In each pair of compounds, pick the one with the higher boiling point. Explain your reasoning. b. CS₂ or CO₂

Video transcript

hey everyone were asked which between nitrogen try fluoride and nitrogen tri chloride has a higher boiling point. To answer this question, let's first go ahead and draw out our lewis structures. Starting with nitrogen try fluoride, nitrogen will be our central atom and this will have three florins single bonded to it. And we will have one lone pair surrounding our nitrogen and three lone pairs surrounding each flooring to fill its octet, drawing out nitrogen tri chloride. This will have a similar structure and that nitrogen will be single bonded to three chlorine that have three lone pairs and we will have one lone pair surrounding our nitrogen atom. Looking at these two structures, we can see that we have a net dipole moment which means that we have polar compounds. And because we have polar compounds, this means that we have dipole dipole and London dispersion forces present. And as we've learned a higher boiling point will mean that we will have stronger inter molecular forces. We also know that as our molar mass increases, our boiling point will also increase. So since these two have the same inter molecular forces presence, we will have to look at our molar masses. And since nitrogen tri chloride has a higher molar mass than nitrogen try fluoride. This means that it will have a higher boiling point. Now I hope that made sense. And let us know if you have any questions