Difference between revisions of "Oxide" - New World Encyclopedia

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Magnesium oxide.

An oxide is a chemical compound containing an oxygen atom and other elements. Most of the Earth's crust consists of oxides. Oxides result when elements are oxidized by air. Combustion of hydrocarbons affords the two principal oxides of carbon, carbon monoxide and carbon dioxide. Even materials that are considered pure elements often contain a coating of oxides. For example, aluminum foil has a thin skin of Al₂O₃ that protects the foil from further corrosion.

Most oxides are insoluble in water

The oxide anion, O²⁻, is the conjugate base of the hydroxide ion, OH⁻, and is encountered in ionic solid such as calcium oxide. O²⁻ is unstable in aqueous solution − its affinity for H⁺ is so great (pKb ~ -22) that it abstracts a proton from a solvent H₂O molecule:

O²⁻ + H₂O → 2 OH⁻

Although many anions are stable in aqueous solution, ionic oxides are not. For example, sodium chloride dissolve readily in water to give a solution containing the constitutent ions, Na⁺ and Cl^-. Oxides do not behave like this. When an ionic oxide dissolves, the O²⁻ ions become protonated. Although calcium oxide (CaO) is said to "dissolve" in water, the products include hydroxide:

CaO + H₂O → Ca²⁺ + 2 OH^-

In fact, no monoatomic dianion is known to dissolve in water—all are so basic that they undergo hydrolysis. Concentrations of oxide ion in water are too low to be detectable with current technology.

Authentic soluble oxides do exist of course, but they release oxyanions, not O^2-. Well-known soluble salts of oxyanions include sodium sulfate (Na₂SO₄), potassium permanganate (KMnO₄), and sodium nitrate (NaNO₃).

Nomenclature

In the eighteenth century, oxides were named calxes or calces after the calcination process used to produce oxides. Calx was later replaced by oxyd.

Oxides can be named after the number of oxygen atoms in the oxide. Oxides containing only one oxygen are called oxide or monoxide, those containing two oxygen atoms dioxide, three trioxide, four tetroxide, and so on following the Greek numerical prefixes.

Two other types of oxide are peroxide, O₂²⁻, and superoxide, O₂⁻. In such species, oxygen is assigned higher oxidation states than oxide.

Types of oxides

Oxides of more electropositive elements tend to be basic. They are called basic anhydrides; adding water, they may form basic hydroxides. For example, sodium oxide is basic; when hydrated, it forms sodium hydroxide.

Oxides of more electronegative elements tend to be acidic. They are called acid anhydrides; adding water, they form oxoacids. For example, dichlorine heptoxide is acid; perchloric acid is a more hydrated form.

Some oxides can act as both acid and base, at different times. They are amphoteric. An example is aluminum oxide. Some oxides do not show behavior as either acid or base.

The oxides of the chemical elements in their highest oxidation state are predictable and the chemical formula can be derived from the number of valence electrons for that element. Even the chemical formula of ozone is predictable as a group 16 element. One exception is copper for which the highest oxidation state oxide is copper(II) oxide and not copper(I) oxide. Another exception is fluoride that does not exist as expected as F₂O₇ but as OF₂ with the least electronegative element given priority. ^[1]. Phosphorus pentoxide, the third exception is not properly represented by the chemical formula P₂O₅ but by P₄O₁₀

Common oxides sorted by oxidation state

Element in (I) state
- Copper(I) oxide (Cu₂O)
- Dicarbon monoxide (C₂O)
- Dichlorine monoxide (Cl₂O)
- Lithium oxide (Li₂O)
- Nitrous oxide (N₂O)
- Potassium oxide (K₂O)
- Rubidium oxide (Rb₂O)
- Silver(I) oxide (Ag₂O)
- Thallium oxide (Tl₂O)
- Sodium oxide (Na₂O)
- Water (H₂O)

Element in (II) state
- Aluminum monoxide (Al O)
- Barium oxide (Ba O)
- Beryllium oxide (Be O)
- Cadmium oxide (Cd O)
- Calcium oxide (Ca O)
- Carbon monoxide (C O)
- Cobalt(II) oxide (Co O)
- Copper(II) oxide (Cu O)
- Iron(II) oxide (Fe O)
- Lead(II) oxide (Pb O)
- Magnesium oxide (Mg O)
- Mercury(II) oxide (Template:MercuryO)
- Nickel(II) oxide (Ni O)
- Nitrogen oxide (N O)
- Palladium(II) oxide (PdO)
- Silver(II) oxide (Ag O)
- Strontium oxide (Sr O)
- Sulfur monoxide (S O)
- Tin(II) oxide (Sn O)
- Titanium(II) oxide (Ti O)
- Vanadium(II) oxide (V O)
- Zinc oxide (Zn O)

