1. TOPIC 1 STOICHIOMETRIC RELATIONSHIPS
1.1
INTRODUCTION TO THE PARTICULATE NATURE OF MATTER AND CHEMICAL CHANGE

2. ESSENTIAL IDEA
Physical and chemical properties depend on the ways in which different atoms combine.
NATURE OF SCIENCE (3.1)
Making quantitative measurements with replicates to ensure reliability – definite and multiple proportions.

3. UNDERSTANDINGS/KEY IDEA 1.1.A
Atoms of different elements combine in fixed ratios to form compounds, which have different properties from their component elements.

4. UNDERSTANDINGS/KEY IDEA 1.1.B
Mixtures contain more than one element and/or compound that are not chemically bonded together and so retain their individual properties.

5. UNDERSTANDINGS/KEY IDEA 1.1.C
Mixtures are either homogeneous or heterogeneous.

6. Chemistry:
Chemistry is the study of what things are made up of, and the changes that they undergo

7. Physical combinations of two or more substances
MATTER
Anything that has mass
and takes up space
(Pure) Substances
Mixtures
Physical combinations of two or more substances
Homogeneous
Heterogeneous
Uniform throughout,
aka “solution”;
Think: smoothie
Not uniform throughout,
distinct pieces;
Think: fruit salad

8. Pure Substances: Elements & Compounds
occur naturally, same composition throughout the substance and everywhere in the world

9. MATTER (Pure) Substances Mixtures Elements Compounds Homogeneous
Stuff that has mass
and takes up space
(Pure) Substances
Mixtures
Have a specific or definite composition
(homogeneous)
Physical combinations or two or more substances
Elements
Compounds
Homogeneous
Heterogeneous
Uniform throughout,
aka “solution”;
Think: smoothie
Not uniform throughout,
distinct pieces;
Think: fruit salad

10. Elements Elements: The simplest form of matter
Cannot be broken down or separated into a simpler substance
Building blocks for all other substances
Found on the periodic table of elements

11. MATTER (Pure) Substances Mixtures Elements Compounds Homogeneous
Anything that has mass
and takes up space
(Pure) Substances
Mixtures
Have a specific or definite composition
(homogeneous)
Physical combinations of two or more substances
Elements
Compounds
Homogeneous
Heterogeneous
Examples: iron
sulfur, carbon,
Hydrogen, oxygen
Uniform throughout,
aka “solution”;
Think: smoothie
Not uniform throughout,
distinct pieces;
Think: fruit salad

12. Compounds Compounds: Chemical combination of 2 or more substances
Cannot be physically separated
Have properties different than the elements that are combined

13. MATTER (Pure) Substances Mixtures Elements Compounds Homogeneous
Stuff that has mass
and takes up space
(Pure) Substances
Mixtures
Have a specific or definite composition
(homogeneous)
Physical combinations of two or more substances
Elements
Compounds
Homogeneous
Heterogeneous
Examples: iron
sulfur, carbon,
Hydrogen, oxygen
Examples: water,
salt, sugar
Uniform throughout,
aka “solution”;
Think: smoothie
Not uniform throughout,
distinct pieces;
Think: fruit salad

14. Recall separation Techniques

15. APPLICATION/SKILLS
Be able to deduce chemical equations when reactants and products are specified.

16. Atoms cannot be created or destroyed in a chemical reaction, they can only be rearranged.
The reactants (substances on the left side of the arrow) are transformed into products (substances on the right side of the arrow).
All chemical reactions must be balanced – the number of atoms of each element must be the same on each side of the equation.

17. The coefficients in an equation give the molar ratios of the reactants and products.
2H2(g) + O2(g)  2H2O(l)
This tells us that 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.

18. 2H2(g) + O2(g)  2H2O(l)
The mole ratio is a ratio of the coefficients in the balanced chemical equation.
When working stoichiometry problems, the coefficient for the unknown is always on top.
The mole ratio of hydrogen to oxygen is 2 to 1.
The mole ratio of oxygen to water is 1 to 2.

19. APPLICATION/SKILLS
Be able to apply the state symbols (s), (l), (g) and (aq) in equations.

20. 2H2(g) + O2(g)  2H2O(l)
The states of substances are indicated in parenthesis next to the formula.
Solid (s)
Liquid (l)
Gas (g)
Aqueous solution (aq) – indicates that the ions are dissolved in water.
A single arrow  means the rxn essentially goes to completion.
A double arrow means equilibrium.

21. APPLICATION/SKILLS
Be able to explain the observable changes in physical properties and temperature during changes of state.

22. Heating/cooling curve for water
Oxford chemistry companion

23. Identify states of matter at A,B,C,D,E E D C B A A

24. APPLICATION/SKILLS
Be able to name the changes of state – melting, freezing, vaporization (evaporation and boiling), condensation, sublimation and deposition.

