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CHEM101 Lecture Notes - Lecture 2: Mass Number, Elementary Particle, Empty Spaces

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9 Oct 2018

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CHEM101 Full Course Notes

CHEM101 Full Course Notes

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Chemistry is the study of matter and the interaction between them. The food we eat, clothes we wear, medicines, air, cleaners . Developments of the fundamental chemical laws and the atomic theory: democritus first proposed matter was made up of invisible particles called atoms. Law of conservation of mass: matter is neither created nor destroyed. Law of constant composition: a compound and an element put together has the same fraction of mass. In other words, all samples of a given chemical compound have the same elemental composition. e. g all water in a compound or element will have the same ratio, that is two hydrogens and one oxygen. Law of multiple proportions: when two elements ( a and b ) form more than one compound, the masses of element a that combine with a fixed mass of b are in simple ratio.

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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.