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Chapter 10: Problem 90

So-called greenhouse gases, which contribute to global warming, have a dipole moment or can be bent or distorted into shapes that have a dipole moment. Which of the following gases are greenhouse gases: \(\mathrm{N}_{2}, \mathrm{O}_{2}, \mathrm{O}_{3}, \mathrm{CO}, \mathrm{CO}_{2}, \mathrm{NO}_{2}, \mathrm{~N}_{2} \mathrm{O},\) \(\mathrm{CH}_{4}, \mathrm{CFCl}_{3} ?\)

Short Answer

Expert verified
The greenhouse gases among the given gases are \(O_{3}\), \(CO\), \(CO_{2}\), \(NO_{2}\), \(N_{2}O\), \(CH_{4}\) and \(CFCl_{3}\).

Step by step solution

01

Understand Dipole Moment

The dipole moment is a measure of the polarity of a molecule. Nonpolar molecules like \(N_{2}\) and \(O_{2}\) have no dipole moment because they consist of two similar atoms sharing electrons equally. Greenhouse gases tend to be polar or capable of becoming polar, so these two are likely not greenhouse gases.
02

Apply Molecular Structure Knowledge

Evaluate the remaining molecules for their polarity or potential to become polar. \(O_{3}\), \(CO\), \(CO_{2}\), \(NO_{2}\), \(N_{2}O\), \(CH_{4}\) and \(CFCl_{3}\) do have a dipole moment due to the difference in electronegativity of the atoms or asymmetry of their molecular structures which makes them candidates for being greenhouse gases.
03

Confirm with Real World Knowledge

It's known that gases like \(CO_{2}\), \(NO_{2}\), \(CH_{4}\) and \(CFCl_{3}\) are indeed greenhouse gases in our atmosphere. This validates our analysis.

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Most popular questions from this chapter

Given that the order of molecular orbitals for \(\mathrm{NO}\) is similar to that for \(\mathrm{O}_{2}\), arrange the following species in increasing bond orders: \(\mathrm{NO}^{2-}, \mathrm{NO}^{-}, \mathrm{NO}, \mathrm{NO}^{+}\) \(\mathrm{NO}^{2+}\)

Write the ground-state electron configuration for \(\mathrm{B}_{2}\). Is the molecule diamagnetic or paramagnetic?

Assume that the third-period element phosphorus forms a diatomic molecule, \(\mathrm{P}_{2}\), in an analogous way as nitrogen does to form \(\mathrm{N}_{2}\). (a) Write the electronic configuration for \(\mathrm{P}_{2}\). Use \(\left[\mathrm{Ne}_{2}\right]\) to represent the electron configuration for the first two periods. (b) Calculate its bond order. (c) What are its magnetic properties (diamagnetic or paramagnetic)?

Which of the following ions possess a dipole moment: (a) \(\mathrm{ClF}_{2}^{+},\) (b) \(\mathrm{ClF}_{2}^{-},\) (c) \(\mathrm{IF}_{4}^{+},\) (d) \(\mathrm{IF}_{4}^{-} ?\)

For each pair listed here, state which one has a higher first ionization energy and explain your choice: (a) \(\mathrm{H}\) or \(\mathrm{H}_{2},\) (b) \(\mathrm{N}\) or \(\mathrm{N}_{2},\) (c) \(\mathrm{O}\) or \(\mathrm{O}_{2},\) (d) \(\mathrm{F}\) or \(\mathrm{F}_{2}\).
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