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# Chemical reactions

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### Chemical reactions

1. 1. Chemical Reactions
2. 2. What is a chemical reaction?• A chemical reaction is the process by which the atoms of one or more substances are rearranged to form different substances.
3. 3. Chemical Reaction Indicators• Some ways to tell that a chemical reaction have occurred include: 1. Color change – a change indicates the particles have changed. 2. Heat content change – did the temperature go up or down. 3. Gas is produced – if it bubbles (without being heated) it’s a gas! 4. Precipitate forms – a precipitate is a solid produced during a chemical reaction between solutions.
4. 4. Chemical Equations• Chemical equations are used to represent chemical reactions. Fe (s) + Cl2 (g)  FeCl3 (s) Reactants Products
5. 5. Symbols Used in Equations + Used to separate two reactants or products  “Yields” separates reactants from products (s) Identifies solid state (l) Identifies liquid state (g) Identifies gaseous state (aq) Identifies aqueous state – a substance dissolved in water
6. 6. Balanced equations• Chemical equations MUST be balanced to show that the number of atoms in the reactants is the same as the number in the products. What goes in MUST come out!!!
7. 7. Rules for Balancing• The only place you can change any number is the coefficient.• A coefficient is a number written in front of a chemical formula.• Don’t forget diatomic molecules.• Use the smallest ratio of coefficients possible.
8. 8. How to Balance• If you are starting with words, write the equation using formulas.Example: hydrogen and oxygen gases react to form water. (Hint: diatomics!) H2 + O2  H 2O
9. 9. H2 + O2  H 2O2 hydrogens + 2 oxygens  2 hydrogens 1 oxygenNotice that there are two hydrogenatoms on each side however there aretwo oxygen atoms in the reactants butonly one in the products. To balance thiswe must insert a coefficient. H2 + O2  2 H 2O
10. 10. While that evens the number of oxygen atoms – there are now four hydrogen atoms in the products. To balance the hydrogen we go back to the reactants and insert a coefficient. 2H2 + O2  2H2ONow there are equal number of atoms of hydrogen and oxygen on each side of the equation – it is now balanced.
11. 11. Types of Reactions• There are five types of chemical reactions: synthesis, decomposition, single-replacement, double-replacement, and combustion.• Replacement reactions are sometimes called displacement reactions.• Synthesis reactions are also called combination reactions.
12. 12. Synthesis or Combination• Synthesis is a reaction in which two or more substances react to produce a single product. A + B  AB Na + Cl2  2NaCl
13. 13. Decomposition Reactions• Decomposition reactions occur when a single compound breaks down into two or more simpler substances. AB  A + B or ABC  A + BC 2HI  H2 + I2 2Mg(ClO3)2 2MgCl2 + 3O2
14. 14. Single-Replacement Reactions• A reaction in which the atoms of one element replace the atoms of another element in a compound. A + BC  AC + B Mg + Zn(NO3)2  Mg(NO3)2 + Zn
15. 15. Double-Replacement Reactions• A reaction involving the exchange of positive ions between two ionic compounds dissolved in water. AB + CD  AD + CB 2NaOH + CuCl2  2NaCl + Cu(OH)2
16. 16. Combustion Reactions• In a combustion reaction, oxygen combines with a substance and releases energy in the form of heat and light. CH4 + 2O2  CO2 + 2H2O*All hydrocarbons contain carbon and hydrogen and burn in oxygen to yield the same products – CO2 and H2O
17. 17. Heat Content Changes• An exothermic reaction occurs when more energy is released forming new bonds than is required to break bonds in the initial reactants. *These reactions tend to feel warm.• An endothermic reaction occurs when a greater amount of energy is required to break the existing bonds in the reactants than is released when the new bonds form in the products. *These reactions tend to feel cold.