Atomic Structure: Chpt. 4

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Atomic Structure Chpt. 4

• Atom Robert Milliken
• Democritus J.J Thomson
• John Dalton James Chadwick
• Daltons Atomic Theory Ernest Rutherford
  
• Protons
• Electron
• Neutrons
• Cathode Ray
• Eugen Goldstein

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Objectives

• 1. I can classify matter into substances and
  mixtures.
• 2. I can identify and distinguish between
  physical and chemical properties.
• 3. I can identify and distinguish between the
  two types of forces that affect the nature of
  molecules.
• 4. I can understand and distinguish between
  physical and chemical changes.
• 5. I can identify techniques used to separate
  mixtures.

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Daily Objective

• I can define matter.
• I can identify and distinguish between the
  classes of matter.

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What is Matter?
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csc-ut.org
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Whats The Matter?
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fccps.org
maniacworld.com
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What is Matter?

• Students used background knowledge and peers to
  answer this question.

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What do all matter have in common?Atoms!
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What is Matter?

• One or more atoms that take up space and has
  mass.
• Emphasized that all matters properties and
  changes are due to the chemical make-up and
  interactions on the atomic level.

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Students used background knowledge and peers to
write or draw what comes to mind on the following
terms related to matter.
Substance Mixture
Element Homogenous Mixture
Compound Heterogenous Mixture
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Classification of Matter
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Classifying MatterSubstances vs. Mixtures
Substances Definite chemical make-up Elements or compounds Ex. Silicon chip or H2O Mixtures Varied chemical make-up 2 or more substances physically combined Homo or Hetero Mixtures Pizza and salt water
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Classifying MatterSubstances vs. Mixtures
Element Pure and simplest substance One type of atom Periodic table Symbol, (He Helium) Homogenous Mixture 2 or more substances physically combined. Substances are very soluble in one another-mix well one phase Substances in mix properties are preserved Separated by physical processes. Also called a solution Ex. salt water, kool-aid
Compound 2 or more substances chemically combined Definite composition Break-down only thru chemical processes Substances making up cmpd gain new properties. Chemical Formula, H2O Ex. iron rust Heterogenous Mixture 2 or more substances physically combined. Substances are not soluble in one another-do not mix well-multiple phases Substances in mixture properties are preserved. Separated by physical processes Ex. Oil and water, pizza, soil
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Periodic Table
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Compounds Compounds Chemical Combination
of elements in fixed amount. Ex. Sodium
Chloride (salt) NaCl Sodium (Na)
Chlorine (Cl) Salt (NaCl)
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Heterogenous MixuresObserve multiple phases or
parts because substances do not mix well.
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Homogenous MixturesSubstances mix well so
observe one phase or part.
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Homongenous Mixtures

• Also called solutions.
• Solutions
• -Solute what is dissolved
• -Solvent what dissolves
• Solubility the ability of the solute to dissolve
  in the solvent.
• .

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Classify each type of Matter
Iron Rust, FeO
Iron Ore, Fe
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Bell Ringer Matter

• What is matter?
• What is the difference between
• substances and mixtures
• compounds and mixtures
• Classify each of the following examples
• sugar
• sugar water
• gold ring
• Iron rust (FeO)
• Italian dressing

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Classifying Matter

• one kind of atom
• physical combination of substances
• multiple phases
• one phase
• chemical combination of substances
• same chemical make-up from sample to sample
• properties are preserved when substances combine
• varied chemical make-up from sample to sample
• properties change when substances combine
• oxygen (O2)
  
• muddy water
• limestone (CaCO3)
• tap water

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Substances
Element
Compound
Substance
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Mixtures
Homogenous Mix
Heterogenous Mix
Mixtures
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Classifying Matter Lab

• Students with peers observed various samples of
  matter and classified them as an element,
  compound, homo mixture, or hetero mixture.

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Classifying Matter

• 1. Classify each as either an element, compound,
  homo mixture, or hetero mixture
• a. soil
• b. orange juice with no pulp
• c. copper wire
• d. car gasoline (C8H18)
• 2. What is the difference between a compound and
  a mixture?

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Classification of Matter
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Classifying Matter Lab

• Students re-assess their classification of matter
  lab examples.

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Chemical Changes

• A chemical process
• Substance(s) chemical make-up is changed
  producing new substances.
• New properties are observed.
• Ex. Iron Rust (FeO)

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Intramolecular Forces
Forces within a compound that holds the atoms
together. Also called chemical bonds.
H2O compound
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Types of Chemical Changes

• Combustion
• Decaying
• Digesting
• Baking
• Neutralization (acidic and basic chemicals)
• Growing
• Spoiled

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Physical Changes

• Physical process
• Substance(s) chemical make-up is preserved so no
  new substance is produced.
• Properties are preserved
• Ex. Making Lemonade

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Intermolecular Forces
Forces between compounds in a sample of matter.
(group forces)
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Types of Physical Changes

• Most state of matter changes
• Breaks
• Dissolves
• Crushes
• Cuts
• Absorbs

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Physical vs. Chemical Changes

• Re-assess Chemical and Physical Change Lab
• Homework Physical vs. Chemical Change Worksheet
  

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What kind of forces are affected ?
.
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Mixture Separation Lab

• Students work in groups to determine what
  physical processes they can use to separate out
  each substance in a given mixture.
• They will design and carry out their experiment
  to successfully separate out each substance in
  the mixture.
• Reiterate the concept that substances in a
  mixture maintain their physical properties
  because their chemical make-up is preserved.

