1. Learning Objectives General properties of group 15 elements
2. Physical properties of group 15 elements
3. Chemical properties of group 15 elements

2. Group 15 elements Nitrogen N [He] 2s2p3 Phosphorus P [Ne] 3s23p3
Arsenic As [Ar]3d104s24p3
Antimony Sb [Kr]4d105s25p3
Bismuth Bi [Xe]4f145d106s26p3

3. Occurrence
Molecular nitrogen comprises 78% by volume of the atmosphere.
In the earth’s crust, it occurs as sodium nitrate, NaNO3 (called Chile
saltpetre) and potassium nitrate (Indian saltpetre)
It is found in the form of proteins in plants and animals.
Phosphorus occurs in minerals of the apatite family, Ca9(PO4)6CaX2
(X = F, Cl or OH)
Phosphorus is an essential constituent of animal and plant matter. It
is present in bones as well as in living cells.
Phosphoproteins are present in milk and eggs.
Arsenic, antimony and bismuth are found mainly as sulphide minerals.

4. General trends of group 15 elements
Atomic and Ionic Radii
Covalent and ionic ( in a particular state) radii increase in size
down the group. There is a considerable increase in covalent radius
from N to P. However, from As to Bi only a small increase in covalent radius is observed. This is due to the presence of completely filled and/or f orbitals in heavier members.
Ionisation energy
The value of ionization energy is quite high for the members of group 15 than the corresponding members of group 14. This is due to smaller atomic radii, increased nuclear charge and stable electronic configuration of half filled orbitals.

5. Illustrative Problem
Why nitrogen exists as N2 whereas phosphorous exists as P4
Solution :
Because d orbitals are not available in nitrogen.

6. Electronegativity
The electronegativity value, in general, decreases down the group with
increasing atomic size. However, amongst the heavier elements, the
difference is not that much pronounced.

7. Physical Properties All the elements of this group are polyatomic.
Dinitrogen is a diatomic gas while all others are solids.
Metallic character increases down the group. Nitrogen and phosphorus are non-metals, arsenic and antimony metalloids and bismuth is a metal.
This is due to decrease in ionisation enthalpy and increase in atomic size.
The boiling points, in general, increase from top to bottom in the group but the melting point increases upto arsenic and then decreases upto bismuth. Except nitrogen, all the elements show allotropy.

8. Chemical Properties Oxidation state
Stability of +3 oxidation state increases down the group while that of +5 oxidation state decreases down the group.
Bi5+ salts are very rare and good oxidising agents
As3+ salts are good reducing agents.

9. Oxidation Number
Nitrogen Compound
Phosphorus Compound N2 P4 +3
HNO2 (nitrous acid)
H3PO3 (phosphorous acid)
N2O3
P4O6 +5
HNO3 (nitric acid)
H3PO4 (phosphoric acid)
NaNO3 (sodium nitrate)
Na3PO4 (sodium phosphate)
N2O5
P4O10

10. Anomalous properties of nitrogen
Nitrogen differs from the rest of the members of this group due to
its smaller size, high electronegativity, high ionisation enthalpy and
non-availability of d orbitals.
Nitrogen has unique ability to form p -p multiple bonds with itself and with other elements having small size and high electronegativity
On the contrary, phosphorus, arsenic and antimony form single bonds as P–P, As–As and Sb–Sb while bismuth forms metallic bonds in elemental state. However, the single N–N bond is weaker than the single P–P bond because of high interelectronic repulsion of the non-bonding electrons, owing to the small bond length.

11. Reactivity towards hydrogen
All the elements of Group 15 form hydrides of the type EH3
where E = N, P, As, Sb or Bi.
Down the group, covalent character, basicity and thermal stability decrease while reducing character increases.
NH > PH > AsH > SbH3 > BiH3
107° 48’ ° 48’ ° 48’ ° 18’ °

12. Illustrative Problem Explain why NH3 is a stronger base than PH3?
Solution
Since phosphorus is bigger in size as compared to nitrogen so, availabilty of lone pair is less. Thus PH3 is a weaker base than NH3

13. Illustrative Problem
Give the order of basicity and reducing character and stability for the following hydrides: NH3, PH3, AsH3, SbH3
Solution :
Basicity NH3 > PH3 > AsH3 > SbH3
Stability NH3 > PH3 > AsH3 > SbH3
Reducing character NH3 < PH3 < AsH3 < SbH3

14. Reactivity towards oxygen
All these elements form two types of oxides: E2O3 and E2O5.
The oxide in the higher oxidation state of the element is more acidic than that of lower oxidation state. Their acidic character decreases down the group.
The oxides of the type E2O3 of nitrogen and phosphorus are purely acidic, that of arsenic and antimony amphoteric and those of bismuth
is predominantly basic.

15. Reactivity towards halogens
These elements react to form two series of halides : EX3
and EX5.
Nitrogen does not form pentahalide due to non availability of the d orbitals in its valence shell.
Pentahalides are more covalent than trihalides. All the trihalides of these elements except those of nitrogen are stable. In case of nitrogen, only NF3 is known to be stable
Trihalides except BiF3 are predominantly covalent in nature.

16. Reactivity towards metals
All these elements react with metals to form their binary compounds exhibiting –3 oxidation state, such as:
Ca3N2(calcium nitride)
Ca3P2 (calcium phosphide),
Na3As2(sodium arsenide),
Zn3Sb2 (zinc antimonide) and
Mg3Bi2(magnesium bismuthide).

17. Oxides of nitrogen

18. Oxides of nitrogen

19. Illustrative Problem Which oxide of nitrogen is coloured ? Solution :
NO2 has unpaired electrons,so it is coloured.

20. Oxides
P, As, Sb and Bi form two types of oxides: M2O3 and M2O5 and exists
as dimer due to reluctance for bonding.
Oxides of phosphorous — P4O6 and P4O10
Both P4O6 and P4O10 are acidic oxides which dissolve in water to give
phosphonic acid and phosphoric acid respectively.