The electronegativity of nitrogen (N) is 3.0, while the electronegativity of hydrogen (H) is 2.1. As it can be seen that nitrogen (N) is more electronegative than that of hydrogen (H),
So electron pairs are attracted towards nitrogen and thus it carries a partial negative charge and hydrogen carries a partial positive charge. The image of electron distribution is attached as follows.
Thus NH₃ is a polar molecule .
None of the statement is not correct about NO, NO+, and NO−.
Explanation:
Those molecules whose all subshells are completely filled are diamagnetic.
Those molecules whose any sub-shell is incomplete is termed paramagnetic.
Let us check the magnetism in all three molecules based on molecular orbital theory and Lewis structure
NO= number of electrons 11
It form N=O having configuration 1s2,2s2,2p6,3s1, it has 1 unpaired electron so it is paramagnetic.
Now NO-, number of electrons 12 having configuration 1s2,2s2,2p6,3s2, no unpaired electron hence dimagnetic.
Now NO+, number of electrons is 10 having configuration 1s2,2s2,2p6,3s2, dimagnetic
Let us calculate the bond order of NO-
N0- have 12 electrons as 5 of nitrogen, 6 of oxygen and 1 of - charge on oxygen.
So, bond order =
= 2 double bonds
bond order of NO+, Number of electrons is 10
bond order=
bond order = 3
bond order of NO, number of electrons 11
bond order=
bond order=2.5
Larger the bond order shorter the bond.