MATTER UNIT

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MATTER UNIT

• What Matter Is
• Mass vs Weight
• Three Phases of Matter
• Classification of Matter
• Matter Summary
• Chemical Physical Changes
• Chemical Physical Properties

Kenneth E. Schnobrich
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MATTER

• What is Matter??

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Matter is generally defined as anything that has
mass and occupies space.
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Mass vs Weight
Mass refers to a quantity of matter and the
mass remains the same no matter where you are.
Weight however is determined by the effect
of gravity on a quantity of matter.
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THE THREE PHASESofMATTER
SOLID LIQUID GAS
Particles closely packed Particles are close but free to move Particles far apart moving randomly
Definite shape and volume No definite shape Definite volume No definite shape No definite volume
Strong interparticle attractions Weak interparticle attractions Almost no attractive forces
Little to no diffusion Moderate diffusion Rapid diffusion
Incompressible Incompressible Compressible
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THE THREE PHASESofMATTER
SOLID LIQUID GAS

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CLASSIFICATION OF MATTER
Elements
PURE SUBSTANCES
Compounds
ELEMENTS - are the building blocks of compounds
COMPOUNDS - are made up of 2 or more different
elements, chemically combined in a definite
ratio by mass
Pure Substances cannot be separated by physical
means
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THE ELEMENTS
You should be looking at the Periodic Table
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PROPERTIES OF METALS

1. They have high melting boiling points
2. They exhibit heat and electrical conductivity
3. They exhibit metallic lustre
4. They are malleable
5. They are ductile
6. They have low specific heats
7. They have high densities
8. Most appear silvery-gray in color (Cu, Au)
9. They have strong interatomic forces of attraction
10. Most are solids at room temperature (Hg)

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METALLOIDSSEMIMETALS
THE SEMIMETALS HAVE PROPERTIES THAT ARE VARIABLE
DEPENDING ON WHAT THEY ARE REACTING WITH - BUT
THEY CAN BEHAVE AS BOTH METALS AND NONMETALS
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NONMETALS

1. They have low melting boiling points
2. They exhibit no heat and electrical conductivity
3. They exhibit a variety of colors
4. They are brittle
5. They are generally gases (C,P,S,Se,Br,Te,I) at
   STP
6. They are dull in appearance
7. They generally show weak attractive forces
8. Many are diatomic (H2. N2, O2, F2, Cl2, Br2. I2)

Diatomic means 2 atoms per molecule
Solids or Liquids at STP
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COMPOUNDS
IONIC COMPOUNDS MOLECULAR COMPOUNDS
Combinations of metals nonmetals Combinations of nonmetals
Most are soluble in water Most are insoluble in water
High MP BP Low MP BP
In solution they are good electrolytes In solution they are poor electrolytes
Crystals are brittle Crystals are soft
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IONIC COMPOUNDS
Ionic compounds are generally combinations of
metals and nonmetals.
METALS - tend to lose electrons and form
cations. Cations are simply ions having a
positive charge. Na -gt Na1 or Ca -gt Ca2
or Al -gt Al3
NONMETALS - tend to gain electrons and form
anions. Anions are simply ions having a negative
charge. Cl -gt Cl-1 or S -gt S-2 or N -gt
N-3 or O -gt O-2
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MOLECULAR COMPOUNDS
Covalent compounds are generally combinations of
nonmetals and nonmetals.
EXAMPLES
CO2
H2O
CH4
C6H12O6
molecular and covalent compounds are the same
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MIXTURES - TWO TYPES
MIXTURES - have no definite composition and they
are easily separated by physical means unlike
elements and compounds.
HOMOGENEOUS MIXTURES - are called SOLUTIONS and
they appear uniform throughout.
HETEROGENEOUS MIXTURES - are very common and
they do not appear uniform throughout.
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Examples of HomogeneousMixtures
SOLID LIQUID GAS
ALLOYS SALT WATER AIR
AMALGAMS KOOLAID ANY GAS MIXTURE
Solid solutions Liquid solutions Gaseous solutions
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EXAMPLES OF HETEROGENEOUSMIXTURES
A CHEESE, PEPPERONI, SAUSAGE, MUSHROOM, AND HOT
PEPPER PIZZA FROM LaNOVA
A RUBY TUESDAYS BOWL OF BROCCOLI CHEESE SOUP
A TIM HORTONS CRANBERRY TEA BISCUIT
A HARRYS HARBOR FRONT FRESH GARDEN SALAD WITH
ITALIAN DRESSING
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MATTER SUMMARY
Definitions of the terms above
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DEFINITIONS
Elements - these are the basic building blocks
for all compounds and cannot be separated by
physical or chemical means Compounds - chemical
combinations of 2 or more different elements in
a definite ratio by mass. Compounds cannot be
separated by physical means only by chemical
means Pure substances - these are either elements
or compounds Mixtures - these are physical
combinations of 2 or more pure substances in no
definite ratio by mass. Mixtures can be
separated by physical means Homogeneous mixtures
- are also called solutions and they appear
uniform throughout Heterogeneous mixtures - the
individual components of a mixture of this type
can be readily seen
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Chemical PhysicalProperties Changes
PHYSICAL PROPERTIES - are those properties that
can be determined using the physical senses
Color Odor Taste Crystal structure Density Specifi
c Heat Heat of Vaporization Heat of
Fusion Melting Point Boiling Point
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Extensive vs IntensivePhysical Properties

• Extensive - properties that are dependent on
  sample size
• Mass
• volume

• Intensive - independent of sample size
• Density
• MP BP
• Specific Heat
• Color
• Heats of Fusion Vaporization
• Taste/Odor

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Chemical PhysicalProperties Changes
CHEMICAL PROPERTIES - are those properties that
identify how one substance reacts with another
Iron rusts Copper develops a patina
Hydrogen combines with Oxygen to form water
Carbon combines with oxygen to form CO2 or CO
The element Na (sodium) combines with water
to form H2 and NaOH
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Chemical PhysicalProperties Changes
PHYSICAL CHANGE - These are changes in a
substance that do not involve a change in
composition
Most common Phase changes
2 phases
2 phases
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Chemical PhysicalProperties Changes
CHEMICAL CHANGE - These are changes that do
involve a change in the composition of a
substance
2H2(g) O2(g)
2H2O(g)

Bonds are actually broken and made
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REACTIONS OF THE ALKALI METALS
When you click on the link below you will see a
demonstration of the activities of the Alkali
Metals in Group 1. It should be noted that the
reactions of Rubidium and Cesium may have been
exaggerated slightly. It is important to note
that Rubidium and Cesium are so reactive that
they have to be kept in a closed vial with an
inert gas atmosphere prior to immersing in the
water. All of the Alkali metals will form oxides
on their surfaces rather quickly because of their
reactivity. Do not try to duplicate these
demonstrations.
Special Note you may want to Preview this
YouTube video.
click