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CH-1010 Lecture Notes - Lecture 1: Electromagnetic Spectrum, Uncertainty Principle, Trailing Zero

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7 Sep 2016

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Clemson University

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Atomic theory- all matter is made up of tiny indivisible particles. Law of conservation of matter- mass is conserved in chemical changes- it is neither created nor destroyed. Law of multiple proportions- 2 elements can form more than one compound. Specific whole number ratios of masses of the second element combines with a fixed mass of the first. 1st law of thermodynamics- energy cannot be created nor destroyed. Exact numbers do not use significant figures. When multiplying, use fewest number of significant figures. When adding, use fewest number of decimal places. Trailing zeros with no decimal do not count (ex. Trailing zeros with decimal point count( (ex. Trailing zeros with decimal point count (ex. Intensive- property that does not depend on size (ex. Extensive- property that does depend on size (ex. Cathode ray experiment - calculated charge mass ratio for electrons. Plum pudding model - atoms contain many negatively charged electrons held in an atom by positivity.

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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.