Chemistry 1st Year Chapter 6 Chemical Bonding Notes MCQs Bank

chemistry 11th notes chapter 6

1. Valence bond theory was proposed by:


2. The geometry of [Cu(NH₃)4] 2+ should be:


3. The process in which the orbitals of different energies and shape mix with each other to give equivalent hybrid orbitals is called:


4. The shape of H₃O⁺ is:


5. Which has the minimum bond angle:


6. F₂ molecule is formed by the overlap of


7. Dipole moment gives the information about:


8. Which of the hydrogen halides has the highest percentage of ionic character:


9. Limitation of valance bond theory (VBT) is that:


10. Which one of the following has the greater ionic character in it:


11. Which of the following has a perfect triangular structure:


12. Total number of valance electrons of a nitrogen atom in an ammonium ion is


13. Which of the following has higher electron affinity:


14. An ionic compound A+B– is most likely to form when:


15. The shape of H₂O molecule is:


16. In which of the following contain co-ordinate covalent bond:


17. Which of the following molecules has zero dipole moment:


18. Which of the following solids does not contain covalent bond:


19. End to end overlapping of orbitals give rise to the formation of:


20. Which one of the following molecule have angle of 1200:


21. In a crystal, cations and anions are held together by:


22. Which of the following molecule is polar:


23. Which of the following molecule is not linear:


24. The bond order of nitrogen molecule and neon:


25. Which pair has trigonal planar geometry?


26. Which of the following elements has least electron affinity value:


27. What type of bonding is present in NH₄Cl:


28. Elements with high ionization potential values are:


29. Which of the following molecule (or molecular ion) has maximum paramagnetism:


30. The shape of SnCl₂ molecule is:


31. Ionic compounds are obtained by the combination of groups


32. Carbon atoms in acetylene (C₂H₂) are


33. In sp² hybridized orbital, the s character is_______.


34. The structure of water is:


35. Bonding affects properties like:


36. The structure of CrO-24 is:


37. The following molecules has a linear structure except?


38. Which of the following molecules has unpaired electrons in anti-bonding molecular orbitals:


39. Which of the following has maximum number of unpaired electrons:


40. In sp³ hybridized orbital, the s character is:


41. In a double bond connecting 2 atoms, there is a sharing of


42. Which of the following species has lone pair of electrons on the central atom?


43. Which of the following compounds has a non-directional bond?


44. Which of the following blocks will have comparatively higher electron affinity?


45. All the metals shine when they are freshly cut. The reason is


46. Number of electrons shared in SF₆ molecule is_______.


47. The bond order of H₂+ is:


48. Which of the following statements is not correct?


49. Which one is not the absolute term of the element:


50. Octet rule is not followed by:


51. In which of the compound, there is an electrovalent linkage:


52. Which one of the following molecule is linear:


53. Which of the following molecule has zero dipole moment:


54. One Debye is equal to:


55. Which one of the following has the maximum number of sp² carbon atoms:


56. Some covalent compounds are soluble in water because of:


57. Oxy-acids of halogens has the co-ordinate covalent bond between:


58. Side by side overlapping of orbitals gives rise to the formation of:


59. Coordinate covalent bond is present in:


60. A molecule in which the distance between two carbon atom is largest is_________.


Short Questions

1. An ionic bond is expected to be fomed between the elements of l-A and ll-A on one hand, while vl-A and vll-A on the other hand? Comment?
2. Bond distance is the compromise distance two atoms. Justify it?
3. Cationic radius is smaller than the parent atom, while anionic radius is larger than parent atom. Why?
4. Compare the radius of chloride ion with its parent atom. Give reasons?
5. Define dipole moment and gives its units?
6. Define electronagativity. How does it very in periodic Table?
7. Greater the amount of positive charged on the ion, smaller the size the size of the ion. Why?
8. How do you justify that all the bonds l.A and ll-A with vl-A and vll-A are not equally ionic?
9. How does the electronegativity difference decide the nature of ionic bond?
10. How MOT justifies that He atoms cannot make the He₂? Hellum is diamagnetic in nature, Justify?
11. How the four sp³-hybridized orbital of carbon are directed in space, to give a tetrahedral structure?
12. In the molecule of N₂, there are three bonds. One of them is sigma and the two are π. Justify it?
13. Ionization energy of the elememt is the binding energy of the nucleus and the electron. Why is it measured when the atom is in the gaseous state?
14. Most of the elements of the periodic table attain the electronic configuration of inert gases during bond formation. Justify it?
