Q. No.Which of the following Group 15 elements forms the strongest bond with hydrogen?
| 1. | N | 2. | P |
| 3. | As | 4. | Sb |
Which of the following correctly explains why NH₃ is highly soluble in water, whereas PH₃ is only sparingly soluble?
| 1. | NH3 forms an H-bond with water, so it is soluble but PH3 does not form an H-bond. |
| 2. | NH3 does not form an H-bond with water, so it is soluble but PH3 does form an H-bond. |
| 3. | NH3 and PH3 both form H-bond with water. |
| 4. | NH3 and PH3 both do not form H-bond with water. |
Which of the following types of π-bonding is present in the N₂ molecule?
1. \(p\pi-p\pi\)
2. \(p\pi-d\pi\)
3. \(d\pi-d\pi\)
4. Only sigma bond
Which of the following Group 15 elements does not have a d-orbital in its valence shell?
| 1. | P | 2. | N |
| 3. | As | 4. | Bi |
Which of the following correctly explains why NH₃ forms hydrogen bonds whereas PH₃ does not?
| 1. | Phosphorus is more electronegative as compared to nitrogen. |
| 2. | Nitrogen is more electronegative as compared to phosphorus. |
| 3. | Nitrogen and phosphorous have equal electronegativity. |
| 4. | Nitrogen is more stable as compared to phosphorus. |
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) |
Match the formulas of oxides given in Column I with the type of oxide given in Column II and mark the correct option.
| Column I | Column II |
| A. Pb3O4 | 1. Neutral oxide |
| B. N2O | 2. Acidic oxide |
| C. Mn2O7 | 3. Basic oxide |
| D. Bi2O3 | 4. Mixed oxide |
Codes
| A | B | C | D | |
| 1. | 1 | 2 | 3 | 4 |
| 2. | 4 | 1 | 2 | 3 |
| 3. | 3 | 2 | 4 | 1 |
| 4. | 4 | 3 | 1 | 2 |
The respective oxidation states of P in H4P2O5, H4P2O6, and H4P2O7 are:
| 1. | +3, +5, and +4 | 2. | +5, +3, and +4 |
| 3. | +5, +4, and +3 | 4. | +3, +4, and +5 |
Which of the following equations correctly represents the catalytic oxidation of ammonia by atmospheric oxygen ?
| 1. | 4NH3 + \(\underset{\text{From air}}{5O_2} \) \(\xrightarrow[\text{500 K; 9 bar}]{\text{Pt / Rh gauge catalyst}}\) 4NO + 6H2O |
| 2. | 3NH4 + \(\underset{\text{From air}}{5O_2} \) \(\xrightarrow[\text{500 K; 9 bar}]{\text{Pt / Rh gauge catalyst}}\) 3NO + 6H2O |
| 3. | 4NH3 + \(\underset{\text{From air}}{5O_2} \) \(\xrightarrow[\text{cold}]{\text{no catalyst}}\) 4NO + 6H2O |
| 4. | 3NH4 + \(\underset{\text{From air}}{5O_2} \) \(\xrightarrow[\text{cold}]{\text{no catalyst}}\) 3NO + 6H2O |
Which of the following is the correct electronic configuration of the element belonging to Group 15 and Period 3 of the periodic table?
1. \(\mathrm{1 s^2 2 s^2 2 p^4} \)
2. \(\mathrm{1 s^2 2 s^2 2 p^3} \)
3. \(\mathrm{1 s^2 2 s^2 2 p^6 3 s^2 3 p^2} \)
4. \(\mathrm{1 s^2 2 s^2 2 p^6 3 s^2 3 p^3}\)
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