Amedeo Avogadro

The future of chemistry depends on embracing the distinction between atoms and molecules, a distinction that clarifies many ambiguities.

To ignore the evidence from gaseous reactions is to build a chemical theory on an incomplete foundation.

My hypothesis is not merely a theoretical construct, but a practical tool for determining the true atomic weights of elements.

The apparent inconsistencies in chemical stoichiometry vanish once the molecular nature of elementary gases is acknowledged.

The path to scientific truth often requires us to question even the most fundamental assumptions.

My work lays the groundwork for a more precise and quantitative understanding of chemical reactions and the nature of matter.

The scientific community's initial skepticism only highlights the profound shift in thinking that my hypothesis demanded.

The simplicity of my law, that equal volumes of gases at the same temperature and pressure contain the same number of molecules, is its greatest strength.

To understand the world, we must be willing to see it as it is, not as we wish it to be.

My hypothesis, though initially overlooked, will ultimately prove indispensable for the advancement of chemistry.

The true measure of a scientific theory is its ability to explain observed phenomena and predict new ones, not its conformity to existing dogma.

The very definition of an element and a compound becomes clearer and more consistent with my molecular hypothesis.

The power of quantitative reasoning in chemistry is fully realized when we correctly differentiate between atoms and molecules.

The path to scientific progress is paved with bold ideas that challenge the status quo.

The number of molecules in the grammolecular weight (mole) of any substance is a constant, which I have proposed to call Avogadro's constant.

Equal volumes of gases, at the same temperature and pressure, contain equal numbers of molecules.

The hypothesis I have proposed seems to me the only one which can account for the facts.

It must then be admitted that very simple relations also exist between the volumes of gaseous substances and the numbers of simple or compound molecules which form them.

The particles of gases are not in immediate contact, but are separated by spaces which are very large compared with their own dimensions.

I have thought it necessary to suppose that the constituent molecules of any simple gas are not formed of a solitary elementary molecule, but are made up of a certain number of these molecules united by attraction to form a single one.