General Chemistry Note - Full Course Pdf Notes For Competitive Exams

 **General Chemistry Note - Full Course Notes For Competitive Exams**

General chemistry is an essential foundation for many other scientific disciplines, such as biology, physics, engineering, and medicine. It is also an important subject for students who are pursuing careers in fields such as environmental science, pharmacy, and materials science.

Chemistry Notes PDF for RRB & SSC Exams - General Science

Chapter 1: 

** Foundations of Chemistry**

• * **Matter:** Any substance that has mass and takes up space.
• * **Properties of matter:** Physical properties (e.g., color, density) and chemical properties (e.g., reactivity).
• * **Changes in matter:** Physical changes (e.g., melting, boiling) and chemical changes (e.g., rusting, burning).
• * **Scientific method:** A process for solving problems and testing hypotheses.

Chapter 2: 

**Atoms, Molecules, and Ions**

• * **Atom:** The basic unit of matter that cannot be broken down into smaller parts.
• * **Subatomic particles:** Protons, neutrons, and electrons.
• * **Atomic number:** The number of protons in an atom.
• * **Mass number:** The sum of the protons and neutrons in an atom.
• * **Isotopes:** Atoms of the same element with different numbers of neutrons.
• * **Ions:** Atoms that have gained or lost electrons.
• * **Chemical bonds:** Forces that hold atoms together to form molecules.

Chapter 3: 

**Chemical Quantities and Stoichiometry**

• * **Mole:** A unit of measurement for the amount of a substance.
• * **Avogadro's number:** The number of particles in one mole of a substance.
• * **Molar mass:** The mass of one mole of a substance.
• * **Stoichiometry:** The relationship between the amounts of reactants and products in a chemical reaction.
• * **Chemical equations:** Balanced equations that represent chemical reactions.

Chapter 4: 

**Types of Chemical Reactions and Solution Stoichiometry**

• * **Types of chemical reactions:** Synthesis, decomposition, single-replacement, double-replacement, and combustion reactions.
• * **Aqueous solutions:** Solutions in which the solvent is water.
• * **Solution stoichiometry:** The use of stoichiometry to calculate the concentrations of solutions.

Chapter 5: 

**Gases**

• * **Ideal gas law:** PV = nRT
• * **Kinetic molecular theory:** A theory that describes the behavior of gases.
• * **Gas laws:** Boyle's law, Charles's law, Gay-Lussac's law, and the combined gas law.
• * **Real gases:** Gases that do not behave ideally.

Chapter 6: 

**Thermochemistry**

• * **Thermochemistry:** The study of energy changes in chemical reactions.
• * **Enthalpy:** A measure of the heat content of a substance.
• * **Hess's law:** The enthalpy of a reaction is the sum of the enthalpies of the steps that make up the reaction.
• * **Entropy:** A measure of the disorder of a system.
• * **Spontaneity:** A process that occurs naturally without outside intervention.

Chapter 7: 

**Quantum Mechanical View of the Atom, and Periodicity**

• * **Quantum mechanics:** A branch of physics that deals with the behavior of matter at the atomic and subatomic level.
• * **Atomic orbitals:** Regions of space around an atom where electrons are likely to be found.
• * **Electron configuration:** The arrangement of electrons in the atomic orbitals of an atom.
• * **Periodic table:** A table of the elements organized by their atomic number and electron configuration.
• * **Periodic trends:** Trends in the properties of the elements as their atomic number increases.

Chapter 8: 

**Chemical Bonding**

• * **Chemical bonding:** Forces that hold atoms together to form molecules.
• * **Types of chemical bonds:** Covalent bonds, ionic bonds, and metallic bonds.
• * **Covalent bonds:** Bonds formed when atoms share electrons.
• * **Ionic bonds:** Bonds formed when one atom transfers an electron to another atom.
• * **Metallic bonds:** Bonds formed by the attraction between metal atoms and their free-moving valence electrons.

Chapter 9: 

**Covalent Bonding and Molecular Orbitals**

• * **Molecular orbital theory:** A theory that describes the bonding of atoms in molecules.
• * **Hybrid orbitals:** Orbitals that are formed when two or more atomic orbitals combine.
• * **VSEPR theory:** A theory that predicts the shape of molecules based on the number of valence electron pairs around the central atom.

Chapter 10: 

**Liquids, Solids, and Intermolecular Forces**

• * **Liquids:** Substances that flow and take the shape of their container.
• * **Solids:** Substances that have a definite shape and volume.
• * **Intermolecular forces:** Forces that hold molecules together.
• * **Types of intermolecular forces:** Dipole-dipole interactions, hydrogen bonding, and London dispersion forces.

Chapter 11: 

**Solutions and Their Properties**

• * **Solutions:** Mixtures in which one substance is dissolved in another substance.
• * **Solubility:** The ability of one substance to dissolve in another substance.
• * **Types of solutions:** Unsaturated, saturated.

Chapter 12: 

**Chemical Kinetics**

• * **Chemical kinetics:** The study of the rates of chemical reactions.
• * **Factors that affect the rate of a chemical reaction:** Concentration of reactants, surface area, temperature, and the presence of a catalyst.
• * **Collision theory:** A theory that describes how chemical reactions occur.
• * **Rate law:** An equation that expresses the relationship between the rate of a chemical reaction and the concentrations of the reactants.

