Grade 11
  1. Basic concepts of chemistry  1.1. Importance of Chemistry  1.2. Nature and scope of chemistry  1.3. laws of chemical combination  1.3.1. Law of conservation of mass  1.3.2. Law of definite proportions  1.3.3. Law of multiple proportions  1.3.4. Law of gaseous volume  1.3.5. Avogadro's Law  1.4. Dalton's atomic theory  1.5. Mole concept and molar mass  1.6. Percent composition  1.7. Empirical and molecular formula  1.8. Stoichiometry and Stoichiometric Calculations  1.9. Limiting reagent concept
  2. Structure of the atom  2.1. Discovery of the electron, proton, and neutron  2.2. Atomic Model  2.2.1. Thomson's model  2.2.2. Rutherford's model  2.2.3. Bohr's model  2.3. Quantum mechanical model of the atom  2.4. Dual nature of matter and radiation  2.5. Heisenberg's uncertainty principle  2.6. Quantum numbers  2.7. Atomic orbitals and their shapes  2.8. Electronic configuration of elements  2.9. Aufbau principle  2.10. Pauli's exclusion principle  2.11. Hund's maximum multiplicity rule  2.12. de Broglie's hypothesis  2.13. Photoelectric effect
  3. Classification of elements and periodicity in properties  3.1. Historical development of the periodic table  3.2. Modern Periodic Law and Periodic Table  3.3. Periodic trends in properties  3.3.1. Atomic and Ionic Radius  3.3.2. Ionization enthalpy  3.3.3. Electron gain enthalpy  3.3.4. Electronegativity  3.3.5. Valency  3.3.6. Metallic and Non-Metallic Properties  3.3.7. Oxidation states  3.4. Unusual Properties of the First Elements
  4. Chemical Bonding and Molecular Structure  4.1. Kossel–Lewis approach to chemical bonding  4.2. Ionic or electrovalent bond  4.3. Covalent bond and its features  4.4. Bond parameters  4.5. VSEPR Theory  4.6. Valence bond theory  4.7. Hybridization and its types  4.8. Molecular orbital theory  4.8.1. Bond order and stability  4.9. Hydrogen bonding
  5. States of matter  5.1. Intermolecular forces  5.2. Gas Laws  5.2.1. Boyle's law  5.2.2. Charles's Law  5.2.3. Avogadro's Law  5.2.4. Dalton's law of partial pressure  5.2.5. Graham's law of spread  5.3. Ideal Gas Equation and Applications  5.4. Real gases and deviations from ideal behaviour  5.5. Kinetic molecular theory of gases  5.6. Liquefaction of gases  5.7. Properties of Liquids  5.8. Surface tension and viscosity
  6. Thermodynamics  6.1. System and environment  6.2. Types of systems in thermodynamics  6.3. Types of procedures  6.4. First law of thermodynamics  6.5. Internal energy and enthalpy  6.6. Heat capacity and specific heat  6.7. Hess's law of constant heat summation  6.8. Bond dissociation enthalpy  6.9. Enthalpy of formation and combustion  6.10. Enthalpy of solution and neutralization  6.11. Spontaneity and the second law of thermodynamics  6.12. Gibbs free energy and its applications
  7. Balance  7.1. The concept of balance  7.2. Equilibrium constant and its applications  7.3. Le Chatelier's principle  7.4. Ionic equilibrium in solutions  7.5. Acid and Base Theory  7.5.1. Arrhenius concept  7.5.2. Bronsted-Lowry concept  7.5.3. Lewis concept  7.6. pH Scale and pOH  7.7. Common ion effect  7.8. Hydrolysis of salts  7.9. Buffer solutions and their mechanism of action  7.10. Solubility equilibrium of sparingly soluble salts
  8. Redox reactions  8.1. Oxidation and reduction concepts  8.2. Oxidation number and its applications  8.3. Redox reactions in terms of electron transfer  8.4. Balancing redox reactions (oxidation number and ion-electron methods)  8.5. Types of redox reactions  8.6. Electrochemical Cells and Redox Reactions
  9. Hydrogen  9.1. Position of Hydrogen in the Periodic Table  9.2. Isotopes of hydrogen  9.3. Preparation of Hydrogen  9.4. Properties of Hydrogen  9.5. Hydrides and their classification  9.6. Water and heavy water  9.7. Hydrogen peroxide and its properties  9.8. Uses of Hydrogen and Its Compounds
  10. S-block elements (alkali and alkaline earth metals)  10.1. Group 1 Elements - Properties and Trends  10.2. Group 2 Elements - Properties and Trends  10.3. Unusual properties of lithium and beryllium  10.4. Important compounds of sodium and their uses  10.5. Important Compounds of Magnesium and Calcium
  11. Some p-block elements  11.1. General Introduction to p-Block Elements  11.2. Group 13 Elements  11.2.1. Boron and its compounds  11.3. Group 14 Elements  11.3.1. Carbon and its allotropes  11.3.2. Important Compounds of Carbon and Silicon
  12. Organic Chemistry - Some Basic Principles and Techniques  12.1. Classification and Nomenclature of Organic Compounds  12.2. Structural representation of organic compounds  12.3. Classification of organic reactions  12.4. Electronic Effects in Organic Chemistry  12.4.1. Inductive effect  12.4.2. Resonance effect  12.4.3. Hyperconjugation  12.5. Reaction mechanism and intermediate species  12.6. Purification and qualitative analysis of organic compounds
  13. Hydrocarbons  13.1. Hydrocarbons  13.1.1. Preparation and Properties of Alkenes  13.2. alkene  13.2.1. Preparation and Properties of Alkenes  13.2.2. Electrophilic addition reactions  13.3. Alkynes  13.3.1. Preparation and Properties of Alkynes  13.4. Aromatic hydrocarbons  13.4.1. Structure and properties of benzene  13.4.2. Electrophilic substitution reactions of benzene
  14. Environmental Chemistry  14.1. Environmental Pollution  14.2. Atmospheric pollution and the greenhouse effect  14.3. Water pollution and treatment methods  14.4. Soil pollution and its effects  14.5. Industrial waste and its treatment  14.6. Strategies for pollution control

