CBSE Class 10 Metals & Non-Metals Notes 2025

Metals and non-metals are all around us, from the iron in your bicycle to the oxygen you breathe! This chapter 3 Metals and Non metals class 10 helps us understand their properties, reactions and uses. You'll learn about how metals are good conductors, how non-metals form covalent bonds, and why some metals like sodium are so reactive. Plus, we’ll break down key concepts all aligned with Class 10 Science Syllabus totally plus study tips, common mistakes, and how to make your own creative notes for better retention. Educart is very helpful, you know ;)

Caution: Too much information ahead, scroll at your own risk 🤭. Let’s get started!

Metals and Non Metals Class 10 Notes PDF Download

This study material for Class 10 explains the basics of Metals and Non-Metals in an easy-to-understand way. Download the PDF to learn key concepts and prepare well for your exams.

Below we have provided the links to downloadable PDFs of class 10 Ch 3 science notes and get an in-depth explanation and understanding of the chapter.

Metals and Non-Metals Part 1 Notes

<cta2>Download<cta2>

Metals and Non-Metals Part 2 Notes

<cta2>Download<cta2>

‍

What are Metals and Non-Metals?

Metals and non-metals represent two different groups of elements. Nonmetals, like phosphorus and sulfur, act as insulators, whereas metals, including copper and aluminium, effectively conduct heat and Metals and Non-metals. The classification of materials is based on their physical and chemical characteristics.

Physical Properties of Metals and Non-Metals

Metals:

• Malleable (can be hammered into thin sheets, e.g., aluminium foil).
• Ductile (can be drawn into wires, e.g., copper wire).
• Lustrous (shiny surface, e.g., gold, silver).
• Good conductors of heat and Metals and Non-metals (e.g., copper, silver).
• High melting and boiling points (except mercury, which is liquid at room temperature).

Non-Metals:

• Brittle (break when hammered, e.g., sulfur, phosphorus).
• Non-ductile (cannot be drawn into wires).
• Dull appearance (except iodine, which is lustrous).
• Poor conductors of heat and Metals and Non-metals (except graphite, which is a good conductor).
• Low melting and boiling points (except carbon in diamond form).

Chemical Properties of Metals and Non-Metals

Reaction with Oxygen

• Metals + Oxygen → Metal Oxide (Basic or Amphoteric)

Example: 4Na + O₂ → 2Na₂O (Sodium oxide)

• Non-Metals + Oxygen → Non-Metal Oxide (Acidic or Neutral in nature)

Example: C + O₂ → CO₂ (Carbon dioxide)

Reaction with Water

• Highly reactive metals react with water to form metal hydroxides & hydrogen gas.

Example: 2Na + 2H₂O → 2NaOH + H₂

• Less reactive metals react slowly or not at all with water.

Reaction with Acids

• Metals + Acid → Salt + Hydrogen Gas

Example: Zn + 2HCl → ZnCl₂ + H₂

• Non-metals do not react with acids.

Reaction with Bases

• Some metals react with strong bases like NaOH to form salt and hydrogen gas.

Example: Al + NaOH + H₂O → NaAlO₂ + H₂

The Reactivity Series Class 10 

The Reactivity Series arranges metals from most reactive to least reactive:

Potassium > Sodium > Calcium > Magnesium > Aluminium > Zinc > Iron > Tin > Lead > Hydrogen > Copper > Silver > Gold

• More reactive metals can displace less reactive metals from their compounds.
• Metals like K, Na, and Ca react vigorously with water and acids, while Cu, Ag, and Au do not react at all.

Corrosion and Rusting

Corrosion:

The gradual destruction of metals due to reactions with oxygen, water, or acids.

• Example: Copper develops a green coating of copper carbonate.
•  Silver turns black due to silver sulfide formation.

Rusting of Iron:

Iron + Oxygen + Water → Rust (Hydrated Iron Oxide, Fe₂O₃·xH₂O)

Prevention Methods:

• Painting
• Galvanization (coating with zinc)
• Alloying (mixing with chromium to make stainless steel)

Metallurgy (Extraction of Metals from Ores)

Steps in Metallurgy:

1. Concentration of Ore – Removing unwanted impurities.
2. Reduction of Metal Oxide to Metal – Heating with carbon or electrolysis.
3. Refining of Metal – Purification using electrolysis.

