1. How can we describe matter? Page 39
Extensive Properties – depend on the amount of matter in a sample
Ex. Mass, Volume
Intensive Properties – depends on the type of matter, not the amount
Ex. Density, Boiling Point, Freezing Point

2. Identifying Substances
Substance - matter that has a uniform and definite composition
Physical Property – a property that can be observed without changing the substance’s composition
Color, Luster, Malleability, Boiling/Melting/Freezing Point, Density, conductivity,

3. States of Matter and Phase Changes P. 41
Chapter 2: Matter and Change
States of Matter and Phase Changes P. 41
Exothermic
Exothermic
P. 59 Q
Exothermic

4. Is it a gas or a vapor?
Vapor – the gaseous state of a substance that is generally a solid or gas at room temperature
Question 40 - P. 58

5. Physical Change – a property of a substance that changes but the identity of the substance does not
Ex. Melting, freezing, splitting, grinding Density of water (l) – 1.00 g/cm3 Density of water (s) g/cm3

6. Classifying Mixtures – a blend of two or more substances
Heterogeneous
Not uniform throughout
Ex. Salad dressing, Sand, chocolate chip cookie dough
Homogeneous
Uniform throughout
Solution – liquid or gas
Coke, Sea water, gold jewelry, air
P. 58 Q-44-46, P. 59 Q 66

8. Separating Mixtures Density
Filtration – separates a solid from a liquid in a heterogeneous mixture
Distillation – separates a homogenous mixture of water and another substance (Boiling Points)
P. 58 Q - 47

9. Element
Simplest form of matter that has a unique set of properties
Ex. Carbon, Oxygen, Iron
Compound
A substance that contains 2 or more elements chemically combined in a fixed proportion
Ex. Salt – NaCl, Glucose C6H12O6
Can be broken down into simpler substances by chemical means

10. Representing Elements and Compounds
Element – first letter capital, second letter lower case K = Potassium Na = Sodium Aspirin – C8H9O2N
Subscript – indicates the number of atoms, follows the element
P. 58 Q - 50,52

11. Compounds - continued Cu(NO3)2
Multiply the subscripts inside and outside the parentheses to determine the number of atoms
Subscript outside the parentheses only refers to the elements inside

12. Indicate the names of each element and the total number of atoms in each compound.
MgCl2 Ca3(PO4)2 CrCO3 Ca(C2H3O2)

13. Breaking Down Compounds
Chemical change –produces matter with a different composition than the original matter Heating – raw egg vs. fried egg Electricity – decomposes water into H2 and O2 gas.

14. Indicators of a Chemical Change
color change
production of a gas
formation of a precipitate (solid)
transfer of energy
Production of light
Change in Temperature
Exothermic – release in heat, increase in temp.
Endothermic – heat absorption, decrease in temp.
multiple forms of evidence are needed
P. 59 Q

15. s = solid, l = liquid, g = gas, aq = aqueous
Chemical Property – the ability of a substance to undergo a specific chemical change Ex. Reactivity with acids, flammability, decomposition
Coefficients – state the number of individual atoms, compounds or molecules
4Fe(s) + 3O2(g)  2Fe2O3(s)
rust
State of matter – before and after the reaction
s = solid, l = liquid, g = gas, aq = aqueous
P. 59 Q - 67

16. Chemical and Physical Properties

17. Law of Conservation of Matter
Mass is neither created nor destroyed in a chemical reaction it is conserved
Mass reactants = Mass products
Antoine Lavoisier ( )

18. Applying the Law of Conservation of Matter
4Fe (s) + 3O2 (g)  2Fe2O3 (s)
3.5 kg
x kg
3.7 kg + =
x = .2 kg

19. Sn (s) + 4HCl (aq)  SnCl4 (s) + 2H2 (g)
When 5.0 g of tin reacts with hydrochloric acid, the mass of the products tin chloride and hydrogen totals 8.1 g.
Sn (s) + 4HCl (aq)  SnCl4 (s) + 2H2 (g)
How many grams of hydrochloric acid were used?
How many atoms of hydrogen are present on the reactants side of the equation? Products?
How many atoms of tin are present on the reactants side of the equation? Products?
How many atoms of chlorine are present on the reactants side of the equation? Products?
Identify the state of each reactant.
Identify the state of each product.
How many molecules of HCl are present? H2?
P. 55 #34, P. 58 # 56 P. 61 #10-14