2. chemistry
matter
Scientific Method
Technology
Observation
Theory
Experiment
Applied Chemistry

3. 1. Inorganic Chemistry
Inorganic is the study of matter that does NOT contain ________
Inorganic chemists study the structure, function, synthesis, and identity of non-carbon compounds
Polymers, Metallurgy
Carbon

4. 2. Organic Chemistry
Organic is the study of matter that contains ______
Organic chemists study the structure, function, synthesis, and identity of carbon compounds
Useful in petroleum industry, pharmaceuticals, polymers
carbon

5. 3. Physical Chemistry
Physical chemistry is the physics of chemistry… the forces of matter
Rates and energy transfers
Much of p-chem is computational

6. 4. Analytical Chemistry
Analytical chemistry is the study of high precision measurement
Find composition and identity of chemicals
Lead in drinking H2O
Forensics, quality control, medical tests

7. 5. Biochemistry
Biochemistry is the study of chemistry in ______ things
Cross between biology and chemistry
Pharmaceuticals and genetics
living

8. Properties of Matter Extensive properties
depend on the amount of matter that is present.
Extensive properties
Volume
Mass
Energy Content (think Calories!)
do not depend on the amount of matter present, but type of matter.
Intensive properties
Melting point, Boiling point
Color
Density
Hardness

9. Law of conservation of mass
In all physical and chemical changes, the mass of the reactants MUST equal the mass of the products.

10. Scientific Method State the problem clearly./Make Observ.
Formulate a hypothesis
Test the hypothesis.
Evaluate the data to form a conclusion.
If the conclusion is valid, then it becomes a theory. If the theory is found to be true over along period of time (usually 20+ years) with no counter examples, it may be considered a law.
5. Share the results.

11. Chapter 2

12. water, ammonia, sucrose, gold, oxygen
Chemistry is the study of matter and the
changes it undergoes
Matter is anything that occupies space and has mass. “stuff”
A substance is a form of matter that has a definite composition and distinct properties.
water, ammonia, sucrose, gold, oxygen

13. Phase Differences
Solid – definite volume and shape; particles packed in fixed positions.
Liquid – definite volume but indefinite shape; particles close together but not in fixed positions
Gas – neither definite volume nor definite shape; particles are at great distances from one another
Plasma – high temperature, ionized phase of matter as found on the sun.

14. Physical Properties What are some physical properties? color
melting and boiling point
odor
Create a definition for “physical properties”

15. Physical Changes boiling of a liquid melting of a solid
can be observed without changing the identity of the substance
Physical change Ex.
boiling of a liquid
melting of a solid
dissolving a solid in a liquid to give a homogeneous mixture
— a SOLUTION.

16. soft drink, milk, salt water
A mixture is a combination of two or more substances in which the substances retain their distinct identities.
Homogenous mixture – composition of the mixture is the same throughout.
soft drink, milk, salt water
Heterogeneous mixture – composition is not uniform throughout.
Rocky Road Ice Cream, soil, pizza chicken noodle soup

17. Types of Mixtures Heterogeneous – visibly separate phases
Homogeneous – Same throughout

18. Physical means can be used to separate a mixture into its pure components.
distillation
magnet
Filtration

19. Separation of a Mixture
Distillation

20. Separation of a Mixture
The components of dyes such as ink may be separated by paper chromatography.

21. An element is a substance that cannot be separated into simpler substances by chemical means.
“116” elements have been identified
82 elements occur naturally on Earth
gold, aluminum, lead, oxygen, carbon
34 elements have been created by scientists
technetium, americium, seaborgium

22. A compound is a substance composed of atoms of two or more elements chemically united in fixed proportions.
Compounds can only be separated into their pure components (elements) by chemical means.
Water (H2O)
Glucose (C6H12O6)
Ammonia (NH3)

23. Separation of a Compound The Electrolysis of water
Compounds must be separated by chemical means.
With the application of electricity, water can be separated into its elements
Reactant  Products
Water  Hydrogen + Oxygen
H2O  H O2

24. Can it be physically separated?
Matter Flowchart Fill in the flow chart AND provide and example for each box.
Matter
yes no
Can it be physically separated?
Mixture
Pure substance
Is the composition uniform? no
yes
Can it be chemically decomposed? no
yes
Homogenous
Heterogenous
Compound
Element

25. Organization of Matter a) Homogeneous (Solutions)
Mixtures:
a) Homogeneous (Solutions)
b) Heterogeneous
Pure Substances
Elements
Compounds
Atoms
Nucleus
Electrons
Protons
Neutrons
Quarks
Quarks

26. Physical vs. Chemical Properties
Examples:
melting point
flammable
density
magnetic
tarnishes in air

27. Physical vs. Chemical Changes
Examples:
rusting iron
dissolving in water
burning a log
melting ice
grinding spices
Chemical
Physical

28. Sure Signs of a Chemical Change
Change in Temp
Light
Gas Produced (not from boiling!)
Precipitate – a solid formed by mixing two liquids together
Color Change???

29. Chemical Properties and Chemical Change
Chemical Property - Ability of a substance to undergo a chemical change
Examples:
Chemical Change – Change that produces matter with a different composition than the original matter.

30. Pure Chemistry – pursuit of chemical knowledge for its own sake.
Use it or not?
Pure Chemistry – pursuit of chemical knowledge for its own sake.
Applied Chemistry – research that is directed toward a practical goal or application.