In each pair of compounds, pick the one with the higher boiling point. Explain your reasoning. c. CH₄ or CH₃CH₃

Video transcript

Hey everyone where ask which between silicon tetrachloride and hex like laura Dis Elaine has a higher boiling point first let's go ahead and draw out our Lewis structures. Starting off with silicon tetrachloride. We know that silicon is going to be our central atom And this will be connected to four chlorine And each corinne will have three lone pairs to fill its octet. Now let's go ahead and draw out hexafluoride, insulin. So we have to silicon atoms and these will be bonded to one another as our central atoms and each one will also be bonded to three chlorine And each chlorine will also have three lone pairs. Looking at our structures we can go ahead and assess their disciple moments and as we can see right here our disciple moments for each one are going to cancel out. And because our di pole moments cancel out, this tells us that we have non polar compounds which means that we have London dispersion forces and as we've learned the higher the boiling point our inter molecular forces will be stronger. And since we only have London dispersion forces will have to look at our molar masses and we know that as our molar mass increases, our boiling point will also increase. Now comparing these two compounds we can see that the one with the higher boiling point is going to be hex like loro discipline due to the high molar mass. Now I hope that made sense. And let us know if you have any questions