Classification of Elements and Periodicity in Properties

Anand Classes presents a comprehensive explanation of the Modern Periodic Table, authored by Neeraj Anand and published by Anand Technical Publishers. This detailed guide is tailored for students preparing for JEE, NEET, and Class 11 CBSE Chemistry, covering the fundamental concepts of the Modern Periodic Law, the structure of the periodic table, and the classification of elements into periods, groups, and blocks. With a focus on clarity, exam relevance, and NCERT alignment, this article serves as an essential resource for mastering one of the most important topics in inorganic chemistry.

ANAND CLASSES notes of s-block elements of the periodic table include all elements whose last electron enters the s-orbital. These elements, which consist of alkali metals (Group 1) and alkaline earth metals (Group 2), are highly significant in inorganic chemistry because of their reactivity, periodic trends, and wide applications in daily life. This article is authored by Neeraj Anand and published by Anand Technical Publishers to provide clear and exam-oriented explanations for JEE and NEET students, following the NCERT Class 11 Chemistry syllabus.

Anand Classes notes of p-Block elements in the modern periodic table consist of Groups 13 to 18, and they include some of the most important families such as the boron family, carbon family, nitrogen family, oxygen family (chalcogens), halogens, and noble gases. Their general electronic configuration is ns²np¹–⁶, which gives them a wide range of properties from highly reactive non-metals (like halogens) to completely inert noble gases. The p-Block contains a unique combination of metals, non-metals, and metalloids, and it plays a crucial role in Class 11 chemistry, JEE, and NEET exam preparation.

Anand Classes Class 11 Notes of Elements with atomic numbers greater than 100 are synthetic, man-made superheavy elements that do not occur naturally and are produced in laboratories or nuclear reactors. Since their discovery often led to naming disputes, the International Union of Pure and Applied Chemistry (IUPAC) introduced a systematic nomenclature based on the digits of the atomic number. According to this system, each digit is replaced with a specific prefix and the name ends with “-ium”, ensuring unique temporary names and symbols until permanent names are officially assigned.

Anand Classes Notes of d-Block elements, also known as transition elements, are located in Groups 3 to 12 of the …

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Anand Classes Notes of f-Block elements, also called inner-transition elements, are located separately at the bottom of the periodic table. In these elements, the f-subshell of the inner-penultimate shell ((n-2)f shell) is progressively filled while the outermost shells have similar configurations. These elements show unique physical and chemical properties and are important for JEE, NEET, and CBSE Class 11 Chemistry.

The periodic table is divided into four main blocks — s-block, p-block, d-block, and f-block elements — based on the type of orbital that receives the last electron. Each block has unique position, electronic configuration, properties, and examples, making their comparison important for Class 11 Chemistry, JEE, and NEET preparation. This comparison covers their position in the periodic table, oxidation states, reactivity, metallic character, and special properties in a clear tabular format along with FAQs for quick revision.

Anand Classes Notes of Metals, non-metals, and metalloids are distributed in the periodic table according to their electronic configuration and chemical properties. Metals occupy the left and central portions of the table, non-metals are located on the right side, and metalloids lie along the zig-zag line separating the two. Understanding their position helps explain periodic trends such as metallic and non-metallic character, reactivity, and the types of oxides they form — an important topic in Class 11 Chemistry, JEE, and NEET.

The period and group number of an element in the periodic table can be determined from its electronic configuration using specific rules for s-, p-, d-, and f-block elements. These rules depend on the principal quantum number (n), the distribution of electrons in the outermost orbitals, and the block to which the element belongs. Knowing these rules is essential for solving periodic table questions in Class 11 Chemistry, JEE, and NEET.

Anand Classes explains the number of elements in each period of the periodic table follows the pattern 2, 8, 8, 18, 18, 32, 32 due to the way electrons fill atomic orbitals according to the Aufbau principle and the (n + l) rule. Each period corresponds to the filling of a new principal energy level, and the number of elements in that period depends on the total electron capacity of the subshells being filled. Understanding this explains why the 1st period has only 2 elements, the 2nd and 3rd periods have 8 elements each, the 4th and 5th periods have 18, and the 6th and 7th periods have 32 elements — an important concept for Class 11 Chemistry, JEE, and NEET.

