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Practise Class 10 Science Chapter 3 – Metals and Non-metals with 5 original NCERT-based MCQs on ionic bond formation, electron transfer, properties of ionic compounds, metal extraction and reactivity, with detailed solutions.
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Chapter Information
Subject: Science
Class: 10
Chapter: Metals and Non-metals
Question Type: Multiple Choice Questions (MCQs)
Practice Set: 4
Difficulty Level: Moderate
Based On: NCERT Syllabus
Content Type: Original Practice Questions
Introduction
Metals and non-metals differ in the way they form chemical compounds. Many metals tend to lose electrons and form positive ions, while many non-metals gain electrons and form negative ions. The electrostatic attraction between these oppositely charged ions results in the formation of ionic compounds.
The properties of ionic compounds are closely connected to their structure. The reactivity of metals also helps determine how they can be extracted from their ores.
This Practice Set 4 focuses on electron transfer, ionic bond formation, properties of ionic compounds and the relationship between metal reactivity and extraction.
What You Will Learn
- Formation of positive and negative ions
- Electron transfer in ionic compounds
- Formation of sodium chloride
- Properties of ionic compounds
- Extraction of metals according to reactivity
- Reduction of metal oxides
- Important chemical concepts for examinations
Why This Topic Is Important
Understanding electron transfer and ionic bond formation helps students explain how metals and non-metals combine to form compounds.
The properties of ionic compounds and the extraction of metals are also important concepts in Class 10 Science. These topics help students solve conceptual MCQs and interpret chemical processes.
5 MCQs with Answers and Detailed Solutions
Q1. What happens to a sodium atom when it forms a sodium ion?
A) It gains one electron.
B) It loses one electron.
C) It gains two electrons.
D) It loses two electrons.
Answer: It loses one electron.
Detailed Solution
A sodium atom has one electron in its outermost shell. During the formation of a sodium ion, it loses this electron and forms a positively charged ion.
The process can be represented as:
$$Na \rightarrow Na^+ + e^-$$
The sodium ion has a positive charge because it contains one fewer electron than the number of protons in its nucleus.
Therefore, Option B is correct.
Exam Tip
Remember:
- Loss of electrons produces a positive ion.
- Gain of electrons produces a negative ion.
Q2. How does a chlorine atom form a chloride ion?
A) By losing one electron.
B) By losing two electrons.
C) By gaining one electron.
D) By gaining two electrons.
Answer: By gaining one electron.
Detailed Solution
A chlorine atom has seven electrons in its outermost shell. It can gain one electron to complete its outermost shell and form a chloride ion.
The process is represented as:
$$Cl + e^- \rightarrow Cl^-$$
The chloride ion has a negative charge because it has gained an additional electron.
In sodium chloride, sodium transfers an electron to chlorine. The resulting sodium and chloride ions attract each other electrostatically.
Therefore, Option C is correct.
Exam Tip
Sodium forms $$Na^+$$ by losing an electron, while chlorine forms $$Cl^-$$ by gaining an electron.
Q3. Which statement correctly explains why solid sodium chloride does not conduct electricity under ordinary conditions?
A) It contains no charged particles.
B) Its ions cannot move freely through the solid.
C) It contains only free electrons.
D) Its ions have no electrical charge.
Answer: Its ions cannot move freely through the solid.
Detailed Solution
Sodium chloride is an ionic compound made up of positively charged sodium ions and negatively charged chloride ions.
In the solid state, these ions occupy fixed positions in the crystal lattice. Because they cannot move freely, they cannot carry electric current through the solid.
When sodium chloride is molten or dissolved in water, its ions become mobile and can conduct electricity.
Therefore, Option B is correct.
Exam Tip
Ionic compounds generally conduct electricity in the molten state or in suitable aqueous solutions, but not in the solid state.
Q4. Which method is generally used to extract highly reactive metals such as sodium from their compounds?
A) Reduction with carbon.
B) Electrolysis of a suitable molten ionic compound.
C) Filtration of an aqueous solution.
D) Heating the metal in ordinary air.
Answer: Electrolysis of a suitable molten ionic compound.
Detailed Solution
Highly reactive metals, such as sodium, cannot generally be extracted from their compounds by reduction with carbon.
Instead, electrolysis of a suitable molten ionic compound is used. Electrical energy causes the metal ions to gain electrons and form metal atoms at the cathode.
For sodium ions, the reduction process can be represented as:
$$Na^+ + e^- \rightarrow Na$$
The compound must be suitable for electrolysis, and the process requires appropriate industrial conditions.
Therefore, Option B is correct.
Exam Tip
Remember the broad extraction principle:
- Highly reactive metals: Usually extracted by electrolysis.
- Moderately reactive metals: Their oxides can often be reduced using carbon or carbon monoxide.
- Less reactive metals: Some can be obtained by heating their ores, depending on the metal and the ore.
Q5. Why can carbon be used to extract zinc from zinc oxide under suitable conditions?
A) Carbon is less reactive than zinc.
B) Carbon can remove oxygen from zinc oxide.
C) Carbon converts zinc into sodium.
D) Carbon prevents zinc oxide from reacting.
Answer: Carbon can remove oxygen from zinc oxide.
Detailed Solution
Zinc is less reactive than carbon in the context of the extraction process, so carbon can reduce zinc oxide under suitable high-temperature conditions.
The reaction can be represented as:
$$ZnO + C \rightarrow Zn + CO$$
Carbon removes oxygen from zinc oxide, leaving zinc metal and forming carbon monoxide.
This process is an example of reduction of a metal oxide using carbon.
Therefore, Option B is correct.
