Identify the compounds $A, X$ and $Z$ in the following reactions.
$$A+2 \mathrm{HC}+5 \mathrm{H}_2 \mathrm{O} \longrightarrow 2 \mathrm{NaC}+X$$
$X \xrightarrow[370 \mathrm{~K}]{\Delta} \mathrm{HBO}_2 \underset{>370 \mathrm{~K}}{\stackrel{\Delta}{\longrightarrow}} Z$
(i) $$\mathop {N{a_2}{B_4}{O_7}}\limits_{Borax\,(A)} + 2HCl + 5{H_2}O \to 2NaCl + \mathop {4{H_3}B{O_3}}\limits_{Orthoboric\,acid\,(X)} $$
(ii) $${H_3}B{O_3}\buildrel {\Delta ,\,370\,K} \over \longrightarrow \mathop {HB{O_2}}\limits_{Metaboric\,acid} + {H_2}O$$
(iii) $$4HB{O_2}\mathrel{\mathop{\kern0pt\longrightarrow} \limits_{ - {H_2}O}^{\Delta > 370\,K}} \mathop {[{H_2}{B_4}{O_7}]}\limits_{Tetraboric\,acid} \mathrel{\mathop{\kern0pt\longrightarrow} \limits_{Heat}^{{\mathop{\rm Re}\nolimits} d}} \mathop {2{B_2}{O_3} + {H_2}O}\limits_{Boron\,trioxide\,(Z)} $$
Complete the following chemical equations.
$$\begin{gathered} \mathrm{Z}+3 \mathrm{LiAlH}_4 \longrightarrow X+3 \mathrm{LiF}+3 \mathrm{AlF}_3 \\ X+6 \mathrm{H}_2 \mathrm{O} \longrightarrow Y+6 \mathrm{H}_2 \\ 3 X+3 \mathrm{O}_2 \xrightarrow{\Delta} \mathrm{B}_2 \mathrm{O}_3+3 \mathrm{H}_2 \mathrm{O} \end{gathered}$$
(i) $$4B{F_3} + 3LiAl{H_4} \to \mathop {2{B_2}{H_6}}\limits_{Diborane\,(X)} + 3LiF + 3Al{F_3}$$
(ii) $$\mathop {{B_2}{H_6}}\limits_{(X)} + 6{H_2}O \to \mathop {2{H_3}B{O_3}}\limits_{Orthoboric\,acid} + 6{H_2}$$
(iii) $$\mathop {{B_2}{H_6}}\limits_{(X)} + 3{O_2}\buildrel \Delta \over \longrightarrow {B_2}{O_3} + 3{H_2}O$$
Match the species given in Column I with the properties mentioned in Column II.
| Column I | Column II | ||
|---|---|---|---|
| A. | BF$$_4^-$$ | 1. | Oxidation state of central atom is +4 |
| B. | AlCl$$_3$$ | 2. | Strong oxidising agent |
| C. | SnO | 3. | Lewis acid |
| D. | PbO$$_2$$ | 4. | Can be further oxidised |
A. $\rightarrow$ (5)
B. $\rightarrow$ (3)
C. $\rightarrow$ (4)
D. $\rightarrow(1,2)$
A. $\mathrm{BF}_4^{-}$Tetrahedral shape $s p^3$ hybridisation regular geometry.
B. $\mathrm{AlCl}_{3^{-}}$Octet not complete of Al , act as Lewis acid.
C. $\mathrm{SnO}^3 \mathrm{Sn}^{2+}$ can show +4 oxidation state.
D. $\mathrm{PbO}_2$ Oxidation state of Pb in $\mathrm{PbO}_2$ is +4 . Due to inert pair effect $\mathrm{Pb}^{4+}$ is less stable than $\mathrm{Pb}^{2+}$, acts as strong oxidising agent.
Match the species given in Column I with properties given in Column II.
| Column I | Column II | ||
|---|---|---|---|
| A. | Diborane | 1. | Used as a flux for soldering metals |
| B. | Gallium | 2. | Crystalline form of silica |
| C. | Borax | 3. | Banana bonds |
| D. | Aluminosilicate | 4. | Low melting, high boiling, useful for measuring high temperatures |
| E. | Quartz | 5. | Used as catalyst in petrochemical industries |
A. $\rightarrow$ (3)
B. $\rightarrow$ (4)
C. $\rightarrow$ (1)
D. $\rightarrow$ (5)
E. $\rightarrow$ (2)
A. $\mathrm{BH}_3$ is unstable forms diborane $\mathrm{B}_2 \mathrm{H}_6$ by 3 centre -2 electron bond show banana bond.
B. Gallium with low melting point and high boiling point makes it useful to measure high temperatures.
C. Borax is used as a flux for soldering metals for heat, scratch resistant coating in earthernwares.
D. Alumino silicate used as catalyst in petrochemical industries.
E. Quartz, is a crystalline form of silica.
Match the species given in Column I with the hybridisation given in Column II.
| Column I | Column II | ||
|---|---|---|---|
| A. | Boron in [B(OH$$_4$$)]$$^-$$ | 1. | sp$$^2$$ |
| B. | Aluminium in $\left[\mathrm{Al}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{3+}$ | 2. | sp$$^3$$ |
| C. | Boron in B$$_2$$H$$_6$$ | 3. | sp$$^3$$d$$^2$$ |
| D. | Carbon in buckminster fullerene | ||
| E. | Silicon in SiO$$_4^{-4}$$ | ||
| F. | Germanium in $\left[\mathrm{GeCl}_6\right]^{2-}$ |
A. $\rightarrow(2)$
B. $\rightarrow$ (3)
C. $\rightarrow(2)$
D. $\rightarrow$ (1)
E. $\rightarrow(2)$
F. $\rightarrow(3)$
A. Boron in $\left[\mathrm{B}(\mathrm{OH})_4\right]^{-} s p^3$ hybridised.
B. Aluminium in $\left[\mathrm{Al}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{3+} s p^3 d^2$ hybridised.
C. Boron in $\mathrm{B}_2 \mathrm{H}_6 s p^3$ hybridised.
D. Carbon in Buckminsterfullerene $s p^2$ hybridised.
E. Silicon in $\mathrm{SiO}_4^{4-} s p^3$ hybridised.
F. Germanium in $\left[\mathrm{GeCl}_6\right]^{2-} s p^3 d^2$ hybridised.