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Ch 3 Metals and Non-metals for class 10
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Ch 3 IMP question science for class 10
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Some examples from this set of practice questions
1.
Explain why calcium metal after reacting with water starts floating on its surface. Write the chemical equation for the reaction. Name one more metal that starts floating after some time when immersed in water.
Answer: When calcium metal reacts with water, it produces hydrogen gas and calcium hydroxide. The hydrogen gas bubbles stick to the surface of the calcium, creating buoyancy, causing calcium to float on the water\'s surface. The chemical equation for the reaction is: Ca (s)+2H2O (l)→Ca(OH)2(aq)+H2(g)
2.
A non-metal X exists in two different forms, Y and Z. Y is the hardest natural substance, whereas Z is a good conductor of electricity. Identify X, Y, and Z.
Answer: X is carbon. Diamond and graphite are allotropes of carbon. Diamond is the hardest natural substance, and hence Y is diamond. Graphite is a good conductor of electricity, and hence Z is graphite.
3.
Why do ionic compounds conduct electricity in molten state and not in solid state?
Answer: Ionic compounds do not conduct electricity in solid state because ions are not free to move. In molten state, ions are free to move
4.
The reaction of metal X with Fe O is highly exothermic and is used to join railway tracks. Identify metal X. Write the chemical equation for the reaction
Answer: X is Aluminium. 2Al + Fe 0 Al O + 2Fe
5.
Differentiate between roasting and calcination.
Answer: Roasting Calcination (a) Ore is heated in excess (a) Ore is heated in the absence or of air. limited supply of air. (b) This is used for sulphide (b) This is used for carbonate ores. ores. (c) SO2 is produced along (c) CO2 is produced along with with metal oxide. metal oxide.
Content preview
, FARHAN ALIMetal & Non-Metal
Metals:
Metals are a group of elements characterized by
their luster, conductivity (thermal and electrical),
malleability, and ductility. They typically have high
melting and boiling points and tend to lose
electrons to form positively charged ions (cations)
in chemical reactions. Common examples include
iron, copper, gold, and aluminum.
Physical properties of metals include:
1. Lustre: Metals exhibit a characteristic shine or luster when freshly
polished, attributed to their ability to reflect light.
2. Conductivity: Metals are excellent conductors of heat and electricity
due to the mobility of electrons in their atomic structure.
3. Malleability: Metals can be easily hammered or rolled into thin sheets
without breaking, displaying malleability.
4. Ductility: Metals can be drawn into thin wires without breaking
demonstrating ductility.
5. High Melting and Boiling Points: Metals generally have high melting
and boiling points compared to nonmetals.
6. Solid State at Room Temperature: Most metals are solid at room
temperature, except for mercury, which is a liquid.
7. Density: Metals are typically dense materials, meaning they have a
high mass per unit volume.
8. Sonorous: Metals often produce a characteristic ringing sound when
struck, known as sonorousness.
, FARHAN ALI
These properties collectively contribute to the wide range of practical
applications of metals in various industries, from construction to
electronics.
Chemical Properties of Metals:
1. Reaction with Oxygen:
● Metals react with oxygen to form metal oxides. The general equation
for this reaction is:
Metal+Oxygen→Metal Oxide
# Potassium and sodium metals are extremely reactive, undergoing vigorous
reactions with the oxygen in the air. In the presence of air, they can readily
catch fire and burn. To prevent these reactive metals from reacting with
oxygen, moisture, and carbon dioxide in the air, they are stored in kerosene oil
This protective measure ensures that the metals remain stable and do not
undergo combustion when exposed to atmospheric conditions.
2. Reaction with Water:
● Some metals react with water to form metal hydroxides and release
hydrogen gas. The general equation is:
Metal+Water→Metal Hydroxide+Hydrogen
3. Reaction with Acids:
● Metals react with acids to produce salts and hydrogen gas. The
general equation is:
Metal+Acid→Salt+Hydrogen
4. Reaction with Salts:
● Metals can displace less reactive metals from their salts in solution
The reactivity series helps predict such displacement reactions.
5. Reaction with Non-Metallic Elements:
● Metals can react with non-metallic elements to form compounds. For
example, metals react with sulfur to form metal sulfides.
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