Anand Classs Notes explain In Chemistry we can easily find the period, group, and block of an element in the periodic table by looking at its electronic configuration. This means, by knowing how the electrons are arranged in an atom, we can tell where the element is placed in the periodic table. It helps us understand the element’s properties and how it reacts with other elements.

Anand Classes explain how To find the position of an element in the periodic table, we can use its electronic configuration. This helps us easily determine the period, group, and block to which the element belongs. In this post, we’ll go through simple solved examples to understand how to apply these rules step by step. This is very helpful for students preparing for JEE, NEET, and CBSE Class 11 exams.

Anand Classes explain in the periodic table, elements are arranged in periods (horizontal rows) based on the way their electrons fill up different energy levels (shells). Each period starts with the filling of a new energy shell, and the number of elements in a period depends on how many orbitals are available in that shell to hold electrons. Let’s explore the electronic configurations of elements in the first three periods and understand why each period has a specific number of elements.

Anand Classes Notes explain the arrangement of elements in the periodic table follows a specific order based on the filling of electrons in atomic orbitals. From the fourth period onward, the pattern becomes more complex due to the involvement of d- and f-block orbitals. These periods include not only s- and p-block elements but also transition and inner transition elements. Understanding how these orbitals are filled explains why some periods have 18 or even 32 elements, unlike the shorter first three periods.

Anand Classes explains the periodic table is not just a list of elements—it’s a powerful tool that reveals the underlying pattern in chemical behavior. This repeating pattern, known as periodicity, occurs because elements with similar valence shell electron configurations exhibit similar chemical and physical properties. As we move across periods or down groups, these patterns repeat at regular intervals due to the systematic arrangement of electrons, especially in the outermost shell. Understanding this cause of periodicity helps explain why elements in the same group behave alike in reactions and form similar compounds.

Anand Classes Notes explains Atomic radius refers to the distance from an atom’s nucleus to its outermost electron shell, measured in different ways depending on context—covalent radius, metallic radius, or van der Waals radius. Understanding these radius types and their trends is vital for solving Class 11, NEET, and JEE chemistry problems on periodic properties and atomic structure.

Anand Classes Notes explains in atoms with more than one electron, the outer electrons are repelled by the inner electrons due to electron–electron repulsion. This repulsion reduces the full attractive force of the positively charged nucleus on the valence electrons. This phenomenon is known as the screening effect or shielding effect. The greater the number of inner electrons, the larger the shielding effect, which decreases the effective nuclear charge (Zeff) experienced by the outermost electrons. Slater, a scientist, formulated rules to calculate this shielding effect quantitatively, which are essential for understanding atomic structure and periodic trends.

Anand Classes Notes explains across any period in the periodic table, atomic radius generally decreases from left to right. This trend occurs because as the atomic number increases, the nuclear charge grows while electrons are added to the same principal energy level. Without significant shielding from electrons in the same shell, the increased effective nuclear pull draws electrons closer to the nucleus, resulting in a smaller atomic size.

Anand Classes explains the atomic radius of elements shows a clear trend when we move down a group in the periodic table. For both alkali metals (Group 1) and halogens (Group 17), the atomic radius increases as we go from top to bottom. This happens because each successive element down the group has an additional electron shell in its electronic configuration. The added shell increases the distance between the outermost electrons and the nucleus, while the shielding effect of inner electrons reduces the effective nuclear pull. As a result, the atoms become larger despite the increasing nuclear charge.

Anand Classes explains the Van der Waals radius is a measure of the size of an atom when it is not bonded to another atom but held together by weak Van der Waals forces in the solid state. Unlike covalent radius, which is measured for bonded atoms, Van der Waals radius is determined for non-bonded atoms in neighbouring molecules. This concept is especially important for noble gases, which do not form covalent bonds and therefore have their atomic radii expressed in terms of Van der Waals radii.

