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Chapter 3 QBA Miguel A. Castro R.

                Substances are
                made of atoms
Natural Philosophy

 Heraclitus   versus Parmenides

 Heraclitus– everything is in the
  process of change
 Parmenides – Change is impossible
Natural Philosophy

 In400 BCE, Democritus stated, All
  matter consists of tiny particles called
  átomos, which are not created and
  cannot be destroyed.
 This was the beginning of the atomism.
Natural Philosophy

 The fight wasn’t over. Plato disagreed.
 He thought that the beauty of the world
  had to be caused by more than mere
  atoms.
 He proposed a system of changing
  elements; water, fire, earth, air.
Natural Philosophy

 Aristotle
          disagreed with both
  Democritus and Plato. He proposed a
  system called Hylomorphism.

 Hylomorphism  is a system of ever
  changing states of matter.
Natural Philosophy

 Atomism  was lost until the 16th Century
 Though it was still not a hard science, it
  was part of a belief system called
  alchemy.
 Thankfully, Robert Boyle put an end to
  the mess when he wrote The Skeptical
  Chemyst.
“Nature works by means of
     bodies unseen.”



            Lucretius
The Elements
SUBSTANCES ARE MADE OF ATOMS
Atomic Theory

 Threelaws provide supporting
 evidence of atoms.
  –   Law of Definite Proportions
  –   Law of Conservation of Mass
  –   Law of Multiple Proportions
Law of Definite Proportions

Every  compound is composed of
 specific elements and whole-
 number ratios of those elements.

Water H20 - 2 Hydrogen: 1 Oxygen
Law of Conservation of Mass

Matter cannot be create or
 destroyed by normal physical or
 chemical processes

i.e.-   What goes in, must come
 out!
SUBSTANCES ARE MADE OF ATOMS
Law of Multiple Proportions

The   same elements can bond
 in differing whole-number ratios
 to form different compounds.

        Methanol CH3O
         Ethanol C2H5O
SUBSTANCES ARE MADE OF ATOMS
Dalton’s Atomic Theory

 Itcontained five principles based on
  current knowledge of atoms.

 We   have summarized those principles
  in the following statements:
Dalton’s Atomic Theory

1.   All matter is made up of tiny
     indestructible particles called atoms.

2.   All atoms of one type (element) have
     the same mass and properties.

3.   Atoms of different types (elements)
     have different masses and properties.
Dalton’s Atomic Theory

4.   In Chemical reactions, atoms
     rearrange, but are not changed,
     created, or destroyed.

5.   When different elements combine,
     they do so in some ratio of whole
     numbers.
Chapter 3




    Structure of Atoms
Atomic dessert

 In 1897 J.J. Thomson was able to control
  light in a vacuum through the use of
  magnets.
 He concluded that the charge of the
  beam was negative.
 He also new that the charge was due to
  movement of something inside atoms
 He concluded that atoms contain
  subatomic particles with + and - charges.
SUBSTANCES ARE MADE OF ATOMS
Atomic Dessert

 He created the
 “plum pudding”
 model of the atom

 The Atom was a big
 positive charge, with
 very small particles
 of negative charges
 embedded in it.
SUBSTANCES ARE MADE OF ATOMS
Radioactive Man
 In1907, Ernest
  Rutherford performed
  “The Gold Foil
  Experiment”
Radioactive Man
 Conclusion:  Atoms have a hard, positively
  charged center called a nucleus.
 The center was packed with tiny particles called
  PROTONS.
 Most of the atom is empty space, while the tiny,
  tiny electrons float around outside.
SUBSTANCES ARE MADE OF ATOMS
SUBSTANCES ARE MADE OF ATOMS
Subatomic Particles
                               ATOM
                               ATOM


                    NUCLEUS
                    NUCLEUS                  ELECTRONS
                                             ELECTRONS


   PROTONS
   PROTONS                NEUTRONS
                          NEUTRONS       NNEGATIVE CHARGE
                                           E G A T IV E C H A R G E


    P O S IT IV E
    POSITIVE                  NEUTRAL
                              NEUTRAL
     CHARG E
     CHARGE                   CHARG E
                              CHARGE


Atomic Number                      equal in a
equals the # of...                neutral atom
Elephants and Fleas

