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The bond angle of NO2+, NO2 and NO2 are, respectively:
A: 180,134,115
B: 115,134,180
C: 134,180,115
D: 115,180,130


Answer
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Hint: For the formation of bond angle there must be at least three atoms and two bonds. The bond angle is the angle that is formed between three atoms across at least two bonds. This angle is different for different compounds.


Complete answer: We know the bond angle is the angle which is formed between two bonds. It depends on many factors which are stated below:
Forces of attraction or repulsion between atoms of molecules may increase or decrease the bond angle.
Hybridization also affects the bond angle. As the s character of hybrid orbital increases bond angle increases.
Electronegativity and lone pair also affect the bond angle. Increasing the lone pair and decreasing the electronegativity decreases the bond angle.
In the given question all atoms are the same but the charge is different so let’s discuss hybridization. Hybridization is the process of mixing atomic orbitals into new hybrid orbitals. NO2+ has two bond pairs and zero lone pairs so hybridization of NO2+is sp, and it will have linear geometry. It is clear that for linear geometry bond angle is 180. Therefore the bond angle of NO2+ is180. NO2 has two bond pairs and one lone pair, so it will have triangular planar geometry and sp2 hybridization and NO2 will have two bond pairs, one lone pair, and also a negative charge. Due to this negative charge, there will be repulsions between negative charge and lone pair and thus it will decrease the bond angle. So the bond angle of NO2will be less than NO2. From the given options 180 is the bond angle of NO2+ remaining angles are 134 and 115, also bond angle of NO2is less than bond angle of NO2. So the bond angle of NO2is 134and bond angle of NO2is 115.

So the correct answer is option A that is 180,134,115.


Note:
Factors that affect the bond angle of a molecule are electronegativity, lone pair, hybridization, Forces of attraction, or repulsion. Lone pair- lone pair repulsions are stronger than lone pair-bond pair repulsions and these are stronger than bond pair-bond pair repulsions.