Activity Series Of Metals Chart

Written By Paramjit Singh
Last Modified xxx-09-2022

Activeness Series of Metals: Meaning, Applications, Examples

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Action Serial of Metals: The electrochemical, electromotive, or action series of the elements is formed when the electrodes (metals and nonmetals) in contact with their ions are ordered on the basis of the values of their standard reduction potentials or standard oxidation potentials. A prepare of standard electrode potentials has been constructed past measuring the potentials of various electrodes vs the standard hydrogen electrode \(\left( {{\rm{SHE}}} \right)\).

Electrochemical Series or Action Series

The standard potentials of electrodes for reduction half-reactions are tabulated according to international convention, reflecting the electrodes' proclivity to behave as cathodes towards \({\rm{SHE}}\). Electrodes with positive \({\rm{E^\circ }}\) values for reduction half-reactions act as cathodes against \({\rm{SHE}}\), whereas those with negative E° values for reduction one-half-reactions human activity equally anodes. The electrochemical series is listed in the table below. The standard state potential of a jail cell is its potential at standard country circumstances, which are approximated at \(ane\) mole per litre \(\left( {one{\rm{ M}}} \right)\) concentrations and \(1\) atmosphere pressure at \(25^\circ {\rm{C}}\). The electrochemical series is given below.

Element	Electrode Reaction (Reduction)	Standard Electrode Reduction potential \({\rm{E^\circ }}\), volt
\({\rm{Li}}\)	\({\rm{L}}{{\rm{i}}^ + } + {{\rm{east}}^ – } \to {\rm{Li}}\)	\( – 3.05\)
\({\rm{K}}\)	\({{\rm{K}}^ + } + {{\rm{east}}^ – } \to {\rm{K}}\)	\( – 2.925\)
\({\rm{Ca}}\)	\({\rm{C}}{{\rm{a}}^{{\rm{2 + }}}}{\rm{ + 2}}{{\rm{east}}^{\rm{ – }}} \to {\rm{Ca}}\)	\( – two.87\)
\({\rm{Na}}\)	\({\rm{Northward}}{{\rm{a}}^ + } + {{\rm{east}}^ – } \to {\rm{Na}}\)	\( – 2.714\)
\({\rm{Mg}}\)	\({\rm{M}}{{\rm{1000}}^{two + }} + {\rm{2}}{{\rm{e}}^ – } \to {\rm{Mg}}\)	\( – 2.37\)
\({\rm{Al}}\)	\({\rm{A}}{{\rm{fifty}}^{3 + }} + 3{{\rm{east}}^ – } \to {\rm{Al}}\)	\( – 1.66\)
\({\rm{Zn}}\)	\({\rm{Z}}{{\rm{due north}}^{2 + }} + 2{{\rm{east}}^ – } \to {\rm{Zn}}\)	\( – 0.7628\)
\({\rm{Cr}}\)	\({\rm{C}}{{\rm{r}}^{three + }} + 3{{\rm{e}}^ – } \to {\rm{Cr}}\)	\( – 0.74\)
\({\rm{Fe}}\)	\({\rm{F}}{{\rm{e}}^{ii + }} + 2{{\rm{e}}^ – } \to {\rm{Fe}}\)	\( – 0.44\)
\({\rm{Cd}}\)	\({\rm{C}}{{\rm{d}}^{ii + }} + 2{{\rm{east}}^ – } \to {\rm{Cd}}\)	\( – 0.403\)
\({\rm{Ni}}\)	\({\rm{N}}{{\rm{i}}^{ii + }} + 2{{\rm{due east}}^ – } \to {\rm{Ni}}\)	\( – 0.25\)
\({\rm{Sn}}\)	\({\rm{S}}{{\rm{northward}}^{2 + }} + 2{{\rm{due east}}^ – } \to {\rm{Sn}}\)	\( – 0.14\)
\({{\rm{H}}_{\rm{2}}}\)	\(2{{\rm{H}}^ + } + 2{{\rm{e}}^ – } \to {{\rm{H}}_2}\)	\(0.00\)
\({\rm{MgCu}}\)	\({\rm{C}}{{\rm{u}}^{2 + }} + 2{{\rm{e}}^ – } \to {\rm{Cu}}\)	\( + 0.337\)
\({{\rm{l}}_{\rm{ii}}}\)	\({{\rm{I}}_2} + 2{{\rm{eastward}}^ – } \to 2{{\rm{I}}^ – }\)	\( + 0.535\)
\({\rm{Ag}}\)	\({\rm{A}}{{\rm{g}}^ + } + {{\rm{e}}^ – } \to {\rm{Ag}}\)	\( + 0.799\)
\({\rm{Hg}}\)	\({\rm{H}}{{\rm{g}}^{2 + }} + two{{\rm{e}}^ – } \to {\rm{Hg}}\)	\( + 0.885\)
\({\rm{B}}{{\rm{r}}_{\rm{2}}}\)	\({\rm{B}}{{\rm{r}}_2} + two{{\rm{e}}^ – } \to 2{\rm{B}}{{\rm{r}}^ – }\)	\( + one.08\)
\({\rm{C}}{{\rm{l}}_{\rm{two}}}\)	\({\rm{C}}{{\rm{l}}_2} + 2{{\rm{e}}^ – } \to 2{\rm{C}}{{\rm{l}}^ – }\)	\( + 1.36\)
\({\rm{Au}}\)	\({\rm{A}}{{\rm{u}}^{3 + }} + 3{{\rm{e}}^ – } \to {\rm{Au}}\)	\( + one.50\)
\({{\rm{F}}_{\rm{2}}}\)	\({{\rm{F}}_2} + ii{{\rm{e}}^ – } \to 2\;{{\rm{F}}^ – }\)	\( + 2.87\)

