Reaction of metals

In reactivity series, reaction of metals or active metal reaction^[1] is the reaction of metals with oxygen, carbon dioxide, water, water vapour, ammonia, acids, salt solutions, chlorine, and hydrogen, organic compounds, etc.^[2]^[3] The reactions include oxidation reaction, oxidation-reduction reaction, metal displacement reaction, corrosion, combustion, etc.^[4]

Reaction of metals with oxygen, water, acids, salt solutions, chlorine, and hydrogen, etc.^[5]^[6]
Chemical Reactions	Chemical equations	Observations
Reaction of Metals with Oxygen (of air):^[7] Metals react with oxygen to form metal oxides Metal oxides are basic in nature.	$4 N a + O_{2} ⟶ 2 N a_{2} O$ $4 K + O_{2} ⟶ 2 K_{2} O$	Sodium and potassium metals react with oxygen of air at room temperature to form basic oxide, sodium oxide and potassium oxide respectively. They are stored under kerosene oil to prevent their reaction with oxygen, moisture, and carbon dioxide of air, so as to protect them. Unlike most metal oxides, sodium oxide and potassium oxide dissolve in water to form alkali.
	$2 M g + O_{2} ⟶ 2 M g O$	Magnesium metal does not react with oxygen at room temperature. But on heating, it burns in air giving intense heat and light to form basic oxide, magnesium oxide. Magnesium oxide partially dissolves in water to form magnesium hydroxide.
	$4 A l + 3 O_{2} ⟶ 2 A l_{2} O_{3}$ $2 Z n + O_{2} ⟶ 2 Z n O$	Aluminium metal, on heating burns in air to form aluminium oxide. Aluminium oxide is amphoteric in nature. Zinc metal, on strong heating burns in air to form zinc oxide. Like aluminium oxide, zinc oxide is also an amphoteric oxide.
	$3 F e + 2 O_{2} ⟶ F e_{3} O_{4}$ $2 C u + O_{2} ⟶ 2 C u O$	Iron and copper metals do not burn in air even on strong heating. Iron reacts with oxygen of air to form Iron(II,III) oxide. Copper, on prolonged heating reacts with the oxygen of air to form copper(II) oxide.
	No reaction	Silver and gold metals do not react with oxygen even at higher temperature.
Reaction of Metals with water: Metals react with cold water and hot water to form metal hydroxide and hydrogen gas. Metals react with steam to form metal oxide and hydrogen gas.	$2 K + 2 H_{2} O ⟶ 2 K O H + H_{2}$ $2 N a + 2 H_{2} O ⟶ 2 N a O H + H_{2}$	Potassium metal reacts violently with cold water to form potassium hydroxide and hydrogen gas. Like potassium metal, sodium metal reacts vigorously with cold water forming sodium hydroxide and hydrogen gas. The reaction is highly exothermic due to which hydrogen gas formed catches fire immediately. The burning of hydrogen causes little explosions.
	$C a + 2 H_{2} O ⟶ C a (O H)_{2} + H_{2}$	Calcium metal reacts with cold water to form calcium hydroxide and hydrogen gas. The heat produced is not sufficient to burn the hydrogen gas which is formed. The piece of calcium metal starts floating in water because the bubbles of hydrogen gas formed during the reaction stick to its surface.
	$M g + 2 H_{2} O ⟶ M g (O H)_{2} + H_{2}$ $M g + H_{2} O ⟶ M g O + H_{2}$	Magnesium metal does not react with cold water. It reacts with hot water to form magnesium hydroxide and hydrogen gas. Like calcium metal, the piece of magnesium metal also starts floating in water due to the bubbles of hydrogen gas sticking to its surface. Magnesium reacts very rapidly with steam to form magnesium oxide and hydrogen gas.
	$2 A l + 3 H_{2} O ⟶ A l_{2} O_{3} + 3 H_{2}$ $Z n + H_{2} O ⟶ Z n O + H_{2}$	Aluminium and zinc metal do not react with either cold water or hot water. They react with steam to form aluminium oxide and zinc oxide respectively, and hydrogen gas. Aluminium metal does not react with water under ordinary conditions because of the presence of a thin but tough layer of aluminium oxide on its surface.
	$3 F e + 4 H_{2} O ⟶ F e_{3} O_{4} + 4 H_{2}$	Like aluminium and zinc metals, Red-hot iron also reacts with steam to form iron (II,III) oxide and hydrogen gas.
	No reaction	Lead, copper, silver, and gold metals do not react with water or even steam.
Reaction of Metals with dilute acids:^[8] Metals react with dilute hydrochloric acid to give metal chlorides and hydrogen gas. Metals react with dilute sulphuric acid to give metal sulphates and hydrogen gas. No hydrogen gas is evolved, if metals react with dilute nitric acid. Nitric acid is a strong oxidizing agent. So as soon as hydrogen gas is formed in the reaction between a metal and dilute nitric acid, the nitric acid oxidizes this hydrogen to water. Now, when nitric acid oxidizes hydrogen to water, then nitric acid itself is reduced to any of the nitrogen oxides such as dinitrogen monoxide, nitrogen monoxide, or nitrogen dioxide, depending on the nature of metal, the temperature of reaction and concentration of nitric acid.^[9]^[10] Further information: Nitric acid § Reactions with metals	$2 N a + 2 H C l ⟶ 2 N a C l + H_{2}$ $2 N a + H_{2} S O_{4} ⟶ N a_{2} S O_{4} + H_{2}$	Sodium metal reacts violently with dilute hydrochloric acid and sulphuric acid to form sodium chloride and sodium sulphate respectively, and hydrogen gas.
