1. Ch 1 Intro to types of Chemistry
Organic-study of all chemicals containing carbon
Inorganic-chemicals not containing carbon
Analytical-composition of matter
Physical- mechanism, rate, energy transfer of matter undergoing change
Biochemistry- study of processes taking place with organisms

2. Chemistry Applications
Macro- (seen) vs Micro- (need aid to see)
Energy: Conservation,Production, Storage
See chemistry in:
Medicine- medicines, materials, technology
Biotechnology-production of biological products/ processes
Agriculture-develop more productive crops, safer/effective ways to protect crops
Environment- identify and prevent pollutants
Universe- gather data and bring it back to Earth

3. Thinking Like a Scientist
History: chemistry came from alchemy
Alchemists developed tools and techniques for working with chemicals
Lavisier transformed science with creation of balance
Manipulated (independent) vs Dependent (responding variable)
Scientific method: observations, making hypothesis, experimentation, developing theories/laws, communicating findings
Collaboration- working together/ sharing ideas

4. Properties of Matter Depends on amount of matter; mass and volume
Depends on the type of matter the object is made of; hardness
Identical intensive properties/ same composition
Solids, liquids, gases (vapor if gas at room temp.)
Properties change but material does not; boil, condense, split, cut
Extensive Properties
Intensive Properties
Substance
States of matter
Physical changes

5. Elements and Compounds
Element simplest form with chem properties; compound 1+ elements
Change that also changes the composition of matter; break chem bonds
Substance has fixed composition; mixture the composition varies;
Represent elements
Chemical formulas represent compounds
Element vs Compound
Chemical changes
Substance vs mixture
Chemical symbols

6. Mixtures Types of mixtures? Solutions vs suspensions
Separating Mixtures?
Heterogeneous: “ingredients” or many parts to composition
Homogeneous: composition uniform; aka solution
Solution: solute “dissapears” but takes up space; Suspension: non-dissolved material
Use physical properties to separate
Filtration: separate solid from liquid
Distillation: boil liquid, condense to liquid with removed impurities

7. Distinguishing Elements
Atomic Number- # p+
Mass Number- #p+ and neutrons
# neutrons= mass # - atomic #
Isotopes- diff # neutrons (diff mass #’s!!)
Atomic Mass Unit (amu)-1/12 of mass of 1 carbon-12 atom
Atomic Mass- weighted avg atomic mass naturally occurring
Periodic Table
Period: rows, pattern of properties as move across
Group: columns, have similar chem/phys properties (family)

8. Metals/ nonmetals/ metalloids:
*Metal:80% elements are metals; properties include good conductors, reflect light because of high luster/ sheen, ductile (make wires), malleable (hammer into shape)
*Nonmetal: properties opposite of metals; poor conductors of heat/ electric currents
*Metalloids: has properties of both based on conditions element is under