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) ↓


Group 2 Elements - Properties and Trends


The elements in group 2 of the periodic table are known as the alkaline earth metals. These include the elements beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). They are found in the second column of the periodic table and have some unique properties and trends that make them an interesting subject for study in chemistry.

General properties of group 2 elements

The elements in group 2 have a number of properties that are quite different from those in the other groups:

  • Valence electrons: All the elements in group 2 have two electrons in their outermost shell, due to which their valency is +2.
  • Oxidation state: They form compounds mainly in +2 oxidation state.
  • Metallic properties: They are all metals and show typical metallic properties, such as good electrical and thermal conductivity, malleability and ductility.
  • Density: Group 2 metals are denser than the alkali metals of Group 1.
  • Melting point and boiling point: Their melting point and boiling point are generally higher than those of alkali metals.

Chemical reactions of group 2 elements

Group 2 elements react with many other elements and compounds. Here are some common reactions:

Reaction with water

The alkaline earth metals react readily with water, although not as vigorously as the Group 1 elements. The typical reaction with water is as follows:

        M + 2H2O → M(OH)2 + H2

where M represents a Group 2 element. For example, the reaction of magnesium with water produces magnesium hydroxide and hydrogen gas:

        Mg + 2H2O → Mg(OH)2 + H2

Reaction with oxygen

Group 2 elements react with oxygen to form metal oxides. The general equation for this reaction is:

        2M + O2 → 2MO

For example, calcium oxide is formed as a result of the reaction between calcium and oxygen:

        2Ca + O2 → 2CaO

Trends in group 2 elements

Moving down the group from beryllium to radium, there are noticeable trends in the properties of the elements:

Atomic and ionic size

Atomic and ionic radii increase as you move down a group. This increase is due to the addition of electron shells as you move from one period to the next.

Visual example:

Happen Milligrams CA Atomic/ionic size Happen Milligrams CA

Ionization energy

Ionization energy decreases going down the group. This is due to the increasing distance of the outer electrons from the nucleus and the increase in the electron shielding effect, which makes it easier to remove an electron.

Visual example:

Happen Milligrams CA Ionization Energy

Jet

The reactivity of the alkaline earth metals increases going down the group. This is due to a decrease in ionization energy, making it easier for atoms to lose electrons and participate in reactions.

Uses of group 2 elements

Group 2 elements have a wide range of applications due to their unique properties:

  • Beryllium: Because of its strength and low mass, it is used in aerospace components and as a moderator in nuclear reactors.
  • Magnesium: It is commonly used in the manufacture of lighter materials, and as an ingredient in fireworks and flares.
  • Calcium: Important in biological systems and widely used in the construction industry in the form of limestone and cement.
  • Strontium: Used in the production of glass for color television cathode ray tubes and for red color in fireworks.
  • Barium: Used in oil and gas drilling fluids, and in medical imaging because of its contrast properties.

Biological importance of group 2 elements

Calcium and magnesium, in particular, play important roles in biological systems:

  • Calcium: Essential for bone and teeth health, muscle function and nerve signalling.
  • Magnesium: Important for enzyme function and energy production in cells.

Conclusion

The elements of group 2 are fascinating in the field of chemistry because of their physical and chemical properties, the trends observed as we move down the group, and their diverse applications in various industries and biological systems. Understanding these elements helps us understand both the complexity and utility of the periodic table in practical and theoretical chemistry.


Grade 11 → 10.2


U
username
0%
completed in Grade 11

← Prev (10.1)
Group 1 Elements - Properties and Trends
Next (10.3) →
Unusual properties of lithium and beryllium

Comments 



Group 2 Elements - Properties and Trends

https://www.chemistryelite.com/g11/10.2?ceal=en