Chapter 1

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Chapter 1 Matter and Change

• Taken from Modern Chemistry written by Davis,
  Metcalfe, Williams Castka

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Chemistry is a Physical Science
Section 1 - Objectives

• Define chemistry
• List examples of the branches of chemistry
• Compare and Contrast
• Basic research
• Applied research
• Technological development

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Section 1-1

• Chemistry is the study of the composition,
  structure, and properties of matter and the
  changes it undergoes.
• What is it made of?
• Makeup and internal arrangement?
• What happens when we
• heat?
• cool?
• Mix with other materials?
• Why does this behavior occur?

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Section 1-1 (continued)

• Six main Branches of Chemistry
• Organic deals with carbon containing compounds
• Inorganic study of substances not classified as
  organic, mainly those that dont contain carbon
• Physical study of properties, changes and
  relationship between energy and matter
• Analytical identification of components and
  composition of materials
• Biochemistry study of substances and processes
  occurring in living things
• Theoretical using math and computers to design
  and predict the properties of new compounds

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Section 1-1 (continued)

• A Chemical is any substance that has a definite
  composition.

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Section 1-1 (continued)
The 3 often overlap understanding of crystals
and basic light allowed lazers to be created
which lead to fiber optics
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Matter and Its Properties
Section 2 - Objectives

• Distinguish between the physical properties and
  chemical properties of matter.
• Classify changes of matter as physical or
  chemical.
• Explain the . . . states in terms of particles
• Gas
• Liquid
• Solid
• Distinguish between a mixture and a pure substance

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Section 1-2

• M M
• Mass is a measure of the amount of matter.
• Measured in Kg, g and for the
• less educated ?in lbs and ozs.
• So . . .Matter is anything that has mass and
  takes up space.

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Section 1-2 (continued)
Basic Building Blocks of Matter

• An Atom is the smallest unit of an element that
  maintains the properties of that element.
• and . . .an element is a pure substance made of
  one only kind of atom.
• and . . .a compound is a substance that is made
  from the atoms of two or more elements that are
  chemically bonded.

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Section 1-2 (continued)
Basic Building Blocks of Matter (continued)

• An molecule is the smallest unit of an element or
  compound that retains the properties of that
  element or compound .

EXAMPLES
O2
H2O
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Section 1-2 (continued)
Properties and Changes in Matter

• Extensive properties depend on the amount of
  matter present
• Volume
• Mass
• Amount of Energy

• Intensive properties do not depend on the amount
  of matter present
• Melting pt.
• Boiling pt.
• Density
• Ability to conduct
• Heat
• Electricity

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Section 1-2 (continued)
Physical Properties and Physical Changes

• Physical property is a characteristic that can be
  observed without changing the identity of the
  substance
• Melting pt.
• Boiling pt.

• A change in a substance that does not involve a
  change in the identity of the substance is called
  a physical change
• Grinding
• Cutting
• Melting Boiling

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Section 1-2 (continued)
Physical Properties and Physical Changes
(continued)

• Change of state is a physical change of a
  substance from one state to another.

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Section 1-2 (continued)
Chemical Properties and Chemical Changes

• A Chemical property relates to a substances
  ability to undergo changes that transform it into
  different substances.
• Ability to burn in air
• Iron rusting by combining with the oxygen in air

• A change in which one or more substances are
  converted into different substances is called a
  chemical change.

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Section 1-2 (continued)
Chemical Properties and Chemical Changes
(continued)
The substances that react in a chemical change
are called the reactants.
The substances that are formed in a chemical
change are called the products.

• Carbon plus oxygen yields (or forms)
  carbon-dioxide

• Carbon oxygen ? carbon-dioxide

• C O2 ? CO2

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Section 1-2 (continued)
Chemical Properties and Chemical Changes
(continued)
Chemical changes and reactions, such as
combustion and decomposition, form products whose
properties differ greatly from those of the
reactants.

• However, chemical changes do not affect the total
  amount of matter present before and after a
  reaction. The amount of matter, and therefore the
  total mass, remains the same.

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Section 1-2 (continued)
Energy and Changes in Matter

• When physical or chemical changes occur, energy
  is almost always involved.
• The energy can take several different forms, such
  as heat or light.
• Although energy can be absorbed or released in a
  change, it is not created or destroyed. It simply
  assumes a different form.

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Section 1-2 (continued)
Classification of Matter - Mixture
A mixture is a blend of two or more kinds of
matter, each of which retains its own identity
and properties.

