Difference Between Peroxide & Dioxide - Redox Reactions Explained

  • Thread starter Whalstib
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In summary, peroxide and dioxide are both compounds that contain oxygen atoms, but they differ in their charge. Peroxide has a charge of 2-, while dioxide has a charge of 1-. This is important in redox reactions, as peroxides are known to be oxidizers due to their higher charge. CO2, on the other hand, is not considered an oxidizer because it has a neutral charge. When looking at covalent compounds, the prefix "per-" is not used and the compound is simply referred to as dioxide.
  • #1
Whalstib
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Hi,

What is the difference between peroxide and dioxide? Why isn't CO2 carbon peroxide?

I'm finding this important in Redox rxns but have not found a way to differentiate the 2 or actually define them.

Any help appreciatted!

Warren
 
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  • #2
Look up the definition of "peroxide" and pay special attention to the O-O
 
  • #3
Thanks for being so quick!

But all I can find is a Wikipedia entry and have gleamed that peroxides are cations 2- as opposed to neutral O2 molecules...right?

So how does one determine if it's a peroxide? NaO2, LiO2, CO2 etc...is it determined by the charge? So Li2O2 a peroxide and LiO2 a dioxide?

I think I got it! Right?

W
 
  • #4
What are the characteristics of peroxides? Are they oxidizers, and if so, why? Is CO2 an oxidizer? If not, why not?
 
  • #5
In beginning chemistry at least, you can look at it this way:

You can tell by the charge. Peroxide is O22- as in Li2O2.
The two oxygens in NaO2, however, are not part of peroxide because that ion has a 1- charge: O2- which is superoxide.
In a covalent compound such as CO2, the two oxygens would be called dioxide.
 

1. What is the difference between peroxide and dioxide?

Peroxide refers to a compound that contains an oxygen-oxygen single bond, such as hydrogen peroxide (H2O2). Dioxide, on the other hand, refers to a compound that contains an oxygen-oxygen double bond, such as carbon dioxide (CO2).

2. How do peroxide and dioxide participate in redox reactions?

Peroxides and dioxides can participate in redox reactions, which involve the transfer of electrons between substances. In these reactions, peroxides are reduced, meaning they gain electrons, while dioxides are oxidized, meaning they lose electrons.

3. Why do peroxides and dioxides have different reactivities in redox reactions?

The difference in reactivity between peroxides and dioxides lies in the strength of their oxygen-oxygen bonds. The single bond in peroxides is weaker than the double bond in dioxides, making peroxides more reactive and easier to break apart in redox reactions.

4. How can peroxides and dioxides be identified in a redox reaction?

Peroxides can be identified by the presence of oxygen-oxygen single bonds, while dioxides can be identified by the presence of oxygen-oxygen double bonds. Additionally, peroxides will be reduced in the reaction, while dioxides will be oxidized.

5. What are some real-world applications of peroxides and dioxides in redox reactions?

Peroxides and dioxides have various real-world applications in redox reactions. For example, hydrogen peroxide is used as a bleaching agent and disinfectant, while carbon dioxide is used in fire extinguishers and as a greenhouse gas in agriculture. Additionally, both peroxides and dioxides play important roles in biological processes, such as cellular respiration and photosynthesis.

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