1. Unit 1 – Matter and Measurement
Introduction
Classification of Matter
Properties of Matter
Units of Measurement
Uncertainty in Measurement
Significant Figures
Dimensional Analysis
Periodic Table

2. Introduction Why should YOU study chemistry? Required for your major
Pre-med
Pre-pharmacy
Pre-dental
Biology
Engineering
Nursing

3. Introduction Chemistry impacts our daily lives!
Food, clothing and shelter
Health care
Environment
Life itself
Chemistry investigates and explains the sub-microscopic reasons for the processes that occur in our macroscopic world!

4. Introduction
Sub-microscopic understanding leads to understanding of the world around you:
How does bleach remove stains?
What causes an air bag to inflate?
Why does DNA have a double helical structure?
What makes a rose smell
sweet and old fish smell awful?

5. Introduction How does carbon dating tell how old a fossil is?
What are electrolytes and why do sports drinks like Gatorade contain them?
What happens to garbage in a landfill? Is it always better to use biodegradable materials?

6. Introduction Chemistry
the study of the properties, composition, and behavior of matter
Matter
the materials or substances that make up the universe
Anything that takes up space and has mass
book
dog
air

7. Introduction Mass A measure of the amount of material in an object
A property of matter related to the resistance of an object to being moved
Mass is independent of gravity
Weight is not!

8. Introduction
All matter is composed of one or more of about 110 very basic substances called elements.
Element:
Fundamental or simplest type of matter
A substance that cannot be separated into simpler substances by chemical means.

9. Introduction Elements: Currently >112 known
Each has specific properties and characteristics.
Each has a unique symbol.

10. Introduction Chemical Symbols: One or two letters
1st is capitalized, 2nd is not
often 1st or first 2 letters of the name
Carbon C
Calcium Ca
Boron B
Bromine Br

11. Introduction Some symbols are derived from names in other languages:
Iron Fe (Ferrum)
Sodium Na (Natrium)
Silver Ag (Argentum)
You must know the symbols and names (including correct spellings) of the elements given in syllabus.

12. Introduction Each element is composed of a unique kind of atom.
The smallest representative particle of an element
Atoms can combine to form various types of compounds:
a pure chemical that is made up of two or more elements that are chemically attached to one another

13. Introduction Examples of compounds: Sodium chloride NaCl Water H2O
Ethyl alcohol
CH3CH2OH

14. Introduction
Water and ethyl alcohol are examples of molecular compounds.
The smallest representative particle of a molecular compound is a molecule.
The chemical combination of two or more atoms in which the atoms share electrons
negatively charged subatomic particles

15. Introduction
Law of Constant Composition: The elemental composition of a pure compound is always the same.
Water always has two hydrogen atoms and one oxygen atom.
Ethyl alcohol always has 2 carbons, 6 hydrogens and one oxygen.

16. Classifications of Matter
Several ways to classify matter:
Physical state
Solid
definite shape and volume
Liquid
definite volume but takes shape of container
Gas
takes volume and shape of container

17. Classifications of Matter
Composition
Pure Substance
Mixture
Pure Substance:
All components have the same fixed properties and composition
Element
Compound

18. Classification of Matter
Examples of Pure Substances:
pure water (not tap water)
carbon
sodium chloride (but not table salt)

19. Classification of Matter
Mixture:
A combination of two or more substances in which each substance retains its own chemical identity and properties
Examples of mixtures:
Salt water
Air
Orange juice
All mixtures can be separated into their individual components using various techniques.

20. Classification of Matter
Two types of mixtures:
Homogeneous mixtures
uniform throughout
salt water
sugar in water
ethyl alcohol in water
air

21. Classification of Matter
Two types of mixtures:
Heterogeneous mixtures
different composition, properties and appearance throughout
sand in water
salt and sugar
sand and salt

22. Properties of Matter
Each substance has unique properties allowing us to recognize and distinguish one from another.
Sodium
Chlorine
Sodium chloride (table salt)
soft, silvery metal
reacts violently with water
pale greenish yellow gas
poisonous
colorless crystals
relatively non-toxic
dissolves easily in water

23. Types of Properties
Physical properties can be measured w/o changing the identity and composition of a substance.
Color, odor, hardness, density, temperature, etc.
Chemical properties describe how a substance changes or reacts to form other substances.
flammability

24. Intensive vs. Extensive Properties
Intensive Properties
depend only on the identity of the substance
temperature, density, boiling point, melting point
Extensive Properties
depend on the amount of substance present
volume, mass

25. Physical and Chemical Changes
A substance can undergo both physical and chemical changes.
Chemical change
One substance is transformed into one or more new chemical substances
2H O H2O O2
H2O H2

26. Physical and Chemical Changes
Physical change
A change that does not involve a change in composition or chemical identity
appearance may change but composition does not
ice water
water steam
What happens when water boils?