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CHY 103 Chapter Notes - Chapter 1: Electrical Energy, Metric System, Kinetic Energy

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5 Oct 2017

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Ryerson University

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Units and measurement for physical changes - chapter 1. The science that seeks to understand the properties and behavior of matter by studying the properties and behavior of atoms and molecules. Physical changes: they are cha(cid:374)ges that do(cid:374) t alter a che(cid:373)ical reactio(cid:374) Chemical changes: are those that alter the composition or the chemical structure; atoms rearrange, and the original substance changes to a different one. (rusting of iron) Physical property: a property that a substance displays without changing its chemical composition. They are used to observe and describe matter. (smell of gasoline) Example: appearance, texture, color, odor, melting/boiling point, density, solubility, etc. Chemical property: a property that a substance displays only by changing its composition via a chemical change. Solubility: maximum amount of a solute in a solvent. Potential energy: energy associated with its position or composition. The total energy of an object is the sum of its kinetic energy and potential energy.

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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.