MDCAT Chemical Bonding MCQs

This comprehensive set of MCQs on Chemical Bonding is designed to cover all essential topics required for success in the Medical and Dental College Admission Test (MDCAT). Focused on key concepts such as ionic, covalent, and metallic bonding, molecular geometry, and hybridization, these MCQs aim to help students build a strong understanding of chemical bonding and its relevance in both chemistry and biological sciences.

Who should practice Chemical Bonding MCQs?

Students preparing for the MDCAT who want to deepen their understanding of the different types of chemical bonds and how they influence molecular properties.
Individuals seeking to enhance their knowledge of important topics like Lewis structures, bond polarity, and bond energy, which are crucial for various medical and dental disciplines.
University students targeting high-yield topics such as molecular orbital theory, resonance, and the VSEPR model.
Anyone aiming to strengthen their understanding of how chemical bonding impacts biological systems, drug interactions, and biochemical reactions.
Candidates focused on developing critical thinking and problem-solving skills related to chemical bonding and molecular interactions.
Suitable for all students preparing for the MDCAT, including those looking to boost their confidence in tackling bonding-related questions in chemistry.

1. Which of the following represents the energy required to break a bond between two atoms?

A) Ionization energy
B) Electron affinity
C) Bond energy
D) Electronegativity

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2. What happens to the atomic size across a period from left to right?

A) Increases
B) Decreases
C) Remains constant
D) Increases and then decreases

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3. Which bond involves the complete transfer of electrons from one atom to another?

A) Covalent bond
B) Ionic bond
C) Sigma bond
D) Pi bond

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4. Which of the following elements has the highest electronegativity?

A) Fluorine
B) Oxygen
C) Nitrogen
D) Chlorine

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5. What type of bond is formed when two atoms share one pair of electrons?

A) Double bond
B) Single bond
C) Ionic bond
D) Triple bond

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6. Which factor decreases the bond length between two atoms?

A) Higher bond energy
B) Higher electronegativity
C) Larger atomic radii
D) Larger ionic radii

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7. What is the bond angle in a molecule with sp2 hybridization?

A) 109.5°
B) 120°
C) 180°
D) 90°

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8. Which of the following bonds has the highest bond energy?

A) C-C single bond
B) C=C double bond
C) C≡C triple bond
D) H-H single bond

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9. What happens to ionization energy as you move down a group in the periodic table?

A) Increases
B) Decreases
C) Remains constant
D) Decreases and then increases

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10. Which of the following has the smallest ionic radius?

A) Na⁺
B) K⁺
C) Mg²⁺
D) Ca²⁺

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11. What type of bond is present in the oxygen molecule (O₂)?

A) Ionic bond
B) Sigma bond
C) Pi bond
D) Both sigma and pi bonds

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12. In VSEPR theory, the shape of a molecule with two bonding pairs and two lone pairs of electrons is:

A) Linear
B) Trigonal planar
C) Tetrahedral
D) Bent

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13. Which of the following best describes a coordinate covalent bond?

A) Both atoms share electrons equally
B) One atom donates both electrons in the bond
C) Electrons are transferred from one atom to another
D) A triple bond is formed

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14. Which of the following molecules is sp3 hybridized?

A) CO₂
B) CH₄
C) C₂H₄
D) C₂H₂

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15. Which of the following factors increases the bond energy?

A) Decrease in bond length
B) Increase in atomic size
C) Decrease in electronegativity
D) Increase in ionic radius

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16. How many sigma bonds are present in an ethene (C₂H₄) molecule?

A) 1
B) 2
C) 4
D) 5

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17. Which of the following has the lowest electronegativity?

A) Carbon
B) Oxygen
C) Sodium
D) Nitrogen

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18. Which molecule has a bond angle of 180°?

A) CH₄
B) CO₂
C) NH₃
D) H₂O

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19. What is the shape of a molecule with sp hybridization?