Anand Classes explains Ionic radius is the measure of the size of an ion, defined as the distance from the nucleus of the ion to the outermost electron shell. When an atom loses electrons to form a cation, the number of protons exceeds the number of electrons, pulling the remaining electrons closer to the nucleus and reducing the ionic radius. In contrast, when an atom gains electrons to form an anion, the increased electron–electron repulsion expands the outer shell, increasing the ionic radius. Understanding ionic radius trends across a period and down a group is important for predicting chemical reactivity, bond strength, and physical properties, making it a key topic for JEE, NEET, and CBSE Board examinations.

Anand Classes explains the radius of a cation is always smaller than that of its parent atom. This is because a cation is formed when one or more electrons are lost from a gaseous atom, often resulting in the complete removal of the outermost electron shell. For example, when a sodium atom (Na) loses its single 3s electron to form a Na+ ion, the entire 3s shell disappears, leading to a significant reduction in size—from 186 pm in Na to just 95 pm in Na+. This size decrease occurs because the nuclear charge remains the same while the number of electrons decreases, causing the remaining electrons to be pulled closer to the nucleus due to the increased effective nuclear charge.

Anand Classes explains the size of a negative ion (anion) is always larger than that of its corresponding neutral atom. This is because an anion is formed when a neutral atom gains one or more electrons, increasing the total number of electrons while the nuclear charge remains the same. The added electrons increase electron–electron repulsion and reduce the effective nuclear pull on each electron. As a result, the electron cloud expands, making the anion significantly larger than the parent atom. For example, chlorine (Cl) has an atomic radius of 99 pm, whereas the chloride ion (Cl⁻) swells to 181 pm.

Anand Classes Isoelectronic ions are ions of different elements that contain the same number of electrons but differ in their nuclear charges. A group of such ions is called an isoelectronic series. In any isoelectronic series, the electron count remains constant, but as the nuclear charge increases, the force of attraction between the nucleus and the electrons also increases. This stronger pull draws the electron cloud closer to the nucleus, resulting in a smaller ionic radius. Consequently, in an isoelectronic series, the size of the ions decreases as the nuclear charge increases.

Anand Classes presents a comprehensive collection of important questions and answers on atomic and ionic radii, specially designed for students preparing for JEE, NEET, and CBSE exams. This compilation focuses on understanding the size variations in atoms and ions, helping learners grasp key concepts such as nuclear charge, electron configuration, and periodic trends. Each question is paired with a detailed explanation, making complex topics easier to remember and apply during exams. Whether you are revising or practicing, these carefully crafted Q&As will strengthen your foundation in chemistry and boost your confidence.

Anand Classes explains that in every atom, electrons are held in place by the strong electrostatic attraction of the positively charged nucleus. This attraction is due to the opposite charges between the negatively charged electrons and the positively charged protons in the nucleus. The outermost or most loosely bound electrons experience a weaker pull compared to the inner electrons because they are farther from the nucleus and shielded by inner shells. To remove such an electron, energy must be supplied to overcome this attraction. The amount of energy needed for this process is called Ionization Enthalpy or Energy (IE) or Ionization Potential (IP). It serves as a quantitative measure in kJ mol⁻¹ of how easily an atom can lose an electron, providing important insight into the atom’s reactivity and chemical behavior.

Anand Classes presents a comprehensive explanation of the Factors Governing Ionization Enthalpy — the minimum amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state. Ionization enthalpy is a key concept in chemistry that reflects how strongly an atom holds its electrons. Its magnitude is influenced by several factors, including the size of the atom, nuclear charge, screening effect, penetration power of electrons, and the stability of the atom’s electronic configuration. Understanding these factors is essential for mastering periodic trends and predicting the chemical reactivity of elements.

Anand Classes explains that ionization enthalpy provides an excellent example for understanding the periodicity of elements in the periodic table. It is defined as the amount of energy required to remove the most loosely bound electron from an isolated gaseous atom in its ground state, and is expressed in kilojoules per mole (kJ mol⁻¹). By studying the variation of ionization enthalpy across periods and groups, we can clearly see the repeating patterns in element properties. The maxima in each period occur at noble gases, which have highly stable ns² np⁶ configurations, while the minima are found in alkali metals, which have a single loosely held ns¹ valence electron.

