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UNIT 6 NOTES

• Chapter 16 Classification of Matter

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What is Matter?

• Anything that contains mass and takes up space!!!

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Types of Matter

• Pure Substances
• Can not be broken down into a simpler form
• Definite Composition

• Mixtures
• Can be broken down into simpler forms.
• Indefinite Composition
• Is made up of two or more pure substances that
  can be separated by physical means.

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Measuring Matter

• Mass
• How much stuff a material is made up of-
• Number of atoms in an object
• Volume
• The amount of space that is taken up by the
  matter.

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Measuring Volume of a Liquid
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Measuring Volume of a Solid
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Measuring Volume of an Irregular Shape Solid
Displacement Method
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Measuring Mass

• Scale
• Measures the gravitational force on an object.
• Measures weight
• Mass is calculated from the weight of the object
  (on earth)

• Balance
• Measures the mass of an object by comparing it to
  another object with a known mass.
• This method of mass measurement is not affected
  by gravity.

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UNIT 6 NOTES

• Chapter 16.3 States of Matter

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Atoms Molecules Review

• Atom

• Molecule

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Kinetic Theory of Matter

• All matter is made up of particles that are in
  constant motion.
• High Temperature Move very fast!
• High Energy
• Low Temperature Move very slow!
• Low Energy

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Temperature?

• The average energy of a materials molecules.
• 100 water has molecules with a very high energy.
• 0 Ice has molecules with low energy

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STATE OF MATTER DEFINITION SHAPE VOLUME EXAMPLES
SOLID Materials with particles close together definite definite Candle, pencil, desk
LIQUID Materials with particles that can slide past one another indefinite definite Water, Kool-Aid
GAS Materials with particles that move randomly in straight lines indefinite indefinite Air, oxygen
PLASMA A gas like mixture of positive and negatively charged particles unknown unknown Stars and Sun 99 of Solar system
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a. definite shape b. definite volume c. variable
shape d. variable volume
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Compare Volumes of a Solid, Liquid and Gas
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Thermal Expansion

• As matter gets hotter, it expands
• As matter cools down, it contracts

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Change of State

• A state of matter is how the material currently
  exists
• Solid
• Liquid
• Gas
• Plasma
• The conversion from one state of matter to
  another.

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Change in State / Phase Change Description of Change Example
Evaporation Liquid to Gas Alcohol and water
Condensation Gas to Liquid Shower doors and pop can
Melting Solid to liquid Ice melting
Freezing Liquid to solid Water freezing
Boiling or Vaporization Liquid to gas Water boiling
Sublimation Solid to gas iodine
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Important Temperatures

• Boiling Point
• The amount of energy (Temperature) that is needed
  to change a material from a liquid to a gas

• Melting Point
• The amount of energy (Temperature) that is needed
  to change a material from a solid to a liquid

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UNIT 6 NOTES

• Chapter 17 Density

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What is Density?

• The relationship between Mass and Volume.
• Density is a property of Matter. It will always
  be the same quantity for a piece of matter
  regardless of shape or size.
• Describes how tightly packed together atoms are
  in different materials.

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Density Calculation

• What is the Density of a bolt that has a mass of
  14g and a volume of 2ml?
• D m / v
• D 14g / 2ml
• D 7 g/ml

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Density Calculation

• What is the volume of liquid silver sample that
  has a density of 0.125 g/ml and a mass of 1.2g?
• V m / D
• V 1.2g / 0.125 g/ml
• V 9.6 ml

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Density of Water

• Density of a solid is typically greater than
  density of a liquid or gas.
• Water is exception- Solid ice is less dense than
  liquid water.
• What are the consequences for life of earth if
  ice (solid) had the greater density?

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UNIT 6 NOTES

• Chapter 17 Fluid and Gas Laws

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Buoyant Force Fluid Law

• The upward force exerted on an object immersed in
  the fluid.

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Archimedes Principal

• The buoyant force of an object in a fluid is
  equal to the weight of the fluid displaced by the
  object.

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Floating vs. Sinking

• If buoyant force is greater than the weight of
  the object, then the object will float.
• If the buoyant force is less than the weight of
  the object, then the object will sink.
• Also depends on the shape of the object. The
  more water displaced by the shape of an object,
  the greater the buoyant force.

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Charles Law Gas Law

• As the Temperature of a gas changes the volume
  will also change.
• As Temperature increases, volume will also
  increase.
• This is a DIRECTLY PROPORTIONAL relationship.

T ? V ?
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Charles Law
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• http//www.riverdeep.net/science/chemistry_gateway
  s/cg_activity_pages/catn.activityi_800045.jhtml

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What is Pressure?

• The amount of force exerted on an area
• Pressure Force / Area
• NEW UNIT!
• Pascal (Pa) usually (kPa)

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Boyles Law Gas Law

• Pressure and Volume have a relationship.
• They will always be opposite each other as long
  as temperature remains the same
• This is called an INVERSE relationship.

V ? P ?
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Boyles Law
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UNIT 6

• CHAPTER 18 ATOMIC STRUCTURE

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What is an Atom?
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Atomic Number

• The number of protons
• Or electrons
• Whole Number!

