Question
Explain the following:
$\mathrm{TI}\left(\mathrm{NO}_3\right)_3$ acts as an oxidising agent.
$\mathrm{TI}\left(\mathrm{NO}_3\right)_3$ acts as an oxidising agent.
✓
Answer
Due ta strong inert pair effect, the +3 oxidation state of TI is less stable than its +1 oxidation state. Since in $\mathrm{TI}\left(\mathrm{NO}_3\right)_3$, oxidation state of TI is +3 , therefore, it can easily gain two electrons to form $\mathrm{TINO}_3$ in which the oxidation state of TI is +1 . Consequently, $\mathrm{TI}\left(\mathrm{NO}_3\right)_3$ acts as an oxidising agent.
Need a full question paper?
Generate a complete, print-ready paper with questions like this in minutes — across 16+ boards, with answer keys.
Explore more
Similar questions
On the basis of intermolecular forces and thermal energy, explain why?
- A solid has rigidity but liquids do not have rigidity?
- Gases have high compressibility but liquids and solids have poor compressibility?
Write the electronic configuration of ${ }_9 \mathrm{~F}^{19},{ }_{16} \mathrm{~S}^{32}$ and ${ }_{18} \mathrm{Ar}^{38}$ and then point out the element with:
→- Maximum nuclear charge.
- Minimum number of neutrons.
- Maximum number of unpaired electrons.
- A gaseous mixture contains 2.2bar He, 1.1bar $\mathrm{H}_2$ and 4.2bar $\mathrm{N}_2$. What is mole fraction of $\mathrm{N}_2$?
- Which has higher viscosity ether or water? Why?
An atom of an element contains $29$ electrons and $35$ neutrons. Deduce
→- The number of protons
- The electronic configuration of the element.
Calculate the temperature above which the reduction of lead oxide in the following reaction becomes spontaneous:
PbO(s) + C(s) → Pb(s) + CO(g)
Given: $[\Delta\text{H}=108.4\text{kJ mol}^{-1};\ \Delta\text{S}=190\text{J K}^{-1}\text{mol}^{-1}]$
→PbO(s) + C(s) → Pb(s) + CO(g)
Given: $[\Delta\text{H}=108.4\text{kJ mol}^{-1};\ \Delta\text{S}=190\text{J K}^{-1}\text{mol}^{-1}]$
Write the name of following compounds using derive system :
How would you convert the following compound into benzene?
Ethene.
Ethene.
Calculate the mole fraction of $20 \%$ (w/w) ethylene glycol $\left( C _2 H _6 O _2\right)$ (Molar mass of $C _2 H _6 O _2=62$ )
→The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
What will be the pOH of $\frac{ M }{100} \quad H _2 SO _4$ solution ?
→