The correct answer is option 1. \(CrO\).
Let us delve into the details to understand why \(CrO\) (chromium(II) oxide) is considered the basic oxide of chromium:
Chromium(II) Oxide (\(CrO\)):
In \(CrO\), chromium is in the +2 oxidation state.
\(CrO\) is a binary compound composed of chromium and oxygen.
Chromium(II) compounds, in general, exhibit basic properties because the +2 oxidation state allows chromium to readily accept two oxygen anions to form a stable compound.
The basic nature of \(CrO\) is evident in its ability to react with acids to form salts and water.
Balanced Equation for Acid-Base Reaction:
\[ CrO + 2HCl \rightarrow CrCl_2 + H_2O \]
In this reaction, \(CrO\) reacts with hydrochloric acid (\(HCl\)) to form chromium(II) chloride (\(CrCl_2\)) and water (\(H_2O\)). The involvement of \(CrO\) in an acid-base reaction supports its classification as a basic oxide.
Comparison with Other Chromium Oxides:
\(Cr_2O_3\) (Chromium(III) Oxide): This oxide is amphoteric, meaning it can exhibit both acidic and basic properties depending on the conditions. While it can react with bases, it is not considered a purely basic oxide like \(CrO\).
\(CrO_2\) (Chromium(IV) Oxide): This compound is less common and does not exhibit typical basic oxide properties.
\(CrO_3\) (Chromium(VI) Oxide): This oxide is a strong acidic oxide due to the high oxidation state of chromium.
Conclusion:
In the context of the options provided, \(CrO\) stands out as the basic oxide of chromium because it involves chromium in the +2 oxidation state, allowing it to display basic properties in reactions with acids. |
