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3.35 states "Write the Lewis structure of (a) tetrahydridoborate ion, BH4"; (b) hypobromite ion, BrO"; (c) amide ion, NH2" I don't understand how you can use covalent bonds for molecules like BH4- or NH2- if they're ions. I know ionic bonds, you gain or lose electrons, and for covalent bonds, you share electrons. I also know how they have those negative charges (Boron has an extra hydrogen then it would've wanted (which would be 3 H)). I thought ions would make ionic bonds. So for instance, NaCl has an ionic bond so you would use brackets for both atoms when drawing the Lewis Structure. Na loss an electron, and Cl gained an electron. Also, I know that covalent bonds are formed between two nonmetals, and NH2- is an example of that. If I drew the Lewis structures without seeing the word "ion" in the question, it would make sense, but now I'm confused between the bonds for ions or bonds in general.
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