Chemistry Data

Chemistry data on chlorine dioxide , chlorine, and oxygen:

By Andreas Kalcker

Chlorine dioxide

The controversy surrounding chlorine dioxide often stems from misconceptions about its properties and uses, leading to misguided assumptions. Many individuals mistakenly equate chlorine dioxide gas with its aqueous solution, overlooking the significant differences in their chemical behavior and safety profiles.

While ClO₂ gas is a potent oxidizer with potential health risks, the aqueous solution is used in controlled environments for disinfection and water treatment at safe concentrations. This misunderstanding has fueled unfounded claims about its efficacy and safety, particularly in medical treatments, where it is misrepresented as a miracle cure. Such assumptions not only mislead the public but also undermine scientific evidence regarding its appropriate applications, highlighting the importance of clear communication and education about chlorine dioxide and its proper uses.

The mixture of sodium chlorite (NaClO₂) with an acid also known as MMS differs significantly from simply dissolving chlorine dioxide (ClO₂) gas in water. When NaClO₂ is combined with an acid, it undergoes a chemical reaction that generates ClO₂ gas, alongside other byproducts. This reaction involves the conversion of chlorite ions (ClO₂⁻) into chlorine dioxide through the protonation of the chlorite ion in the acidic environment.

In contrast, dissolving ClO₂ gas in water does not involve any conversion or secondary reactions; it remains as ClO₂ molecules in solution.

Like ozone and chlorine, chlorine dioxide is an oxidizing biocide and not a metabolic toxin , moreover, the concentration and behavior of the resulting ClO₂ will differ between the two scenarios. In the case of mixing sodium chlorite with an acid, the reaction can produce varying amounts of ClO₂ depending on the concentration of the acid and sodium chlorite, leading to potential variations in efficacy and safety. This distinction is crucial because the chemical environment and concentration can influence the effectiveness of ClO₂ as a disinfectant or its safety profile when ingested. Understanding these differences is key to recognizing the appropriate contexts for using each form.

Property	Chlorine Dioxide Gas (ClO₂)	Chlorine Dioxide Aqueous Solution
Chemical Name	Chlorine Dioxide	Chlorine Dioxide
Chemical Formula	ClO₂	ClO₂
Molar Mass (g/mol)	67.45	67.45
Appearance	Yellowish-green gas	Yellowish liquid
State	Gas	Aqueous solution
Solubility in Water	Low solubility (generally not applicable)	Highly soluble
Concentration in Aqueous Solution	Not applicable	Varies (typically 0.1% to 5%)
pH	Not applicable	Typically 4.5 to 7.5
Oxidation State of Chlorine	+4	+4
Boiling Point (ºC)	11.8	Evaporates in the open from 11.8º C
Melting Point (ºC)	-59.5	Not applicable
Density (g/ml)	1.64	Approximately 1.0 (depends on concentration)
Reactivity	Strong oxidizing agent	Strong oxidizing agent
Common Uses	Disinfectant in gaseous form	Water treatment, disinfectant, bleaching, and medicinal applications
Toxicity	Toxic at high concentrations; irritant	Established by EPA as 292 mg/kg when present as gas in water
Regulatory Status	Regulated as a hazardous material	Regulated as a disinfectant and sanitizer; studied for medical use
Stability	Unstable; decomposes	Decomposes over time; requires proper storage
Decomposition Products	Chlorine and other byproducts	small amounts of Chlorine, chlorite, and other byproducts
Oxidizing Properties	Effective oxidant against lower ORP	Effective oxidant against lower ORP
Reducing Properties	Not significant	Acts as a reductant against OH* and superoxide radicals
Medical Applications	Not typically used in gas form	Used successfully in medicine with proven studies for treating infections, wounds, and water purification
Mechanism of Action	Disrupts cellular function through oxidation	Increases oxygen levels and electromolecular charge (ORP) in the body; disrupts microbial cell membranes and virus through oxidation
Stability in Storage	Requires careful handling due to instability	Should be stored in a cool, dark place to maintain effectiveness
Interactions with Other Chemicals	Can cause explosions under pressure (>10%) or strong UV light; reacts vigorously with organic materials and ammonia; can generate heat and toxic gases	Generally stable; should be handled with care; does not pose the same explosive risks as gas; can react with certain organic compounds but is less hazardous than the gas form
Magnetic Forces	paramagnetic	ClO₂ is paramagnetic due to unpaired electrons, maintaining magnetic properties in diamagnetic water. *
Environmental Impact	Can produce harmful byproducts if not managed	Biodegradable under certain conditions; can affect aquatic life at high concentrations

*

1. Dissolution and Magnetic Properties:
   • ClO₂, being paramagnetic due to unpaired electrons, retains its magnetic characteristics even when dissolved in diamagnetic water. This indicates that the magnetic properties of a solute can remain unaffected by the diamagnetic nature of the solvent.
2. Interactions in Solution:
   • Upon dissolving ClO₂ in water, the interaction may lead to changes in the electronic environment of ClO₂, but it does not eliminate its paramagnetic behavior. The solution may exhibit unique interactions due to the presence of a paramagnetic species in a diamagnetic solvent.
3. Chemical Behavior:
   • The presence of ClO₂ in water can influence its chemical reactivity, allowing it to participate in redox reactions or act as an oxidizing agent. This has implications for its use in disinfecting water or other chemical processes.
4. Impact on Measurements:
   • The paramagnetism of ClO₂ could be detected through techniques such as Electron Spin Resonance (ESR) spectroscopy, even when it is in a solution with diamagnetic properties.

