43 practice MCQs on ionic, covalent and metallic bonds, hybridization, molecular shapes, polarity and intermolecular forces. Every question has the correct answer and an explanation.
Start free — 20 questionsChemical Bonding is part of the MDCAT Chemistry syllabus. This page collects Chemical Bonding MCQs in the style of past MDCAT papers — below are 12 of them with answers and explanations, and the full set of 43 questions is in the HighYield MDCAT QBank.
This chapter covers: ionic, covalent and metallic bonds, hybridization, molecular shapes, polarity and intermolecular forces.
Correct answer: C. Electronegativity
Electronegativity is the measure of an atom's ability, within a covalent bond, to attract the shared bonding electron pair toward itself.
Correct answer: A. 1π and 5σ bonds
In H2C=CH2 (ethene), there are 5 sigma bonds (4 C-H and 1 C-C) and 1 pi bond (part of the C=C double bond).
Correct answer: D. Catenation
Catenation is the property of carbon that allows it to form long chains and rings by bonding repeatedly with other carbon atoms.
Correct answer: D. 290 kJ mol⁻¹
The average bond energy of a C-Br bond is approximately 290 kJ/mol.
Correct answer: D. C2*H5*OH
Ethanol contains carbon, hydrogen, and oxygen atoms. The hydrogen atoms in ethanol are directly bonded to an oxygen atom. Oxygen is highly electronegative, creating a large dipole moment between the hydrogen and oxygen atoms. This polarity allows ethanol molecules to form hydrogen bonds with each other, making ethanol the correct option.
Correct answer: D. moles
The number of moles of a substance does not depend on the strength of dipole-dipole forces. The number of moles is determined by the amount of substance present, which is independent of the intermolecular forces.
Correct answer: B. The change is oxidation, because there has been a loss of electrons
In the formation of an ionic bond between magnesium and chlorine, magnesium atoms lose two electrons to achieve a stable electronic configuration. The loss of electrons is called oxidation. Magnesium has an electronic configuration of 2, 8, 2. By losing two electrons, it forms Mg2+ ions with a stable electronic configuration of 2, 8. This process involves the loss of electrons, which is characteristic of oxidation. Therefore, during the formation of an ionic bond between magnesium and chlorine, the change in magnesium atoms is oxidation because there is a loss of electrons.
Correct answer: C. 436 KJ/mol
So, the correct bond energy of hydrogen in an H2 molecule is C. 436 KJ/mol.
Correct answer: C. Geometric
Geometric isomerism, also known as cis-trans isomerism, is a form of stereoisomerism where molecules have the same molecular formula but differ in the spatial arrangement of atoms or groups around a rigid structure, such as a double bond or a ring.In the official UHS 2024 paper, option C was marked as correct. Therefore, we will retain option C here to maintain alignment with the original key for authenticity.
Correct answer: C. Amine and H2O
Option C is correct. Amines and water can form hydrogen bonds due to the presence of hydrogen atoms attached to the electronegative nitrogen in amines, which can interact with the oxygen in water. This interaction is crucial for many biological and chemical processes.In contrast, Option A (Methanal and Ethanol) cannot bond due to the lack of sufficiently electronegative hydrogen in methanal. Option B (Propane and Ethyl Methyl Ketone) involves nonpolar molecules that do not form hydrogen bonds. Lastly, Option D (Acetone and Acetaldehyde) fails to bond as neither has hydrogen directly bonded to an electronegative atom, preventing hydrogen bonding.
Correct answer: A. 1.34A°
The bond length between double-bonded carbon atoms is 1.34A°, which reflects the nature of double bonds being shorter due to increased electron density between the bonded atoms. In contrast, the other options represent lengths that are not characteristic of double bonds: 1.10A° is too short and would suggest a triple bond; 1.54A° is more aligned with a single bond; and 1.82A° is even longer, indicating a weaker single bond. Therefore, 1.34A° is the only correct answer for the bond length of double-bonded carbon.
Correct answer: D. C2H2
The bond lengths in the given molecules are:- C3H8 (propane): 1.54 Å (single bond)- C2H6 (ethane): 1.53 Å (single bond)- C2H4 (ethylene): 1.33 Å (double bond)- C2H2 (acetylene): 1.20 Å (triple bond)The shortest C-C bond length is found in acetylene (C2H2), which has a triple bond between the two carbon atoms. This is because triple bonds are shorter than double bonds, which are shorter than single bonds.
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