Physical Property

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Physical Property

• Describes form or behavior of matter

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Physical Properties

• Color
• Luster
• Malleability
• Conductivity
• Hardness
• Cleavage
• Phase at room temp.
• Vapor pressure

• Melting point
• Boiling point
• Heat of fusion
• Heat of vaporization
• Density
• Specific Heat Capacity

Physical constants!
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Chemical Property

• Describes how matter interacts with other matter
  reactivity

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Chemical Change

• Identity Change

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Examples of Chemical Change

• Synthesis, Decomposition, Single Replacement,
  Double Replacement, Combustion, Polymerization,
  Esterification, etc.

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Monatomic

• One-atom Molecule

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1 uppercase letter in formula

• Element

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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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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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Mixtures

• Heterogeneous or Homogeneous

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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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Heterogeneous

• Non-uniform composition.
• May see regions that look different. May be more
  than 1 phase present.

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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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Density, melting point, boiling point

• Examples of physical constants

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Law of conservation of matter

• Mass Before Mass After

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Given X 2Y ? Q 3Z

• Mass Before Mass After

The equation is a distractor. 44 128 32
grams Z 140 g.
When 44 grams of X react completely with 128
grams of Y, 32 grams of Q are produced. How much
Z will be made?
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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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Phys. M.
Chem.
(solutions)
(suspensions)
Mixtures ? Separated by physical
methods. Compounds ? Separated by chemical
methods.
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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
Liquid to gas

• Evaporation
• Freezing
• Melting
• Condensation
• Boiling
• Deposition
• Fusion
• Vaporization
• Sublimation

Liquid to solid
Solid to liquid
Gas to liquid
Liquid to gas
Gas to solid
Solid to liquid
Liquid to gas
Solid to gas
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Crystallization and Solidification

• More change of phase terms.
• Liquid to Solid.

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Substances that sublimate

• CO2 and I2

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Molecules are relatively far apart from each
other can move from place to place.

• Gas Phase

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One substance dissolved in another substance

• Solution

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Phase at room temperatrue

• Physical property

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

• Liquid Phase

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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

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

• Law of Conservation of Matter

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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

• Physical changes

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Dissolving

• Physical Change

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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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Particle Diagrams
Pure substance units the same. molecules of a
triatomic compound.
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Mixture units differ. monatomic element,
diatomic element, triatomic compound.
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Mixture
Pure Substance
Pure Substance
Pure Substance
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Compounds vs. Mixtures
Always homogeneous May be homogeneous or heterogeneous
Definite composition Variable composition
Definite unique properties No unique properties
Separated into elements by chemical reaction Separated into components by physical methods