Here it says to identify each of the following as a Lewis acid or base. Bronsted-lowry acid or base or both. So for the first one we have cobalt 2 ion. Here it is a positively charged metal ion, so we could easily accept an electron pair. Therefore represents a Lewis acid. Here it wouldn't represent a Bronsted-lowry acid because of the lack of an H plus group. So here we're going to say that this is a Lewis acid.
For B we have nitric acid. Now nitric acid has the presence of an H plus group, so it could serve as a Bronsted-lowry acid now, but could it serve as a Lewis acid? Well, it doesn't have the presence of an H plus immediately doesn't have a positive metal. It doesn't have a central element that has less than 8 electrons around it. So we wouldn't exactly say that it it's a Lewis acid. We're just going to say here it's a Bronsted-lowry acid.
For the next one, this is. If we were to draw it out, it'd be Chapter 3, which is connected to a carbon double bonded to an oxygen and then bonded 2 and H2. So this is our structure. We're going to say The presence of these lone pairs here could mean that they can serve as electron pair donors. So this could serve as a Lewis base. Also, because of the presence of lone pairs, they could accept H plus ions, so that's also a possibility. So it could serve as a Bronsted-lowry base. So we're going to say it could serve both types of bases. So it's both.
Then finally we have CO32-. The presence of a negative charge means that it has extra electrons that it could share, so it could act as an electron pair donor and therefore be a Lewis base. At the same time it is CO32-. It could accept an H plus to become HCO3-, which is bicarbonate, so it could also serve as a Bronsted-lowry base. So it could be both types of bases.
Now this is how we describe each of the following compounds on whether they're a Lewis acid or base or Bronsted-lowry acid or base.