why nitrogen exist as a gas and phosphorus exist a solid?

 nitrogen has tendency to form multiple bonds with itself. so it exists as a ''discrete'' molecule. whereas phosphorus, and other group members being bigger donot form stable multiple bonds with themselves and hence exist as a solid form.

this the reason for nitrogen existing as a gaseous molecule and phosphorus as a solid.

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according to me nitrogen is least rective that, why it exist as gase

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As Nitrogen pairs up,into N2 molecule which has very strong triple bond there is relatively little attraction between one nitrogen molecule and another, so they move indipendently and form gas.

In phosphorus, the atom do not pair up,they bond to there neighbouring atoms, thus forming a network of bonding holds the atoms together into a solid.

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Nitrogen does not catenate like carbon or phosphorous here and hence forms triple bond with another N-atom, which is a very very strong bond and satisfies its octet thus it has no requirement to catenate and form long chains, and exists as an almost inert gas in atmosphere. 
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But that does not exactly state why it is a gas.
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N2 is exist as diatomic molecule in which two nitrogen atoms are attached to each other by triple bond this triple bond is due to p(pie)-p(pie) multiple bonding (sidewise overlapping) and such bonding is not possible in phosphorus due to it's large size but possible in nitrogen due to it's small size.

In case of phosphorus four atoms are associated so it have high molecular mass ,large magnitude of venderwall forces so phosphorus is solid and nitrogen is gas.
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nitrogen hs p pie p pie bondins but phosphorous has d pie p pie bonding which is more strong than p pie ppie bond and hence phosphrous is solid
 
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Nitrogen is chemically less reactive. This is because of the high stability of its molecule N2 . In N2 the two nitrogen atoms form a triple bond . This triple bond has very high bond strength, which is very difficult to break . It is because of nitrogen's small size p pi - p pi bomd with itself. Thus phosphorus exist as solid and nitrogen as gas...
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Nitrogen is chemically less reactive. This is because of the high stability of its molecule N2 . In N2 the two nitrogen atoms form a triple bond . This triple bond has very high bond strength, which is very difficult to break . It is because of nitrogen's small size p pi - p pi bond with itself. Thus phosphorus exist as solid and nitrogen as gas...
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Nitrogen exists as diatomic molecules with a triple bond; hence, its bond enthalpy is very high (941.4 kJ mol−1). On the other hand, P, As and Sb form single bonds as P−P, As−As and Sb−Sb; bismuth exists in elemental state
 
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This is due to the formation of p(pie)-p(pie) multiple  bonds due to the small size and high electron negativity of nitrogen, nitrogen exits as a gas at room temperature.
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This is becoz in nitrogen there is present weak vandervaal forces but on other hand P exists as a tetrahedral P4 molecule which is attached to other 3 phosphorous atoms by P-P single bonds.
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Fe3O4 is ferrimagnetic in room temperature bt becomes paramagnetic in 850K why?
 
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N-N single bond dissociation enthalpy is low compared to Phosphorus which makes it have no catenation property and makes pi bond and exists only as di atomic molecule as a gas whereas Phosphorus has the property of catenation to form big structures to exist in solid form due to high bond dissociation enthalpy. 
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N2 exist as diatomic molecule because of its smaller size and higher electronegativity, it has tensency to form p(pi)-p(pi) bonding. this tendency decreases down to group due to increase in size and decrease in electronegativity.
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good
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Nitrogen has tendency to form multiple bond with itself.so it exists as "GAS". Where as phosphorus being bigger donor form stable multiple bond with themselves and hence exists as a solid form.
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Due to strong p pie-p pie multiple bonding, nitrogen forms a triple bond with other nitrogen atom giving N2 molecules. Wheras phosphorous does not form p pie-p pie multiple bonding it forms d pie- p pie single bond with other phosphorus atom giving P4 molecules. Thus nitrogen exists as gas and phosphorus as a solid.
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NITROGEN DUE TO ITS HIGH E.N. AND SMALL SIZE IS ABLE TO FORM Ppie-Ppie MULTIPLE BONDS WITH ITSELF AND THEREFORE EXIST AS DIATPOMIC N2 GAS
WHEREAS PHOSHORUS DUE TO ITS LARGE SIZE IS ONLY ABLE TO FORM SINGLE BONDS
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As nitrogen is diatomic gas bcz is exists as a dicrete molecule which means no force attraction set up b/w the two neighbouring nitrogen molecules however, phosphorous exists as solid bcz of its high atomicity..
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If n2 forms single bond it is weak bcos inerelectron repulsions of non bonded electrons but in triple bond the non bonded and bonded electrons are in such arrangement that there is less repulsions.n2 in tripple bond the bond lenth is greater than the single bonded nitrogen thats it is in gaseus
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Nitrogen does not have vacent d orbital in its valence shell. It cannot extend its velency beyond 3.but on the other side phosphorus has vacent 3d-orbital in the valence shell and promoted one electron from 3s to 3d orbital
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Nitrogen exists as diatomic molecule. Because of its small size and less no. Of electrons, van der walls force of attractions between N2 molecules is less so it exists as gas. But phosphorus exists as P4. Its size is big and has more mass as well as more no. Of electrons as compared to N2. So it exists as solid
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He is used in diving apparatus as a dilute for o2
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Idk
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NO IDEA
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In the molecules of nitrogen their is a very linkage or attraction, so its atoms are lose everywhere that is why it exist as gas. while in phosphorus the atoms are tightly bonded and linked. There is no loose movement so it is a solid. 
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How are you today?
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due to more M-M bond strength in phosphorous.
as P4 can make pπ-dπ bond.
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I am a class 8th student so it is not possible for me to tell the answer .
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Phosphor show catenation.wheteas nitrogen not
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n2 has very low BP
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Due to larger atomic size P is unable to form pi bonds and so it is tetra-atomic in which each P atom is linked with 3 other P atoms by 3 sigma bond. But, due to smaller atomic size N forms 1 sigma and 2 pi bonds i.e. triple bonds with other N atom and exists as diatomic molecule.
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Plz answer another questions also..there is no such need for involving too many experts for a single query...we also need ur expertisation in our query also...mine many queries are still pending to answer by you all....thank u
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nitrogen exists as a diatomic molecule thus the intermolecular force of attraction is weak vanderwaal force and thus it's molecular weight is less....  but in sulphur as it is polyatomic(S8) therefore the intermolecular force of attraction is quite high and thus the molecular weight of sulphur is high.... thus due to this reason sulphur is a solid in room temperature and nitrogen is  a gas in room temperature.....
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Nitrogen has the ability to form p?-p? mutiple bond while phosphorous can form p?-d? multiple bond
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Because N2 is lighter in weight as comparison to P . and N2 has the tendency to form bonding with itself.
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Because catenation power of is less than phosphorous
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Nitrogen exist as diatomic where as p exist as tetra atomic.this is because smaller size ,high electronegativity of n2 and can form multiple bond by pπ-pπ overlap.on the other hand,the size of p4 is larger lesser electronegative and can't form multiple bond by pπ-pπ overlap
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Due to higher vanderwaal force existong between phosphorus than in between nitrogen...similar case can be observed in case of o2 and sulfur.
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Please find this answer

