Activity series of the metals

Tables containing the same sequence of reactions as in Table 1, but without the voltage data, were in common use long before electrochemical cells were studied and half-cell potentials had been measured. If you read down the central column, you will notice that it begins with the sequence of metals Na, Zn, Fe, etc. This sequence is known as the activity series of the metals, and expresses the decreasing tendency these species to lose electrons- that is, to undergo oxidation.

The activity series of the metals, Table 4-12, tells us that copper and silver do not displace hydrogen from solutions of nonoxidizing acids. Aluminum is an active metal that can displace H2 from HCl and form aluminum chloride. 

Magnesium is above iron on the activity series of the metals, meaning it is more readily oxidized than iron. As a result, it will replace the iron in solution. 

The activity series of the metals. Metals can be ranked by their ability to displace H2 (actually reduce H ) from various sources or by their ability to displace one another from solution. 

Figure 4.14 The activity series of the metals. This list of metals (and H2) is arranged with the most active metal (strongest reducing agent) at the top and the least active metal (weakest reducing agent) at the bottom. The four metals below H2 cannot displace it from any source.

Any reaction that includes a free element as reactant or product is a redox reaction. In combination reactions, elements combine to form a compound, or a compound and an element combine. Decomposition of compounds by absorption of heat or electricity can form elements or a compound and an element. In displacement reactions, one element displaces another from solution. Activity series rank elements in order of reactivity. The activity series of the metals ranks metals by their ability to displace H2 from water, steam, or acid, or to displace one another from solution. Combustion typically releases heat and light energy through reaction of a substance with O2. 

Section 4.1 polar molecule (109) solvated (110) electrolyte (110) nonelectrolyte (112) Section 4.2 molecular equation (113) total ionic equation (114) spectator ion (114) net ionic equation (114) Section 4.3 precipitation reaction (115) precipitate (115) metathesis reaction (116) Section 4.4 acid-base reaction (117) neutralization reaction (117) acid (117) base (118) salt (119) titration (11 9) equivalence point (120) end point (120) Section 4.5 oxidation-reduction (redox) reaction (123) oxidation (124) reduction (124) oxidizing agent (124) reducing agent (124) oxidation number (O.N.) (or oxidation state) (124) Section 4.6 activity series of the metals (130)... 

Relative Reactivities of Metals In Chapter 4, we discussed the activity series of the metals (see Figure 4.14), which ranks metals by their ability to displace one another from aqueous solution. Now you ll see why this displacement occurs, as well as why many, but not all, metals react with acid to form H2, and why a few metals form H2 even in water. 

The Activity Series of the Metals Metals are ranked by their ability to displace H2 from various sources and another metal from solution. In all displacements of H2, the metal is the reducing agent (O.N. increases), and water or acid is the oxidizing agent (O.N. of H decreases). The activity series of the metals is based on these facts ... 

Many such reactions form the basis of the activity series of the metals. Note... 

Writing Spontaneous Redox Reactions 701 Explaining the Activity Series of the Metals 704... 

---