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Cupric oxide (CuO), commonly known as the “firework propellant,” is one of the most widely used compounds in the world. CuO has many uses, including as an additive to water and other household products, as a firework propellant, and as a component of a number of catalysts, dyes, pigments, and other chemical compounds.
CuO’s melting point is determined by the oxidation state of its atoms. The oxidation state of CuO atoms is either Cu2+ or OH-, depending on the ionic concentration and pH of the solution.
The ionic states of CuO atoms have a significant influence on their electronic structure and thermal properties, such as melting and boiling points. For example, the presence of oxygen in an ionic state of CuO causes it to decompose into Cu2O and oxygen at high temperature. This is a useful process for producing pure oxygen at high temperatures, although it limits the amount of CuO that can be recycled to Cu2O for further use.
Another important application of CuO is its ability to detect glucose in the blood. CuO is capable of catalyzing the oxidation of glucose to gluconolactone and H2O2. This allows for the measurement of glucose level using a simple electrochemical sensor.
Synthetic route to Cu, CuO, and CuO nanoparticles
The first step in the synthesis of NPs is to control their nucleation. This is achieved by adjusting the starting materials and solvents to achieve a desired morphology.
The second step is to control the growth process. This is achieved by adjusting the initial concentration and ratio of the precursor solutions to achieve the desired size and morphology.