1. | The acidic strength of HX (X=F, Cl, Br and I) follows the order: HF > HCI > HBr >HI |
2. | Fluorine exhibits - 1 oxidation state whereas other halogens exhibit +1, +3, +5 and +7 oxidation states also. |
3. | The enthalpy of dissociation of F2 is smaller than that of Cl2. |
4. | Fluorine is stronger oxidising agent than chlorine. |
List-I (Atom/Molecule) |
List-II (Property) |
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A. | Nitrogen | I. | Paramagnetic |
B. | Fluorine molecule | II. | Most reactive element in group 18 |
C. | Oxygen molecule | III. | Element with highest ionisation enthalpy in group 15 |
D. | Xenon atom | IV. | Strongest oxidising agent |
1. | A- III, B-I, C-IV, D-II | 2. | A-I, B-IV, C-III, D-II |
3. | A-II, B-IV, C-I, D-II | 4. | A-III, B-IV, C-I, D-II |
List-I (Oxoacids of Sulphur) |
List-II (Bonds) |
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A. | Peroxodisulphuric acid | I. | Two S-OH, Four S=O, One S-O-S |
B. | Sulphuric acid | II. | Two S-OH, One S=O |
C. | Pyrosulphuric acid | III. | Two S-OH, Four S=O, One S-O-O-S |
D. | Sulphurous acid | IV. | Two S-OH, Two S=O |
Options: | A | B | C | D |
1. | III | IV | II | I |
2. | I | III | II | IV |
3. | III | IV | I | II |
4. | I | III | IV | II |
(a) | F–F bond has a low enthalpy of dissociation. |
(b) | Flouride ion (F–) has high hydration enthalpy. |
(c) | Electron gain enthalpy of fluorine is less negative than chlorine. |
(d) | Fluorine has a very small size. |
1. | (a) and (b) only | 2. | (a) and (c) only |
3. | (a) and (d) only | 4. | (b) and (c) only |
1. | \(\mathrm{NaNO}_3+\mathrm{H}_2 \mathrm{SO}_4\xrightarrow[500~K, \ 9\text{ bar}]{Pt} \mathrm{NaHSO}_4+\mathrm{HNO}_3\) |
2. | \(4 \mathrm{NH}_3+5 \mathrm{O}_2 \text{(from air)}\xrightarrow[500~K, \ 9\text{ bar}]{Pt} 4 \mathrm{NO}+6 \mathrm{H}_2 \mathrm{O}\) |
3. | \(4 \mathrm{HPO}_3+2 \mathrm{~N}_2 \mathrm{O}_5\xrightarrow[500~K, \ 9\text{ bar}]{Pt} 4 \mathrm{HNO}_3+\mathrm{P}_4 \mathrm{O}_{10}\) |
4. | \(\mathrm{Cu}\left(\mathrm{NO}_3\right)_2+2 \mathrm{NO}_2+2 \mathrm{H}_2 \mathrm{O} \\ \xrightarrow[500~K, \ 9\text{ bar}]{Pt} 4 \mathrm{HNO}_3+\mathrm{Cu}\) |