Classify each species as either a Lewis acid or a Lewis base. c. B(OH)₃

Verified step by step guidance

1. Identify the definition of a Lewis acid and a Lewis base: 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.
2. Examine the chemical structure of B(OH)_3: Boron in B(OH)_3 has an incomplete octet, meaning it has only six electrons in its valence shell.
3. Determine the ability of B(OH)_3 to accept electron pairs: Since boron has an incomplete octet, it can accept an electron pair to complete its octet, making it a potential Lewis acid.
4. Consider the role of hydroxyl groups (OH) in B(OH)_3: The hydroxyl groups are not donating electron pairs to other species, so they do not contribute to B(OH)_3 being a Lewis base.
5. Conclude the classification: Based on its ability to accept electron pairs due to the incomplete octet of boron, classify B(OH)_3 as a Lewis acid.

Key Concepts

Lewis Acids and Bases

Lewis acids are defined as electron pair acceptors, while Lewis bases are electron pair donors. This theory expands the concept of acids and bases beyond the traditional definitions, allowing for a broader classification based on electron interactions. Understanding this distinction is crucial for identifying the role of a species in chemical reactions.

Boron Compounds

Boron compounds, such as B(OH)3 (boric acid), often exhibit unique properties due to the electron deficiency of boron. In this case, boron can accept electron pairs, making it a Lewis acid. Recognizing the behavior of boron in chemical contexts is essential for classifying its compounds accurately.

Chemical Classification

Classifying chemical species as Lewis acids or bases involves analyzing their ability to donate or accept electron pairs. This classification is important for predicting reaction mechanisms and understanding the behavior of substances in various chemical environments. Proper classification aids in the comprehension of complex chemical interactions.