Explanation
Due to H –bonding, NH3 has a much higher b. p. than PH3
Out of P, Sb, B and As , phosphorus has highest electronegativity and therefore, its oxide P2O3 will be most acidic.
Both NH3 and PH3 are basic in nature; the former is more basic than the latter. Odour of both is different and also NH3 is not combustile whereas PH3 undergoes combustion.
Basic character of hydrides decreases down the group. Thus PH3 is less basic than NH3.
In PCl5 , P is sp3d-hybridized
The phenomenon of phosphoresence shown by white phosphorus is called ‘cold fire’ and also the disease caused by the constant touch with white phosphorus is called ‘Phossy jaw’.
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SO2 is highly soluble in water and therefore cannot be collected over water.
In SO2 molecule, S is sp2-hybridized,one of the hybrid orbitals contains a lone pair of electrons due to which the O – S – O bond angle is slightly reduced to 119.50 giving a V- shape to the molecule.
SO3 + H2O → H2SO4 ; thus SO3 is acidic in nature.
(a) SO2.
S in H2S because of its lower electro – negativitiy does not form hydrogen bonding.
Geometry of H2S is angular like H2O molecule and it has a particular value of dipole moment.
CO2 cannot be further oxidised hence it cannot act as a reducing agent.
H2S is a weak acid in water and not a weak base.
SO2 contains two σ bonds, two π (pπ - p π and p π -dπ ) bonds and one lone pair of electrons on S atom.
The oxidation number of S in H2S2O8 is + 6 as it contains one peroxo (-O-O-) linkage.
Noble gases are monoatomic
Both He (1s2) and Li+ (1s2) have two electrons (dielectron species) and thus their spectrum would be similar
As odd oxidation state of xenon is not formed, it can not form XeF3.
Atoms of noble gases are held together by weak vander Waals forces of attraction.
In the clathrate of Xe with water, the nature of bonding between Xe and H2O is dipole induced dipole interaction
XeF4 on partial hydrolysis produces XeOF2 as shown below XeF4 + H2O → XeOF2 + 2HF
Peaks represent the highest values. Since noble gases have highest ionization energy values in their respective periods, these occupy peak position in the ionization energy curve.
In XeF2 Xe is sp3d hybridized with all the three equatorial positions occupied by lone pairs of electrons giving a linear shape to XeF2.
XeF4 has square planar structure.
Xe posses three lone pairs of electrons in equatorial positions in XeF2
XeF2 and CO2 both have linear (identical) shapes
XeO3 is an explosive compound when dry and its explosion power is 22 times more than TNT
(d) He
Because of higher bond dissociation energy due to smaller H-Cl bond,HCl is most stable to heat.
CN‒ behaves like a halide ion but is not a true halide and is called pseudohalide.
Since HF is the weakest reducing agent of all hydracids (hydrides) ofhalogens, it cannot reduce H2SO4, KMnO4 and K2Cr2O7.
Hydrogen bonding is strongest between H atom of one molecule and most electronegative atom of the other molecule.
Chlorine is stronger oxidising agent than bromine therefore, chlorine water will liberate bromine from KBr solution
2KBr + Cl2 → 2KCl + Br2
The more the electronegativity and oxidation number of the central atom (here Cl), the higher is the acidity.
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