Grade 10
  1. Matter and its properties  1.1. States of matter  1.2. Physical and chemical properties of matter  1.3. Classification of substances (elements, compounds, mixtures)  1.4. Changes in Matter (Physical and Chemical Changes)  1.5. Law of conservation of mass and law of definite proportions
  2. Atomic Structure  2.1. Historical development of the atomic model  2.2. Subatomic particles (protons, neutrons, electrons)  2.3. Atomic number, mass number and isotopes  2.4. Electronic Configuration and Energy Levels  2.5. Valency, ion formation and oxidation state
  3. Periodic table  3.1. History and Development of the Periodic Table  3.2. Modern Periodic Law and Periodic Trends  3.3. Groups and Periods in the Periodic Table  3.4. Trends in the Periodic Table  3.5. Metals, non-metals, metalloids and their properties  3.6. Noble gases and their chemical inertness
  4. Chemical bond  4.1. Formation of Chemical Bonds (Octet Rule)  4.2. Ionic Bonding and Properties of Ionic Compounds  4.3. Covalent Bond and Properties of Covalent Compounds  4.4. Metallic bond and its properties  4.5. Molecular geometry and VSEPR theory  4.6. Polarity and dipole moment of molecules  4.7. Intermolecular forces
  5. Chemical Reactions and Equations  5.1. Types of Chemical Reactions  5.2. Writing and balancing chemical equations  5.3. Law of conservation of mass in chemical reactions  5.4. Factors Affecting Chemical Reactions  5.5. Catalysts and their role in chemical reactions  5.6. Exothermic and Endothermic Reactions
  6. Stoichiometry and Chemical Calculations  6.1. Mole concept and Avogadro number  6.2. Molar Mass and Gram-Mole Conversions  6.3. Empirical and molecular formula  6.4. Stoichiometric calculations and chemical yield  6.5. Limiting and Excess Reactants
  7. Acids, Bases and Salts  7.1. Properties and Definitions of Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)  7.2. pH Scale, pOH, and Indicators  7.3. Neutralization reactions and salt formation  7.4. Strength of Acids and Bases (Strong vs. Weak Acids and Bases)  7.5. Common Acids and Bases in Daily Life  7.6. Salts, their solubility and applications
  8. Metals and Nonmetals  8.1. Physical and chemical properties of metals  8.2. Physical and Chemical Properties of Non-Metals  8.3. Reactivity Series of Metals and Displacement Reactions  8.4. Extraction of metals from ores  8.5. Corrosion, its causes and prevention  8.6. Alloys, their composition and uses
  9. Carbon and its compounds  9.1. Allotropes of Carbon  9.2. Hydrocarbons and their classification (alkanes, alkenes, alkynes)  9.3. Functional groups in organic compounds  9.4. Nomenclature of organic compounds (IUPAC system)  9.5. Isomerism in organic chemistry (structural and geometrical)  9.6. Important organic reactions (combustion, addition, substitution, polymerization)  9.7. Applications of organic compounds in industry and daily life
  10. Environmental Chemistry  10.1. Air Pollution (Sources, Effects and Control)  10.2. Water Pollution (Causes, Effects and Remedies)  10.3. Greenhouse effect and global warming  10.4. Ozone layer depletion and its effects  10.5. Green Chemistry and Its Applications  10.6. sustainable chemistry practice
  11. Thermochemistry  11.1. Heat and Energy Changes in Chemical Reactions  11.2. Exothermic and Endothermic Reactions  11.3. Enthalpy, enthalpy change, and heat of reaction  11.4. Specific heat capacity and calorimetry  11.5. Energy Changes in Combustion Reactions
  12. Electrochemistry  12.1. Electrolytes and non-electrolytes  12.2. Electrolysis and its applications (electroplating, extraction of metals)  12.3. Redox reactions (oxidation and reduction)  12.4. Galvanic cell and electrochemical series  12.5. Corrosion and electrochemical prevention methods
  13. Chemical kinetics and equilibrium  13.1. Rate of chemical reactions and its measurement  13.2. Factors affecting the reaction rate (catalyst, temperature, concentration)  13.3. Reversible and irreversible reactions  13.4. Dynamic equilibrium and equilibrium constant  13.5. Le Chatelier's principle and its applications
  14. Gases and Gas Laws  14.1. Properties of gases and kinetic molecular theory  14.2. Boyle's Law (Pressure-Volume Relation)  14.3. Charles's Law  14.4. Gay-Lussac's Law  14.5. Combined Gas Law and Ideal Gas Law  14.6. Real Gases vs Ideal Gases
  15. Nuclear Chemistry  15.1. Introduction to Radioactivity and Nuclear Reactions  15.2. Types of radioactive decay (alpha, beta, gamma)  15.3. Half-life and applications of radioactive isotopes  15.4. Nuclear fission and fusion reactions  15.5. Nuclear power generation and its environmental impact

Grade 10 ↓


Metals and Nonmetals


In chemistry, elements are classified into two primary categories: metals and nonmetals. This classification is based on the physical and chemical properties that these elements exhibit. It is important to understand the difference between metals and nonmetals to understand the various chemical reactions and physical properties.

