They are much more stable meaning they are less reactive. The metals below hydrogen in the series do not react with aqueous hydrogen ions or water. The remaining metals (above hydrogen) will not react with water but do react with aqueous hydrogen ions. In fact, the first five metals in the series, both Group 1A and 2A metals, will react with pure water to form hydrogen gas.Ģ K (s) + 2 H 2O (l) c 2 K + (aq) + 2 OH – (aq) + H 2 (g) The metals above hydrogen will react with aqueous hydrogen ion to form hydrogen gas. Notice the position of hydrogen in the activity series.

The aluminum is a stronger reducing agent than silver and will reduce the Ag + ion to solid Ag.ģ Ag 2S (s) + 2 Al(s) → 6 Ag (s) + Al 2S 3 (s) Tarnish can be removed chemically with aluminum. Silver tarnishes according to the following reaction with H 2S gas.Ģ Ag (s) + H 2S (gas) → Ag 2S (s) + H 2 (g)Ĭommercial silver polishes will remove the tarnish from silver, but some of the silver is lost because these polishes are abrasive. Chromium can reduce Cu 2+ ion, but it cannot reduce Mn 2+. A metal can reduce any ion below it in the series. For example, zinc is a weaker reducing agent than sodium, but it is a stronger reducing agent than copper. Gold is at the end of the list and is not as easily oxidized and is therefore the weakest reducing agent on this activity series.īoth the ease of oxidation and the reducing strength of the metals decrease going down the column. Lithium is at the top of the list and is the most easily oxidized metal which means it is the strongest reducing agent in the activity series below. Below is a table of a partial activity series for metals in aqueous solution. Metals are strong reducing agents, but their reducing power decreases going across a period of the periodic table. This means metals lose electrons more easily than nonmetals. Knowledge of chemistry is endless, so to know more about various types of chemical reactions.Metals are more easily oxidized than nonmetals. Therefore, nonmetals that gain electrons rapidly are more active than others. We determine the reactivity of nonmetals, upon their capability to gain electrons in the solution state to form negatively charged ions or anions. What determines the reactivity of nonmetals?Īns. Therefore, the more readily metal loses its electrons, the more active it is, and higher up it is in the reactivity series. We determine the reactivity of metals, upon their capability to lose electrons in the solution state to form positive ions or cations.

What determines the reactivity of metals?Īns. Fluorine is the most active nonmetals and it displaces all other nonmetals in salt solutions. Which is the most active or reactive nonmetal?Īns. Due to its low reactivity, it found uses in the manufacture of laboratory equipment, electrodes, platinum resistance thermometers, dentistry equipment, and jewelry. It has remarkable resistance to corrosion, even at high temperatures, and is therefore considered a noble metal. Platinum is one of the least reactive metals and therefore lies at the bottom of the reactivity series.

Which is the least active or reactive metal?Īns. The table below, explain the reactions of metals with oxygen (air), water, dilute acids, and other salt solutions, at various level of the reactivity series. Metals at the top of the reactivity series are difficult to obtain from their ores.The activity series facilitates the comparative study of the metals in terms of the degree of their reactivity.Metals at the top of the reactivity series have the ability to displace metals that are placed lower from their salt solutions.It is because, like metals, it too loses an electron and becomes a positively charged (H +) ion. Although a non-metal, hydrogen is included in the reactivity series of metals.The ease, with which a metal in solution loses electrons and forms a positive ion, decreases down the series, i.e., from cesium to platinum.Special Features of the Reactivity or Activity Series of Metals:

Among the most commonly known metals, the most active cesium is at the top and the least active platinum is at the bottom of the reactivity series. The more readily metal loses its electrons, the more active it is, and the higher up it is in the reactivity series. The activity of a metal depends upon its capability to lose electrons in the solution state to form positive ions. For example, zinc being more active than copper replaces it with copper sulfate in the solution state to form zinc sulfate and free copper. In a displacement reaction, a metal higher up in the reactivity series displaces all other metals in a compound, which lies below it. It helps us to predict whether particular metal can displace another metal from a compound or not. Metal activity or reactivity series finds its utility in the study of displacement reactions.

Activity series of metals table j