Chemical Bonding and Molecular Structure Mock Test – Class 11 Chemistry

1. Intramolecular hydrogen bonding means that the hydrogen bond is formed

2. Water has a bent shape because the oxygen atom has

3. A metal with low ionization enthalpy is more likely to form a simple cation because

4. The central atom in is commonly assigned

5. 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

6. A symbolic record for forming magnesium oxide is shown:


The formula of the ionic compound formed from these ions is

7. The pair of terms that describes shared and non-shared electron pairs in bonding is

8. Consider these statements about coordinate bonds.
I. The shared pair is supplied by one atom at the time of bond formation.
II. A lone-pair donor and an electron-pair acceptor are needed.
III. After formation, the coordinate bond is always weaker and visibly different from all ordinary covalent bonds in the same ion.
The valid set is

9. The first useful step in drawing a Lewis structure for a covalent molecule is usually to

10. Read the short case below.

The better prediction is that

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

12. The shape of is best predicted from the fact that sulfur has

13. The following data refer to two possible ionic formation paths with the same non-metal: Path I has , , and . Path II has , , and . The better comparison is

14. Adding one electron to to form places the electron in an antibonding molecular orbital. The expected effect is

15. A representative element belongs to Group . The number of dots in the Lewis symbol of its neutral atom is normally

16. When two atomic orbitals combine out of phase, the molecular orbital formed has

17. A neutral molecule has total valence electrons. The central atom forms three single bonds. Each terminal atom completes its octet using three lone pairs. What are the steric number, electron-pair geometry, and molecular shape around ?

18. A compound contains and ions. The formula is decided by charge balance as

19. The bond angle in a molecule is the angle between

20. The attraction in solid is mainly between

21. The bond pair in a covalent molecule means

22. If a diatomic species has electrons in bonding molecular orbitals and electrons in antibonding molecular orbitals, its bond order is

23. For , the usual Lewis structure contains how many total lone pairs?

24. Atomic orbitals combine effectively to form molecular orbitals only when they have

25. Use the passage below.

The most suitable bond between the two atoms is

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

27. Consider these statements about molecules and compounds.
I. Every compound contains atoms of at least two different elements.
II. Every molecule must contain atoms of at least two different elements.
III. is a molecule but not a compound.
The valid combination is

28. A comparison of , , and is made using molecular orbital theory. Removing one electron from antibonding orbitals to form will

29. Read the short case and answer the question.

How many more electrons must count through sharing to complete the octet?

30. A claim says, "Higher lattice enthalpy always means a compound is more covalent." The best evaluation is that the claim

31. The nitrate ion, , has three equivalent resonance contributors with one bond in each contributor. The average bond order is

32. A graph description is given below.

The species represented by this simplest diagram is most consistent with

33. For two hypothetical ionic solids, use the qualitative relation

Solid P has ions and with . Solid Q has ions and with . The approximate ratio is

34. The structural formula shows that the two carbon atoms are joined by

35. The oxygen species table below summarizes bond order and relative bond length.

The table mainly shows that

36. A diatomic species has the molecular orbital electron count shown below.

The bond order and magnetic nature of the species are

37. A carbon atom in a Lewis structure has four single bonds and no lone pair. Its formal charge is

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

This relation suggests that lattice enthalpy magnitude increases when

39. The octet rule is most useful for explaining bonding when main-group atoms tend to reach

40. The Lewis symbol of neutral sodium, , contains one dot because sodium

41. A learner says that the compound with the largest electronegativity difference will always be the most stable ionic solid. The best evaluation is that the statement is

42. The VSEPR type is non-polar when all atoms are identical because

43. In an ionic solid such as , the formula unit represents

44. A salt is more likely to form readily when the metal has low ionization enthalpy, the non-metal has favourable electron gain enthalpy, and the ionic solid has high lattice stabilization. This combination works because

45. The role of a small highly charged ion in ionic bonding is best understood through

46. Dipole moment is a measure of

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

48. The difference between and in simple molecular orbital theory is that

49. Covalent bond formation is most directly described as

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