1. Chapter 3
Matter – Properties and Changes

2. Warm-Up
Complete the Following Conversion: How many centimeters are in 1 mile? Remember to convert them into the most reduced/simplistic format. Required Information 1 Mile = 5280 Ft. 1 Ft. = 12 Inches 1 Inch = 2.54 cm.

3. Warm-Up
Complete the Following Conversion: How many centimeters are in 10 miles? Remember to convert them into the most reduced/simplistic format. 10 Miles x 5280 ft x 12 inches x 2.54 cm = 1,609,344 1 Mile 1 Ft. 1 Inch *Put into Rounded Scientific Notation* 1.61 x 106

4. Substances What is matter? Substance:
Anything that has mass and takes up space
Substance:
Matter that has a uniform and unchanging composition
AKA “Pure Substance”
NOT a mixture
Example: both H2O (dihydrogen monoxide) and Na2 (Table Salt) are both considered Substances. H20+Na2 = Salt Water is NOT a substance, but is a mixture.

5. Physical Properties of Matter
Physical Property: Any property that can be observed and/or measured without changing the physical composition of the sample.
Common Physical Properties:
Density
Color
Odor
Taste
Hardness
Melting Point
Boiling Point

6. Physical Properties and Matter, Cont.
Extensive Properties
Depends on the amount of substance present
Mass, volume and length
Intensive Properties
Independent of the amount of substance present
Density

7. Quick Write
What is the difference between intensive and extensive properties?
What is substance?
What is the difference between a substance and a compound?

8. Quick Write
What is the difference between intensive and extensive properties?
Intensive properties don’t depend on the amount of substance, as they stay they same. Extensive properties depend on the amount of the substance.
What is substance?
A pure substance, that doesn’t have any mixtures, that remains the same wherever the sample is taken.

9. Properties of Matter Chemical Properties Observations of Matter
The ability/inability of a substance to combine with or change into one or more other substances
Iron turns to rust when combined with air
When there is NO chemical change
Observations of Matter
Observing and classifying physical vs. chemical properties of matter
May change depending on the environmental conditions
Think water, which changes state with temperature

10. States of Matter Vapor: States of Matter Solid Liquid Gas
The different physical forms which matter can take.
Solid
Has a definite shape and volume. Molecules are tightly packed and when heated only slightly expands.
Liquid
Matter that flows and has constant volume. Will take the shape of its container. Molecules/particles are not rigidly held in place, less tightly packed and expands when heated.
Gas
Matter that flows to conform to the shape of its container and will fill the entire volume of the container. Gasses are easily compressed, as their molecules are so widely spread.
Vapor:
The gaseous state of a substance that is solid or liquid at room temperature.

11. Changes in Matter Physical Changes Chemical Changes
Altering a substance without changing its composition
Cutting Paper
Breaking a Crystal
Cutting Flowers
Sawing Wood
Chemical Changes
Altering a substance which changes it into a new substance
AKA chemical reaction
Rusting Iron
Burning wood
Terms related to chemical changes: rust, oxidize, corrode, tarnish, ferment, burn, rot

12. Massproducts = Massreactants
Conservation of Mass
Law of Conservation of Mass
Mass is neither created nor destroyed during a chemical reaction – instead, it is conserved.
ALL mass within a reaction, both the products and reactants, must remain the same.
Massproducts = Massreactants

13. Conservation of Mass Practice
If 50 grams of sodium reacts with chlorine to form 126 grams of salt. How many grams of chlorine reacted?
If 20 grams of aluminum reacts with 200 grams of bromide to form aluminum bromide, and no aluminum is left after the reaction, but 23 grams of bromine remained unreacted. How any grams of aluminum bromide were formed?
If g of water is separated into hydrogen and oxygen gas, and the hydrogen gas has a mass of 20.0 g. What is the mass of the oxygen gas produced?

