Question Video: Understanding How to Draw Lewis Structures for Fluoride Ions Chemistry • 10th Grade

Which of the following is the correct Lewis structure for a fluoride ion? [A] Structure A [B] Structure B [C] Structure C [D] Structure D [E] Structure E


Video Transcript

Which of the following is the correct Lewis structure for a fluoride ion?

The first step in creating our Lewis structure is to write the appropriate atomic symbol. We need to create a Lewis structure for a fluoride ion. Fluoride ions are an ion of the element fluorine, which has the atomic symbol F. Next, we need to determine the number of valence electrons. Fluorine is in group seven of the periodic table. Fluorine, like the other elements in group seven, have seven valence electrons. When the atoms of elements in group seven form ions, they tend to gain one electron. This forms an ion with a charge of negative one and gives the ion a full valence shell. So we know the fluoride ion has eight valence electrons.

Now that we know the number of valence electrons, we’ll place a number of dots equal to the number of valence electrons around the atomic symbol. We can place two dots on each side of the atomic symbol until we’ve used up all of the valence electrons. And now, because we’re creating the Lewis structure for an ion, we have one more step. We need to surround our Lewis structure with square brackets and indicate the charge of the ion in the top-right corner. As we can see, the Lewis structure we’ve created for a fluoride ion matches the structure in answer choice (E).

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