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Chemical Bonding and Molecular Structure EXERCISES Solutions
- Q4.1: Explain the formation of a chemical bond.
- Q4.10: Define the bond length.
- Q4.11: Explain the important aspects of resonance with reference to the $CO_3^{2-}$ ion.
- Q4.12: $H_3PO_3$ can be represented by structures 1 and 2 shown below. Can these two structures be taken as the canonical forms of the resonance hybrid representing $H_3PO_3$ ? If not, give reasons for the same.
- Q4.13: Write the resonance structures for $SO_3$, $NO_2$ and $NO_3^{-}$.
- Q4.14(a): Use Lewis symbols to show electron transfer between the following atoms to form cations and anions : (a) K and S
- Q4.14(b): Use Lewis symbols to show electron transfer between the following atoms to form cations and anions : (b) Ca and O
- Q4.14(c): Use Lewis symbols to show electron transfer between the following atoms to form cations and anions : (c) Al and N.
- Q4.15: Although both $CO_2$ and $H_2O$ are triatomic molecules, the shape of $H_2O$ molecule is bent while that of $CO_2$ is linear. Explain this on the basis of dipole moment.
- Q4.16: Write the significance/applications of dipole moment.
- Q4.17: Define electronegativity. How does it differ from electron gain enthalpy ?
- Q4.18: Explain with the help of suitable example polar covalent bond.
- Q4.19: Arrange the bonds in order of increasing ionic character in the molecules: $LiF$, $K_2O$, $N_2$, $SO_2$ and $ClF_3$.
- Q4.2: Write Lewis dot symbols for atoms of the following elements : Mg, Na, B, O, N, Br.
- Q4.20: The skeletal structure of $CH_3COOH$ as shown below is correct, but some of the bonds are shown incorrectly. Write the correct Lewis structure for acetic acid.
- Q4.21: Apart from tetrahedral geometry, another possible geometry for $CH_4$ is square planar with the four H atoms at the corners of the square and the C atom at its centre. Explain why $CH_4$ is not square planar ?
- Q4.22: Explain why $BeH_2$ molecule has a zero dipole moment although the Be–H bonds are polar.
- Q4.23: Which out of $NH_3$ and $NF_3$ has higher dipole moment and why ?
- Q4.24: What is meant by hybridisation of atomic orbitals? Describe the shapes of $sp$, $sp^2$, $sp^3$ hybrid orbitals.
- Q4.25: Describe the change in hybridisation (if any) of the Al atom in the following reaction. $AlCl_3 + Cl^{-} \rightarrow AlCl_4^{-}$
- Q4.26: Is there any change in the hybridisation of B and N atoms as a result of the following reaction?
- Q4.27: Draw diagrams showing the formation of a double bond and a triple bond between carbon atoms in $C_2H_4$ and $C_2H_2$ molecules.
- Q4.28(a): What is the total number of sigma and pi bonds in the following molecules? (a) $C_2H_2$
- Q4.28(b): What is the total number of sigma and pi bonds in the following molecules? (b) $C_2H_4$
- Q4.29: Considering x-axis as the internuclear axis which out of the following will not form a sigma bond and why? (a) $1s$ and $1s$ (b) $1s$ and $2p_x$; (c) $2p_y$ and $2p_y$ (d) $1s$ and $2s$.
- Q4.3: Write Lewis symbols for the following atoms and ions: S and $S^{2-}$; Al and $Al^{3+}$; H and $H^{-}$
- Q4.30(a): Which hybrid orbitals are used by carbon atoms in the following molecules? (a) $CH_3–CH_3$
- Q4.30(b): Which hybrid orbitals are used by carbon atoms in the following molecules? (b) $CH_3–CH=CH_2$
- Q4.30(c): Which hybrid orbitals are used by carbon atoms in the following molecules? (c) $CH_3-CH_2-OH$
- Q4.30(d): Which hybrid orbitals are used by carbon atoms in the following molecules? (d) $CH_3-CHO$
- Q4.30(e): Which hybrid orbitals are used by carbon atoms in the following molecules? (e) $CH_3COOH$
- Q4.31: What do you understand by bond pairs and lone pairs of electrons? Illustrate by giving one exmaple of each type.
- Q4.32: Distinguish between a sigma and a pi bond.
- Q4.33: Explain the formation of $H_2$ molecule on the basis of valence bond theory.
- Q4.34: Write the important conditions required for the linear combination of atomic orbitals to form molecular orbitals.
- Q4.35: Use molecular orbital theory to explain why the $Be_2$ molecule does not exist.
- Q4.36: Compare the relative stability of the following species and indicate their magnetic properties; $O_2$, $O_2^+$, $O_2^-$ (superoxide), $O_2^{2-}$ (peroxide)
- Q4.37: Write the significance of a plus and a minus sign shown in representing the orbitals.
- Q4.38: Describe the hybridisation in case of $PCl_5$. Why are the axial bonds longer as compared to equatorial bonds?
- Q4.39: Define hydrogen bond. Is it weaker or stronger than the van der Waals forces?
- Q4.4: Draw the Lewis structures for the following molecules and ions : $H_2S$, $SiCl_4$, $BeF_2$, $CO_3^{2-}$, $HCOOH$
- Q4.40: What is meant by the term bond order? Calculate the bond order of : $N_2$, $O_2$, $O_2^+$ and $O_2^-$.
- Q4.5: Define octet rule. Write its significance and limitations.
- Q4.6: Write the favourable factors for the formation of ionic bond.
- Q4.7: Discuss the shape of the following molecules using the VSEPR model: $BeCl_2$, $BCl_3$, $SiCl_4$, $AsF_5$, $H_2S$, $PH_3$
- Q4.8: Although geometries of $NH_3$ and $H_2O$ molecules are distorted tetrahedral, bond angle in water is less than that of ammonia. Discuss.
- Q4.9: How do you express the bond strength in terms of bond order ?
Chapters in CBSE - Class 11 Chemistry
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