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Lewis definition Knowledge-Based Practice

Chemistry · Acids & Bases · Chemistry · Acid–Base Concepts

5 Chemistry practice questions on Lewis definition. Questions that assess core concepts and understanding.

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Questions

  1. 1.

    Which statement correctly describes the relationship between the Brønsted–Lowry and Lewis definitions of acids and bases?

    • A) All Lewis acids are Brønsted–Lowry acids, but not all Brønsted–Lowry bases are Lewis bases.
    • B) A species must release hydroxide ions in aqueous solution to be classified as a Lewis base.
    • C) All Brønsted–Lowry bases are Lewis bases, whereas not all Lewis acids are Brønsted–Lowry acids.
    • D) The Lewis theory restricts acid–base reactions exclusively to proton-transfer processes in polar solvents.
  2. 2.

    What type of product and chemical bond are formed when a Lewis acid reacts with a Lewis base?

    • A) An ionic salt containing a bond formed by the complete transfer of an electron pair from the acid to the base
    • B) A conjugate pair containing a nonpolar covalent bond formed by equal one-electron contributions from each reactant
    • C) A hydrated complex containing an electrostatic bond formed exclusively through dipole–dipole attractions
    • D) A Lewis adduct containing a coordinate covalent bond formed by the donation of an electron pair from the base
  3. 3.

    Which of the following chemical species acts as a Lewis acid due to having an electron-deficient central atom with an incomplete octet?

    • A) H2O\text{H}_2\text{O}
    • B) NH3\text{NH}_3
    • C) AlCl3\text{AlCl}_3
    • D) F−\text{F}^-
  4. 4.

    In the reaction between boron trifluoride and ammonia (BF3+NH3→F3B-NH3\text{BF}_3 + \text{NH}_3 \rightarrow \text{F}_3\text{B-NH}_3), which statement correctly describes the role of ammonia according to the Lewis definition?

    • A) It acts as a Lewis acid because it accepts a proton.
    • B) It acts as a Lewis acid because it accepts an electron pair.
    • C) It acts as a Lewis base because it donates an electron pair.
    • D) It acts as a Lewis base because it releases a hydroxide ion.
  5. 5.

    According to the Lewis acid–base theory, which statement correctly defines a Lewis acid?

    • A) A substance that donates an unshared electron pair to form a covalent bond
    • B) A substance that accepts an electron pair to form a coordinate covalent bond
    • C) A substance that donates a proton to another chemical species in a reaction
    • D) A substance that produces hydroxide ions when dissolved in an aqueous solution

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