Chemical Bonding: Lewis Dot Structure for HCl (4 of 6)

The Lewis Structure for HCl (hydrochloric acid) is one of the easier dot structures to draw. When you draw the structure remember that Hydrogen (H) only needs two valence electrons to have a full outer shell.

Watch the video of Dr. B. drawing the dot structure for hydrochloric acid (HCl) and answer the questions below.

Hint: look at the questions before watching the video.

Video Transcript: For this one, we're going to try hydrochloric acid: HCl. The first thing we have to do is find out how many valcence electrons we're working with. If we look at our periodic table, we can see that H is in group 1, so it has 1 valence electron, and Cl is in group 7 over here, also called 17, so it has 7 valence electrons. So I have a total of 8 valence electrons to work with. There's really no center to this, so it doesn't matter about putting the least electronegative at the center, so let's just write HCl.

We're going to put two electrons between the atoms to form bonds, so now they're bonded together. I've used 2. I have 6 more electrons. And now I can put the remaining electrons around to fill the octet. Hydrogen has two so I'm done with that, but Chlorine needs 8, so 2, 4, 6, 8. I've used up all my electrons. Hydrogen has 2 valence electrons, so it's satisfied. And then Chlorine has 8. So Hydrogen's the only one that's going to need 2 valence electrons to be satisfied here. Chlorine, Sodium, anything else, any of the other atoms are going to need eight to fulfill their octet. Right, so we did hydrochloric acid there.

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