MATTER

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MATTER

• What it is all about

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Chemistry Matter Unit

• What is matter?
• What is the organization of matter?
• What is the nature of matter?

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MATTER
Can the matter be separated by physical means?
Pure Substances
Constant composition
Separation by chemical means
Heterogeneous
Compounds
Elements
Homogeneous
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Matter

• Matter is anything that occupies space and
  has mass.
• The particle theory of matter.
• The particle theory states that
• all matter is made from particles
• different particles have different properties
• particles are constantly in motion

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States of Matter A solid has a definite shape
and volume. A liquid has a definite volume but no
definite shape. A gas has neither a definite
volume or shape.
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• SOLIDS
• the attraction between particles is strong so
  the matter holds its shape. The particles are
  still moving, but they are not able to slide past
  each other

• LIQUIDS
• the attractive forces are not as strong. The
  particles are able to move past each other and
  slide around

• GAS
• the attraction between particles is so weak that
  they fly in every direction filling the container
  that they are held

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Phases Changes of Matter
sublimation
vaporization
sublimation
condensation
Phase changes
solidification (freezing)
melting
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Properties of Matter

• Physical Properties
• a quality of a substance that can be observed
  or measured without changing the substances
  chemical composition
• Examples color, texture, boiling point,
  density, mass etc

• Chemical properties
• Properties that do change the chemical nature
  of matter
• Properties the matter exhibits when chemical
  change occurs
• Ex. oxidation, flammability, corrosiveness, pH,
  reactivity

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Physical Properties Subcategories

• Extensive Properties depend upon the amount of
  matter that is present.
• Ex. Length, mass, volume, heat etc
• Intensive Properties do not depend on the amount
  of matter present. These properties are the same
  for a given substance regardless of how much of
  the substance is present.
• Ex. Color, density, melting point, ductility,
  temp etc

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Examples of physical properties

• Boiling point
• Specific gravity (at constant temperature)
• Surface tension
• Viscosity (at constant pressure and temp.)
• Freezing point
• Solubility in water (hot/cold)
• Density
• Melting point
• Mass
• Volume
• Specific heat capacity
• Heat
• Temperature

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Density

• the mass of a substance per a specific amount of
  volume
• Density mass
• volume
• The mass and volume are directly proportional. If
  one increases the other increases

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Physical and chemical change

• Physical change
• the altering of the physical form but not
  composition of matter
• ex. Pounding, pulling, changes of state

• Knowledge of physical change leads to
• the understanding of separation of mixtures
• ex. Distillation, crystallization,
  chromatography, filtration

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Chemical change

• Chemical change
• change in which the matter is converted into
  matter with different composition and properties

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Indicators of chemical change

• heat and/or light energy
• Energy changes within the system

• Production of gas
• - release of gas from the system

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3. Formation of a precipitate - when two (or
more) solutions are put together an insoluble
solid is produced
4. Color change - the system changes color -
not always an indicator of chemical change (can
be physical
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MATTER
Can the matter be separated by physical means?
Pure Substances
Constant composition
Separation by chemical means
Heterogeneous
Compounds
Elements
Homogeneous
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MIXTURES

• mixture
• - combination of two or more kinds of matter
  each of which retains its own composition and
  properties
• - physical blend of two or more substances

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More of Mixtures
heterogeneous mixture - a mixture containing
substances that are not evenly distributed -
different from point to point ex. granite ---gt
quartz, feldspar, and mica

• Phase
• mixtures that are obviously heterogeneous and
  have separate, distinct parts
• Ex. Oil forming layers in water is another
• Interface the region where two or more phases
  meet

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M o M

• homogeneous mixture
• - a mixture containing substances that are
  uniformly distributed with the particles blended
  completely
• - composition and properties are uniform
  throughout
• - also called solutions (mixed on a scale of
  individual particles) ex. I molar copper II
  sulfate
• To the eye, the mixture appears to be pure
  substance.

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Solutions(Homogeneous Mixtures)

• Can you tell the difference?

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Parts of a Solution

• SOLUTE the part of a solution that is being
  dissolved (usually the lesser amount)
• SOLVENT the part of a solution that dissolves
  the solute (usually the greater amount)
• Solute Solvent Solution

Solute Solvent Example
solid solid Brass Copper and Zinc
solid liquid Seawater NaCL in water
gas solid Moth balls naphthalene
liquid liquid Ethyl alcohol and water (miscible)
gas liquid SODA CO2 gas in water
gas gas AIR O2 gas, N2 gas
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Definitions

• Solutions can be classified as saturated or
  unsaturated.
• A saturated solution contains the maximum
  quantity of solute that dissolves at that
  temperature.
• An unsaturated solution contains less than the
  maximum amount of solute that can dissolve at a
  particular temperature

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Definitions

• SUPERSATURATED SOLUTIONS contain more solute than
  is possible to be dissolved in a given amount of
  solvent
• Supersaturated solutions are unstable.
• -- the supersaturation is only temporary
• -- need to warm the solvent so that it will
  dissolve more
• -- then need to cool the solution slowly

http//www.youtube.com/watch?vjVhPZg3dxIg
http//www.youtube.com/watch?vHnSg2cl09PIfeature
related
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Somewhere In Between

• Some mixtures are in-between heterogeneous
  mixtures and homogeneous solutions.

• suspension
• has clumps that stay floating
• filtering a suspension will usually separate the
  particles.

• colloid
• has very small clumps that almost make a
  solution
• the clumps are so small that they pass through
  most filters
• milk is an example of a colloid.

• emulsion
• the clumps of particles are held with an
  emulsifying agent.
• mayonnaise as an example

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Define the following words solubility.     Miscib
le   Immiscible  
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Separation of Mixturestypes of

• Filtration
• Separation of mixture on the basis of differences
  in the size of the particles
• Mostly used to separate solids from liquids (but
  filtration is used to separate all phases of
  matter from one another)
• Ex. Air filters separate gas (air) from solid
  (dirt particles)

http//www.youtube.com/watch?vnJVbFIIycKo
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• Distillation
• Based on the tendency of a substance to vaporize
  (turn to a gas)
• Based on boiling point differences
• The substance in the mixture with the lowest
  boiling point will vaporize first from the
  mixture
• Ex. Crude oil ? http//www.youtube.com/watch?v26A
  N1LfbUPc

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• Chromatography
• Based on the differences in solubility
• Two types ? Gas and Paper
• Mixture separates as it travels (most soluble
  separates first)
• Solute substance that gets dissolved
• Solvent substance that does the dissolving
• Ex. Separating ink in a marker

http//www.youtube.com/watch?vLY44uD2miYM
http//www.youtube.com/watch?vOKxRx0ctrl0feature
related
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• Crystallization
• Separation of the mixture is based on solubility
  differences
• Temperature changes within the mixtures change
  solubility of parts of the mixture
• Solubility the amount of a solute that is able
  to dissolve in a given amount of solvent
• Ex. Rock candy http//www.youtube.com/watch?vl_U
  SYub3djYfeaturerelated

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SOLUTION CHEMISTRY

• Concentration
• amount of solute in a given amount of solvent
  (can be determined quantitatively)
• Dilute
• a solution with a small amount of solute per
  solvent amount (relative term)
• Concentrated
• a solution with a large amount of solute per
  solvent amount (relative term)
• BOTH DILUTE AND CONCENTRATED ARE QUALITATIVE

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Concentration of Solute

• The amount of solute in a solution is given by
  its concentration.

The concentration of a solution is said to be its
molarity. Ex. 1 M CuSO4 1 molar copper II
sulfate