NCERT Solutions for Class 10 Science Chapter 1 Question 1
In this comprehensive guide, we will explore the NCERT Solutions for Class 10 Science Chapter 1 Question 1, which asks why a magnesium ribbon should be cleaned before burning in air. This is a fundamental concept in understanding chemical reactions and oxidation processes. Understanding this question helps students grasp the importance of surface preparation in chemical experiments and the reactivity of metals with atmospheric gases.
Understanding the Question 🧐
The NCERT Solutions for Class 10 Science Chapter 1 Question 1 focuses on the chemical behavior of magnesium when exposed to air. Magnesium is a highly reactive metal that readily combines with oxygen and carbon dioxide present in the atmosphere. This question teaches us about surface reactions and the importance of clean surfaces for efficient chemical reactions. When we study ncert solutions for class 10 science, we learn that metals like magnesium form protective layers that can hinder further reactions.
📝 Question: Why should a magnesium ribbon be cleaned before burning in air?
Explanation 🧪
Let me explain this concept step by step, just like a teacher would explain to a student who’s learning this for the first time.
Step 1: Understanding What Happens to Magnesium in Air
When a magnesium ribbon is stored or left exposed to air, it doesn’t remain in its pure metallic form. The shiny silver surface of magnesium gradually develops a dull white coating. This happens because magnesium is a reactive metal that combines with gases present in the atmosphere.
Two main reactions occur:
- Reaction with Oxygen: Magnesium reacts with oxygen (\(O_2\)) in the air to form magnesium oxide (\(MgO\))
- Reaction with Carbon Dioxide: Magnesium also reacts with carbon dioxide (\(CO_2\)) to form magnesium carbonate (\(MgCO_3\))
The chemical equation for the formation of magnesium oxide is:
\(2Mg + O_2 \rightarrow 2MgO\)
Step 2: Why This Coating is a Problem
The layer of magnesium oxide and magnesium carbonate that forms on the surface acts as a protective barrier. Think of it like a shield that prevents the pure magnesium underneath from coming into direct contact with oxygen in the air. This is similar to how a raincoat prevents water from reaching your clothes!
Important Point: This coating significantly reduces the efficiency of combustion because the oxygen cannot reach the metallic magnesium easily.
Step 3: The Solution – Cleaning the Ribbon
To ensure proper burning, we need to remove this oxide layer. This is done by:
- Rubbing the magnesium ribbon with sandpaper
- Using steel wool to scrape off the coating
- Exposing the shiny metallic surface underneath
Once cleaned, the pure magnesium surface is directly exposed to air, allowing for rapid and efficient combustion.
Step 4: What Happens When We Burn Clean Magnesium
When the cleaned magnesium ribbon is burned in air, it undergoes a spectacular exothermic reaction (a reaction that releases heat and light). The reaction is:
\(2Mg_{(s)} + O_{2(g)} \rightarrow 2MgO_{(s)} + \text{Energy}\)
This reaction produces:
- A brilliant white flame 🔥
- Intense heat and light
- White ash of magnesium oxide
Conclusion and Key Principles ✅
Understanding the NCERT Solutions for Class 10 Science Chapter 1 Question 1 teaches us an important principle in chemistry: surface preparation is crucial for chemical reactions. The magnesium ribbon must be cleaned to remove the oxide and carbonate layer that forms naturally in air. This ensures that the pure metal can react efficiently with oxygen during combustion, producing the characteristic bright flame and magnesium oxide. This concept applies to many other reactive metals and is fundamental to understanding oxidation reactions and metal reactivity.
🎯 Points to Remember:
- Magnesium is a reactive metal that forms a coating of \(MgO\) and \(MgCO_3\) when exposed to air
- The oxide layer acts as a protective barrier that prevents efficient combustion
- Cleaning with sandpaper removes the coating and exposes the pure metal surface
- The combustion reaction is: \(2Mg + O_2 \rightarrow 2MgO\)
- Burning magnesium produces a brilliant white flame and white ash of magnesium oxide
- This is an exothermic reaction that releases heat and light energy
- The reaction demonstrates the principle of oxidation and combination reactions
FAQ ❓
Q1: Why does magnesium ribbon need cleaning before burning?
Magnesium ribbon needs cleaning because it develops a layer of magnesium oxide (\(MgO\)) and magnesium carbonate (\(MgCO_3\)) on its surface when exposed to air. This layer prevents the ribbon from burning efficiently by acting as a barrier between the pure magnesium and oxygen in the air.
Q2: What forms on magnesium ribbon when exposed to air?
When magnesium ribbon is exposed to air, a white coating forms on its surface. This coating consists of magnesium oxide (\(MgO\)) formed by reaction with oxygen (\(O_2\)), and magnesium carbonate (\(MgCO_3\)) formed by reaction with carbon dioxide (\(CO_2\)) present in the atmosphere.
Q3: What is the chemical equation for burning magnesium in air?
The balanced chemical equation for burning magnesium in air is: \(2Mg + O_2 \rightarrow 2MgO\). This equation shows that two atoms of magnesium react with one molecule of oxygen to produce two molecules of magnesium oxide, along with the release of heat and light energy.
Q4: How do you clean magnesium ribbon before burning?
Magnesium ribbon is cleaned by rubbing it with sandpaper or steel wool. This mechanical action removes the dull white coating of oxides and carbonates, exposing the shiny metallic surface underneath. The ribbon should be cleaned just before the experiment for best results.
Q5: What happens if you burn magnesium without cleaning it?
If magnesium is burned without cleaning, the oxide layer (\(MgO\) and \(MgCO_3\)) acts as a barrier, preventing direct contact between pure magnesium and oxygen. This results in slow or incomplete combustion, reduced brightness of the flame, and less efficient energy release.
Q6: Is burning magnesium an exothermic or endothermic reaction?
Burning magnesium is an exothermic reaction because it releases a large amount of heat and light energy during the combustion process. The reaction \(2Mg + O_2 \rightarrow 2MgO + \text{Energy}\) shows that energy is produced as a product, making it exothermic.
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💬 Common Questions
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