1. Unit 1: (1)Classification of Matter
Physical Science
PSc.2.1 Understand types, properties, and structure of matter.

2. Classifying Matter Matter is………
anything that has mass and takes up space
made up of atoms
NOT matter: Light, Sound, and
Electricity

4. Classification of Matter
Matter is usually categorized by make-up and/or composition.
Things are grouped together that have certain similarities.
Classification – grouping things together based on similarities.
Matter can be classified as:
Pure substance
Mixture

5. Pure Substances and Mixtures
Always has same composition
Every sample of a given substance has the same properties because a substance has a fixed, uniform composition.
Can be classified into two categories: Elements and Compounds
Mixtures
Made of 2+ substances
Mixed together physically but not chemically (think of lemonade).

6. Pure Substances
Sugar cannot be broken into other substances by physical means; only by chemical changes.

7. Other Pure Substances
Salt, a compound
Gold, an element
These substances are all elements or compounds. They have fixed compositions, which means they never change. These are pure substances.
Water, a compound
Chromium, an element

8. Elements Elements Simplest pure substance.
Cannot be broken down into any simpler substance.
Example: oxygen, nitrogen, carbon, etc.
Atom = smallest particle of element.
Atoms of different elements are different.
There are about 115 known elements at this time.
92 occur naturally; the rest were made in laboratories.

9. Symbols Chemical symbols
Shorthand way to write the name of an element.
One or two letters.
First letter always capitalized.
Second letter lowercase.
Most symbols come from the element’s English name.
A few come from the element’s Latin name.

10. Elements & Symbols
2nd

11. Elements & Symbols
The symbols of the following elements come from their English name:
Oxygen (O)
Lithium (Li)
Strontium (Sr)
Nickel (Ni)

12. Elements & Symbols
The symbols of the following elements come from their Latin name:
Iron (Fe: Latin name = Ferrum)
Gold (Au: Latin name = Aurum)
Potassium (K: Latin name = Kalium)
Lead (Pb: Latin name = Plumbum)

13. Compounds Two or more elements
Chemically combined in a fixed proportion
Pure substances
Each particle or unit of a compound is exactly alike
Can be broken down into elements by chemical means only.
Ex. Sodium Chloride = sodium + chloride

14. Compounds Have diff. properties from the elements that make them up.
Example:
Hydrogen is an extremely flammable gas.
Oxygen supports burning.
Together they make water, which is not flammable and does not support burning.
Water has different properties from the elements that make it up.

15. Chemical Formulas Chemical formula Formula for water = H2O
Shows the ratio of each element present.
Formula for water = H2O
Understood 1 behind the O
2 atoms of hydrogen (H) to 1 atom of oxygen (O)

16. Chemical Formulas Formula for calcium nitrate = Ca(NO3)2
When a formula has parentheses, the number after the parentheses multiplies everything inside.
1 atom of calcium (Ca)
2 atoms of nitrogen (N)
6 atoms of oxygen (O)

17. Mixtures
Tend to retain some of the properties of their individual substances
Properties can vary because the composition of a mixture is not fixed
Can be classified by how well the parts of the mixture are distributed throughout the mixture.
Can be homogenous or heterogeneous

18. Mixtures Heterogeneous- parts of the mixture are noticeably different
Example: Sand, chocolate chip cookie
These are also called suspensions when they separate from one another. These are substances you must shake before using.
Example: Salad dressing

20. Mixtures
Homogeneous- “same”; not able to distinguish the individual components
These are also called solutions
Ex: swimming pool, stainless steel (mixture of iron, chromium, and nickel), sweet tea.

22. Solutions, Suspensions, and Colloids
The size of the particles in a mixture has an effect on the properties of the mixture.
Based on the size of its largest particles, a mixture can be classified as a solution, a suspension, or a colloid.

23. Solutions (homogenous mixture)
Solutions have 2 parts:
A. Solute- what you are adding to be dissolved; the part that is being dissolved
B. Solvent- what is being used to dissolve something else. Water is the “universal solvent”
Example: Kool-aid

25. Suspensions (heterogeneous mixture)
Separates into layers over time.
Made of larger particles that can scatter light in all directions.
Sometimes appear to look cloudy.
Ex: salad dressing, sand and water, blood and plasma.

26. Colloid- contains medium sized particles that scatter light
Does NOT separate into layers
Example: Fog, milk, whipped cream

27. Review
_____________________ is the study of matter and how it changes.
_____________
Anything that has mass and takes up space
Ex: desk, books, air, water
______________
Combination of more than one pure substance
______________ _ (solution)
a mixture that looks the same throughout
ex: air, salt water, gasoline
________________
A mixture that shows different parts
Ex: pizza, sand, salad dressing, oil and water
Separates into layers over time
Ex: sand and water
Has particles intermediate in size
Ex: fog, smoke
_______________
Matter that has a fixed composition
Can be found on the Periodic Table
Ex: carbon (C); hydrogen (H)
Substance of more than one element bonded together
Ex: water (H2O); salt (NaCl); carbon dioxide (CO2)

28. CHEMISTRY is the study of matter and how it changes.
Anything that has mass and takes up space
Ex: desk, books, air, water
MIXTURE
Combination of more than one pure substance
HOMOGENEOUS (solution)
a mixture that looks the same throughout
ex: air, salt water, gasoline
HETEROGENEOUS
A mixture that shows different parts
Ex: pizza, sand, salad dressing, oil and water
_SUSPENSION__
Separates into layers over time
Ex: sand and water
COLLOID
Has particles intermediate in size
Ex: fog, smoke
PURE SUBSTANCE
Matter that has a fixed composition
ELEMENT
Can be found on the Periodic Table
Ex: carbon (C); hydrogen (H)
COMPOUND
Substance of more than one element bonded together
Ex: water (H2O); salt (NaCl); carbon dioxide (CO2)