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N2 is exist as diatomic molecule in which two nitrogen atoms are attached to each other by triple bond this triple bond is due to p(pie)-p(pie) multiple bonding (sidewise overlapping) and such bonding is not possible in phosphorus due to it's large size but possible in nitrogen due to it's small size.?


In case of phosphorus four atoms are associated so it have high molecular mass ,large magnitude of venderwall forces so phosphorus is solid and nitrogen is gas.
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The single N-N is weaker than single P-P bond because of high interelectronic repulsions of non-bonding electrons due to small length (109pm).As a result,nitrogen exist as a gas and phosphorus exist as solid.
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This is due to the forces of attraction between phosphorus atoms being high whereas nitrogen atoms being low that makes them exist in solid and gas state respectively
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N2 is exist as diatomic molecule in which two nitrogen atoms are attached to each other by triple bond this triple bond is due to p(pie)-p(pie) multiple bonding (sidewise overlapping) and such bonding is not possible in phosphorus due to it's large size but possible in nitrogen due to it's small size.?


In case of phosphorus four atoms are associated so it have high molecular mass ,large magnitude of venderwall forces so phosphorus is solid and nitrogen is gas.
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Nitrogen ki bond enthalpy phosphorus see Jada hoti hai
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Nitrogen can able to form triple bond with another nitrogen atom and it can also forms p pie-p pie bond. But phosphorus can't able to form triple bound with it co ordinate . Thus nitrogen exist in gaseous phase and phosphorus in solid state.
 
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Because nitrogen make p pie p pie bond but phosphorus make d pie p pie bond hence phosphorus has a solid
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Difference of boiling or melting points
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  • N2 is exist as diatomic molecule in which two nitrogen atoms are attached to each other by triple bond this triple bond is due to p(pie)-p(pie) multiple bonding (sidewise overlapping) and such bonding is not possible in phosphorus due to it's large size but possible in nitrogen due to it's small size.

          In case of phosphorus four atoms are associated so it have high molecular mass ,large magnitude of venderwall forces so phosphorus is                      solid and nitrogen is gas.
  • Nitrogen exists as diatomic molecule. Because of its small size and less no. Of electrons, van der walls force of attractions between N2 molecules is less so it exists as gas. But phosphorus exists as P4. Its size is big and has more mass as well as more no. Of electrons as compared to N2. So it exists as solid.
  •  nitrogen has tendency to form multiple bonds with itself. so it exists as a ''discrete'' molecule. whereas phosphorus, and other group members being bigger donot form stable multiple bonds with themselves and hence exist as a solid form.

    this the reason for nitrogen existing as a gaseous molecule and phosphorus as a solid.

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Nitrogen exists as gas but phosphorus not because of strong bonds in P4 molecule than in N2
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due to lone pair?
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Please find this answer

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N2 exist as a gas whereas P as solid because nitrogen shows  p pie - p pie multiple bonding. this multiple bonding in N2 occurs due to its small size. Thus N2 forms diatomic molecule and exist as gas. whereas P exist in elemental state.



 
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Nitrogen is chemically less reactive. This is because of the high stability of its molecule N2 . In N2 the two nitrogen atoms form a triple bond . This triple bond has very high bond strength, which is very difficult to break . It is because of nitrogen's small size p pi - p pi bond with itself. Thus phosphorus exist as solid and nitrogen as gas...
 
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Nitrogen has the tendency to form multiple bond with itself l.So it exists as a gas.Where as phosphorus being bigger donour from stable multiple bond with themselves and hence exists as a solid form.
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Sugar cane
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Of sn2
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Bhour model
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Due to interhalogen compounds in the outermost shell the gass formation of phosphorus does not exist.
In other words nitrogen forms diatomic molecules while phosphorus does not. As a result nitrogen exists as a gas and phosphorus exist as a solid.
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Please find this answer

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