Ch.4 Atomic Theory Explains the formation of compounds

1. Ch.4 Atomic Theory Explains the formation of compounds 4.3 Chemical Equationsp.202 - 215 Words to Know: *balanced chemical equation *products *chemical equation *reactants *chemical reaction *skeleton equation *conservation of mass *symbolic equation

2. A chemical change is the process by which one or more substances are changed into one or more new, different substances. • It has new properties Chemical changes occur when new substances are created. Copper reacting in nitric acid See pages 202 - 203

3. How do we know a Chemical Change has occurred? 1) Formation of a gas. 2) Formation of heat and light together. 3) Formation of a precipitate. 4) Color change. 5) Temperature change. https://www.sophia.org/tutorials/indicators-of-a-chemical-change

4. The original substance(s), called reactants, change into new substance(s) called products. A + B --------------------- C AB + CD ---------------- AC + BD Reactants -------------------- Products

5. Chemical reactions can be represented by chemical equations: A word equation: iron(III) chloride + sodium hydroxide  iron(III) hydroxide + sodium chloride A symbolic equation: FeCl3+ NaOH Fe(OH)3 + NaCl

6. Both show: • reactants • products • a reaction arrow pointing from reactants to products • addition signs

7. Chemical equations may also show: • Coefficients:integers placed in front of the formula or chemical symbol FeCl3+ 3 NaOH Fe(OH)3 + 3NaCl • used to determine the ratios between the various compounds in the reaction

8. States of Matter States of matter: shown byletters written in brackets to the right of the formula or chemical symbol. FeCl3(aq) + NaOH(aq) Fe(OH)3(s) + NaCl(aq)

9. State of matter • Letters indicate the state of each compound (aq) =aqueous/ dissolved in water (s) = solid (l) = liquid (g) = gas 2NO(g) + O2(g) 2NO2(g) Coefficients • indicate the ratio of compounds in the reaction • here, there is twice as much NO and NO2 than there is O2 See pages 202 - 203

10. Conservation of Mass in Chemical Change Chemical change means new compounds are created. • BUT no new matter is created or destroyed; atoms are just rearranged. All matter in reactants = all matter in products See pages 204 - 205

11. Law of Conservation of Mass In 1785 French Chemist, Antoine Lavoisier and his wife Maire-Anne stated, "We may lay it down as an incontestible axiom, that, in all the operations of art and nature, nothing is created; an equal quantity of matter exists both before and after the experiment; the quality and quantity of the elements remain precisely the same; and nothing takes place beyond changes and modifications in the combination of these elements."

12. Law of Conservation of Mass: Matter can not be created nor can it be destroyed Total Mass of = Total Mass of Reactants Products

13. Law of Conservation of Mass John Dalton, 200 years ago, realized that atoms simply rearrange themselves during chemical reactions.

14. The Law of Conservation of Mass • Mass is constant in chemical reactions, • The total mass of the products is always equal to the mass of the reactants Mass of reactants = Mass of products If you could collect and measure all of the exhaust from this car, you would find that mass of reactants (gas + O2) = mass of products (exhaust)! See pages 204 - 205

16. Writing and Balancing Chemical Equations • The simplest form of chemical equation is a word equation Potassium metal + oxygen gas  potassium oxide See page 206

17. Writing and Balancing Chemical Equations • A skeletonequation shows only the formulas of the reactants and compounds • Shows types of atoms, but not quantities • K(s) + O2(g) K2O(s) • A balanced chemical equation shows all atoms and their quantities • Balancing ensures that the number of each atom is the same on both sides of the reaction arrow • Always use the smallest whole number ratio • 4K(s) + O2(g) 2K2O(s) See page 206

18. Writing and Balancing Chemical Equations • A balanced chemical equation shows all types of atoms and their quantities. • Balancing ensures that the number of each atom is the same on both sides of the reaction arrow • Can only add/change coefficients to balance. • Always use the smallest whole number ratio • 4K(s) + O2(g) 2K2O(s)

