Honors Chemistry, Chapter 1

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Chapter 1Chemistry Is a Physical Science
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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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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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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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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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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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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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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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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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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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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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Chemical Property

• A chemical property relates to a substances
  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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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)

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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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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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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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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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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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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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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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Elements

• Periodic Table
• Vertical Columns
• 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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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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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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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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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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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.