CLASS 10 NOTES
SCIENCE
Metals & Non-Metals
PRASHANT KIRAD
, PRASHANT KIRAD
Metal & 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.
, PRASHANT KIRAD
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.
SCIENCE
Metals & Non-Metals
PRASHANT KIRAD
, PRASHANT KIRAD
Metal & 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.
, PRASHANT KIRAD
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.
