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CHE 106 Lecture Notes - Lecture 1: Oil Drop Experiment, Cathode Ray, Atomic Number

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cerisegiraffe538

9 Oct 2014

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Syracuse University

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CHE 106 Full Course Notes

CHE 106 Full Course Notes

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Che 106: general chemistry- lecture 1-3: law of conservation of mass the total mass of substances present at the end of a chemical process is the same as the mass of substances present before the process took place. Matter is not created nor destroyed in chemical reactions. This was one of the laws on which dalton"s atomic theory was based. The british chemist john dalton (1766-1844) is credited with the formulation of the atomic theory of matter. Offers an explanation of the structure of matter in terms of combinations of atoms: very small particles. If two elements, a and b, form more than one compound, the masses of b that combine with the given mass of a are in the ratio of small whole numbers. When two or more compounds exist from the same elemens, they can not have the same relative number of atoms. H2o and h2o2 are okay, but h2o2,127 is not!

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Chemical Reactions and Equations Learning objectives To observe physical and chemical properties associated with chemical changes To be able to give evidence for the occurrence of a chemical reaction To write a balanced chemical equation To identify areaction as a combination, decomposition, precipitation, single or double replacement, or combustion reaction ntroduction When a substance undergoes a physical change, it changes its appearance but not its composition. For example, when ice melts to form water, it undergoes a physical change from solid to liquid. In a chemical change, the composition of a substance is changed to give a new substance with different physical and chemical properties. For example, when silver tarnishes, the shiny silver (Ag) changes to a dull gray silver sulfide (AgaS). Not only has the chemical formula changed from Ag to Agus, but also the physical properties (shininess) of the substance have changed. Some examples of physical and chemical changes are listed in Table 1 below. Table 1. Comparison of Physical and Chemical Changes Examples of Physical changes Examples and Evidence of Chemical Changes Change in state (melting, freezing, evaporating Formation of a gas (bubbles) subliming) Formation of a solid (precipitate) Change in size Tearing Change in Color Heat is given off or absorbed A solid dissolving in a solvent In a chemical reaction, atoms in the reactants are rearranged to produce new combinations of atoms in the products. However, the total number of atoms of each element in the reactants is equal to the total number of atoms in the products. This is true according to the Law of Conservation of Mass, which states that the total mass remains constant during a chemical reaction. In other words, matter cannot be created or destroyed in a chemical reaction. In a chemical equation, the reactants are shown on the left and the products are on the right. An arrow in between indicates that a chemical reaction occurs. Finally, the physical state of each compound is designated in parentheses after the chemical formula. Solid, liquid, gas, and aqueous (dissolved in water) are shown as(s,(n,(g), and (aq), respectively.