Metals & Non-metals Important Questions Class 10 Science with Solution

Having adequate knowledge of metals and nonmetals is important for the students preparing for their first board exams. This chapter explains the different properties, reactions, and uses of metals and nonmetals, helping students understand both their knowledge of theory and practical experiments. By preparing with these questions, students will be well prepared for the exams and have a solid foundation in chemistry. 

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Chapter 3 Metals and Non-Metals Important Questions

1. Three pieces of a rust free iron rod are completely coated with the following:

(i) plastic

(ii) oil paint

(iii) zinc

An identical scratch is made on each piece, thus exposing the iron. The pieces of iron are kept exposed to moist air for 10 days and then checked for rust formation.

(a) State if rusting will be observed at the point of the scratch on the three iron pieces.

(b) Give reasons for your answer in each case.

(c) Name the process of applying a protective zinc coating to steel or iron.

Answer: 

(a) Rusting will be observed on the scratched areas of some of the iron pieces.

(b) (i) Plastic Coating:

Observation: Rusting will occur.

Reason: The scratch exposes the iron underneath the plastic coating. Plastic is not reactive and does not offer any galvanic protection to the exposed iron, allowing moisture and oxygen to come in direct contact with it, leading to rusting.

(ii) Oil Paint Coating:

Observation: Rusting will occur.

Reason: Similar to the plastic coating, oil paint only acts as a physical barrier. Once scratched, it exposes the iron directly to moisture and oxygen, leading to rusting at the scratch.

Zinc Coating:

Observation: Rusting will not occur.

Reason: Zinc is more reactive than iron and undergoes oxidation in preference to iron (a process called sacrificial protection). Even if the iron is exposed at the scratch, the zinc coating prevents rusting by corroding itself instead of the iron.

(c) The process of applying a protective zinc coating to steel or iron is called galvanization.

2. Listed here is the reactivity of certain metals.

From the list above, identify the metal(s) that are likely to be found in a pure state in the Earth's crust.

Answer: 

From the given table, metals that are likely to be found in a pure (native) state in the Earth's crust are those that are least reactive and do not readily react with air, water, or dilute acids.

Based on the table:

Gold (Au):

• Does not oxidize or burn in air.
• Does not react with water or dilute acids.
• Gold is chemically inert and highly unreactive, so it is often found in its pure, metallic state in the Earth's crust.

Platinum (Pt):

• No reaction with air, water, or dilute acids.
• Platinum is also highly unreactive and often found in its pure, metallic state in nature.

Conclusion:

The metals Gold (Au) and Platinum (Pt) are the ones likely to be found in a pure state in the Earth's crust.

3. The blue-coloured solution of the sulphate salt of metal W is taken in a beaker. Metal powders X, Y and Z are added one after the other to the beaker. The colour changes occurring in the solution are shown below.

State what colour change, if any, will occur if metal X is again added to the green solution in the beaker. Explain why.

Answer: 

If metal X is added again to the green solution in the beaker, the solution will turn colorless.

Explanation:

The given series of reactions involves the displacement of metals from their sulphate solutions based on the reactivity series of metals.

In this sequence:

Metal X is more reactive than metal W, as it displaces metal W from its sulphate (W-SO₄), turning the solution colorless.

Metal Y is more reactive than metal X, displacing it from the solution to form a pink solution.

Metal Z is more reactive than metal Y, displacing it to form a green solution.

When metal X is added to the green solution (which is likely to be the sulphate of metal Z, Z-SO₄), the solution turns colorless because metal X is more reactive than metal Z and displaces it from its sulphate.

This process aligns with the reactivity series of metals, where a more reactive metal always displaces a less reactive one from its compound.

4. A piece of iron rusts when it comes in contact with air and moisture. Prakash had two identical shiny iron pieces P and Q. To prevent the pieces from rusting, he coated piece P with oil paint and he galvanized piece Q with a coat of zinc metal. He noticed that the coatings were not complete and that a small part of the iron was exposed in both the pieces.

What is Prakash likely to observe about the exposed parts of the two iron pieces after some days? Explain why.

Answer: 

Prakash is likely to observe the following:

Piece P (coated with oil paint):

The exposed part of the iron piece will rust.

Reason: The oil paint acts as a barrier to air and moisture, but since the coating is incomplete, the exposed part remains in direct contact with air and moisture, leading to the formation of rust (Fe₂O₃⋅xH₂O).

Piece Q (galvanized with zinc):

The exposed part of the iron piece will not rust (or rust very slowly).

Reason: Galvanization involves coating the iron with zinc, which protects the iron even if the coating is incomplete. Zinc is more reactive than iron, so it preferentially reacts with air and moisture, undergoing oxidation to form a protective layer of zinc oxide and zinc hydroxide. This sacrificial protection prevents the iron from rusting.