25. Melting: solid to liquid Freezing: liquid to solid Vaporization: liquid to gas Condensation: gas to liquid Sublimation: solid to gas Deposition: gas to solid

26. Be able to balance a variety of reaction types.
APPLICATION/SKILLS
Be able to balance a variety of reaction types.

27. Writing Chemical formula
 Ionic compounds are neutral compounds made of positive cations and negative anions.
Writing the chemical formula for ionic compounds is fairly easy.
Write the cation symbol, then the anion symbol. Find the lowest common multiple for the ions to make the compound neutral.

28. Practice Workout Chemical formula

29. You need to be familiar with these Poly atomic Ions

30. Some Important Acids

31. Balancing Equations H2 + O2  H2O hydrogen + oxygen  water Reactants
Products H 2 O 2 1

32. YOU CANNOT CHANGE THE SUBSCRIPTS
Balancing Equations X
hydrogen oxygen  hydrogen peroxide
H O  H2O2
YOU CANNOT CHANGE THE SUBSCRIPTS
Reactants
Products H 2 O

33. Balancing Equations 2 H2 + O2  H2O hydrogen + oxygen  water
Reactants
Products H 2 O 1

34. Balancing Equations H2 + O2  H2O 2 hydrogen + oxygen  water
Reactants
Products H 2 4 O

35. Balancing Equations 2 H2 + O2  H2O 2 hydrogen + oxygen  water
Reactants
Products H 4 O 2

36. Balancing Tricks Balance chemical equations by following these steps:
Trial and error will work but can be very inefficient.
USE A TABLE (write atoms underneath reactants and products)
If they look the same on both sides of the equation, treat polyatomic ions (such as SO42–) as a group & balance them as such.
If ‘OH’ and H2O are in the equation, write water as HOH.
Balance one compound at a time & rewrite the # of atoms in the chart as things change.
Only add coefficients; NEVER change subscripts!!!
If H and O appear in more than one place, attempt to balance them LAST.
Balance everything that isn’t ‘H’ or ‘O’ 1st.
Balance the ‘H’s 2nd to last.
Balance the ‘O’s last.
Always double-check after you think you are finished.
CHECK YOUR ANSWERS!!!

37. Balance the following:
Fe + Br2 FeBr3
Sn(NO2)4 + K3PO4  KNO2 + Sn3 (PO4)4
C2H6 + O2  CO2 + H2O

38. ____Ba + ____H2O  ____Ba(OH)2 + ____H2
 ____CO2 + ____H2O  ____H2CO3   
____Fe2O3 + ____C  ____Fe + ____CO
____Fe + ____H2O  ____H2 + ____Fe2O3

39. Types of Reaction A B C D

40. Combustion Reaction

41. 5 Basic Types of Reactions
1. Combination or synthesis
2. Decomposition
3. Single Replacement
4. Double Replacement
5. Combustion

42. 2 3 2 Al + Cl2 AlCl3 Combination
Reaction where 2 substances combine into a single substance.
A + B → AB 2 3 2
Al + Cl2 AlCl3

43. The equation is already balanced
Decomposition
Reaction where 1 substance breaks into 2 or more substances.
AB → A + B
CaCO3 → CaO + CO2
The equation is already balanced

44. Single Replacement
Reaction where an element replaces a similarly charged ion in a compound.
A + BC → B + AC
AgNO3 + Cu  Cu(NO3)2 + Ag 2 2

45. Double Replacement
Reaction where two compounds react to produce two new compounds.
AD + BC → BD + AC
Na3PO KOH  NaOH + K3PO4
Write the charges on top of the elements in the reactants and exchange the positive ions to make new compounds.
You must have a positive followed by a negative to make a compound. 3 3

46. Combustion
Reaction where an element or compound(usually a hydrocarbon) reacts with oxygen.
Usually the products are Carbon dioxide and water
CH O2 → CO H2O 2 2

47. Atom Economy
Atom Economy looks into the efficiency of a chemical reaction by comparing the molecular masses of the reactants to the molecular masses of the useful compound.
% Atom Economy = Mass of desired product from equation x 100
Total mass of reactants from equation

48. Atom Economy
A number between 0 and 100 that shows how economically a reaction produces the desired product.
The higher the number the more economical the reaction is.
No practical work is required to find the atom economy of a reaction.

49. Find atom Economy for hydrogen gas
C H2O CO H2
8.3%

50. TRUE Quick Question Atom Economy for C + O2 CO2 is 100% TRUE or False
Answer is
TRUE

51. Citations
Brown, Catrin, and Mike Ford. Higher Level Chemistry. 2nd ed. N.p.: Pearson Baccalaureate, Print. Most of the information found in this power point comes directly from this textbook. The power point has been made to directly complement the Higher Level Chemistry textbook by Catrin and Brown and is used for direct instructional purposes only.