Скачать или смотреть Exercise Short Questions, Chapter 3, Chemical Bonding, Class 11 Chemistry, PECTAA, GS Academy

11th Chemistry PECTAA by Dr Khurram PhD Scholar University of Education GS Academy
   • 11th Chemistry PECTAA Exercises  

(VBT)    • 3.6 Valence Bond Theory VBT | & Molecular ...  
Timeline
SHORT ANSWER QUESTIONS
Q.2 Attempt the following short-answer questions:
00:00 a. Define the following:
(i) Dipole (ii) Bond order (iii) Permanent dipole-permanent dipole force (iv) London dispersion force
07:28 b. Draw the Lewis (electron dot) structures for the following species:
(i) HCN (ii) \text{NCl}_3 (iii) CO (iv) \text{O}_3 (v) \text{NO}_2
09:56 c. Xenon is a noble gas (group 18); xenon trioxide has the following structure:
i. By counting electron pairs around the central atom, explain why xenon trioxide has this shap e.
ii. Draw a structure of xenon trioxide showing partial charges on the atoms and the direction of the dipole moment in the molecule.
14:40 d. Explain the difference between the formation of \sigma and \pi bonds in terms of VBT.
16:44 e. The structure of propanone (acetone) is:
i. Show how the central carbon atom forms \sigma and \pi bonds through hybridization.
ii. Can propanone make a hydrogen bond with water when both are intermixed?
25:13 f. Predict the shapes of sulfate ([\text{SO}_4]^{2-}), borate ([\text{BH}_4]^-) and tri-iodide ions ([\text{I}_3]^-) according to the VSEPR model.
30:27 g. Sketch the molecular orbital pictures of \pi(2p) and \pi^*(2p).
32:28 h. Sketch the hybrid orbitals and bond formation in \text{PCl}_3, \text{SiCl}_4, and \text{NH}_4^+.
39:01 i. The structures of \text{PF}_3 and \text{SiF}_4 are given below. Redraw these with partial charges and state which is polar and which is non-polar.
41:05 j. Draw the orbital structure of the \text{CO}_2 molecule in terms of VBT.
43:34 k. Draw the Lewis structures and tell whether the following ions involve expanded octets.
i) \text{ClO}_4^- ii) \text{ICl}_4^- iii) \text{NH}_4^+ iv) \text{I}_3^-
48:14 l. The bond between K and Cl is ionic but that between Si and Cl is polar covalent. Explain why.
49:48 m. \text{SO}_2 is a polar molecule but \text{SO}_3 not. Justify.
51:22 n. Which of \text{O}_2^{2+}, and \text{O}_22- would be paramagnetic? Give reason in the light of MOT.
53:00 o. Which of the following bonds would be most polar?
i) C-Cl ii) Si-F iii) Se-F
55:00 p. Compare the bond energies of single, double, and triple bonds between the same two atoms (e.g., H-H, O=O, N≡N). Explain the trend in terms of the number of shared electrons.

Exercise Short Questions, Chapter 3, Chemical Bonding, Class 11 Chemistry, PECTAA, GS Academy, New Course