How do colloids differ from solutions with regard to dispersed particle size and homogeneity?

When discussing colloids and solutions, one key factor to consider is the size of the particles that are dispersed throughout the mixture. Colloids contain particles that are significantly larger than those found in solutions. Specifically, the particles in colloids range from 1 to 1000 nanometers (nm) in size. To visualize this, consider that human hair has a diameter of about 75,000 nm, making colloid particles minuscule in comparison, yet they are large enough to distinguish colloids from true solutions.
In solutions, the dispersed particles, such as ions or molecules, are typically smaller than 1 nm. Due to their incredibly small size, these particles can completely dissolve in the solvent, creating a mixture where the individual components cannot be seen or easily separated. This fundamental difference in particle size affects other characteristics of colloids and solutions, including how they interact with light and how uniform they appear to the naked eye.

The concept of homogeneity in mixtures is central to understanding the difference between colloids and solutions. Simply put, homogeneity refers to how uniformly the particles are spread throughout the mixture. Solutions are revered for their impeccable homogeneity, meaning the particles are so uniformly distributed that every portion of the mixture is exactly the same as any other, at the molecular level.
Colloids, while often considered homogeneous because their particles do not settle out and remain evenly distributed, have a catch. Due to the larger size of their particles, they can sometimes display characteristics of heterogeneity under specific conditions. Although the particles in colloids are in constant motion, keeping them suspended, they are large enough that some unique optical properties emerge, resulting in phenomena such as the Tyndall effect. This effect can make a colloid look somewhat less uniform when observed closely, as it scatters light in a distinctive way not seen in true solutions.

The Tyndall effect is a fascinating optical phenomenon that serves as a litmus test to distinguish colloids from solutions. Named after the 19th-century physicist John Tyndall, this effect occurs when light passes through a colloid and is scattered by the larger particles within. To witness the Tyndall effect, you need only shine a beam of light through a colloidal mixture. What you'll observe is a path of light, created as the particles within the colloid scatter the light beam.
This phenomenon cannot be observed in a true solution. The homogeneity and minuscule size of the particles in solutions mean that light passes through without being scattered, rendering the beam invisible. Interestingly, this effect is not only proof of the colloidal nature of a mixture but also a demonstration of the relative size of dispersed particles within it. The ability of colloidal particles to scatter light can vary depending on their size, shape, and concentration, providing a degree of insight into the nature of the colloid. The Tyndall effect emphasizes the unique nature of colloids in comparison to solutions and is a handy tool for identifying the type of mixture being examined.