A) Tetrahedral
B) Trigonal planar
C) Linear
D) Bent

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20. Which bond is stronger, sigma or pi?

A) Sigma bond
B) Pi bond
C) Both are equal
D) Depends on the molecule

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21. Which atom has the highest ionization energy?

A) Fluorine
B) Oxygen
C) Helium
D) Hydrogen

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22. The molecule with the highest ionic character is:

A) H₂O
B) CO₂
C) NaCl
D) NH₃

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23. Which of the following molecules has sp2 hybridization?

A) CH₄
B) C₂H₂
C) C₂H₄
D) CO₂

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24. The bond angle in methane (CH₄) is:

A) 90°
B) 109.5°
C) 120°
D) 180°

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25. Which of the following bonds is considered purely covalent?

A) HCl
B) O₂
C) NaCl
D) H₂O

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26. How many pi bonds are present in a nitrogen molecule (N₂)?

A) 0
B) 1
C) 2
D) 3

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27. The formation of which bond releases the most energy?

A) Covalent bond
B) Ionic bond
C) Metallic bond
D) Van der Waals bond

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28. The atomic radius decreases across a period due to:

A) Decrease in nuclear charge
B) Increase in nuclear charge
C) Increase in electron shielding
D) Decrease in ionization energy

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29. Which molecule has a trigonal planar geometry?

A) NH₃
B) H₂O
C) BF₃
D) CH₄

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30. A covalent bond is most likely to form between:

A) Two metals
B) A metal and a non-metal
C) Two non-metals
D) An alkali metal and a halogen

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31. Which of the following bonds is the shortest?

A) C-C
B) C=C
C) C≡C
D) C-H

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32. In which type of hybridization do atomic orbitals form four equivalent sp3 orbitals?

A) sp hybridization
B) sp2 hybridization
C) sp3 hybridization
D) d2sp3 hybridization

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33. What is the bond angle in a molecule with sp hybridization?

A) 90°
B) 120°
C) 180°
D) 109.5°

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34. Which molecule is linear in shape due to sp hybridization?

A) H₂O
B) NH₃
C) CO₂
D) CH₄

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35. The bond formed between two atoms where both electrons come from the same atom is called:

A) Ionic bond
B) Covalent bond
C) Coordinate covalent bond
D) Hydrogen bond

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36. Which of the following represents a pair of atoms with the largest difference in electronegativity?

A) Na and Cl
B) H and O
C) C and N
D) K and Br

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37. In VSEPR theory, the shape of a molecule with three bonding pairs and no lone pairs is:

A) Linear
B) Trigonal planar
C) Tetrahedral
D) Bent

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38. Which element has the highest electron affinity?

A) Oxygen
B) Fluorine
C) Chlorine
D) Nitrogen

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39. How many sigma bonds are present in ethyne (C₂H₂)?

A) 1
B) 2
C) 3
D) 4

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40. The bond formed between H and O in a water molecule is:

A) Ionic bond
B) Covalent bond
C) Coordinate bond
D) Metallic bond

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41. Which molecule has sp3 hybridization and a bond angle of 109.5°?

A) BF₃
B) CH₄
C) CO₂
D) C₂H₄

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42. In which molecule is the central atom sp2 hybridized?

A) CH₄
B) H₂O
C) BCl₃
D) C₂H₂

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43. Which of the following molecules has the greatest ionic character?

A) HCl
B) NaF
C) HF
D) NH₃

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44. The energy required to remove the outermost electron from a neutral atom is called:

A) Electron affinity
B) Ionization energy
C) Bond energy
D) Electronegativity

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45. Which molecule has a pyramidal shape according to VSEPR theory?

A) CH₄
B) NH₃
C) H₂O
D) CO₂

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46. What type of bond exists between two nitrogen atoms in an N₂ molecule?

A) Single bond
B) Double bond
C) Triple bond
D) No bond

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47. Which of the following molecules has the highest bond energy?

