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Unlock Potential with Future Classes - Exploring Metals and Non-Metals for Class 10 CBSE Students

CBSE Class 10 Science Metal and Non Metal is an important topic for students to understand. Our website provides a wealth of resources to help students learn and understand the difference between metals and non-metals. Our free PDF notes provide detailed explanations of all the key concepts associated with this topic. Additionally, we offer a range of interactive activities and exercises to help students practice and apply their knowledge. With our resources, students can gain a comprehensive understanding of metals and non-metals to help them in their studies.

CBSE Class 10 Science Metal and Non Metal is an important topic for students to understand. Our website provides a wealth of resources to help students learn and understand the difference between metals and non-metals. Our free PDF notes provide detailed explanations of all the key concepts associated with this topic. Additionally, we offer a range of interactive activities and exercises to help students practice and apply their knowledge. With our resources, students can gain a comprehensive understanding of metals and non-metals to help them in their studies.

CHAPTER - 3 METALS AND NON-METALS

Metal

Element that are electropositive in nature are called metal, e.g., copper.

Physical Properties of Metal

  1. Malleability It is the property of metals due to which they can be beaten into thin sheets. Most of the metals are malleable.

  2. Ductility It is the property due to which a metal can be drawn into wires. Metals are generally ductile. Gold is the most ductile metal.

  3. Hardness Most of the metals are hard. But some alkali metals like sodium and potassium are so soft that they can be cut easily with knife.

  4. Metallic Luster Metals in their pure state have bright shining surfaces. This property is called metallic luster.

  5. Electrical Conductivity Most of the metals are good conductors of electricity.

  6. Thermal Conductivity Generally metals are good conductors of heat, except lead and mercury, which are poor conductors of heat. The best conductors of heat are copper and silver among all metals.

  7. Melting and Boiling Points Metals generally have high melting and boiling point, except mercury, gallium and alkali metals. Tungsten has the highest melting point among metals while mercury has the lowest.

  8. Sonority When metals are struck with a hard substance, they produce sound. This property is called sonority and the metals are said to be sonorous bells are made up of metal due to this property.

CHEMICAL PROPERTIES OF METALS

Most of the chemical properties of metals are due to their electropositive nature. It means metal atom loses electrons to form cation.

formation of metal cation

Reaction with Air:

Metals combine with oxygen to form metal oxide.

metal react with oxygen equation

Examples:

example of metal react with oxygen

Different metals show different reactivity’s towards oxygen.

  • Na and K react so vigorously that they catch fire if kept in open so they are kept immersed in kerosene.

  • Surfaces of Mg, Al, Zn, Pb are covered with a thin layer of oxide which prevent them from further oxidation.

  • Fe does not burn on heating but iron fillings burn vigorously.

  • Cu does not burn but is coated with black copper oxide.

  • Au and Ag does not react with oxygen.

Amphoteric Oxides:

Metal oxides which react with both acids as well as bases to produce salts and water are called amphoteric oxides.

Examples

formation of amphoteric oxide

Reaction of Metals with Water:

Reaction of Metals with Water

  • React with cold water Na, K, Ca

  • React with steam Al, Fe, Zn        

  • React with hot water Mg

  • No reaction with water Pb, Cu, Au, Ag            

  • Ca and Mg float as bubbles of H2 stick to their surface

Examples

example of metal and water reaction

Reaction of Metals with Acids (Dilute):

equation of reaction between metal and acids

Cu, Ag, Hg do not react with dilute acids

Examples

metal and acids reaction example

Reaction of Metals with Solutions of other Metal Salts

Reaction of Metals with Solutions of other Metal Salts

  • Reactive metals can displace less reactive metals from their compounds in solution form.

Reaction of Metals with Solutions of other Metal Salts

REACTIVITY SERIES OR ELECTROCHEMICAL SERIES OF METALS

The reactivity series is a list of metals arranged in the order of their decreasing activities.

REACTIVITY SERIES OR ELECTROCHEMICAL SERIES OF METALS

Non-metal

Element that are electronegative in nature are called non-metal. It means non-metals gain electrons to form negative ions, e.g., iodine

Physical Properties of Non-metals

  1. Brittleness Non-metals are neither malleable nor ductile but they are brittle in nature.

  2. Physical State Most of the non-metals are soft (if solid). Only diamond, a form of carbon is the hardest known substance. Other non-metals are gases except bromine which is a liquid.