14. Conservation of Mass Practice, Answers
If 50 grams of sodium reacts with chlorine to form 126 grams of salt. How many grams of chlorine reacted?
Massproducts = Massreactants
Masssodium + Masschlorine = Masssalt
50 grams + Masschlorine = 126 grams
Masschlorine = 76 grams
If 20 grams of aluminum reacts with 200 grams of bromide to form aluminum bromide, and no aluminum is left after the reaction, but 23 grams of bromine remained unreacted. How any grams of aluminum bromide were formed?
If g of water is separated into hydrogen and oxygen gas, and the hydrogen gas has a mass of 20.0 g. What is the mass of the oxygen gas produced?

15. Conservation of Mass Practice, Answers
If 50 grams of sodium reacts with chlorine to form 126 grams of salt. How many grams of chlorine reacted?
If 20 grams of aluminum reacts with 200 grams of bromide to form aluminum bromide, and no aluminum is left after the reaction, but 23 grams of bromine remained unreacted. How any grams of aluminum bromide were formed?
Massproducts = Massreactants
Massaluminum + Massbromide = Massaluminumbromide
20+ (200-23) = Massaluminumbromide
Massaluminumbromide = 197 grams
Massbromide = 23 grams
If g of water is separated into hydrogen and oxygen gas, and the hydrogen gas has a mass of 20.0 g. What is the mass of the oxygen gas produced?

16. Conservation of Mass Practice, Answers
If 50 grams of sodium reacts with chlorine to form 126 grams of salt. How many grams of chlorine reacted?
If 20 grams of aluminum reacts with 200 grams of bromide to form aluminum bromide, and no aluminum is left after the reaction, but 23 grams of bromine remained unreacted. How any grams of aluminum bromide were formed?
If g of water is separated into hydrogen and oxygen gas, and the hydrogen gas has a mass of 20.0 g. What is the mass of the oxygen gas produced?
Massproducts = Massreactants
Masswater = Masshydrogengas + Massoxygengas
178.8 grams = 20.0 grams + Massoxygengas
Massoxygengas = grams

17. Elements and Compounds
Pure substance that cannot be separated into simpler substances by any means, including physical or chemical
These are the elements on the periodic table
Dimitri Medeleev
Organized the periodic table into the rows and columns format that is used today
He organized the table into rows called “periods” and columns called “groups”
Traits repeat from period to period, which is why the table is called periodic
Groups have similar physical and chemical characteristics

18. The Periodic Table
Groups
Periods

19. Compounds A chemical combination of two or more elements
Can be broken down into simpler substances, the basic elements
Examples
Na + Cl = NaCl (Sodium Chloride)
N + H3 = NH3 (Ammonia)
C12H22O11 (Sucrose)

20. Mixtures Pure Substances Matter Compounds Heterogeneous Mixtures
Homogenous Mixtures
Pure Substances
Elements
Compounds
Physical Changes
Chemical Changes

21. Law of Definite Proportions
The elements comprising a compound combine in definite proportions by mass
percent by mass (%) = mass of element x 100
mass of compound

22. Law of Definite Proportions Example Problems
There are 200 grams of Ba(NO3)2
Ba = 50 grams
N = 70 grams
0 = 80 grams
50 g Ba / 200 g Ba(NO3)2 x 100 = 25% Ba
70 g N / 200 g Ba(NO3)2 x 100 = 35% N
80 g O / 200 g Ba(NO3)2 x 100 = 40% O

23. Law of Multiple Proportions
When compounds of different elements are formed, they aren’t exactly identical. They might have different amounts of each element, in relative comparison to another.
The law of multiple proportions creates a mass ratio for different elements in similar compounds
Mass Ratio Compound I
Mass Ration Compound II

24. Analysis Data of Two Nitrogen Compounds (NO)
Finding Mass Ratios
Analysis Data of Two Nitrogen Compounds (NO)
Compound
% N
% O
Mass of Nitrogen (N) in g of Compound
Mass of Nitrogen (O) in g of Compound
Mass Ratio
(Mass N / Mass O) I
42.80
57.2
0.74 g N / 1 g O II
56.7
43.6
1.3 g N/ 1 g O
Mass Ratio Compound I = g N/ 1 g O = .57
Mass Ratio Compound II g N/ 1 g O
Final Ratio: .57 : 1

25. Practice Problems
Complete the following problems on page 83 of the textbook. Please show all your work. You should complete these within your lab binder. 61 66 67 69