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प्रश्न
Which of the following statements are true?
(i) Only type of interactions between particles of noble gases are due to weak dispersion forces.
(ii) Ionisation enthalpy of molecular oxygen is very close to that of xenon.
(iii) Hydrolysis of XeF6 is a redox reaction.
(iv) Xenon fluorides are not reactive.
उत्तर
(i) Only type of interactions between particles of noble gases are due to weak dispersion forces.
(ii) Ionisation enthalpy of molecular oxygen is very close to that of xenon.
Explanation:
Weak dispersion forces are present between particles of noble gases. The Ionization enthalpy of molecular oxygen is very close to that of xenon.
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संबंधित प्रश्न
Account for the following: Fluorine does not exhibit positive oxidation state.
F2 has lower bond dissociation enthalpy than Cl2. Why?
Which halogen compound in each of the following pairs will react faster in SN2 reaction
(CH3)3 C – Cl or CH3 – Cl
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Arrange the following in the order of property indicated for each set:
HF, HCl, HBr, HI - increasing acid strength.
Which of the following pairs of ions are isoelectronic and isostructural?
Bond dissociation enthalpy of E–H (E = element) bonds is given below. Which of the compounds will act as the strongest reducing agent?
| Compound | \[\ce{NH3}\] | \[\ce{PH3}\] | \[\ce{AsH3}\] | \[\ce{SbH3}\] |
| Δdiss (E – H)/kJ mol–1 | 389 | 322 | 297 | 255 |
Give reason to explain why ClF3 exists but FCl3 does not exist.
Statement I: Acid strength increases in the order given as HF << HCl << HBr << HI.
Statement II: As the size of the elements F, Cl, Br, and I increase down the group, the bond strength of HF, HCl, HBr, and HI decreases and so the acid strength increases.
In the light of the above statements, choose the correct answer from the options given below.
Write the name and formula of oxoacid of fluorine.
