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MatterProperties and Change
Section 3.1 Properties of Matter Section 3.2
Changes in Matter Section 3.3 Mixtures of
Matter Section 3.4 Elements and Compounds
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Section 3-1
Section 3.1 Properties of Matter

• Identify the characteristics of a substance.

• Distinguish between physical and chemical
  properties.
• Differentiate among the physical states of matter.

density a ratio that compares the mass of an
object to its volume
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Section 3-1
Section 3.1 Properties of Matter (cont.)
states of matter solid liquid gas Vapor Plasma
physical property extensive property intensive
property chemical property
Most common substances exist as solids, liquids,
and gases, which have diverse physical and
chemical properties.
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Section 3-1
Substances

• Matter is anything that has mass and takes up
  space.

• Matter is everything around us.
• Matter with a uniform and unchanging composition
  is a pure substance.
• Particles of matter are always in motion.
• The kinetic energy (speed) of these particles
  increases as temperature increases.

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Section 3-1
States of Matter

• The physical forms of matter, either solid,
  liquid, or gas, are called the states of matter.

• Solids are a form of matter that have their own
  definite shape and volume. Very Low Kinetic
  Energy

• Liquids are a form of matter that have a definite
  volume but take the shape of the container. Low
  Kinetic Energy

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Section 3-1
States of Matter (cont.)

• Gases have no definite shape or volume. They
  expand to fill their container. Very High
  Kinetic Energy

• Vapor refers to the gaseous state of a substance
  that is normally a solid or liquid at room
  temperature.
• Plasma very high kinetic energy- particles
  collide with enough energy to break into charged
  particles (/-).
• gas-like, variable shape volume

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Section 3-1
Physical Properties of Matter

• A physical property is a characteristic that can
  be observed or measured without changing the
  samples composition.

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Section 3-1
Physical Properties of Matter (cont.)

• Extensive properties are dependent on the amount
  of substance present, such as

• Intensive properties are independent of the
  amount of substance present, such as

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A. Extensive vs. Intensive
Extensive vs. Intensive

• intensive
• extensive
• extensive
• intensive
• intensive

• Examples
• boiling point
• volume
• mass
• density
• conductivity

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Section 3-1
Chemical Properties of Matter

• The ability of a substance to combine with or
  change into one or more other substances is
  called a chemical property.
• describes the ability of a substance to undergo
  changes in identity

• Examples

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Section 3-1
Observing Properties of Matter

• A substance can change

• Chemical properties can change with specific
  environmental conditions, such as temperature and
  pressure.

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B. Physical vs. Chemical
Physical vs. Chemical

• physical
• chemical
• physical
• physical
• chemical

• Examples
• melting point
• flammable
• density
• magnetic
• tarnishes in air

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Section 3-2
Section 3.2 Changes in Matter

• Define physical change and list several common
  physical changes.

• Define chemical change and list several
  indications that a chemical change has taken
  place.
• Apply the law of conservation of mass to chemical
  reactions.

observation orderly, direct information
gathering about a phenomenon
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Section 3-2
Section 3.2 Changes in Matter (cont.)
physical change phase change chemical change law
of conservation of mass
Matter can undergo physical and chemical changes.
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Section 3-2
Physical Changes

• A change that alters a substance without changing
  its composition is known as a physical change.

• A phase change is a transition of matter from one
  state to another.
• Examples

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• SOLID ? LIQUID Melting
• LIQUID ? GAS Boiling or Evaporation
• GAS ? LIQUID Condensing
• SOLID ? GAS Sublimation
• GAS ? SOLID Reverse Sublimation or
  Deposition
• LIQUID ? SOLID Freezing, Solidifying or
  Crystallizing

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Section 3-2
Chemical Changes

• A change that involves one or more substances
  turning into new substances is called a chemical
  change.
• changes the identity of a substance
• products have different properties

• Examples

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B. Physical vs. Chemical

• Signs of a Chemical Change
• change in color or odor
• formation of a gas
• formation of a precipitate (solid)
• change in light or heat
• http//www.youtube.com/watch?vQL7V3L3dfDM

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B. Physical vs. Chemical
Physical vs. Chemical

• chemical
• physical
• chemical
• physical
• physical

• Examples
• rusting iron
• dissolving in water
• burning a log
• melting ice
• grinding spices

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B. Physical vs. Chemical

• Reaction occurs when one or more substances are
  changed into new substances.
• Reactants- stuff you start with elements or
  compounds
• Products- What you make
• products have NEW PROPERTIES
• Yields Arrow separates reactants and products

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Section 3-2
Conservation of Mass

• The law of conservation of mass states that mass
  is neither created nor destroyed in a chemical
  reaction, it is conserved.

