Neeraj Anand, Param Anand

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.