How is elemental phosphorus prepared industrially?

Calcium phosphate is heated with silica and coke; phosphorus vapor leaves the furnace and is condensed or burned to form $\mathrm{P_4O_{10}}$.

Which oxidation states are common for phosphorus in compounds?

The common oxidation states are $-3$, $+3$, and $+5$. Phosphorus–phosphorus bonds can lead to less familiar oxidation-number patterns.

What acids form when phosphorus oxides react with water?

$\mathrm{P_4O_6}$ forms phosphorous acid, $\mathrm{H_3PO_3}$; $\mathrm{P_4O_{10}}$ forms phosphoric acid, $\mathrm{H_3PO_4}$.

Why is phosphorus(V) oxide an effective drying agent?

$\mathrm{P_4O_{10}}$ has a strong affinity for water and can remove it from gases, solvents, and many compounds.

How can phosphorus pentahalides behave as Lewis acids?

They accept electron pairs from halide ions, which can produce hexahalide ions such as $\mathrm{PX_6^-}$.

Inorganic chemistryLesson 8 of 12 in the course Representative Metals, Metalloids, and Nonmetals

Occurrence, Preparation, and Properties of Phosphorus

5 flashcards · 4 quiz questions · 5 match pairs · 5 fill-in sentences · English

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Summary

Phosphorus is an active nonmetal used in fertilizers, matches, pesticides, plastics, and specialized alloys. This lesson follows phosphorus from its source in phosphate rock through its industrial preparation and examines the chemistry of its important oxides and halides.

$2\mathrm{Ca_3(PO_4)_2}(s)+6\mathrm{SiO_2}(s)+10\mathrm{C}(s)\xrightarrow{\Delta}6\mathrm{CaSiO_3}(l)+10\mathrm{CO}(g)+\mathrm{P_4}(g)$

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How is elemental phosphorus prepared industrially?: Calcium phosphate is heated with silica and coke; phosphorus vapor leaves the furnace and is condensed or burned to form $\mathrm{P_4O_{10}}$ .
Which oxidation states are common for phosphorus in compounds?: The common oxidation states are $-3$ , $+3$ , and $+5$ . Phosphorus–phosphorus bonds can lead to less familiar oxidation-number patterns.
What acids form when phosphorus oxides react with water?: $\mathrm{P_4O_6}$ forms phosphorous acid, $\mathrm{H_3PO_3}$ ; $\mathrm{P_4O_{10}}$ forms phosphoric acid, $\mathrm{H_3PO_4}$ .
Why is phosphorus(V) oxide an effective drying agent?: $\mathrm{P_4O_{10}}$ has a strong affinity for water and can remove it from gases, solvents, and many compounds.
How can phosphorus pentahalides behave as Lewis acids?: They accept electron pairs from halide ions, which can produce hexahalide ions such as $\mathrm{PX_6^-}$ .

Quiz questions

Which materials are heated with calcium phosphate to produce elemental phosphorus?Answer: Silica and coke
How is phosphorus pentachloride prepared from phosphorus trichloride?Answer: By reacting it with excess chlorine
Which ions make up solid phosphorus pentachloride?Answer: $[\mathrm{PCl_4}]^+$ and $[\mathrm{PCl_6}]^-$
What is the physical structure of phosphorus pentafluoride in all states?Answer: It is molecular in every physical state

Based on Chemistry 2e by Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson, PhD (OpenStax), licensed CC BY 4.0. Adapted into a summary, flashcards and quizzes.

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