what is the bond order of n2 positive, n2neagative, n2 2neagative?

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My dear it is 2.5 use rule 2 2 2 2 6 6

To determine the bond order of a molecule, you need to calculate the number of bonding electrons and divide it by 2. The bonding electrons can be found by subtracting the number of antibonding electrons from the number of bonding electrons.

1. N2+ (nitrogen cation): Nitrogen normally has 5 valence electrons. With a positive charge, it loses one electron, making it N2+ with 4 valence electrons. The molecular orbital diagram for N2+ shows that all 4 electrons are in bonding orbitals, so there are no antibonding electrons. Bond order = (4 - 0) / 2 = 2.

2. N2- (nitride anion): Nitrogen normally has 5 valence electrons. With a negative charge, it gains one electron, making it N2- with 6 valence electrons. The molecular orbital diagram for N2- shows that there are 5 electrons in bonding orbitals and 1 electron in an antibonding orbital. Bond order = (5 - 1) / 2 = 2.

3. N2 2- (dinitrogen dianion): Nitrogen normally has 5 valence electrons. With a double negative charge, it gains two electrons, making it N2 2- with 7 valence electrons. The molecular orbital diagram for N2 2- shows that there are 5 electrons in bonding orbitals and 2 electrons in antibonding orbitals. Bond order = (5 - 2) / 2 = 1.5.

So, the bond order of N2+, N2-, and N2 2- is 2, 2, and 1.5, respectively.