Types of Chemical Reactions

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Presentation transcript:

Types of Chemical Reactions Review Part 1 Types of Chemical Reactions

Chemical Reactions a) Definition: A reaction that alters the nature and characteristic properties of matter. The atoms are rearranged. New molecules are formed

Chemical Reactions b) Observable characteristics: A chemical reaction occurs when: A gas is released Heat is absorbed (endothermic) or released (exothermic) Light is emitted The color changes A precipitate forms

Chemical Reactions c) Types of chemical reactions: i) Basic reactions: Synthesis Two or more reactants become one product Decomposition One reactant is decomposed into two or more products Oxidation A reaction where one of the reactants is oxygen (O2) Precipitation A reaction where two liquid reactants form a solid product

Chemical Reactions ii) Other chemical reactions Acid-Base Neutralization Reactants: Acid + Base Products: Water + Salt Combustion Type of oxidation that releases a large amount of energy Combustion requires Oxidation agent Ignition temperature Fuel

Cellular respiration: Takes O2 + glucose to form CO2 +water + energy Photosynthesis: Takes CO2 + water + energy to form O2 + glucose

Review part 2 Solutions

Important Definitions Molecule: A group of two or more chemically bonded atoms Ion: - an atom that has become electrically charged by loosing or gaining one or more electrons An ion is negatively charged when it has more electrons (-) than protons (+) An ion is positively charged when it has less electrons than protons

Solutions Definition: a solution is a homogeneous mixture. Composed of the solute (e.g. powder) and the solvent (what is in greater quantity e.g. water) In an aqueous solution, water is the solvent.

Solutions A) Characteristics of solutions 1. Solubility 2. Concentration 3. Electrical Conductivity 4. pH

A) Characteristics of solutions 1. Solubility Definition the amount of solute that you can put into a solution Many factors will affect the solubility of a substance: The Temperature of the solvent As temperature increase so does solubility for solids The nature of the solvent

Properties of solutions 2. Concentration Definition: The amount of solute placed in a given solvent Once the concentration of a solution reaches the solubility point we have a saturated solution Can be measured in % (g/100ml) Can be measured in g/L Can be measured in ppm (g/1 000 000 ml) Can be measured in mol/L

3. Electrical Conductivity Definition: The capacity of a solution to conduct electricity Electrolytic solutions are solutions that contain electrolytes Types of electrolytes Acid Base Salts

Side note on acids: pH lower than 7 Release H+ ions Often begin with an H followed by a non-Metal

Side note on bases: pH higher than 7 Release OH- ions Often end with an OH

Side note on salts: Combination of a non-metal and a metal

Characteristics of solutions 4. pH Definition: Scale that measures the concentration of H+ ions in a solution (measures the acidity) The pH scale is a logarithmic scale, each level is ten times more acidic than the previous.

Identifying solutions In order to identify an unknown solution there are many basic test to conduct: Cobalt Chloride Identifies if the unknown is an aqueous solution (if there is water in the solution) pH paper, red litmus, blue litmus Identifies if the unknown is an acid or a base Electrical conductivity Identifies if the unknown is an electrolytic solutions (if it contains an acid, a base or salt)