Which of the following compounds is expected to have the strongest interaction between its molecules? CO2, NO2, SO2, H2S
Which of the following compounds is expected to have the weakest interactions between its molecules? CO2
Strongest interaction?
SO2
so2 deltaEN=1(having the greatest intermolecular forces of the polar bonds listed), deltaEN of h2s=.4 (having the weakest intermolecular forces of the polar bonds listed)
To determine which compound is expected to have the strongest interaction between its molecules, we need to consider the intermolecular forces present in each compound. Intermolecular forces are the forces of attraction between molecules that influence the physical properties of substances.
Here are the intermolecular forces present in each compound:
1. CO2 (carbon dioxide): CO2 is a linear molecule, and the only intermolecular force between its molecules is London dispersion forces (also known as Van der Waals forces). These forces occur due to temporary fluctuations in electron distribution, creating temporary dipoles that induce dipoles in nearby molecules.
2. NO2 (nitrogen dioxide): NO2 is a bent molecule with a lone electron on the central nitrogen atom. It exhibits two types of intermolecular forces: London dispersion forces and dipole-dipole interactions. The lone electron on nitrogen makes it a polar molecule, which leads to dipole-dipole interactions. London dispersion forces also play a role.
3. SO2 (sulfur dioxide): SO2 is a bent molecule similar to NO2. It also exhibits London dispersion forces and dipole-dipole interactions due to its polar nature.
4. H2S (hydrogen sulfide): H2S is a bent molecule, and similar to the previous compounds, it displays London dispersion forces and dipole-dipole interactions.
Among these compounds, dipole-dipole interactions are generally stronger forces than London dispersion forces. It means that compounds with dipole-dipole interactions tend to have stronger intermolecular forces.
Comparing the compounds, we can see that NO2 and SO2 both have dipole-dipole interactions in addition to London dispersion forces. These molecules have a polar bond due to the electronegativity difference between the central atom and the adjacent atoms, resulting in a net molecular dipole. On the other hand, CO2 and H2S do not have net dipoles since their molecular shapes cancel the dipole moments.
Therefore, the compounds NO2 and SO2 are expected to have the strongest interaction between their molecules due to the presence of dipole-dipole interactions in addition to London dispersion forces.