Which of the following oxidation states of chromium forms the most stable compounds?
- A$Cr(I)$
- B$Cr(II)$
- C$Cr(III)$
- D$Cr(V)$
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Similar Questions
The metal that does not give the borax bead test is
Medium
View Solution$K_2Cr_2O_7 + H_2O_2 \xrightarrow{H^{+}} $
Medium
View SolutionMatch the aqueous solutions given in List-$I$ with their colors given in List-$II$:
List-$I$ (Aqueous solution of salt) List-$II$ (Color) $A$. $FeSO_4 \cdot 7H_2O$ $i$. Green $B$. $NiCl_2 \cdot 4H_2O$ $ii$. Pale pink $C$. $MnCl_2 \cdot 4H_2O$ $iii$. Blue $D$. $CoCl_2 \cdot 6H_2O$ $iv$. Light green $E$. $Cu_2Cl_2$ $v$. Pink $vi$. Colorless
| List-$I$ (Aqueous solution of salt) | List-$II$ (Color) |
| $A$. $FeSO_4 \cdot 7H_2O$ | $i$. Green |
| $B$. $NiCl_2 \cdot 4H_2O$ | $ii$. Pale pink |
| $C$. $MnCl_2 \cdot 4H_2O$ | $iii$. Blue |
| $D$. $CoCl_2 \cdot 6H_2O$ | $iv$. Light green |
| $E$. $Cu_2Cl_2$ | $v$. Pink |
| $vi$. Colorless |
Medium
View SolutionSuperconductors are derived from compounds of
Easy
View SolutionMatch the following:
List-$I$ (Aquated Ion) List-$II$ (Colour) $A. Ni^{2+}$ $I. \text{Violet}$ $B. Fe^{3+}$ $II. \text{Blue}$ $C. Mn^{3+}$ $III. \text{Yellow}$ $D. V^{4+}$ $IV. \text{Red}$ $V. \text{Green}$
| List-$I$ (Aquated Ion) | List-$II$ (Colour) |
|---|---|
| $A. Ni^{2+}$ | $I. \text{Violet}$ |
| $B. Fe^{3+}$ | $II. \text{Blue}$ |
| $C. Mn^{3+}$ | $III. \text{Yellow}$ |
| $D. V^{4+}$ | $IV. \text{Red}$ |
| $V. \text{Green}$ |
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