a nonpolar molecule. [ Select ] [""False"", ""True""]
5) The hybridization scheme around the central atom is sp^2. [ Select ] [""False"", ""True""] "
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Answer
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Step 1I will solve each statement step-by-step as instructed.
Step 2
In the best Lewis structure, the central atom has an expanded octet.
Final Answer
2. The molecular geometry and the electron geometry are the same. Step 1: Determine the molecular geometry. PBr^3 has a trigonal bipyramidal molecular geometry with a seesaw shape. This is due to the central atom (P) forming 3 bonds and having 1 lone pair of electrons. Step 2: Determine the electron geometry. Electron geometry considers all electron pairs (bonding and lone) around the central atom. With 3 bonding pairs and 1 lone pair, the electron geometry is a tetrahedral shape. 3. The Br−P−Br bond angle is equal to 120°. Step 1: Determine the bond angle for the trigonal bipyramidal molecular geometry with a seesaw shape. The bond angle for this geometry is not 120°. The bond angle for the Br-P-Br bonds is approximately 109.5° (tetrahedral angle minus 35.3° due to lone pair repulsion). 4. It is a nonpolar molecule. Step 1: Determine if the molecule is polar or nonpolar. PBr^3 is a polar molecule due to the presence of polar bonds (P-Br) and the uneven distribution of electron density. 5. The hybridization scheme around the central atom is sp^2. Step 1: Determine the hybridization of the central atom. Phosphorus (P) forms 3 bonds with Bromine (Br) atoms. Therefore, the hybridization scheme around the central atom is sp^3, not sp^2.
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