A) H₂
B) O₂
C) N₂
D) F₂

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48. Which bond is formed by head-to-head overlap of atomic orbitals?

A) Pi bond
B) Sigma bond
C) Ionic bond
D) Dative bond

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49. What is the hybridization of carbon in ethene (C₂H₄)?

A) sp
B) sp2
C) sp3
D) dsp3

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50. Which molecule is planar due to sp2 hybridization?

A) CH₄
B) NH₃
C) BF₃
D) H₂O

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51. What is the shape of CO₂ according to VSEPR theory?

A) Linear
B) Bent
C) Trigonal planar
D) Tetrahedral

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52. Which bond has the least ionic character?

A) HCl
B) NaCl
C) HF
D) CCl₄

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53. Which molecule has only one pi bond?

A) Ethyne
B) Ethene
C) Methane
D) Water

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54. The atomic radius of an atom increases when:

A) Moving across a period
B) Moving down a group
C) Electrons are removed
D) The bond energy increases

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55. Which hybridization results in a molecule with 180° bond angles?

A) sp
B) sp2
C) sp3
D) dsp2

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56. In VSEPR theory, what is the predicted shape of a molecule with two bonding pairs and no lone pairs?

A) Linear
B) Bent
C) Tetrahedral
D) Trigonal planar

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57. What is the bond angle in a molecule of ammonia (NH₃)?

A) 180°
B) 120°
C) 107°
D) 90°

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58. Which element has the lowest electronegativity?

A) Fluorine
B) Oxygen
C) Sodium
D) Chlorine

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59. How many sigma bonds and pi bonds are present in a molecule of carbon dioxide (CO₂)?

A) 1 sigma bond and 2 pi bonds
B) 2 sigma bonds and 2 pi bonds
C) 1 sigma bond and 1 pi bond
D) 2 sigma bonds and 1 pi bond

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60. Which bond is present in an ionic compound?

A) Sigma bond
B) Covalent bond
C) Ionic bond
D) Pi bond

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61. Which of the following elements has the smallest atomic radius?

A) Sodium
B) Fluorine
C) Oxygen
D) Nitrogen

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62. What type of bond is present between the carbon atoms in ethyne (C₂H₂)?

A) Single bond
B) Double bond
C) Triple bond
D) No bond

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63. The shape of BF₃ can be explained using which type of hybridization?

A) sp
B) sp2
C) sp3
D) dsp3

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64. Which molecule contains both sigma and pi bonds?

A) Methane (CH₄)
B) Ethene (C₂H₄)
C) Ammonia (NH₃)
D) Water (H₂O)

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65. Which bond in H₂O has the highest ionic character?

A) H-H bond
B) O-H bond
C) O-O bond
D) H-O-H bond

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66. Which of the following has the smallest bond angle?

A) CH₄
B) NH₃
C) H₂O
D) CO₂

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67. What is the shape of a PCl₅ molecule according to VSEPR theory?

A) Trigonal planar
B) Tetrahedral
C) Trigonal bipyramidal
D) Octahedral

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68. Which of the following molecules is non-polar?

A) HCl
B) NH₃
C) CO₂
D) H₂O

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69. Which molecule is predicted to have a tetrahedral shape?

A) BCl₃
B) NH₄⁺
C) CO₂
D) NO₃⁻

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70. How many bonding pairs and lone pairs of electrons are in a water molecule?

A) 2 bonding pairs, 0 lone pairs
B) 2 bonding pairs, 2 lone pairs
C) 3 bonding pairs, 1 lone pair
D) 4 bonding pairs, 0 lone pairs

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71. Which molecule contains a coordinate covalent bond?

A) H₂O
B) NH₄⁺
C) CH₄
D) HCl

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72. Which molecule has the highest bond angle?

A) NH₃
B) CH₄
C) H₂O
D) CCl₄

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73. The bond between Na⁺ and Cl⁻ in NaCl is:

A) Covalent
B) Ionic
C) Coordinate
D) Metallic

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74. What is the hybridization of carbon atoms in diamond?

