Oxidation states of P in H4P2O5, H4P2O6, H4P2O7, are respectively:
1. | +3, +5, +4 | 2. | +5, +3, +4 |
3. | +5, +4, +3 | 4. | +3, +4, +5 |
Among the following which is the strongest oxidising agent?
1.
2.
3.
4.
The electronegativity difference between N and F is greater than that between N and H yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2 D). This is because:
1. | In NH3 as well as in NF3 the atomic dipole and bond dipole are in the same direction |
2. | In NH3 the atomic dipole and bond dipole are in the same direction whereas in NF3 these are in opposite directions |
3. | In NH3 as well as in NF3 the atomic dipole and bond dipole are in opposite directions |
4. | In NH3 the atomic dipole and the bond dipole is in opposite directions whereas in NF3 these are in the same directions |
Which of the following compounds has the lowest melting point?
1.
2.
3.
4.
Sulphur trioxide can be obtained by which of the following reaction:
1.
2.
3.
4.
The incorrect statement regarding oxoacids of phosphorus is:
1. | Orthophosphoric acid is used in the manufacture of triple superphosphate. |
2. | Hypophosphorous acid is a diprotic acid. |
3. | All oxoacids contain tetrahedral four coordinated phosphorus. |
4. | All oxoacids contain at least one P=O unit and one P-OH group. |
Which of the following compounds does not release oxygen when heated?
1. Zn(ClO3)2
2. K2Cr2O7
3. (NH4)2Cr2O7
4. KClO3
The acidity of diprotic acids in aqueous solution increases in the order:
1. H2S < H2Se < H2Te
2. H2Se < H2S < H2Te
3. H2Te < H2S < H2Se
4. H2Se < H2Te < H2S
The strong reducing behaviour of H3PO2 is due to:
1. Presence of one -OH group and two P-H bonds.
2. High electron gain enthalpy of phosphorus.
3. High oxidation state of phosphorus.
4. Presence of two -OH groups and one P-H bond.