1. Chapter 1 Basic Concepts About Matter
Chemistry = the study of the composition, structure, properties and reactions of matter.
Matter = anything that has mass and occupies space (all the substances that make up our world).
Chemistry is a science that requires us to deal with all the stuff that we see around us. Chemistry happens all around you every day.

2. States of Matter
Shape:
Volume:
Particles:
Interaction:
Movement:

3. Properties of Matter: distinguishing characteristics that help us to identify a substance
Physical Properties
can be determined without
changing the composition of
substances

4. Chemical Properties
Describe the way a substance undergoes change (or resists change) to form a new substance.

5. Physical Changes – the state or appearance may change, but the composition remains the same
A Change in State is a Physical Change:
Melting & Freezing
Evaporation, Boiling, Condensation
Sublimation & Deposition

6. Other examples of Physical Change:
Cutting
Dissolving (creating a mixture?)
Changing Shape

7. Chemical Changes – the original substance is converted into a new substance, which has different physical & chemical properties
Examples of Chemical Change:
Rusting (Corrosion)
Combustion
Decompostion
Fermentation

8. Is it a Physical Change or a Chemical Change?
An ice cube melts
Paper is cut into pieces
Sugar dissolves in water
Silver becomes tarnished
Wet clothes dry on a clothesline
Milk turns sour and becomes curdled when heated
wood is burned in a campfire

9. Classification of Matter
2 Types of Pure Substances
Elements: Compounds:
The simplest type of pure substance Composed of 2 or more elements
Composed of only one kind of atom Atoms of different types
Cannot be broken down chemically Held together by bonds
Designated by symbols Can be broken down chemically Cannot be broken down physically Chemical formula

10. Some Elements can be found free in nature

11. Some Common Compounds

12. Mixtures: 2 or more pure substances
Each substance retains its identity
Variable composition
2 types of mixtures:
Homogeneous = 2 or more substances in one phase
(also called a solution)
Heterogeneous = 2 or more substances in 2 or more phases

13. Can be separated by physical means

15. Is it an Element? Compound? Homogeneous Heterogeneous Mixture?
Dry ice Room air Orange juice Diet Coke on ice Diamond Blood Brass Milk Water Table salt Quartz Salt water Tap water Gasoline Sucrose Iron Fruit salad Baking soda

16. Abundance of the Elements:
EARTH’S CRUST
HUMAN BODY

17. Elements in the Human Body:

18. Names and Symbols of the Elements:
Chemical Symbols: 1- or 2-letter designation for an element
Symbols are derived from the element’s name
a few are from Latin/German names
118 known elements
88 occur naturally—most as part of a compound
30 have been made in the laboratory

19. Atoms and Molecules:
Atom = the smallest particle of an element that can exist and still have the properties of the element.
Pure Element = a substance composed of atoms of a single type.
Molecule = a group of 2 or more atoms bound together to form a unit.
Atoms in a molecule may be of the same element or of different elements.
Compound = 2 or more different elements chemically combined.

20. Homoatomic Molecules:
All atoms are of the same element
Heteroatomic Molecules: H H
Two or more kinds of atoms O

21. Chemical Formulas: Diatomic Molecules: Triatomic Molecules:
Chemical Symbols of element(s)
Numerical Subscripts
Compounds or Homonuclear Molecules

22. [Not all compounds are “molecules”]
Chemical Formulas of Ionic Compounds:
Smallest whole number ratio of elements in the compound
“Formula Unit”

23. Interpretation of Chemical Formulas:
How many atoms of each element are present in one molecule or one formula unit:
C9H8O4
Al2(SO4)3
COCl2
CoCl2 O2