Presentation is loading. Please wait.

Presentation is loading. Please wait.

Chemical Reactions Chapter 10. Evidence of Chemical Reactions Chemical Reaction: The process by which the atoms of one or more substances are rearranged.

Similar presentations


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:

1 Chemical Reactions Chapter 10

2 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

3 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

4 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)

5 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

6 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

7 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

8 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

9 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

10 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.

11 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.

12 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)

13 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)

14 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

15 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) →

16 Types of reactions


Download ppt "Chemical Reactions Chapter 10. Evidence of Chemical Reactions Chemical Reaction: The process by which the atoms of one or more substances are rearranged."

Similar presentations


Ads by Google