# Problem: Based on formal charges, draw the most preferred Lewis structure for the chlorate ion, ClO3-.To add lone pairs, click the button before clicking on the molecule. To add bonds connect atoms with a line .To add formal charges, click the  or  button before clicking on the molecule.on the molecule.Draw the molecule by placing atoms on the grid and connecting them with bonds. Include lone pairs of electrons. Use square brackets to denote the overall charge.Use the following steps to draw Lewis structures from molecular formulas:1. Sum the valence electrons from all of the atoms.2. Connect the appropriate atoms using a single bond (a line, which represents two electrons). The central atom is usually the least electronegative atom, but never hydrogen.3. Add lone pairs to complete the octets of the outer atoms. Keep in mind that hydrogen fills its "octet" with only two electrons.4. Place any leftover electrons on the central atom. Keep in mind that elements in row 3 of the periodic table and beyond can exceed the general octet.5. If any atom lacks an octet, try using double or triple bonds. You may have to use one or more lone pairs to make the double or triple bonds so that the total number of valence electrons remains the same.

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###### Problem Details

Based on formal charges, draw the most preferred Lewis structure for the chlorate ion, ClO3-.

To add lone pairs, click the button before clicking on the molecule. To add bonds connect atoms with a line .To add formal charges, click the  or  button before clicking on the molecule.

on the molecule.

Draw the molecule by placing atoms on the grid and connecting them with bonds. Include lone pairs of electrons. Use square brackets to denote the overall charge.

Use the following steps to draw Lewis structures from molecular formulas:

1. Sum the valence electrons from all of the atoms.
2. Connect the appropriate atoms using a single bond (a line, which represents two electrons). The central atom is usually the least electronegative atom, but never hydrogen.

3. Add lone pairs to complete the octets of the outer atoms. Keep in mind that hydrogen fills its "octet" with only two electrons.
4. Place any leftover electrons on the central atom. Keep in mind that elements in row 3 of the periodic table and beyond can exceed the general octet.

5. If any atom lacks an octet, try using double or triple bonds. You may have to use one or more lone pairs to make the double or triple bonds so that the total number of valence electrons remains the same.