Anand Classes provides a clear and detailed explanation of the variation of ionization enthalpy down a group in the periodic table, an important topic for JEE, NEET, and CBSE Class 11 Chemistry. As we move from the top to the bottom of a group, ionization enthalpy gradually decreases due to factors such as an increase in atomic size, an increase in the shielding effect, and a relatively smaller impact of increasing nuclear charge. Understanding this periodic trend helps students predict the chemical reactivity, metallic character, and bonding nature of elements, making it a crucial concept for competitive exams and board preparation.

Anand Classes presents detailed study material on Ionization Enthalpy (Periodic Table) Class 11 Important Conceptual NCERT Question Answers for JEE, NEET, and CBSE Board students. Ionization enthalpy is a fundamental periodic property that explains the energy required to remove an electron from an isolated gaseous atom. Understanding this concept not only strengthens your basics of atomic structure but also helps in solving higher-order conceptual and numerical problems. In this article, you will find well-explained answers to NCERT questions, along with extra tips, solved examples, and exam-oriented insights.

Anand Classes brings you a clear and detailed explanation of Electron Gain Enthalpy (Electron Affinity), an important concept in Chemistry for JEE, NEET, and CBSE Class 11 students. Electron gain enthalpy is defined as the energy change that occurs when an electron is added to an isolated gaseous atom to form a negatively charged ion. Understanding this concept helps students grasp the reactivity trends of elements, periodic variations, and the stability of ions, making it a crucial topic for competitive exams.

Anand Classes brings you a detailed explanation of the important topic Factors Affecting Electron Gain Enthalpy for JEE, NEET, and CBSE Class 11 Chemistry. Electron gain enthalpy refers to the energy change when an isolated gaseous atom gains an extra electron to form a negative ion. Understanding how nuclear charge, atomic size, electronic configuration, and shielding effect influence electron gain enthalpy is crucial for mastering periodic trends and solving exam-based questions. This article provides clear theory, examples, FAQs, and comparisons to help students build strong conceptual clarity and score high in competitive as well as board examinations.

Anand Classes provides the best study material for JEE, NEET, and CBSE students. In this article, we explain one of the most important periodic properties – Electron Gain Enthalpy. It refers to the energy change when an atom gains an extra electron to form a negative ion. Understanding the periodic trends of electron gain enthalpy (variation across a period and down a group) is crucial for competitive exams like JEE Main, JEE Advanced, NEET, and Board examinations, as it helps in predicting the reactivity and chemical behavior of elements.

Anand Classes brings you a detailed explanation of why halogens have the highest negative electron gain enthalpies in the periodic table. Halogens (Group 17 elements) like fluorine, chlorine, bromine, iodine, and astatine possess the electronic configuration ns²np⁵, which makes them just one electron short of achieving the stable noble gas configuration. This unique property gives halogens a very strong tendency to accept an additional electron, releasing a large amount of energy in the process. As a result, their electron gain enthalpies are highly negative, a key concept often asked in JEE, NEET, and CBSE Class 11 Chemistry exams.

Anand Classes explains the concept of electron gain enthalpy of noble gases, beryllium (Be), magnesium (Mg), nitrogen (N), and phosphorus (P) in detail for JEE, NEET, and CBSE examinations. While most elements have negative electron gain enthalpy due to their tendency to attract electrons, noble gases exhibit positive electron gain enthalpy because of their stable octet configuration (ns2np6). On the other hand, Be and Mg with completely filled s-orbitals, and N and P with half-filled p-orbitals, show very low or nearly zero electron gain enthalpy values due to their extra stability. Understanding these exceptions is crucial for mastering trends in the periodic table and is a frequently asked concept in competitive exams.

Anand Classes explains the important concept of electron gain enthalpy of halogens in a simple yet detailed way for JEE, NEET, and CBSE students. The trend of electron gain enthalpy in halogens (F, Cl, Br, I, At) is an essential topic of the periodic table, often asked in competitive exams. While generally electron gain enthalpy becomes less negative down the group, fluorine shows an anomaly where its value is less negative than chlorine. Understanding this exception, along with the overall trend, helps students strengthen their grasp on periodic properties and improve exam performance.

