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प्रश्न
Why are halogens coloured?
Why are all halogens coloured?
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उत्तर
Almost all halogens are coloured. This is because halogens absorb radiation in the visible region. This results in the excitation of valence electrons to a higher energy region. Since the amount of energy required for excitation differs for each halogen, each halogen displays a different colour.
संबंधित प्रश्न
Iodine exists as
- polar molecular solid
- ionic solid
- nonpolar molecular solid
- hydrogen bonded molecular solid
Draw structure of Chlorine pentafluoride
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
Give two examples to show the anomalous behaviour of fluorine.
With what neutral molecule is ClO− isoelectronic? Is that molecule a Lewis base?
Complete chemical reactions are:Cl2 + H2O →
Select the correct alternative from the choices given :
The correct order of increasing acidic strength of the oxoacids of chlorine is:
Tincture of iodine is ____________.
Which is the strongest acid in the following:
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 |
In solid state \[\ce{PCl5}\] is a ______.
Reduction potentials of some ions are given below. Arrange them in decreasing order of oxidising power.
| Ion | \[\ce{CIO^{-}_{4}}\] | \[\ce{IO^{-}_{4}}\] | \[\ce{BrO^{-}_{4}}\] |
| Reduction potential EΘ/V |
EΘ = 1.19 V | EΘ = 1.65V | EΘ = 1.74 V |
Give reason to explain why ClF3 exists but FCl3 does not exist.
Solubility of iodine in water may be increase by adding
The reaction \[\ce{3ClO- (aq) -> ClO3- (aq) + 2Cl- (aq) + 2Cl- (aq)}\] is an example of
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.
