XI Chemistry Chemical Bonding Online Test Mdcat-2024

Instructions for Chapter Chemical Bonding Online Test Mdcat-2024:

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Test Details:

Subject: Chemistry
Class: 1st year or 11
Chapter name: Chemical Bonding
Test: MDCAT 2024
Book: Sindh Textbook
Total No. Of MCQS: 50
Time Allowed: 50 Minutes
Price : Free

596

Created on July 15, 2024 By

medicoengineer.com

XI Chemistry Chemical Bonding Online Test Mdcat-2024

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NameEmailPhone Number

1 / 50

1. The molecule which has maximum bond angle is

a) CS₂

b) H₂O

c) NH₃

d) BF₃

2 / 50

2. The highest bond energy in the following is

a) Cl-Cl

b) H-F

c) H-O

d) H-N

3 / 50

3. If the bond angle in AB₂ type molecule is 104.5°, its geometry should be

a) Linear

b) Pyramidal

c) Bent

d) Planar Trigonal

4 / 50

4. At the time of bond formation, Potential energy :

a) Increases

b) Decreases

c) Remains Same

d) None

5 / 50

5. X-ray analysis of diamond shows that bond length between two carbon atoms is 1.54A°, then radius of carbon will be.?

a) 0.77 × 10^-10 m

b) 7.7 × 10^-11 m

c) 0.077 Å

d) BOTH A and BD

6 / 50

6. S-Character is directly proportional to

a) Bond Angle

b) Bond Energy

c) Bond Order

d) All of these

7 / 50

7. Which of the following polar compounds have zero dipole moment?

a) CS₂

b) C0₂

c) CH₄

d) All of these

8 / 50

8. Covalent character of HCl is

a) 17%

b) 43%

c) 57%

d) 83%

9 / 50

9. Which of the following compounds show maximum ionic character

a) HCl

b) HF

c) HBr

d) CCl

10 / 50

10. Select the incorrect statement

a) Measurement of energy in bond dissociation is more accurate than the bond formation

b) Bond dissociation is endothermic process

c) The bond energy of heterodiatomic molecules is less the homodiatomic molecules

d) Bond length is experimentally determined by x-ray diffraction technique

11 / 50

11. 1Debye=?

a) 1 × 10^-18 esu.cm

b) 3.336 × 10^-30 Cm

c) 1 × 10^-10 esu.cm

d) Both A and B

12 / 50

12. S.I unit of Dipole moment is?

a) C.m

b) Debye

c) C/m

d) A and B

13 / 50

13. Which type of hybridization involves the mixing of one s orbital and two p orbitals?

a) sp hybridization

b) sp2 hybridization

c) sp3 hybridization

d) dsp3 hybridization

14 / 50

14. What is the hybridization of the carbon atom in ethylene (C₂H₄)?

a) sp

b) sp2

c) sp3

d) dsp2

15 / 50

15. Which type of hybridization occurs in a molecule with a central atom that has four single bonds?

a) sp hybridization

b) sp2 hybridization

c) sp3 hybridization

d) dsp3 hybridization

16 / 50

16. What is hybridization in chemistry?

a) The process of combining different chemical elements

b) The mixing of atomic orbitals to form new hybrid orbitals

c) The formation of ions from neutral atoms

d) The process of chemical bonding through ionic bonds

17 / 50

17. According to VSEPR theory, what determines the shape of a molecule?

a) The number of atoms in the molecule

b) The number of valence electron pairs around the central atom

c) The total number of protons in the molecule

d) The atomic masses of the elements in the molecule

18 / 50

18. What is the molecular shape of a molecule with three bonding pairs and one lone pair around the central atom?

a) Tetrahedral

b) Trigonal pyramidal

c) Trigonal planar

d) Bent

19 / 50

19. Which molecular shape is expected for a molecule with four bonding pairs and no lone pairs around the central atom?

a) Trigonal planar

b) Linear

c) Tetrahedral

d) Bent

20 / 50

20. Which of the following is not considered in active set of electrons?

a) Lone Pair

b) Bond Pair

c) Pi Bond

d) Sigma Bond

21 / 50

21. How many active set of electrons are there in CO₂?

a) 4

b) 2

c) 1

d) 3

22 / 50

22. Which of the following molecules has no unpaired electrons according to molecular orbital theory?

a) O²

b) B²

c) N²

d) C²

23 / 50

23. Which molecular orbital is filled first according to the aufbau principle?

a) Sigma 2p

b) Sigma 2s

c) Pi 2p

d) All of these

24 / 50

24. In a diatomic molecule, how many molecular orbitals can be formed from the combination of two p orbitals?

a) Two

b) Three

c) Four

d) Five

25 / 50

25. Which of the following statements is true about the molecular orbital theory's description of O₂?

a) O₂ is diamagnetic

b) O₂ is paramagnetic

c) O₂ has a bond order of 1

d) O₂ does not have any antibonding electrons

26 / 50

26. Which of the following molecules has a bond order of 3 according to molecular orbital theory?

a) O₂

b) N₂

c) F₂

d) H₂

27 / 50

27. What is the bond order of a molecule with 8 bonding electrons and 4 antibonding electrons?

a) 1

b) 2

c) 3

d) 4

28 / 50

28. Select the correct statement:

a) Valence Bond theory tells that all valence electrons are involved in the bond formation