Anand Classes explains that the electron gain enthalpy of second-period elements (such as N, O, F) is generally less negative than their third-period counterparts (such as P, S, Cl). This trend arises because second-period elements are very small in size, and when an extra electron is added, it experiences strong electron–electron repulsions in the compact 2p orbitals. In contrast, third-period elements have larger atomic sizes and more diffused orbitals, so the incoming electron experiences less repulsion and greater attraction from the nucleus, resulting in more negative electron gain enthalpy values. This concept is important for JEE, NEET, and CBSE Class 11 Chemistry as it explains anomalies in periodic trends.

Anand Classes explains that successive electron gain enthalpies (EA₁, EA₂) represent the energy changes when one or more electrons are added to a gaseous atom. The first electron gain enthalpy (EA₁) is usually negative because a neutral atom attracts the incoming electron and energy is released. However, the second electron gain enthalpy (EA₂) is always positive, since the electron is being added to a negatively charged ion and experiences strong Coulombic repulsion, requiring external energy input. For example, in oxygen, EA₁ = –141 kJ mol⁻¹ (energy released), while EA₂ = +780 kJ mol⁻¹ (energy absorbed).

🔹 Welcome to Anand Classes!In this session, we dive into “Classification of Elements & Periodicity – Modern Periodic Law, Periods …

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Why Fluorine (F) has a more negative electron gain enthalpy than Oxygen (O) ?
because: (a) It has a 2s²2p⁵ configuration, needing only one electron to complete its octet.
(b) Its small size and high nuclear charge attract the extra electron strongly.

Anand Classes provides comprehensive notes on Electron Gain Enthalpy in the Periodic Table with a clear comparison between fluorine and chlorine for JEE, NEET, and CBSE Class 11 Chemistry. Understanding why chlorine has a more negative electron gain enthalpy than fluorine is essential for mastering concepts of periodic trends and scoring high in exams. These detailed explanations, tables, FAQs, and solved examples will help students build a strong foundation in chemistry. Click the print button to download study material and notes.

Anand Classes provides the best JEE/NEET study material, notes, and solved examples to help aspirants master important concepts like electron gain enthalpy for NEET, JEE, and CBSE exams. Our step-by-step solutions, FAQs, and numerical problems are designed to strengthen conceptual clarity and improve exam performance. Click the print button to download NEET, JEE, and CBSE study material and notes.

Anand Classes provides the best study material and notes for JEE, NEET, and CBSE students, helping them master important concepts …

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Anand Classes brings you detailed study material on Electronegativity, an essential concept in Chemistry for JEE, NEET, and CBSE Board exams. Electronegativity explains the ability of an atom to attract shared electrons in a chemical bond and plays a vital role in understanding bond polarity, reactivity, and periodic trends. This comprehensive guide covers the definition, Pauling scale, Mulliken scale, other electronegativity scales, FAQs, and applications with easy-to-understand explanations for students. Click the print button to download study material and notes.

Anand Classes brings you a detailed explanation of Factors Affecting Electronegativity in Chemistry, an important concept for JEE, NEET, and CBSE Class 11 exams. Electronegativity is not a fixed property of an atom; rather, it varies with factors such as oxidation state, type of hybridisation, and the nature of substituents. Understanding these variations helps students build strong conceptual clarity and perform better in competitive exams. Click the print button to download study material and notes.

Anand Classes brings you a detailed explanation of the Periodic Variation of Electronegativity for Class 11, NEET, and JEE aspirants. Electronegativity is a fundamental concept in chemistry that helps us understand how atoms attract shared electrons in a covalent bond. In this study material, we explain how electronegativity changes across a period and down a group in the periodic table, along with its relation to atomic size, effective nuclear charge, and ionization enthalpy. This topic is extremely important for competitive exams as well as CBSE board preparation. Click the print button to download study material and notes.

