Presentation on theme: "P-BLOCK ELEMENT General electronic configuration : ns² np¹ˉ ⁶."— Presentation transcript:
General electronic configuration : ns² np¹ˉ ⁶
Atomic and ionic radii : increases down the group Ionisation Enthalpy : 1 st I.E. Of group 15 elements are higher than group 14 elements and on going down the group, IE decreases. Electronegativity : Value of Group 15 are higher than group 14 and on going down the group, value decreases. Metallic Character : On going down the group metallic character increases from N to Bi.
Catenation : group 15 show a tendancy towards catenation, but to a much smaller extent than Carbon. Allotropy : Except N and Bi, all elements of the group show allotropy. Oxidation States : They exhibit oxidation states from -3 to +5. The tendancy to exhibit -3 oxidation state decreases down the group and the stability of +5 oxidation state decreases while that of +3 increases due to inert pair effect.
Reactivity towards hydrogen (formation of hydrides) All the elements of group 15 form gaseous tri hydrides of the formula EH 3 (where E=N, P, As, Sb or Bi) such as : NH 3 PH 3 AsH 3 SbH 3 BiH 3 The lighter elements also form hydrides of the fomula M 2 H 4 such as N 2 H 4 (hydrazine), P 2 H 4 (diphosphine) and HN3 known as hydrogen azide or hydrazoic acid.
The tri hydrides can be easily obtained by the hydrolysis of their binary metal compounds with water of dilute acids : Mg 3 N 2 + 6H 2 O Mg(OH) 2 + 2NH 3 Ca 3 N 2 + 6H 2 O Ca(OH) 2 + 2NH 3 Ca 3 P 2 + 6H 2 O Ca(OH) 2 + 2PH 3 Zn 3 E 2 + 6HCl ZnCl 2 + 2EH 3 Zn 3 As 2 + 6HCl ZnCl 2 + 2AsH 3 Mg 3 Bi 2 + 6HCl MgCl 2 + 2BiH 3
The tri chlorides of these elements except that of bismuth give the corresponding hydrides on reduction with Zn/acid or LiAlH4 ECl 3 + 3LiAlH EH 3 + 3LiCl + 3AlH 3 (E=N,P, As, Sb) Ammonia (H3) is the most important trihydride of the group and is extensively used in the manufacture of nitric acid (HNO3) and important chemical fertilizers such as ammonium sulphate, urea, calcium ammonium nitrate, calcium cyanamide, etc. it is prepared on an industrial scale by Haber process. In this process, nitrogen combines with hydrogen at K under a pressure of atm in the presence of iron catalyst and Mo as promoter. N 2 + 3H NH 3 ; H = kJ mol -1 Phosphine (PH3) can be prepared by heating white phosphorus with concentrated caustic alkali in an inert atmosphere of oil gas : P 4 + 3KOH + 3H 2 O PH 3 + PH 3 + 3KH 2 PO 2
All these hydrides are covalent in nature and have pyramidal structure. These involves sp 3 hybridization of the central atom and one of the tetrahedral position is occupied by a lone pair. The structure of NH 3 molecule is shown in Fig. 2. Due to the presence of lone pair, the bond angle in NH 3 is less than the normal tetrahedral angle. It has been found to be 107. as we go down the group the bond angle decreases as : NH 3 PH 3 AsH 3 SbH 3 BiH
In all these hydrides, the central atom is surrounded by four electron pairs, three bond pairs and one lone pair. Now, as we move down the group from N to Bi, the size of the atom goes on increasing and its electro negativity decreases. Consequently, the position of bond pair shifts more and more away from the central atom in moving from NH 3 to BiH 3. for example, the bond pair in NH 3 is close to N in N-H bond than the bond pair in P-H bond in PH 3. As a result, the force of repulsion between the bonded pair of electrons in NH 3 is more than in PH 3. in general, the force of repulsion between bonded pairs of electrons decreases as we move from NH 3 to BiH 3 and therefore, the bond angle also decreases in the same order.
