🛡️

Content Protected

Screenshots and recording are not allowed.

Click anywhere or refocus to continue

Class 10  »  Chemistry  »  Metals and Non Metals

Ionic Bond Formation - UNSOLVED PRACTICE SET

Class 10

Chapter: Metals and Non Metals | Topic: Ionic Bond Formation

Unsolved Paper
Study Material.
Class 10

IONIC BOND FORMATION - UNSOLVED PRACTICE SET

Topic: Ionic Bond Formation

Time: 40 mins | Marks: 30 | Difficulty: Medium

Multiple Choice Questions

Q1. Ionic bonds are formed by:

  1. Sharing of electrons between atoms
  2. Transfer of electrons from one atom to another
  3. Exchange of protons between atoms
  4. Mutual attraction between neutrons

Q2. Which of the following compounds is formed by ionic bonding?

  1. HCl
  2. H₂O
  3. NaCl
  4. CH₄

Q3. In the formation of sodium chloride, sodium atom:

  1. Gains one electron
  2. Loses one electron
  3. Shares one electron
  4. Gains seven electrons

Q4. The formula of magnesium chloride is:

  1. MgCl
  2. MgCl₂
  3. Mg₂Cl
  4. MgCl₃

Q5. Covalent bonds are formed by:

  1. Transfer of electrons
  2. Sharing of electrons
  3. Exchange of protons
  4. Transfer of neutrons

Q6. Which of the following is a covalent compound?

  1. Na₂O
  2. MgCl₂
  3. HCl
  4. CaF₂

Short Answer Questions

Q7. Explain the formation of ionic bond in sodium chloride (NaCl) using electron dot structures.

Q8. What is the difference between an ionic bond and a covalent bond? Give one example of each.

Q9. Your teacher explains ionic bonding using the analogy of a generous student (sodium) giving away an electron to a needy student (chlorine), and both becoming stable. Explain this analogy and why both atoms achieve stable electronic configurations.

Q10. Write the electron dot structures for the formation of: (i) MgO, (ii) CaCl₂, (iii) Na₂O.

Q11. Why do ionic compounds have high melting and boiling points? Explain in terms of the structure of ionic compounds.

Q12. Why are ionic compounds generally soluble in water but insoluble in organic solvents like kerosene? Explain.

Long Answer Questions

Q13. Explain the formation of ionic bonds with examples. Describe how sodium and chlorine atoms form sodium chloride through electron transfer. Draw electron dot structures for the formation of NaCl and MgCl₂. Why do ionic compounds conduct electricity in molten or aqueous state but not in solid state?

Q14. A student is confused about why metals and non-metals form ionic bonds while non-metals form covalent bonds with each other. Help the student by:

(a) Explaining why metals lose electrons and non-metals gain electrons.

(b) Explaining the octet rule and how it is satisfied in ionic compounds.

(c) Drawing electron dot structures for the formation of CaO and Al₂O₃.

(d) Explaining why hydrogen forms covalent bonds with chlorine but sodium forms ionic bonds with chlorine.

(e) Comparing the properties of ionic compounds (NaCl) and covalent compounds (HCl).

Q15. "Ionic and covalent bonds are the two fundamental ways atoms combine, and understanding them helps us explain the properties of the substances around us." Discuss this statement by explaining: (i) how ionic bonding explains the high melting point of table salt, (ii) how covalent bonding explains the low melting point of wax, (iii) why ionic compounds form crystals while covalent compounds often form molecules, and (iv) the role of both bond types in biological molecules like DNA and proteins.

Numerical / Application-Based Problems

Q16. A chemistry teacher explains ionic bonding using atomic numbers and electron configurations:

Table

Element Atomic Number Electron Configuration

Na 11 2, 8, 1

Mg 12 2, 8, 2

Al 13 2, 8, 3

Cl 17 2, 8, 7

O 8 2, 6

(a) Predict the ion formed by each element.

(b) Write the formula of the compound formed between: (i) Na and Cl, (ii) Mg and Cl, (iii) Al and O.

(c) Calculate the total number of electrons transferred in the formation of Al₂O₃.

(d) If sodium metal reacts with chlorine gas, and 2.3 g of sodium is used, calculate the mass of NaCl formed. (Atomic masses: Na = 23, Cl = 35.5)

(e) Draw the electron dot structure for the formation of MgCl₂.

Q17. A pharmaceutical company uses ionic compounds in medicine preparation.

(a) Sodium chloride (NaCl) is used in saline solution. If a 0.9% NaCl solution is required, calculate the mass of NaCl in 500 mL of solution. (Assume density = 1 g/mL)

(b) Calcium fluoride (CaF₂) is used in toothpaste. If a toothpaste tube contains 0.2% CaF₂, and the tube has 100 g of toothpaste, calculate the mass of CaF₂.

(c) Magnesium oxide (MgO) is used as an antacid. If a tablet contains 400 mg of MgO, calculate the number of moles. (Molar mass of MgO = 40 g/mol)

(d) Why are ionic compounds like NaCl and MgO safe for consumption while covalent compounds like HCl are dangerous in concentrated form?

(e) If the company produces 10,000 tablets per day, each containing 400 mg of MgO, calculate the annual requirement of MgO in tonnes.

Q18. In the solid state, ionic compounds do not conduct electricity, but they do conduct in molten or aqueous state.

(a) Explain why ionic compounds do not conduct electricity in solid state.

(b) Explain why they conduct in molten state.

(c) If a current of 2 A passes through molten NaCl for 30 minutes, calculate the total charge passed. (Q = I × t)

(d) If 1 mole of electrons carries 96,500 C of charge, calculate the number of moles of electrons transferred.

(e) If sodium is deposited at the cathode, calculate the mass of sodium deposited. (Atomic mass of Na = 23)

(f) Why is electrolysis of molten NaCl preferred over aqueous NaCl for producing sodium metal?


Total: 30 Marks | Time: 40 mins

Explore more topics in Metals and Non Metals

Physical Properties of Metals and Non Metals Chemical Properties of Metals Reactivity Series Occurrence of Metals in Nature Ores and Minerals Extraction of Metals Low Medium High Reactivity Refining of Metals Corrosion Causes and Prevention Alloys