lead dioxide

Being a strong oxidant, lead dioxide is a poison when ingested.

Lead dioxide is used as anode material in electrochemistry.

Lead dioxide can also withstand chlorine evolution in hydrochloric acid.

Lead dioxide is an amphoteric compound with prevalent acidic properties.

The synthetic orthorhombic form of lead dioxide, α-PbO, was known from 1941.

Lead dioxide is well known for being a good oxidizing agent with example reaction listed below:

Lead dioxide decomposes upon heating in air as follows:

He achieved this by mixing the phosphorus with lead dioxide instead of the potassium chlorate used previously.

The most important use of lead dioxide is as the cathode of lead acid batteries.

Lead dioxide is representative of the +4 oxidation state, and is a powerful oxidizing agent.

Lead(IV) oxide, also known as lead dioxide, is a chemical compound.

Lead dioxide dissolves in alkali hydroxide solutions to form the corresponding plumbates.

Lead dioxide - used in friction-sensitive compositions, e.g. matches

Lead dioxide is an odorless dark-brown crystalline powder which is nearly insoluble in water.

Therefore, thermal decomposition of lead dioxide is a common industrial way of producing various lead oxides.

Lead dioxide electrodes have a dual action, that is both the lead and oxygen ions take part in the electrochemical reactions.

The electrodes are usually made of lead dioxide and metallic lead, while the electrolyte is a sulfuric acid solution.

Lead dioxide is a strong oxidizing agent which is used in the manufacture of matches, pyrotechnics, dyes and other chemicals.

Lead dioxide is used in the production of matches, pyrotechnics, dyes and the curing of sulfide polymers.

Like metals, lead dioxide has a characteristic electrode potential, and in electrolytes it can be polarized both anodically and cathodically.

When the battery is recharged, the chemical reaction is reversed: the lead sulfate reforms into lead dioxide and lead.

It may be synthesized by oxidation of the parent phenol with lead dioxide or potassium hexacyanoferrate(III).

Lead and lead dioxide, the active materials on the battery's plates, react with sulfuric acid in the electrolyte to form lead sulfate.

Lead dioxide anodes are inexpensive and were once used instead of conventional platinum and graphite electrodes for regenerating potassium dichromate.

Treatment of lead dioxide with hydrochloric acid gives lead(II) chloride as well as chlorine gas: