Ozone is extremely important to us; it can be said that without ozone, we would all perish under intense ultraviolet radiation! Here is a translation of some information about ozone, sourced from Wikipedia (English) and Wikipedia (Chinese).
Ozone, also known as trioxygen, has the chemical formula O_3. Each ozone molecule contains three oxygen atoms, making it a triatomic molecule. It is an allotrope of oxygen (composed of the same element but with a different structure and different properties), though it is much more unstable than diatomic oxygen (O_2). At ground level, ozone is an air pollutant that has harmful effects on the respiratory systems of humans and animals. However, the ozone layer in the upper atmosphere absorbs a large amount of ultraviolet radiation, protecting life on Earth from excessive UV exposure.
After a thunderstorm, we may notice a peculiar odor; this is ozone. It is formed under discharge conditions via the reaction 3O_2 = 2O_3. In 1840, the German-Swiss chemist Christian Friedrich Schönbein identified it as ozone. It gained widespread recognition after 1867.
Physical Properties:
The concentration of ozone in the atmosphere surrounding us is approximately 0.01 ppm (parts per million). Exposure to ozone concentrations higher than 0.1 ppm can cause headaches, eye irritation, and respiratory irritation.
At -112^\circ\text{C}, ozone is a dark blue liquid; at temperatures below -193^\circ\text{C}, it forms a violet-black solid. Its density is approximately 1.5 times that of oxygen.
Ozone is diamagnetic, which means it tends to oppose the formation of a magnetic field and reduces the energy of magnetic information transmission.
Chemical Properties:
Ozone is a powerful oxidizing agent, with an oxidizing capacity far higher than that of oxygen. At high concentrations and under 1 atmosphere of pressure, it decomposes over half an hour as follows: 2O_3 = 3O_2.
Ozone can oxidize metals (except for gold, platinum, and iridium) to their highest oxidation states, for example: 2Cu^{+}(aq) + 2H_3O^{+}(aq) + O_{3}(g) = 2Cu^{2+}(aq) + 3H_{2}O(l) + O_2(g)
Ozone can also increase the oxidation state of oxides, such as converting nitric oxide to nitrogen dioxide: NO + O_3 = NO_{2} + O_2 This reaction is generally accompanied by chemiluminescence. NO_2 can be further oxidized: NO_{2} + O_3 = NO_{3} + O_2 The resulting NO_3 can then react with NO_2: NO_{3} + NO_2 = N_{2}O_5.
At room temperature, ozone reacts with carbon to produce carbon dioxide: C + 2O_3 = CO_{2} + 2O_2
Ozone does not react with ammonium salts, but it can react with ammonia gas or aqueous ammonia to produce ammonium nitrate: 2NH_{3} + 4O_3 = NH_{4}NO_{3} + 4O_{2} + H_{2}O
Ozone reacts with sulfides to produce sulfates: PbS + 4O_3 = PbSO_{4} + 4O_2
Ozone can also be used to produce sulfuric acid from sulfur or sulfur dioxide: S + H_{2}O + O_3 = H_{2}SO_4 \quad \text{and} \quad 3SO_{2} + 3H_{2}O + O_3 = 3H_{2}SO_4
Other chemical properties of ozone include: 3SnCl_2 + 6 HCl + O_3 = 3 SnCl_4 + 3 H_2O
H_2S + O_3 = SO_2 + H_2O (in hydrogen
sulfide gas)
H_2S + O_3 = S + O_2 + H_2O (in
hydrosulfuric acid) \begin{aligned}
3H_2S + 4 O_3 &= 3 H_2SO_4 \\
I_2 + 6 HClO_4 + O_3 &= 2 I(ClO_4)_3 + 3 H_2O \\
2 NO_2 + 2 ClO_2 + 2 O_3 &= 2 NO_2ClO_4 + O_2 \\
3 C_4N_2 + 4 O_3 &= 12 CO + 3 N_2
\end{aligned} H + O_3 = HO_2 +
O
2 HO_2 = H_2O_4 \begin{aligned}
KO_2 + O_3 &= KO_3 + O_2 \\
2 KOH + 5 O_3 &= 2 KO_3 + 5 O_2 + H_2O \\
CsO_3 + Na^+ &= Cs^+ + NaO_3 \\
3 Ca + 10 NH_3 + 6 O_3 &= Ca\cdot 6NH_3 + Ca(OH)_2 + Ca(NO_3)_2 + 2
NH_4O_3 + 2 O_2 + H_2 \\
2 Mn^{2+} + 2 O_3 + 4 H_2O &= 2 MnO(OH)_2 (s) + 2 O_2 + 4 H^+ \\
CN^{-} + O_3 &= CNO^{-} + O_2 \\
(NH_2)_2CO + O_3 &= N_2 + CO_2 + 2 H_2O
\end{aligned}
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