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Match the following graphical variation with their description.
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- Which orbital is non-directional?
- What are the frequency and wavelength of a photon emitted during a transition from n = 5 state to n = 2 state in the hydrogen atom?
Predict the hybridization of each carbon in the molecule of organic compound given below. Also indicate the total number of sigma and pi bonds in this molecule.
Consider the reactions :
a. $6 CO _2(g)+6 H _2 O ( I ) \longrightarrow C _6 H _{12} O _6( aq )+6 O _2(g)$
b. $O _3(g)+ H _2 O _2( I ) \longrightarrow H _2 O ( I )+2 O _2(g)$
Why it is more appropriate to write these reactions as :
a. $6 CO _2+12 H _2 O ( I ) \longrightarrow C _6 H _{12} O _6( aq )+6 H _2 O ( I )+6 O _2(g)$
b. $O _3(g)+ H _2 O _2( I ) \longrightarrow H _2 O ( I )+ O _2(g)+ O _2(g)$
Also suggest a technique to investigate the path of the above (a) and (b) redox reactions.
→a. $6 CO _2(g)+6 H _2 O ( I ) \longrightarrow C _6 H _{12} O _6( aq )+6 O _2(g)$
b. $O _3(g)+ H _2 O _2( I ) \longrightarrow H _2 O ( I )+2 O _2(g)$
Why it is more appropriate to write these reactions as :
a. $6 CO _2+12 H _2 O ( I ) \longrightarrow C _6 H _{12} O _6( aq )+6 H _2 O ( I )+6 O _2(g)$
b. $O _3(g)+ H _2 O _2( I ) \longrightarrow H _2 O ( I )+ O _2(g)+ O _2(g)$
Also suggest a technique to investigate the path of the above (a) and (b) redox reactions.
What happens:
→- When $\mathrm{F}_2$ reacts with hot water
- Barium peroxide reacts with phosphoric acid
- Hydrogen peroxide reacts with ozone.
Consider the reactions:$2\text{S}_2\text{O}^{2-}_{3}(\text{aq})+\text{I}_2(\text{s})\rightarrow\text{S}_4\text{O}^{2-}_{6}(\text{aq})+2\text{I}^{-}(\text{aq})$
$\text{S}_2\text{O}^{2-}_{3}(\text{aq})+2\text{Br}_2(\text{l})+5\text{H}_2\text{O(l)}\rightarrow\\2\text{SO}^{2-}_{4}(\text{aq})+4\text{Br}^{-}(\text{aq})+10\text{H}^+(\text{aq})$
Why does the same reductant, thiosulphate react differently with iodine and bromine?
→$\text{S}_2\text{O}^{2-}_{3}(\text{aq})+2\text{Br}_2(\text{l})+5\text{H}_2\text{O(l)}\rightarrow\\2\text{SO}^{2-}_{4}(\text{aq})+4\text{Br}^{-}(\text{aq})+10\text{H}^+(\text{aq})$
Why does the same reductant, thiosulphate react differently with iodine and bromine?
If $6.022 \times 10^{23}$ molecules of $\mathrm{N}_2$, react completely with $\mathrm{H}_2$ according to the equation:
$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$
then calculate the number of molecules of $\mathrm{NH}_3$ formed.
→$\mathrm{N}_2(\mathrm{~g})+3 \mathrm{H}_2(\mathrm{~g}) \rightarrow 2 \mathrm{NH}_3(\mathrm{~g})$
then calculate the number of molecules of $\mathrm{NH}_3$ formed.
What happens when:
→- Mg is burnt in air?
- $\mathrm{Cl}_2(\mathrm{g})$ reacts with slaked lime?
Give one method of preparation of $\mathrm{H}_2 \mathrm{O}_2$. Write chemical reactions to justify that $\mathrm{H}_2 \mathrm{O}_2$ can function as an oxidising as well as reducing agent. Write its two uses.
→Which of the two: $\mathrm{O}_2 \mathrm{NCH}_2 \mathrm{CH}_2 \mathrm{O}$ - or $\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{O}$ - is expected to be more stable and why?
→What are the oxidation number of the underlined elements in the following and how do you rationalise your results?
$KI_3$
→$KI_3$