Chapter 13: 

**Chemical Equilibrium**

• * **Chemical equilibrium:** A state in which the rates of the forward and reverse reactions in a chemical reaction are equal.
• * **Le Chatelier's principle:** If a change is made to a system at equilibrium, the system will shift to a new equilibrium position in order to counteract the change.
• * **Buffer solutions:** Solutions that resist changes in pH.
• * **Solubility equilibria:** Equilibria involving the dissolution of solids in liquids.

Chapter 14: 

**Acids and Bases**

• * **Acids:** Substances that produce hydrogen ions (H+) in water.
• * **Bases:** Substances that produce hydroxide ions (OH-) in water.
• * **pH:** A measure of the acidity or basicity of a solution.
• * **Titration:** A laboratory technique used to determine the concentration of an acid or base.
• * **Strong acids and bases:** Acids and bases that completely dissociate in water.
• * **Weak acids and bases:** Acids and bases that partially dissociate in water.

Chapter 15: 

**Applications of Acid-Base Equilibria**

• * **Acid-base indicators:** Substances that change color depending on the pH of their surroundings.
• * **Buffers:** Solutions that resist changes in pH.
• * **Salt solutions:** Solutions that contain ions.
• * **Hydrolysis:** The reaction of water with an ion to produce an acid or base.
• * **Acid rain:** Rain that is more acidic than normal due to the presence of dissolved pollutants.

Chapter 16: 

**Spontaneity, Entropy, and Free Energy**

• * **Spontaneity:** A process that occurs naturally without outside intervention.
• * **Entropy:** A measure of the disorder of a system.
• * **Free energy:** A measure of the spontaneity of a process.
• * **Gibbs free energy equation:** ΔG = ΔH - TΔS
• * **Spontaneity under standard conditions:** If ΔG is negative, the reaction is spontaneous under standard conditions.
• * **Spontaneity under non-standard conditions:** If ΔG is negative, the reaction is spontaneous under the given conditions.

Chapter 17: 

**Electrochemistry**

• * **Electrochemistry:** The study of the relationship between electricity and chemical reactions.
• * **Oxidation-reduction reactions:** Reactions in which one species loses electrons and another species gains electrons.
• * **Redox potentials:** Potentials that measure the tendency of a species to undergo oxidation or reduction.
• * **Electrochemical cells:** Devices that convert chemical energy into electrical energy or vice versa.
• * **Galvanic cells:** Electrochemical cells that produce electricity.
• * **Electrolytic cells:** Electrochemical cells that use electricity to produce chemical changes.

Chapter 18: 

**Transition Metals and Coordination Chemistry**

• * **Transition metals:** Metals that have incompletely filled d-orbitals.
• * **Coordination complexes:** Compounds in which a metal ion is bound to a number of Lewis bases.
• * **Ligands:** Lewis bases that bind to metal ions to form coordination complexes.
• * **Isomerism:** The existence of compounds with the same molecular formula but different structures.
• * **Types of isomerism:** Structural isomerism, stereoisomerism, and linkage isomerism.

Chapter 19: 

**The Nucleus and Nuclear Chemistry**

• * **Nucleus:** The central part of an atom that contains the protons and neutrons.
• * **Nuclear forces:** The forces that hold the nucleus together.
• * **Nuclear reactions:** Reactions that involve changes to the nucleus of an atom.
• * **Types of nuclear reactions:** Alpha decay, beta decay, and gamma decay.
• * **Nuclear fission:** The splitting of a heavy nucleus into two smaller nuclei.
• * **Nuclear fusion:** The combination of two light nuclei to form a heavier nucleus.

Chapter 20: 

**An Introduction to Organic Chemistry**

• * **Organic chemistry:** The study of compounds that contain carbon.
• * **Functional groups:** Groups of atoms that give organic compounds their characteristic properties.
• * **Types of organic compounds:** Hydrocarbons, alcohols, aldehydes, ketones, carboxylic acids, amines, esters, and amides.
• * **Organic reactions:** Reactions that involve organic compounds.
• * **Types of organic reactions:** Substitution reactions, addition reactions, elimination reactions, and rearrangement reactions.

Key Features ~

 Additionally, referring to standard science textbooks and study materials can be helpful.

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Chemistry Notes for Competitive Exams !! रसायन विज्ञान के नोट्स हिंदी माध्यम में

How to prepare chemistry for competitive exams?

To prepare for this section, solve many mock tests and clear basics. Read important topics and books that cover the whole Chemistry syllabus. These articles will explain to you the concepts of chemistry in an easy and comprehensive language. It will act as a quick reference for doubts and will also help in revision.

What are the most important topics in general science?

Physics, Chemistry, Biology and Ecology are among the important General Science topics.

How many types of general science are there?

General Science includes an array of basic topics from the three branches of Science namely, Physics, Biology, and Chemistry [BiPC subjects]. Generally, the topics covering the practical aspects of the common principles of the 3 subjects are put under this section.

Conclusion:~

It's important to note that the specific topics and emphasis on each topic may vary depending on the competitive exam you are preparing for. I recommend referring to the syllabus or study materials provided by the exam organization for a more detailed and tailored approach to your preparation. Additionally, practicing with sample questions and previous exam papers can also be helpful in familiarizing yourself with the exam format and question types.

I hope this full course notes is helpful for your general chemistry studies. Good