Exam Tip
When studying metal extraction, learn how the reactivity of a metal determines the method used to obtain it from its ore.
Important Concepts
Formation of Positive Ions
Metals commonly lose electrons to form positive ions.
For example:
$$Na \rightarrow Na^+ + e^-$$
A positive ion is called a cation.
Formation of Negative Ions
Many non-metals gain electrons to form negative ions.
For example:
$$Cl + e^- \rightarrow Cl^-$$
A negative ion is called an anion.
Formation of Ionic Compounds
Ionic compounds form through the electrostatic attraction between oppositely charged ions.
For sodium chloride, sodium transfers an electron to chlorine. The resulting ions are:
$$Na^+ \quad \text{and} \quad Cl^-$$
Their electrostatic attraction produces an ionic compound.
Properties of Ionic Compounds
Ionic compounds generally have high melting and boiling points because their ions are held together by strong electrostatic forces.
They generally conduct electricity when molten or dissolved in water because their ions can move. In the solid state, the ions are fixed in position.
Extraction of Highly Reactive Metals
Highly reactive metals, such as sodium, are generally extracted by electrolysis of suitable molten compounds.
Electrical energy enables metal ions to gain electrons and form metal atoms.
Reduction of Metal Oxides
Reduction can involve the removal of oxygen from a compound.
For example:
$$ZnO + C \rightarrow Zn + CO$$
In this reaction, zinc oxide is reduced to zinc.
Related Practice Questions
Q1. What is the difference between a cation and an anion?
Q2. Write the electron-loss equation for the formation of a sodium ion.
Q3. Why do ionic compounds generally have high melting points?
Q4. Why is electrolysis used to extract highly reactive metals?
Q5. Explain how carbon can help extract zinc from zinc oxide.
Mini Quiz Challenge
Try answering these questions without looking at the answers.
Q1. Which ion is formed when a sodium atom loses one electron?
A) $$Na^-$$
B) $$Na^+$$
C) $$Na^{2+}$$
D) $$Na^{2-}$$
Q2. What happens when a chlorine atom gains one electron?
A) It forms a chloride ion.
B) It forms a sodium ion.
C) It becomes a neutral metal atom.
D) It loses its nucleus.
Q3. Which process is generally used to extract sodium from a suitable compound?
A) Filtration
B) Electrolysis
C) Sedimentation
D) Simple distillation of an aqueous solution
Q4. Which substance is used as a reducing agent in the extraction reaction below?
$$ZnO + C \rightarrow Zn + CO$$
A) Zinc oxide
B) Zinc
C) Carbon
D) Carbon monoxide
Q5. Why does molten sodium chloride conduct electricity?
A) Its ions can move freely.
B) Its ions are fixed in a solid lattice.
C) It contains no charged particles.
D) It conducts only through free metal electrons.
Exam Tips
- Practise electron-transfer equations for common ions.
- Learn the difference between cations and anions.
- Understand why ionic compounds have high melting points.
- Remember the difference between the electrical conductivity of solid and molten ionic compounds.
- Study the relationship between metal reactivity and extraction methods.
- Practise identifying the reducing agent in chemical equations.
- Check the charges of ions carefully when writing chemical formulas.
Quick Revision Notes
- Metals commonly lose electrons to form cations.
- Non-metals commonly gain electrons to form anions.
- Sodium forms $$Na^+$$ by losing one electron.
- Chlorine forms $$Cl^-$$ by gaining one electron.
- Ionic compounds are held together by electrostatic attraction between oppositely charged ions.
- Solid ionic compounds generally do not conduct electricity because their ions cannot move freely.
- Molten ionic compounds can conduct electricity because their ions are mobile.
- Highly reactive metals are generally extracted by electrolysis.
- Carbon can reduce zinc oxide under suitable conditions.
Common Mistakes Students Make
- Confusing the loss of electrons with the gain of electrons.
- Assigning a negative charge to a sodium ion.
- Assuming that solid sodium chloride conducts electricity like a metal.
- Forgetting that electrolysis requires electrical energy.
- Assuming that carbon can extract every metal from its compounds.
- Confusing oxidation with reduction.
- Writing incorrect charges when representing ions.
Key Takeaways
- Electron transfer helps explain the formation of ionic compounds.
- Metals commonly form positive ions, while non-metals commonly form negative ions.
- Ionic compounds generally have high melting points.
- Ionic compounds conduct electricity when their ions are mobile.
- The reactivity of a metal influences the method used for its extraction.
- Reduction of a metal oxide can produce the corresponding metal.
FAQs
Q. How does sodium form a positive ion?
Answer:
Sodium loses one electron and forms a positively charged sodium ion.
$$Na \rightarrow Na^+ + e^-$$
Q. How does chlorine form a chloride ion?
Answer:
Chlorine gains one electron and forms a negatively charged chloride ion.
$$Cl + e^- \rightarrow Cl^-$$
Q. Why do ionic compounds generally have high melting points?
Answer:
Strong electrostatic forces hold oppositely charged ions together. Considerable energy is required to overcome these forces sufficiently for melting.
Q. How are highly reactive metals extracted?
Answer:
Highly reactive metals such as sodium are generally extracted by electrolysis of suitable molten ionic compounds.
Q. What is the role of carbon in zinc extraction?
Answer:
Carbon acts as a reducing agent and removes oxygen from zinc oxide under suitable conditions, producing zinc.
$$ZnO + C \rightarrow Zn + CO$$
Conclusion
Class 10 Science Chapter 3 – Metals and Non-metals covers electron transfer, ionic compounds, electrical conductivity and metal extraction. These original practice questions help students understand how chemical bonding and reactivity influence the properties and preparation of metals.
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