no, it is stable.
No, sodium chloride does not decompose when heated.
When sodium iodide is exposed to light, it may undergo a photochemical reaction where it can decompose or form other products. This is because the light energy can excite the molecules in sodium iodide, leading to potential photoreactions.
The ionic compound of sodium iodide is NaI. It is composed of sodium (Na+) ions and iodide (I-) ions held together by ionic bonds.
The IUPAC name for sodium iodide is sodium iodide.
Yes, when heated with a Bunsen burner, sodium carbonate (Na2CO3) decomposes to form sodium oxide (Na2O) and carbon dioxide (CO2).
No, sodium chloride does not decompose when heated.
When sodium iodide is exposed to light, it may undergo a photochemical reaction where it can decompose or form other products. This is because the light energy can excite the molecules in sodium iodide, leading to potential photoreactions.
Sodium Carbonate
The ionic compound of sodium iodide is NaI. It is composed of sodium (Na+) ions and iodide (I-) ions held together by ionic bonds.
The IUPAC name for sodium iodide is sodium iodide.
Yes, when heated with a Bunsen burner, sodium carbonate (Na2CO3) decomposes to form sodium oxide (Na2O) and carbon dioxide (CO2).
Sodium Carbonate
When copper II hydroxide and sodium nitrate are heated together, they may undergo a decomposition reaction. Copper II hydroxide will decompose into copper II oxide and water, while sodium nitrate will decompose into sodium nitrite and oxygen.
Sodium iodide
The formula for sodium iodide is NaI. It is formed by the combination of sodium (Na) and iodide (I-) ions, with sodium donating an electron to iodine to form a stable compound.
Yes, sodium carbonate decomposes when heated by a Bunsen burner. At high temperatures, sodium carbonate breaks down into sodium oxide and carbon dioxide gas through a process called thermal decomposition.
Sodium carbonate does decompose when heated, but it requires a high temperature of around 851°C. At this temperature, sodium carbonate decomposes to form sodium oxide and carbon dioxide gas. Lower temperatures may not provide enough energy for the chemical reaction to occur visibly.