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Theories of Covalent Bonding and Shapes of Molecules Quiz
Test your understanding of covalent bonding, molecular shapes, and the theories that explain them.
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1. Which of the following molecules is nonpolar despite having polar bonds?
Answer: c) CO₂. CO₂ is linear, and the bond dipoles cancel each other out.
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2. According to VSEPR theory, what is the molecular geometry of BF₃?
Answer: b) Trigonal planar. Boron has 3 bonding pairs and no lone pairs.
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3. Which hybridization is associated with a tetrahedral electron geometry?
Answer: c) sp³. Four hybrid orbitals are required for a tetrahedral arrangement.
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4. Which molecule has the shortest bond length?
Answer: b) N₂. Nitrogen has a triple bond, which is shorter than double or single bonds.
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5. What is the bond angle in a molecule with a trigonal pyramidal shape?
Answer: d) <109.5°. The lone pair repels the bonding pairs, reducing the bond angle.
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6. Which of the following molecules exhibits hydrogen bonding?
Answer: c) HF. Hydrogen bonding occurs when hydrogen is bonded to highly electronegative atoms like F, O, or N.
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7. Which theory explains the formation of sigma and pi bonds?
Answer: b) Valence Bond Theory. VB theory describes the overlap of atomic orbitals to form bonds.
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8. Which molecule is linear?
Answer: b) BeCl₂. Beryllium has two bonding pairs and no lone pairs.
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9. What is the hybridization of the central atom in SF₆?
Answer: c) sp³d². Six hybrid orbitals are needed for an octahedral shape.
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10. Which of the following has the highest bond energy?
Answer: c) Triple Bond. Triple bonds involve greater electron density between the atoms, leading to stronger attraction.
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11. Which molecule has a dipole moment of zero?
Answer: c) CCl₄. The symmetrical tetrahedral shape causes the bond dipoles to cancel.
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12. The concept of resonance is best described by:
Answer: b) Lewis structures. Resonance involves multiple valid Lewis structures for a molecule.
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13. Which molecule has a bent shape?
Answer: c) H₂O. Oxygen has two bonding pairs and two lone pairs.
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14. What is the bond order of O₂ according to Molecular Orbital Theory?
Answer: b) 2. O₂ has 12 electrons filling bonding and antibonding molecular orbitals.
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15. What is the shape of a molecule with sp³d hybridization and one lone pair?
sp³d hybridization means the molecule has 5 regions (bonds or lone pairs) around the central atom. With 1 lone pair, the remaining 4 bonds form a shape like a "see-saw" because the lone pair pushes the bonds into this arrangement.
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16. Which of the following is paramagnetic?
Answer: b) O₂. Oxygen has unpaired electrons in its molecular orbitals.
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17. Which of the following molecules has the largest bond angle?
Answer: d) BF₃. BF₃ is trigonal planar with 120° bond angles.
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18. Which of the following is an exception to the octet rule?
Answer: c) BF₃. Boron only has 6 electrons around it.
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19. Which theory explains the delocalization of electrons?
Answer: c) Molecular Orbital Theory. MO theory describes electrons as being spread over the entire molecule.
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20. Which molecule has a trigonal bipyramidal shape?
Answer: c) PCl₅. Phosphorus has 5 bonding pairs and no lone pairs.
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21. What is the molecular geometry of XeF₄?
Answer: b) Square planar. Xenon has 4 bonding pairs and 2 lone pairs.
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22. Which hybridization is associated with a linear electron geometry?
Answer: a) sp. Two hybrid orbitals are required for a linear arrangement.
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23. Which of the following molecules does not exhibit hydrogen bonding in its pure liquid state?
Answer: d) HCl. Hydrogen bonding requires hydrogen bonded to F, O, or N.
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24. What is the shape of a molecule with sp³d² hybridization and two lone pairs?
Answer: b) Square planar. The lone pairs are trans to each other.
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25. Which molecule has the longest bond length among the following?
Answer: d) I₂. Bond length increases down the halogen group.
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26. Which molecule has the highest bond order?
Answer: a) O₂. O₂ has a bond order of 2. B2 has a bond order of 1, H2 has a bond order of 1 and He2 has a bond order of 0.
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27. What is the hybridization of the central atom in XeF₂?
Answer: b) sp³d. Xenon has 2 bonding pairs and 3 lone pairs.
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28. Which molecule has a T-shaped geometry?
Answer: a) BrF₃. Bromine has 3 bonding pairs and 2 lone pairs.
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29. Which of the following is an example of a molecule with an expanded octet?
Answer: c) SF₆. Sulfur has 12 electrons around it.
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30. The strength of a covalent bond is directly related to:
Answer: b) Bond order. Higher bond order means stronger bonds.
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31. Which of the following has the weakest bond?
Answer: c) F-F. Fluorine has a small atomic radius and high electron-electron repulsion.
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32. What is the bond order of He₂⁺?
Answer: b) 0.5. There are 3 electrons in bonding and antibonding orbitals so (2-1)/2=0.5
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33. Which of these molecules has the largest dipole moment?
Answer: c) CHCl₃. Because of the difference in electronegativity between H and Cl and the asymmetrical shape of the molecule.
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34. Which intermolecular force is the strongest?
Ion-Dipole Interactions: Strongest, occur between ions and polar molecules. The full charge of the ion interacts strongly with the partial charges of the dipole, making this the strongest intermolecular force.
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35. What is the molecular geometry of a molecule with sp³d hybridization and two lone pairs?
Answer: a) T-shaped. The lone pairs occupy equatorial positions, resulting in a T-shape.
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36. Which molecule has the weakest bond?
Answer: c) F₂. Due to small size and high electron-electron repulsion.
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37. Which of the following species has the highest bond order?
Answer: a) O₂⁺. O₂⁺ has a bond order of 2.5, O₂ has 2, O₂⁻ has 1.5, and O₂²⁻ has 1.
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38. Which of the following is an example of a molecule that violates the octet rule by having fewer than eight electrons around the central atom?
Answer: c) BeCl₂. Beryllium has only four electrons around it.
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39. Bond enthalpy is a measure of:
Answer: b) Bond strength. It is the energy required to break a bond.
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40. Which intermolecular force is present in all molecules?
Answer: c) London Dispersion Forces. These forces arise from temporary fluctuations in electron distribution.
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41. Which of the following is a correct representation of resonance?
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