Write reactivity series of metal
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Answer:
Potassium
Strontium
Calcium
Explanation:
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Explanation:
Metals
Reactivity Series of Metals
Metals, in general, are substances which have high electrical conductivity, high thermal conductivity, and high density. Typically they are malleable and ductile, deforming under stress without cleaving. In terms of optical properties, metals are shiny and lustrous. This article is on reactivity series of metals.
Metals are usually inclined to form cations through electron loss, reacting with oxygen in the air to form oxides over various timescales (iron rusts over years, while potassium burns in seconds). Examples:
4 Na + O2 → 2 Na2O (sodium oxide)
2 Ca + O2 → 2 CaO (calcium oxide)
4 Al + 3 O2 → 2 Al2O3 (aluminium oxide).
The transition metals (such as iron, copper, zinc, and nickel) are slower to oxidize because they form a passive layer of oxide that protects the interior. Others, like palladium, platinum and gold do not react with the atmosphere at all.
Reactivity Series of Metals
Reactivity Series of Metals
Reactivity Series in chemistry is an experimental, structural and logical progression of series of metals in order of reactivity from highest to lowest. Metals react differently with different substances. It gives a descriptive detail on metal reactions with the extraction of metals from ores and with acids and water. In other words, the most reactive metal is presented at the top and the least reactive metal at the bottom, as shown in the reactivity series chart below.
All metals have a tendency to lose electrons and form metal ions. In other words, all metals are good reducing agents and easily oxidize themselves.
M → Mn+ + ne–
The reactivity series of metals can be shown in another way, which includes oxidation reaction of each metal to the respective metal ion. It gives information regarding the reducing power of the metal atom and the oxidation number of the metal ion.
Before discussing the reactivity order of metals, it is important to discuss about the differences between metals and non-metals.
Differences between metals & non-metals:
S.No Metals Non-metals
1 Malleable & ductile in nature Brittle in nature
2 Good conductor of heat & electricity Insulator in nature
3 Form ionic compounds Form covalent compounds
4 Have lustrous surface Not applicable
5 Have high melting point Low melting point compared to metals
6 Usually solid at room temperature Can exist in solid, liquid & gaseous state
7 They are good reducing agents Good oxidizing agent
8 Form basic oxides Form acidic oxides
9 Have low electronegativity High electronegativity
10 Have a tendency to lose electrons Have a tendency to gain electrons
Reactivity Series of metals Chart
In the reactivity series, as we move from bottom to top, the reactivity of metals increases. Metals present at the top of the series can lose electrons more readily to form positive ions and corrode or tarnish more readily. They require more energy to be separated from their ores, and become stronger reducing agents, while metals present at the bottom of the series are good oxidizing agent.
We can summarize the reactivity of metals in a reactivity series chart as shown below:
Metal
Symbol
Reactivity
Extraction
Lithium Li Displaces H2 gas from water, steam and acids and forms hydroxides. Electrolysis
Potassium K
Strontium Sr
Calcium Ca
Sodium Na
Magnesium Mg Displaces H2 gas from steam and acids and forms hydroxides.
Aluminium Al
Carbon C Included for comparison.
Manganese Mn Displaces H2 gas from steam and acids and forms hydroxides. Smelting with coke
Zinc Zn
Chromium Cr
Iron Fe Displaces H2 gas from acids only and forms hydroxides.
Cadmium Cd
Cobalt Co
Nickel Ni
Tin Sn
Lead Pb
Hydrogen gas H2 Included for comparison.
Antimony Sb Combines with O2 to form oxides and cannot displace H2. Heat or physical extraction methods.
Arsenic Ar
Bismuth Bi
Copper Cu
Mercury Hg Found free in nature, oxides decompose with heating.
Silver Ag
Palladium Pd
Platinum Pt
Gold Au
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