1. Matter & Its Properties
Modern Chemistry Textbook: Ch. 1

2. Basic Building Blocks of Matter

3. What is matter? Anything that takes up space and has mass
Takes up space  volume
Certain amount of stuff  mass
How does one make stuff?
Start with the ATOM!

4. What is chemistry? The study of matter and the changes it undergoes
Composition
Structure
Properties
Energy changes

5. Elements vs. Compounds
Atom – smallest unit of an element that has the chemical identity of that element
Element – Pure substance that cannot be broken down into simpler, stable substances
So only 1 kind of atom
Examples; Na, H2, Cl2, Ca
Compound – Pure substance that can be broken into simpler, stable substances
must have 2 different kinds of atoms
Examples; H2O, NaCl, CO2

6. Is this an element?

7. What’s the Difference between States of Matter Video
Elements & Compounds can be found in many different states of matter or phases
What’s the Difference between States of Matter Video
Substances only move from one phase to another by physical means.
States of Matter

8. Physical vs. Chemical Properties
Physical change – change in which identity of substance is not altered
Examples: ripping, heating, freezing
Physical property – characteristic of a substance that can be observed/measured without altering substances identity
Examples: color, size, texture

9. Extensive Property: a property of a substance that changes when the amount changes; it is dependent on the AMOUNT of substance present
Examples: volume, mass, energy…
Intensive Property: a property of a substance that is always the same for that substance; it is NOT dependent on the AMOUNT of substance present
Examples: density, boiling point, melting point, conductivity…

10. Physical changes will always require the absorption/release of energy
(Heat or light)

11. What physical characteristics can you observe to determine a substance’s state of matter?
Shape
volume
Indefinite volume
Indefinite shape
Definite volume
Definite shape
Definite volume
Indefinite shape

12. Plasma: high-temperature state of matter in which atoms lose most of their electrons

13. What if a substance’s identity is altered?
Chemical Property – ability to undergo changes that transforms substance into a new substance Chemical change – change in which 1 or more substances are converted into different substances

14. substances that are formed
Chemical Changes
yields
Reactants
substances that react
Products
substances that are formed

15. Evidences of Chemical Change
Evolution of energy (heat/light)
Color change
Formation of a gas
Formation of precipitate

16. Energy is always involved in physical and in chemical changes
Law of Conservation of Energy: energy can be absorbed or released, but is never destroyed or created.

17. Physical
Chemical
Extensive
Intensive
1. Color
2. Combustibility
3. Hardness
4. Luster
5. Flammability
6. Reacts with acids to form H2
7. Mass
8. Density
9. Melting Pt.
10. Can neutralize a base
11. Ductility
12. Odor
13. Weight
14. Malleability
15. Tendency to corrode
16. Length ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔ ✔

18. C C
_______ 1 . Hydrochloric acid reacts with potassium hydroxide to produce a salt, water and heat. _______ 2. A pellet of sodium is sliced in two. _______ 3. Water is heated and changed to steam. _______ 4. Iron rusts. _______ 5. Evaporation _______ 6. Milk sours. _______ 7. Ice melting.
_______ 8. Wood rotting. _______ 9. When placed in H2O, a sodium pellet catches on fire as H2 gas is liberated and sodium hydroxide forms. _______ 10. Grass growing in a lawn. _______ 11. A tire is inflated with air. _______ 12. Food is digested in the stomach. _______ 13. Water is absorbed by a paper towel. _______ 14. Sugar dissolved in water. C P C P P C C P C P P P

19. Classification of Matter
Grouping matter to make identification easier

20. Mixtures
Blend of 2 or more kinds of matter, each that retain its own identity and properties
Mixed together physically
Can be separated physically (no chemical rxn’s needed)
Homogeneous (solutions): uniform in composition
Salt – water solution
Heterogeneous: not uniform throughout
Clay-water mixture

21. Heterogeneous mixture
Homogenous mixture
Heterogeneous mixture

22. Heterogeneous Mixtures
Suspensions – particles in solvent so large that they settle out unless constantly stirred/agitated
Colloids – particles of intermediate size that stay dispersed throughout a mixture.
Often appears cloudy
Use Tyndall Effect to identify (shine light source through mixture and particles become visible in beam of light)

23. Pure Substances Fixed composition
Every sample of pure substance has exactly the same properties and composition
Ex: Water is always 11.2% hydrogen and 88.8% oxygen by mass (determined from periodic table)

26. Pure substance or mixture Column B
Column A
Pure substance or mixture
Column B
Element or Compound/Heterogeneous or Homogeneous
1. Chlorine
2. Water
3. Soil
4. Sugar water
5. Oxygen
6. Carbon dioxide
7. Rocky road ice cream
8. Alcohol
9. Pure air
10. Iron

28. Introduction to the Periodic Table
Section 1.3

29. What is the periodic table?
Why don’t elements and their symbols always look like they correspond to each other?

31. Groups
Periods

32. Groups & Families
The vertical columns of the periodic table are called groups, or families.
Each group contains elements with similar chemical properties.
The horizontal rows of elements in the periodic table are called periods.
Physical and chemical properties change somewhat regularly across a period.

33. 4 Basic Categories of Elements

35. elements to the left of the zigzag line
Metals
elements to the left of the zigzag line
Properties of metals
Most solids at room temperature
Malleable (hammered or rolled into thin sheets)
Ductile (drawn into a thin wire)
conduct electricity and heat well

36. Metals
Gold, copper, aluminum

37. Nonmetals right of the zigzag line
an element that is a poor conductor of heat and electricity
Properties of nonmetals
many are gases
solids are brittle
poor conductors of heat and electricity

38. (a) carbon, (b) sulfur, (c) phosphorus (d) iodine
Nonmetals
(a) carbon, (b) sulfur, (c) phosphorus (d) iodine

39. Metalloids surrounds zigzag line
an element that has some characteristics of metals and some characteristics of nonmetals
Properties of metalloids
all metalloids are solids at room temperature
semiconductors of electricity
**Aluminum is not a metalloid – it’s a metal!

40. Noble Gases Elements in Group 18 Properties of Noble Gases
Generally unreactive (i.e. “inert”)
Gases at room temperature
Glow if electricity is passed through them