b) According to molecular orbital theory, both the atomic orbitals possess their individual identity

c) VBT describe the idea about the bond order

d) All are incorrect

29 / 50

29. In molecular orbital theory, what is the bond order formula?

a) (Number of bonding electrons + Number of antibonding electrons) /2

b) (Number of bonding electrons - Number of antibonding electrons) / 2

c) (Number of bonding electrons - Number of antibonding electrons) / 4

d) (Number of bonding electrons + Number of antibonding electrons) / 4

30 / 50

30. Which molecular orbital is higher in energy, bonding or antibonding?A. Bonding

a) Bonding

b) Antibonding

c) Both have the same energy

d) Energy levels vary randomly

31 / 50

31. According to molecular orbital theory, what happens when atomic orbitals combine?

a) They form only bonding molecular orbitals

b) They form only antibonding molecular orbitals

c) They form both bonding and antibonding molecular orbitals

d) They do not form any new orbitals

32 / 50

32. What is the primary difference between valence bond theory and molecular orbital theory?

a) Valence bond theory uses atomic orbitals, while molecular orbital theory uses molecular orbitals

b) Valence bond theory considers electron pairs, while molecular orbital theory considers individual electrons

c) Valence bond theory applies to ionic compounds, while molecular orbital theory applies to covalent compounds

d) Valence bond theory is a qualitative approach, while molecular orbital theory is a quantitative approach

33 / 50

33. One of the main limitations of valence bond theory is its inability to explain which of the following phenomena?

a) The formation of sigma and pi bonds

b) The shapes of molecules

c) The magnetic properties of molecules

d) The concept of hybridization

34 / 50

34. Where is the electron density concentrated in a pi bond?

a) Along the internuclear axis

b) Above and below the internuclear axis

c) On the internuclear axis

d) At the center of the bond

35 / 50

35. In valence bond theory, which of the following bonds is expected to be the strongest?

a) A bond formed by the overlap of two s orbitals

b) A bond formed by the overlap of an s orbital and a p orbital

c) A bond formed by the overlap of two p orbitals

d) All of these

36 / 50

36. According to valence bond theory, which factor most significantly influences the strength of a covalent bond?

a) The number of electrons in the bond

b) The extent of orbital overlap between bonding atoms

c) The difference in electronegativity between the bonded atoms

d) The hybridization of the orbitals involved

37 / 50

37. In a molecule of ethene (C₂H₄), how many pi bonds are present?

a) 0

b) 1

c) 2

d) 4

38 / 50

38. Which orbitals can participate in the formation of a pi bond?

a) s orbitals only

b) p orbitals only

c) d orbitals only

d) s and p orbitals

39 / 50

39. Pi bonds are found in which type(s) of covalent bonds?

a) Only single bonds

b) Only double bonds

c) Double and triple bonds

d) Only triple bonds

40 / 50

40. What type of head-to-head overlapping exist in F₂ molecule

a) s-s overlapping

b) s-p overlapping

c) p-p overlapping

d) None

41 / 50

41. Ionic Character depends upon

a) difference of electronegativity

b) Polarity

c) Bond Energy

d) All of these

42 / 50

42. In a molecule of ethane (C2H6), how many sigma bonds are present?

a) 4

b) 6

c) 7

d) 8

43 / 50

43. Which orbitals can participate in the formation of a sigma bond?

a) s orbitals only

b) p orbitals only

c) d orbitals only

d) s, p, and hybrid orbitals

44 / 50

44. Sigma bonds are found in which type(s) of covalent bonds?

a) Only single bonds

b) Single and double bonds

c) Single, double, and triple bonds

d) Only triple bonds

45 / 50

45. Which of the following statements is true about sigma bonds?

a) Sigma bonds are weaker than pi bonds

b) Sigma bonds allow free rotation around the bond axis

c) Sigma bonds are formed by the sideways overlap of orbitals

d) Sigma bonds can only occur in single bonds

46 / 50

46. What is a sigma bond?

a) A bond formed by the sideways overlap of p orbitals

b) A bond formed by the end-to-end overlap of atomic orbitals

c) A bond formed by the overlap of hybrid orbitals

d) A bond formed by the overlap of d orbitals

47 / 50

47. Bond formed by the mutual sharing of electrons

a) Ionic Bond

b) Covalent Bond

c) Electrovalent Bond

d) A and C

48 / 50

48. Bond formation process is

a) Always exothermic

b) Always endothermic

c) Maybe endo or exothermic

d) None

49 / 50

49. "A covalent bond is formed due to the overlap of half filled orbital of combining atoms." This is the postulate of ?

a) Molecular Orbital Theory

b) Valence Bond Theory

c) Lewis Theory

d) All of these

50 / 50

50. What are the drawbacks of Lewis concept for covalent bond formation

a) It does not describes the nature of bonding forces

b) It does not describe the shape of molecule

c) It can describe paramagnetic behavior of molecule

d) A and B

e) All of theseAll of these

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