Copper vs. Cuprous Oxide: What is the Difference?

by Erica Mitchell | July 17 2015 | 2 Comments

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Copper is the oldest-known metal used by humankind to make tools and decorations, helping form the transition from the Stone Age to the Bronze Age. After millennia of using wood, stones, and animal bones, copper transformed the abilities of early peoples, pushing them to invent ore smelting, mining, and metalworking. As a result of these skills honed over generations, cultures around the world took the next step, combining metal ores to create harder metals, such as bronze, a combination of copper and tin. What is special about copper, and how will it take us to the next level in healthcare safety?


A reddish-orange metal, copper is highly conductive to heat and electricity. It shares this ability with silver and gold, as these elements each have an "free agent" electron that is open to negotiations for chemical bonds with any surrounding available atom.  All the other electrons are firmly contracted to stay with their team, but this one can be easily influenced to transfer. 

The metallic bond of a copper wire, for example, creates a crystalline form with a sea of electrons that are in a state of attraction to all surrounding nuclei, existing in a stable, shared state. As a result of these valence electrons, when electricity or heat is introduced to the wire, these free electrons move through the material, creating a current.

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The valence electron gets a bad reputation for his freeloading ways, but he can't help that he out there all by himself with a weaker bond to the team.

 

Right underneath the free agent electron level is a level jam-packed with electrons - no more can fit on this level. This means that transferring electrons from this level is very difficult. As a result, copper's metallic bonds only exist on this outer layer of free-moving electrons, a pretty weak bond as far as metals are concerned. This is why copper is so soft and easy to bend and cut.

This same free agent electron plays a role in oxidation, or rusting. When copper is exposed to water molecules (two hydrogen, one oxygen), this free electron is transferred to a neighboring oxygen atom, bonding it into a molecule. If only one atom of copper bonds to an oxygen molecule, it is called cupric oxide. If two copper atoms bond to an oxygen atom, it is cuprous oxide. Cupric oxide is considered "fully oxidized," while cuprous oxide is still in an active state.

Stability of Copper Ions

The key to cuprous oxide, the aspect that makes is extremely effective as a biocide, is that active state. It is still producing reactive oxygen species, highly reactive molecules. These are unstable molecules that cause damage to cell structures.

When it comes to killing bacteria, you want highly reactive molecules. They are very good at pulling away electrons, releasing free radicals, and generally smashing up their environment. In the case of a pathogen, they tear through membranes and destroy DNA-making machinery like a hot knife through butter. Copper needs to oxidize to reach the same level of toxicity, and while cupric oxide is oxidized, it's in a more stable oxidation state so it doesn't wreak the same havoc as his brother, cuprous oxide.


So why is cuprous oxide so toxic to bacteria and so safe for humans? It all comes down to size. A surface infused with cuprous oxide to a bacteria cell is a highly toxic landscape because the ratio of Cu2O to cell is smaller. So a beautiful countertop or table to us is a toxic minefield to pathogens. (Which is just the way we like it.)