Anand Classes provides comprehensive study material on Electronegativity and its relation to Metallic and Non-Metallic Character for Class 11, NEET, and JEE preparation. Understanding electronegativity trends across the periodic table is essential to predict the chemical behavior of elements, bond formation, and the distinction between metals, non-metals, and metalloids. This concept also helps students in mastering important topics like periodic properties, bond polarity, and the classification of elements. Click the print button to download study material and notes.

Anand Classes provides a detailed explanation of the difference between electron gain enthalpy and electronegativity, covering their definitions, properties, measurable …

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Anand Classes brings you a detailed explanation of Periodicity of Valence and Oxidation States for JEE, NEET, and CBSE students. Valence, the combining capacity of an atom, depends on the number of electrons present in the outermost shell, and it plays a vital role in determining the chemical properties of elements. Understanding how valency and oxidation states vary across periods and groups in the Periodic Table is essential for mastering competitive exams as well as board exams. Click the print button to download study material and notes.

Anand Classes brings you detailed notes on Periodic Trends and Chemical Reactivity with clear explanations of metallic and non-metallic character, ionization enthalpy, electron gain enthalpy, and electronegativity. These well-structured notes are designed for JEE, NEET, and CBSE Class 11 students to strengthen their conceptual understanding and improve exam performance. Click the print button to download study material and notes.

Anand Classes provides a detailed NCERT Intext 3.1 solution for the question “What would be the IUPAC name and symbol …

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Anand Classes provides a detailed NCERT Intext 3.2 solution for Class 11 Chemistry: How would you justify the presence of 18 elements in the 5th period of the Periodic Table? The explanation is based on the electronic configuration, filling of orbitals, and periodic trends that determine why exactly 18 elements are present in the 5th period. This makes it easier for JEE, NEET, and CBSE students to understand the concept clearly with proper reasoning. Click the print button to download study material and notes.

Anand Classes provides the detailed NCERT Intext 3.3 solution for Class 11 Chemistry: The elements Z = 117 and 120 have not yet been discovered. In which family/group would you place these elements and also give the electronic configuration in each case? The solution explains how Z = 117 belongs to the halogen family (Group 17) with configuration [Rn] 5f¹⁴ 6d¹⁰ 7s² 7p⁵, and Z = 120 belongs to the alkaline earth metals (Group 2) with configuration [Uuo] 8s². This explanation is important for JEE, NEET, and CBSE students to understand periodic table predictions. Click the print button to download study material and notes.

Anand Classes provides the NCERT Intext 3.4 solution for Class 11 Chemistry: Considering the atomic number and position in the periodic table, arrange the following elements in the increasing order of metallic character: Si, Be, Mg, Na, P. The solution is explained with periodic trends, showing how metallic character increases down a group and decreases across a period. Hence, the increasing order of metallic character is P < Si < Be < Mg < Na. This clear explanation is highly useful for JEE, NEET, and CBSE Class 11 students. Click the print button to download study material and notes.

Anand Classes provides the NCERT Intext 3.5 solution for Class 11 Chemistry: Which of the following species will have the largest and the smallest size: Mg, Mg²⁺, Al, Al³⁺? The solution is explained using periodic trends, effect of cation formation, and the concept of isoelectronic species. It is concluded that the largest species is Mg, while the smallest species is Al³⁺. This step-by-step explanation is very useful for JEE, NEET, and CBSE Class 11 Chemistry students. Click the print button to download study material and notes.

Anand Classes brings you detailed solutions for **Classification of Elements and Periodicity in Properties | NCERT Intext Problems 3.1, 3.2, 3.3, 3.4, 3.5, 3.6, 3.7, 3.8, 3.9, and 3.10**. These step-by-step NCERT solutions are explained in simple language with proper reasoning and are highly useful for **Class 11 Chemistry, CBSE Exams, JEE, and NEET preparation**. Each problem is solved in detail to help students strengthen their understanding of periodic trends, periodic table, and properties of elements. Click the print button to download study material and notes.

