Graphene and its derivatives have proven to be biocompatible and biodegradable materials, with great potential in biomedical and technological applications. Studies have validated their safety in tissues and organs, as well as their ability to be degraded by enzymes that limit their persistence both in the body and in the environment. Graphene and its derivatives are rarely found in their free form, as to harness their properties, they must be combined with three-dimensional materials or functionalized with other molecules or nanostructures to give them a specific property. This is of vital importance because such functionalizations reduce potential adverse effects, facilitating their integration into various industries and their use in sensitive applications like tissue engineering or biomedical products. Their continuous development reinforces their position as an innovative and safe material for future applications.

Graphene is emerging as a key material for the evolution of solar energy. Its integration into solar cells promises to improve efficiency, reduce costs, and accelerate the global adoption of solar energy. Thanks to advances in research and development, graphene solar cells are on its way to be available in the market.

Graphene aerogels combine the three-dimensional properties of aerogels with graphene's stability and versatility, amplifying their adsorption and regeneration capacities in decontamination processes.

Graphene The Most Versatile Carbon Allotrope with Extraordinary Properties  Carbon is one of Earth’s most abundant elements and vital for living organisms. Known as the “king” of the periodic table, its chemical properties are exceptional due to an electronic structure capable of forming single, double, and triple bonds, allowing it to create up to ten million compounds.  Carbon allotropes are carbon-based materials with different molecular configurations and, consequently, unique properties. For instance, in graphite, a soft, thermally resistant, and electrically conductive material, carbon atoms form three covalent bonds in a hexagonal pattern, arranged in stacked layers loosely bonded together.  Graphite's common uses include pencils, batteries, and lubricants. Meanwhile, in diamond, an insulating material highly valued in jewelry, carbon atoms are bonded covalently in a tetrahedral structure, giving it extreme hardness used mainly for cutting tools.  Other lesser-known carbon allotropes are nanometric in size (smaller than 0.1 microns). These include fullerenes, which resemble a soccer ball and can act as semiconductors...