	$M g + 2 H C l ⟶ M g C l_{2} + H_{2}$ $M g + H_{2} S O_{4} ⟶ M g S O_{4} + H_{2}$ $M g + 2 H N O_{3} ⟶ M g (N O_{3})_{2} + H_{2}$ $M n + 2 H N O_{3} ⟶ M n (N O_{3})_{2} + H_{2}$	Magnesium metal reacts quite rapidly with dilute hydrochloric acid to form magnesium chloride and hydrogen gas. Magnesium metals reacts with very dilute nitric acid to form magnesium nitrate and hydrogen gas. Like magnesium metal, manganese metal also reacts with very dilute nitric acid to form manganese nitrate and hydrogen gas.
	$2 A l + 6 H C l ⟶ 2 A l C l_{3} + 3 H_{2}$ $2 A l + 3 H_{2} S O_{4} ⟶ A l_{2} (S O_{4})_{3} + 3 H_{2}$	Aluminium metal reacts slowly with dilute hydrochloric acid at first, due to the presence of tough protective layer of aluminium oxide on its surface. But when the thin, outer oxide layer gets dissolved in acid, then fresh aluminium metal is exposed which reacts rapidly with dilute hydrochloric acid to form aluminium chloride and hydrogen gas. Similarly, aluminium metal reacts with sulfuric acid to produce aluminium sulfate and hydrogen gas.
	$Z n + 2 H C l ⟶ Z n C l_{2} + H_{2}$ $Z n + H_{2} S O_{4} ⟶ N a_{2} S O_{4} + H_{2}$ $F e + 2 H C l ⟶ F e C l_{2} + H_{2}$ $F e + H_{2} S O_{4} ⟶ F e S O_{4} + H_{2}$	Zinc metal reacts with dilute hydrochloric acid to give zinc chloride and hydrogen gas. Iron metal reacts slowly with cold dilute hydrochoric acid to give iron(II) chloride and hydrogen gas. Copper metal does not react with dilute hydrochloric acid or dilute sulphuric acid at all.
	No reaction	Silver and gold metals also do not react with dilute acids.
Reaction of metals with salt solutions: A more reactive metal displaces a less reactive metal from its salt solution.	$C u S O_{4} + Z n ⟶ Z n S O_{4} + C u$	When zinc metal reacts with copper sulphate solution, then the blue colour of the solution fades gradually due to the formation of colourless zinc sulphate solution, and red-brown copper metal is deposited on zinc metal. Copper metal, however, does not react with zinc sulphate solution. Similarly, silver metal does not react with copper sulphate solution. Iron and magnesium metals, however, react with copper sulphate solution.
	$C u S O_{4} + F e ⟶ F e S O_{4} + C u$	When iron metal reacts with copper sulphate solution, then the blue colour of the solution fades gradually and red-brown copper metal is deposited on iron metal. Copper metal however does not react with iron(II) sulphate solution.
	$2 A g N O_{3} + C u ⟶ C u (N O_{3})_{2} + 2 A g$	When copper metal reacts with silver nitrate solution, the solution gradually becomes blue and a shinning greyish-white deposit of silver metal is formed on copper metal. Silver metal however does not react with copper nitrate solution or copper sulphate solution.
Reaction of metals with chlorine: Metals react with chlorine to form ionic chloride. Metal chlorides are electrolytes; they are usually solid and conduct electricity in solution or in molten state. Metal chlorides are non-volatile; they have high melting points and boiling points.	$2 N a + C l_{2} ⟶ 2 N a C l$ $C a + C l_{2} ⟶ C a C l_{2}$ $M g + C l_{2} ⟶ M g C l_{2}$ $2 A l + 3 C l_{2} ⟶ 2 A l C l_{3}$ $Z n + C l_{2} ⟶ Z n C l_{2}$ $2 F e + 3 C l_{2} ⟶ 2 F e C l_{3}$ $C u + C l_{2} ⟶ C u C l_{2}$	sodium metal reacts readily with chlorine to form an ionic chloride called sodium chloride. calcium metal reacts vigorously with chlorine to form an ionic chloride called calcium chloride. magnesium metal, on heating with chlorine, readily forms magnesium chloride. aluminium metal, on heating, reacts with chlorine to form aluminium chloride. zinc metal combines directly with chlorine to form zinc chloride. iron metal, when heated, combines with chlorine to form iron(III) chloride. copper metal, on heating, reacts with chlorine to form copper(II) chloride.
Reaction of metals with hydrogen: Most of the metals do not combine with hydrogen. Only a few reactive metals like sodium, potassium, calcium and magnesium react with hydrogen to form metal hydrides.^[11]	$2 N a + H_{2} ⟶ 2 N a H$ $2 K + H_{2} ⟶ 2 K H$	When hydrogen gas is passed over heated sodium and potassium metals, then sodium hydride and potassium hydride are formed, respectively.
	$C a + H_{2} ⟶ C a H_{2}$ $M g + H_{2} ⟶ M g H_{2}$	When hydrogen gas is passed over heated calcium metal, then calcium hydride is formed. Similarly, when hydrogen gas is passed over heated magnesium metal, then magnesium hydride is formed. Zinc, copper, and iron metals do not react with hydrogen to form hydrides.

