Based on molecular mass and boiling point of the five compounds in the table below, which should have the high?
est dipole moment:
first # molecular mass 2nd: boiling point
compound 1 244 203
compound 2 346 255
compound 3 250 138
compound 4 246 146
compound 5 241 100
i know its compound 2 and im reviewing an old test, but why is it compound 2?
You would expect the highest boiling point to be the highest molar mass (other things being equal). And the dipole moment makes it harder to escape the liquid when boiling; therefore, the higher dipole moment also leads to higher boiling points. Compound two has the highest boiling point and the highest molar mass of any of the others. It wins on both counts.
To determine which compound has the highest dipole moment based on the given information, we need to consider the molecular mass and boiling point of each compound.
Dipole moment is a measure of the separation of positive and negative charges in a molecule. It depends on the polarity of the bonds within the molecule and the molecular shape. Generally, larger differences in electronegativity between the atoms involved in the bond lead to a higher dipole moment.
In the case of the given compounds, we need to compare their molecular masses and boiling points to determine the trend. However, it's important to note that without additional information about the molecular structures of these compounds, we can only make an educated guess based on the given data.
Looking at the boiling points, compound 2 has the highest boiling point of 255°C. Boiling points are related to the intermolecular forces between molecules. Compounds with stronger intermolecular forces tend to have higher boiling points. These intermolecular forces can be influenced by factors such as molecular size, shape, and polarity.
Since compound 2 has the highest boiling point, it suggests that it likely has stronger intermolecular forces compared to the other compounds. One common intermolecular force is dipole-dipole interactions, which occur between polar molecules. In these interactions, the positive end of one molecule is attracted to the negative end of another molecule.
Based on this, we can infer that compound 2 likely has a higher dipole moment compared to the other compounds. It has a larger molecular mass and a higher boiling point, indicating that it may have a more polar structure with greater separation of charges.
It's important to note that this is a simplified explanation without knowing the molecular structures and other factors that could affect dipole moments accurately. Confirmation of the dipole moment would require a more detailed analysis, including the actual molecular structures of the compounds.