General
✓✗Dioxygen is paramagnetic. This is explained by
- its double bond in the Lewis structure
- its linear shape
- its high bond energy
- molecular orbital theory, which shows two unpaired electrons
General
✓✗Which of the following species has the same shape as XeF2?
- H2O
- I3−
- SO2
- NO2
General
✓✗Oxygen exists as O2 whereas sulphur exists as S8 because
- sulphur is more electronegative
- sulphur cannot form any covalent bonds
- oxygen has d orbitals
- oxygen forms strong pπ−pπ bonds, but sulphur prefers single bonds and catenation
General
✓✗Arrange the following in increasing order of electronegativity: N, P, As
- N < P < As
- As < P < N
- N < As < P
- P < As < N
General
✓✗The bond dissociation enthalpy of F2 is lower than that of Cl2 because
- F is larger than Cl
- of strong repulsion between the lone pairs of the small F atoms
- F is less electronegative than Cl
- F−F is a double bond
General
✓✗The radioactive element of group 16 is
- tellurium
- selenium
- polonium
- sulphur
General
✓✗In the Ostwald process for the manufacture of nitric acid, the first step is
- catalytic oxidation of NH3 to NO over Pt/Rh gauze at about 500 K and 9 bar
- reduction of HNO2
- direct combination of N2 and O2
- heating NaNO3 with H2SO4
General
✓✗Assertion: PCl5 is more covalent than PCl3.
Reason: P in the +5 oxidation state has a higher polarising power than P in the +3 state.
Reason: P in the +5 oxidation state has a higher polarising power than P in the +3 state.
- Both Assertion and Reason are true and Reason is the correct explanation of Assertion
- Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
- Assertion is true but Reason is false
- Both Assertion and Reason are false
General
✓✗The boiling points of the hydrogen halides vary in the order HF > HI > HBr > HCl. What explains the higher boiling point of hydrogen fluoride?
- The effect of nuclear shielding is much reduced in fluorine, which polarises the HF molecule
- There is strong hydrogen bonding between HF molecules
- The electronegativity of fluorine is much higher than that of the other elements in the group
- The bond energy of HF molecules is greater than in the other hydrogen halides
General
✓✗The oxoacids of fluorine are limited to
- HOF only
- four oxoacids like chlorine
- HOF and HOFO
- no oxoacids at all
General
✓✗The first noble gas compound prepared by Neil Bartlett was
- XeF2
- Xe+PtF6−
- XeO3
- XeF4
General
✓✗Hydrofluoric acid is a weak acid in water mainly because
- HF is non-polar
- HF is a gas
- the H−F bond is very strong
- F− is a large ion
General
✓✗Assertion: Oxygen shows a +2 oxidation state in OF2.
Reason: Fluorine is more electronegative than oxygen.
Reason: Fluorine is more electronegative than oxygen.
- Both Assertion and Reason are true and Reason is the correct explanation of Assertion
- Both Assertion and Reason are true but Reason is not the correct explanation of Assertion
- Assertion is true but Reason is false
- Both Assertion and Reason are false
General
✓✗Match List I (element) with List II (property).
Choose the correct answer from the options given below.
| List I | List II |
| P. Fluorine | I. Most negative electron gain enthalpy |
| Q. Chlorine | II. Highest electronegativity |
| R. Iodine | III. Radioactive noble gas |
| S. Radon | IV. Solid halogen at room temperature |
- P-II, Q-I, R-IV, S-III
- P-I, Q-II, R-IV, S-III
- P-II, Q-IV, R-I, S-III
- P-III, Q-I, R-IV, S-II
General
✓✗Among the group 16 hexafluorides, SF6 is exceptionally inert mainly because
- S has no lone pair
- six F atoms sterically protect the S atom
- S−F bonds are ionic
- it is a liquid