Chemical Bonding and Molecular Structure Mock Test – Class 11 Chemistry

1. A sample of pure water contains molecules. This means that each molecule contains

2. A molecule has five electron domains around its central atom, out of which one is a lone pair. The hybridization and molecular shape are respectively

3. A graph is described below.

The graph is best used to decide hybridization by

4. A graph description is given below.

The decreasing trend is mainly due to

5. A noble-gas configuration is often used as a stability reference because noble gases generally have

6. Equal and opposite bond dipoles arranged in a straight line give a net dipole moment expected to be

7. Use the arrangement described below. Two fluorine atoms approach each other. Each fluorine atom has valence electrons and one unpaired electron available for sharing. The molecule formed is best represented as

8. For the Lewis structure of , the valence electron total is

9. In ozone, , two equivalent resonance contributors show one single bond and one double bond. The average bond order of each bond in the resonance hybrid is

10. A Lewis structure for a molecule is rejected only because one atom has fewer than electrons around it. The safest conclusion is that the rejection is

11. One common Lewis contributor of shows nitrogen with one bond and two single bonds. More than one contributor is possible because

12. For carbon-carbon bonds involving the same pair of atoms, the usual order of increasing bond length is

13. From the table below, identify the row that correctly describes molecular orbital formation.

The correct rows are

14. The molecular shapes of and are different because

15. In ethyne, , each carbon atom has

16. When changes to , the Lewis symbol of the ion is commonly written without the original valence dot because

17. For a diatomic molecule, increasing bond order usually corresponds to

18. A comparison of two bonds shows that Bond P has length and bond enthalpy , while Bond Q has length and bond enthalpy . The better conclusion is that

19. Use the passage below.

The most suitable bond between the two atoms is

20. A student writes the Lewis symbol of with dots because aluminium has electrons in more than one shell. The best correction is that Lewis symbols

21. The hybridization and approximate bond angle around each carbon in are

22. For , the usual expanded-octet Lewis description places around sulfur

23. The internally consistent description of is

24. Read the case below.

The most suitable VSEPR shape of the molecule is

25. The Kossel-Lewis approach connects chemical bonding mainly with

26. In ice, water molecules are arranged through hydrogen bonding in an open structure. This explains why ice

27. The observed dipole moment of a bond is , while the dipole moment calculated for complete ionic character is . The percentage ionic character is

28. A row in a Lewis-structure table is inconsistent. Identify it.

The inconsistent row is

29. A data note lists two lattice processes:
Case 1: ,
Case 2: ,
The value represents

30. Consider this arrangement: a central atom has six electron domains, four bond pairs, and two lone pairs. The two lone pairs occupy opposite positions in an octahedral set. The expected hybridization and molecular shape are

31. A central atom has the VSEPR type . The molecular shape is

32. Ionic compounds often dissolve better in polar solvents such as water because

33. For comparing the magnitude of lattice enthalpy, the most useful qualitative relation is

This relation suggests that lattice enthalpy magnitude increases when

34. The table below includes one incorrect hybridization-geometry link.

The row that needs correction is

35. A molecular orbital comparison gives the following data.

The row that needs correction is

36. A species has the Lewis structure with three lone pairs on oxygen. This structure best represents

37. In choosing the central atom for many simple Lewis structures, the atom usually selected is

38. Before any multiple-bond representation is considered, the skeleton of has how many sigma-type connections?

39. A molecule contains an bond and another molecule has a nitrogen atom with a lone pair. The interaction between the hydrogen of the first molecule and the lone pair of the second molecule is best described as

40. A molecule contains hydrogen, but the hydrogen is bonded to carbon rather than to , , or . The safest conclusion is that the molecule

41. Each resonance contributor has one bond and two single bonds. The average bond order in the resonance hybrid is

42. The Lewis structure for contains

43. A comparison of two possible ionic compounds is given below.

The better prediction is that

44. In hybridization, the number of hybrid orbitals formed is

45. A Lewis-structure attempt uses electrons for . The most likely error is

46. Match each molecule with the simplest shared-pair description.

The proper matching is

47. The species is predicted by simple molecular orbital theory to have bond order and no unpaired electrons. Its magnetic nature is

48. Match each bond description with the number of shared electron pairs.

The suitable matching is

49. For an oxygen atom with two lone pairs and one single bond in a Lewis structure, the formal charge is

50. A molecule or ion with resonance is usually more stable than any single contributor because