Example: Extraction of Iron

• Ore used: Hematite (Fe₂O₃)
• Reduced using carbon to form iron metal:
  Fe₂O₃ + 3C → 2Fe + 3CO₂

All Important Equations & Formulae from Metals and Non-Metals Class 10

1. Reaction of Metals with Oxygen

Metal + Oxygen → Metal Oxide

• 4Na + O₂ → 2Na₂O (Sodium Oxide)
• 2Mg + O₂ → 2MgO (Magnesium Oxide)

Amphoteric Oxides (react with both acids & bases):

• Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O (Reaction with acid)
• Al₂O₃ + 2NaOH + 3H₂O → 2NaAl(OH)₄ (Reaction with base)

2. Reaction of Metals with Water

Metal + Water → Metal Hydroxide + Hydrogen Gas 

(For highly reactive metals like Na, K, Ca)

• 2Na + 2H₂O → 2NaOH + H₂
• Ca + 2H₂O → Ca(OH)₂ + H₂

Metal + Steam → Metal Oxide + Hydrogen Gas 

(For moderately reactive metals like Mg, Fe, Zn)

• 3Fe + 4H₂O → Fe₃O₄ + 4H₂
• Mg + H₂O (steam) → MgO + H₂

Less reactive metals (Cu, Ag, Au, Pb) do not react with water.

3. Reaction of Metals with Acids

Metal + Acid → Salt + Hydrogen Gas 

(Metals like Zn, Mg, Fe react with acids)

• Zn + 2HCl → ZnCl₂ + H₂
• Mg + 2HCl → MgCl₂ + H₂
• Fe + 2HCl → FeCl₂ + H₂

Exception: Copper (Cu), Silver (Ag), and Gold (Au) do not react with dilute acids.

4. Reaction of Metals with Bases

Metal + Base → Salt + Hydrogen Gas

(Few metals react with strong bases like NaOH & KOH)

• Al + NaOH + H₂O → NaAlO₂ + H₂ (Sodium Aluminate)
• Zn + 2NaOH → Na₂ZnO₂ + H₂ (Sodium Zincate)

5. Metal Displacement Reactions

More reactive metal displaces less reactive metal from its salt solution.

• Zn + CuSO₄ → ZnSO₄ + Cu
• Fe + CuSO₄ → FeSO₄ + Cu
• Mg + FeSO₄ → MgSO₄ + Fe

6. Corrosion & Rusting of Iron

Rusting of Iron:

• Iron + Oxygen + Water → Hydrated Iron Oxide (Rust)
• 4Fe + 3O₂ + 6H₂O → 4Fe(OH)₃
• Fe(OH)₃ → Fe₂O₃·xH₂O (Rust)

Prevention Methods:

• Galvanization: Coating with Zinc
• Alloying: Mixing with Chromium (Stainless Steel)

7. Electrolysis of Molten Ionic Compounds

Electrolysis of NaCl (Molten Sodium Chloride):

• At Cathode (-): Na⁺ + e⁻ → Na (Sodium metal forms)
• At Anode (+): 2Cl⁻ → Cl₂ + 2e⁻ (Chlorine gas released)

8. Extraction of Metals (Metallurgy Process)

Step 1: Ore Concentration (Removing Impurities)

• Froth Floatation (for Sulphide Ores)
• Magnetic Separation (for Magnetic Ores like Fe₃O₄)
• Gravity Separation (for Heavy Ores like Haematite - Fe₂O₃)

Step 2: Reduction of Metal Oxides to Metals

By Carbon (for moderately reactive metals like Fe, Zn, Pb, Cu)

• Fe₂O₃ + 3C → 2Fe + 3CO₂ (Extraction of Iron)
• ZnO + C → Zn + CO (Extraction of Zinc)

By Electrolysis (for highly reactive metals like Na, K, Al)

• Al₂O₃ → 2Al + 3O₂ (Electrolysis of Alumina in Cryolite)

9. Alloy Formation

• Brass = Copper + Zinc
• Bronze = Copper + Tin
• Stainless Steel = Iron + Chromium + Nickel
• Solder = Lead + Tin

Important Questions from Ch 3 Metals and Non Metals Class 10

Ch 3 Metals and Non-Metals covers important concepts about the properties, reactions, and uses of metals and non-metals. Here are some important questions that will help you understand and master this chapter effectively.

