Ncert Solutions for Class 11 Chemistry Chapter 3 in English
Class 11 Chemistry Chapter 3 NCERT solutions: Adda247 provides NCERT solutions for class 11 chemistry. The NCERT Solutions provided here will enhance the concepts of the students, as well as suggest alternative methods to solve particular problems to the teachers.
These NCERT Solutions Class 11 chemistry are presented in a very simple language so that you can understand the basic of chemistry with ease. These NCERT Solutions class 11 Chemistry cover chapters 1 to 14 with all important questions and answers explained in a detailed way.
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The solutions available are in depth and simplest way. Thus will help the students beyond examination marks. This will help them develop a core understanding of the subject. Because this subject demands to understand rather than just memorizing solutions of Class 11 Chemistry. Here below we are providing you with the overview of all the chemistry Class 11 Chapters that are there in the NCERT textbook.
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NCERT Solutions for Class 11 Chemistry Chapter – 3: Classification of Elements and Periodicity in Properties
Due to discovery of different elements, it was difficult to organize the information and properties of the elements, so there was a strong need to find some pattern in the properties of different elements so that they can be grouped together. That’s why we classify elements.
Elements can be classified as metals, metalloids, and nonmetals, or as a main-group elements, transition metals, and inner transition metals.
Properties That Display Periodicity
Ionization Energy – This is the energy needed to completely remove an electron from an atom or ion. …
Electronegativity – A measure of how readily an atom forms a chemical bond. …
Atomic Radius – This is half the distance between the middle of two atoms just touching each other.
The elements and their compounds can be classified according to their chemical and physical characteristics. A couple of major classifications that you are no doubt already familiar with are: acids vs. bases, metals vs.
What is called periodicity?
- The tendency, quality, or fact of recurring at regular intervals.
- Chemistry. The occurrence of similar properties in elements occupying similar positions in the periodic table.
NCERT Solutions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties are provided on this page for perusal of CBSE class 11 students. Comprehensive, student-friendly answers to all exercise questions provided in Chapter 3 of the NCERT class 11 Chemistry textbook can be accessed on this page. Students can understand the fundamental concepts effectively using the solutions present at Adda247.
In Chapter 3, all crucial topics are explained with much importance as questions based on them can appear in the final exam and other competitive exams. The detailed explanations provided for each concept provides students with a good learning experience. The faculty design the solutions in such a way that students will learn how to approach complex questions and answer them. Also, these NCERT Solutions can be downloaded in a PDF format by clicking the downloaded button provided below.
Topic covered in this chapter include:
- Genesis of periodic classification
- Modern periodic law and the present of the periodic table
- Nomenclatures of elements with atomic number greater than 100
- Electronic configuration of elements and the periodic table
- The s-block, p-block, d-block, and f-block elements
- Metals, non-metals and metalloids
- Periodic trends in properties of elements
- Trends in physical properties
- Trends in chemical properties
- Trends in chemical reactivity
The NCERT Solution for Class 11 Chemistry provided on this page feature the following types of questions
- Questions on trivial systems for the classification of elements
- Questions on the modern periodic table and the nomenclature of elements with Z > 100
- Problems based on quantum numbers and electron configurations
- Atomic/ ionic radii, ionization enthalpy, electron affinity, electronegativity and reactivity of elements and their trends.
Important question of NCERT Solutions of Chemistry Class 11 Chapter 3
Question: 1 What is the basic theme of organisation in the periodic table?
The basic theme of organization of elements in the periodic table is to classify the elements in period and groups according to their properties. This arrangement makes the study of elements and their compounds simple and systematic. In the periodic table, elements with similar properties are placed in the same group’
Question: 2 Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?
Mendeleev was the first to develop a periodic table & he gave a law called Mendeleev periodic law which states that the physical & chemical properties of the elements are a periodic function of their atomic masses. On the basis of this law he developed a Mendeleev periodic table, where he arranged the elements in his periodic table ordered by atomic weight or mass. He arranged the elements in periods and groups in order of their increasing atomic weight. He placed the elements with similar properties in the same group.
However, he did not stick to this arrangement for long. He found out that if the elements were arranged strictly in order of their increasing atomic weights, then some elements did not fit within this scheme of classification.
Therefore, he ignored the order of atomic weights in some cases. For example, the atomic weight of iodine is lower than that of tellurium. Still Mendeleev placed tellurium (in Group VI) before iodine (in Group VII) simply because iodine’s properties are so similar tofluorine, chlorine, and bromine
Question: 3 What is the basic difference in approach between the Mendeleev’s Periodic Law and the Modern Periodic Law?
Mendeleev’s periodic law states that the physical and chemical properties or the elements are periodic function of their atomic weight. On the other hand, the Modern periodic law states that the physical and chemical properties of the elements are the periodic function of their atomic numbers.
Question: 4 On the basic of quantum numbers, justify that the sixth period of the
periodic table should have 32 elements.