• The mass of the reactants equals the mass of the
  products.
• massreactants massproducts

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Section 3-3
Section 3.3 Mixtures of Matter

• Contrast mixtures and substances.

• Classify mixtures as homogeneous or
  heterogeneous.
• List and describe several techniques used to
  separate mixtures.

substance a form of matter that has a uniform
and unchanging composition also known as a pure
substance
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YES NO WHY?

• All mixtures can be separated though some type of
  physical process.
• Yes, I agree with this statement because
• No, I disagree with this statement because

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Section 3-3
Mixtures

• A mixture is a physical combination of two or
  more pure substances in which each pure substance
  retains its individual chemical properties.

• A homogenous mixture is a mixture where the
  composition is constant throughout.

Homogeneous mixtures are also called
solutions. Examples
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C. Mixtures

• Solution
• homogeneous
• very small particles
• no Tyndall effect

• particles dont settle
• EX rubbing alcohol

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Section 3-3
Mixtures (cont.)
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Section 3-3
Mixtures (cont.)

• A heterogeneous mixture is a mixture where the
  individual substances remain distinct.
• mixture is not uniform in composition
• Examples

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C. Mixtures

• Colloid
• heterogeneous
• medium-sized particles
• Tyndall effect
• particles dont settle
• EX milk

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C. Mixtures

• Suspension
• heterogeneous
• large particles
• Tyndall effect
• particles settle
• EX fresh-squeezed lemonade

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C. Mixtures

• colloid
• suspension
• colloid
• solution
• suspension

• Examples
• mayonnaise
• muddy water
• fog
• saltwater
• Italian salad dressing

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Section 3-3
Separating Mixtures

• Filtration is a technique that uses a porous
  barrier to separate a solid from a liquid in a
  heterogeneous mixture.

• Distillation is a separation technique for
  homogeneous mixtures that is based on the
  differences in boiling points of substances.
• Crystallization is a separation technique for
  homogenous mixtures that results in the formation
  of pure solid particles from a solution
  containing the dissolved substance.

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Section 3-3
Separating Mixtures (cont.)

• Sublimation is the process of a solid changing
  directly to a gas, which can be used to separate
  mixtures of solids when one sublimates and the
  other does not.

• Chromatography is a technique that separates the
  components of a mixture on the basis of tendency
  of each to travel across the surface of another
  material.

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Section 3-4
Section 3.4 Elements and Compounds

• Distinguish between elements and compounds.

• Describe the organization of elements in the
  periodic table.
• Explain how all compounds obey the laws of
  definite and multiple proportions.

proportion the relation of one part to another
or to the whole with respect to quantity
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Section 3-4
Elements

• An element is a pure substance that cannot be
  separated into simpler substances by physical or
  chemical means.

• 92 elements occur naturally on Earth.
• Each element has a unique name and a one, two, or
  three-letter symbol.
• The periodic table organizes the elements into a
  grid of horizontal rows called periods and
  vertical columns called groups.

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Section 3-4
Compounds

• A compound is a made up of two or more elements
  combined chemically.

• Most of the matter in the universe exists as
  compounds.
• Table salt, NaCl, and water, H2O, are compounds.

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Section 3-4
Compounds (cont.)

• Elements can never be separated.

• Compounds can be broken into components by
  chemical means.

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A. Matter Flowchart
MATTER
no
Can it be physically separated?
yes
Compound
Element
Homogeneous Mixture (solution)
Heterogeneous Mixture
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Section 3-4
Law of Definite Proportions

• The law of definite proportions states that a
  compound is always composed of the same elements
  in the same proportion by mass, no matter how
  large or small the sample.

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Section 3-4
Law of Definite Proportions (cont.)

• The relative amounts are expressed as percent by
  mass, the ratio of the mass of each element to
  the total mass of the compound expressed as a
  percentage.

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Section 3-4
Law of Definite Proportions (cont.)

• This table demonstrates that the percentages of
  elements in sucrose remain the same despite
  differences in sample amount.

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Section 3-4
Law of Multiple Proportions

• The law of multiple proportions states that when
  different compounds are formed by a combination
  of the same elements, different masses of one
  element combine with the same relative mass of
  the other element in whole number ratios.

• H2O2 and H2O
• Copper(I) chloride and copper(II) chloride

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Section 3-4
Law of Multiple Proportions (cont.)