Anand Classes presents detailed NCERT Class 11 Chemistry Chapter 3 solutions on Classification of Elements and Periodicity in Properties (Intext …

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Anand Classes presents NCERT Solutions for Chemistry Class 11 Chapter 3 – Classification of Elements and Periodicity in Properties (Questions 3.6, 3.7, 3.8, 3.9, 3.10). These solutions provide detailed explanations about the periodic table, atomic number determination, element naming, similarities in group properties, atomic radius, ionic radius, and periodic trends in atomic size. The step-by-step answers make it easier for students to understand and prepare effectively for exams. Click the print button to download study material and notes.

Anand Classes provides complete NCERT solutions for Class 11 Chemistry, covering exercises 3.11, 3.12, 3.13, 3.14, and 3.15 on the topic Classification of Elements and Periodicity in Properties. This post explains concepts such as ionic radii, ionization enthalpy, electron gain enthalpy, and calculations related to the hydrogen atom in a simple, step-by-step manner. Each solution is designed to help students understand the fundamentals of atomic structure, periodic trends, and chemical properties effectively. Click the print button to download study material and notes.

Anand Classes provides complete NCERT solutions for Class 11 Chemistry, covering exercises 3.16, 3.17, 3.18, 3.19, and 3.20 on the topic Classification of Elements and Periodicity in Properties. This post explains key concepts such as ionization enthalpy, electron gain enthalpy, deviations in periodic trends, and factors affecting atomic and ionic properties with clear, step-by-step explanations. Each solution is designed to help students understand periodic behavior and atomic structure effectively. Click the print button to download PDF study material and notes.

Anand Classes brings you detailed NCERT Solutions for Class 11 Chemistry Chapter 3 – Classification of Elements and Periodicity in Properties covering Questions 3.21, 3.22, 3.23, 3.24, and 3.25. These step-by-step solutions explain important concepts like electron gain enthalpy, electronegativity, atomic radius, and ionization enthalpy of isotopes. Our solutions are designed to help Class 11 students build strong conceptual clarity and prepare effectively for exams. Click the print button to download pdf study material and notes.

Anand Classes provides detailed NCERT Solutions for Class 11 Chemistry Chapter 3 – Classification of Elements and Periodicity in Properties (Questions 3.31 to 3.35). These step-by-step solutions explain important concepts such as ionization enthalpy, electron gain enthalpy, reactivity trends, electronic configurations, periodic table structure, quantum numbers, and factors affecting valence electrons. These solutions are highly useful for CBSE board exams as well as competitive exams like NEET and JEE. Click the print button to download study material and notes.

Anand Classes provides detailed NCERT Solutions for Class 11 Chemistry Chapter 3 – Classification of Elements and Periodicity in Properties. In this section, we cover questions 3.36 to 3.40 with step-by-step explanations, focusing on concepts like isoelectronic species, ionization enthalpy, metallic and non-metallic character, and oxidizing properties of elements. These solutions help students strengthen their conceptual clarity and prepare effectively for school exams and competitive entrance tests. Click the print button to download study material and notes.

Anand Classes presents NEET Topicwise PYQ Previous Year Questions & Solutions on Periodic Table & Classification of Elements. These detailed, chapter-wise solutions are designed to help NEET aspirants strengthen their concepts in the periodic table, modern periodic law, classification of elements, electronic configuration, periodic trends, and properties of elements. By practicing previous year NEET questions with step-by-step solutions, students can build strong exam strategies and boost their problem-solving skills. Click the print button to download study material and notes.

Anand Classes provides detailed NCERT Solutions for Class 11 Chemistry Chapter 3 – Classification of Elements and Periodicity in Properties (Questions 3.26 to 3.30). These step-by-step solutions help students understand the concepts of periodic table, periodic trends, electronic configuration, ionization enthalpy, reactivity, and properties of s, p, d, and f block elements. This study material is designed for CBSE and competitive exam preparation like NEET and JEE. Click the print button to download study material and notes.

Anand Classes provides detailed NEET PYQs MCQs Solutions on Periodic Table Properties with clear explanations and solved answers to help students master important concepts for competitive exams. These step-by-step solutions cover tricky questions on periodic trends such as atomic radius, ionization enthalpy, electronegativity, and the properties of s-block, p-block, d-block, and f-block elements. Designed for quick revision and exam preparation, this study material ensures conceptual clarity for NEET aspirants. Click the print button to download study material and notes.