Sixth period corresponds to n = 6. In this period 16 orbitals, viz, one 6 s, seven 4f, five 5d and three 6p orbitals are filled. These sixteen orbitals can accommodate 32 elements. So, there are 32 elements in the sixth period
Question: 5 In terms of period and group where would you locate the element with Z=114?
Elements with atomic numbers from Z = 87 to Z = 114 are present in the 7th period of the periodic table. Thus, the element with Z = 114(Flerovium) with atomic weight 289 and a poor metal is present in the 7th period & 14th group of the periodic table
In the 7th period, first two elements with Z = 87 and Z= 88 are s-block elements, the next 14 elements excluding Z = 89 i.e., those with Z = 90 – 103 are f – block elements, ten elements with Z = 89 and Z = 104 – 112 are d – block elements, and the elements with Z = 113 – 118 are p – block elements. Therefore, the element with Z = 114 is the second p – block element in the 7th period
Question: 6 Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
There are two elements in the 1st period and eight elements in the second period. The third period starts with the element with z = 11. Now there are eight elements in the third period. Thus, the third period ends with the element with z = 18 I,e, the element in the 18th group of the 3rd period has z = 18. Hence, the element in the 17th group of the third period has atomic number z = 17.
Question: 7 Which element do you think would have been named by
- Lawrence Berkeley Laboratory
- Seaborg’s group?
- Lawrencium (Lr) with z = 103 and Berkelium (Bk) with z = 97
- Seaborgium (Sg) with z = 106.
Question: 8 Why do elements in the same group have similar physical and chemical properties?
The physical and chemical properties of an elements depend on the no. of valence electrons. Elements present in the same group have the same number of valence electrons. Therefore, elements present in the same group have similar physical and chemical properties.
Question: 9 What does atomic radius and ionic radius really mean to you?
Atomic radius & ionic radius are the periodic properties which are directly or indirectly related to the electronic configuration of their atoms & shows gradation on moving down a group or along a period.
Atomic radius is defined as the distance from the centre of the nucleus to the outer most shell containing the electrons. It measures the size of an atom.It is of 3 types:
- A) Covalent radius- It is the one half of the distance between the centres of the nuclei of two adjacent similar atoms joined to each other by single covalent bond.
Covalent radius = inter nuclear distance in the bonded atoms/ 2
- B) Metallic radius- It is defined as half the distance between the centres of the nuclei of two adjacent atoms in the metallic crystal
- C) Van der waal’s radius- It is defined as one half of the inter nuclear distance between 2 similar adjacent atoms belonging to the two neighbouring molecules of the same substance in the solid state.
Ionic radius means the radius of an ion (cation or anion). It is defined as the distance from the centre of the nucleus of the ion upto which it exerts its influence on the electron cloud.The ionic radii can be calculated by measuring the distances between the cations and anions in ionic crystals.
Since a cation is formed by removing an electron from an atom, the cation has fewer electrons than the parent atom resulting in an increase in the effective nuclear charge. Thus, a cation is smaller than the parent atom. For example, the ionic radius of Na+ ion is 95 pm, whereas the atomic radius of Na atom is 186 pm. On the other hand, an anion is larger in size than its parent atom. This is because an anion has the same nuclear charge, but more electrons than the parent atom resulting in an increased repulsion among the electrons and a decrease in the effective nuclear charge. For example, the ionic radius of F– ion is 136 pm, whereas the atomic radius of F atom is 64 pm.
Question: 10 How do atomic radius vary in a period and in a group? How do you explain the variation?
Atomic radius generally decreases from left to right across a period. This is because within a period, the outer electrons are present in the same valence shell and the atomic no. increases from left to right
across a period, resulting in an increased nuclear charge. As a result, the attraction of electrons to the nucleus increased.
On the other hand, the atomic radius generally increase down a group. This is because down a group, the principal quantum number increases which results in an increase of the distance b/w the nucleus and valence electrons.
Frequently asked questions on NCERT Solution Chemistry Class 11 Chapter 3
- Write the key benefits of NCERT Solutions for Class 11 Chemistry Chapter 3 Classifications of Elements and Periodicity in Properties.
- The solutions provided in NCERT Solutions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties are Offered in a step by step approach for a comfortable and better understanding of concepts.
- It also provides explanatory diagrams and tables for comparative study, which creates an interest in learning.
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- How NCERT Solutions for Class 11 Chemistry Chapter 3 helpful for Class 11 Students?
Ans. The NCERT Solutions for class 11 Chemistry chapter 3 can help the students to clear their doubts and prepare themselves for the exam in a better way. The NCERT questions not only help for board exams preparation but also for different competitive exams.
- How to score high marks using NCERT Solutions for Class 11 Chemistry Chapter 3 in final exams?
Answer: Students are advised to follow the NCERT Solutions for Class 11 Chapter 3 on a regular basis to get in-depth knowledge about all the concepts covered in the syllabus. These NCERT Solutions for Class 11 are prepared by our Adda247 expert team, focusing completely on accuracy. Using these solutions regularly helps you score high marks in final exams.