1. Chapter 1 Chemistry Is a Physical Science
Honors Chemistry, Chapter 1
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2. Chemistry
The Study of The Composition, Structure, and Properties of Matter and the Changes it Undergoes.
Branches
Organic Chemistry – Study of Carbon Containing Compounds
Inorganic Chemistry – Study of All Substances Not Classified As Organic
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3. Chemistry Branches (Continued):
Physical Chemistry – The Study of the Properties and Changes of Matter and Their Relation to Energy
Analytical Chemistry – Identification of the Components and Composition of Materials
Biochemistry – The Study of Substances and Processes Occurring in Living Things
Theoretical Chemistry – The Use of Mathematics to Understand the Principles behind Observed Chemical Behavior
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4. Types of Chemical Research
Basic Research – A Fundamental Study of How and Why a Specific Reaction Occurs and What The Properties of a Substance Are.
Applied Research – Applied Research is Carried out to solve a Problem.
Technological Development – Uses Basic and Applied Research Results to Develop New Products
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5. Branches of Chemistry Many major areas of study for specialization
Several career opportunities
Also used in many other jobs

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

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

8. 3. Biochemistry
Biochemistry is the study of chemistry in living things
Cross between biology and chemistry
Pharmaceuticals and genetics

9. 4. Physical Chemistry
HONK if you passed p-chem
Physical chemistry is the physics of chemistry… the forces of matter
Much of p-chem is computational
Develop theoretical ideas for new compounds

10. 5. Analytical Chemistry
Analytical chemistry is the study of high precision measurement
Find composition and identity of chemicals
Forensics, quality control, medical tests

11. Types of Observations and Measurements
We make QUALITATIVE observations of reactions — changes in color and physical state.
We also make QUANTITATIVE MEASUREMENTS, which involve numbers.
Use SI units — based on the metric system

12. Chapter 1, Section 1 Review
What is chemistry?
Give examples of branches of chemistry.
How are basic research, applied research, and technology the same.
How are they different?
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13. Matter and Its Properties
Mass is the Quantity of Matter
Unit of Measure = gram
Not Weight (Weight = Acceleration x Mass)
Volume is the Space an Object Occupies
Calculated by V = H x W x D
Unit of Measure = cm3
Matter is Anything Which Has Mass and Volume
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14. Basic Building Blocks of Matter
Atom – The Smallest Unit of an Element That Maintains the Properties of the Element.
Element – A Pure Substance Made up of Only One Kind of Atom.
Compound – A Substance That is Made From Atoms of Two or More Elements That are Chemically Bonded.
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15. Properties of Matter
Extensive Properties – Depend Upon the Amount of Matter
Mass
Volume
Energy
Intensive Properties – Do Not Depend Upon the Amount of Matter
Melting Point
Boiling Point
Density
Conductivity
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16. Matter And Energy
SAVE PAPER AND INK!!! When you print out the notes on PowerPoint, print "Handouts" instead of "Slides" in the print setup. Also, turn off the backgrounds (Tools>Options>Print>UNcheck "Background Printing")!

17. The Nature of Matter Gold Mercury
Chemists are interested in the nature of matter and how this is related to its atoms and molecules.

18. Chemistry & Matter
We can explore the MACROSCOPIC world — what we can see —
to understand the PARTICULATE worlds we cannot see.
We write SYMBOLS to describe these worlds.

19. A Chemist’s View of Water
Macroscopic
H2O
(gas, liquid, solid)
Symbolic
Particulate

20. A Chemist’s View Macroscopic 2 H2(g) + O2 (g) --> 2 H2O(g)
Particulate
Symbolic

21. Kinetic Nature of Matter
Matter consists of atoms and molecules in _____.

22. STATES OF MATTER
_______ — have rigid shape, fixed volume. External shape can reflect the atomic and molecular arrangement.
Reasonably well understood.
_______ — have no fixed shape and may not fill a container completely.
Not well understood.
_______ — expand to fill their container.
Good theoretical understanding.

23. OTHER STATES OF MATTER
PLASMA — an electrically charged gas; Example: the sun or any other star
BOSE-EINSTEIN CONDENSATE — a condensate that forms near absolute zero that has superconductive properties; Example: supercooled Rb gas

24. Physical Properties What are some physical properties? color
melting and boiling point
odor

25. Physical Properties and Physical Changes
Physical Property – A Characteristic That Can be Observed or Measured Without Changing the Identity of the Substance.
Examples:
Melting Point
Boiling Point
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26. Physical Change
Physical Change - A Change in a Substance That Does Not Involve a Change in the Identity of the Substance.
Examples:
Change of State (Gas to Liquid, etc.)
Change in Temperature/Energy
Change in Pressure
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27. Physical States of Matter
Solids
Definite Volume and Shape
Molecules Rigidly Locked Together
Liquids
Definite Volume, Take the Shape of the Container (Indefinite Shape)
Molecules Closely Packed But Move Past Each Other
Gas
Neither a Fixed Volume Nor a Fixed Shape
Molecules Widely Spaced
Plasma
High Energy State of Matter
Electrons and Nuclei Separated
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28. Physical Properties What are some physical properties? color
melting and boiling point
odor

29. Graphite — layer structure of carbon atoms reflects physical properties.

30. Physical Changes Some physical changes would be boiling of a liquid
can be observed without changing the identity of the substance
Some physical changes would be
boiling of a liquid
melting of a solid
dissolving a solid in a liquid to give a homogeneous mixture — a SOLUTION.

