Chapter 1 Chemistry Is a Physical Science Honors Chemistry, Chapter 1 Page 1

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 Honors Chemistry, Chapter 1 Page 2

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 Honors Chemistry, Chapter 1 Page 3

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 Honors Chemistry, Chapter 1 Page 4

Branches of Chemistry Many major areas of study for specialization Several career opportunities Also used in many other jobs

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

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

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

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

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

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

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? Honors Chemistry, Chapter 1 Page 12

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 Honors Chemistry, Chapter 1 Page 13

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. Honors Chemistry, Chapter 1 Page 14

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 Honors Chemistry, Chapter 1 Page 15

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")!

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

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.

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

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

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

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.

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

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

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 Honors Chemistry, Chapter 1 Page 25

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 Honors Chemistry, Chapter 1 Page 26

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 Honors Chemistry, Chapter 1 Page 27

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

Graphite — layer structure of carbon atoms reflects physical properties.

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.

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. Honors Chemistry, Chapter 1 Page 31

Chemical Change In a Chemical Change the Identities of Substances Change and New Substances Form Example: Mercury(II)Oxide  Mercury + Oxygen or 2 HgO  2 Hg + O2 Starting Materials = Reactants (Left Hand) Final Materials = Products (Right Hand) Honors Chemistry, Chapter 1 Page 32

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 Honors Chemistry, Chapter 1 Page 33

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%) Honors Chemistry, Chapter 1 Page 34

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 Honors Chemistry, Chapter 1 Page 35

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) Honors Chemistry, Chapter 1 Page 36

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 Honors Chemistry, Chapter 1 Page 37

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 Honors Chemistry, Chapter 1 Page 38

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. Honors Chemistry, Chapter 1 Page 39

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

The Periodic Table Dmitri Mendeleev (1834 - 1907)

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

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 Honors Chemistry, Chapter 1 Page 43

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) Honors Chemistry, Chapter 1 Page 44

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.) Honors Chemistry, Chapter 1 Page 45

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 Honors Chemistry, Chapter 1 Page 46

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) Honors Chemistry, Chapter 1 Page 47

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. Honors Chemistry, Chapter 1 Page 48