Ozone Formula

Ozone Formula

Ozone is a colourless to bluish gas that forms a dark blue liquid or blue-black crystals when it condenses.

The chemical formula for the inorganic molecule ozone, often known as trioxygen, is O₃. This gas is of pale blue colour with an odour that’s quite strong. It’s a less stable oxygen allotrope than the diatomic allotrope O₂, breaking down to O₂ in the lower atmosphere (dioxygen). The Earth’s atmosphere produces ozone, which is made up of dioxygen when UV rays and electrical discharges mix. It is found in extremely low amounts throughout the latter, with the maximum concentration high in the stratosphere’s ozone layer, which absorbs most of the Sun’s ultraviolet (UV) energy. In quantities less than 2 ppm, it has a distinct odour. ozonolysis of unsaturated fatty acids to pelargonic and other acids; manufacturing of ink; catalyst; water treatment for taste and odour management; mould and bacteria inhibitor in cold storage; bleaching agent.

Structure of Ozone

Ozone is a bent molecule with C_2v symmetry, according to experimental evidence from microwave spectroscopy (like the water molecule). 127.2 pm (1.272) are the O – O distances. The angle O – O – O is 116.78°. One lone pair is sp² hybridised with the center atom. Having a dipole moment of 0.53 D, ozone is a polar molecule. The molecule is a resonance hybrid, with two contributing structures, one with a single bond on one side and a double bond on the other. Both sides of the arrangement have an overall bond order of 1.5. Substituted isotopes can be found in naturally occurring ozone (¹⁶O, ¹⁷O, ¹⁸O).

Chemical Reaction of Ozone

Ozone is one of the most powerful oxidizers known, significantly more powerful than O₂. At large quantities, it is likewise unstable, decomposing into regular diatomic oxygen. Its half-life is affected by environmental factors such as temperature, humidity, and air movement. Half-Life Time (HLT) in still air at room temperature (24 °C), 0% humidity, and zero air changes per hour will average 1500 minutes (25 hours) in laboratory settings (ACH).

2O₃ → 3O₂

The rate of this reaction accelerates as the temperature rises. A spark can cause ozone deflagration, which can occur at ozone concentrations of 10 wt percent or greater.

At the anode of an electrochemical cell, ozone can also be made from oxygen. For research purposes, this process can produce modest amounts of ozone.

O₃(g) + 2H⁺ + 2e^– ↔ O₂(g) + H₂O

Example

1. It’s used as a disinfectant, germicide, and water steriliser.

2. Oils, starch, ivory, flour as well as other materials are bleached using it.

3. It works as an oxidising agent in the formation of potassium permanganate.

4. In water treatment facilities without filtration systems, ozone is employed.

Important formulas: