Class 11 Chemistry Chapter 4 Notes Pdf Download

[Badomero Schoulund]

Scienceis a subject that explains how the world around us is made and the chemical reactions that make things happen around us. From rust to decomposition, chemical reactions provide a more in-depth insight into how molecular interaction and changes occur. Chapter 1 of CBSE class 10 Science explains how a substance changes form.

Learn more about chemical reactions and equations by exploring CBSE Notes for Class 10 Science Chapter 1. These CBSE notes are comprehensive and detailed yet concise enough to glance through for exam preparations.

A chemical reaction occurs when one or more reactants are changed into one or more products. The constituent atoms of the reactants are rearranged in a chemical reaction, resulting in the formation of various substances as products.

A chemical reaction can be determined with the help of any of the following observations.

a) Evolution of a gas

b) Change in temperature

c) Formation of a precipitate

d) Change in colour

e) Change of state

A chemical reaction is a process that causes one set of chemical components to change into another. Chemical reactions are defined as changes in the locations of electrons in the formation and breaking of chemical bonds between atoms, with no change in the nuclei, and are described using a chemical equation. At a given temperature and chemical concentration, chemical reactions occur at a predictable rate. Reaction speeds often increase as the temperature rises because more thermal energy is available to attain the activation energy required to break bonds between atoms.

A symbol is a chemical code for an element. Each element has a one or two-letter atomic symbol, which is, in most cases, the abbreviated form of its name.

Valency is the combining capacity of an element. It can be considered as the number of electrons lost, gained or shared by an atom when it combines with another atom to form a molecule.

According to the Law of Conservation of Mass, no atoms can be created or destroyed in a chemical reaction, so the number of atoms for each element on the reactants side has to balance the number of atoms that are present on the products side.

In other words, the total mass of the products formed in a chemical reaction is equal to the total mass of the reactants participating in a chemical reaction.

Chemical equations are balanced using coefficients. A coefficient is a numerical value that is added to the front of a chemical symbol or formula. It indicates the number of atoms or molecules of the material involved in the process.

Hit and trial method: While balancing the equation, change the coefficients (the numbers in front of the compound or molecule) so that the number of atoms of each element is the same on each side of the chemical equation.

A single reactant decomposes on the application of heat or light, or electricity to give two or more products.

Types of decomposition reactions:

a. Decomposition reactions which require heat-thermolytic decomposition or thermolysis.

One of the best examples of precipitation reactions is the chemical reaction between potassium chloride and silver nitrate, in which solid silver chloride is precipitated out. This is the insoluble salt formed as a product of the precipitation reaction. The chemical equation for this precipitation reaction is provided below.

A redox reaction occurs when the oxidation states of the substrate change. The loss of electrons or an increase in the oxidation state of a chemical or its atoms is referred to as oxidation. The gain of electrons or a decrease in the oxidation state of a chemical or its atoms is referred to as reduction.

It refers to the oxidation of fats and oils in food that is kept for a long time. It gives foul smell and bad taste to food. Rancid food causes stomach infections during consumption.

Prevention:

(i) Use of air-tight containers

(ii) Packaging with nitrogen

(iii) Refrigeration

(iv) Addition of antioxidants or preservatives

In the electrolysis of water (acidified), the gases that are evolved at the anode and cathode, respectively, are oxygen and hydrogen. Hydrogen ions gain electrons from the cathode and form hydrogen gas, and oxygen ions give electrons to the anode and form oxygen gas.

Although the notes below have been proofread, there may well be mistakes in them. I would appreciate it if you would let me know when you find mistakes. Please let me know either by telephone (x6486) or email (cast...@marshall.edu). There is a date at the end of each chapter's notes. When substantive corrections are made, that date will be changed so you know how current is the posted version. Finally, the notes are a work in progress. For that reason, when you click on a link you may get an error message. In all likelihood, it means that those notes haven't been posted yet.

How to Study video series:Prof. Stephen Chew of Samford University was the 2011 U.S. Professor ofthe Year for baccalureate institutions. His area of research is studentlearning and he has produced a series of five videos on how to studymost effectively. Each video is 5-7 minutes long. The first is morebackground material, while the other four are more applied. They have alot of good advice.

The Khan Academy has over 100 videos discussing topics from both this course and CHM 212. The videos range from a few minutes to around 20 minutes. Each is on an individual topic, so if you have trouble with one item and want to see a short discussion on it, this website might be very helpful. It has videos on a wide range of subjects so this could help you with a variety of topics.

OUTSIDE LECTURE AVAILABILITY: If you would like additional discussion of the material we cover in class, there are two sources of high quality lecture materials that I know of that you might find helpful.

The Orbitron by Mark Winter at the Univesity of Sheffield (also the creater of WebElements) shows images of the different orbitals at various energy levels (e.g. 1s, 2s, 3s, ...) as well as molecular orbitals. Animations of orbital formation are also included. If you're having trouble imagining what the orbitals look like or how MOs come into existence this is a great site.

A company called 3DChem.comhas a website that shows the 3-dimensional structure of a large numberof molecules that can be manipulated by you much including the VSEPRfigures available in the table shown on this page. The structuresof the top 50 prescription medicines are available, as are 1600structures of inorganic compounds (e.g. the structure of the gemstonesRuby and Garnet), and assorted other molecules (e.g. the molecules thatgive rise to the scents of garlic and cloves).

It can be difficult to keep your notes organized throughout the school year, especially in a class that covers so much content. This article will give you links to notes on every topic included in the AP Chemistry curriculum. If you're missing some of your notes, or if you just want a more structured overview of what you need to know for the exam, you've come to the right place! We'll also give you some study tips so that you can use both these notes and the notes you took throughout the year to your best advantage.

The notes in this article can be used to study smaller portions of the curriculum or to review for the final AP Chemistry exam. There are currently nine units that organize all the concepts in the course, so we've categorized these notes according to that framework. Topics should be listed in roughly the same order as you learned them in class.

These notes will provide a ton of background information, but keep in mind that AP Chemistry is less about memorization of facts and more about the ability to apply your knowledge to a variety of experimental scenarios. Reading notes can only get you so far. Practice problems are essential (a point that I will emphasize again later in this article).

Take a diagnostic test before you dive into these notes if you plan on using them to review for the full AP test. Based on your results, you can see which areas need the most improvement, and then you can focus on the notes that are most relevant.

These notes come from several sources. Some are in-depth, others give a broad overview. Some are in-depth, others give a broad overview. Some focus more on explaining concepts, others on working through practice questions. The overall goal of these notes is to give you a comprehensive guide of what you need to know for AP Chemistry.

If you want to use these notes to your full advantage, you shouldn't just read them all and consider yourself prepared. For chemistry, you need to dig deeper to understand the material fully. That said, here are some tips to keep in mind:

If you're studying for chemistry, you should work your way through concepts in the order of when they show up in the curriculum. You need to master the basics first, or more advanced problems will look like complete gibberish to you. If there are any topics in Unit 1 that you don't feel comfortable with, start your studying with those. Everything else in the course builds on the concepts you learned in the first couple of months!

Every time you read a set of notes, do a few practice problems to make sure you've absorbed the information. Reading through these notes is a waste of time if they don't provide you with the background information and skills you need to solve relevant problems. If you find that you're having trouble with practice problems after you read through notes, this should be a red flag that you need to modify your study strategy.

Don't forget about the notes you took in class, handouts your teacher gave to you, and any other resources you've accumulated throughout the year. It's worthwhile to shop around and see whether certain explanations of concepts resonate more than others. You might decide that videos explaining concepts are more useful to you than notes, or you may choose to buy a review book that provides more guidance in planning out your studying.

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