• A mixture that is uniform in composition they
  are said to be homogeneous
• Examples
• salt-water solutions

• A mixture that is not uniform in composition is
  said to be heterogeneous
• Examples
• clay water

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Section 1-2 (continued)
Classification of Matter Pure substances
A pure substance has a fixed composition and
differ from a mixture in the following ways

• Every sample of a pure substance has exactly the
  same characteristic properties.
• Every sample of a given pure substance has
  exactly the same composition.

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Section 1-2 (continued)
Classification of Matter Laboratory Chemicals
and Purity
Chemicals in laboratories are generally treated
as if they are pure. However all chemicals have
some impurities.

• Purity ranking depends on the needs of the users.

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Elements
Section 3 - Objectives

• Use a periodic table to name elements, given
  their symbols.
• Use a periodic table to write the symbols of
  elements given their names.
• Describe the arrangement of the periodic table.
• List the characteristics that distinguish metals,
  nonmetals, and metaloids.

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Section 1-3
Introduction to the Periodic Table

• The vertical columns of the periodic table are
  called groups.
• The horizontal rows of elements in the periodic
  table are called periods.

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Section 1-3 (continued)
Oxygen
Carbon
Hydrogen
Nitrogen
Calcium
Phosphorus
Potassium
Sulfur
Chlorine
Sodium
Magnesium
Iron
Cobalt
Copper
Zinc
Iodine
Selenium
Introduction to the Periodic Table (continued)
Seventeen most common elements in the Human Body
Ten most common elements in the Milky Way Galaxy
Hydrogen
Helium
Oxygen
Carbon
Neon
Iron
Nitrogen
Silicon
Magnesium
Sulfur
Ten most common elements in the Earths Crust
Oxygen
Silicon
Aluminum
Iron
Calcium
Sodium
Magnesium
Potassium
Titanium
Hydrogen
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Section 1-3
The periodic table is divided into two main
groups metals and non-metals. Metals to the
left and non-metals to the right.

Types of Elements - Metals

• An element that is a good conductor of heat and
  electricity is a metal.
• Most metals are malleable they can be hammered
  or rolled into thin sheets
• They are also ductile which means they can be
  drawn in to fine wire. Metals that behave this
  way have a high tensile strength.

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Section 1-3

Types of Elements - Nonmetals

• A nonmetal is an element that is a poor conductor
  of heat and electricity.
• Many nonmetals are gas at room temperature ,
  when solid they tend to be brittle.

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Section 1-3
Types of Elements - metalloids

• A metalloid is an element that has some
  characteristics of metals and some
  characteristics of nonmetals.
• Metalloids tend to be semiconductors.

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Section 1-3
Types of Elements Noble Gases

• The elements in group 18 of the periodic table
  are generally unreactive.

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Chapter Summary Questions

• HW page 26
• 1 ,5-13 ,17 ,19 , 20 23

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Chapter Summary Questions

• 1 - Chemistry is the study of the compostion,
  structure and properties of substances and the
  changes they under go

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• A measure of the amount of matter
• the amount of space occupied by matter

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• The portions of elements in a pure substance are
  fixed.

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1. A property is any characteristic of a substance
   or material.
2. Properties can be compared in order to classify
   unknown materials as members of known groups or
   subgroups of substances, or to identify
   substances directly.

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8

• Extensive properties depend on the amount of
  matter that is present. Intensive properties do
  not.

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1. a characteristic that can be observed or measured
   without changing the identity of the substance.
2. Examples include color, odor, length, size ,
   melting point boiling point.

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1. a property that describes the ability of a
   substance to undergo changes that alter its
   identity.
2. Examples include the ability of coal to burn and
   the ability of iron (Fe) to rust.

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• A physical change is a change in a substance that
  does not involve a change in its identity. A
  chemical change is a change in which a substance
  is converted into other substances.

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1. solids, liquids gases
2. A solid has a definite shape and fixed volume ,
   whereas a liquid has a fixed volume but takes the
   shape of the vessel it is in.
3. A gas has neither fixed volume or definite shape.
4. Liquids and gases take the shape of the container
   they are in.

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• A change of a substance from one state of matter
  to another.

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• The reactants are potassium (K) and water (H2O)
  and the products are potassium hydroxide (KOH)
  and hydrogen (H2)

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1. physical , wood still wood
2. chemical , composition change think taste
3. physical, butter still butter

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• potassium (K) ? metal
• Silver (Ag) ? metal
• Silicon (Si) ? metalloid
• sodium (Na) ? metal
• Mercury (Hg) ? metal
• helium (He) ? noble gas

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• Group 14, period 2
• Group 18, period 3
• Group 6, period 4
• Group 2, period 6
• Group 17, period 5
• Group 11, period 6