Element in (III) state
- Aluminum oxide (Al₂O₃)
- Antimony trioxide (Sb₂O₃)
- Arsenic trioxide (As₂O₃)
- Bismuth trioxide (Bi₂O₃)
- Boron oxide (B₂O₃)
- Chromium(III) oxide (Cr₂O₃)
- Dinitrogen trioxide (N₂O₃)
- Erbium(III) oxide (Er₂O₃)
- Gadolinium(III) oxide (Gd₂O₃)
- Gallium(III) oxide (Ga₂O₃)
- Holmium(III) oxide (Ho₂O₃)
- Indium(III) oxide (In₂O₃)
- Iron(III) oxide (Fe₂O₃)
- Lanthanum(III) oxide (La₂O₃)
- Lutetium(III) oxide (Lu₂O₃)
- Nickel(III) oxide (Ni₂O₃)
- Phosphorus trioxide (P₄O₆)
- Promethium(III) oxide (Pm₂O₃)
- Rhodium(III) oxide (Rh₂O₃)
- Samarium(III) oxide (Sm₂O₃)
- Scandium(III) oxide (Sc₂O₃)
- Terbium(III) oxide (Tb₂O₃)
- Thallium(III) oxide (Tl₂O₃)
- Thulium(III) oxide (Tm₂O₃)
- Titanium(III) oxide (Ti₂O₃)
- Tungsten(III) oxide (W₂O₃)
- Vanadium(III) oxide (V₂O₃)
- Ytterbium(III) oxide (Yb₂O₃)
- Yttrium(III) oxide (Y₂O₃)

Element in (IV) state
- Carbon dioxide (C O₂)
- Cerium(IV) oxide (Ce O₂)
- Chlorine dioxide (Cl O₂)
- Chromium(IV) oxide (Cr O₂)
- Dinitrogen tetroxide (N₂O₄)
- Germanium dioxide (Ge O₂)
- Hafnium(IV) oxide (Hf O₂)
- Lead(I) peroxide (Pb O₂)
- Manganese(IV) oxide (Mn O₂)
- Nitrogen dioxide (N O₂)
- Ozone (O₃)
- Plutonium dioxide (Pu O₂)
- Ruthenium(IV) oxide (Ru O₂)
- Selenium dioxide (Se O₂)
- Silicon dioxide (Si O₂)
- Sulfur dioxide (S O₂)
- Tellurium dioxide (Te O₂)
- Thorium dioxide (Template:ThoriumO₂)
- Tin dioxide (Sn O₂)
- Titanium dioxide (Ti O₂)
- Tungsten(IV) oxide (W O₂)
- Uranium dioxide (U O₂)
- Vanadium(IV) oxide (V O₂)
- Zirconium dioxide (Zr O₂)

Element in (V) state
- Antimony pentoxide (Sb₂O₅)
- Arsenic pentoxide (As₂O₅)
- Dinitrogen pentoxide (N₂O₅)
- Phosphorus pentoxide (P₂O₅)
- Tantalum pentoxide (Ta₂O₅)
- Vanadium(V) oxide (V₂O₅)

Element in (VI) state
- Carbon trioxide (C O₃)
- Molybdenum(VI) oxide (Mo O₃)
- Rhenium trioxide (Re O₃)
- Selenium trioxide (Se O₃)
- Sulfur trioxide (S O₃)
- Tellurium trioxide (Te O₃)
- Tetraoxygen (O₄)
- Tungsten trioxide (W O₃)
- Uranium trioxide (U O₃)
- Xenon trioxide (Xe O₃)

Element in (VII) state
- Dichlorine heptoxide (Cl₂O₇)
- Manganese(VII) oxide (Mn₂O₇)
- Rhenium(VII) oxide (Re₂O₇)

Element in (VIII) state
- Osmium tetroxide (Os O₄)
- Ruthenium tetroxide (Ru O₄)
- Xenon tetroxide (Xe O₄)

Notes

↑ Fully Exploiting the Potential of the Periodic Table through Pattern Recognition Schultz, Emeric. J. Chem. Educ. 2005 82 1649.

