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Decreasing order of reducing power hydrogen halides is:
reducing tendency of HYDRA acid increase down the group,due to increase in bond length
Which one is most basic in character?
Acidic strength is in the order
HI > HBr > HCl > HF
So the conjucate bases are
I- < Br- < Cl- < F-
Thus fluoride ion is the strongest base and iodide ion ​is the weakest base
Which is bad conductor of electricity?
H2F2
Due to the bonding that exists in this compound in aqueous solution, there are no free ions available to conduct electricity. For this reason, H2F2 is a bad conductor of electricity.
HBr and HI reduce sulphuric acid; HCl can reduce and HF reduces:
Fluorine is most electronegative element and its size is very small, so it does not have a tendency to lose electrons. Hence, never behave as a reducing agent. HF is a good oxidising agent.
The hydrogen fluoride is liquid unlike the other hydrogen halides, because:
Hydrogen fluoride (HF) is a liquid at room temperature due to the strong intermolecular hydrogen bonding present between HF molecules. The small size of the fluorine atom allows the hydrogen bond to form easily, resulting in a higher boiling point compared to other hydrogen halides.
The correct order of the thermal stability of hydrogen halide (H-X) is:
(2)
As the size of the halogen atom increases from F to I, H – X bond length in HX molecules also increases from H – F to H – I (H – F < H – Cl < H – Br < H – I).
The increase in H – X bond length decreases the strength of H – X bond from H – F to H – I (H – F > H – Cl > H – Br > H – I). The decrease in the strength of H – X bond is evident from the fact that H – X bond dissociation energies decrease from H – F to H – I.
Due to successive decrease in the strength of H – X bond from H – F to H – I, thermal stability of HX molecules also decreases from HF to HI (HF > HCl > HBr > HI).
Which acid can combine with its own salt again?
is unique in forming acid salts as difluoride ion as forms bond with as
HF present as impurity in gaseous can be removed by passing over:
HF is a Lewis acid and can form a complex with the Lewis base NaF. This complex formation removes HF from the gaseous F2 stream. NaF is commonly used as a desiccant to remove trace amounts of HF from fluorine gas.
Hydrofluoric acid is not preserved in glass bottles because:
When silicon dioxide (SiO2) is heated with hydrogen fluoride (HF), it forms silicon tetrafluoride (SiF4).
Usually the Si-O bond is a strong bond and it resists any attack by halogen and most acids, even at a high temperature, However it is attacked by HF.
SiO2 + 4HF ----→ SiF4 + 2H2O
The SiF4 formed in this reaction can further react with HF to form Hydrofluorosilicic acid.
SiF4 + 2HF -----→ H2SiF6
Pure HF does not attack:
(1)
Hydrofluoric acid won't eat through plastic
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