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 ↓


Physical and chemical properties of metals


Metals are fascinating elements that have been used throughout history due to their wide range of properties and versatility. In this comprehensive guide, we will explore the physical and chemical properties of metals in depth. We will discuss how metals differ from non-metals, including aspects such as electrical conductivity, malleability, ductility, and chemical reactivity.

Physical properties of metals

The physical properties of metals make them different and unique from nonmetals. These properties include:

Aura

Metals have a shiny appearance called lustre. This lustre is due to the metals' ability to reflect light. A good example of this is gold, which is known for its vibrant yellow sheen. In the world of jewellery, lustre is a key and desirable feature.

A.U.

Conductivity

Metals are excellent conductors of electricity and heat. This is because their atomic structure allows free electrons to move easily, making the transfer of energy easier. Silver and copper are examples of metals that are highly conductive, and this property makes them suitable for wiring and other electrical applications.

Growability

Malleability is the ability of metals to be hammered or rolled into thin sheets. This property is due to the ability of metal atoms to slide over each other without breaking metallic bonds. Aluminum foil is a common example of malleability.

Aluminum Foil

Resilience

Ductility is the property of metals to be able to be stretched into wires. Like malleability, ductility occurs because the atoms of the metal can slide past one another while maintaining their bonds. Copper, which is often used in electrical wiring, is a prime example of a ductile metal.

Density

Metals have high density, which means they are heavy for their size. This is due to the dense packing of atoms in their crystal structure. Lead is one such metal that is known for its high density.

Rigidity

Most metals are hard, which means they are resistant to being shaped and deformed under pressure. Steel, an alloy of iron, is particularly noted for its hardness.

steel

Chemical properties of metals

In addition to their physical characteristics, metals have unique chemical properties and reactivity. Let's take a closer look at the common chemical behaviors exhibited by metals.

Reactivity with water

Many metals react with water to form metal hydroxides and hydrogen gas. Metals such as sodium and potassium react vigorously with water. For example, when sodium reacts with water, the reaction is as follows:

2Na + 2H2O → 2NaOH + H2

In this reaction, sodium hydroxide (NaOH) and hydrogen gas (H2) are formed.

Reactivity with acids

Metals react with acids to form hydrogen gas and salts. This property is commonly used to identify the reactivity of a metal. For example, when zinc reacts with hydrochloric acid, the reaction can be represented as follows:

Zn + 2HCl → ZnCl2 + H2

Here, zinc chloride (ZnCl2) and hydrogen gas (H2) are produced.

Oxidation

Metals oxidize, meaning they easily lose electrons. This is an important part of the chemical reactivity of metals, which is known as corrosion when unwanted. When metals such as iron oxidize, they form iron oxide, commonly seen as rust:

4Fe + 3O2 → 2Fe2O3

Manufacture of alloys

Metals can combine with other metals to form alloys, which are mixtures that retain the properties of metals. Alloys such as bronze (a mixture of copper and tin) and steel (iron and carbon) are important in a variety of applications because of their enhanced properties such as strength and corrosion resistance.

Comparison with non-metals

To better understand metals, it is important to distinguish them from non-metals. Non-metals generally have opposite properties, such as:

  • Poor conductors of heat and electricity (except graphite).
  • Brittle when solid and non-ductile.
  • No metallic luster; they appear dull.
  • Lower density than metals.
  • High electronegativities and ionization energies, tendency to gain electrons during reactions.

Conclusion

Metals have many remarkable physical and chemical properties that distinguish them from non-metals. Their ability to conduct electricity, be molded without cracking, and form colorful compounds when chemically reacted has made them indispensable in modern technology and industry. Understanding these properties not only contributes to our knowledge of materials science but also expands our abilities to create better materials for the future.


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Physical and chemical properties of metals

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