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YOUR FOCUS Unit 2 · Compound Structure and Properties 77 MCQ questions available in this scope.
CourseAll courses AP Chemistry AP Biology AP Calculus AB AP Physics 1 AP English Language AP U.S. History AP Human Geography UnitAll units Unit 1 · Atomic Structure and Properties Unit 2 · Compound Structure and Properties Unit 3 · Properties of Substances and Mixtures Unit 4 · Chemical Reactions Unit 5 · Kinetics Unit 6 · Thermochemistry Unit 7 · Equilibrium Unit 8 · Acids and Bases Unit 9 · Thermodynamics and Electrochemistry TopicAll topics 2.1 · Types of Chemical Bonds 2.2 · Intramolecular Force and Potential Energy 2.3 · Structure of Ionic Solids 2.4 · Structure of Metals and Alloys 2.5 · Lewis Diagrams 2.6 · Resonance and Formal Charge 2.7 · VSEPR and Hybridization
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AP Chemistry · Topic 2.1: Types of Chemical Bonds Open topic Practice question Original PrepAtlas question. This is not an official College Board question.
A researcher compares four single covalent bonds: H–F, H–Cl, H–Br, and H–I. The electronegativity values of the atoms are H = 2.1, F = 4.0, Cl = 3.0, Br = 2.8, and I = 2.5. Using the qualitative electronegativity-difference model for these single bonds, which bond is predicted to have the greatest polarity? This question does not ask for a numerical dipole moment. A H–Br, because bromine has a larger atomic radius than fluorine.B H–I, because iodine has more occupied electron shells than the other halogens.C H–F, because it has the greatest electronegativity difference between the bonded atoms.D H–Cl, because chlorine has a greater nuclear charge than fluorine.
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