1. Chapter 3
3.1 – Properties of Matter

2. Substances Matter – has mass & takes up space
Substance – matter with uniform and definite composition
Ex: Salt, pure water, air, etc.

3. States of Matter
All matter can be classified as one of 3 physical forms:
Solid – definite shape and volume
-Particles tightly packed & do not conform to
container.

4. States of Matter
Liquid – Matter that flows, constant volume, & takes shape of container
-Particles are NOT rigidly held in place and are
less closely packed than those of a solid.

5. States of Matter
Gas – flows to conform to container & fills entire volume
-Large amounts of space between particles & a
gas will compress easily.

6. States of Matter

7. States of Matter
**NOTE** Vapor is NOT the same as gas! ~ Vapor is a solid or liquid at room temp (a gas is still a gas at room temp!) ex: Steam is a vapor

8. Physical Properties of Matter
Physical Property – characteristic that is observable or measured w/o changing composition.
Ex: Denisty, color, melting point, boiling point, smell, etc.

9. Physical Properties of Matter – cont.
Physical properties can be broken down into further into two types:
Extensive Properties – dependent on amount of substance present (mass, length, etc.)
Intensive Properties – amount of substance is not important (density, color, etc.)

10. Chemical Properties
Chemical Property – ability of substance to combine w/ or change into one or more other substances Ex: Rust

11. Observing Properties of Matter
Do surrounding conditions affect properties? How or why not?
When making observations, be sure to state specific conditions such as temperature, pressure, etc. for more repeatable results!

12. Chapter 3
3.2 – Changes in Matter

13. ex: water cycle – (freeze, boil, condense, vaporize, etc)
Physical Changes
Physical Change – change that alters substance w/o changing composition
ex: wadding up paper
Phase Change – transition of matter from one state to another
physical since depends on temp & pressure of surroundings
ex: water cycle – (freeze, boil, condense, vaporize, etc)

14. Chemical Change
Chemical Change – one or more substances changing into new substance
The new substance will have different composition and properties!
Reactants – starting substance
Products – new substance formed
**Decompose, rust, explode, oxidize, corrode, tarnish, burn, rot, etc = chemical rxn.

15. 𝑚𝑎𝑠𝑠 𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 = 𝑚𝑎𝑠𝑠 𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠
Conservation of Mass
Mass is neither created nor destroyed during a chemical rxn ~ it’s conserved!
𝑳𝒂𝒘 𝒐𝒇 𝑪𝒐𝒏𝒔𝒆𝒓𝒗𝒂𝒕𝒊𝒐𝒏 𝒐𝒇 𝑴𝒂𝒔𝒔:
𝑚𝑎𝑠𝑠 𝑟𝑒𝑎𝑐𝑡𝑎𝑛𝑡𝑠 = 𝑚𝑎𝑠𝑠 𝑝𝑟𝑜𝑑𝑢𝑐𝑡𝑠

16. Example 1
In catalytic converter found in car exhaust, carbon monoxide (CO) reacts with oxygen gas ( 𝑂 2 ) to form carbon dioxide ( 𝐶𝑂 2 ). If CO reacts with 16g of 𝑂 2 to form 44g of 𝐶𝑂 2 , what is the mass of CO in the catalytic converter?
𝑚 𝐶𝑂 + 𝑚 𝑂 2 = 𝑚 𝐶𝑂 2
16𝑔+𝑥=44𝑔
28g CO

17. Chapter 3
3.3 – Mixtures of Matter

18. Mixtures Pure Substance – uniform and definite composition
Mixture – Combo of 2 or more pure substances
Each pure substance retains individual chem properties
**Most everyday matter occurs as mixtures since pure substances tend to mix naturally (difficult to keep pure!)

19. Types of Mixtures
Heterogeneous Mixtures – does not blend smoothly throughout (composition is NOT uniform)
Ex: Italian Salad Dressing
Homogeneous Mixture – Constant composition throughout
Ex: Tea
AKA – solutions (can occur as solid, liquid and/or gas)

20. Tyndall Effect
Tyndall Effect – Quick test to differentiate solution from heterogeneous mixture
Shine thin beam (laser) of light through beaker (glass container)
If light does not shine through => solution
If light shines though - heterogeneous

21. Separating Mixtures
Since most substances are physically combined, most can be physically separated! **Take advantage of the physical properties to separate if possible!

22. Techniques for Separating Mixtures
Filtration- easy on heterogeneous solid/liquid mixtures
Use porous barrier to separate solids from liquids (coffee filters)
Distillation – most homogeneous mixtures can be separated using distillation
Based on ∆ in BP
Mixture heated until substance w/ lowest BP boils to a vapor that can be condensed & collected as a liquid

23. Techniques for Separating Mixtures – Cont.
Crystallization – results in the formation of pure solid particles of a substance from soln containing dissolved substance (collects as crystals)
Ex: rock candy
Sublimation – process of changing solid to vapor without melting/going through liquid phase
Can be used to separate 2 solids in mixture when one solid will sublimate and not other

24. Techniques for Separating Mixtures – Cont.
Chromatography – separates compounds of mixture based on ability of each component (gas or liquid) to travel/be drawn across surface of another material (chromatography paper)
Components w/ strongest attraction to surface travel slower

25. 3.4 – Elements and Compounds
Chapter 3
3.4 – Elements and Compounds

26. Elements
All matter can be broken down into small, basic building blocks
Element – pure substance that can’t be separated into simpler substance by phys/chem means
92 elements occur naturally
Each has unique chem name & symbol
1st letter ALWAYS capitalized and other letters are lowercase.
Ex: Gold - Au, Silver – Ag, Oxygen – O, etc.

27. 1st Periodic Table
1869 Russian Chemist (Mendeleev) created 1st version of periodic table
Classification based upon similarities and masses of elements.
Periodic Table – organizes elements into a grid of horizontal rows (periods) & vertical columns (groups/families)

28. Compounds
Compound – made up of 2 or more different elements that are combined chemically
~10 million known compounds
Increases at a rate of ~100,000/year
Chemical symbols make it easy to write formulas for compounds (ex: NaCl, H2O)

29. Compounds – cont. Properties:
Prop. of compound different than prop of individual elements.

30. Classification of Matter
Mixtures
Heterogeneous
Homogeneous
Pure Substance
Elements
Compounds

31. Law of Definite Proportions
Elements that make up compounds always combine in definite proportions.
Law of Definite Proportions – compound is always composed of same elements in same proportion by mass, regardless of sample size

32. Law of Definite Proportions – cont.
Relative amts of elements in compound can be found by percent mass.
% 𝑏𝑦 𝑀𝑎𝑠𝑠= 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑒𝑙𝑒𝑚𝑒𝑛𝑡 𝑚𝑎𝑠𝑠 𝑜𝑓 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 ×100

33. Example 2
A 78.0g sample of unknown compound contains 12.4g of hydrogen. What is % by mass of hydrogen?
12.4𝑔 𝐻 78.0𝑔 𝑐𝑜𝑚𝑝𝑜𝑢𝑛𝑑 ×100=
15.9%

34. Practice
Do #72 & 75 on p. 95