The Periodic table and p-Block elements are an essential topics from the JEE Main 2026 Chemistry syllabus, and form a significant part of the Inorganic Chemistry section. Having a strong hold over these subjects is not only important for conceptual knowledge but also to improve problem-solving skills, which is key in achieving a good score in the
JEE Main 2026
exam. This paper gives a thorough introduction to periodic trends and the p-Block elements, and how to succeed in this study area.
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Recent Trends in Periodic Table for JEE Main 2026
The modern periodic table is arranged on the basis of increasing atomic number, reflecting the periodic recurrence of chemical properties. Understanding key periodic trends is essential for predicting element behaviour and reactivity.
Atomic and Ionic Radii: Across a period, atomic size decreases due to increasing nuclear charge pulling electrons closer. Down a group, radii increase due to additional electron shells.
Ionisation Energy: The energy required to remove an electron from an atom generally increases across a period and decreases down a group. This relates to the effective nuclear charge and distance of outer electrons.
Electron Affinity and Electronegativity: Electron affinity tends to increase across periods, while electronegativity follows similar periodic trends, playing a major role in bond formation.
Metallic and Non-metallic Character: Metallic character decreases across a period and increases down a group; non-metallic character changes inversely.
Valence Electrons and Oxidation States: The position in the periodic table aids in deducing valence electrons and common oxidation states, crucial for understanding chemical reactivity.
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Focus on p-Block Elements (Groups 13-18) for JEE Main 2026
The p-block elements consist of group 13-18 of the periodic table and have various properties and uses as they can be metals, metalloids and non-metals. Their chemistry is differentiated by the fact that the electrons in the p-orbital are valence electrons.
Group-wise Electronic Configuration and Trends: Elements in the p-block have the general valence configuration ns2np1−6ns^2 np^{1-6}ns2np1−6. The properties systematically change moving from group 13 (Boron family) to group 18 (Noble gases).
Physical and Chemical Properties: Trends in atomic size, ionisation energies, and electronegativity follow periodic patterns. The inertness of noble gases, reactivity of halogens, and amphoteric nature of some elements like aluminium are commonly examined topics.
Anomalous Behaviour of First Elements: The first elements of groups often exhibit exceptional behaviour; for example, Boron is a metalloid unlike other group 13 metals, and Oxygen exhibits different oxidation states compared to heavier chalcogens.
Important Compounds and Uses: Familiarity with oxides, hydrides, halides, and important industrial compounds (e.g., boric acid, sulfuric acid, nitrogen oxides) is essential for JEE.
Oxidation States and Allotropes: Variable oxidation states and the existence of allotropes like phosphorus (white, red, black) and sulfur enrich the chemical diversity of p-block elements.
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The elements of the periodic table and p-block are a pillar in inorganic chemistry for JEE Main 2026. The mastery of these subjects is based on a focused study program, which includes clarity of the concepts and a lot of practice of both theory and numbers. With new strategic changes based on syllabus weight and continuous self-assessment with the help of mock exams, the ability to achieve good results in the Chemistry part of JEE Main 2026 will be improved.
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FAQs
Build conceptual clarity on electronic configurations and periodicity, practice numerical and conceptual problems regularly, and review previous year questions extensively to understand question patterns and difficulty level.
Focus on common oxidation states, allotropes (like different forms of phosphorus and sulfur), and important oxides, hydrides, and halides of groups 13-18 elements relevant to the syllabus.
The first elements (e.g., Boron, Carbon, Oxygen) often exhibit unique properties due to their small size, high ionisation energy, and absence of d-orbitals, leading to deviations in trends and chemical behaviour.
Across a period, atomic size decreases, ionisation energy and electronegativity increase, while metallic character decreases. Down a group, atomic size increases, ionisation energy and electronegativity decrease, and metallic character increases.
Key trends include atomic and ionic radii, ionisation energy, electron affinity, electronegativity, metallic and non-metallic character, and reactivity patterns across periods and groups.
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