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Of the following compounds, which has the strongest dipole?

Select one:

a. [tex]CCl_4[/tex]
b. BrCl
c. [tex]SiO_2[/tex]
d. [tex]PCl_3[/tex]
e. [tex]H_2O[/tex]

Sagot :

GinnyAnswer
To determine which compound has the strongest dipole moment, we need to consider both the molecular geometry and the electronegativity differences between the atoms in each molecule.

1. Carbon Tetrachloride ([tex]$CCl_4$[/tex]):
- Structure: Tetrahedral
- Electronegativity difference between C and Cl creates individual C-Cl bond dipoles.
- However, the tetrahedral shape is symmetrical, and the dipoles cancel each other out.
- Result: No net dipole moment (non-polar molecule).

2. Bromine Chloride (BrCl):
- Structure: Linear
- Electronegativity difference between Br and Cl creates a bond dipole.
- While this molecule has a dipole moment, it is moderate because the electronegativity difference is not extremely large.
- Result: Moderate dipole moment.

3. Silicon Dioxide ([tex]$SiO_2$[/tex]):
- Structure: In its most common form (quartz), [tex]$SiO_2$[/tex] is a network solid rather than a discrete molecule.
- In a linear molecular context, as two Si=O bonds (like CO2), the dipoles cancel each other.
- Result: No net dipole moment (non-polar molecule).

4. Phosphorus Trichloride ([tex]$PCl_3$[/tex]):
- Structure: Trigonal pyramidal
- The electronegativity difference between P and Cl creates bond dipoles.
- The molecular shape is asymmetrical, which means the dipoles do not cancel out completely.
- Result: Strong dipole moment.

5. Water ([tex]$H_2O$[/tex]):
- Structure: Bent (due to lone pairs on oxygen)
- The electronegativity difference between H and O creates bond dipoles.
- The bent shape means that the dipoles do not cancel each other out.
- Result: Very strong dipole moment due to the combination of shape and high electronegativity difference.

Given these analyses, the strongest dipole moment is found in the molecule with both a large electronegativity difference and an asymmetrical shape that prevents dipole cancellation. Water ([tex]$H_2O$[/tex]) meets these criteria best, as it has a strong dipole moment due to its bent shape and significant electronegativity difference between hydrogen and oxygen.

Therefore, the compound with the strongest dipole moment of the given options is:

e. [tex]$H_2O$[/tex]
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