Q. No.The variation of the boiling point of the hydrogen halides is in the order HF > HI > HBr > HCl.
The higher boiling point of hydrogen fluoride is explained as:
1.
The electronegativity of flourine is much higher than other elements in group
2.
There is strong hydrogen bonding between HF molecules
3.
The bond energy of HF molecules is greater than in other hydrogen halides
4.
The effect of nuclear shielding is much reduced in flourine which polarizes the HF molecule
The higher boiling point of hydrogen fluoride is explained as:
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.
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
Which of the following compounds does not release oxygen when heated?
1. Zn(ClO3)2
2. K2Cr2O7
3. (NH4)2Cr2O7
4. KClO3
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. |
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 |
The correct thermal stability order for \(\mathrm{{H}_2 {E}},\) \(\mathrm{{ E}= {O}, {S}, {Se}, {Te}} \text { and } \mathrm{Po}\) among the following is:
1. \(\mathrm{{H}_2 {Se}<{H}_2 {Te}<{H}_2 {Po}<{H}_2 {O}<{H}_2 S}\)
2. \(\mathrm{{H}_2 {~S}<{H}_2 {O}<{H}_2 {Se}<{H}_2 {Te}<{H}_2 {Po}}\)
3. \(\mathrm{{H}_2 {O}<{H}_2 {~S}<{H}_2 {Se}<{H}_2 {Te}<{H}_2 {PO}}\)
4. \(\mathrm{{H}_2 {Po}<{H}_2 {Te}<{H}_2 {Se}<{H}_2 {~S}<{H}_2 {O}}\)
Match the Xenon compounds in Column I with their structure in Column II and assign the correct code:
| Column I | Column II | ||
| (a) | XeF4 | (i) | Pyramidal |
| (b) | XeF6 | (ii) | Square planar |
| (c) | XeOF4 | (iii) | Distorted octahedral |
| (d) | XeO3 | (iv) | Square pyramidal |
Code:
| (a) | (b) | (c) | (d) | |
| 1. | (iii) | (iv) | (i) | (ii) |
| 2. | (i) | (ii) | (iii) | (iv) |
| 3. | (ii) | (iii) | (iv) | (i) |
| 4. | (ii) | (iii) | (i) | (iv) |
Match the name of process given in Column I with the name of compound given in Column II and mark the correct option.
| Column I | Column II | ||
| (a) | Pure nitrogen | (i) | Chlorine |
| (b) | Haber process | (ii) | Sulphuric acid |
| (c) | Contact process | (iii) | Ammonia |
| (d) | Deacon's process | (iv) | Sodium azide or Barium azide |
| (a) | (b) | (c) | (d) | |
| 1. | (iv) | (iii) | (ii) | (i) |
| 2. | (i) | (ii) | (iii) | (iv) |
| 3. | (ii) | (iv) | (i) | (iii) |
| 4. | (iii) | (iv) | (ii) | (i) |
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