Chapter 8: Chemical Bonding — Online MCQ Test
PHYSICAL SCIENCES · CLASS 10th · Telangana State Board
Practice Chapter 8: Chemical Bonding with a free chapter-wise online MCQ test.
This chapter covers: Focusing on how atoms combine to achieve stable octet configurations this chapter examines ionic and covalent bonding mechanisms. Students learn about Lewis dot structures lattice....
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Chapter 8: Chemical Bonding — Important Questions & Answers
What is the primary condition for atoms to form chemical bonds?
- A. To achieve stable octet configuration
- B. To increase atomic mass
- C. To reduce atomic size
- D. To change color
Answer: A. To achieve stable octet configuration
Atoms form chemical bonds primarily to achieve a stable electron configuration, following the octet rule (8 electrons in the outermost shell).
Atoms form chemical bonds primarily to achieve a stable electron configuration, following the octet rule (8 electrons in the outermost shell).
Which of the following is an example of an ionic compound?
- A. H₂O
- B. CH₄
- C. NaCl
- D. NH₃
Answer: C. NaCl
NaCl is an ionic compound formed by electron transfer from Na (metal) to Cl (non-metal), resulting in Na⁺ and Cl⁻ ions held together by electrostatic attraction.
NaCl is an ionic compound formed by electron transfer from Na (metal) to Cl (non-metal), resulting in Na⁺ and Cl⁻ ions held together by electrostatic attraction.
What is lattice energy in the context of ionic compounds?
- A. Energy required to form one mole of ionic compound from gaseous ions
- B. Energy released when atoms share electrons
- C. Heat produced during melting
- D. Energy needed to break a covalent bond
Answer: A. Energy required to form one mole of ionic compound from gaseous ions
Lattice energy is the energy required to completely separate one mole of a solid ionic compound into gaseous ions, reflecting the strength of ionic bonding.
Lattice energy is the energy required to completely separate one mole of a solid ionic compound into gaseous ions, reflecting the strength of ionic bonding.
Compare the melting points of ionic compounds (like NaCl) and covalent compounds (like H₂O). Why is NaCl's melting point higher?
- A. Covalent bonds are stronger than ionic bonds
- B. NaCl has higher molecular mass
- C. Ionic compounds have very strong electrostatic attractions in the crystal lattice requiring more energy to break
- D. H₂O doesn't have a melting point
Answer: C. Ionic compounds have very strong electrostatic attractions in the crystal lattice requiring more energy to break
NaCl has a much higher melting point (~801°C) than H₂O (0°C) because the strong electrostatic forces in the ionic lattice require significantly more energy to overcome during melting.
NaCl has a much higher melting point (~801°C) than H₂O (0°C) because the strong electrostatic forces in the ionic lattice require significantly more energy to overcome during melting.
Consider three bonds: N≡N (triple bond in N₂), O=O (double bond in O₂), and F-F (single bond in F₂). Which statement correctly relates bond strength to bond parameters?
- A. All three bonds have equal strength because they connect same elements
- B. The triple bond (N≡N) is strongest, requiring most energy to break, and has the shortest bond length
- C. The single bond (F-F) is strongest due to high electronegativity of fluorine
- D. Bond strength is independent of the number of shared electron pairs
Answer: B. The triple bond (N≡N) is strongest, requiring most energy to break, and has the shortest bond length
Bond strength increases with the number of shared electron pairs: triple bonds are stronger than double bonds, which are stronger than single bonds. Shorter bonds are also stronger. N≡N (bond length ~110 pm) is significantly stronger than O=O (~121 pm) and F-F (~142 pm).
Bond strength increases with the number of shared electron pairs: triple bonds are stronger than double bonds, which are stronger than single bonds. Shorter bonds are also stronger. N≡N (bond length ~110 pm) is significantly stronger than O=O (~121 pm) and F-F (~142 pm).