Well! NCERT is not enough for chemical bonding chapter in the NEET. NCERT will definitely help you to understand the basic concepts related to the chapter. However, to score well in NEET demands more effort. As you know that National Eligibility cum Entrance Test, abbreviated as NEET is one of the toughest exam of India. Securing a seat in government medical college is highly competitive as lakhs of student participate in this exam to fulfil their dream of becoming a doctor. In that case, you need to be serious for this exam.
The topic on chemical bonds is studied in class 11. Students commonly believe that Class 11th Chemistry is difficult and that good grades are impossible to achieve in this subject, however this does not appear to be the case. In Class 11th, good grades in Chemistry can be readily acquired with right supervision and sufficient notes. In Class 11 Chemistry, there are many significant and simple chapters that can easily assist students achieve good exam results. Chapter 4 – Chemical Bonding and Molecular Structures is one such chapter. Chapter 4 Chemistry Class 11 Revision Notes will help students achieve good grades in Class 11th examinations since they cover all of the important themes, concepts, and words in a fun and simple style that students can grasp. Chemical Bonding and Molecular Structures notes become very significant throughout the examination for Class 11th Chemistry Chapter 4. These notes have been created by some of the best Chemistry teachers in the country. Chemical bonding Class 11 notes make it simple for students to understand all of the important concepts covered in the chapter.
Any of the interactions that account for the association of atoms into molecules, crystals, ions, and other stable species that make up the familiar compounds of everyday life are referred to as chemical bonding. When atoms come close together, their nuclei and electrons interact and tend to distribute themselves in space in such a way that the total energy is lower than in any other configuration. When the overall energy of a collection of atoms is less than the sum of the energies of the component atoms, they bond together, and the energy difference is known as the bonding energy.
After the electron was discovered and quantum mechanics gave a language for describing the behaviour of electrons in atoms, the ideas that contributed to determine the nature of chemical bonding came to fruition in the early twentieth century. Despite the fact that quantum physics is required to achieve a precise quantitative understanding of bond formation, chemists’ pragmatic grasp of bonding is stated in simple intuitive models. These models distinguish between two types of bonds: covalent and ionic. The sort of bond most likely to form between two atoms may be anticipated based on the elements’ positions in the periodic table, and the qualities of the substances generated can be related to the type of bonding to some extent.
Valence bonding: In the nineteenth century, chemists accumulated a huge body of empirical data that led to the understanding that there are patterns in the types of compounds that elements can create. The valence of an element, which was originally described in terms of the greatest number of hydrogen atoms that might connect to one atom of the element, is the most useful rationalising feature. Because research observed that one atom of hydrogen is never found in association with more than one other atom, it was chosen as the valence probe because it is the most primordial of the elements. It was discovered that oxygen (O) has a valence of 2 (as in water, H2O), nitrogen (N) has a valence of 3 (as in ammonia, NH3), and chlorine (Cl) has a valence of 1 (as in water, H2O) (as in hydrogen chloride, HCl). Despite the fact that their compounds with hydrogen were unknown, exploring the patterns of atom bonding allowed for the assignment of conventional valences to all elements.
Do you know the answer of the below question:
- A) CH4
- B) H2
- C) KCN
- D) KCl
Ionic and covalent compounds: In the early days of chemistry, a second general property of bonding became apparent. It was discovered that when dissolved in water, there are two main classes of compounds that can be identified. Electrolytes are a type of substance that dissolves to form solutions that conduct electricity. Nonelectrolytes, on the other hand, dissolve to produce solutions that do not conduct electricity. Because of the distinction between the two classes, the idea that there are two sorts of chemical bonds arose. In solution, electrolytes produce ions; an ion is an electrically charged atom that carries its charge through a solution. As a result, electrolytes either contain ions before dissolving or produce ions after dissolving. When nonelectrolytes dissolve, they do not produce ions, and they do not contain ions in their undissolved condition.