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Chemical Reactions

By: Indya Evans . Chemical Reactions . What is a Chemical Reaction?. a process in which one or more substances are changed into others A change in the arrangement of atoms or molecules to yield substances of different composition and properties

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Chemical Reactions

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  1. By: Indya Evans Chemical Reactions

  2. What is a Chemical Reaction? • a process in which one or more substances are changed into others • A change in the arrangement of atoms or molecules to yield substances of different composition and properties • the interaction of two or more chemical substances producing new substances with different properties from the original ones

  3. What is there to know? • Reactants Products • The coefficient is the whole number in front of the elements • Catalyst: is a substance that speeds up a reaction but is not used up in the reaction. • A chemical equation represents the reaction • A balanced equation has an equal number of atoms on both sides of the equation

  4. Symbols • +: used to separate two reactants or two products • : “Yields” separate reactant from product • (s): Solid state after reaction • (l): liquid state after reaction • (g): Gaseous State after reaction • (aq): aqueous State after reaction (meaning the substance is dissolved in water) • heat tells that heat is supplied to the reaction • Pt: indicates the use as a catalyst (for ex: platinum)

  5. Definitions • Law of conservation of mass: mass is conserved • Mass is neither created nor destroyed in a reaction…. That means that one must account for everything! • Law of conservation of charge: same deal except charge…. • Means one must account for all charge within a reaction

  6. The 5 types of Chemical Reactions • Combination Reaction • Equation: R + SRS • Decomposition Reaction • RSR + S • Single- Replacement Reaction • T + RSTS + R • Double- Replacement Reaction • R+ S- + T+ U-R+ U- + T+ S- • The outsides come together + the insides

  7. Combustion reaction 5. Combustion Reaction • Cx Hy + ( x=y/4)O2 xCO2 + (y/2)H2O • Burning fire

  8. How to balance an equation 1st: Identify what type of reaction it is 2nd: list each element and it’s number 3rd: Balance equation by using whole number coefficients EXAMPLE: Li+O2 Li2 O • Decomposition reaction • Li =1 Li=2 O =2 O=1 • 4Li+O22Li2O

  9. Multiplying equation by 2 • When an equation does not have all whole number coefficients to make the equation balanced. The equation is to be multiplied by 2 (only) EXAMPLE: C3H6+O2 CO2+H2O C=3 C=1 H=6 H=2 O=2 O=3 2(C3H6+ 4 1/2 O2 3 CO2+3H2O) • 2 times 4 ½ is 9 which is a whole number! NEW EQUATION • 2C3H6+ 9O26 CO2+ 6H2O • Be sure to multiply the other numbers be 2!

  10. Net Ionic Equations • When writing a complete ionic equation the compound elements split into one element each (and everything is there) • If the ion is unchanged in the equation it can be deleted (spectator ion) • When writing a net ionic equation one only writes what is directly involved in the chemical change

  11. Solubility Rules for ionic compounds

  12. Reminder • KNOW YOUR DIATOMIC ATOMS • H( hydrogen) Ham • N(nitrogen) ~N~ • O (Oxygen) Old • F (Fluorine) Flaming • Cl (Chlorine) Cheese • Br (Bromine) Before • I (Iodine) Ice cream

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