How do Metals and Non-Metals React?

Exploring Electron Transfer and Ionic Bond Formation

Core Concept
Elements react to achieve a stable electronic configuration like noble gases. Metals lose electrons to form positive ions (cations), while non-metals gain electrons to form negative ions (anions). These oppositely charged ions attract each other to form ionic compounds.
Electronic Configuration
Noble gases have completely filled valence shells, making them stable and chemically inactive.
Na → Na⁺ + e⁻
Sodium loses one electron

Element Colors

Sodium (Na)
Chlorine (Cl)
Magnesium (Mg)
Electrons
Element Atomic Number K L M N
Helium (He)22---
Neon (Ne)1028--
Argon (Ar)18288-
Sodium (Na)11281-
Chlorine (Cl)17287-

📚 Theory & Concepts

Deep dive into the fundamental principles of metal and non-metal reactions

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Electronic Configuration

🔹 Noble Gas Stability

Noble gases have completely filled outer shells (octet rule), making them chemically stable and unreactive.

🔹 Valence Electrons

Electrons in the outermost shell determine an atom's chemical behavior and bonding capacity.

🔹 Shell Structure

K(2), L(8), M(8), N(18) - each shell can hold a maximum number of electrons following 2n² rule.

⚡

Ion Formation

🔹 Cation Formation

Metals lose electrons to achieve noble gas configuration, forming positive ions (cations).

🔹 Anion Formation

Non-metals gain electrons to complete their octet, forming negative ions (anions).

🔹 Energy Changes

Ionization energy (losing e⁻) vs. Electron affinity (gaining e⁻) determines feasibility.

🔗

Ionic Bond Formation

🔹 Electrostatic Attraction

Oppositely charged ions attract each other due to Coulombic forces, forming ionic bonds.

🔹 Lattice Energy

Energy released when gaseous ions form a solid ionic compound - determines stability.

🔹 Formula Writing

Ionic compounds have no discrete molecules - formula shows simplest ratio of ions.

🔬

Properties of Ionic Compounds

🔹 Crystal Structure

Ions arrange in regular 3D patterns (lattices) with alternating positive and negative charges.

🔹 High Melting Points

Strong ionic bonds require significant energy to break, resulting in high melting points.

🔹 Solubility

Polar solvents like water can dissolve ionic compounds by surrounding and separating ions.

🔹 Electrical Conductivity

Conduct electricity when molten or dissolved due to free-moving charged particles.

💡

Applications of Ionic Compounds

🔹 Fertilizers

Many ionic salts (e.g. KNO₃, NH₄SO₄) supply key crop nutrients essential for plant growth.

🔹 Medicines

Ionic compounds act as antacids (Mg(OH)₂), electrolytes, and drug salts for enhanced absorption.

🔹 Everyday Items

Table salt (NaCl), detergents, and batteries all utilize ionic compounds in daily life.

🔹 Industry

Used for extraction, purification, ceramics, glass, LEDs, and water treatment processes.

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Ionic vs Covalent Bonds

🔹 Bond Nature

Ionic: Full electron transfer between atoms.
Covalent: Electrons are shared between atoms.

🔹 Structure

Ionic: Forms continuous lattices.
Covalent: Forms discrete molecules.

🔹 Physical Properties

Ionic: Solid, high melting pt., conducts in solution.
Covalent: Often gas/liquid/soft solid, low melting pt., non-conducting.

🔹 Examples

Ionic: NaCl.
Covalent: H₂O, CO₂, O₂.