15. No bond is chemistry is 100 % ionic. Justify it?
16. On the hybridization of the carbon atom, the promotion of the electrons require the energy but hybridized carbon atom is more stable than unhybridized state. Why?
17. Solid sodium chloride does not conduct electricity, but when electric current is passed through molten sodium chloride or its aqueous solution, electrolysis takes place. Give reason?
18. The abnormality of bond length and bond strength in Hl is less prominent than that of HCI. Give reasons?
19. The dipole moment is the property of those molecules in which there is a polarity. Justify it?
20. The melting points, boiling points, heat of vaporizations and heat of sublimation of electrovalen compounds are higher as compared to those of covalent compounds. Why?
21. Throw light on the term bond order?
22. What is octet rule?
23. What is sequence of molecular orbital in nitrogen molecule? Is it diamagnetic?
24. When two oxygen atoms approach each other, they produce two bonds but one of the bonds is sigma and the other is π-bond. Justify it?
25. Why a coordinate covalent bond is produced between NH₃ and BF₃, but no such bad is produced between two similar atoms?
26. Why CO₂ and CS₂ have linear structure?
27. Why is molecule of BF₃ is triangular planar?
28. Why MOT is superior to VBT?
29. Why NH₃ and PH₃ give coordinate covalent bonds with H⁺?
30. Why positively charged ions are mostly smaller in size than their natural atoms?
31. Why second l.P. of an element is always greater than first l.P?
32. Why sigma bond is stronger than pi-bond?
33. Why the actual bonds dissociation energy of HCI ,molecule is greater than theoretical bond dissociation energy?
34. Why the atomic radii increase down the group?
35. Why the atomic size decreases from left to the right in a period? Can they be measured precisely?
36. Why the bond angles of H₂O and NH₃ like that of CH₄ although O and N-atoms are sp³- hybridized?
37. Why the bond energies of the multiple bonds are greater than those of single bonds?
38. Why the distinction between a coordinate covalent bond and a covalent bond vanishes after bond formation in NH₄ and H₃O⁺?
39. Why the electron affinities of ll-A ree less than those of l.A?
40. Why the energy of the ABMO is greater than the BMO?
41. Why the first electron affinity for most of the elements is positive?
42. Why the ionization energies decrease down the group although the nuclear charges increase?
43. Why the ionization energies of lll-a group elements are less as compared to ll-A, although the values should increase from left to the right in a period?
44. Why the lone pairs of electrons on an atom occupy greater space? Give example of NH₃?
45. Why the repulsion between the electron pair around the central atom is in the following order? Give reason?
46. π-bonds are more diffused than sigma bond. Justify it?

Long Questions

1. Define ionization energy. Give factors upon which it depends. How does it vary in periodic table?
2. What is electronegativity? Give its variation in periodic table. How does it affect the bond strength?
3. Differentiate between coovalent and coordinate covalent bonds with examples.
4. Write the postulates of VSEPR theory and discuss the structure of NH₃ with reference to this theory.
5. Explain VSEPR theory with suitable examples.
6. Explain valence bond theory with examples.
7. What is orbital hybridization? Explain the structure of CH₄ on the basis of sp³ hybridization.
8. Define atomic orbital hybridization with examples.
9. Define sp³ hybridization and on its basis explain the structure of ethene.
“10. Explain the molecular orbital structures of following molecules on the basis of the MOT
Nitrogen, Oxygen.”
11. Explain paramagneetic nature of oxygen on the basis of molecular orbital theory.
12. Describe the bonding in O₂ according to molecular orbital theoryy and explain its paramagnetic properties.
13. Define bond energy. Discuss two factors effecting the bond energy.
14. What are dipole moments? Give its SI units. How does it explain the geometry of CO₂ and BF₃ molecules.
15. Explain paramagnetic nature of O₂ molecules on the basis of MOT.
16. What is orbital hybridization? Explain sp hybridization with reference to ethyne.
17. How dipole moment can be used to decide the shapes of molecules?
“18. Predict the shapes of following molecules on the basis of VSEPR theory.
(i) NFS (ii) SO₂ (iii) PCl₅ (iv) NH₃”
19. What is octet rule?
20. Define electron affinity. How does it very in periodic table?
21. What is relationship of bond energy with ionic character of covalent bond?
22. When a second electron enters in a uninegative ion, energy is absorbed. Explain why?
23. How the bonding in the following molecules can be explained with respect to valance bond theory?
24. What is co-ordinate covalent bond? Give examples.
25. The bond length of H-Br is 1.4 X 10⁻¹⁰m. Its observed dipole moment is 0.79D. Find the percentage ionic character of the bond.

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