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CHEM 110 Lecture Notes - Lecture 11: Magnesium Oxide, Calcium Chloride, Magnesium Carbonate

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10 Mar 2017

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Chemistry and Biochemistry

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The following can be visual evidence of a reaction. Co2 is released when acid is placed in a solution containing co3. A solution containing ag+ ions mixed with a solution containing cl- ions. Heat or light is absorbed or emitted. Changes in the way the substances behave in an electrical or magnetic field before and after a reaction. We will learn to identify the following patterns of chemical reactions. The joining of two or more elements or compounds, producing a product of different composition. Produce two or more products from a single reactant. One atom replaces another in the compound producing a new compound. Two compounds undergo a change of partners . Two compounds react by exchanging atoms to produce two new compounds. Recognizing the pattern will help you write and understand reactions. Hydrogen reacts with oxygen to produce water. Above reaction written as a chemical equation: Calcium mixing with chloride to produce calcium chloride.

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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.