Anand Classes provides detailed NEET PYQs Chapterwise Solutions for Periodic Table Properties to help students strengthen their preparation for competitive exams. With step-by-step explanations and accurate answers, these solutions make it easier to understand the concepts and improve problem-solving skills. Whether you are revising important topics or practicing previous year questions, this resource will boost your confidence for NEET Chemistry. Click the print button to download study material and notes.

Anand Classes provides comprehensive NEET Periodic Table PYQs with detailed solutions and practice MCQs in PDF format to help students prepare effectively for their medical entrance exam. The study material includes important questions from previous years, solved examples, and additional practice sets to strengthen concepts related to the periodic table and classification of elements. This resource is designed to help students revise, practice, and score better in the NEET exam with ease. Click the print button to download study material and notes.

Anand Classes provides comprehensive study material and practice questions for medical entrance exams, including NEET PYQs and AIIMS MCQs with solutions. This detailed guide on the classification of elements and periodicity in properties helps students understand key concepts, solve previous years’ questions, and boost their exam preparation effectively. With expert explanations and structured notes, students can master this important topic and gain confidence in tackling complex problems. Click the print button to download study material and notes.

Anand Classes provides NEET PYQs (Periodic Table) Competency Based Questions (CBQs) with detailed step-by-step solutions from the chapter Classification of Elements and Periodicity in Properties. These solved past year questions help students understand periodic trends like ionisation energy, electronegativity, atomic size, metallic character, and chemical reactivity. Mastering these concepts is essential for cracking NEET Chemistry with accuracy and speed. Click the print button to download study material and notes.

Anand Classes brings you JEE Main Previous Year Questions (PYQs) on Periodic Table & Periodicity, arranged chapter-wise and topic-wise in MCQ format with detailed solutions. These practice questions are designed to help students master concepts of the periodic table, trends, and periodic properties, ensuring high scores in competitive exams like JEE Main and Advanced. With comprehensive coverage of all important topics, this PDF study material is perfect for revision and last-minute preparation. Click the print button to download study material and notes.

Anand Classes presents JEE Main PYQs Topicwise Chapterwise Periodic Table & Periodicity PDF Download designed to help students prepare effectively for their exams. This study material covers previous year questions arranged systematically by topic and chapter, making it easier for aspirants to practice and strengthen concepts of Periodic Table and Periodicity. With well-structured notes and solved questions, students can enhance their understanding and improve their performance in JEE Main. Click the print button to download study material and notes.

Anand Classes brings you the most important and frequently asked MCQs with solutions from previous years’ JEE Main papers based on the Periodic Table. This study material is carefully curated to help students strengthen their concepts, revise efficiently, and score better in exams. Each question comes with a detailed solution to enhance understanding and problem-solving skills. Click the print button to download study material and notes.

Anand Classes provides JEE Main important previous years’ questions (PYQs) along with chapterwise MCQs and solutions from the Periodic Table chapter. This resource is designed to help students practice effectively, understand concepts clearly, and perform confidently in the exam. Each question is accompanied by step-by-step solutions to aid learning and revision. Click the print button to download study material and notes.

Anand Classes provides carefully curated Periodic Table JEE Main PYQs and Competency Based Questions (CBQs) with detailed solutions to help students strengthen their understanding of chemistry concepts. This study material covers important multiple-choice questions (MCQs) from past years, ensuring that learners practice the most relevant topics for competitive exams like JEE Main. Designed for self-study and classroom learning, these resources will guide students to improve their accuracy and problem-solving skills. Click the print button to download study material and notes.

Anand Classes provides the most comprehensive Periodic Table Class 11 JEE Main PYQs : MCQs With Solutions PDF Download to help students prepare effectively for competitive exams. This study material includes previous years’ questions, multiple-choice questions (MCQs), and detailed solutions based on the JEE Main syllabus. The notes are designed to strengthen conceptual understanding and boost problem-solving skills for better performance. Click the print button to download study material and notes.

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