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KEAM Chemical Bonding and Molecular Structure — practice questions — page 2

Explore 97 free Chemical Bonding and Molecular Structure questions in KEAM Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Chemical Bonding and Molecular Structure questions and exercises with answers

Showing questions 31–60 of 97.

The paramagnetism of O₂ is explained by MO theory because the molecule has:Read the answer and worked solution →The bond order in N₂, O₂ and O₂²⁻ (peroxide) are respectively:Read the answer and worked solution →A hydrogen bond is formed when an H atom is covalently bonded to:Read the answer and worked solution →Which of the following is an example of *intramolecular* hydrogen bonding?Read the answer and worked solution →Isoelectronic species N₂, CO and NO⁺ all have a bond order of:Read the answer and worked solution →An ELECTROVALENT (ionic) bond is formed when:Read the answer and worked solution →A COVALENT bond is formed by:Read the answer and worked solution →The octet rule states atoms tend to:Read the answer and worked solution →VSEPR stands for:Read the answer and worked solution →The shape of methane (CH₄) is:Read the answer and worked solution →Water (H₂O) molecular shape is:Read the answer and worked solution →Bond order in N₂ molecule is:Read the answer and worked solution →Dipole moment of CO₂ is:Read the answer and worked solution →In NH₃, hybridization of N is:Read the answer and worked solution →BF₃ has shape:Read the answer and worked solution →In SF₆, central S has hybridization:Read the answer and worked solution →The order of bond strength: single < double < triple. Bond LENGTHS go in:Read the answer and worked solution →Bond angle in NH₃ compared to H₂O:Read the answer and worked solution →Molecule with linear shape (besides CO₂):Read the answer and worked solution →Number of σ and π bonds in C₂H₄ (ethene):Read the answer and worked solution →Bond order from MOT (molecular orbital theory):Read the answer and worked solution →Among NaCl, HCl, H₂O — order of bond polarity:Read the answer and worked solution →Lattice energy of an ionic crystal depends on:Read the answer and worked solution →Hybridization in PCl₅ (gaseous phosphorus pentachloride):Read the answer and worked solution →XeF₄ has shape:Read the answer and worked solution →In benzene C₆H₆, each C is:Read the answer and worked solution →Number of π bonds in HCN:Read the answer and worked solution →Among HF, HCl, HBr, HI: order of bond ENTHALPY (strength):Read the answer and worked solution →Effective nuclear charge (Z_eff) felt by an electron in 2p orbital of nitrogen, given Z = 7, screening constant σ ≈ 3.25:Read the answer and worked solution →Among NaCl, NaBr, NaI: order of melting points:Read the answer and worked solution →

Worked practice questions

The paramagnetism of O₂ is explained by MO theory because the molecule has:

  1. sp² hybridisation
  2. Two unpaired electrons in π*2p_x and π*2p_y MOs
  3. Two lone pairs on each oxygen
  4. A triple bond
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Correct answer: B. Two unpaired electrons in π*2p_x and π*2p_y MOs

O₂ MO configuration: KK(σ2s)²(σ*2s)²(σ2p_z)²(π2p_x)²(π2p_y)²(π*2p_x)¹(π*2p_y)¹. The two π* orbitals are each singly occupied → **two unpaired electrons** → paramagnetic — a triumph of MO theory over Lewis.

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The bond order in N₂, O₂ and O₂²⁻ (peroxide) are respectively:

  1. 3, 1, 1
  2. 2, 3, 1
  3. 2, 2, 2
  4. 3, 2, 1
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Correct answer: D. 3, 2, 1

N₂: 10 b, 4 a → ½(6) = **3**. O₂: 10 b, 6 a → ½(4) = **2**. O₂²⁻ adds 2 electrons to π* MOs: 10 b, 8 a → ½(2) = **1**. Bond order falls as we go N₂ → O₂ → O₂²⁻ — and bond length correspondingly grows.

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A hydrogen bond is formed when an H atom is covalently bonded to:

  1. Only metals
  2. Only carbon
  3. A highly electronegative atom — F, O or N
  4. Any non-metal
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Correct answer: C. A highly electronegative atom — F, O or N

H-bonding requires H to be attached to a *highly electronegative, small* atom — **F, O or N**. The polarised H δ⁺ then attracts the lone pair of another electronegative atom.

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