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Today's topic was Daltons' atomic theory, which explains and describes everything about atoms in general. In the first part of his theory, he claims that all matter is composed of indivisible atoms. According to the second component of the theory, the mass and characteristics of every atom in a specific element are the same. Compounds, according to the third section, are combinations of two or more different kinds of atoms. We also talked about how to distinguish between physical and chemical properties, as well as extensive and intensive aspects of matter. Overall, I believe that the chemistry lessons I took helped me to understand that matter is made up of atoms and that it has a variety of different properties.

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We talked extensively about chemical compounds, which are defined as any substance made up of similar molecules made up of atoms from two or more different chemical elements. We also talked about the four categories of identifying inorganic chemicals: ionic compounds, molecular compounds, acids, and bases. Positively charged ions, known as cations, and negatively charged ions, known as anions, make up ionic compounds, which are neutral substances. The name of the cation is written first, followed by the name of the anion, for binary ionic compounds (ionic compounds that only contain two types of elements). For instance, potassium chloride is the name of the ionic compound KCl, which consists of K+ and Cl⁻ ions. When naming acids, the prefix hydro- is used. It is then followed by the anion's base name, followed by the suffix -ic. Acid naming formula: hydro- and base name of nonmetal and -ic + acid Hydrochloric acid is an example of HCl. Therefore,  naming acids begins with a prefix, then the anion's base name, followed by the suffix. Overall, I learnt a lot of things, such as how to name inorganic chemical compounds and the definition of compounds, which will assist me with my next lesson, which will involve writing the formula for compounds.

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We had a lengthy discussion regarding compound compositions. Since writing a chemical compound formula requires knowing the element symbols, molar mass, charge, and prefixes included in the chemical compound. The ability to distinguish between different substances is important because it enables you to determine the components of the substance and their organizational structures. Discussing the chemical formula is crucial because it enables you to identify a substance by its scientific name, make predictions about its nature and qualities, and formulate balanced chemical equations and do stoichiometric calculations for the reactions in which the substances are involved.

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This session focused entirely on the various types of chemical compounds, including synthesis, decomposition, single-replacement, double-replacement, and combustion. A combination reaction is a type of synthetic reaction that takes place when two or more reactants combine to create a single product. Decomposition, on the other hand, is defined as a reaction in which a single compound splits into two or more simpler compounds. A chemical process known as single-replacement occurs when a more reactive element removes a less reactive element from its aqueous salt solution. A double displacement reaction is one in which ions are moved between two reactants to create a new product, as opposed to double replacement. Finally, combustion is defined as a chemical reaction that releases energy when a fuel undergoes oxidation through a reaction with an oxidizing agent.

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In this lecture, the concept of stoichiometry was covered. which defines the field of research as one that looks at how much of various substances are consumed and created during chemical reactions. We also discussed more about the formula mass, also known as formula weight of a substance is the sum of the atomic mass, also known as atomic weights of the atoms in the chemical formula of the substance. Furthermore, stoichiometry is based on an understanding of atomic masses, chemical formulas, chemical equations, and the law of conservation of mass. We also talked about moles, which are the units of measurement that chemists use to describe vast amounts of atoms or molecules. This statistic is known as the 6.02 * 1023 Avogadro number in honor of the Italian mathematician Amedeo Avogadro. We also talked extensively about molar masses, which are defined as a substance's molecular mass expressed in grams. Any substance's formula weight in atomic mass units is numerically equivalent to its molar mass in grams per mole. I discovered how to calculate a molecule's weight, molar mass, and mole.

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In this session, we continued our study of stoichiometry while figuring out a chemical compound's % composition. For scientists to determine the purity of a component to be utilized in a lab experiment, they might use the percent composition of a chemical compound. The percentage of the compound's total mass that each element contributes can be determined using the formula.

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We covered all of the topics of limiting reactant, surplus reactant, theoretical yield, and percent yield in this session. The substance that is completely absorbed at the end of the chemical reaction is known as the limiting reactant. The excess reactant, on the other hand, is a substance that isn't completely consumed or reacted in a chemical process. While the amount of product you experimentally receive from a chemical reaction is the actual yield. A theoretical yield, on the other hand, is the quantity of product you would get if all of the reactant converted to product.