Characteristics of Electrochemical Series

The substances that are more powerful reducing agents than hydrogen are positioned above hydrogen in the series and have standard reduction potentials that are negative.
All of the chemicals in the serial below hydrogen that have positive reduction potentials are weaker reducing agents than hydrogen. In the series, substances that are more strong oxidisers than the \({{\rm{H}}^{\rm{ + }}}\) ion are mentioned after hydrogen. The metals at the elevation (with high negative standard reduction potentials) have a proclivity for losing electrons. These are metals that are in use. The nonmetals at the lesser (with high positive standard reduction potentials) have a proclivity for accepting electrons. These are nonmetals that are active.

Applications of Electrochemical Series

Reactivity of Metals

The action of a metal is determined past its tendency to lose electrons or course cations. The magnitude of the standard reduction potential influences this tendency. The metal with a high negative (or smaller positive) standard reduction potential chop-chop loses an electron or electrons and becomes a cation. Chemical action is a term used to describe a metal similar this.

Electropositive Character of Metals

The tendency to lose electrons or electrons also influences the electropositive grapheme. The electropositive feature of metals decreases from top to bottom in the electrochemical series, like to reactivity. To determine if a given metal volition displace another from its salt solution, utilize the following formula: A metal higher in the serial volition evict a metal lower in the series from its solution, i.east., a metal with low standard reduction potential will evict a metal from its table salt'south solution with a greater standard reduction potential value. A metal higher in the serial has a greater tendency to provide electrons to the cations of the metallic to be precipitated.

Deportation of Hydrogen from Dilute Acids by Metals:

Dilute acids are reduced by a metallic that may donate electrons to \({{\rm{H}}^{\rm{ + }}}\) ions in the presence of dilute acids. A metal with a negative reduction potential has the power to lose an electron or electrons. As a result, the metals at the top of the electrochemical series readily free hydrogen from dilute acids, just the tendency to liberate hydrogen gas from dilute acids reduces every bit the series progresses. \({\rm{Cu}},{\rm{ Hg}},{\rm{ Au}},{\rm{ Pt}}\), and other metals in the electrochemical series below hydrogen do not produce hydrogen from dilute acids.

Deportation of Hydrogen from H2o

The metals above iron have the power to liberate hydrogen from water. In the electrochemical series, the tendency diminishes from pinnacle to lesser. Coldwater liberates hydrogen for alkali and alkaline earth metals, but hot h2o or steam liberates hydrogen for \({\rm{Mg}},{\rm{ Zn}}\), and \({\rm{Atomic number 26}}\).

Reducing Ability of Metals

The tendency to lose an electron or electrons is the basis for reducing nature. The higher negative the reduction potential, the more than likely it is that an electron or electrons volition be lost. As a effect, in the electrochemical series, decreasing nature diminishes from peak to bottom. As the typical reduction potential becomes more and more negative, the reducing agent's power grows.

Sodium is a more powerful reducing agent than zinc, while zinc is more than powerful than iron. Alkali and element of group i world metals are constructive reducers.

Products of Electrolysis

When there are 2 or more types of positive and negative ions in a solution, certain ions are discharged or freed at the electrodes in preference to others during electrolysis. In such a competition, the ion with the higher standard reduction potential (stronger oxidising agent) is discharged beginning at the cathode.

