Presentation on theme: "Chemical Reactions Chapter 10. Evidence of Chemical Reactions Chemical Reaction: The process by which the atoms of one or more substances are rearranged."— Presentation transcript:
Chemical Reactions Chapter 10
Evidence of Chemical Reactions Chemical Reaction: The process by which the atoms of one or more substances are rearranged to form different substances. Temperature change Color change Gas or solid appears
Representing Chemical Reactions Chemical Equation Reactants: substances reacting; on left side Products: substances produced; on right side SymbolMeaning +Separates two or more products or reactants →Separates reactants from products (s)Solid State (l)Liquid State (g)Gaseous State (aq)Identifies water solution
Representing Chemical Reactions How would you write an equation for sodium reacting with chloride to make sodium chloride? Reactant 1 + Reactant 2 → Product 1 sodium + chloride → sodium chloride Na (s) + Cl 2 (g) → NaCl (s)
Representing Chemical Reactions Law of Conservation of Mass: atoms cannot be created or destroyed. All atoms in reactants must be in products, and visa versa Balancing the equation Na (s) + Cl 2 (g) → NaCl (s) Can not occur without coefficients: number written in front
Balancing Equations 1. Write Equation 2. Count atoms in of elements in reactants 3. Count atoms of elements in products 4. Change the coefficients to make # of atoms equal 5. Write coefficients in their lowest ratio 6. Check
Balancing Equations Na (s) + Cl 2 (g) → NaCl (s) H 2 (g) + O 2 (g) → H 2 O (l) AgNO 3 (aq) + Cu(s) → CuNO 3 (aq) + Ag Al(s) + O 2 (s) → Al 2 O 3
Classifying Chemical Reactions 5 types Need to be able to recognize different types. Need to be able to predict products of different types of reactions
Synthesis Reactions A chemical reaction in which two or more substances react to produce a single product. A + B → AB Na (s) + Cl 2 (g) → NaCl (s) Compounds combining is also synthesis CaO(s) + H 2 O(l) → Ca(OH) 2
Combustion Reaction Oxygen combines with a substance to produce heat and energy 2H 2 (g) + O 2 (g) → 2H 2 O(g) All combustion are synthesis not all synthesis are combustion.
Combustion Reaction CH 4, methane, is a hydrocarbon hydrocarbon + oxygen → carbon dioxide + water CH 4 (g) + 2O 2 (g) → CO 2 (g) + 2H 2 O(g) Can be tough to balance, always balance O 2 last.
Decomposition Reactions Single compound breaks down into two or more elements or compounds. AB → A + B Often requires an energy source. NH 4 NO 3 (s) → N 2 O(g) + 2H 2 O(g) Air Bags 2NaN 3 (s) → 2Na(s) + 3N 2 (g)
Single Replacement Reactions A reaction in which the atoms of one element replace the atoms of another A + BX → AX + B Cu(s) + 2AgNO 3 (aq) → 2Ag(s) + Cu(NO 3 ) 2 (aq)
Double Replacement Reactions Exchange of ions between two compounds AX + BY → AY + BX Ca(OH) 2 (aq) + 2HCl (aq) → CaCl 2 (aq) + 2 H 2 O(l) All double replacement reactions produce either a precipitate, a gas, or water
Double Replacement Reactions Precipitate: a solid being produced during a chemical reaction in a solution Pair cations with other anion for both compounds LiI(aq) + AgNO 3 (aq) →