A + BC → AC + B
In this reaction, element A replaces element B in the compound BC, resulting in the formation of a new compound AC and the release of element B. The reactivity of elements plays a crucial role in determining whether a single-replacement reaction will occur. The activity series of elements, also known as the reactivity series, lists elements in order of their decreasing reactivity. Metals that are higher on the activity series are more reactive than those lower on the series.
In a single-replacement reaction, a more reactive element (A) displaces a less reactive element (B) from its compound. For example, when iron (Fe) is added to a solution of copper(II) sulfate (CuSO4), the following reaction takes place:
Fe(s) + CuSO4(aq) → FeSO4(aq) + Cu(s)
In this reaction, iron (Fe) is more reactive than copper (Cu), so it replaces copper in copper(II) sulfate, forming iron(II) sulfate (FeSO4) and releasing copper in its elemental form (Cu).
Here are the key points to remember about single-replacement reactions:
- A more reactive element replaces a less reactive element in a compound.
- The reaction involves the exchange of one element for another.
- The products formed are a new compound and the displaced element in its elemental form.
- The reactivity of elements is crucial in determining whether a single-replacement reaction will occur.
- Single-replacement reactions are commonly observed with metals and their compounds.