Grade 11 ↓


Basic concepts of chemistry


Chemistry is the scientific study of matter, its properties, and its transformations. In this lesson, we will explore the basic concepts of chemistry, which lay the foundation for further study in this field. Understanding these concepts is essential because they form the basis of how we interact with and understand the physical world.

What is the matter?

Matter is everything that has mass and occupies space. It is made up of atoms and molecules. Almost everything you can see and touch is made of matter. The only exceptions to this are forms of energy, such as light and sound. Matter can exist in different states: solid, liquid, gas, and plasma.

States of matter

Solid (ice): At least a definite shape and volume.
Liquid (water): It has no definite shape but has definite volume.
Gas (Steam): Neither definite shape nor volume.
Plasma: Ionized gas that emits light.

Elements and compounds

An element is a substance that cannot be broken down into simpler substances by chemical means. There are over 100 known elements, each with unique properties. Elements are represented by chemical symbols, such as H for hydrogen, O for oxygen, and Na for sodium.

A compound is a substance that is formed by two or more elements joining together chemically. The smallest unit of a compound is a molecule. An example of a compound is water (H 2 O), which has two hydrogen atoms and one oxygen atom.

Molecular visualization

HeyHH

This diagram shows a water molecule. The red circle symbolizes the oxygen atom, while the two blue circles represent hydrogen atoms. The lines represent the bonds between the atoms.

Atoms and molecules

An atom is the smallest unit of an element, consisting of a nucleus surrounded by electrons. The nucleus contains protons and neutrons. The number of protons determines the atomic number of an element and defines the type of element.

A molecule is a group of two or more atoms bonded together, which may be of the same type, such as O 2, or of different types, such as H 2 O.

Visualization of atoms

Nucleus

In this atomic view, the green circle represents the nucleus containing the protons and neutrons. The orange circles represent the electrons orbiting the nucleus.

Periodic table

The periodic table arranges elements based on their atomic number. Elements are arranged in periods (rows) and groups (columns). Elements in the same group share similar chemical properties. This layout helps in understanding the relationships and properties of different elements.

Period 1 – H, He
Period 2 - Li, Be, B, Si, N, O, F, Ne
Group 1 - H, Li, Na, K, Rb, Cs, Fr (alkali metals)
Group 17 - F, Cl, Br, I, At (halogens)

Chemical reactions

A chemical reaction is a process in which substances (reactants) are transformed into different substances (products). It involves the breaking and formation of chemical bonds. Chemical equations represent these reactions, for example:

H 2 + O 2 → H 2 O

In this reaction, hydrogen gas and oxygen gas combine to form water.

Law of conservation of mass

This fundamental principle states that mass is neither created nor destroyed in a chemical reaction. The mass of the reactants is always equal to the mass of the products. For example, when a piece of paper is burned, the mass of the ashes and gases left behind is equal to the original mass of the paper and the oxygen used in the burning.

Moles and Avogadro's number

The mole is a unit used to measure the amount of a substance. It is defined as exactly 6.02214076 × 1023 particles (Avogadro's number). This number provides a bridge between the atomic scale and the real-world scale.

For example:

  • 1 mole of carbon atoms = 6.022 × 1023 carbon atoms
  • 1 mole of water molecules = 6.022 × 10 23 H 2 O molecules

Applications: Calculating moles

Using the concept of the mole, chemists can calculate how much of a substance is involved in a reaction. To perform these calculations, consider the molar mass (the mass of one mole):

Molar mass of H 2 O = (2 x 1.01 g/mol) + (16.00 g/mol) = 18.02 g/mol
If you have 36.04 grams of water:
Number of moles = 36.04 g / 18.02 g/mol = 2 moles

Closing thoughts

After understanding these basic concepts, you have a foundation to delve deeper into chemistry. The importance of these concepts cannot be underestimated as they are essential for understanding more complex chemical interactions and the behavior of substances in different situations.

Remember, chemistry gives us the tools to understand the world at the molecular level. From the smallest particles to the largest compounds, the principles explained here are vital in applying chemistry both academically and practically.


Grade 11 → 1


U
username
0%
completed in Grade 11

Next (1.1) →
Importance of Chemistry

Comments 



Basic concepts of chemistry

https://www.chemistryelite.com/g11/1?ceal=en