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Which metal(s) can be oxidized with a sn2+ solution but not with an fe2+ solution? (hint: the reactions are occurring under standard conditions.)?

Kyle Mckinney

in Chemistry

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Ronald Miller on September 26, 2018

To do this we must take into account that the reactive series of metals in which the metals are ordered according to their reactivity order.The oxidation of a metal can be defined as the ability to lose electrons to become positively charged metal and a metal that will lose electrons when reacting with a metal that is to have low chemical reactivity of an increase in reactive metal can lose its electrons to a low reactive metal. So here's a metal must be one that is more reactive than the tin so that it can lose its electrons to the can is positively charged and less reactive than iron, so it will not give its electrons to the iron that is positively charged. If we look in reagents of the series of metal which we are going to find that the nickel is the example of a metal that is more reactive than tin and less reactive than iron.


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