Metals and non-metals class 10 pdf

 

Metals and non-metals notes

•  Introduction to metals and non-metals

•  Physical and chemical properties of   metals

•  Physical and chemical properties of   non-   metals 

• Occurrence and extraction of metals

•  Reactivity series of metals

•  Corrosion and its prevention

•  Uses of metals and non-metals

•  Difference between metals and non-metals

Class 10 science all chapter series 

Chapter: 1 click here

Chapter : 2 click here 

Define metals and non-metals 

Metals and non-metals are two categories of elements in the periodic table. They are distinguished from each other based on their physical and chemical properties.

Metals:

Metals are elements that are good conductors of heat and electricity. They are typically located on the left side and middle of the periodic table. 

 Examples of metals:

 Iron (Fe)

 Copper (Cu) 

 Aluminum (Al)

 Gold (Au) 

 Silver (Ag)

Non-metals: 

 Non-metals are elements that are poor conductors of heat and electricity. They are usually located on the right side of the periodic table. 

 Examples of non-metals:

 Carbon (C) 

 Oxygen (O)

 Chlorine (Cl) 

 Nitrogen (N) 

 Sulfur (S)  

Physical and chemical properties of metals

 Physical properties: 

 Lustre: 

Metals have a shiny, reflective surface known as lustre. This is due to their ability to reflect light.

 Malleability:

 Metals are malleable, which means they can be pounded into thin sheets without breaking or cracking. 

 Ductility: 

Metals are ductile, which means they can be drawn into wires without breaking.

 Conductivity:

 Metals are good conductors of heat and electricity. They have free electrons that can move around easily, which makes them good conductors. 

 Density: 

Metals have a high density, which means they are heavy for their size.

 Chemical properties:

 Reactivity: 

Metals are highly reactive and readily react with non-metals to form ionic compounds.

 Corrosion: 

Metals are prone to corrosion, which is a gradual wearing away of the metal due to chemical reactions with the environment.

 Oxidation: 

Metals tend to lose electrons when they react, and form positive ions or cations. This process is known as oxidation.

 Electropositivity: 

Metals have a tendency to donate electrons and become positively charged ions.

 Reaction with acids: 

Most metals react with acids to produce hydrogen gas and a salt. These physical and chemical properties of metals make them useful in many applications such as construction, electrical wiring, and transportation.

Physical and chemical properties of non-metals 

 Non-metals are elements that lack the characteristics of metals. They are located to the right of the periodic table and include elements such as carbon, nitrogen, oxygen, and sulfur. Non-metals have distinct physical and chemical properties that differentiate them from metals. Some of the most important physical and chemical properties of non-metals are: 

 Physical Properties:

•  Non-metals are typically brittle, meaning that they are not malleable or ductile and can break easily.

•  They have low melting and boiling points, which means they usually exist as gases or solids at room temperature. 

•  Non-metals are poor conductors of electricity and heat. They do not have the ability to conduct electricity due to the lack of free electrons in their outer shells.

•  Non-metals are often soft and have low densities, making them lightweight and easy to manipulate. They are not shiny or lustrous in appearance.

 Chemical Properties: 

•  Non-metals have a tendency to gain electrons, forming anions, which is why they are often found in ionic compounds with metals.

•  They are usually more Electronegative than metals, meaning they have a greater attraction for electrons. 

•  Non-metals typically form covalent bonds with other non-metals to share electrons and form molecules. They are generally not reactive with acids, but can react with bases to form salts and water.

• Non-metals are often found in organic compounds and are essential building blocks for life, such as carbon in DNA and proteins. 

 Overall, non-metals have unique properties that make them important for a wide range of applications in science, technology, and industry.  

Metals :  occurrence and extraction.

 Occurrence of Metals: 

 Metals occur in nature in different forms - as minerals, ores, and rocks. Some metals, like gold, silver, and copper, are found in pure form, while others are found in the form of compounds. For example, iron is found in the form of iron oxide (Fe2O3), which is known as hematite. 

 Extraction of Metals: 

 Metals can be extracted from their ores by various methods. The method used depends on the reactivity of the metal and the nature of the ore. 

 Extraction of highly reactive metals: 

 Highly reactive metals, like sodium, potassium, calcium, and magnesium, are extracted by electrolysis of their molten chlorides or oxides. 

 Extraction of moderately reactive metals:

 Moderately reactive metals, like zinc, iron, and lead, are extracted by reducing their oxides with carbon (in the form of coke) in a blast furnace. 

 Extraction of low reactive metals:

 Less reactive metals, like copper, silver, and gold, are extracted from their ores by various methods, including leaching, electrolysis, and reduction with carbon or hydrogen. 