Today, we believe that the atom has
 three subatomic parts:

PROTON – positive charge in the
 nucleus
NEUTRON – no charge in the nucleus
ELECTRON – negative charge, orbiting
 the nucleus
Elephants and Fleas

 Atomic Number – number of protons
 Atomic Mass – number of protons +
  number of neutrons

 Whyaren’t electrons added into the
 mass of the atom?
Isotopes

 ISOTOPE     - atoms of the same element
  that have a different number of
  neutrons
 This happens rather frequently, that is
  why the atomic mass on the periodic
  table is not a whole number. It is an
  average of the different isotopes for
  that element.
Chapter 3



    Electron
    Configurations
The not so great “greats”

 Dalton,  Thomson, and Rutherford were
  great men of science, but they had yet
  to understand the atom.
 It wasn’t until Niels Bohr began to think
  about Hydrogen that were started to
  understand how complex an atom
  really is.
SUBSTANCES ARE MADE OF ATOMS
SUBSTANCES ARE MADE OF ATOMS
Bohr: What is it good for?!

 Bohr, using a technique called Line
 Emission Spectrums, saw that electron
 didn’t just fly randomly around the
 nucleus. In fact, they are in distinct
 orbits called ENERGY LEVELS.
SUBSTANCES ARE MADE OF ATOMS
Bohr: What is it good for?!

 Ifyou put energy into an electron, it will
  change energy level into an EXCITED
  STATE. It will eventually drop back
  down to it’s GROUND STATE and give
  off energy in the form of light.
SUBSTANCES ARE MADE OF ATOMS
The colors of chemistry

 Electromagnetic    Spectrum – radiation
  moving at the speed of light ranging
  from low-energy radio waves to high-
  energy cosmic rays; includes visible
  light
 It is often referred to as “light”
 The spectrum is created by the
  “jumping” of electrons between orbits
Visible Spectrum

 The more energy a wave has, the
  higher the frequency
 Red has the lowest frequency,
  therefore it has the lowest energy
 The most energetic color is violet
 ROY G BIV
Electrons are wavicles.

 Bohr model of the atom shows
 electrons orbiting a nucleus.
  –   Electrons are particles

 When  we attempt to observe an
 electron, it changes position
  –   Electrons are waves
De Broglie to the rescue

 In 1924, Louis De
  Broglie suggested
  that electrons do not
  travel in perfect
  orbits, but rather in
  orbitals.
 The resulting image
  was an “electron
  cloud.”
SUBSTANCES ARE MADE OF ATOMS
Electron Configuration Rules

 Takenotes on Hog Hilton and work on
 board.

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SUBSTANCES ARE MADE OF ATOMS

