Acids and Bases

# Calculate the net formal charge of this species HNO3?

91011 ###### 2010-08-10 16:17:35

The formal charge of HNO3 is 0 because the charge on NO3 is -1 and the charge on H is always +1.

formal charge of an atom in a bond is measured by the number of electrons in it's last energy level.for an example Nitrogen has 5 electrons in it's last energy level.and when calculating the net formal charge, if the number of electrons in the last energy level of any atom increases,as electrons have a negative charge -1 should be added for each increased electron.

as an example in (NO3)^- nitrogen has contributed only 4 electrons to create bonds with oxygen as each bond is created sharing one electron from each atom.so there's a decrease of electrons in the last energy level of nitrogen.so it gets a +1 charge as it lacks one electron.

but if we consider the 3 oxygens around the nitrogen atom,one has 6 electrons which is the correct number of electrons in it's last energy level.but the other two has 7 which gives -1 charges for each atom.

and the total of all these charges equals to -1 which is the net formal charge of NO3.

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## Related Questions Using the (M1*V1)=(M2*V2) equation, we can calculate the necessary volume of concentrated acid to make the diluted acid: [(16M HNO3)*(x mL HNO3)] = [(0.50M HNO3)*(250 mL HNO3)] Solve for x: x = [(0.50M HNO3)*(250 mL HNO3)] / (16M HNO3) x = 7.813 mL (of 16 M HNO3) Nitric acid, HNO3 has covalent bonds. Two nitrogen-oxygen single bonds, one nitrogen-oxygen double bond and an oxygen-hydrogen single bond. There is a formal +1 charge on the nitrogen center, and a formal -1 charge on the single-bonded oxygen without the hydrogen atom.

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