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Chapter 6: Problem 10

Is phosphorus trichloride, \(P C l_{3}\), a polar molecule? If it is, draw the dipole moment vector for the entire molecule and show where the \(\delta+\) and \(\delta-\) regions of the molecule are.

Short Answer

Expert verified
Phosphorus trichloride (PCl3) is a polar molecule due to its trigonal pyramidal structure and the electronegativity difference between Phosphorus (approx. \(2.19\)) and Chlorine (approx. \(3.16\)). There is a net dipole moment with the δ+ region located at the Phosphorus atom and δ- regions at the Chlorine atoms.

Step by step solution

01

Find the molecular structure of PCl3

To determine the polarity of PCl3, we first need to find its molecular structure. Phosphorus has 5 valence electrons, and each Chlorine atom has 7. When they bond, they form a trigonal pyramidal structure, with the Phosphorus atom in the center and the three Chlorine atoms surrounding it.
02

Determine Electronegativity Difference

Next, consider the electronegativity of Phosphorus and Chlorine atoms. Electronegativity is a measure of how strongly an atom attracts electrons in a bond. The greater the difference in electronegativity, the more polar the bond will be. The electronegativity value of Phosphorus is approximately \(2.19\) and that of Chlorine is approximately \(3.16\). There is an electronegativity difference of \(0.97\), which implies that the P-Cl bond is polar.
03

Identify the Direction of the Dipole Moment in P-Cl bonds

As Chlorine is more electronegative than Phosphorus, the electrons in the P-Cl bond are pulled closer to Chlorine, giving a partial negative charge (δ-) to the Chlorine atoms and a partial positive charge (δ+) to the Phosphorus atom. The P-Cl bond dipoles have their positive ends towards the Phosphorus atom and their negative ends towards the Chlorine atoms.
04

Determine the Overall Dipole Moment of PCl3

To find the overall dipole moment of PCl3, we need to consider the dipole moments of all three P-Cl bonds in the trigonal pyramidal structure. Since the P-Cl bond dipoles do not cancel each other out due to the molecular geometry, there is a net dipole moment present in PCl3. This means PCl3 is a polar molecule.
05

Draw the Dipole Moment Vector and Identify δ+ and δ- Regions

To represent the dipole moment in PCl3: 1. Draw the PCl3 molecule in its trigonal pyramidal structure. 2. Mark the Phosphorus atom with a δ+ symbol and the Chlorine atoms with δ- symbols. 3. Draw an arrow from the Phosphorus atom to each Chlorine atom, indicating the direction of the dipole moment in each P-Cl bond. 4. Draw a resultant dipole moment vector from the Phosphorus atom (δ+) towards the center of the triangle formed by the three Chlorine atoms (δ-). As a result, PCl3 is a polar molecule with the δ+ region at the Phosphorus atom and the δ- regions at the Chlorine atoms.

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Most popular questions from this chapter

Consider \(\mathrm{SO}_{2}\) and \(\mathrm{CO}_{2}\). Both have polar covalent bonds. One of these molecules is polar and the other is nonpolar. Which is which and why?

List the steps you take to decide (a) whether or not. a covalent bond is polar and (b) whether or not a molecule is polar.

Using lines, solid wedges, and dashed wedges, draw the threedimensional shape of ethane, \(\mathrm{C}_{2} \mathrm{H}_{6}\). Indicate the numeric value of all bond angles.

Consider the molecule \(\mathrm{BrCl}_{3}\). (a) Draw a dot diagram for the molecule. (b) Predict the molecule's electron group geometry. (c) Predict the molecule's shape (name the shape and draw it using wedges, lines, and broken lines, and indicate the ideal value of the bond angles). (d) Predict if the molecule is polar or nonpolar. If polar, draw the dipole moment for the molecule.

Consider the molecule \(\mathrm{SO}_{3}\). (a) Draw the dot diagram. (b) Draw the molecule's three-dimensional shape, and label the numeric value of all bond angles. (c) What is the shape of this molecule? (d) Draw in the individual bond dipole moments. (e) Is the molecule polar? If yes, draw the molecular dipole moment vector.
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