Answer
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Step 1:: Draw the Lewis structure for the first possible case, where a lone pair from one of the two oxygen atoms not bonded to hydrogen is used to form a bond with the carbon atom.
\begin{array}{ccccc} & & \mathrm{O} & & \ & & | & & \ \mathrm{H}-\mathrm{C}-\mathrm{O} & \longrightarrow & \mathrm{O} & - & \mathrm{C}-\mathrm{O}^{-} \ & & | & & \ & & \mathrm{H} & & \end{array}
Step 2:: Draw the Lewis structure for the second possible case, where a lone pair from the oxygen atom bonded to the hydrogen is used to form a bond with the carbon atom.
\begin{array}{ccccc} \mathrm{H} & - & \mathrm{C} & = & \mathrm{O} \ & & | & & | \ & & \mathrm{O}^{-} & - & \mathrm{H} \end{array}
Step 3:: Explain why the first Lewis structure is more stable.
The first Lewis structure is more stable because it results in a charge separation, with a negative charge on the oxygen atom that initially had two bonds and a positive charge on the oxygen atom that initially had one bond. This charge separation leads to a more stable electronic configuration, as it reduces electrostatic repulsion between like charges.
Final Answer
a.) The Lewis structure when using a lone pair from one of the two oxygen atoms not bonded to hydrogen: \begin{array}{ccccc} & & \mathrm{O} & & \ & & | & & \ \mathrm{H}-\mathrm{C}-\mathrm{O} & \longrightarrow & \mathrm{O} & - & \mathrm{C}-\mathrm{O}^{-} \ & & | & & \ & & \mathrm{H} & & \end{array} b.) The Lewis structure when using a lone pair from the oxygen atom bonded to the hydrogen: \begin{array}{ccccc} \mathrm{H} & - & \mathrm{C} & = & \mathrm{O} \ & & | & & | \ & & \mathrm{O}^{-} & - & \mathrm{H} \end{array} c.) The first Lewis structure is more stable due to charge separation and reduced electrostatic repulsion.
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