31. Chemical Property
A chemical property relates to a substance’s ability to undergo changes that transform it into different substances.
Examples:
Ability of charcoal (carbon) to burn.
Ability of iron to rust when contacted with water.
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32. Chemical Change
In a Chemical Change the Identities of Substances Change and New Substances Form
Example: Mercury(II)Oxide  Mercury + Oxygen or HgO  2 Hg + O2
Starting Materials = Reactants (Left Hand)
Final Materials = Products (Right Hand)
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33. Energy and Changes in Matter
Energy is Always Involved in Chemical And Physical Changes
Examples:
Heat Required to Melt Ice
Heat Evolved When Charcoal Burns
Heat Absorbed When Chemicals in a “Cold Pack” Are Mixed
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34. Classification of Matter
Two Groups: Mixtures and Pure Substances
Mixture – A Blend of Two or More Kinds of Matter, Each of Which Retains Its Own Identity and Properties
Mixture Examples:
Sand and Iron Filings
Sugar in Water
18-karat Gold (Alloy of Gold, Silver, Copper, and Nickel) (18-karat/24-karat = 75%)
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35. Types of Mixtures
Homogeneous Mixtures – Mixtures Uniform in Composition, Also Called Solutions
Clear Washing Detergent
Sprite
Heterogeneous Mixtures – Mixtures Which are Not Uniform Throughout
Orange Juice (With Pulp)
Fur Lined Jacket
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36. Separation of Mixtures
Filtration (Separation of Precipitate from Supernate)
Centrifugation (Separation of High Density Materials from Low Density Materials)
Chromatography
Gas Phase (Like Distillation)
Liquid Phase (Different Diffusion Rates)
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37. Pure Substance
Every Sample of a Pure Substance Has Exactly the Same Characteristic Properties
Every Sample of a Pure Substance Has Exactly the Same Composition
Examples:
A Clear Liquid Which Freezes at 0 C. and Boils at 100 C. Is Probably Water
All Water Molecules are Composed of Two Parts Hydrogen and One Part Oxygen
A Metal Which Melts at 1083 C. Is Probably Copper
May Be Either a Compound or an Element
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38. Purity of Laboratory Chemicals
All Chemicals Have Some Impurities
Primary Standard
ACS Grade
USP Grade
CP Grade Increasing Purity
NF Grade
FCC Grade
Technical Grade
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39. Chapter 1, Section 2 Review
What is the difference between a physical property and a chemical property?
How does a physical change differ from a chemical change?
Explain gas, liquid, and solid states in terms of particles.
Distinguish between a mixture and a pure substance.
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40. The Language of Chemistry
The elements, their names, and symbols are given on the PERIODIC TABLE
How many elements are there?
117 elements have been identified
82 elements occur naturally on Earth
Examples: gold, aluminum, lead, oxygen, carbon
35 elements have been created by scientists
Examples: technetium, americium, seaborgium

41. The Periodic Table
Dmitri Mendeleev ( )

42. Glenn Seaborg (1912-1999) Discovered 8 new elements.
Only living person for whom an element was named.

43. Elements Periodic Table Vertical Columns Horizontal Rows
Groups or Families
Similar Ability to Bond to Other Elements
Horizontal Rows
Called Periods
Two Main Sections
Metal on Left
Non-Metals on Right
Metalloids In between
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44. Metals
Definition: A Metal Is an Element That Is a Good Conductor of Heat and Electricity
Characteristics
Malleable
Ductile
High Tensile Strength
Shiny
Silver Appearance (Except for Copper, Gold)
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45. Non-Metals
A Non-Metal Is an Element That Is a Poor Conductor of Heat And Electricity
Tend to Be Brittle Rather Than Malleable or Ductile
Examples:
Phosphorous (Necessary for Life)
Sulfur
Carbon
Oxygen
Halogens (Fluorine, Chlorine, etc.)
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46. Metalloids Metalloids Have Properties of Both Metals and Non-Metals
Tend to Be Less Malleable Than Metals And Not as Brittle as Non-Metals
Tend to Be Semiconductors of Electricity
Examples:
Silicon
Germanium
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47. Noble Gases
Elements in Group 18 (Far Right-hand Column) Are The Noble Gases
Very Low Reactivity (No Compounds Known Before 1962 When Xenon Hexafluoride Discovered)
Examples:
Helium (Lighter Than Air Balloons)
Neon (Neon Signs)
Argon (About 1% of the Air We Breathe)
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48. Chapter 1, Section 3 Review
Illustrate the use of a Periodic Table to give element names and symbols.
Given the name of an specific element, give the symbol for that element.
How is the Periodic Table arranged?
What are the characteristics of metals, non-metals, and metalloids.
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