Lewis Dot Structures: Ions Video Lessons

Concept

# Problem: Draw the Lewis structure of NO2-To add lone pairs, click the button before clicking on the molecule. To add bonds connect atoms with a line .Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all 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.Lewis structures of ionsA charge on a formula affects the total number of valence electrons that should appear in the structure. For anions, add the magnitude of the charge to the total. For cations, subtract the magnitude of the charge from the total.

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###### Problem Details

Draw the Lewis structure of NO2-

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

Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all 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.

Lewis structures of ions

A charge on a formula affects the total number of valence electrons that should appear in the structure. For anions, add the magnitude of the charge to the total. For cations, subtract the magnitude of the charge from the total.