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A chemical combination is a phenomenon that describes the interaction between chemical substances and new substances. Chemical combinations can be represented by the equations of the chemical reactions they represent. In this sense, chemical combinations are subject to the chemical laws of reactions. These laws are: The law of mutual proportions formulated by Jeremiah Richter in 1792 is an important postulate among chemical laws. This law states that if two different elements, each with a certain weight, are able to combine with a given weight of a third element, the weights of these elements are able to combine with each other, or multiples or submultiples of these weights. For example, sodium (Na) and oxygen gas react with sulfur (S) to form sodium sulfide {eq}(Na_2O) {/eq} and hydrosulfic acid {eq}(H_2S) {/eq}: The basic principles pursued by interacting atoms and molecules are described by the laws of chemical combination for elements and compounds. These interactions have many combinations that occur in different ways. Here are the five basic laws of chemical combination for elements and compounds: Law of Preservation of Mass Law of Certain Proportions Law of Multiple Proportions Gay Lussac`s Law of Gaseous Volumes Law of Avagadro`s Chemical Combination When people learn to drive, they must learn the rules of the road, such as who leads first to an intersection with four stops and how to change lanes correctly. If you are learning chemistry, you need to understand four primordial laws that determine how atoms connect: The Aristotelian view of the composition of matter prevailed for more than two thousand years until the English scientist John Dalton revolutionized chemistry with his hypothesis that the behavior of matter could be explained by an atomic theory. First published in 1807, many of Dalton`s hypotheses about the microscopic characteristics of matter in modern atomic theory are still valid. Chemistry is the science that studies matter, its structure, formation and the transformations it undergoes, taking into account the energy involved in the whole process.

In ancient Greece, philosophers like Aristotle were already interested in knowing what matter was made of and how its transformations occurred. Today, we know that, unlike Aristotle, matter is not made up of the essential substances of water, fire, earth and air. However, his philosophical work in questioning the origin of matter formed the basis for the discussion of chemical elements and their combinations. Since matter cannot be produced or destroyed, we must have four hydrogens and two oxygens on either side of the equation – on both sides of the chemical reaction. The preservation of MassMatter cannot be created or destroyed, although it can be rearranged. The mass remains constant with an ordinary chemical change. This principle is also known as the preservation of matter. The law of constant proportions, also known as the law of certain proportions, is one of the chemical laws and was developed in 1797 by the chemist Joseph Louis Proust.

He found that the masses of reactants and the masses of products involved in a chemical reaction always obey a constant ratio. This proportion is characteristic of each reaction and regardless of the number of substances introduced into the reaction. So, if you look at the formation of copper sulfide (CuS) by copper (Cu) and sulfur (S): The law of mass preservation states that the total mass remains constant before and after a chemical reaction. Thus, 18 g of water decomposes into 2 g of hydrogen and 16 g of oxygen. This is the standard reaction between nitrogen and oxygen, that is, an oxide is formed with 2 nitrogen atoms and 1 oxygen atom. If the mass of oxygen is varied while maintaining the mass of nitrogen in different experiments, the result will be: Chemical laws empirically derived by scientists such as Lavoisier, Proust and Dalton allow the calculation of the quantities of substances present in reactions as well as the establishment of mathematical relationships between such quantities in a chemical combination. These laws were formulated even before the theories of chemical bonding and electronic structure were known and served as the basis for classical atomic theory. Chemical combinations are subject to four laws: This law was drafted in 1774 by the French chemist Antoine Laurent Lavoisier and is one of the general chemical laws for reactions. The experimental studies conducted by Lavoisier led him to the conclusion that in a chemical reaction that takes place in a closed system, the sum of the masses of the reactants is equal to the sum of the masses of the products: you must now understand the laws of chemical combination, which should facilitate the observation and study of the compounds in the laboratory! Early Greeks such as Democritus first developed the idea of Atomos, the smallest indivisible unit of matter.

This concept was later presented by the English scientist John Dalton as an atomic theory. The law of mass preservation was discovered by the French chemist Antoine Lavoisier. It states that atoms are neither created nor destroyed during a chemical change; The total mass of matter present when matter passes from one type to another remains constant. Dalton used three laws of chemical reactions as the basis of his theory: (1) The law of preservation of mass, (2) The law of certain proportions, and (3) the law of multiple proportions. Dalton`s atomic theory provides a microscopic explanation of the many macroscopic properties of matter. The law of definitive fractions states that regardless of the source in a given chemical compound, the mass ratio of the constituents always remains fixed. Thus, a pure water sample always has a mass ratio of 1 to 8 of hydrogen to oxygen, regardless of the total mass of the water. The preservation of mass laws, the law of the determined relation and the law of multiple proportions. Joseph Proust, a French chemist, explained that the percentage by weight of the elements of a given compound will always remain exactly the same. In simple terms, we can say that regardless of their source, origin or quantity, the percentage composition of the elements by weight in a particular compound always remains the same.