Unit 2: Structure 2: Models of Bonding and Structure
Topic 2.2: The Covalent Model Questions
Practice 20 exam-style questions for IB Chemistry Topic 2.2. Review the question stems below, then unlock the full Question Bank to access markschemes, model answers, and AI grading.
1State1 mark
2026
State the shape of the molecule and its bond angle.
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2026
Draw the Lewis structure of a carbon dioxide molecule.
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Draw a diagram showing hydrogen bonding between two water molecules.
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State the number of sigma and pi bonds in one molecule of propyne, CH3-C(triple bond)CH.
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State what is meant by a coordinate (dative) covalent bond.
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State the formula used to calculate formal charge.
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Calculate the formal charge on the nitrogen atom in the nitrate ion, NO3-, drawn with one double and two single N-O bonds.
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Explain why the boiling point of water is much higher than that of hydrogen sulfide, even though both are group 16 hydrides with similar molar masses.
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Explain why the boiling points of the halogens increase from fluorine to iodine.
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Explain why ethanol is soluble in water but hexane is not.
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Using VSEPR theory, predict and explain the shape and bond angle of BF₃.
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Predict and explain the shape and bond angle of the ammonium ion, NH₄⁺.
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Predict the shape and bond angle of SO₂ and explain why it differs from CO₂.
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State the basis of VSEPR theory and explain why lone pairs are treated differently from bonding pairs.
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Define electronegativity and state the trend in electronegativity across a period and down a group.
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Explain what makes a covalent bond polar, and state which of H-Cl, Cl-Cl and O-H is the most polar.
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Explain how the difference in electronegativity between two atoms determines whether their bond is described as non-polar covalent, polar covalent or ionic.
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State whether CCl₄ contains polar bonds and whether the molecule is polar, explaining your answer.
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Explain why diamond has a very high melting point and does not conduct electricity.
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Explain why the nitrate ion is described as having resonance structures.
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