Lithium oxide

Lithium oxide
Lithium oxide
Are common
Systematic ; name	Lithium oxide
Traditional names	Lithium oxide
Chem. formula	Li 2 O
Rac formula	Li 2 O
Physical properties
condition	solid
Molar mass	29.8774 g / mol
Density	2,013 g / cm³
Thermal properties
T. melt.	1570
T. Kip.	2600 ° C
Chemical properties
Water solubility	6.67 (0 ° C)
Classification
Reg. CAS number	12057-24-8
Pubchem
Reg. EINECS number
SMILES
Inchi
RTECS	OJ6360000
Chemspider

Lithium oxide ( lithium oxide ) is a binary inorganic substance having the chemical formula Li ₂ O. It belongs to the class of basic oxides .

Content

Description

Lithium oxide under standard conditions is a colorless, hygroscopic crystals with a cubic lattice. The space group F m3m, a = 0.4628 nm, Z = 4.

At temperatures above 1000 ° C, it is sublimated, in the presence of water vapor , sublimation is accelerated. In the gaseous state at temperatures above 1500 ° C, lithium oxide partially dissociates into Li and O ₂ . Diamagnetic. It does not react with hydrogen , oxygen , carbon and carbon monoxide even when heated. At high temperatures, it reacts with most metals , with the exception of gold , platinum and nickel . Under the action of magnesium , aluminum or manganese at temperatures above 1000 ° C, lithium oxide is reduced to metallic lithium . With oxides of a number of metals gives oxometallates , double and ternary oxides . Lithium oxide is the only alkali metal oxide formed as the main product when the metal is heated above 200 ° C in air (only traces of lithium peroxide are present). ^[2]

Getting

The interaction of metallic lithium with oxygen :

{\mathsf {4\ Li+\ O_{2}\longrightarrow 2\ Li_{2}O}}

{\ displaystyle {\ mathsf {4 \ Li + \ O_ {2} \ longrightarrow 2 \ Li_ {2} O}}}

The decomposition of lithium peroxide at a temperature of 195 ° C:

{\mathsf {2\ Li_{2}O_{2}{\xrightarrow {195^{\circ }C}}\ 2\ Li_{2}O+\ O_{2}\uparrow }}

{\ displaystyle {\ mathsf {2 \ Li_ {2} O_ {2} {\ xrightarrow {195 ^ {\ circ} C}} \ 2 \ Li_ {2} O + \ O_ {2} \ uparrow}}}

Chemical Properties

Interacts with water to form alkali:

{\mathsf {\ Li_{2}O+H_{2}O{\xrightarrow {\ }}\ 2\ LiOH}}

{\ displaystyle {\ mathsf {\ Li_ {2} O + H_ {2} O {\ xrightarrow {\}} \ 2 \ LiOH}}}

with acids:

{\mathsf {\ Li_{2}O+2\ HCl{\xrightarrow {\ }}\ 2\ LiCl+H_{2}O}}

{\ displaystyle {\ mathsf {\ Li_ {2} O + 2 \ HCl {\ xrightarrow {\}} \ 2 \ LiCl + H_ {2} O}}}

lithium oxide is displaced by some metals and non-metals:

{\mathsf {\ Li_{2}O+Mg{\xrightarrow {800^{\circ }C}}\ 2\ Li+MgO}}

{\ displaystyle {\ mathsf {\ Li_ {2} O + Mg {\ xrightarrow {800 ^ {\ circ} C}} \ 2 \ Li + MgO}}}

{\mathsf {2\ Li_{2}O+Si{\xrightarrow {1000^{\circ }C}}\ 4\ Li+SiO_{2}}}

{\ displaystyle {\ mathsf {2 \ Li_ {2} O + Si {\ xrightarrow {1000 ^ {\ circ} C}} \ 4 \ Li + SiO_ {2}}}}

forms salts with acid-forming oxides:

{\mathsf {Li_{2}O+CO_{2}{\xrightarrow {500^{\circ }C}}\ Li_{2}CO_{3}}}

{\ displaystyle {\ mathsf {Li_ {2} O + CO_ {2} {\ xrightarrow {500 ^ {\ circ} C}} \ Li_ {2} CO_ {3}}}

Application

Lithium oxide is used as an additive to mixtures of reagents for solid-phase synthesis of binary and ternary oxides to lower the process temperature ; as a component in the production of special glasses (in particular, with a small temperature coefficient of linear expansion and transparent to x-rays ), glazes and enamels , which increases their chemical and thermal resistance, strength and reduces the viscosity of melts . Also used in thermal barrier coatings along with yttrium and zirconium oxides to increase durability.

Notes

↑ ¹ ² Lithium oxide on XuMuK.Ru
↑ Description of lithium oxide on XuMuK.Ru

[Вещество-1] ¹ ² Lithium oxide on XuMuK.Ru

[2] Description of lithium oxide on XuMuK.Ru