Calculation of Standard emf \({{\rm{E}}^{\rm{O}}}\) of Electrochemical Jail cell

The total of the standard reduction potentials of the ii half cells (reduction half cell and oxidation one-half cell) is the cell'due south standard emf.

\({\rm{E}}_{{\rm{cell}}}^{\rm{O}}{\rm{ = E}}_{{\rm{red}}}^{\rm{O}}{\rm{ + E}}_{{\rm{OX}}}^{\rm{O}}\)

As is typical, the standard oxidation potential is ever expressed in terms of reduction potential.

As a effect, the conventional oxidation and reduction potentials are the aforementioned.

Therefore,

\({\rm{Eastward}}_{{\rm{cell}}}^{\rm{O}}{\rm{ = }}\) ( standard reduction potential of reduction half jail cell) – ( standard reduction potential of oxidation half cell)

As oxidation takes place at the anode and reduction takes place at the cathode. Hence,

\({\rm{E}}_{{\rm{cell}}}^{\rm{O}}{\rm{ = Eastward}}_{{\rm{cathode}}}^{\rm{O}}{\rm{ – E}}_{{\rm{anode}}}^{\rm{O}}\)

Summary

The electrochemical, electromotive, or activity series of the elements is formed when the electrodes (metals and nonmetals) in contact with their ions are ordered on the footing of the values of their standard reduction potentials or standard oxidation potentials.
The standard country potential of a prison cell is its potential at standard state circumstances, which are approximated at \(1\) mole per litre \(\left( {ane{\rm{ M}}} \right)\) concentrations and \(i\) atmosphere pressure at \({25^{\rm{o}}}{\rm{C}}\).
The substances that are more powerful reducing agents than hydrogen are positioned above hydrogen in the series and have standard reduction potentials that are negative.
The metal with a loftier negative (or smaller positive) standard reduction potential apace loses an electron or electrons and becomes a cation. Chemical activity is a term used to describe a metal like this.
A metal with a negative reduction potential has the ability to lose an electron or electrons. As a result, the metals at the top of the electrochemical series readily free hydrogen from dilute acids.
When there are two or more than types of positive and negative ions in a solution, sure ions are discharged or freed at the electrodes in preference to others during electrolysis

Q.one. What is the activeness series of metals?
Ans: The electrochemical, electromotive, or activity serial of the elements is formed when the electrodes (metals and nonmetals) in contact with their ions are ordered on the ground of the values of their standard reduction potentials or standard oxidation potentials. A prepare of standard electrode potentials has been constructed by measuring the potentials of various electrodes vs the standard hydrogen electrode \(\left( {{\rm{SHE}}} \right)\).

Q.2. How can the reactivity of metals be determined by activity series?
Ans: The activity of a metallic is determined by its tendency to lose electrons or form cations. The magnitude of the standard reduction potential influences this trend.
The metal with a loftier negative (or smaller positive) standard reduction potential rapidly loses an electron or electrons and becomes a cation. Chemic activity is a term used to describe a metallic similar this.

Q. 3. How are the products of electrolysis determined with activity serial?
Ans: When there are two or more types of positive and negative ions in a solution, sure ions are discharged or freed at the electrodes in preference to others during electrolysis. In such a competition, the ion with the higher standard reduction potential (stronger oxidising agent) is discharged beginning at the cathode.

Q.4. Which type of metals can displace hydrogen from the dilute acids?
Ans: Dilute acids are reduced by a metal that may donate electrons to \({{\rm{H}}^{\rm{ + }}}\) ions in the presence of dilute acids. A metal with a negative reduction potential has the power to lose an electron or electrons. Equally a result, the metals at the peak of the electrochemical series readily free hydrogen from dilute acids, but the tendency to liberate hydrogen gas from dilute acids reduces as the serial progresses. \({\rm{Cu}},{\rm{ Hg}},{\rm{ Au}},{\rm{ Pt}}\), and other metals in the electrochemical series below hydrogen do not produce hydrogen from dilute acids.

Q.5. Which type of metals can readapt hydrogen from water?
Ans: The metals above iron take the ability to liberate hydrogen from water. In the electrochemical series, the tendency diminishes from top to bottom. Coldwater liberates hydrogen for alkali and alkaline earth metals, but hot water or steam liberates hydrogen for \({\rm{Mg}},{\rm{ Zn}}\), and \({\rm{Fe}}\).

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