What determines whether one metal will replace another metal from a compound in a single-replacement reaction?
The position of the metal and metal ion in the activity series.
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In a single-replacement reaction, one metal can replace another metal in a compound based on the "activity series" of metals. The activity series is a list that ranks metals in order of their reactivity.
The more reactive metal will replace the less reactive metal from a compound. This is because the more reactive metal has a greater tendency to lose electrons and form positive ions in a chemical reaction. It is able to displace the less reactive metal from the compound by bonding with the non-metal element in the compound.
For example, if metal A is higher on the activity series than metal B, metal A can replace metal B from a compound if metal A is added to the compound. However, if metal B is higher on the activity series, it cannot replace metal A from a compound.
It is important to note that the activity series is specific to the conditions of the reaction, such as temperature and concentration.
In a single-replacement reaction involving metals, the reactivity of metals determines whether one metal can replace another metal from a compound. This reactivity is determined by the position of the metal in the reactivity series.
The reactivity series is a list of metals arranged in order of decreasing reactivity. The most reactive metals are at the top of the series, while the least reactive metals are at the bottom. For example, the reactivity series commonly used includes metals such as potassium (K), sodium (Na), calcium (Ca), magnesium (Mg), aluminum (Al), zinc (Zn), iron (Fe), lead (Pb), copper (Cu), mercury (Hg), silver (Ag), and gold (Au).
In a single-replacement reaction, a more reactive metal can replace a less reactive metal from its compound. This is because metals that are higher in the reactivity series have a greater tendency to lose electrons and form positive ions. When a more reactive metal is added to a compound containing a less reactive metal, the more reactive metal displaces the less reactive metal, forming a new compound with itself.
For example, if you have a solution of copper sulfate (CuSO4) and add a piece of zinc metal, a single-replacement reaction occurs. The zinc (Zn) is more reactive than copper (Cu) in the reactivity series, so it displaces the copper from the compound. The reaction can be represented by the equation:
Zn + CuSO4 -> ZnSO4 + Cu
In this reaction, zinc replaces copper from copper sulfate, resulting in the formation of zinc sulfate and copper.
So, in summary, the reactivity of metals, determined by their position in the reactivity series, is what determines whether one metal can replace another metal from a compound in a single-replacement reaction.