@DHMO "Whether di-, tri-, or
tetracoordinate, carbon obeys the octet rule with great predictability
and has four 2-electron (2e) covalent bonds. Atoms with more than
four bonds are known as hypervalent,1 while those with fewer are
said to be electron-deficient. Hypervalence is common in heavier
main group compounds (e.g., PF5 and SF6) but very rare in carbon
compounds. It is widely accepted in the transition state of an SN2
reaction, but the high improbability of actually isolating examples
of hypervalent carbon was dogma for a long time." From "hexacoordinate carbon paper from JACS