References
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[1] Fully Exploiting the Potential of the Periodic Table through Pattern Recognition Schultz, Emeric. J. Chem. Educ. 2005 82 1649.

[1]

@@ Line 1: / Line 1: @@
-An '''oxide''' is a [[chemical compound]] containing an [[oxygen]] atom and other elements.  Most of the earth's crust consists of oxides.  Oxides result when elements are oxidized by air.  Combustion of [[hydrocarbon]]s affords the two principal oxides of carbon, [[carbon monoxide]] and [[carbon dioxide]].  Even materials that are considered to be pure elements often contain a coating of oxides.  For example, [[aluminium foil]] has a thin skin of [[alumina|Al<sub>2</sub>O<sub>3</sub>]] that protects the foil from further [[corrosion]].
+{{Claimed}}
+[[Image:Magnesium oxide.jpg|thumb|right|Magnesium oxide.]]
+An '''oxide''' is a [[chemical compound]] containing an [[oxygen]] atom and other elements. Most of the [[Earth]]'s crust consists of oxides. Oxides result when elements are oxidized by air.  Combustion of [[hydrocarbon]]s affords the two principal oxides of carbon, [[carbon monoxide]] and [[carbon dioxide]]. Even materials that are considered pure elements often contain a coating of oxides. For example, [[aluminum]] foil has a thin skin of [[alumina|Al<sub>2</sub>O<sub>3</sub>]] that protects the foil from further [[corrosion]].
 ==Most oxides are insoluble in water==
 The oxide [[ion|anion]], O<sup>2−</sup>, is the [[conjugate acid|conjugate base]] of the [[hydroxide]] ion, OH<sup>−</sup>, and is encountered in [[ionic compound|ionic]] solid such as [[calcium oxide]].  O<sup>2−</sup> is unstable in [[water|aqueous]] [[solution]] − its affinity for H<sup>+</sup> is so great (pKb ~ -22) that it abstracts a [[proton]] from a solvent H<sub>2</sub>O molecule:
 :O<sup>2−</sup>  +  H<sub>2</sub>O  →  2 OH<sup>−</sup>
-Although many [[anion]]s are stable in aqueous solution, ionic oxides are not.<!--period: they "dissolve by reacting—>  For example, [[sodium chloride]] dissolve readily in water to give a solution containing the constitutent ions, Na<sup>+</sup> and Cl<sup>-</sup>.  Oxides do not behave like this.  When an ionic oxide dissolves, the O<sup>2−</sup> ions become protonated.  Although [[Calcium oxide]], CaO, is said to "dissolve" in water, the products include [[hydroxide]]:
+Although many [[anion]]s are stable in aqueous solution, ionic oxides are not. For example, [[sodium chloride]] dissolve readily in water to give a solution containing the constitutent ions, Na<sup>+</sup> and Cl<sup>-</sup>. Oxides do not behave like this. When an ionic oxide dissolves, the O<sup>2−</sup> ions become protonated. Although [[calcium oxide]] (CaO) is said to "dissolve" in water, the products include [[hydroxide]]:
 :CaO  +  H<sub>2</sub>O  &rarr;  Ca<sup>2+</sup>  +  2 OH<sup>-</sup>
-In fact, no monoatomic dianion is known to dissolve in water - all are so basic that they undergo [[hydrolysis]]. Concentrations of oxide ion in water are too low to be detectable with current technology.
+In fact, no monoatomic dianion is known to dissolve in water&mdash;all are so basic that they undergo [[hydrolysis]]. Concentrations of oxide ion in water are too low to be detectable with current technology.
-Authentic soluble oxides do exist of course, but they release [[oxyanion]]s, not O<sup>2-</sup>.  Well known soluble salts of oxyanions include [[sodium sulfate]] (Na<sub>2</sub>SO<sub>4</sub>), [[potassium permanganate]] (KMnO<sub>4</sub>), and sodium nitrate (NaNO<sub>3</sub>).
+Authentic soluble oxides do exist of course, but they release [[oxyanion]]s, not O<sup>2-</sup>.  Well-known soluble salts of oxyanions include [[sodium sulfate]] (Na<sub>2</sub>SO<sub>4</sub>), [[potassium permanganate]] (KMnO<sub>4</sub>), and sodium nitrate (NaNO<sub>3</sub>).
