Matter Properties and Changes

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Matter Properties and Changes

• Physical Chemical Properties
• Classify matter element, compound, mixture
• Identify observable characteristics of chemical
  reactions
• Law of conservation of mass

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Substance

• Matter that has a uniform and unchanging
  composition
• Salt, water, 3M HCl,

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Physical Property

• A characteristic that can be observed of measured
  without changing the samples composition

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Physical Properties

• Extensive properties
• Dependent on the amount of substance present
• Mass, length, volume,
• Intensive properties
• Independent of the amount of substance present
• Density

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Chemical Properties

• The ability of a substance to combine with or
  change into one or more other substances
• Rust,

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States of Matter

• Changing between physical phases depending on
  temperature and/or pressure
• Melting Boiling points
• Solid
• Liquid
• Gas
• Plasma
• The way it fills a container

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Solids

• Form of matter that has its own definite shape
  and volume
• Tightly packed particles
• Expands when heated

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Liquids

• A form of matter that flows, has constant volume
  and takes the shape of its container
• Particles move past each other
• Particles expand when heated

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Gases

• Form of matter that flows to conform to the shape
  of its container and fills the entire volume of
  the container
• Easily compressed
• Vapor
• Gaseous state of a substance that is a solid or
  liquid state at room temperature

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Physical Changes

• Changes that alter the a substance without
  changing its composition
• Cutting paper, breaking a beaker,

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Chemical Changes

• Referred to as a chemical reaction
• New substances formed in the reaction have
  different compositions and different properties
  from the substances present before the reaction
  occurred

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Conservation of mass

• States that mass is neither created nor destroyed
  in any process it is conserved.
• Massreactants Massproducts
• Antoine Lavoisier
• Analytical balance
• Mercury (II) oxide yeilds mercury oxygen
• 216 g 200 g 16 g

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Mixtures

• Combination of 2 or more pure substances in which
  each pure substance retains its individual
  chemical properties
• Salt and water or sand and water

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Types of mixtures

• Heterogeneous mixture
• Does not blend smoothly throughout and in which
  the individual substances remain distinct
• Sand and water

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Types of mixtures

• Homogeneous mixture
• Has consistent composition throughout, it always
  has a single phase
• Solutions
• Solid, liquid or gas

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Separating Mixtures

• Filtration
• Uses a porous barrier to separate a liquid from a
  solid
• Distillation
• Based on differences in boiling points of the
  substances involved

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Crystallization

• Separation technique that results in the
  formation of pure particles of a substance from a
  solution containing the dissolved substance

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Chromatography

• Technique that separates the components of a
  mixture on the basis of the tendency of each to
  travel or be drawn across the surface of another
  material

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Elements

• A pure substance that cannot be separated into
  simpler substances by physical or chemical means
• 91 occur on earth naturally
• Cu, O, Ag

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Periodic Table of Elements

• Organizes elements into a grid of horizontal rows
  called periods and vertical columns called groups
  or families

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Dmitri Mendeleev

• Based on similarities and masses
• Could accommodate for elements that had not even
  been discovered yet
• Was able to predict the properties of elements
  that were not yet discovered

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Compounds

• Combination of two or more different elements
  that are combined chemically
• Water, salt, sugar, aspirin

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Law of Definite Proportions

• States that, regardless of the amount, a compound
  is always composed of the same elements in the
  same proportions by mass
• Percent by mass
• The ratio of the mass of each element to the
  total mass of the compound as a percent
• Percent by mass () (mass of element / mass of
  compound) x 100

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Copper Carbonate
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Sucrose Analysis
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Law of Multiple Proportions

• States that when different compounds are formed
  by combinations of same elements, different
  masses of one element combine with the same
  relative mass of the other element in a ratio of
  small whole numbers.

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Analysis Data of Two Copper Compounds
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Compare ratio of mass of copper to the mass of
chlorine for each compound

• Mass ratio compound I / mass ratio compound II
• 1.793 g Cu/g Cl / 0.896 g Cu/g Cl 2.000