Chemistry · Textbook solutions

Chemical Bonding

Every solved example, exercise, and miscellaneous question — in the order the textbook teaches them. · 45 questions

5. Chemical Bonding — worked examples

4 q

Solved Examples

Worked · 4
  1. Solved Ex.5.1
    Write Lewis structure of nitrite ion NO2⊖\mathrm{NO_2^{\ominus}}.
  2. Solved Ex.5.2
    Write the Lewis structure of CO\mathrm{CO} molecule.
  3. Solved Ex.5.3
    Find out the formal charges on S, C, N. (S=C=N)⊖(\mathrm{S} = \mathrm{C} = \mathrm{N})^{\ominus} ; (S−C≡N)⊖(\mathrm{S} - \mathrm{C} \equiv \mathrm{N})^{\ominus}; (S≡C−N)⊖(\mathrm{S} \equiv \mathrm{C} - \mathrm{N})^{\ominus}
  4. Solved Ex.5.4
    Explain the formation of BeCl2\mathrm{BeCl_2}.

Exercises

41 q

1. Select and write the most appropriate alternatives from the given choices.

Practice · 6
  1. Select and write the most appropriate alternatives from the given choices.
    Ex Q.1 (A)
    Which molecule is linear?
    1. A.
      SO3\mathrm{SO_3}
    2. B.
      CO2\mathrm{CO_2}
    3. C.
      H2S\mathrm{H_2S}
    4. D.
      Cl2O\mathrm{Cl_2O}
  2. Ex Q.1 (B)
    When the following bond types are listed in decreasing order of strength (strongest first). Which is the correct order ?
    1. A.
      covalcnt > hydrogen > vander waals'
    2. B.
      covalent > vander waal's > hydrogen
    3. C.
      hydrogen > covalent > vander waal's
    4. D.
      vander waal's > hydrogen > covalent.
  3. Ex Q.1 (C)
    Valence Shell Electron Pair repulsion (VSEPR) theory is used to predict which of the following :
    1. A.
      Energy levels in an atom
    2. B.
      the shapes of molecules and ions.
    3. C.
      the electrone getivities of elements.
    4. D.
      the type of bonding in compounds.
  4. Ex Q.1 (D)
    Which of the following is true for CO2\mathrm{CO_2}?
    1. A.
      C=O\mathrm{C=O} bond : polar ; CO2\mathrm{CO_2} molecule : non-polar
    2. B.
      C=O\mathrm{C=O} bond : non-polar ; CO2\mathrm{CO_2} molecule : polar
    3. C.
      C=O\mathrm{C=O} bond : polar ; CO2\mathrm{CO_2} molecule : polar
    4. D.
      C=O\mathrm{C=O} bond : non-polar ; CO2\mathrm{CO_2} molecule : non-polar
  5. Ex Q.1 (E)
    Which O2\mathrm{O_2} molecule is pargmagnetic. It is explained on the basis of :
    1. A.
      Hybridisation
    2. B.
      VBT
    3. C.
      MOT
    4. D.
      VSEPR
  6. Ex Q.1 (F)
    The angle between two covalent bonds is minimum in:
    1. A.
      CH4\mathrm{CH_4}
    2. B.
      C2H2\mathrm{C_2H_2}
    3. C.
      NH3\mathrm{NH_3}
    4. D.
      H2O\mathrm{H_2O}

2. Draw

Practice · 4
  1. Draw
    Ex Q.2 (A)
    Lewis dot diagrams for the folowing a. Hydrogen (H2)(\mathrm{H_2}) b. Water (H2O)(\mathrm{H_2O}) c. Carbon dioxide (CO2)(\mathrm{CO_2}) d. Methane (CH4)(\mathrm{CH_4}) e. Lifthium Fluoride (LiF)(\mathrm{LiF})
  2. Ex Q.2 (B)
    Diagram for bonding in ethene with sp2sp^2 Hybridisation.
  3. Ex Q.2 (C)
    Lewis electron dot structures of a. HF\mathrm{HF} b. C2H6\mathrm{C_2H_6} c. C2H4\mathrm{C_2H_4} d. CF3Cl\mathrm{CF_3Cl} e. SO2\mathrm{SO_2}
  4. Ex Q.2 (D)
    Draw orbital diagrams of a. Fluorine molecule b. Hydrogen fluoxide molecule

