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 → Periodic table ↓


Metals, non-metals, metalloids and their properties


The periodic table is a fascinating array full of elements that are fundamental to the world we live in. It is not just a collection of elements but a scientific method of arranging them based on their properties. Elements can generally be classified into three categories: metals, nonmetals and metalloids. This classification is based on their distinctive physical and chemical properties.

Metals

Most of the elements in the periodic table are metals, located in the left and middle portions. Generally, metals are solid at room temperature, the exception being mercury. Let's explore some of the defining characteristics of metals:

Properties of metals

  • Conductivity: Metals are excellent conductors of heat and electricity because of their freely moving delocalized electrons. This property makes them ideal for electrical wires.
  • Ductility and ductility: Metals can be hammered into thin sheets (ductile) or drawn into wires (ductile). This is an important property for manufacturing and industrial applications.
  • Lustre: Metals are usually shiny and reflect light well.
  • Density: Most metals have high density.
  • Melting and boiling points: Metals generally have high melting and boiling points. Exceptions include metals such as lithium.
  • Hardness: Most metals are hard, although there are exceptions such as sodium.
  • Reactivity: Metals lose electrons to form positive ions. For example, sodium loses an electron to form Na+.
Physical Properties of Metals

Common metals include iron, which is important for construction; copper, which is used for electrical wiring; and aluminum, which is known for being lightweight and corrosion resistant.

Nonmetals

Nonmetals are located on the right side of the periodic table and are quite different from metals in their properties. They form a smaller part of the periodic table compared to metals but are equally important.

Properties of non-metals

  • Poor conductivity: Nonmetals are generally poor conductors of electricity and heat, and behave as insulators.
  • Brittleness: Non-metals are brittle in the solid state and are not malleable or ductile.
  • Lack of luster: Nonmetals do not have the shiny appearance of metals; they can appear dull.
  • Different states: Nonmetals can be solids, liquids, or gases at room temperature. For example, oxygen is a gas, bromine is a liquid, and carbon is a solid.
  • Low Density: Generally non-metals have lower density than metals.
  • Reactivity: Nonmetals gain or share electrons when they react. For example, chlorine gains an electron to form Cl-.
Physical Properties of Nonmetals

Examples of nonmetals include oxygen, which is essential for respiration; nitrogen, which is a major component of the air we breathe; and carbon, which is fundamental to organic chemistry and life.

Metalloids

Located between metals and nonmetals in the periodic table, metalloids or semimetals have properties of both categories. This unique position allows them to play a vital role in various applications, especially electronics.

Properties of metalloids

  • Semiconductors: Metalloids have intermediate electrical conductivity, which is useful in the semiconductor industry.
  • Mixed Properties: Metalloids can exhibit properties similar to metals (such as luster) and nonmetals (such as brittleness).
  • Variable reactivity: The reactivity of metalloids depends on the element they are interacting with; they can either lose or gain electrons.
  • Physical State: Most metalloids are solid at room temperature.
Physical Properties of Metalloids

Common examples of metalloids include silicon, which is a key component of computer chips; germanium, which is used in transistors; and arsenic, which has a variety of industrial uses.

Understanding the periodic table layout

The layout of the periodic table is based on atomic number and electron configuration, which affect an element's physical and chemical properties. Understanding its structure can help identify the family or group, which includes metals, nonmetals, and metalloids.

Visual example: rough layout

MetalsMetalloids Nonmetals

This flexible organization allows scientists to predict the properties and behavior of an element based on its position relative to other elements in its family.

Periodic trends

In addition to classifying elements as metals, nonmetals or metalloids, the periodic table also reveals patterns or trends in element properties.

Trends among elements

  • Atomic radius: Decreases from left to right in a period and increases down the group.
  • Ionization energy: increases across a period and decreases down a group. This is the energy required to remove an electron from an atom.
  • Electronegativity: Tends to increase across a period and decrease down a group. It describes the ability of an atom to attract electrons in a bond.

Understanding these trends can help predict how an element will interact with other elements, and affect its use in compounds and reactions.

Chemical reactions and bonding

Elements interact through chemical reactions, forming bonds to achieve stability. Metals, nonmetals, and metalloids have different ways of reacting:

Metals

Metals often lose electrons to form cations in reactions, usually reacting with non-metals to form ionic compounds. For example:

2 Na + Cl 2 → 2 NaCl

Nonmetals

Nonmetals gain electrons or share electrons in covalent bonds. For example, two hydrogen atoms share electrons with an oxygen atom to form water:

2 H 2 + O 2 → 2 H 2 O

Metalloids

Metalloids can participate in covalent bonding, which demonstrates flexibility in their chemical interactions. For example, silicon forms covalent bonds in silicon dioxide:

Si + O 2 → SiO 2

Applications and uses

Each category of elements finds its place in different areas due to their different properties:

Metals

  • Construction: Iron and steel are used to construct buildings.
  • Electronics: Copper and aluminum are used for wiring because of their excellent conductivity.
  • Transportation: Lightweight aluminum is used in aircraft and car manufacturing.

Nonmetals

  • Essential Gases: Oxygen is vital to life and many industrial processes.
  • Plastic: Carbon in the form of polymers is used for a variety of products, including containers and clothing.
  • Lighting: Neon is used in neon signs because of its glowing properties.

Metalloids

  • Semiconductors: Silicon and germanium are vital to electronics, which form the basis of modern computing.
  • Solar Cells: Silicon is widely used in solar panels for energy conversion.

Conclusion

The periodic table is not just a collection of elements, but a framework that organizes them based on similar properties. Understanding the characteristics of metals, nonmetals, and metalloids can help us learn how the elements behave and interact, leading to insights into their wide-ranging applications and importance. By studying these categories, we can appreciate the diversity and complexity of the elements that make up our world.


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