References

↑ "Active Metal Reactions". chemed.chem.purdue.edu. Retrieved 2020-11-03.
↑ Livens, Francis R. (1991-01-01). "Chemical reactions of metals with humic material". Environmental Pollution. 70 (3): 183–208. doi:10.1016/0269-7491(91)90009-L. ISSN 0269-7491.
↑ Pettit, Frederick S.; Meier, Gerald H.; Birks, Neil, eds. (2006), "Reactions of metals in mixed environments", Introduction to the High Temperature Oxidation of Metals (2 ed.), Cambridge: Cambridge University Press, pp. 176–204, ISBN 978-0-521-48042-0, retrieved 2020-11-03
↑ "Metal Reactions". Good Science. Retrieved 2020-11-03.
↑ "Prelim Chemistry : Introduction to Predicting Reactions of Metals". Art Of Smart. Retrieved 2020-11-03.
↑ https://www.edb.gov.hk/attachment/tc/curriculum-development/major-level-of-edu/gifted/resources_and_support/ijso/HKIJSO_TrainingManual/Phase3/Chemistry/Lesson5_ReactionOfMetals/PhaseIII_Chem_L5_ReactionOfMetals_ppt.pdf
↑ "Open Textbooks | Siyavula". intl.siyavula.com. Retrieved 2020-11-03.
↑ Foundation, In association with Nuffield. "Reactions of metals with acids producing salts". RSC Education. Retrieved 2020-11-03.
↑ "Nitric acid", Wikipedia, 2020-09-10, retrieved 2020-10-07
↑ Kurushkin, Mikhail (2015-06-09). "Writing Reactions of Metals with Nitric Acid: A Mnemonic Device for Introductory Chemistry Students". Journal of Chemical Education. 92 (6): 1125–1126. Bibcode:2015JChEd..92.1125K. doi:10.1021/ed5006773. ISSN 0021-9584.
↑ "Hydrogen - Reactivity of hydrogen". Encyclopedia Britannica. Retrieved 2020-10-07.

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[1] "Active Metal Reactions". chemed.chem.purdue.edu. Retrieved 2020-11-03.

[2] Livens, Francis R. (1991-01-01). "Chemical reactions of metals with humic material". Environmental Pollution. 70 (3): 183–208. doi:10.1016/0269-7491(91)90009-L. ISSN 0269-7491.

[3] Pettit, Frederick S.; Meier, Gerald H.; Birks, Neil, eds. (2006), "Reactions of metals in mixed environments", Introduction to the High Temperature Oxidation of Metals (2 ed.), Cambridge: Cambridge University Press, pp. 176–204, ISBN 978-0-521-48042-0, retrieved 2020-11-03

[4] "Metal Reactions". Good Science. Retrieved 2020-11-03.

[5] "Prelim Chemistry : Introduction to Predicting Reactions of Metals". Art Of Smart. Retrieved 2020-11-03.

[6] ttps://www.edb.gov.hk/attachment/tc/curriculum-development/major-level-of-edu/gifted/resources_and_support/ijso/HKIJSO_TrainingManual/Phase3/Chemistry/Lesson5_ReactionOfMetals/PhaseIII_Chem_L5_ReactionOfMetals_ppt.pdf

[7] "Open Textbooks | Siyavula". intl.siyavula.com. Retrieved 2020-11-03.

[8] Foundation, In association with Nuffield. "Reactions of metals with acids producing salts". RSC Education. Retrieved 2020-11-03.

[9] "Nitric acid", Wikipedia, 2020-09-10, retrieved 2020-10-07

[10] Kurushkin, Mikhail (2015-06-09). "Writing Reactions of Metals with Nitric Acid: A Mnemonic Device for Introductory Chemistry Students". Journal of Chemical Education. 92 (6): 1125–1126. Bibcode:2015JChEd..92.1125K. doi:10.1021/ed5006773. ISSN 0021-9584.

[11] "Hydrogen - Reactivity of hydrogen". Encyclopedia Britannica. Retrieved 2020-10-07.

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Reaction of metals

See also

References