5. A teacher asks her students to identify a metal, M. She gives them the following clues to help them.

(P) Its oxide reacts with both HCI and NaOH.

(Q) It does not react with hot or cold water but reacts with steam.

(R) It can be extracted by electrolysis of its ore.

(a) Identify the metal.

(b) Write the chemical equations for the reaction of the metal with HCI and NaOH respectively.

(c) What would happen if the metal is reacted with iron oxide?

Answer: 

(a) Identify the metal.

‍The metal M is aluminum (Al).
This identification is based on the following clues:

• (P): Its oxide (Al₂O₃​) is amphoteric, meaning it reacts with both acids (e.g., HCll) and bases (e.g., NaOH.
• (Q): Aluminum does not react with cold or hot water but reacts with steam, forming aluminum oxide and hydrogen gas.
• (R): Aluminum is extracted by electrolysis of its ore (bauxite) through the Hall-Héroult process.

(b) Write the chemical equations for the reaction of the metal with HCI and NaOH respectively.

‍Reaction with HCl (acid):

2Al+6HCl→2AlCl₃+3H₂↑

Aluminum reacts with hydrochloric acid to form aluminum chloride and release hydrogen gas.

Reaction with NaOH (base):
2Al+2NaOH+6H₂O→2NaAl(OH)₄+3H₂↑

Aluminum reacts with sodium hydroxide and water to form sodium aluminate and release hydrogen gas.

‍(c) What would happen if the metal is reacted with iron oxide?

‍When aluminum reacts with iron oxide (Fe₂O₃), a highly exothermic reaction known as the thermite reaction occurs. Aluminum reduces iron oxide to iron while forming aluminum oxide:2Al+Fe₂O₃→2Fe+Al₂O₃

_‍Outcome:

• Molten iron is produced.
• This reaction is used in the thermite welding process to join railway tracks or large metal components.

6. A metallic element, M, has the following properties:

- floats on water

- can be cut with a knife

- occurs naturally as its chloride, of formula MCI

- its oxide dissolves in water to form the hydroxide

(a) State the method of manufacture of the metal M. 

(b) Name the major byproduct obtained in the process.

Answer: 

(a) State the method of manufacture of the metal M. 

The metal M (sodium or potassium) is manufactured using the electrolysis of its molten chloride (e.g., sodium chloride for sodium, potassium chloride for potassium).

During the process:

• The molten chloride is electrolyzed in an electrolytic cell.
• The metal is produced at the cathode (reduction of metal ions to metal).
• Chlorine gas is released at the anode.

For sodium, the reaction is:
At cathode: Na⁺+e⁻→Na (l)
At anode: 2Cl⁻→Cl₂(g)+2e⁻

(b) Name the major byproduct obtained in the process.

The major byproduct of this process is chlorine gas (Cl₂​).

This process is highly efficient and widely used for producing sodium and other reactive metals.

7. A metal oxide on being heated with carbon does NOT produce carbon dioxide.

Give a possible explanation for this behaviour of the metal oxide.

Answer: 

If a metal oxide does not produce carbon dioxide when heated with carbon, the most likely explanation is that the metal in the metal oxide is more reactive than carbon.

• The reduction of a metal oxide by carbon depends on the reactivity of the metal relative to carbon.
• If the metal is more reactive than carbon (e.g., metals like aluminum or magnesium), carbon cannot reduce the metal oxide effectively.
• This is because the bond between the metal and oxygen in the metal oxide is stronger than the bond carbon can form with oxygen to produce carbon dioxide.
• Metals high in the reactivity series (e.g., aluminum, magnesium, calcium) have oxides that are not reduced by carbon.
• Instead, these oxides require more energy-intensive methods like electrolysis for reduction.

This behavior can be summarized using the reactivity series, where metals above carbon in the series are resistant to reduction by carbon.

8. Krunal now replaces the iron plate with a silver plate. He sees that there is no deposition of copper on the silver plate before starting the current.

Which of the following could be the reason?

a. Silver is more reactive than iron.

b. Silver is less reactive than copper.

c. Silver is a poorer conductor of electricity than iron. 

d. Silver is a better conductor of electricity than copper.

Answer: (b) Silver is less reactive than copper

Explanation: 

In an electrochemical reaction, a metal that is more reactive will displace a less reactive metal from its solution.

Iron is more reactive than copper, so copper deposits on the iron plate when used. However, silver is less reactive than copper. Therefore, silver cannot displace copper ions from the solution to form a copper deposit.

The reactivity series of metals confirms this:

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

This aligns with the observation that no deposition occurs on the silver plate before the current is applied.

