Q. No.Match the species given in Column I with the shape given in Column II and mark the correct option:
| Column I (Species) | Column II (Shape) | ||
| A. | \(\mathrm{SF}_4\) | (I) | Tetrahedral |
| B. | \(\mathrm{BrF}_3\) | (II) | Pyramidal |
| C. | \(\mathrm{BrO}_3^{-}\) | (III) | Sea-saw shaped |
| D. | \(\mathrm{NH}_4^{+}\) | (IV) | Bent T-shaped |
Codes:
| A | B | C | D | |
| 1. | III | II | I | IV |
| 2. | III | IV | II | I |
| 3. | I | II | III | IV |
| 4. | I | IV | III | II |
Given below are two statements:
| Assertion (A): | Fluorine exhibits only –1 oxidation state whereas other halogens exhibit +1, +3, +5 and +7 oxidation states. |
| Reason (R): | Other halogens possess d-orbitals and can expand their octet to exhibit higher oxidation states |
Choose the correct option:
| 1. | Both (A) and (R) are true and (R) is the correct explanation of (A). |
| 2. | Both (A) and (R) are true but (R) is not the correct explanation of (A). |
| 3. | (A) is true but (R) is false. |
| 4. | (A) is false but (R) is true. |
The structure of IF7 is :
1. Square pyramidal
2. Trigonal bipyramidal
3. Octahedral
4. Pentagonal bipyramidal
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:
| Options: | A | B | C | D |
| 1. | 1 | 2 | 3 | 4 |
| 2. | 4 | 1 | 2 | 3 |
| 3. | 3 | 2 | 4 | 1 |
| 4. | 4 | 3 | 1 | 2 |
Column II and mark the appropriate option.
| Column-I | Column-II | ||
| a. | Chloroform | (i) | H2S2O7 |
| b. | Mustard gas | (ii) | \(CHCl_3 \) |
| c. | Phosgene | (iii) | \(ClCH_2CH_2SCH_2CH_2Cl \) |
| d. | Oleum | (iv) | \(COCl_2 \) |
1. a(iv), b(iii), c(ii), d(i)
2. a(ii), b(iii), c(i), d(iv)
3. a(i), b(ii), c(iii), d(iv)
4. a(ii), b(iii), c(iv), d(i)
Which of the following accounts for the highly negative electron gain enthalpy of halogens in their respective periods of the periodic table?
1. It has smallest size and high effective nuclear charge
2. It has the largest size in in the respective periods
3. It is a strong reducing agent
4. None of the above
| Assertion (A): | The bond dissociation enthalpy of Cl2 is higher than F2 . |
| Reason (R): | Larger electron-electron repulsion among the lone pair in F2 molecule. |
| 1. | Both (A) and (R) are correct and (R) is the correct explanation of (A) |
| 2. | Both (A) and (R) are correct but (R) is not the correct explanation of (A) |
| 3. | (A) is True but (R) is False. |
| 4. | (A) is False but (R) is True. |
| 1. | Fluorine is stronger oxidising agent than chlorine. |
| 2. | Fluorine is weaker oxidising agent than chlorine. |
| 3. | Fluorine is stronger reducing agent than chlorine. |
| 4. | Bond dissociation energy of fluorine is more than chlorine. |
Arrange the following compounds in increasing order of their acidity:
HF, HCl, HBr, HI
1. HCl < HBr < HI<HF
2. HF < HCl < HI< HBr
3. HF < HCl < HBr < HI
4. HF< HBr < HI< HCl
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