Boron
Start with the big picture
Boron has the electronic configuration [He] 2s² 2p¹ and commonly exhibits the +3 oxidation state. It occurs in minerals rather than as a free element and exists as amorphous or crystalline allotropes. Its electron-deficient compounds include boranes with three-center–two-electron bonds, while boric acid and borax display distinctive behavior on heating and in analytical tests. The lesson also introduces boron trihalides as Lewis acids, boron’s anomalous character within Group 13, and its resistance to some reagents. Applications include glass, fiberglass, detergents, and nuclear control rods; safety considerations distinguish boron’s low toxicity in small amounts from the hazards of boranes.
What you'll learn
- Relate boron’s electronic structure to its covalent bonding and common oxidation state.
- Distinguish boron’s amorphous and crystalline allotropes.
- Describe key features of boranes, boric acid, borax, and boron trihalides.
- Recognize boron’s occurrence, reactivity, diagnostic features, and applications.
- Identify the stated safety distinction between boron and boranes.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
