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 ↓


S-block elements (alkali and alkaline earth metals)


Introduction to s-block elements

The s-block elements are located on the left side of the periodic table. They are made up of two groups: group 1, which includes the alkali metals, and group 2, which includes the alkaline earth metals. These elements are characterized by having their outermost electrons in the s-orbital.

General characteristics of s-block elements

The s-block elements have several distinctive properties:

  • They are metallic in nature.
  • They are highly reactive, especially the alkali metals.
  • They are good conductors of electricity and heat.
  • They have low ionization energy and low electronegativities.

Alkali metals (Group 1 elements)

The alkali metals include lithium (Li), sodium (Na), potassium (K), rubidium (Rb), caesium (Cs) and francium (Fr). They have one electron in their outermost shell, which gives them their distinctive properties.

Characteristics of alkali metals

  • They are soft and can be cut with a knife.
  • Their melting and boiling points are lower compared to other metals.
  • They have low densities; for example, lithium, sodium, and potassium are less dense than water.
  • They quickly turn black when exposed to air due to the formation of a layer of metal oxide.

Example reaction of alkali metals

When alkali metals react with water, they form alkaline solutions with the evolution of hydrogen gas. For example, sodium reacts with water as follows:

2Na + 2H2O → 2NaOH + H2↑

Trends in the alkali metals

As you move from lithium to francium in group 1:

  • The atomic and ionic radii increase.
  • The ionization energy decreases as the distance of the outer electron from the nucleus increases.
  • Reactivity increases as the ionization energy decreases, making it easier to lose the outer electron.

Alkaline earth metals (Group 2 elements)

The alkaline earth metals include beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). These elements have two electrons in their outermost shell.

Characteristics of alkaline earth metals

  • They are harder than the alkali metals.
  • Their melting and boiling points are higher than those of alkali metals.
  • They are denser than the alkali metals.
  • They form colorless compounds unless the anion itself is colored.

Example reactions of alkaline earth metals

Alkaline earth metals also react with water, but less vigorously than alkali metals. Magnesium reacts with water as follows:

Mg + 2H2O → Mg(OH)2 + H2↑

Trends in alkaline earth metals

As you move from beryllium to radium in group 2:

  • The atomic and ionic radii increase.
  • The ionization energy decreases.
  • Reactivity increases, although not as dramatically as with the alkali metals.

Visual example

Bohr model of sodium (Na)

No

In this diagram, the nucleus is in the center, surrounded by two electron shells. Sodium's valence electrons are in the outer shell.

Bohr model of magnesium (Mg)

Milligrams

For magnesium, we see two electrons in the outer shell, which is typical for an alkaline earth metal.

Applications of s-block elements

Both alkali and alkaline earth metals have various applications in industry and daily life:

  • Sodium (Na): It is used in street lighting, in sodium vapor lamps, and in the production of various compounds such as sodium hydroxide and sodium carbonate.
  • Potassium (K): Important in biological functions, used in fertilizers and to make some types of glass.
  • Magnesium (Mg): It is used in the making of light alloys, flash photography, and as a reducing agent in the production of titanium.
  • Calcium (Ca): Essential for living organisms, especially in cell physiology, and used to make cement and mortar.

Conclusion

The s-block elements, which include the alkali and alkaline earth metals, play a vital role in chemistry and have important applications in a variety of fields. Their properties are greatly affected by their electronic configuration, and understanding these can provide important information about their reactivity and uses.


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S-block elements (alkali and alkaline earth metals)

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