Lithium nitrate: Difference between revisions
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Other [[group I]] nitrates decompose differently, forming the [[nitrite]] salt and [[oxygen]]. Because of its relatively small size, the lithium [[cation]] is very [[polarizing]], which favors the formation of the oxide. |
Other [[group I]] nitrates decompose differently, forming the [[nitrite]] salt and [[oxygen]]. Because of its relatively small size, the lithium [[cation]] is very [[polarizing]], which favors the formation of the oxide. |
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When placed in a |
When placed in a solution of water and in the presence of a catalyst (usually aluminium), it reacts violently to produce large quantities of hydrogen gas. |
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Lithium nitrate is not poisonous under standard conditions, although when potassium permanganate is mixed with it, it lets of large quantities of toxic ammonia gas. |
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Lithium nitrate can be formed by electrolysing baking soda, although this method is very inefficient. |
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==References== |
==References== |
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Revision as of 22:28, 20 March 2010
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| Identifiers | |
|---|---|
| ECHA InfoCard | 100.029.290 |
PubChem CID
|
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CompTox Dashboard (EPA)
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| Properties | |
| LiNO3 | |
| Molar mass | 68.946 g/mol |
| Appearance | White to light yellow solid |
| Density | 2.38 g/cm3 |
| Melting point | 255 °C (491 °F; 528 K) |
| Boiling point | 873 °C decomp. |
| 90 g/100 mL (28 °C) 234 g/100 mL (100 °C) | |
| Solubility | soluble in methanol, pyridine, ammonia |
Refractive index (nD)
|
1.735 [1] |
| Thermochemistry | |
Std enthalpy of
formation (ΔfH⦵298) |
-7.007 kJ/g |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards
|
Oxidant, irritant |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Related compounds | |
Other cations
|
Sodium nitrate Potassium nitrate Rubidium nitrate Caesium nitrate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lithium nitrate is an inorganic compound with the formula LiNO3. This deliquescent colourless salt is an oxidizing agent used in the manufacture of red-colored fireworks and flares.
Upon thermal decomposition, LiNO3 gives lithium oxide (Li2O), nitrogen dioxide, and oxygen:
- 4 LiNO3 → 2 Li2O + 4 NO2 + O2
Other group I nitrates decompose differently, forming the nitrite salt and oxygen. Because of its relatively small size, the lithium cation is very polarizing, which favors the formation of the oxide.
When placed in a solution of water and in the presence of a catalyst (usually aluminium), it reacts violently to produce large quantities of hydrogen gas.
Lithium nitrate is not poisonous under standard conditions, although when potassium permanganate is mixed with it, it lets of large quantities of toxic ammonia gas.
Lithium nitrate can be formed by electrolysing baking soda, although this method is very inefficient.
References
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
External links
 | This inorganic compound–related article is a stub. You can help Wikipedia by expanding it. |