Physical Property

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Physical Property

• Describes form or behavior of matter

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Independent of sample size(density, melting
point, boiling point, etc.)

• Intensive Properties

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Depend on how much stuff!(Mass Volume)

• Extensive Properties

4
Chemical Property

• Describes how matter interacts with other matter

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Chemical Change

• Identity Change
• A new substance is formed.

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Chemical ChangeIdentities change!
Note particle diagram shows conservation of
mass same of each type of atom on reactant
and product sides.
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Monatomic

• One-atom Molecule

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2 or more uppercase letters in formula

• Compound

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Physical Change

• Identity stays the same

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H2O(l) ? H2O(g)

• Phase changes are physical changes. Identity
  stays the same.

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2H2O(l) ? 2H2 O2(g)

• Identity changes.
• Chemical change.

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Diatomic

• 2-Atom Molecule

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Smallest particle of an element that retains the
properties of the element and that can
participate in a chemical reaction.

• Atom

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Gases

• Take the shape volume of their container

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Physical Constant

• Physical property expressed with a unit.
  Independent of sample size.

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Liquids

• Definite volume but no definite shape

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Solids

• Definite volume definite shape

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Compound

• 2 or more elements chemically combined

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Element

• Cannot be broken down into anything simpler by
  ordinary chemical or physical methods

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Mixture

• Physical combination of 2 or more pure substances.

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Pure Substances

• Elements Compounds

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Pure Substances
The particles in each case are identical to each
other.
Type of Matter?
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Mixtures

• Heterogeneous or Homogeneous

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Heterogeneous Mixtures
Type of Mixtures?
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Homogeneous Mixtures!
Type of Mixtures?
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Pure Substance!
Mixture or Pure Substance?
27
Distillation

• Physical method of separating mixture of 2 or
  more liquids based on differences in boiling
  points.

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Solution

• Homogeneous Mixture. Liquid gas phase
  solutions transmit light. Look translucent. Do
  not separate on standing.

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Suspension

• Heterogeneous Mixture. Scatter light. Look
  cloudy. Need to be shaken or stirred. Separate
  on standing.

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NaCl(aq)

• Homogeneous Mixture. NaCl dissolved in water.

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NaCl(s)

• Pure substance. NaCl in the solid phase.

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Variable Composition

• Mixture

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NaCl(l)

• Pure substance. NaCl in the liquid phase.

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NaCl(g)

• Pure substance. NaCl in the gas phase.

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Homogeneous

• Uniform, constant, the same throughout.

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Always Homogeneous

• Pure substance Element or Compound

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Filtration

• Physical separation technique used to separate
  heterogeneous mixtures. Based on differences in
  particle size.

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Sorting

• Physical separation technique used to separate
  heterogeneous mixtures. Based on differences in
  appearance.

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Definite Unique Properties

• Pure substance. Element or Compound.

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Broken into components by chemical decomposition
reaction

• Compound

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Definite Composition

• Pure substance. Element or Compound.

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Separated by physical technique

• Mixture

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Triatomic

• 3-atom Molecule

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May be homogeneous or heterogeneous

• Mixture

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Compare pure substances mixtures
Pure Substances Mixtures
Unique Properties No unique properties
Definite Composition Variable Composition
Always Homogeneous in a single phase May be homogeneous or heterogeneous
Elements cannot be broken down. Compounds can be separated into elements using chemical separation techniques. Can be separated into component substances using physical methods.
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Density, melting point, boiling point

• Examples of physical constants

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Law of conservation of mass (lab scale)

• Total Mass of Reactants
• Total Mass of Products

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• Total of atoms of each type on reactant side
  
• Total of atoms of each type on product side

Law of conservation of mass (microscale)
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No new properties. Properties are a mix of
properties of components.

• Mixture

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C6H12O6(s) ? C6H12O6(aq)

• Equation represents dissolving. Dissolving is a
  physical change.

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Physical Properties

• Used to identify substances.

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Atoms can vibrate back forth about a fixed
position.

• Solid state

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Ways to separate heterogeneous mixtures

• Sorting
• Filtration
• Crystallization
• Evaporation
• Distillation
• Chromatography
• Differences in density

• Differences in magnetic properties
• Differences in solubility

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Change of phase terms

• Evaporation l to g
• Freezing l to s
• Melting s to l
• Condensation g to l
• Boiling l to g
• Deposition g to s
• Fusion s to l
• Sublimation s to g

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Names of Phase Changes
Evaporation, Boiling, or Vaporization
Melting or Fusion
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Molecules are relatively far apart from each
other can move from place to place.

• Gas Phase

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Molecules are pretty close, but have enough room
to slide past each other.

• Liquid Phase

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One substance dissolved in another substance

• Solution

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Homogeneous mixture in a single phase

• Solution

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CANNOT be separated by filtration. Liquid phase
MUST be evaporated.

• Solution

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(aq) means dissolved in waterIts a solution!

• NaCl(aq)

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Heterogeneous mixture of a solid in a
liquidMust be shaken or stirred
constantlyLooks murky or opaque

• Suspension

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Solid phase can be separated by filtration

• Suspension

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Heterogeneous Mixture
Separate the sand by filtration. Evaporate the
water to retrieve the salt.

• SiO2(s) NaCl(aq)

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Phase at room temperatrue

• Physical property

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Chromatography

• Physical separation technique based on
  differences in intermolecular forces.

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Vapor

• Gas phase of a substance that is usually a liquid
  at room temperature.

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Names for some chemical changes

• Corrosion, Decomposition, Neutralization,
  Burning, Fermentation, Rotting

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of atoms of each element before of atoms of
each element after

• Law of Conservation of Mass

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Percent

• Part X 100

Whole
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1 upper case letter in formula

• Element

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Cutting, Crumpling, Tearing, Pulling into wire,
Hammering into sheet

• Examples of physical changes

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Phase Changes

• Examples of physical changes

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Evidence of Chemical Change

• Production of heat light
• Formation of a gas (bubbles)
• Formation of a precipitate
• Change in identifying properties

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Opposite of dissolving. Solid comes out of
solution.

• Precipitation

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Particles arranged in a regular geometric pattern.

• Solid

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Endothermic
G
Potential Energy
L
Exothermic
S
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The solid phase the particles are closest
together! (Molecules are always attracted to one
another.)
For a given substance, which phase has the lowest
potential energy?
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They are the same size!
How do the centigrade degree and the Kelvin
compare?
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Phase change sublimationEndothermic

• H2O(s) ? H2O(g)

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Phase Change condensationExothermic

• H2O(g) ? H2O(l)

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Phase change meltingendothermic

• H2O(s) ? H2O(l)

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CO2(s) or dry ice and I2(s)

• Two common substances that sublimate?

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Mixture
Pure Substance
Pure Substance
Pure Substance
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Molecules have potential energy as a result of
their structure and composition.

• Chemical Potential Energy