Question

Chlorine forms a number of oxides with the following oxidation numbers: \(+1,+3,+4,+6,\) and \(+7 .\) Write a formula for each of these compounds.

Short answer

The formulas are: \(\text{Cl}_2\text{O}\), \(\text{Cl}_2\text{O}_3\), \(\text{ClO}_2\), \(\text{Cl}_2\text{O}_7\), and \(\text{Cl}_2\text{O}_7\).

Step-by-step solution

Review Oxidation Numbers

The oxidation numbers given are +1, +3, +4, +6, and +7. These indicate the charge on the chlorine atom in its oxides.

Determine the Formula for +1 Oxidation Number

For an oxidation number of +1, chlorine forms the oxide hypochlorous oxide, which is \(\text{Cl}_2\text{O}\). The formula is derived from balancing the charges: two chlorine atoms each with a +1 charge balance with one oxygen atom with a -2 charge.

Determine the Formula for +3 Oxidation Number

For an oxidation number of +3, chlorine forms chlorous oxide, represented as \(\text{Cl}_2\text{O}_3\). This happens because two chlorine atoms carry a total charge of +6, balancing with three oxygen atoms with a total charge of -6.

Determine the Formula for +4 Oxidation Number

At an oxidation number of +4, chlorine forms chlorine dioxide, which is expressed as \(\text{ClO}_2\). One chlorine atom with a +4 charge balances with two oxygen atoms with a -4 charge.

Determine the Formula for +6 Oxidation Number

With an oxidation number of +6, chlorine forms chloric oxide, \(\text{Cl}_2\text{O}_7\). Here, two chlorine atoms each with a +6 charge add up to a total +12 charge, balanced with seven oxygen atoms providing a -14 charge.

Determine the Formula for +7 Oxidation Number

For an oxidation number of +7, chlorine forms perchloric oxide, given by \(\text{Cl}_2\text{O}_7\). Although similar to chloric oxide, each chlorine atom has a +7 charge, summing up to +14, which balances with the -14 from the seven oxygen atoms.

Key concepts

Oxidation Numbers

Oxidation numbers are a fundamental concept in chemistry, representing the charge an atom would have in a molecule if electrons were completely transferred. They help us understand the electron distribution in compounds. For chlorine oxides, oxidation numbers vary from +1 to +7. This range reflects different electronic environments in these oxides.The oxidation number is crucial for determining how atoms combine to form a molecule. Knowing these numbers allows chemists to predict the formula of a compound by ensuring that the total charge is balanced. In chlorinated compounds, such as

• hypochlorous oxide (\(\text{Cl}_2\text{O}\)
• chlorous oxide (\(\text{Cl}_2\text{O}_3\)
• chlorine dioxide (\(\text{ClO}_2\)
• chloric oxide (\(\text{Cl}_2\text{O}_5\)
• and perchloric oxide (\(\text{Cl}_2\text{O}_7\)

chlorine's oxidation state varies depending on how many oxygen atoms are present. This understanding facilitates the comprehension of complex chemical reactions and the formation of various compounds.

Chemical Formulas

Chemical formulas represent a compound's composition in terms of its elements and their ratios. For chlorine oxides, these formulas are not mere symbols; they provide insight into the specific identities and proportions of the atoms involved. For example, in the chemical formula \(\text{Cl}_2\text{O}\), two chlorine atoms bond with one oxygen atom. This formula indicates that each chlorine atom carries a +1 oxidation state while the oxygen is -2. This knowledge tells us that the charge balances, leading to a neutral compound.When writing chemical formulas, it is essential to correctly represent the ratio of atoms so the total oxidation state of the atoms sums to zero, or the charge of the compound is as it appears. These formulas help chemists communicate information effectively and predict the behavior of substances in a reaction.

Chlorine Chemistry

Chlorine chemistry is a fascinating area of study due to the element's ability to form multiple oxides and other compounds. Chlorine's versatility is primarily due to its electronic configuration, which allows it to exhibit various oxidation states. This versatile nature means that chlorine can form compounds with a wide range of applications, from bleaching agents to disinfectants, and plays a role in manufacturing many chemicals. The different oxides, such as

• hypochlorous (Cl2O) used in bleaching,
• chlorous (Cl2O3), and
• chlorine dioxide (ClO2) which is frequently used in paper mill industry for pulp bleaching,

are distinguished by their distinct structures and properties. Understanding the unique chemical behavior of chlorine can lead to innovations in various industries and further advancement in chemical science.

Balancing Charges

Balancing charges is essential when determining chemical formulas, ensuring that the total positive charge equals the total negative charge. Without charge balance, a compound isn't stable.When forming oxides, chlorine atoms can adopt various oxidation states, and oxygen typically has an oxidation state of -2. For example, in \(\text{Cl}_2\text{O}_3\), the combined oxidation state of chlorine atoms (+6) must balance with the oxidation state of oxygen atoms (-6). This balance results in a neutral compound.The process of balancing requires:

• Determining the oxidation state for each atom involved.
• Adding them up to check if the compound's total charge is neutral or has the intended charge.

By practicing this consistently, chemists can accurately develop true chemical representations of compounds.