Chemical Properties of Metals: Definition, Reactions and Examples

Metals are one of the most important classes of elements found in nature. They are widely used in construction, transportation, electrical appliances, machinery and countless everyday products. Their usefulness is largely due to their unique chemical behaviour. The chemical properties of metals explain how metals react with substances such as oxygen, water, acids and salt solutions to form new compounds. These reactions also help us understand the reactivity of different metals and their practical applications. 

The article is about the chemical properties of metals, along with balanced chemical equations, examples that will strengthen your chemistry fundamentals and help you prepare for school and competitive examinations. 

Table of Contents 

• What are Metals
• What are Chemical Properties of Metals
• Why Do Metals Show Chemical Properties
• Important Chemical Reactions of Metals
• Reactivity Series of Metals
• Applications of Metals
• Frequently Asked Questions on Chemical Properties of Metals

What are Metals

Metals are elements that readily lose electrons to form positive ions (cations) during chemical reactions. They are generally hard, lustrous, malleable, ductile and excellent conductors of heat and electricity. Most metals are found in the Earth's crust as ores, while a few, such as gold and platinum, occur in their native state.

The chemical properties of metals arise from their tendency to donate electrons, making them highly reactive with substances like oxygen, water, acids and non-metals.

Examples of Metals:

Some common examples of metals are iron, copper, aluminium, gold, silver, zinc, sodium, calcium, magnesium and lead. Iron is widely used in construction, copper is commonly used for electrical wiring, aluminium is preferred for making aircraft and kitchen utensils, while gold and silver are mainly used in jewellery and decorative items. Each of these metals has unique properties that make it suitable for different applications. 

Also Read: Non- Metals

What are Chemical Properties of Metals

The chemical properties of metals describe how metals behave when they react with other substances. Metals are generally electropositive elements, which means they readily lose electrons to form positive ions (cations). This ability to donate electrons makes metals highly reactive with substances such as oxygen, water, acids and salts.

The general representation of a metal losing an electron is:

$M \rightarrow M^{+} + e^{-}$

For example,

$Na \rightarrow Na^{+} + e^{-}$

The extent to which a metal reacts depends on its position in the reactivity series. Highly reactive metals react rapidly, while less reactive metals show little or no reaction under normal conditions.

Why Do Metals Show Chemical Properties?

Metals have one, two, or three electrons in their outermost shell. Since it is easier for them to lose these electrons than to gain more, they readily form positive ions. This tendency to lose electrons is responsible for most of the chemical reactions shown by metals.

When metals lose electrons:

• They form positively charged ions.
• They react with non-metals to form ionic compounds.
• They produce metal oxides, hydroxides and salts during different chemical reactions.
• Their reactivity depends on how easily they can lose electrons.

For this reason, metals are called electropositive elements.

Important Chemical Reactions of Metals 

Reaction of Metals with Oxygen

One of the most common chemical properties of metals is their reaction with oxygen. Most metals react with oxygen to form metal oxides.

General Equation

$Metal + Oxygen \rightarrow Metal\ Oxide$

Examples

Potassium reacts with oxygen to form potassium oxide.

$4K + O_2 \rightarrow 2K_2O$

Magnesium burns with a bright white flame to form magnesium oxide.

$Mg + O_2 \rightarrow 2MgO$

Iron reacts with oxygen in the presence of moisture to form rust.

$4Fe + 3O_2 + xH_2O \rightarrow 2Fe_2O_3 \cdot xH_2O$

Nature of Metal Oxides

Most metal oxides are basic in nature because they react with acids to produce salt and water.

Example:

$MgO + 2HCl \rightarrow MgCl_2 + H_2O$

Some metal oxides, however, are amphoteric, meaning they react with both acids and bases.

Examples include:

• Aluminium oxide ( $Al_2O_3$)
• Zinc oxide (ZnO)

Why Are Sodium and Potassium Stored in Kerosene?

Sodium and potassium are extremely reactive metals. They react rapidly with oxygen and moisture present in the air and may catch fire. Therefore, they are stored under kerosene oil to prevent contact with air and water.

