Ionisation Energy | Periodic Table Part 2 | For JEE Mains and Advanced 2026 | @InfinityLearn-JEE

In this power-packed session, we dive deep into Ionisation Energy—a crucial concept in the Periodic Table chapter that frequently appears in both JEE Main and Advanced exams. Get conceptual clarity with visual explanations, trends across periods and groups, and tricks to tackle tough questions in seconds!

Ionisation Energy (IE), also known as Ionisation Enthalpy, is the minimum amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state.

In this video, you will learn:
➜Definition and significance of ionisation energy: M(g)→M⁺(g)+e^−
The energy required for this process is called the first ionisation energy (IE₁). The second ionisation energy (IE₂) refers to the energy needed to remove another electron from the resulting cation (M⁺), and so on.
➜Trends across periods and down groups
🔹 Across a Period (Left to Right): Ionisation energy increases.
►Why?
Atomic size decreases
Nuclear charge increases
Electrons are held more tightly
🔹 Down a Group (Top to Bottom): Ionisation energy decreases.
►Why?
Atomic size increases
Increased electron shielding
Valence electron is farther from the nucleus
➜Exceptions and the reasons behind them: Some elements deviate from the general trend due to:
Stable electron configurations (like full or half-filled subshells)
Electron-electron repulsion in orbitals
➜Factors affecting ionisation energy
Atomic size: Larger atoms → lower IE
Nuclear charge: More protons → higher IE
Shielding effect: More inner electrons → lower IE
Electron configuration: Stable configurations resist losing electrons
➜Previous year JEE questions and quick-solving techniques

Ideal for JEE 2026 aspirants who want a strong grasp of periodic properties to build a solid foundation in inorganic chemistry.

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Видео Ionisation Energy | Periodic Table Part 2 | For JEE Mains and Advanced 2026 | @InfinityLearn-JEE канала Infinity Learn JEE