Classify each species as either a Lewis acid or a Lewis base. a. Fe³⁺ b. BH₃ c. NH₃ d. F^-

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Understand the definition of Lewis acids and bases: A Lewis acid is a species that can accept an electron pair, while a Lewis base is a species that can donate an electron pair.

Analyze Fe^{3+}: It is a metal cation with a positive charge, which means it can accept electron pairs, classifying it as a Lewis acid.

Examine BH_3: Boron in BH_3 has an incomplete octet and can accept an electron pair, making it a Lewis acid.

Consider NH_3: Ammonia has a lone pair of electrons on the nitrogen atom, which it can donate, classifying it as a Lewis base.

Evaluate F^-: The fluoride ion has extra electrons and can donate an electron pair, making it a Lewis base.

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Lewis Acids and Bases

Lewis acids are species that can accept an electron pair, while Lewis bases are species that can donate an electron pair. This definition expands the concept of acids and bases beyond protons (H+) to include a broader range of chemical interactions, focusing on electron pair transfer.

Electron Pair Donation

In the context of Lewis theory, electron pair donation is the process by which a Lewis base provides a pair of electrons to form a covalent bond with a Lewis acid. This interaction is fundamental in many chemical reactions, influencing the stability and reactivity of the resulting compounds.

Charge and Coordination

The charge of a species plays a crucial role in determining its behavior as a Lewis acid or base. For example, positively charged species like Fe³⁺ are typically Lewis acids due to their ability to accept electron pairs, while negatively charged species like F⁻ can act as Lewis bases by donating electron pairs.

Classify each species as either a Lewis acid or a Lewis base. a. Fe3+ b. BH3 c. NH3 d. F-