The reactivity of metals and non-metals is determined by their tendency to lose or gain electrons to achieve a stable electron configuration, similar to noble gases. Metals tend to lose electrons to form positive ions (cations), while non-metals tend to gain electrons to form negative ions (anions). This exchange of electrons forms ionic bonds in compounds. Here’s a detailed explanation of how metals and non-metals react with each other.
Ionic Bond Formation
Metals react with non-metals to form ionic compounds. In these reactions, metals donate electrons to non-metals. As a result:
- Metals become cations (positively charged ions).
- Non-metals become anions (negatively charged ions).
These oppositely charged ions attract each other to form a stable ionic compound.
Example:
- Sodium Chloride (
): Sodium (
), a metal, has one electron in its outermost shell. It donates this electron to chlorine (
), a non-metal that requires one electron to complete its valence shell.
), a metal, has one electron in its outermost shell. It donates this electron to chlorine (
), a non-metal that requires one electron to complete its valence shell.
The electrostatic attraction between 
and 
forms sodium chloride (
), or table salt.
Real-life Application:
Salt in daily life: Sodium chloride (table salt) is one of the most common ionic compounds used in food and industry. It plays a vital role in human health by regulating fluid balance and nerve function.
Properties of Ionic Compounds
Ionic compounds formed by the reaction between metals and non-metals exhibit distinct properties:
- High Melting and Boiling Points: Due to the strong electrostatic forces between the cations and anions, a large amount of energy is required to break the bonds, resulting in high melting and boiling points.
- Solubility: Ionic compounds are generally soluble in water but insoluble in organic solvents like kerosene and petrol.
- Electrical Conductivity: Ionic compounds conduct electricity when dissolved in water or in the molten state. This is because the ions are free to move and carry electric current.
Example:
- Sodium chloride () dissolves in water to form
and 
ions, which can move freely and conduct electricity.
Formation of Magnesium Oxide (MgO)
Magnesium, a metal, reacts with oxygen, a non-metal, to form magnesium oxide. Magnesium donates two electrons to oxygen, forming a strong ionic bond.
This results in the formation of magnesium oxide (
), a compound used in refractory materials for high-temperature applications.
Amphoteric Nature of Certain Metal Oxides
Some metal oxides, like aluminum oxide (
) and zinc oxide (
), exhibit both acidic and basic properties. They react with both acids and bases to form salts and water. These oxides are called amphoteric oxides.
Example:
- Aluminum oxide (
) reacts with hydrochloric acid (
) to form aluminum chloride (
) and water:
) to form aluminum chloride (
) and water:
- It also reacts with sodium hydroxide (
) to form sodium aluminate (
) and water:
) to form sodium aluminate (
) and water:
Real-life Application:
Aluminum Oxide in Ceramics: Aluminum oxide is used in the production of ceramics and refractory materials due to its high melting point and resistance to chemical attack.
Practice Questions with Answers
Q1: What type of bond is formed between sodium and chlorine in sodium chloride ()?
- Answer: An ionic bond is formed between sodium and chlorine, where sodium donates one electron to chlorine.
Q2: Explain why magnesium reacts with oxygen to form magnesium oxide ().
- Answer: Magnesium loses two electrons to form a
ion, and oxygen gains two electrons to form an 
ion. The electrostatic attraction between these oppositely charged ions results in the formation of magnesium oxide.
ion, and oxygen gains two electrons to form an 
ion. The electrostatic attraction between these oppositely charged ions results in the formation of magnesium oxide.Q3: How does aluminum oxide exhibit amphoteric behavior?
- Answer: Aluminum oxide reacts with both acids (to form salts like aluminum chloride) and bases (to form sodium aluminate), showing its amphoteric nature.
FAQs
An amphoteric oxide is a metal oxide that can react with both acids and bases to form salts and water. Examples include aluminum oxide () and zinc oxide ().
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