3. Answer the following questions

Practice · 15
  1. Answer the following questions
    Ex Q.3 (A)
    Distinguish between sigma and pi bond.
  2. Ex Q.3 (B)
    Display electron distribution around the oxygen atom in water molecule and state shape of the molecule, also write H-O-H bond angle.
  3. Ex Q.3 (C)
    State octel rule. Explain its inadequecies with respect to a. Incomplete octel b. Expanded octel
  4. Ex Q.3 (D)
    Explain in brief with one example: a. Ionic bond b. covalend bond c. co-ordinate bond
  5. Ex Q.3 (E)
    Give reasons for need of Hybridisation
  6. Ex Q.3 (F)
    Explain geometry of methane molecule on the basis of Hybridisation.
  7. Ex Q.3 (G)
    In Ammonia molecule the bond angle is 107∘107^\circ and in water molecule it is 104∘35′104^\circ 35', although in both the central atoms are sp3sp^3 hybridized Explain
  8. Ex Q.3 (H)
    Give reasons for: a. Sigma (σ)(\sigma) bond is stronger than Pi (π)(\pi) bond. b. HF is a polar molecule c. Carbon is a tetravalent in nature.
  9. Ex Q.3 (I)
    Which type of hybridization is present in ammonia molecule? Write the geometry and bond angle present in ammonia.
  10. Ex Q.3 (J)
    Identify the type of orbital overlap present in a. H2\mathrm{H_2} b. F2\mathrm{F_2} c. H-F molecule. Explain diagramatically.
  11. Ex Q.3 (K)
    F-Be-F is a liner molecule but H-O-H is angular. Explain.
  12. Ex Q.3 (L)
    BF3\mathrm{BF_3} molecule is planar but NH3\mathrm{NH_3} pyramidal. Explain.
  13. Ex Q.3 (M)
    In case of bond formation in Acetylene molecule : a. How many covalend bonds are formed ? b. State number of sigma and pi bonds formed. c. Name the type of Hybridisation.
  14. Ex Q.3 (N)
    Define : a. Bond Enthalpy b. Bond Length
  15. Ex Q.3 (O)
    Predict the shape and bond angles in the following molecules: a. CF4\mathrm{CF_4} b. NF3\mathrm{NF_3} c. HCN\mathrm{HCN} d. H2S\mathrm{H_2S}

4. Using data from the Table, answer the following :

Practice · 4
  1. Using data from the Table, answer the following :
    ExamolesC2H6\mathrm{C_2H_6} EthaneC2H4\mathrm{C_2H_4} EtheneC2H2\mathrm{C_2H_2} Ethyne
    Structure−C−C−-\mathrm{C}-\mathrm{C}-C=C\mathrm{C}=\mathrm{C}−C≡C−-\mathrm{C} \equiv \mathrm{C}-
    Type of bond between carbonssingledoubletriple
    Bond length (nm)0.1540.1340.120
    Bond Enthalpy kJ mol−1\mathrm{kJ\ mol^{-1}}348612837
    Ex Q.4 (a)
    What happens to the bond length when unsaturation increases?
  2. Ex Q.4 (b)
    Which is the most stable compound?
  3. Ex Q.4 (c)
    Indicate the relation between bond strength and Bond enthalpy.
  4. Ex Q.4 (d)
    Comment on overall relation between Bond length, Bond Enthalpy and Bond strength and stability.

5. Complete the flow chart

Practice · 1
  1. Ex Q.5
    Complete the flow chart
    Molecular FormulaStructural FormulaShape/GeometryBond angle
    BeCl2\mathrm{BeCl_2}??180∘180^\circ
    ?O=C=O\mathrm{O}=\mathrm{C}=\mathrm{O}Linear?
    C2H2\mathrm{C_2H_2}???

7. Answer in one sentence:

Practice · 10
  1. Answer in one sentence:
    Ex Q.7 (A)
    Indicate the factor on which stalility of ionic compound is measured?
  2. Ex Q.7 (B)
    Arrange the following compounds on the basis of lattice energies in decreasing (descending) order: BeF2\mathrm{BeF_2}, AlCl3\mathrm{AlCl_3}, LiCl\mathrm{LiCl}, CaCl2\mathrm{CaCl_2}, NaCl\mathrm{NaCl}
  3. Ex Q.7 (C)
    Give the total number of electrons around sulphur (S) in SF6\mathrm{SF_6} compound.
  4. Ex Q.7 (D)
    Covalant bond is directional in nature. Justify.
  5. Ex Q.7 (E)
    What are the interacting forces present during formation of a molecule of a compound ?
  6. Ex Q.7 (F)
    Give the type of overlap by which pi (π)(\pi) bond is formed.
  7. Ex Q.7 (G)
    Mention the steps involved in Hybridization.
  8. Ex Q.7 (H)
    Write the formula to calculate bond order of molecule.
  9. Ex Q.7 (I)
    Why is O2\mathrm{O_2} molecule paramagnetic?
  10. Ex Q.7 (J)
    What do you mean by formal charge ? Explain its significance with the help of suitable example.

6. Complete the following Table

Practice · 1
  1. Ex Q.6
    Complete the following Table
    MoleculeType of HybridisationType of bondsGeometryBond angle
    CH4\mathrm{CH_4}?4C-H, 4σ4\sigma bondsTetrahedral?
    NH3\mathrm{NH_3}sp3sp^33N-H, 3σ3\sigma bonds, 1 lone pair??
    H2O\mathrm{H_2O}??angular104.5∘104.5^\circ
    BF3\mathrm{BF_3}sp2sp^2??120∘120^\circ
    C2H4\mathrm{C_2H_4}???120∘120^\circ
    BeF2\mathrm{BeF_2}?2 Be-FLinear?
    C2H2\mathrm{C_2H_2}spsp(3σ+2π)(3\sigma + 2\pi), 1C-C σ\sigma, 2C-H σ\sigma, 2C-C π\pi??