Chemical reactions
2 likes513 views
This document provides an overview of chemical equations and the major types of chemical reactions. It defines key terms like reactants, products, and coefficients. It also explains the laws of conservation of mass and atoms that chemical equations must satisfy. Finally, it outlines the six major types of chemical reactions: synthesis, decomposition, single displacement, double displacement, acid-base, and combustion. It provides examples of each type and asks the reader to balance several example equations and identify the reaction type.
More Related Content
What's hot (20)
Similar to Chemical reactions (20)
Recently uploaded (20)
Chemical reactions
- 2. Chemical Equation -describes exactly what happens in a chemical reaction
- 3. Reactants - the reacting substances -the substances that enter into the reaction
- 4. Products - substances produced by the reaction
- 6. 5. (s) 6. (l) 7. (g) 8. (aq)
- 8. 7 Diatomic Elements 1. Hydrogen (H2) 2. Oxygen (O2) 3. Nitrogen (N2) 4. Fluorine (F2) 5. Chlorine (Cl2) 6. Bromine (Br2) 7. Iodine (I2)
- 9. Word Equation gives the names of the chemical substances involved in the reaction
- 10. Formula Equation uses symbols and formulas to represent names of elements and compounds
- 11. Factors in Equation Writing 1.The equation must represent the facts.
- 12. 2. The equation must include the symbols and formulas that are used as reactants and products.
- 13. 3. The Law of Conservation of Mass must be satisfied
- 14. Law of Conservation of Mass In any ordinary chemical reaction, the total mass of the reactants is equal to the total mass of the products
- 15. Law of Conservation of Atoms There must be the same number of atoms of each element represented on each side of the equation
- 16. Coefficient - a whole number written before a symbol or formula in order to balance a chemical equation
- 17. Example: 1. Hydrogen gas burns in oxygen gas to yield water vapor
- 18. Example: 2. Hydrogen reacts with nitrogen to form ammonia
- 19. Example: 3. Magnesium + oxygen magnesium oxide
- 20. 4. potassium chlorate (s) potassium chloride (s) + oxygen (g) 5. Chlorine + potassium bromide potassium chloride + bromine
- 21. 6. ammonia + hydrogen sulfide ammonium sulfide 7. Calcium chlorate calcium chloride + oxygen
- 22. 8. zinc + copper (II) sulfate zinc sulfate + copper 9. Magnesium oxide magnesium + oxygen 10. Aluminum + sulfuric acid aluminum sulfate + hydrogen
- 23. MAJOR TYPES OF CHEMICAL REACTIONS
- 24. Major Types of Chemical Reactions
- 25. 1) Synthesis two or more simple substances combine to form a more complicated substance. general form: A + X AX
- 26. 2) Decomposition - the opposite of a synthesis reaction; a complex substance breaks down to make simpler ones. General form: AX ---> A + X
- 27. 3) Single displacement: This is when one element trades place with another element in a compound. These reactions come in the general form of: A + BX AX + B AY + X AX + Y
- 28. Activity Series of Elements: Li Al Pb K Zn (H) Ba Fe Cu Ca Cd Hg Na Ni Ag Mg Sn Au
- 29. 4) Double displacement: This is when the anions and cations of two different molecules switch places, forming two entirely different compounds. General form: AX + BY AY + BX
- 30. Example: Reaction of lead (II) nitrate with potassium iodide to form lead (II) iodide and potassium nitrate.
- 31. 5. Acid-base Reaction (Neutralization) This is a special kind of double displacement reaction that takes place when an acid and base react with each other. Generally, the product of this reaction is some ionic salt and water HX + A(OH) ---> H2O + AX
- 32. 6. Combustion - oxygen combines with another compound to form water and carbon dioxide. These reactions are exothermic. Example: burning of butane
- 33. Balance the following equations and identify the type of reaction: 1) NaOH + Ca(NO3)2--> NaNO3 + Ca(OH)2 2) C2H4 + O2 --> CO2 + H2O 3) Fe + NaBr --> FeBr3 + Na 4) CaSO4 + KOH --> Ca(OH)2 + K2SO4 5) NH4OH + HBr --> H2O + NH4Br 6) Pb + O2 --> PbO2 7) CaCO3 --> CaO + CO2