Lewis Dot Structures - Complex Examples

Lewis Dot Structures - Complex Examples

Example 1: Nitrogen and Fluorine

• Start with the Lewis dot symbols for Nitrogen (N) and Fluorine (F).

• Nitrogen is placed in the middle because it has the most singles (3) to form bonds.

• Fluorine atoms are placed on the outside since they each have only one single electron.

• Connect the dots to form covalent bonds.

• The resulting Lewis structure depicts nitrogen bonded to three fluorine atoms.

Example 2: Multiple Atoms and Resonance

• Determine which atom will be the central atom. Oxygen has two singles, while Nitrogen has three. Either of the nitrogens could serve as the middle atom.

• Attempt to pair up the single electrons to form bonds.

• If stuck with unpaired electrons, consider alternative arrangements.

• Loop electrons to create double bonds, but be mindful of remaining signals.

• For complex structures, breaking a loop to form a triple bond might be necessary.

• In some cases, an electron can be moved to pair with another atom.

• This may result in one atom having a positive charge.

Charge Considerations

• Moving electrons can lead to formal charges on atoms within the structure.

• Not all structures are this complicated, but it illustrates the challenges that can arise as molecules become complex.