 ==Nomenclature==
-In the [[18th century]], oxides were named '''calxes''' or '''calces''' after the [[calcination]] process used to produce oxides.  ''Calx'' was later replaced by ''oxyd''.
+In the eighteenth century, oxides were named '''calxes''' or '''calces''' after the [[calcination]] process used to produce oxides. ''Calx'' was later replaced by ''oxyd''.
 Oxides can be named after the number of oxygen atoms in the oxide. Oxides containing only one oxygen are called oxide or [[mono-|monoxide]], those containing two oxygen atoms [[di-|dioxide]], three [[tri-|trioxide]], four [[tetra-|tetroxide]], and so on following the [[Greek_language|Greek]] [[numerical prefix]]es.
@@ Line 19: / Line 24: @@
 ==Types of oxides==
 Oxides of more [[electropositive]] elements tend to be basic. They are called '''basic anhydrides'''; adding water, they may form basic [[hydroxide]]s. For example, [[sodium oxide]] is basic; when hydrated, it forms [[sodium hydroxide]].
 Oxides of more [[electronegative]] elements tend to be acidic. They are called '''acid anhydrides'''; adding water, they form [[oxoacid]]s. For example, [[dichlorine heptoxide]] is acid; [[perchloric acid]] is a more hydrated form.
-Some oxides can act as both acid and base, at different times. They are [[amphoteric]]. An example is [[aluminium oxide]]. Some oxides do not show behavior as either acid or base.
+Some oxides can act as both acid and base, at different times. They are [[amphoteric]]. An example is [[aluminum oxide]]. Some oxides do not show behavior as either acid or base.
 The oxides of the [[chemical element]]s in their highest [[oxidation state]] are predictable and the [[chemical formula]] can be derived from the number of [[valence electron]]s for that element. Even the chemical formula of [[ozone]] is predictable as a [[group 16 element]]. One exception is [[copper]] for which the highest oxidation state oxide is [[copper(II) oxide]] and not [[copper(I) oxide]]. Another exception is [[fluoride]] that does not exist as expected as F<sub>2</sub>O<sub>7</sub> but as [[oxygen difluoride|OF<sub>2</sub>]] with the least [[electronegative]] element given priority. <ref>''Fully Exploiting the Potential of the Periodic Table through Pattern Recognition'' Schultz, Emeric. J. Chem. Educ. '''2005''' 82 1649.</ref>. [[Phosphorus pentoxide]], the third exception is not properly represented by the chemical formula  [[Phosphorus|P]]<sub>2</sub>[[Oxygen|O]]<sub>5</sub> but by [[Phosphorus|P]]<sub>4</sub>[[Oxygen|O]]<sub>10</sub>
@@ Line 67: / Line 73: @@
 * Element in (III) state
-** [[Aluminium oxide]] ([[Aluminium|Al]]<sub>2</sub>[[Oxygen|O]]<sub>3</sub>)
+** [[Aluminum oxide]] ([[Aluminium|Al]]<sub>2</sub>[[Oxygen|O]]<sub>3</sub>)
 ** [[Antimony trioxide]] ([[Antimony|Sb]]<sub>2</sub>[[Oxygen|O]]<sub>3</sub>)
 ** [[Arsenic trioxide]] ([[Arsenic|As]]<sub>2</sub>[[Oxygen|O]]<sub>3</sub>)
@@ Line 155: / Line 161: @@
 == See also ==
-* Other oxygen ions [[ozonide]], O<sub>3</sub><sup>−</sup>, [[superoxide]], O<sub>2</sub><sup>−</sup>, [[peroxide]], O<sub>2</sub><sup>2−</sup> and [[dioxygenyl]], O<sub>2</sub><sup>+</sup>.
+* [[ozonide]], O<sub>3</sub><sup>−</sup>
+* [[superoxide]], O<sub>2</sub><sup>−</sup>
+* [[peroxide]], O<sub>2</sub><sup>2−</sup>
+* [[dioxygenyl]], O<sub>2</sub><sup>+</sup>.
 * See [[:Category:Oxides]] for a list of oxides.
-== References ==
+== Notes ==
 <references />
-[[Category:Oxides|*]]
+== References ==
+<<Refs needed>>
+[[Category:Physical sciences]]
+[[Category:Chemistry]]
+[[Category:Earth sciences]]
+[[Category:Minerals]]
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