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Mass Number

• Number of protons and neutrons in an atoms.

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Atomic Mass

• The average mass of all isotopic forms of an
  element.

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• Hydrogen 1 (hydrogen) 1 proton, 0 neutronsMass
  number 1
• Hydrogen 2 (deuterium) 1 proton, 1 neutronMass
  number 2
• Hydrogen 3 (tritium) 1 proton, 2 neutronsMass
  number 3

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UNIT 6

• CHAPTER 18 PERIODIC TABLE

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Periodic Table

• The word periodic means repeated in a pattern.
• The design of the periodic table has many
  patterns.
• It arranges elements in order by size and property

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Chemical Symbol

• A shorthand abbreviation representing a chemical
  element
• The first letter is always a capital
• 1, 2 or 3 letters in a symbol
• 1-92 are natural anything above 93 is manmade

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Atomic Number and Atomic Mass

• The modern periodic table is in order by atomic
  number across the periods.
• The atomic mass naturally increases also, but not
  systematically.

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Part of the Table Location Characteristics
Groups Columns Organized by similar properties
Periods Rows Determined by the e- orbital used
Metals Left side Good conductors, mostly solids, ductile, malleable
Non-Metals Right side Poor conductors, gases
Metalloids Stairs Properties fall in between
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Electron Configuration

• Electrons are organized on the outside of the
  atom in orbitals.
• An orbital is a region of space around the
  nucleus of an atom where an electron is likely to
  be located.
• They move like planets around the sun.
• Each electron in an atom has a specific amount of
  energy and the energy of an electron can change.

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Energy Levels

• The possible energies an atom can have are called
  energy levels.
• An electron in an atom can move from one energy
  level to another when the atom gains or loses
  energy.
• Staircase analogy
• The level closest to the nucleus that has the
  least energy has the lowest number of electrons,
  2.

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Energy Levels

• An electron configuration is the arrangement of
  electrons in the orbital of an atom.
• The most stable electron configuration is the one
  in which the electrons are in orbits with the
  lowest possible energy.

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Valence Energy Level

• A valence electron is an electron that is in the
  highest occupied energy level of an atom.
• These electrons play a key role in chemical
  reactions.
• Elements in a group have similar properties
  because they have the same number of valence
  electrons.
• (Hydrogen location on periodic table)
• When the highest occupied energy level is full an
  atom is stable. (HAPPY.)

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UNIT 6

• XTRAS

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Flame test

• When compounds are placed in the flame, atoms
  absorb energy and move to a higher energy levels.
• As these electrons move back to lower energy
  levels, they release energy as visible light.
• The color of light produced depends on the
  difference in energy between two specific energy
  levels in an atom

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Electron Dot Diagram

• An electron dot diagram is a model of an atom in
  which each dot represents a valence electron.
• The symbol in the center represents the nucleus
  of and all other electrons in an atom.

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Stable Electron Configurations

• When the highest occupied energy level of an atom
  is filled with electrons, the atom is stable and
  not likely to react.
• Noble gases

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Pascals Principle

• The pressure applied to a fluid is transmitted
  unchanged throughout the fluid.

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Bernoullis Principle

• As the velocity of a fluid increases the pressure
  exerted by the fluid decreases.

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Notes 9.1

• Types of Matter

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Solution

• A homogeneous mixture.
• The particles are so small that they can not be
  seen with a microscope.

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Suspension

• A Heterogeneous mixture that settles.
• Muddy water

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Colloid

• A heterogeneous mixture that never settles.
• Ex. Milk

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Tyndall Effect

• The scattering of light particles in a mixture.

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COLLOIDS SOLUTIONS
Clouds Sugar water
Smoke Air
blood Salt water
Shaving cream Steel
Jell-O Carbonated water
Mayonnaise tea
milk Metal alloys
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Notes 9.3

• Physical and Chemical Properties and Changes

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Comparison of Physical and Chemical Properties
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Physical Property

• Any characteristic of a material that can be
  observed or measured without change in the
  composition of the substances in the material.
• Properties include
• Size
• Shape
• State
• Ex. Braiding Hair / Cutting Hair

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Examples of Physical Properties
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Using Physical Properties to Separate Mixtures

• Filtration a process that separates materials
  based on the size of their particles.
• Distillation A process that separates materials
  based on their boiling points.

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Chemical Properties

• Can be observed only when the substances in a
  sample of matter are changing into different
  substances.

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Is a Change Chemical or Physical?

• When matter undergoes a chemical change, the
  composition of the matter changes. When matter
  undergoes a physical change, the composition of
  the matter remains the same.

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Changes

• Physical
• Ice to Water to Steam

• Chemical
• Flammability, Reactivity
• Change in color
• Production of a gas
• Formation of a precipitate

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Law of Conservation of Mass

• Mass can not be created or destroyed by a
  chemical reaction (change).

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Mendeleev and Moseley

• Dmitri Mendeleev was a Russian chemist who
  organized the known elements by atomic mass.
• Henry Moseley was an English scientist who
  organized the elements by atomic number and
  properties.
• Today the periodic table is arranged by atomic
  number.