Answer :
Final Answer:
The true statements are as follows:
- The total number of valence electrons in the ion is 24.
- The number of bonds in the ion is 3.
- The formal charge on nitrogen is +1.
Explanation:
To draw the Lewis structure of the NO₃⁻ ion (nitrate ion), we need to consider the valence electrons of each atom. Nitrogen (N) has 5 valence electrons, and each oxygen (O) atom has 6 valence electrons. Since there are three oxygen atoms, the total number of valence electrons is:
Total valence electrons = Valence electrons of N + Valence electrons of O (3 atoms)
Total valence electrons = 5 + (6 x 3) = 5 + 18 = 23
So, the statement "The total number of valence electrons in the ion is 23" is incorrect. The correct total is 23.
Next, we can determine the number of bonds. In the nitrate ion (NO₃⁻), there are two single bonds between nitrogen and oxygen atoms and one coordinate (dative) bond, totaling three bonds. So, the statement "The number of bonds in the ion is 3" is correct.
Lastly, let's calculate the formal charge on nitrogen. The formula for formal charge (FC) is:
FC = Valence electrons of the atom - Non-bonded electrons - 1/2 * Bonded electrons
For nitrogen in the NO₃⁻ ion:
FC = 5 (valence electrons) - 4 (non-bonded electrons) - 1/2 * 6 (bonded electrons) = 5 - 4 - 3 = -2
So, the statement "The formal charge on nitrogen is +1" is incorrect; the correct formal charge on nitrogen is -2.
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