1. Reactions and Equations

2.  Chemical Reaction - One or more substances change into one or more new substances

3.  Represents with symbols and formulas  The identities and relative amounts of the reactants and products in a chemical reaction

4.  Reactants-Left side of an equation- what starts the reaction  Products- right side of an equation- what a rxn ends with

5. 1. Production of heat/light 2. Production of gas 3. Formation of a precipitate  Precipitate: a solid produced- separates from a solution 4. Color Change

6.  Word equation- uses words  Formula equation- formulas and symbols  Complete Ionic Formula- shows soluble substances in their dissociate form  Net Ionic equation- removes the spectator ions which are present on both sides of the equation. spectator ions = IONS that are exactly the same on both sides

7.  - yield s- solid g - gas aq- aqueous  - solid produced  heat as a catalyst l - liquid  - gas produced reversible reaction

8.  Reversible reaction - products can reform reactants  Catalyst - “speeds” up a reaction- lowers the activation energy

9. 1. Write the correct formulas 2. Use coefficients to balance (big # in front) 3. Check each individual element 4. Reduce coefficients if needed

10. 1. Synthesis- (combination) two or more substances combine to produce a more complex substance. x + y  xy 2. Decomposition- A substance breaks down into two or more simpler substances. xy  x + y 3. Single Replacement (displacement)- a single element replaces a similar element in a compound metal will replace metal nonmetal will replace nonmetal x + ay  xy + a 4. Double Replacement (double displacement)- positive ion exchange xy + ab  ay + xb 5. Combustion- rapid reaction that involves O 2 Organic + O 2  CO 2 + H 2 O

11.  Solute- small part- is dissolved  Solvent- large part- does dissolving  Spectator ions- present in solution on both sides of the yield

12. % Composition – Element x100 Compound Empirical Formula – Lowest whole number ration of elements in a compound. Empirical Formula From % Composition- % → grams → moles → divide my lowest number of moles = Ratio! :D

13. Molecular Formula : From empirical Molecular Mass x Empirical Formula Empirical Mass Hydrates: Crystals that contain water in crystal.