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Red Phosphorus is less reactive than white phosphorus. Explain

less the stability,more the reactivity.white phosphorous is less stable and more reactive bcoz of angular strain in the P4 molecule whare the angles are only 60 degree

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White phosphorus has a tetrahedral basic unit where four phosphorus atoms arranged at the four corners of a tetrahedron are joined together by a total of six single bonds. This creates a very highly strained system which is unstable and very reactive. 

Red phosphorus has an amormous structure (only short range order, no long range one) and is therefore a lot more stable and less reactive

Red phosphorous
 
 
 
 
 
 
 
 
 
 
 

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White phosphorus has a tetrahedral basic unit where four phosphorus atoms arranged at the four corners of a tetrahedron are joined together by a total of six single bonds. This creates a very highly strained system which is unstable and very reactive. 
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White phosphorus has a tetrahedral basic unit where four phosphorus atoms arranged at the four corners of a tetrahedron are joined together by a total of six single bonds. This creates a very highly strained system which is unstable and very reactive. 

Red phosphorus has an amormous structure (only short range order, no long range one) and is therefore a lot more stable and less reactive eg it ignites in air at 240 deg Celsius whereas white Phosphorus at 30 deg Celsius.
 
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White phosphorus is less stable hence more reactive than the other solid phase under normal conditions because of the angular strain in the P4 molecule where the angles are only 60. It consists of discrete tetrahedral molecule.
                  Chemically, red phosphorous is much less reactive than white phosphorus.
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White phosphorous consist of discrete P4 molecule which is tetrahedral so reactive, but in red phosphorous the P4 molecule are linked in extended chain structure so it is less reactive
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BECAUSE POLYMERIC FORM OF RED PHOSPHORUS PREVENT REACTION.
 
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White phosphorus is made up of discrete P4 tetrahedra which are subjected to very high angular strain as the angles is 60 degrees. Red phosphorus is a polymer of P4 tetrahedra, which has much less angular strain. This high angular strain makes white phosphorus unstable and highly reactive.
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White phosphorus consists of discrete P4 molecules. Moreover, the P4 molecule is tetrahedral. This results in low melting point, and low boiling point, and high reactivity, as the bond angles, necessarily 60 ∘, are highly constrained in the tetrahedron. You can actually steam distill white (and yellow) phosphorus, and get a greasy distillate of white phosphorus that is fiercely reactive, and must be stored under water.

On the other hand, in red phosphorus, there is linking between phosphorus atoms across the material.
 

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White phosphorus is made up of discrete P4 tetrahedral which are subjected to very high angular strain as the angles is 60 degrees. Red phosphorus is a polymer of P4 tetrahedral, which has much less angular strain. This high angular strain makes white phosphorus unstable and highly reactive.
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Due to angle strain of 60 degree white phosphorus is more reactive than red phosphorus.
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i) Red phosphorus is less reactive than white?phosphorus?.
(ii) Electron gain enthalpies of halogens are largely negative.
(iii) N2O5 is more acidic than
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less the stability,more the reactivity.white phosphorous is less stable and more reactive bcoz of angular strain in the P4 molecule whare the angles are only 60 degree
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i) Red phosphorus is less reactive than white?phosphorus?.?
(ii) Electron gain enthalpies of halogens are largely negative.?
(iii) N2O5 is more acidic than
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May it help you
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Arman Malik

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This is due to polymeric structure of red phosphorus or angular strain in P4 molecule of white phosphorus where the angle is only 60?.
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Kno3/H2So4
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X=2
Solve
2x+5(102+10)=500
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Due to very high igneous temperature of red phosphorus it is less reactive
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Characters
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Hhnz
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draw the structure of xeof2
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White phosphorus is more reactive due to its distinct tetrahedral structure and angular strain.
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Please find this answer

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Sonar
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To get a common market
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the tendency of the two electrons in the outermost atomic s-orbital to remain unshared in compounds of post-transition met
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