Final answer:
Boron typically forms three covalent bonds and is stable with six valence electrons, unlike other elements which seek an octet. Boron trifluoride (BF3) illustrates this, with the central boron having six electrons. Boron's unique electron configuration makes it a strong Lewis acid.
Step-by-step explanation:
Boron commonly makes only three covalent bonds and is happy with six valence electrons around the B atom. Despite other elements aiming for a full octet of electrons around them, boron is an exception and functions well with just six. This happens because of its 2s²2p¹ valence electron configuration, which naturally allows for only three bonding sites. A notable example of boron's bonding behavior is boron trifluoride (BF3), where the central boron atom is surrounded by three fluorine atoms, each contributing one electron to the bond, resulting in six valence electrons around boron. This characteristic also contributes to boron's ability to act as a Lewis acid, as seen in the BF3 molecule, which has powerful electron-accepting properties.