  3. Metallic Luster The non-metals do not have luster, i.e., shining surface. However, diamond, graphite (forms of carbon) and iodine have luster, even they are non-metals.

  4. Electrical and Thermal Conductivity Non-metals are generally poor conductors of heat and electricity.

  5. Melting and Boiling Points Generally, non-metals have low melting and boiling points. But non-metals that are solids have comparatively higher boiling points (e.g., B, Si, C, etc.).

Chemical properties of non-metal

Reaction with oxygen

Nonmetal react with oxygen to form oxides. These oxides are generally acidic. Only some of the non-metallic oxides are neutral.

non metal react with oxygen chemical equation

Displacement reaction

Nonmetal also show displacement reaction like metal.

Displacement reaction

Reaction of Metals with Non-metals

  • Reactivity of elements is the tendency to attain a completely filled valence shell.

  • Atoms of the metals lose electrons from their valence shell to form cation. Atom of the non-metals gains electrons in the valence shell to form anion.

Example - Formation of NaCl

Reaction of Metals with Non-metals

  • The strong electrostatic forces of attraction which help to bind Na+ and Cl- ions together is called ionic bond or electrovalent bond.

Ionic Compounds

The compounds formed by the transfer of electrons from a metal to a non-metal are called ionic compounds or electrovalent compounds.

Properties of Ionic Compounds

  1. Physical nature: They are solid and hard, generally brittle.

  2. Melting and Boiling Point: They have high melting and boiling point.

  3. Solubility: Generally soluble in water and insoluble in solvents such as kerosene, petrol etc.

  4. Conduction of electricity: Ionic compounds conduct electricity in molten and solution form but not in solid state.

Occurrence of Metals

Minerals: The elements or compounds which occur naturally in the earth’s crust are called minerals.

Ores: Minerals that contain very high percentage of particular metal and the metal can be profitably extracted from it, such minerals are called ores.

Occurrence of Metals

Extraction of Metals from Ores

Step 1. Enrichment of ores.

Step 2. Extraction of metals.

Step 3. Refining of metals.

Extraction of Metals from Ores

Steps Involved in Extraction of Metals from Ores

Some Important Terms

Gangue: Ores are usually contaminated with large number of impurities such as soil, sand etc. called gangue.

Roasting: The sulphide ores are converted into oxides by heating strongly in the presence of excess air. This process is called roasting.

roasting

Calcination: The carbonate ores are changed into oxides by heating strongly in limited air. This process is called calcination.

calcination

Reduction: Metal oxides are reduced to corresponding metals by using reducing agent like carbon.

reduction

Refining of Metals

The most widely used method for refining impure metal is electrolytic refining.

  • Anode: Impure copper

  • Cathode: Strip of pure copper

  • Electrolyte: Solution of acidified copper sulphate

  1. On passing the current through electrolyte, the impure metal from anode dissolves into the electrolyte.

  2. An equivalent amount of pure metal from the electrolyte is deposited at the cathode.

  3. The insoluble impurities settle down at the bottom of the anode and is called anode mud.

Corrosion

The surface of some metals such as iron is corroded when they are exposed to moist air for a long period of time. This is called corrosion.

  1. Silver becomes black when exposed to air as it reacts with air to form a coating of silver sulphide.

  2. Copper reacts with moist carbon dioxide in the air and gains a green coat of copper carbonate.

  3. Iron when exposed to moist air acquires a coating of a brown flaky substance called rust.

Prevention of Corrosion

The rusting of iron can be prevented by painting, oiling, greasing, galvanizing, chrome plating, anodizing or making alloys.

Galvanization:

It is a method of protecting steel and iron from rusting by coating them with a thin layer of zinc.

Alloy:

An alloy is a homogenous mixture of two or more metals or a metal and a non-metal.

Iron: Mixed with small amount of carbon becomes hard and strong.

Steel: Iron + Nickel and chromium

Brass: Copper + Zinc

Bronze: Copper + Tin (Sn)

Solder: Lead + tin

Amalgam: If one of the metals is mercury (Hg).

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