General chemistry of group 13 elements
Start with the big picture
The +3 oxidation state is characteristic of Group 13, while heavier members can also show +1 as the inert-pair effect becomes more significant; +1 is most stable for thallium. Down the group, metallic character and electrical conductivity rise, while ionization energy, electronegativity, and Lewis acidity decrease. The elements also differ in bonding and compounds: boron forms covalent halides and polyhedral boranes, whereas aluminium halides can dimerize and its oxide and hydroxide are amphoteric. The chapter connects these patterns to oxide and hydroxide acid–base behavior, oxoanions, complex formation, the boron–silicon diagonal relationship, passivation, and disproportionation. Together, these themes provide a framework for comparing the chemistry of boron with that of the heavier Group 13 elements.
What you'll learn
- Relate the ns² np¹ valence configuration to characteristic Group 13 oxidation states.
- Describe how metallic character, conductivity, and selected periodic properties change down the group.
- Compare the bonding and structures of Group 13 halides and hydrides.
- Explain trends in oxide and hydroxide acid–base behavior, complex formation, and oxoanions.
- Identify the roles of the inert-pair effect, passivation, and the boron–silicon diagonal relationship.
Continue your study
Work through the complete notes and reinforce the topic with the study tools available in the full lesson.