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Mixture Separation Lab

• What physical properties did you use to separate
  the substances in the mixture?

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Scientific Skills Exam
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Homongenous Mixtures

• Also called solutions.
• Solutions
• -Solute what is dissolved
• -Solvent what dissolves
• .

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What comes to mind?
.
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Mixture Separation Lab

• What physical properties did you use to separate
  the substances in the mixture?

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Physical Separation of MixturesExtraction

• 1. Extraction- separating substances in a
  heterogenous mixture from one another based on
  their unique physical properties..

Physically separate oil from water because they
are not soluble in one another.
How could we separate iron fillings and sand?
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Solubility of Mixtures
Solubility How well substances physically
combine.
Sciencephoto.com
Chemistryland.com
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Solubility of Mixtures
Chemistryland.com
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Physical Separation of MixturesFiltration

• Commonly used to separate a solid from a liquid
  in a heterogenous mixture due to differences in
  size or solubility.

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Physical Separation of MixturesDistillation
Separation of liquids in a mixture by their
differences in boiling points. Ex. Ethanol
(78 0C) and Water (1000C)
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Chromotography

• Separates homogenous mixtures based on
  solubility.
• Chromotography has two phases
• -Stationary Phase solid
• Mobile Phase liquid or gas
• Substances in mixture will separate
• based on their degree of solubility
• toward the mobile phase.

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Physical Separation Techniques
Separation Technique Heterogenous Mixture Homogenous Mixture What physical properties are used?
Filtration
Extraction
Distillation
Chromotography
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Matter and Energy

• I can.
• Establish a relationship between changes in
  matter, the forces involved, and the flow of
  energy.

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Phases of Matter
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Phase Change Processes

• A. Melting
• B. Freezing
• C. Evaporation
• D. Condensation
• E. Sublimation
• F. Deposition
• G. Ionization
• H. Deionization

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Phase Changes
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Particles in Matter

• The particles that make-up matter are in constant
  motion.
• The particles speed of motion depends upon?

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Heat Energy

• Heat Energy Energy that is transferred between
  matter of different temperatures.
  (joules/calories)
• How does heat energy move between objects?
• Heat Energy Flow
• System matter you are studying/measuring
• Surrounding environment around the system
• Endothermic Process heat ______by system
• Exothermic Process heat ________by system
• (released or absorbed)

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Heat Energy

• Heat energy alters the
• -speed of particles
• -strength of the intermolecular forces

Heat Energy
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Temperature Scales
Temperature only measures the heat energy that
alters the speed of particles.
Visionlearning.com
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Molecular Kinetic Theory
Establishes a relationship between physical
changes, intermolecular forces, and energy flow.
OC
Heat Energy
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Conservation of Matter and Energy
Matter Matter undergoes changes, but the atoms
are conserved as a whole or as parts.
Energy Energy is also conserved during changes
that matter undergoes. If energy increases for a
system, then its surroundings must decrease in
energy by the same amount.

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Pre-AP

• The following slides pertain only to pre-AP
  chemistry classes.

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Heat Capacity

• Heat Capacity
• The amount of heat needed to raise the
  temperature of a substance 1.0 oC.
• What does heat capacity depend upon?

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Specific Heats of Common Substances
Substances Specific Heat J/g 0C Specific Heat Cal/g0c
water 4.18 1.00
Grain alcohol 2.4 0.58
ice 2.1 0.50
steam 1.7 .40
aluminum 0.90 0.21
silver 0.24 0.057
mercury 0.14 0.033
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Specific Heat Capacity

• Specific Heat Capcity
• The amount of heat it takes to raise 1g of the
  substance 1 0C.

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Heat Calculation

• The temperature of a 95.4 g piece of copper
  increases from 25.0oC to 48.0oC when the copper
  absorbs 849 Joules of heat. What is the specific
  heat of copper?

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Heat Calculations

• How much heat is required to raise the
  temperature of 250.0g of mercury to 52oC?

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Bell Ringer

• What is the difference between heat energy (q)
  and specific heat energy (C)?
• When 150.0 J of energy is absorbed by a 42.1 g
  sample of silver the temperature increases by
  15.0oC. What is the specific heat of silver?
• 3. If an 8.8 gram sample of aluminum increases in
  temperature from 25oC to 55oC how much heat was
  absorbed by the aluminum sample?

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Specific Heats of Common Substances
Substances Specific Heat J/g 0C Specific Heat Cal/g0c
water 4.18 1.00
Grain alcohol 2.4 0.58
ice 2.1 0.50
steam 1.7 .40
aluminum 0.90 0.21
iron 0.46 0.11
silver 0.24 0.057
mercury 0.14 0.033