  • 1. Chapter 3 QBA Miguel A. Castro R. Substances are made of atoms
  • 2. Natural Philosophy  Heraclitus versus Parmenides  Heraclitus– everything is in the process of change  Parmenides – Change is impossible
  • 3. Natural Philosophy  In400 BCE, Democritus stated, All matter consists of tiny particles called átomos, which are not created and cannot be destroyed.  This was the beginning of the atomism.
  • 4. Natural Philosophy  The fight wasn’t over. Plato disagreed.  He thought that the beauty of the world had to be caused by more than mere atoms.  He proposed a system of changing elements; water, fire, earth, air.
  • 5. Natural Philosophy  Aristotle disagreed with both Democritus and Plato. He proposed a system called Hylomorphism.  Hylomorphism is a system of ever changing states of matter.
  • 6. Natural Philosophy  Atomism was lost until the 16th Century  Though it was still not a hard science, it was part of a belief system called alchemy.  Thankfully, Robert Boyle put an end to the mess when he wrote The Skeptical Chemyst.
  • 7. “Nature works by means of bodies unseen.” Lucretius
  • 10. Atomic Theory  Threelaws provide supporting evidence of atoms. – Law of Definite Proportions – Law of Conservation of Mass – Law of Multiple Proportions
  • 11. Law of Definite Proportions Every compound is composed of specific elements and whole- number ratios of those elements. Water H20 - 2 Hydrogen: 1 Oxygen
  • 12. Law of Conservation of Mass Matter cannot be create or destroyed by normal physical or chemical processes i.e.- What goes in, must come out!
  • 14. Law of Multiple Proportions The same elements can bond in differing whole-number ratios to form different compounds. Methanol CH3O Ethanol C2H5O
  • 16. Dalton’s Atomic Theory  Itcontained five principles based on current knowledge of atoms.  We have summarized those principles in the following statements:
  • 17. Dalton’s Atomic Theory 1. All matter is made up of tiny indestructible particles called atoms. 2. All atoms of one type (element) have the same mass and properties. 3. Atoms of different types (elements) have different masses and properties.
  • 18. Dalton’s Atomic Theory 4. In Chemical reactions, atoms rearrange, but are not changed, created, or destroyed. 5. When different elements combine, they do so in some ratio of whole numbers.
  • 19. Chapter 3 Structure of Atoms
  • 20. Atomic dessert  In 1897 J.J. Thomson was able to control light in a vacuum through the use of magnets.  He concluded that the charge of the beam was negative.  He also new that the charge was due to movement of something inside atoms  He concluded that atoms contain subatomic particles with + and - charges.
  • 22. Atomic Dessert  He created the “plum pudding” model of the atom  The Atom was a big positive charge, with very small particles of negative charges embedded in it.
  • 24. Radioactive Man  In1907, Ernest Rutherford performed “The Gold Foil Experiment”
  • 25. Radioactive Man  Conclusion: Atoms have a hard, positively charged center called a nucleus.  The center was packed with tiny particles called PROTONS.  Most of the atom is empty space, while the tiny, tiny electrons float around outside.
  • 28. Subatomic Particles ATOM ATOM NUCLEUS NUCLEUS ELECTRONS ELECTRONS PROTONS PROTONS NEUTRONS NEUTRONS NNEGATIVE CHARGE E G A T IV E C H A R G E P O S IT IV E POSITIVE NEUTRAL NEUTRAL CHARG E CHARGE CHARG E CHARGE Atomic Number equal in a equals the # of... neutral atom
  • 29. Elephants and Fleas Today, we believe that the atom has three subatomic parts: PROTON – positive charge in the nucleus NEUTRON – no charge in the nucleus ELECTRON – negative charge, orbiting the nucleus
  • 30. Elephants and Fleas  Atomic Number – number of protons  Atomic Mass – number of protons + number of neutrons  Whyaren’t electrons added into the mass of the atom?
  • 31. Isotopes  ISOTOPE - atoms of the same element that have a different number of neutrons  This happens rather frequently, that is why the atomic mass on the periodic table is not a whole number. It is an average of the different isotopes for that element.
  • 32. Chapter 3 Electron Configurations
  • 33. The not so great “greats”  Dalton, Thomson, and Rutherford were great men of science, but they had yet to understand the atom.  It wasn’t until Niels Bohr began to think about Hydrogen that were started to understand how complex an atom really is.
  • 36. Bohr: What is it good for?!  Bohr, using a technique called Line Emission Spectrums, saw that electron didn’t just fly randomly around the nucleus. In fact, they are in distinct orbits called ENERGY LEVELS.
  • 38. Bohr: What is it good for?!  Ifyou put energy into an electron, it will change energy level into an EXCITED STATE. It will eventually drop back down to it’s GROUND STATE and give off energy in the form of light.
  • 40. The colors of chemistry  Electromagnetic Spectrum – radiation moving at the speed of light ranging from low-energy radio waves to high- energy cosmic rays; includes visible light  It is often referred to as “light”  The spectrum is created by the “jumping” of electrons between orbits
  • 41. Visible Spectrum  The more energy a wave has, the higher the frequency  Red has the lowest frequency, therefore it has the lowest energy  The most energetic color is violet  ROY G BIV
  • 42. Electrons are wavicles.  Bohr model of the atom shows electrons orbiting a nucleus. – Electrons are particles  When we attempt to observe an electron, it changes position – Electrons are waves
  • 43. De Broglie to the rescue  In 1924, Louis De Broglie suggested that electrons do not travel in perfect orbits, but rather in orbitals.  The resulting image was an “electron cloud.”
  • 45. Electron Configuration Rules  Takenotes on Hog Hilton and work on board.