Free Chemical Bonding MCQs with Answers
964 Chemical Bonding MCQs from Chemistry, each with the correct answer and a written explanation of why it is correct. Free and unlimited, with no account needed.
Chemical bonding explains molecular shape through VSEPR theory and distinguishes sigma bonds from pi bonds. Questions involve hybridization, bond angles, dipole moment and bond energy, including how electron-pair repulsion determines geometry and how bond polarity differs from the overall polarity of a molecule.
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Read the Chemical Bonding notesFree MDCAT chapter notes with key terms964 questions · page 36 of 49
- A. Bond strength
- B. Bond length
- C. Dipole moment
- D. Shape
Explanation: The polarity of a molecule is expressed in terms of its dipole moment. The dipole moment is a measure of the overall electrical charge…
Correct answer: Dipole moment- A. Ionic bond
- B. Polar bond
- C. Covalent bond
- D. Coordinate covalent bond
Explanation: The bonding in MgO is an example of ionic bonding. This is because the difference in electronegativity between magnesium and oxygen is…
Correct answer: Ionic bond- A. sp, sp2, sp3
- B. sp2, sp, sp3
- C. sp, sp3, sp2
- D. sp2, sp3, sp
Explanation: The hybridization of atomic orbitals of central atoms in CO2, BF3, and NH4+ are sp, sp2, and sp3, respectively.
Correct answer: sp, sp2, sp3- A. sp2-s
- B. sp-s
- C. p-p
- D. sp3-s
Explanation: The O-H bonds in H2O molecule are formed by overlapping sp3-s orbitals.
Correct answer: sp3-s- A. 90o
- B. 104.5o
- C. 92o
- D. 105.5o
Explanation: The bond angle of H2S is 92.1 degrees. This is because the sulfur atom is sp3 hybridized, and the three H-S bonds are arranged in a…
Correct answer: 92o- A. M+>M++>M+++
- B. M++>M+++>M+
- C. M+++>M++>M+
- D. M++>M+>M+++
Explanation: This is because it takes more energy to remove an electron from an atom that already has a positive charge.
Correct answer: M+++>M++>M+- A. Ionization energy
- B. Electronegativity
- C. Electron affinity
- D. Atomic size
Explanation: Electronegativity is not an absolute term for an element. Electronegativity is a relative measure of an element's ability to attract…
Correct answer: Electronegativity- A. SO3
- B. SnCl2
- C. CO2
- D. BF3
Explanation: In SnCl2, both the Sn-Cl bonds are angular with each other. Thus, the dipole moment of one Sn-Cl bond cannot be cancelled by each other…
Correct answer: SnCl2- A. HF
- B. CsCl
- C. NaCl
- D. H2O
Explanation: CsCl is the most ionic compound out of the four listed. The other three compounds, HF, NaCl, and H2O, are all polar covalent compounds.The…
Correct answer: CsCl- A. The ionization energy of A is high and the electron affinity of B is super high
- B. The ionization energy of Ais high and the electron affinity of B is low.
- C. The ionization energy of A and the electron affinity of B is high.
- D. The ionization energy of A and the electron affinity of B is low.
Explanation: An ionic bond A+B- is most likely to be formed when the ionization energy of A is low and the electron affinity of B is high.beacause A…
Correct answer: The ionization energy of Ais high and the electron affinity of B is low.- A. Sugar, C12H22OI l(s)
- B. Graphite C(s)
- C. Carbon dioxide CO2(s)
- D. Magnesium Fluoride, MgF2(s)
Explanation: Ionic solids are formed when positively charged ions (cations) and negatively charged ions (anions) are attracted to each other.
Correct answer: Magnesium Fluoride, MgF2(s)- A. pie-bond is formed from sp hybrid orbitals.
- B. pie-bond is formed by the parallel overlap of p-orbitals.
- C. pie-bond is formed when as sigma bond is already present.
- D. pie-bond is weaker than sigma bond.
Explanation: The statement that "pie-bond is formed from sp hybrid orbitals" is not true.
Correct answer: pie-bond is formed from sp hybrid orbitals.- A. 90o
- B. 109.5o
- C. 180o
- D. 104.5o
Explanation: The bond angle in H2O is 104.5 due to presence of two lone pair of electrons.This fact can be explained by the help of VSEPR.
Correct answer: 104.5o- A. NH3
- B. H2O
- C. BF3
- D. CH3OH
Explanation: This is true because octet of B is not complete in BF3. they accept a pair of electrons from a donor and form a coordinate covalent bond.
Correct answer: BF3- A. HCl
- B. H2O
- C. CO2
- D. SO2
Explanation: Carbon dioxide: CO2 has polar bonds but is a nonpolar molecule. The structure of CO2 is linear.
Correct answer: CO2- A. Decreases.
- B. Increases.
- C. Becomes zero.
- D. Does not change.
Explanation: The correct answer is that the bond angle decreases. Hybrid orbitals with higher 's' character (e.g., sp) have larger bond angles (180°)…
Correct answer: Decreases.- A. Benzene.
- B. Phosphorus trichloride.
- C. Ethene.
- D. Boron trifluoride.
Explanation: The correct answer is Phosphorus trichloride (PCl3) because it has a trigonal pyramidal geometry, which results from the lone pair on the…
Correct answer: Phosphorus trichloride.718. Liquid oxygen is:
- A. Diamagnetic.
- B. Paramagnetic.
- C. Antimagnetic.
- D. Ferromagnetic.
Explanation: Liquid oxygen is paramagnetic because it contains unpaired electrons, which cause it to be attracted to a magnetic field.
Correct answer: Paramagnetic.- A. 1
- B. 2
- C. 3
- D. 4
Explanation: In a carbon dioxide (CO2) molecule, the carbon atom forms two double bonds, one with each oxygen atom.
Correct answer: 2- A. H2S molecule is linear, while BeF2 is angular.
- B. H2S molecule is angular, while BeF2 molecule is linear.
- C. Fluorine has more electronegativity.
- D. Be is more electronegative than S.
Explanation: The molecular geometry determines the net dipole moment of a molecule. H2S has a bent shape due to the presence of lone pairs on the…
Correct answer: H2S molecule is angular, while BeF2 molecule is linear.