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Table with information about oxygen:

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Oxygen is a highly reactive element and a strong oxidant, playing a crucial role in various chemical processes. It is known to be harmful to many pathogens, as its reactive nature can damage their cellular structures and lead to their destruction. For instance, oxygen can produce reactive oxygen species (ROS) that are toxic to bacteria and viruses.

Additionally, in its liquid form, oxygen exhibits bleaching properties. Interestingly, oxygen possesses magnetic properties, specifically being paramagnetic; it has two unpaired electrons that allow it to be attracted to magnetic fields. These magnetic properties are essential for the uptake of oxygen by red blood cells (RBCs) in the lung alveoli, as they facilitate the binding of oxygen to hemoglobin. This is complemented by osmotic pressure, which also plays a role in the transport of gases.

Despite its reactivity and potential hazards, oxygen is essential for human life, as it is critical for cellular respiration. Human cells utilize oxygen to convert glucose into ATP (adenosine triphosphate), the energy currency of the cell, through aerobic respiration. This process not only supports energy production but also plays a vital role in metabolic functions necessary for sustaining life.

Property	Value
Name	Oxygen
Atomic Number	8
Group	16 (Chalcogens)
Period	2
Block	p-block
Valence	2
Oxidation State	-2
Electronegativity	3.5
Covalent Radius (Å)	0.73
Ionic Radius (Å)	1.40
Atomic Radius (Å)	-
Electronic Configuration	1s² 2s² 2p⁴
First Ionization Potential (eV)	13.70
Atomic Mass (g/mol)	15.9994
Density (kg/m³)	1.429
Boiling Point (ºC)	-183
Melting Point (ºC)	-218.8
Discoverer	Joseph Priestley 1774
Color	Colorless gas; blue when liquid
Taste	Tasteless
Odor	Odorless
Natural Occurrence	About 21% in the atmosphere
Isotopes	, ,
Reactivity	Highly reactive
Uses	Essential for respiration, water purification, rocket fuel oxidizer
Molecular Form	Diatomic
Allotropes	Ozone (03)
Magnetic forces	Paramagnetic

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Table with the information about chlorine:

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Chlorine and chlorine dioxide are distinct chemical entities, each with unique properties and behaviors in an aqueous solution. Chlorine (Cl₂) is a diatomic molecule that acts as a strong oxidizing agent, primarily used for disinfection and water treatment. When dissolved in water, it forms hydrochloric acid (HCl) and hypochlorous acid (HClO), which contribute to its disinfecting properties. However, chlorine is highly toxic, and its presence in drinking water can pose serious health risks, including respiratory issues and irritation to the eyes and skin.

On the other hand, chlorine dioxide (ClO₂) is a compound made up of one chlorine atom and two oxygen atoms, known for its effectiveness as a bleaching agent and disinfectant. In an aqueous environment, chlorine dioxide remains largely undissociated and does not convert into chlorine or any chlorine-containing species. The mechanisms by which these two substances operate are different; while chlorine primarily targets organic contaminants through oxidation, chlorine dioxide is more selective, efficiently targeting specific pathogens without forming chlorinated by-products. Therefore, despite their similar names and overlapping applications in water treatment, chlorine and chlorine dioxide operate independently and do not interact to form one another in an aqueous solution.

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Property	Value
Name	Chlorine
Atomic Number	17
Valence	+1, -1, 3, 5, 7
Oxidation State	-1
Electronegativity	3.0
Covalent Radius (Å)	0.99
Ionic Radius (Å)	1.81
Atomic Radius (Å)	0.99
Electron Configuration	[Ne] 3s² 3p⁵
First Ionization Potential (eV)	13.01
Atomic Mass (g/mol)	35.453
Density (g/ml)	1.56
Boiling Point (ºC)	-34.7
Melting Point (ºC)	-101.0
Discoverer	Carl Wilhelm Scheele (1774)
Color	Greenish-yellow gas
State at Room Temperature	Gas
Isotopes	Cl-35, Cl-37
Solubility in Water	Soluble
Molecular Weight (g/mol)	70.906
Common Compounds	NaCl, HCl, ClO₂
Uses	Disinfectants, bleach, water treatment