Properties of metals

Metals are often considered solid materials that exhibit interesting and useful physical and chemical properties. These properties are essential in many applications such as construction, technology, and manufacturing.

Physical properties of metals

  • State: Most metals are solid at room temperature, only mercury is a liquid.
  • Luster: Metals have a shiny or metallic luster. Because of this property they can reflect light.
  • Malleability: Metals can be hammered into thin sheets. This property makes them excellent for applications such as making sheets for automobiles and airplanes.
  • Ductility: Metals can be stretched into thin wires. Copper is an example of this, and is often used for electrical wires.
  • Conductivity: Metals are good conductors of heat and electricity, which is why they are used in electrical wires and cooking utensils.
  • Density: Metals have high density, that is, they are heavy in proportion to their size.
  • Melting point and boiling point: The melting point and boiling point of metals are generally high.

Visual example: metal lattice structure

The arrangement of metal atoms is often represented in a lattice structure as shown below:

Chemical properties of metals

  • Electropositivity: Metals lose electrons to form positive ions or cations.
  • Reactivity: Metals like sodium and potassium are highly reactive with water, while other metals like gold are less reactive.
  • Oxides: Metals react with oxygen to form metallic oxides, which are basic in nature. For example, when magnesium burns in the presence of oxygen, magnesium oxide is formed.

Characteristics of non-metals

Nonmetals differ significantly from metals, especially in their physical and chemical properties. Nonmetals are not as widely used as metals in industrial applications, but they still play an important role in a variety of chemical processes.

Physical properties of nonmetals

  • State: Non-metals can be solid, liquid, or gas at room temperature. For example, carbon is a solid, bromine is a liquid, and oxygen is a gas.
  • Luster: Except iodine, other non-metals are generally lustrous.
  • Malleability and ductility: Nonmetals are brittle in the solid state and cannot be hammered or drawn into wires.
  • Conductivity: Nonmetals are poor conductors of heat and electricity which makes them good insulators.
  • Density: Non-metals generally have lower densities than metals.
  • Melting point and boiling point: Nonmetals generally have lower melting and boiling points than metals.

Visual example: structure of a nonmetal

Nonmetals have more varied structures, as shown in the simplified diagram of a molecular nonmetal:

Chemical properties of nonmetals

  • Electronegativity: Nonmetals gain or share electrons to form anions or covalent bonds.
  • Reactivity: Nonmetals such as fluorine are very reactive, especially with metals. Nonmetals can react with each other to form covalent compounds.
  • Oxides: Nonmetals react with oxygen to form nonmetal oxides, which are acidic in nature. For example, carbon reacts with oxygen to form carbon dioxide.

Comparison of metals and nonmetals

By understanding the difference between metals and nonmetals, it is easier to predict their reactions and uses. Metals and nonmetals are given different positions in the periodic table, which shows their reactive behavior and inter-reactions.

Examples of metals and nonmetals

Here are examples of some common metals:

  • Iron (Fe): Used in construction and manufacturing because of its strength.
  • Copper (Cu): It is widely used in electrical wiring due to its excellent electrical conductivity.
  • Aluminium (Al): It is known for its light weight and is used in the manufacturing of airplanes and packaging.

Here are examples of some common nonmetals:

  • Oxygen (O2): Necessary for respiration and combustion reactions in living organisms.
  • Carbon (C): Found in all organic compounds and is essential for life.
  • Nitrogen (N2): This is a large part of the Earth's atmosphere and is used in fertilizers.

Visual example: elements on the periodic table

Metals are usually found on the left side of the periodic table, while nonmetals are found on the right. The following is a simplified periodic table showing this layout:

Applications of metals and nonmetals

Because of their properties, metals and nonmetals are used in a variety of ways across many industries. Selecting the proper element is important when designing or manufacturing products.

Uses of metals

  • Construction: Metals such as steel and aluminium are widely used in the construction of infrastructure due to their strength and durability.
  • Electronics: Metals such as copper and gold exhibit excellent conductivity, making them ideal for use in electronic components.
  • Aerospace: Lightweight metals such as aluminum are essential in aircraft manufacturing because of their excellent strength-to-weight ratio.

Uses of non-metals

  • Agriculture: Nonmetals such as nitrogen are important in the production of fertilizers for plant growth.
  • Health: Oxygen is vital for medical applications, while carbon is fundamental in pharmaceuticals.
  • Environmental management: Non-metallic applications include air purification and water treatment processes.

Conclusion

The study of metals and nonmetals provides us with important information about the nature and behavior of the elements on the periodic table. Each has unique properties that lend themselves to specific practical applications, impacting a variety of fields from technology to healthcare. By understanding these fundamental differences, we gain an appreciation for the diverse functionalities that metals and nonmetals contribute to everyday life.


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Metals and Nonmetals

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