Answer :
Final answer:
The formal charge on a nitrogen atom with no lone pairs and forming two double bonds is 1. This is calculated using the formula: formal charge = valence electrons - (non-bonding electrons + 1/2 * bonding electrons).
Explanation:
The formal charge of an atom can be calculated using the formula: formal charge = valence electrons - (non-bonding electrons + 1/2 * bonding electrons). The nitrogen atom in this case forms two double bonds and has no lone pairs. Each double bond consists of two bonding electrons thus, from four bonds, there will be eight bonding electrons. Given that nitrogen normally has five valence electrons, applying the formula gives us: formal charge = 5 - (0 + 1/2 * 8) = 5 - 4 = 1. Therefore, the formal charge on a nitrogen atom with no lone pairs and forming two double bonds is 1.
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Answer:
+1
Explanation:
A nitrogen atom that forms two double bonds and has no lone pairs would have a formal charge of +1.
The formal charge of an atom is calculated by subtracting the number of lone pair electrons and half the number of bonding electrons from the number of valence electrons. In the case of nitrogen, it has five valence electrons. If it forms two double bonds, then it is sharing four electrons with each bond, for a total of 8 electrons. This means that nitrogen has lost 3 electrons compared to the neutral atom, which gives it a formal charge of +1.