19. Counting Atoms We count atoms in the following way: Reactants: Na2­CO3 + CaCl2 Na2­CO3 means 1 molecule of Na2­CO3 ( 1 x 2 Na, 1 C, and 1 x 3O) CaCl2means 1 molecule of CaCl2 ( 1 x Ca and 1 x 2 Cl)

20. Counting Atoms Products: CaCO3 + 2 NaCl CaCO3 means 1 molecule of CaCO3 ( 1 x 1 Ca, 1 C, and 1 x 3O) 2 NaCl means 2 molecules of NaCl ( 2 x 1Na and 2 x 1 Cl)

21. Counting Atoms to Balance an Equation Word equation: Methane + oxygen  water + carbon dioxide Skeleton equation: CH4(g) + O2 (g)  H2O(l) + CO2(g) • To balance the compounds, take note of how many atoms of each element occur on each side of the reaction arrow. • 1 Carbon, 4 Hydrogen, 2 Oxygen  1 Carbon, 2 Hydrogen, 3 Oxygen See page 207

22. Counting Atoms to Balance an Equation To balance, attempt to find values that equate atoms on both sides • Balanced equation: CH4(g) + 2O2 (g)  2H2O( ) + CO2(g) 1 Carbon, 4 Hydrogen, (2x2) Oxygen  1 Carbon, (2x2) Hydrogen, (2x1)+2 Oxygen See page 207

23. Ex. Zinc metal and hydrochloric acid react to form zinc chloride and hydrogen gas word equation: zinc + hydrochloric acid  zinc chloride + hydrogen gas

24. Try to write the following chemical reaction as a word equation Aluminium metal and copper(II) chloride solution react to form copper metal and aluminium chloride.

26. Copper(II) chloride solution reacts with sodium hydroxide to form copper(II) hydroxide and sodium chloride

27. Hints for Writing Word Equations • Chemical equations can be written using chemical names instead of formulas. Eg. The chemical reaction of photosynthesis in plants consumes light energy and covnerts it into chemical energy in the form of sugar. Word equation: carbon dioxide + water  glucose + oxygen

28. Hints for Writing Chemical Equations • Several common covalent molecules containing hydrogen have common names that do not help in writing chemical formulas • For example, • methane = CH4, • glucose = C6H12O6, • Ethane = C2H6, • Ammonia = NH3 See page 208

29. Hints for Writing Chemical Equations • The chemical symbol is used for most elements when they represent a single element. Eg Fe • Remember the formulas for the three common compounds containing hydrogen; methane CH4, ammonia NH3, and water H2O. • Be careful of polyatomic ions such as ammonium (NH4 +), and carbonate (CO32-).

30. Hints for Writing Chemical Equations • Be careful of diatomic and polyatomic elements such as O2, P4 and S8 • The “special seven” are all diatomic elements (hockey stick & puck) • H2, N2, O2, F2, Cl2, Br2, I2 See page 208

31. word equation: zinc + hydrochloric acid  zinc chloride + hydrogen gas

32. Try to write the following word equation as a skeleton equation: • aluminium + copper(II) chloride solution  copper + aluminium chloride

33. copper(II) chloride + sodium hydroxide  copper(II) hydroxide + sodium chloride

34. Balancing Equations Examples Balance the following: Fe + Br2 FeBr3 Left Right • Balance Fe: 1 1 • Balance Br 2 3 X3 X2 Br = 6 6 3. Balance Fe again X2 X2 2 2 2 Fe + 3 Br2  2 FeBr3 See pages 209 - 211

35. Balancing Equations Examples Balance the following: Sn(NO2)4 + K3PO4  KNO2 + Sn3 (PO4)4 See pages 209 - 211

36. Balancing Equations Examples Balance the following: C2H6 + O2  CO2 + H2O Take the Section 4.3 Quiz See pages 209 - 211

37. Strategies for Balancing Equations • Trial and error will work, but can be very inefficient • Balance compounds first, single elements last • Balance one compound at a time • Only add coefficients; NEVER change subscripts! • Balance metals first, then nonmetals, then H & O • If H and O appear in more than one place, attempt to balance them LAST • Polyatomic ions (such as SO42–) can often be balanced as a whole group • Always double-check after you think you are finished! See pages 209 - 211