1. Introduction to Matter
Chapter 2 Note-Packet
Introduction to Matter

2. Section 1

3. The study of properties of matter and how matter changes
Chapter 2 Notes
Chemistry
The study of properties of matter and how matter changes
Physical properties
Matter has two kinds of properties
Chemical properties
Matter
Anything that has mass and takes up space
Substance
The same composition and properties
Always has
A single kind of matter that is pure

4. Can be used to classify matter
Chapter 2 Notes
Properties of Matter
Physical property
Chemical property
Characteristic of a pure substance that can be seen without changing it into another substance
Characteristic of a pure substance that describes its ability to change into different substances
Example
Example
Can be used to classify matter
Liquid water freezing into ice
Iron combines with oxygen to form rust

5. Elements are the simplest substance!
Chapter 2 Notes
Element
Elements are the simplest substance!
Pure substance that cannot be broken down into any other substance by chemical or physical means
Molecules
Group of 2 or more atoms held together by a chemical bond
When atoms combine
A chemical bond forms- a force of attraction between the two atoms
Example
The basic particle from which all elements are made
Two Hydrogen atoms and one Oxygen atom forms water
Atoms

6. C O C O 2 Chapter 2 Notes Compounds Chemical Formula
Pure substance made of two or more different elements chemically combined in a set ratio
Shows the elements in a compound and the ratio of atoms
Elements that are chemically combined have different properties from the uncombined elements
Chemical Formula C O C O 2
A different ratio equals a different compound
The ratio of Carbon to Oxygen is 1:2

7. Compounds- The combined elements change their properties.
Chapter 2 Notes
Contrast
Mixture
Compounds- The combined elements change their properties.
Mixtures- The combined elements keep their properties.
A mix of two or more substances that retain their own properties
Heterogeneous
Homogeneous
Mixture where you can see the different parts
Mixture where you cannot see the different parts
A homogeneous mixture is called a solution
Examples
Salad in a bowl
Dissolved sugar in water

8. Section 2

9. The measure of the force of gravity on you
Weight
Mass
The measure of the force of gravity on you
The measure of the amount of matter in an object
Relates to
Units
Grams (g)
Does not change with location
Formula
Volume = Length x Width x Height
Units
Density
g / cm3
Volume
The mass of a material in a given volume
The amount of space that matter occupies
Formula
Units
Density = Mass
Volume
Liter (L), milliliter (mL) and cubic centimeter (cm3)

10. Section 3

11. Combination of fuel with oxygen
Physical Change
Chemical Change
When a substance changes, but is still the same substance after the change
When a substance changes into a new substance with properties different from the original
Combustion
Combination of fuel with oxygen
Changes of state
Electrolysis
Using electricity to break down compounds
Changes of shape or form
Oxidation
Tarnishing
Combination of substance with oxygen
Combining metals with substances, producing dark coat on metal

12. A change in matter that produces one or more new substances
Chemical Reactions
Changes in Color
A change in matter that produces one or more new substances
A color change may signal that a chemical change has occurred
Chemical changes occur when bonds break and new bonds form
Precipitate may form
A solid that forms from solution during a chemical reaction is a precipitate
Evidence for chemical Reactions, or changes
A gas may form
If a chemical change occurs from liquids or solids, a gas may form

13. The next video shows a color change, and a precipitate!

15. Chemical or physical changes in matter includes a change in energy
The ability to do work or cause change
Always flows from hot to cold
Temperature
Thermal Energy
The average energy from the random motion of matter particles
The total energy of all the particles in an object
Endothermic Change
Exothermic Change
Change in which energy is taken in
Change in which energy is released

16. + Law of Conservation of Mass
All the atoms present at the start of a reaction are present at the end
Matter cannot be created or destroyed
In a chemical reaction, the total mass of the reactants must equal the total mass of the products
Matter can only be changed!
Iron (6 atoms)
Sulfur (6 atoms)
Iron Sulfide (12 atoms) +

17. Section 4

18. The energy of matter in motion
Kinetic Energy
Potential Energy
The energy of matter in motion
The energy an object has because of its position
Forms of Energy
Electric Energy
Chemical Energy
Electromagnetic Energy
Energy of electrically charged particles moving from one place to another
Energy stored in chemical bonds
Energy form that travels through space as waves
Chemical energy may be changed to other forms of energy. Other forms of energy may also be changed to chemical energy!

20. Chapter 2 Notes
Chemistry
Matter has two kinds of properties
Matter
Substance
Always has

21. Chapter 2 Notes
Properties of Matter
Physical property
Chemical property
Example
Example

22. Chapter 2 Notes
Element
Elements are the simplest substance!
Molecules
When atoms combine
Example
Atoms

23. Chapter 2 Notes
Compounds
Chemical Formula
Chemical Formula C O C O 2

24. Contrast
Chapter 2 Notes
Mixture
Compounds- ____________________ _____________________________________________________________________________________________
Mixtures- _______________________ _______________________________
Homogeneous
Heterogeneous
Examples

25. Weight
Mass
Relates to
Units
Formula
Units
Density
Volume
Formula
Units

26. Physical Change
Chemical Change
Combustion
Electrolysis
Oxidation
Tarnishing

27. Evidence for chemical Reactions, or changes
Changes in Color
Precipitate may form
Evidence for chemical Reactions, or changes
A gas may form

28. Energy
Temperature
Thermal Energy
Endothermic Change
Exothermic Change

29. __________________
__________________
__________________________ +

30. Kinetic Energy
Potential Energy
Forms of Energy
Electric Energy
Chemical Energy
Electromagnetic Energy
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