1. Why do metals conduct Metals and Non-metals while non-metals do not?

Answer: Metals conduct Metals and Non-metals because they have free electrons that can move through the metal structure. These electrons create an electric current when a voltage is applied.

Non-metals, on the other hand, lack free electrons because their atoms hold onto their electrons tightly. Since there are no free-moving electrons, non-metals do not conduct Metals and Non-metals.

Example:

• Copper, silver, and aluminum are excellent conductors.
• Non-metals like sulfur, phosphorus, and carbon (except graphite) are poor conductors.

2. Why do ionic compounds (like NaCl) conduct Metals and Non-metals in molten or aqueous state but not in solid state?

Answer:

• In solid state: The ions in ionic compounds are held in a rigid structure and cannot move, so they do not conduct Metals and Non-metals.
• In molten or aqueous state: The ions get free to move in the liquid, allowing them to carry charge and conduct Metals and Non-metals.

Example:

• Solid NaCl (table salt) does not conduct Metals and Non-metals.
• When dissolved in water (NaCl → Na⁺ + Cl⁻), it allows current to pass through.

3. What is the reactivity series? Why is it important?

Answer: The reactivity series is a list of metals arranged in order of their reactivity, from most to least reactive.

Reactivity Series:
Potassium > Sodium > Calcium > Magnesium > Aluminium > Zinc > Iron > Tin > Lead > Hydrogen > Copper > Silver > Gold

Importance:

• It helps predict metal displacement reactions (e.g., zinc can displace copper from copper sulfate).
• It explains why some metals react more violently with acids and water than others.
• It is useful in choosing methods for metal extraction (more reactive metals require more complex extraction).

4. Why does aluminium not corrode easily even though it is highly reactive?

Answer:

• Aluminium is highly reactive and forms aluminium oxide (Al₂O₃) when exposed to air.
• This oxide layer is strong and non-porous, preventing further corrosion by acting as a protective barrier.

Example:

• Unlike iron, which keeps rusting because rust is porous, aluminium remains protected due to its oxide layer.
• This property is used in aircraft bodies and kitchen utensils to prevent damage.

5. Why do metals like sodium and potassium catch fire when exposed to water? How are they stored?

Answer:

• Sodium (Na) and potassium (K) are highly reactive metals that react violently with water, producing hydrogen gas and a large amount of heat, which causes them to catch fire.

Reaction:
2Na + 2H₂O → 2NaOH + H₂ (hydrogen gas) + heat

• Storage: These metals are stored in kerosene oil to prevent them from coming into contact with air or water.

6. Explain the reaction of metals with acids. Why do non-metals not react with acids?

Answer:

• Metals react with acids to form salt and hydrogen gas.
• The reaction is more vigorous for highly reactive metals like sodium and calcium and slow for less reactive metals like iron and zinc.

Example:
Zn + 2HCl → ZnCl₂ + H₂ (Zinc chloride + Hydrogen gas)

• Non-metals do not react with acids because they do not release electrons to form positive ions, which is necessary for the reaction.

7. What is galvanization? Why is it done?

Answer: Galvanization is the process of coating iron or steel with a thin layer of zinc to prevent rusting.

Why is it done?

• Zinc is more reactive than iron and forms a protective layer that prevents moisture and oxygen from reaching the iron.
• Even if the coating is scratched, zinc reacts first (sacrificial protection), stopping the iron from rusting.

Example:

• Galvanized iron pipes and roofs last longer in humid conditions.
• Iron bridges and railway tracks are galvanized to prevent rusting.

Common Mistakes to Avoid in Metals and Non Metals

🚫 Forgetting exceptions – Example: Aluminium is a metal, but it reacts with acids AND bases (Amphoteric).

🚫 Mixing up the reactivity series – Always remember, potassium and sodium are super reactive!

🚫 Writing wrong equations – Balance chemical equations carefully.

