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Chapter 18: Problem 2

Molecules in the upper atmosphere tend to contain double and triple bonds rather than single bonds. Suggest an explanation. [Section 18.1]

Short Answer

Expert verified
Molecules in the upper atmosphere tend to contain double and triple bonds rather than single bonds due to their greater stability under high-energy conditions, such as intense radiation and the presence of high-energy particles. This stability is mainly attributed to the stronger and shorter bonds, which make these molecules less susceptible to being broken apart and better suited to withstand the harsh conditions of the upper atmosphere.

Step by step solution

01

Understanding Single, Double, and Triple Bonds

A single bond is formed when two atoms share one pair of electrons, while a double bond involves the sharing of two pairs of electrons, and a triple bond involves the sharing of three pairs of electrons. Generally, as the number of shared electron pairs increases, the bond becomes stronger and shorter, leading to a more stable molecule.
02

Conditions in the Upper Atmosphere

The upper atmosphere is an environment with high-energy particles and intense radiation. Ultraviolet (UV) radiation from the Sun, for example, can split apart molecules and create highly reactive species, such as free radicals. Molecules in this region must be able to withstand these conditions and remain stable under high-energy interactions.
03

Stability of Molecules with Double and Triple Bonds

Molecules with double and triple bonds tend to be more stable under high-energy conditions in the upper atmosphere. Due to their shorter bond lengths and stronger bonds, they are less susceptible to being broken apart by radiation and other high-energy particles. Additionally, these molecules often have fewer overall bonds, allowing them to better withstand the energetic environment of the upper atmosphere.
04

Conclusion: Why Molecules Contain Double and Triple Bonds in the Upper Atmosphere

In conclusion, molecules in the upper atmosphere tend to contain double and triple bonds rather than single bonds due to their greater stability under high-energy conditions, which is mainly attributed to the stronger and shorter bonds. These characteristics make them better suited to withstand the harsh conditions of the upper atmosphere, such as intense radiation and the presence of high-energy particles.

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Most popular questions from this chapter

(a) Explain why \(\mathrm{Mg}(\mathrm{OH})_{2}\) precipitates when \(\mathrm{CO}_{3}{ }^{2-}\) ion is added to a solution containing \(\mathrm{Mg}^{2+}\) - (b) Will \(\mathrm{Mg}(\mathrm{OH})_{2}\) precipitate when \(4.0 \mathrm{~g}\) of \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) is added to \(1.00 \mathrm{~L}\) of a solution containing 125 Ppm of \(\mathrm{Mg}^{2+}\) ?

In the lime soda process at one time used in large scale municipal water softening, calcium hydroxide prepared from lime and sodium carbonate are added to precipitate \(\mathrm{Ca}^{2+}\) as \(\mathrm{CaCO}_{3}(s)\) and \(\mathrm{Mg}^{2+}\) as \(\mathrm{Mg}(\mathrm{OH})_{2}(\mathrm{~s})\) : $$ \begin{gathered} \mathrm{Ca}^{2+}(a q)+\mathrm{CO}_{3}{ }^{2-}(a q) \longrightarrow \mathrm{CaCO}_{3}(s) \\ \mathrm{Mg}^{2+}(a q)+2 \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{MgOH}_{2}(a q) \end{gathered} $$ How many moles of \(\mathrm{Ca}(\mathrm{OH})_{2}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) should be added to soften \(1200 \mathrm{~L}\) of water in which $$ \begin{aligned} {\left[\mathrm{Ca}^{2+}\right] } &=5.0 \times 10^{-4} \mathrm{M} \text { and } \\\ {\left[\mathrm{Mg}^{2+}\right] } &=7.0 \times 10^{-4} \mathrm{M} \end{aligned} $$

Air pollution in the Mexico City metropolitan area is among the worst in the world. The concentration of ozone in Mexico City has been measured at \(441 \mathrm{ppb}(0.441 \mathrm{ppm})\). Mexico City sits at an altitude of 7400 feet, which means its atmospheric pressure is only \(0.67\) atm. (a) Calculate the partial pressure of ozone at \(441 \mathrm{Ppb}\) if the atmospheric pressure is \(0.67 \mathrm{~atm}\). (b) How many ozone molecules are in \(1.0 \mathrm{~L}\) of air in Mexico City? Assume \(T=25^{\circ} \mathrm{C}\).

The main reason that distillation is a costly method for purifying water is the high energy required to heat and vaporize water. (a) Using the density, specific heat, and heat of vaporization of water from Appendix B, calculate the amount of energy required to vaporize \(1.00 \mathrm{gal}\) of water beginning with water at \(20^{\circ} \mathrm{C}\). (b) If the energy is provided by electricity costing \(\$ 0.085 / \mathrm{kWh}\), calculate its cost. (c) If distilled water sells in a grocery store for \(\$ 1.26\) per gal, what percentage of the sales price is represented by the cost of the energy?

An impurity in water has an extinction coefficient of \(3.45 \times 10^{3} \mathrm{M}^{-1} \mathrm{~cm}^{-1}\) at \(280 \mathrm{~nm}\), its absorption maximum (A Closer Look, p. 582 ). Below \(50 \mathrm{ppb}\), the impurity is not a problem for human health. Given that most spectrometers cannot detect absorbances less than \(0.0001\) with good reliability, is measuring the absorbance of a water sample at \(280 \mathrm{~nm}\) a good way to detect concentrations of the impurity above the 50 -ppb threshold?
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