Drawing the Lewis Structure for HBr

Viewing Notes:

  • HBr is very similar to HF and HCl. Hydrogen has 1 valence electron and Br (in Group 7 with F and Cl) has 7 valence electrons.
  • With the Lewis Structure for HBr remember that Hydrogen only needs 2 valence electrons to have a full outer shell.
  • Be sure that you don't use more than the 8 valence electrons available.

Transcript: Hi, this is Dr. B. Let's do the Lewis structure for HBr, hydrobromic acid. On the periodic table, Hydrogen is in group 1, so it has 1 valence electron, and Bromine is in group 7, sometimes called 17, it has 7 valence electrons; for a total of 8 valence electrons. We draw our H, we draw our Br, and we have 8 valence electrons. So let's do this: let's put 2 right here. That bonds Hydrogen and Bromine together; 4, 6, 8. Now Hydrogen only needs two valence electrons for a full outer shell. It's satisfied, it has its full outer shell. Bromine, it needs eight. Take a look at Bromine, 2, 4, 6, 8. It has eight valence electrons, and we've only used 2, 4, 6, 8; the eight valence electrons that we had to start with.

That is the Lewis structure for HBr. This is Dr. B., and thanks for watching.