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Some eye catching facts about lithium oxide is that when lithium is burned to air, it forms lithium oxide. This reaction also makes lithium nitrite. It can also be made by heating lithium peroxide. It is corrosive when dissolved in water. Lithium oxide dissolves in water to make lithium hydroxide. It reacts with acids to make lithium salts. It reacts with carbon dioxide to form lithium carbonate. Lithium carbonate is much less corrosive. It makes a red color in a flame.

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Lithium oxide Lithium oxide (Li 2O) or lithia is an inorganic chemical compound.Lithium oxide is formed along with small amounts of lithium peroxide when lithium metal is burned in the air and combines with oxygen: 4Li + O 2 → 2Li 2O.

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Lithium atoms have one valence electron, whereas oxygen atoms have six. Lithium atoms tend to give up their single valence electrons, and oxygen tends to gain two valence electrons from other atoms, like lithium. They do this so they will have filled valence shells.

During the formation of Li2O, Li atoms transfer their single valence electrons to Oatoms, forming two Li+ ions for every individual O2− ion. The electrostatic force of attraction between oppositely charged ions forms the ionic bonds.

4Li + O2 → 4Li+ + 2O2− → 2Li2O
Lithium oxide is formed along with small amounts of lithium peroxide when lithium metal is burned in the air and combines with oxygen: 4Li + O 2 → 2Li 2O. Pure Li 2O can be produced by the thermal decomposition of lithium peroxide

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To the best of our knowledge the chemical, physical and toxicological properties of lithium oxide have not been thoroughly investigated and reported.

The toxicity of lithium compounds is a function of their solubility in water.  Lithium ion has central nervous system toxicity.  The initial effects of lithium exposure are tremors of the hands, nausea, micturition, slurred speech, sluggishness, sleepiness, vertigo, thirst, and increased urine volume.  Effects from continued exposure are apathy, anorexia, fatigue, lethargy, muscular weakness, and changes in ecg.  Long-term exposure leads to hypothyroidism, leukocytosis, edema, weight gain, polydipsia/polyuria (increased water intake leading to increased urinary output), memory impairment, seizures, kidney damage, shock, hypotension, cardiac arrhythmias, coma, death.

Inhalation:  severe irritant and corrosive.  Causes irritation to the respiratory tract and mucous membranes.

Ingestion:  severe irritant and corrosive.  May cause central nervous system effects, circulatory failure and cardiovascular collapse.

Skin:  severe irritant and corrosive.

Eye:  severe irritant and corrosive.

Chronic effects:

Inhalation:  may cause pulmonary edema and lung damage.

Ingestion:  may cause gastrointestinal irritation, renal dysfunction, derangement of neuromuscular activity, diabetes and kidney damage.

Skin:  may be an irritant and corrosive.

Eye:  may cause blurred vision.

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In the solid state lithium oxide adopts an anti fluorite structure which is related to the CaF2, fluorite structure with Li cations substituted for fluoride anions and oxide anions substituted for calcium cations.The ground state gas phase Li2O molecule is linear with a bond length consistent with strong ionic bonding. The VSEPR theory would predict a bent shape similar to H2O.

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The molar mass of lithium oxide is 29.88 g/mol
The appearance of lithium oxide is that its white solid it has no odor.

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This is how the ionic bond forms in Lithium Oxide (Li2O).

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This short flash animation looks at how the ionic bond forms in Lithium Oxide (Li2O).

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2.013 g/cm³

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2,600 °C (4,710 °F; 2,870 K)

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1,438 °C (2,620 °F; 1,711 K)

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Lithium oxide is very corrosive. It reacts with water to make lithium hydroxide. It is toxic because of its strong alkalinity (being a base).

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Lithium was discovered in the mineral petalite (LiAl(Si₂O₅)₂) by Johann August Arfvedson in 1817. It was first isolated by William Thomas Brande and Sir Humphrey Davy through the electrolysis of lithium oxide (Li₂O). Today, larger amounts of the metal are obtained through the electrolysis of lithium chloride (LiCl). Lithium is not found free in nature and makes up only 0.0007% of the earth's crust.

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In this video its shows both point of view.

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Making Lithium Hydroxide (precursor to lithium drugs and CO2 absorber)

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In this video, we will be making lithium hydroxide by reacting lithium metal with water! I plan to use the lithium hydroxide to make some lithium based drugs (used to treat bipolar disorder) and to make lithium peroxide (reacts with CO2 and produces O2) I plan to do an Q and A video, so if you have any questions you'd like me to address in the video, leave them in the comments.

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Two lithium atoms will each give one electron to the oxygen atom. forms the ionic bond between lithium and oxygen. The formula for lithium oxide is Li ₂ O.

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29.88

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Li2O

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Lithium oxide; Lithium monoxide; Lithium oxide (LiO); MCD00016183; Lithium monooxide; Monolithium monoxide

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Lithium oxide is used aboard the space shuttle to remove water from the air supply according to the equation Li2O(s)+H2O(g)❝2LiOH(s) If 80.0 kg of water is to be removed and 65 kg of Li2O is available,

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Lithium oxide is used as a flux in ceramic glazes; and creates blues with copper and pinks with cobalt. Lithium oxide reacts with water and steam, forming lithium hydroxide and should be isolated from them.Its usage is also being investigated for non-destructive emission spectroscopy evaluation and degradation monitoring within thermal barrier coating systems. It can be added as a co-dopant with yttria in the zirconia ceramic top coat, without a large decrease in expected service life of the coating. At high heat, lithium oxide emits a very detectable spectral pattern, which increases in intensity along with degradation of the coating. Lithium metal might be obtained from lithium oxide by electrolysis, releasing oxygen as by-product. Lithium Oxide is a highly insoluble thermally stable Lithium source suitable for glass, optic and ceramic applications. Lithium oxide is a white solid also known as lithia, it is produced when lithium metal burns in the presence of oxygen. Oxide compounds are not conductive to electricity. However, certain perovskite structured oxides are electronically conductive finding application in the cathode of solid oxide fuel cells and oxygen generation systems. They are compounds containing at least one oxygen anion and one metallic cation. They are typically insoluble in aqueous solutions (water) and extremely stable making them useful in ceramic structures as simple as producing clay bowls to advanced electronics and in light weight structural components in aerospace and electrochemical applications such as fuel cells in which they exhibit ionic conductivity. Metal oxide compounds are basic anhydrides and can therefore react with acids and with strong reducing agents in redox reactions. Lithium Oxide is also available in pellets, pieces, sputtering targets, tablets, and nanopowder (from American Elements' nanoscale production facilities). American Elements produces to many standard grades when applicable, including Mil Spec (military grade); ACS, Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP it also follows applicable testing standards. Typical and custom packaging is available. Lithium Oxide is generally immediately available in most volumes. Ultra high purity, high purity, submicron and nanopowder forms may be considered. American Elements produces to many standard grades when applicable, including Mil Spec (military grade) , Reagent and Technical Grade; Food, Agricultural and Pharmaceutical Grade; Optical Grade, USP and it follows applicable testing standards. Typical and custom packaging is available. Additional technical, research and safety  information is available as is a Reference Calculator for converting relevant units of measurement.