Following was written in by a student:
Hi, I have a Chemistry question..
A metallic element, M, has the following properties:
- less dense than water
- melts below 100C
- occurs naturally as its chloride, formula MCl
- the oxide of M reacts with water to form a solube hydroxide
Suggest how metal M can be extracted from its compounds. Explain your reasoning.
Also, how do I distinguish between hydrogen gas and nitrogen gas?
1st step is to identify the reactivity of this metal in order to check out the extraction method of these metals from its compounds (etc, their ores or chlorides)
The properties given suggest clearly that it belongs to Group 1 of the periodic table.
For Group 1 Alkali Metals, they are classified as the most reactive metals/elements.
You should already know about the metal reactivity series by now.
For these reactive metals, the compounds they formed are known to be unreactive (or stable).
Yes. Reactive Metals will formed Stable Compounds!
As such, for these Unreactive Compounds, the only way to extract the pure Metals is by electrolysis of their salts/compounds in aqueous (water) or in molten state.
Hope this information helps.
PS: For the N2 and H2 gases, i am not sure what you mean. But it you really want to differentiate N2 and H2 in the lab, you can just test for the POP sound with a lighted splint.
To Your Academic Success in Chemistry,