Problem 28 - Chemistry in 30 days

Question

Oxidation number of \(\mathrm{Cl}\) in \(\mathrm{NOClO}_{4}\) and \(\mathrm{NOCl}\) is respectively (a) \(-\mid\) and \(+1\) (b) \(+\mathrm{I}\) and \(-1\) (c) \(+7\) and \(-1\) (d) \(+5\) and \(+1\)

Step-by-Step Solution

Answer

Oxidation numbers of Cl are +3 in NOClO4 and -1 in NOCl, but none of the options match this exactly.

Step 1: Calculating Chlorine Oxidation Number in NOClO4

Start by identifying the known oxidation states: nitrogen (N) typically is "+5" in nitrates, and oxygen (O) is "-2".For NOClO4, the oxidation state of the whole compound sums to zero. Let the oxidation number of Cl be x. The equation becomes: \[ 5 + x + 4(-2) = 0 \] \( 5 + x - 8 = 0 \) which simplifies to \( x = +3 \)

Step 2: Calculating Chlorine Oxidation Number in NOCl

Identify the known oxidation numbers: nitrogen (N) is typically in oxidation state "+3" in nitrosyl derivatives and oxygen (O) is "-2".For NOCl, the total oxidation state must be zero. Let the oxidation number of Cl be y:\[ 3 + y - 2 = 0 \] Solving gives \( y = -1. \)

Key Concepts

Chlorine Compounds

Chlorine is an incredibly versatile element found in many compounds with varying oxidation states. When chlorine forms compounds, its oxidation state can differ greatly. In the compound \( \text{NOClO}_4 \), chlorine takes on an oxidation state which depends on the surrounding atoms.
\( \text{NOClO}_4 \) is unique as it combines elements from nitrates with chlorine, leading to different oxidation characteristics than typical chlorides or oxychlorides.
This diversity makes chlorine compounds highly valuable in numerous chemical processes and applications. Understanding chlorine's oxidation state helps chemists determine the behavior and reactivity of these compounds in various environments.

Nitrate Chemistry

Nitrates are chemical compounds that contain the nitrate ion \( \text{NO}_3^- \), often important for their oxidizing properties. These compounds play crucial roles in both industrial applications and biological processes.In nitrate chemistry, the central nitrogen atom typically maintains an oxidation state of +5. This is due to its bonding with three oxygens, each contributing a c-2 oxidation state. The balance helps dictate the overall charge of the nitrate group. Nitrates, such as those seen in \( \text{NOClO}_4 \), illustrate the intersection of nitrogen's potential to form complex oxidizing agents. Despite sometimes being overshadowed by the nitrogen atom, the nitrate ion's ability to form stable compounds significantly impacts chemical reactions.

Oxidation Numbers Calculation

Calculating oxidation numbers, or states, in a compound involves a few key rules that help assess how electrons are distributed among atoms:

• For a neutral compound, the sum of oxidation numbers is zero.
• Oxygen usually has an oxidation number of -2.
• Chlorine varies but often adopts negative values in simple halogen compounds.

By using these guidelines, you solve for unknown oxidation states like the one of chlorine in *\( \text{NOClO}_4 \) and \( \text{NOCl} \). In \( \text{NOClO}_4 \), given nitrogen at +5 and oxygen at -2, chlorine's oxidation state is calculated to balance the rest: \( 5 + x - 8 = 0 \), resulting in chlorine being +3.
Meanwhile, in \( \text{NOCl} \), recognizing nitrogen at +3 and oxygen at -2 enables calculation: \( 3 + y - 2 = 0 \), deriving chlorine's oxidation number as -1.
Understanding oxidation states allows clearer insight into reactivity and binding characteristics within compounds, enhancing comprehensive chemical comprehension.