A) sp
B) sp2
C) sp3
D) dsp3

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75. Which molecule contains both sp2 and sp hybridized atoms?

A) C₂H₆
B) C₂H₂
C) C₂H₄
D) CH₃Cl

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76. The number of lone pairs on the central atom of ammonia (NH₃) is:

A) 0
B) 1
C) 2
D) 3

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77. In the case of an ionic bond, which type of elements generally forms positive ions?

A) Metals
B) Non-metals
C) Metalloids
D) Noble gases

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78. Which of the following represents a molecule with both ionic and covalent bonds?

A) NaCl
B) NH₃
C) H₂O
D) NaOH

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79. Which of the following factors affects the polarity of a bond?

A) Bond energy
B) Bond length
C) Electronegativity difference
D) Atomic size

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80. What type of bonds hold together the atoms in metallic substances?

A) Covalent bonds
B) Ionic bonds
C) Metallic bonds
D) Van der Waals bonds

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81. What type of hybridization occurs in carbon dioxide (CO₂)?

A) sp
B) sp2
C) sp3
D) dsp3

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82. Which of the following statements is true regarding bond length?

A) It increases as bond energy increases
B) It increases with increasing bond order
C) It is shorter for triple bonds than single bonds
D) It is shorter for bonds between larger atoms

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83. The shape of an SF₆ molecule is:

A) Tetrahedral
B) Trigonal planar
C) Octahedral
D) Trigonal bipyramidal

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84. Which molecule has sp3 hybridization and two lone pairs?

A) H₂O
B) NH₃
C) CH₄
D) BF₃

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85. The hybridization of the central atom in NH₃ is:

A) sp
B) sp2
C) sp3
D) dsp3

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86. Which of the following represents a molecule with a double bond?

A) CO₂
B) NH₃
C) H₂O
D) CCl₄

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87. What is the bond angle in an sp hybridized molecule?

A) 90°
B) 109.5°
C) 120°
D) 180°

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88. How many sigma and pi bonds are in acetylene (C₂H₂)?

A) 2 sigma, 1 pi
B) 3 sigma, 1 pi
C) 2 sigma, 2 pi
D) 1 sigma, 2 pi

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89. In which of the following molecules are all bonds single?

A) CO₂
B) O₂
C) CH₄
D) C₂H₄

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90. Which of the following best explains why metals conduct electricity?

A) They have covalent bonds
B) They have free-moving electrons
C) They have strong ionic bonds
D) They have a rigid crystal lattice

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91. The electron pair geometry of water (H₂O) is:

A) Tetrahedral
B) Trigonal planar
C) Bent
D) Linear

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92. Which of the following has the highest bond dissociation energy?

A) H₂
B) F₂
C) N₂
D) O₂

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93. The bond formed by side-to-side overlap of p orbitals is called a:

A) Sigma bond
B) Pi bond
C) Ionic bond
D) Metallic bond

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94. Which molecule contains a triple bond?

A) H₂O
B) O₂
C) C₂H₂
D) CH₄

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95. In which of the following molecules does the central atom have sp2 hybridization?

A) CH₄
B) H₂O
C) BF₃
D) C₂H₂

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96. How many lone pairs are there on the oxygen atom in a water molecule?

A) 1
B) 2
C) 3
D) 0

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97. Which of the following elements has the largest ionic radius?

A) Na⁺
B) K⁺
C) Mg²⁺
D) Ca²⁺

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98. What is the geometry of ammonia (NH₃) according to VSEPR theory?

A) Tetrahedral
B) Trigonal planar
C) Trigonal pyramidal
D) Linear

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99. The hybridization of the central atom in BeCl₂ is:

A) sp
B) sp2
C) sp3
D) dsp3

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100. Which type of bond is formed between hydrogen and fluorine in HF?

A) Covalent
B) Ionic
C) Coordinate covalent
D) Metallic

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