 Overall, the extraction of metals from their ores requires a lot of energy and resources, and it can have significant environmental impacts. Therefore, recycling of metals is becoming increasingly important as a way to conserve resources and reduce environmental pollution.

Reactivity series of metals

     The reactivity series of metals is a list of metals arranged in order of their relative reactivity towards chemical reactions. The series is based on the tendency of metals to lose electrons and form positive ions. The reactivity series of metals from the most reactive to the least reactive is as follows:

•  Potassium (K) 

•  Sodium (Na) 

•  Calcium (Ca) 

•  Magnesium (Mg) 

•  Aluminium (Al) 

•  Zinc (Zn)

•  Iron (Fe) 

•  Nickel (Ni)

•  Tin (Sn) 
•  Lead (Pb) 
•  Hydrogen (H)
•  Copper (Cu)
•  Silver (Ag) 
•  Gold (Au) 

 Note that metals higher up in the series are more reactive and can displace metals lower down the series from their compounds. For example, magnesium can displace copper from copper sulfate solution

Metal Corrosion Prevention. 

 Corrosion is the process by which metals are gradually destroyed or deteriorated due to chemical reactions with their environment. The most common form of corrosion is rusting, which occurs when iron or steel reacts with oxygen and water to form iron oxide. 

 Preventing corrosion of metals involves taking several measures such as: 

 Use of coatings: 

Applying a protective coating such as paint, varnish, or enamel can help prevent corrosion by creating a barrier between the metal and the environment. 

 Galvanization:

 Coating a metal with a thin layer of zinc, which is more reactive than the metal itself, can provide protection against corrosion. This process is called galvanization. 

 Use of alloys: 

Using an alloy instead of a pure metal can provide better resistance to corrosion. For example, stainless steel contains chromium, which forms a protective oxide layer on the surface of the metal. 

 Cathodic protection: 

This technique involves connecting the metal to be protected to a more reactive metal, such as magnesium or zinc. The more reactive metal acts as an anode and corrodes instead of the metal to be protected. 

 Maintenance: 

Regular cleaning and maintenance of the metal surface can help prevent corrosion. Removing dirt, grime, and other substances can prevent the build-up of corrosive agents. 

 In summary, preventing corrosion of metals involves taking measures such as using coatings, galvanization, using alloys, cathodic protection, and regular maintenance.  

Uses of metals and non-metals 

 Uses of Metals: 

 Electrical Conductors: 

Metals like copper, aluminum, and gold are used in making electrical wires and cables as they are good conductors of electricity.

 Construction and Architecture: 

Metals like iron, steel, and aluminum are widely used in construction and architecture. 

For example, iron is used in making beams and columns, while steel is used in making structures like bridges and buildings.

 Transportation: 

Metals like iron, steel, and aluminum are used in the manufacturing of vehicles, airplanes, ships, and trains. 

 Coins:

 Metals like copper, nickel, and silver are used in making coins. Jewelry: Precious metals like gold and silver are used in making jewelry. 

 Medicine:

 Some metals like silver, gold, and copper have medicinal properties and are used in medicines. 

 Uses of Non-Metals:

 Oxygen: 

Oxygen is a non-metal and is essential for the survival of all living organisms. It is used for respiration and combustion.

 Carbon: 

Carbon is a non-metal and is used in making fuels like coal and charcoal.

 Graphite:

 Graphite is a non-metal and is used in making pencils, lubricants, and electrodes.

 Sulphur: 

Sulphur is a non-metal and is used in making fertilizers and chemicals. 

 Chlorine: 

Chlorine is a non-metal and is used in making disinfectants and bleach.

 Phosphorus:

 Phosphorus is a non-metal and is used in making fertilizers and detergents.  

Difference between metals and non-metals

     Metals and non-metals are two broad categories of elements that are classified based on their physical and chemical properties. Here are some of the main differences between metals and non-metals: 

 Physical appearance:

 Metals are generally shiny, opaque, and have a metallic luster, while non-metals are dull, translucent or transparent, and have a non-metallic luster. 

 Conductivity: 

Metals are good conductors of heat and electricity, while non-metals are poor conductors of both. 

 Malleability and ductility: 

Metals are malleable and ductile, meaning they can be hammered or rolled into thin sheets or drawn into wires. Non-metals, on the other hand, are brittle and cannot be easily molded into different shapes.

 Density: 

Metals are generally dense, while non-metals are less dense. 

 Melting and boiling points:

 Metals have high melting and boiling points, while non-metals have low melting and boiling points.

 Reactivity:

 Metals tend to lose electrons and form positive ions, while non-metals tend to gain electrons and form negative ions. Metals are generally more reactive than non-metals, and many of them react with water and acids to produce hydrogen gas. 

 Examples of metals include iron, copper, gold, and aluminum, while examples of non-metals include carbon, sulfur, nitrogen, and oxygen.