Fluorine exhibits an oxidation state of only -1 because:
it can readily accept an electron
it is very strongly electronegative
it is a non-metal
it belong to halogen family
Which among the following factors is the most important in making fluorine the strongest oxidizing agent ?
Electron affinity
Ionization enthalpy
Hydration enthalpy
Bond dissociation energy
Which one of the following compounds, is not a protonic acid ?
SO(OH)2
SO2(OH)2
B(OH)3
PO(OH)3
C.
B(OH)3
B(OH)3 is not protonic acid because it does not give proton on ionisation directly while it acts as Lewis acid due to acceptance of OH- from water and forms a hydrated species.
B(OH)3 + H2O → [B(OH)4]- + H+
The oxidation states of iodine in HIO4 H3IO5 and H5IO6, are respectively :
+ 1, + 3, + 7
+ 7, + 7, + 3
+ 7, + 7, + 7
7, + 5, + 3
Amphoteric-oxide combinations are in:
ZnO, K2O, SO3
ZnO, P2O5, Cl2O7
SnO2, Al2O3, ZnO
PbO2, SnO2, SO3