# What is the lewis structure for bicarbonate?

$H - O - C \left(= O\right) {O}^{-}$
There are $1 + 4 + 3 \times 6$ valence electrons to distribute $+ 1$ electrons for the negative charge; thus $24$ electrons or $12$ electron pairs.
Bonding electrons account for $10$ electrons; the remaining $14$ electrons are distributed around the oxygen centres, i.e. $7$ lone pairs. The formally negative oxygen atom has $3$ lone pairs. Of course, this negative charge can be delocalized over the the formally, doubly bound oxygen.