🚫 Confusing displacement reactions – Only a more reactive metal can displace a less reactive one.

🚫 Ignoring corrosion prevention – Don’t just learn what rusting is; remember how to prevent it!

How Can Notes Help?

• Better Retention – Writing notes in your own words helps you remember concepts more effectively than just reading.
• Quick Revision – Well-organized notes save time before exams, allowing you to review important topics in minutes.
• Clarity in Answers – Structuring your notes improves your ability to write clear and precise answers in exams.
• Personalized Learning – When you create your own notes, you understand topics in a way that makes sense to you.
• Active Engagement – The process of making notes keeps you focused and reduces passive learning.
• Stronger Conceptual Understanding – Summarizing and organizing information helps you connect different topics better.
• Improved Writing Speed – Regular note-making enhances your ability to recall and write answers quickly in exams.
• Less Stress Before Exams – Well-prepared notes reduce last-minute cramming and boost confidence.

How to Make Creative Notes for This Chapter?

Make Mind Maps

• Draw a big circle in the center with the title Metals vs. Non-Metals.
• From this, branch out to physical properties, chemical properties, reactions, and uses.
• Add small drawings or symbols (e.g., a shiny coin for metals, a dull piece of coal for non-metals).

2. Use the Story Method for the Reactivity Series

• Create a funny or weird sentence to remember the order:

1. Example: "Please Stop Calling Me A Zebra Instead Try Learning How Copper Saves Gold."
2. (Potassium, Sodium, Calcium, Magnesium, Aluminium, Zinc, Iron, Tin, Lead, Hydrogen, Copper, Silver, Gold)

• Imagine a funny scene where a zebra is arguing with an iron rod, and gold is calmly watching. The crazier, the better—your brain remembers weird stuff easily.

3. Color Code & Highlight Reactions

• Use three different colors for reactions:

1. Red for metals reacting with oxygen.
2. Blue for metals reacting with acids.
3. Green for displacement reactions.

• This way, your brain connects colors with concepts, making recall easier.

4. Create Your Own "Why" Questions

• Instead of memorizing blindly, ask yourself:

1. Why does iron rust, but gold doesn’t?
2. Why does zinc react with acid, but copper doesn’t?
3. Why do metals conduct electricity, but non-metals don’t?

• Answering these in your own words will deepen your understanding and make it stick.

5. Doodle & Relate to Real Life

• Draw a bridge rusting to remember corrosion.
• Sketch a lightning bolt hitting a metal rod to recall conductivity.
• Make a small comic strip showing a metal displacing another from a compound—turn it into a funny conversation.

6. Quick Flashcards for Revision

• Write questions on one side and answers on the other.
• Keep them handy for quick revision before the exam.
• Shuffle them and try recalling answers without looking—turn it into a game.

7. Summarize in One Page with Key Formulas & Reactions

• At the end of your notes, create a single page with all important reactions, formulas, and definitions.
• Stick this on your study table for a quick glance before the exam.

Metals and non-metals are essential in our daily lives, from cooking utensils to life-saving oxygen! Understanding their properties and reactions helps us in chemistry and in real-life applications. By making creative notes, avoiding common mistakes, and practicing important questions, you can learn and practice this chapter easily. Happy Learning!

‍

Frequently Asked Questions

1. What are the main differences between metals and non-metals?
   Metals are generally shiny, good conductors of heat and electricity, and are malleable. Non-metals, on the other hand, are usually dull, poor conductors, and brittle in nature.
2. What is the reactivity series, and how is it useful?
   The reactivity series is a list that arranges metals in order of their reactivity with substances like water, acids, and oxygen. It helps predict how metals will react in different conditions.
3. What are the properties of metals that make them useful in everyday life?
   Metals are ductile, malleable, and have high melting points, which makes them useful in various applications like wires, building materials, and machinery.
4. Why do metals form basic oxides while non-metals form acidic oxides?
   Metals tend to lose electrons and form basic oxides, whereas non-metals tend to gain electrons and form acidic oxides when they react with oxygen.
5. What are the common methods used to extract metals from ores?
   Metals are extracted from their ores using processes like roasting, smelting, and electrolysis, depending on the reactivity of the metal.