The important characteristics of these hydrides are : I) Basic Strength : All these hydrides have one lone pair of electrons on their central atom. Therefore, they act as Lewis bases. The can donate an electron pair to electron deficient species (Lewis acids). As we go done the group, the basic character of these hydrides decreases. For example, NH 3 is distinctly basic; PH 3 is weakly basic; AsH 3, SbH 3 and BiH 3 are very weakly basic. Explanation Nitrogen atom has the smallest size among the hydrides. Therefore the lone pair is concentrated on a small region and electron density on its is the maximum. Consequently, its electron releasing tendency is maximum. As the size of the central atom increases down the family, the electron density also decreases. As a result, the electron donor capacity or the basic strength decreases down the group.
Thermal stability of the hydrides of group 15 elements decreases as we go down the group. Therefore, NH 3 is most stable and BiH 3 is least stable. The stability of the hydrides of group 15 elements decreases in the order : NH 3 > PH 3 > AsH 3 > SbH 3 > BiH 3 Explanation : This is due to the fact that on going down the group, the size of the central atom increases and therefore its tendency to form stable covalent bond with small hydrogen atom decreases. As a result the M-H bond strength decreases and therefore thermal stability decreases.
The reducing character of the hydrides of group 15 elements increases from NH3 to BiH3. thus, increasing order of reducing character is as follows: NH 3 < PH 3 < AsH 3 < SbH 3 < BiH 3 Explanation : The reducing character depends upon the stability of the hydride. The greater unstability of group 15 hydrides decreases from NH 3 to BiH 3, hence the reducing character increases. For example, NH 3 being most stable among the group 15 hydrides is not a good reducing agent. The other hydrides being unstable act as good reducing agents. However, it may be noted that ammonia at high temperature reduces copper oxide to copper : 3CuO + 2NH Cu + N 2 + 3H 2 O
Ammonia has a higher boiling point than phosphine and then the boiling point increases down the group because of increase in size. Molecule NH 3 PH 3 AsH 3 SbH 3 BiH 3 Boiling Point (K) Melting Point (K) Similar behavior is observed for melting points. Explanation : The abnormally high boiling point of ammonia is due to its tendency to form hydrogen bonds. The electro negativity of N(3.0) is much higher than that H(2.1). As a result N-H bonds are polar and therefore NH3 undergoes intermolecular hydrogen bonding. In PH 3 and other hydrides, the intermolecular forces are van der waals forces. There van der waals forces increase with increase in molecular size and therefore, boiling points increase on moving from PH 3 to BiH 3.
Ammonia forms hydrogen bonding with water molecules while phosphine and other hydrides do not form hydrogen bonding with water. Therefore NH 3 is soluble I water while PH 3 ad other hydrides are insoluble I water. The trends in the properties of hydrides of group 15 are given
Elements of group 15 form gaseous tri- hydrdides of the formula EH 3 These hydrides are covalent in nature and have pyramidal structure. These involve sp 3 hybridisation of the central atom and one of the tetrahedral position is occupied by a lone pair. Bond angle decreases down the group due to presence of lone pair and increase in size of atom. Basic strength decreases down the group due to increase in size and the electron donor capacity decreases. Thermal stability decreases down the group due to increase in size. Reducing character increases down the group since the stability decreases from NH 3 to BiH 3. Ammonia has high BP due to its tendency to form H-bond. All hydrides are insoluble except NH 3 due to H-bonding.
Write the electronic configuration of the given element P(15) and Sb (51)? Explain why ammonia is basic in nature. How is ammonia manufactured industrially? Discuss the trend in chemically reactivity of group 15. Why ammonia is a good complexing agent.
(a)Assignment for bright students: 1.How dose ammonia react with a solution of Cu PCl 5 is ionic in solid state.why. 3.Give the shape of the following: P 4, PF 5, NF The HNH angle value is higher than HPH, HASH and HSbH angles. Why ? 5. PH3 forms bubbles when passed slowly in water but NH3 dissolves. Why?
1.Discuss the hydrides of group 15 elements. 2.Draw the structure of the NH 3 & PH 3 3.Why NH 3 is basic in nature. 4.Why NH 3 is more soluble in water. 5.Which hydride of group 15 element has lowest boiling point and why?
1.Write the electronic configuration of group 15 element. 2.Phosphine has lower boiling point than ammonia. why. 3.Explain Habers process for ammonia.with condition.
1.TO PREPARE STRUCTURAL DIAGRAM OF HYDRIDE OF NITROGEN AND PHOSPHOROUS. 2.WRITE TEN REASONING QUESTIONS FROM THE TOPIC.