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CHEMICAL BONDING AND MOLECULAR STRUCTURE
Study Material
CHEMICAL BONDING AND MOLECULAR STRUCTURE
Very Short Answer Questions
Q2. Write Lewis dot structures for $\ce{S}$ and $\ce{S^{2-}}$
Q3. Write the possible resonance structures for $\ce{SO_3}$.
Q4. Predict the change if any, in hybridization of Al atom in the following reaction $\ce{AICI_3 +CI^- -> AICI^{-}_{4}}$
Q5. Which of the two ions $\ce{Ca^{2+}}$ or $\ce{Zn^{2+}}$ is more stable and why?
Q6. $\ce{Cl^-}$ ion is more stable than $\ce{Cl}$ atom Why?
Q7. Why argon does not form $\ce{Ar_2}$ molecule?
Q8. What is the best possible arrangement of four bond pairs in the valence shell of an atom to minimise repulsions?
Q9. If A and B are two different atoms when does AB molecule become Covalent?
Q10. What is meant by localized orbitals?
Q11. How many Sigma and Pi bonds are present in (a) $\ce{C_2 H_2}$ and (b)$\ce{C_2 H_4}$?
Q12. Is there any change in the hybridization of Boron and Nitrogen atoms as a result of the following reaction? $\ce{BF_3 + NH_3 -> F_3BNH_3}$
Q1. Explain Kossel-Lewis approach to Chemical bonding.
Q2. Write the general properties of Ionic Compounds.
Q3. State Fajan's rules, and give suitable examples.
Q4. What is Octet rule?. Briefly explain its significance and limitations.
Q5. Write the resonance structures for $\ce{NO_2}$, and $\ce{NO^{-}_{3}}$
Q6. Use Lewis symbols to show electron transfer between the following pairs of atoms to form cations and anions: (a)K and S (b) Ca and O (c) Al and N.
Q7. Explain why $\ce{H_2O}$ has dipole moment while $\ce{CO}$ does not have.
Q8. Define Dipole moment. Write its applications.
Q9. Explain why $\ce{BeF_2}$, molecule has zero dipole moment although the $\ce{Be-F}$ bonds are polar.
Q10. Explain the structure of $\ce{CH_4}$ molecule.
Q11. Explain Polar Covalent bond with a suitable example.
Q12. Explain the shape and bond angle in $\ce{BCI_3}$ molecule in terms of Valence Bond Theory.
Q13. What are $\ce{\sigma }$ and $\ce{ \pi }$ bonds? Specify the differences between them.
Q14. Even though nitrogen in ammonia is in sp³ hybridization, the bond angle deviate from 109°28. Explain.
Q15. Show how a double and triple bond are formed between carbon atoms in (a) $\ce{C_2H_4}$ and (b) $\ce{C_2H_4}$ respectively
Q16. Explain the hybridization involved in $\ce{PCI_5}$ molecule.
Q17. Explain the hybridization involved in $\ce{SF_6}$ molecule.
Q18. Explain the formation of Coordinate Covalent bond with one example.
Q19. Which hybrid orbitals are used by Carbon atoms in the following molecules? (a)$\ce{CH_3 - CH_3}$ (b)$\ce{CH_3 -CH=CH_2}$ (c) $\ce{CH_3 -CH_2 -OH}$ (d)$\ce{CH_3 - CHO}$
Q20. What is Hydrogen bond? Explain the different types of Hydrogen bonds with examples
Q21. Explain the formation of $\ce{H_2}$, molecule on the basis of Valence Bond theory
Q22. Using Molecular Orbital Theory explain why the $\ce{B_2}$ molecule is paramagnetic?
Q23. Write the important conditions necessary for linear combination of atomic orbitals
Q24. What is meant by the term Bond order? Calculate the bond orders in the following (a) $\ce{N_2}$ (b)$\ce{O_2}$ (c) $\ce{O^+_2}$ and (d) $\ce{O^-_2}$
Q25. Of $\ce{BF_3}$ and $\ce{NF_3}$, dipole moment is observed for $\ce{NF_3}$ and not for $\ce{BF_3}$ Why?
Q26. Eventhough both $\ce{NH_3}$and $\ce{NF_3}$ are Pyramidal,$\ce{NH_3}$ has a higher dipole moment compared to $\ce{NF_3}$ Why?
Q27. How do you predict the shapes of the following molecules making use of VSEPR Theory? (a) $\ce{XeF_4}$ (b)$\ce{BrF_5}$ (c)$\ce{CIF_5}$ and (d) $\ce{ICl^-_2}$
Q1. Explain the formation of ionic Bond with a suitable example
Q2. Explain the factors favourable for the formation of ionic Compounds
Q3. Draw Lewis Structures for the following molecules (a)$\ce{H_2S}$ (b) $\ce{SiCI_4}$ (c)$\ce{BeF_2}$(d)$\ce{HCOOH}$
Q4. Write notes on (a)BondAngle (b) Bond Enthalpy (c) Bond length and (d) Bond order
Q5. Give an account of VSEPR Theory and its applications
Q6. How do you explain the geometry of the molecules on the basis of Valence bond Theory?
Q7. What do you understand by Hybridisation? Explain different types of hybridization involving s and p orbitals
Q8. Write the sallent features of Molecular Orbital Theory
Q9. Give the Molecular Orbital Energy diagram of (a) $\ce{N_2}$ and (b)$\ce{O_2}$Calculate the respective bond order Write the magnetic nature of $\ce{N_2}$ and $\ce{O_2}$ molecules