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Metals and Non-metals One-Shot Class 10 Science (Chemistry) Concepts | CBSE Class 10 Board Exams

BYJU'S - Class 9 & 10・77 minutes read

Studying metals and non-metals involve understanding their properties and characteristics, with metals known for luster, malleability, and conductivity while non-metals lack these traits, highlighting the importance of active engagement to grasp these concepts. The text delves into the reactivity of metals, processes of obtaining clean metal, methods for preventing corrosion, and the significance of alloying in strengthening metals, underscoring the need for patience and practice in mastering metal extraction and chemical properties.

Insights

Metals are known for properties like luster, malleability, and conductivity, while non-metals lack these characteristics, with exceptions like graphite and diamond.
The extraction of metals involves processes like concentration, purification, and reduction, with impurities removed through methods like magnetic separation and flotation, showcasing the complexity and precision required in obtaining pure metals.

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Recent questions

What are the properties of metals and non-metals?
Metals have luster, malleability, and ductility, while non-metals lack these properties.
How do metals conduct heat and electricity?
Metals are good conductors, unlike non-metals.
What are the exceptions to the high melting points of metals?
Gallium and tin are exceptions to high melting points in metals.
How do metals react with water?
Metals react with water to form metal oxide or metal hydroxide.
What is the process of obtaining clean metal from minerals?
Clean metal is obtained through reduction processes like calcination, roasting, and electrolytic reduction.

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Summary

00:00

Metals and Non-Metals: Properties and Characteristics

The session is focused on studying metals and non-metals, with a chapter on the topic.
The chapter covers the basics of metals and non-metals, including their properties and characteristics.
Metals are known for their luster, malleability, and ductility, while non-metals lack these properties.
Gold and silver are highlighted as the most malleable metals.
The ability of metals to conduct heat and electricity is discussed, with non-metals generally not being good conductors.
The high melting points of metals are emphasized, with exceptions like gallium and tin.
Graphite is mentioned as an exception for electrical conductivity among non-metals.
Metals are noted for being sonorous, producing a ringing sound when struck.
The importance of understanding these properties for academic success and future endeavors is stressed.
The session encourages active participation and engagement in learning about metals and non-metals.

20:26

Metal and Non-Metal Properties and Reactions

Most metals are solid at room temperature, except for mercury which is a liquid.
Non-metals can exist in solid, liquid, or gas forms, with examples like carbon, sulfur, phosphorus, iodine, and bromine.
Hydrogen, oxygen, and nitrogen are examples of non-metals that can exist in all three states.
Metals generally have high melting points, but there are exceptions like gallium, lithium, sodium, and potassium which have low melting points.
Non-metals like iodine do not have luster, except for diamond which is the hardest non-metal.
Aluminum and zinc form oxide layers on their surfaces when exposed to oxygen.
Metal oxides are generally basic in nature, but aluminum oxide is an exception and can be acidic.
Amphoteric oxides like aluminum oxide can behave as both acids and bases.
Zinc oxide is another example of an amphoteric oxide, reacting with both hydrochloric acid and sodium hydroxide to form corresponding salts and water.
Understanding the nature of metal oxides and their reactions with acids and bases is crucial for identifying their properties and behavior.

42:06

Metal Reactions with Water and Acids

Black colored copper oxide layer forms on copper.
Specific metals correspond to specific gases.
Some metals like gold and silver do not react with oxygen even at high temperatures.
Metals react with water to form metal oxide or metal hydroxide.
Sodium and potassium react violently with cold water, producing hydrogen gas.
Calcium reacts with cold water to form calcium hydroxide and hydrogen gas.
Magnesium reacts with hot water to form magnesium hydroxide, hydrogen gas, and energy.
Oxide is formed when metals react with steam, while hydroxide is formed when they react with water.
Metals like copper, gold, and silver do not react with water.
Metals react with dilute acids to form salts and hydrogen gas.

01:03:04

Metal Reactivity and Ionic Compounds Explained

Magnesium and Manganese are noble metals that release hydrogen even with dilute nitric acid.
The reaction of magnesium with nitric acid forms nitrate and hydrogen gas.
Gold and platinum react with acids, showcasing reactivity.
Royal Water is a mixture of concentrated hydrochloric acid and concentrated nitric acid in a 3:1 ratio.
Zinc is more reactive than iron and copper, leading to displacement reactions.
Copper sulfate turns green, while ferrous sulfate appears reddish-brown in reactions with metals.
The reactivity series includes potassium, sodium, lithium, calcium, magnesium, aluminum, zinc, iron, lead, copper, silver, and gold.
Metals can displace hydrogen in reactions, following a reactivity series.
Noble gases have complete outer shells, making them stable.
Ionic compounds form through the transfer of electrons from metals to non-metals, creating oppositely charged ions.

01:30:19

Metal Extraction: Processes and Techniques Explained

Minerals are naturally occurring substances that include metals, with iron present in hematite and magnetite.
Minerals with a high percentage of metal are called simerals, making extraction easy and economical.
The metallurgical process of obtaining metal involves three stages: concentration, purification, and refining.
Impurities in minerals are removed through processes like magnetic separation, gravity separation, and flotation.
Reduction is crucial in obtaining clean metal, with reactivity determining the method used.
Calcination and roasting are processes that involve heating minerals in the presence or absence of oxygen.
Metals with low reactivity, like zinc and copper, are obtained through calcination or roasting followed by reduction.
Displacement reactions with reactive metals like aluminum can also be used to obtain metals from oxides.
Liquid metal is obtained through exothermic reactions, useful for welding and joining tracks.
Electrolytic reduction is necessary for metals with high reactivity, as carbon is unable to reduce their oxides effectively.

01:50:56

Metal Extraction and Corrosion Prevention Techniques

The process of producing electricity through the reduction of Molton tap and the generation of electrons from graphite is discussed.
The reaction involving sodium and chlorine separately to produce sodium and chloride ions is explained.
The electrolytic refining of copper using acidic copper sulphate as an electrolyte is detailed.
The process of copper oxidation and reduction, leading to the deposition of copper on the cathode, is described.
The prevention of corrosion through galvanization, painting, and alloying, such as with stainless steel, is outlined.
The benefits of alloying, like strengthening iron with carbon or chromium and nickel for stainless steel, are highlighted.
The formation of basic copper carbonate and rust due to the reaction of copper with carbon dioxide and moisture is explained.
The concept of corrosion, its causes, and prevention methods, including the use of amalgams, is discussed.
The importance of practice, understanding concepts, and staying patient in learning about extraction of metals and chemical properties is emphasized.

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