9. After a few minutes, even before he turned the switch on, he noticed that copper was deposited on the iron plate.

This could have been due to

a. electrolysis

b. a combination reaction

c. electroplating

d. a displacement reaction

Answer: 

(d) a displacement reaction

Explanation:

Even before the switch was turned on, the deposition of copper on the iron plate occurred because iron is more reactive than copper in the reactivity series. When the iron plate was placed in the solution containing Cu²⁺ ions (like copper sulfate solution), a displacement reaction occurred:

Fe (s)+Cu2+(aq)→Fe²⁺(aq)+Cu 

In this reaction:

• Iron (Fe) displaced copper (Cu) from its compound because iron has a higher tendency to lose electrons and form ions compared to copper.

10. Which of the following is likely to happen when the current is started?

a. Iron will be deposited on the copper plate.

b. Copper will continue to be deposited on the iron plate.

c. No reaction will occur at the iron plate or at the copper plate.

d. The copper already deposited on the iron plate will go back into the solution.

Answer

(d) The copper already deposited on the iron plate will go back into the solution.

Explanation: 

When a current flows in an electrolytic setup involving iron and copper:

• Copper ions (Cu²⁺) in solution are reduced at the cathode to form copper metal.
• Iron atoms at the anode are oxidized to Fe²⁺, dissolving into the solution.

Iron will be deposited on the copper plate.

• Unlikely, as Fe²⁺ ions are not being introduced into the solution, and copper ions are more likely to be reduced.

Copper will continue to be deposited on the iron plate.

• This is possible only if the iron plate is acting as the cathode in the circuit, as Cu²⁺ ions are reduced to metallic copper.

No reaction will occur at the iron plate or at the copper plate.

• Unlikely, since current is flowing and redox reactions will occur at the electrodes.

The copper already deposited on the iron plate will go back into the solution.

• This will happen if the iron plate is made the anode. The deposited copper will oxidize back into Cu²⁺, entering the solution.

What are metals and nonmetals?

Metals and nonmetals are two types of elements with different properties. Metals like iron, copper, and gold are known for being malleable, ductile, and excellent conductors of electricity. Whereas nonmetals like oxygen, sulphate, and carbon are often brittle, poor conductors, and play a major role in numerous chemical processes. 

Class 10 Metals and Non-Metals provides knowledge about the chemical reactions of metals and non-metals, including how metals react with oxygen, water, acids, and bases. Important topics like corrosion, prevention methods, reactivity, and metal extraction are also included. These topics are important for understanding high-level chemistry, so it is important to know them well.

Example of Class 10 Metal and Non-Metal Important Questions

MCQs: An iron nail was suspended in solution and kept for a while. The solution is

(a) Remained blue and coating was found on the nail.

(b) turned green and a coating was formed on the nail.

(c) remained blue and no coating was formed on the nail.

(d) turned green and no coating was formed on the nail.

Very Short Answer Questions: Why does copper not liberate hydrogen on reacting with dilute sulphuric acid?

Short Answer Type Questions: An element reacts with oxygen to form an oxide, which dissolves in dilute hydrochloric acid. The oxide formed also turns a solution of red litmus blue. Is the element metal or nonmetal?  Explain with the help of a suitable example.

To score well in your Class 10 exams, it’s important to focus on the chapter on metals and nonmetals. By practicing important questions in class 10 metals and non-metals, along with solving extra questions and using additional resources like PDFs, NCERT solutions, and sample papers, you’ll make your understanding strong. 

Benefits of Class 10: Metals and Non-Metals: Important Questions

Using Class 10 metals and non-metals for important questions offers several advantages:

• These questions cover all the key topics in the chapter, making sure that you don’t miss any important concepts.
• Regular practice will help you review important topics.
• As you become familiar with various types of questions, your confidence will increase, reducing exam anxiety.
• Practicing under timed conditions helps improve your speed, which is essential in finishing the exam on time.
• With the help of metal and non-metal important questions in Class 10, students will become confident in solving each question of this chapter. 

How to use Class 10 metals and non-metals for important questions? 

Just practicing from the class 10 metals and nonmetals and using it correctly includes a little bit of difference. Here are some tips to help students use the metals and nonmetals important questions correctly:

• Before any questions, make sure you've fully understood the concepts of metals and nonmetals.
• Break down your practice into specific topics like reactivity with acids, the properties of metals and non-metals, and the extraction of metals. This will help you master each section.
• Consistent practice is essential. Aim to solve a few questions every day—at least 15 questions each day—so you don’t feel anxious about the exam.
• Solving previous year's question papers will give you an idea of the question pattern and difficulty level.
• Don’t hesitate to ask your teacher or peers if you find certain questions difficult. Group discussions often provide new ideas. 

In addition to Metals and Non-Metals Class 10 Important Questions with Answers, other resources like NCERT solutions, sample papers, and video lectures can help in your preparation. These will provide detailed explanations and ensure you cover all topics of the chapter.