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Chapter 14 NOTES – Chemical Reactions Section 1 – Forming New Substances Chemical Reaction – the process by which _________ or _____________ substances undergo _____________ to _____________ one or more _____________ substances • The new substances have new _____________ and _____________ properties. • A chemical reaction is when _____________ bonds are _____________, atoms _____________ and _____________ chemical _____________ are _____________. Clues to a chemical reaction: Gas Formation – _______________________________________ Solid Formation – _______________________________________ Color Change – _______________________________________ Energy Change – _______________________________________ Chemical Formula – shorthand _____________ for a _____________ or a diatomic element using chemical _____________ and _____________ A chemical _____________ shows the _____________ of _____________ present for each _____________. Writing Formulas for Covalent Compounds: The names of covalent compounds use _____________ to tell you how many _____________ of each _____________ are in the formula. Prefixes Used In Chemical Names: Example: Carbon Dioxide 1 6 2 7 3 8 4 9 5 10 CO2 The lack of a _____________ on carbon means ______ carbon atom and the prefix ______ means _______ oxygen atoms are present. Writing Formulas for Ionic Compounds: To write the formula for an ionic compound, you must make sure the compound’s overall charge is _____________ (has __________________). Example: Magnesium chloride MgCl2 Mg has a ______ charge and Cl has a ______ charge. In order to make a _____________ compound we must use __________________________to neutralize the ________ charge of the Mg. Chemical Equations – a shorthand _____________ of a chemical _____________ using chemical _____________ and _____________ Example: C + O2 Reactants Yields CO2 Products Reactants – the _____________ materials of a chemical _____________ Products – the substances _____________ as a _____________ of a chemical _____________ Coefficient – a _____________ placed in _____________ of a chemical _____________ or _____________ All chemical equations must be balanced. Steps to Balancing Chemical Equations: 1. Count the atoms of each element in the reactants and in the products. 2. To balance the atoms, add in coefficients. 3. Make sure that there are equal numbers of each element on both sides of the equation. Example: HCl + Al + Na2S Cl2 H2S AlCl3 + NaCl Law of Conservation of Mass – mass is __________________________ nor _____________ in ordinary chemical and physical changes Developed by Antoine Lavoisier in the 1700’s Section 14-3 Energy and Rates of Chemical Reactions Exothermic Reaction – a chemical _____________ in which _____________ is _____________ Examples: fires, batteries Endothermic Reaction – a chemical _____________ in which _____________ is _____________ Example: photosynthesis Law of Conservation of Energy – states that _____________ is neither _____________ nor _____________ Activation Energy – _____________ amount of _____________ needed for substances to _____________ Factors that Affect Rates of Reaction: Temperature Concentration of the substance Surface Area Presence of a catalyst or inhibitor Catalyst – a substance that _____________ up a _____________ without _____________ change to the reaction A catalyst will _____________ the activation energy, which allows the reaction to occur _____________. Examples: enzymes, platinum and palladium (in cars) Inhibitor – _____________ down or _____________ a chemical reaction Example: preservatives, poisons