Reaction of Metals with Water

The reaction of metals with water varies depending on the reactivity of the metal. Some metals react vigorously, while others react only with hot water or steam. A few metals do not react with water at all.

Highly Reactive Metals

Metals such as sodium and potassium react violently with cold water to form metal hydroxides and hydrogen gas.

$2Na + 2H_2O \rightarrow 2NaOH + H_2$

Potassium reacts even more vigorously than sodium and may catch fire during the reaction.

Moderately Reactive Metals

Calcium reacts less vigorously with cold water to produce calcium hydroxide and hydrogen gas.

$Ca + 2H_2O \rightarrow Ca(OH)_2 + H_2$

Metals Reacting with Hot Water

Magnesium reacts slowly with hot water to form magnesium oxide and hydrogen gas.

$Mg + H_2O \rightarrow MgO + H_2$

Metals Reacting with Steam

Iron does not react with cold or hot water but reacts with steam to form magnetic iron oxide and hydrogen gas.

$3Fe + 4H_2O \rightarrow Fe_3O_4 + 4H_2$

Metals That Do Not React with Water

Less reactive metals such as copper, silver, gold and platinum do not react with water under normal conditions.

Reaction with Dilute Acids

Another important chemical property of metals is their reaction with dilute acids. Most metals react with dilute hydrochloric acid (HCl) or dilute sulphuric acid (H₂SO₄) to produce a salt and hydrogen gas.

General Equation

$Metal + Dilute\ Acid \rightarrow Salt + Hydrogen$

Examples

Magnesium reacts with dilute hydrochloric acid.

$Mg + 2HCl \rightarrow MgCl_2 + H_2$

Iron reacts with dilute sulphuric acid.

$Fe + H_2SO_4 \rightarrow FeSO_4 + H_2$

Highly reactive metals such as sodium, potassium, lithium and calcium react vigorously with dilute acids. Metals like magnesium, zinc and iron react at a moderate rate.

Metals below hydrogen in the reactivity series, such as copper, silver, gold and platinum, do not react with dilute acids because they cannot displace hydrogen from the acid.

Reaction of Metals with Other Metal Salt Solutions

Metals also react with salt solutions of other metals. A more reactive metal displaces a less reactive metal from its salt solution. This type of reaction is known as a displacement reaction.

Example

Zinc is more reactive than copper, so it displaces copper from copper sulphate solution.

$Zn + CuSO_4 \rightarrow ZnSO_4 + Cu$

Similarly,

$Fe + CuSO_4 \rightarrow FeSO_4 + Cu$

However, copper cannot displace zinc from zinc sulphate solution because copper is less reactive than zinc. These displacement reactions are useful for comparing the reactivity of different metals.

Reactivity Series of Metals

The reactivity series is a list of metals arranged in decreasing order of their chemical reactivity.

Order	Metal
1	Potassium (K)
2	Sodium (Na)
3	Calcium (Ca)
4	Magnesium (Mg)
5	Aluminium (Al)
6	Zinc (Zn)
7	Iron (Fe)
8	Lead (Pb)
9	Hydrogen (H)
10	Copper (Cu)
11	Mercury (Hg)
12	Silver (Ag)
13	Gold (Au)
14	Platinum (Pt)

Applications of Metals 

Metals are widely used because of their strength, durability and excellent conductivity. Some important applications of metals include:

• Construction: Iron and steel are used in buildings, bridges and railway tracks.
• Electrical Industry: Copper and aluminium are used for electrical wiring, cables and motors.
• Transportation: Steel and aluminium are used to manufacture cars, trains, ships and aircraft.
• Kitchenware: Stainless steel, aluminium, and copper are used to make cookware and kitchen utensils.
• Jewellery: Gold, silver and platinum are commonly used to make ornaments and coins.

Read More: Acid, Base and Salts 

We learned that the chemical properties of metals explain how metals interact with oxygen, water, acids and salt solutions. Studying these properties helps students build a strong foundation in chemistry while also understanding the practical uses of metals in industries and everyday life.