Chapter 3 Atomic Theory. Early Theories 4 elements.
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Transcript of Chapter 3 Atomic Theory. Early Theories 4 elements.
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Chapter 3Atomic Theory
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Early Theories• 4 elements
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Democritus(460 - 370 BC)
• Greek philosopher• Atomos –
indivisible particles
• Atoms are the smallest particle that retains the chemical identity
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The Greeks Used Logic
• The Greeks also believed in a combination of elements to make new things.
• For example: Water and Earth = Mud
• Mud might just seem like a nuisance to us, but back then it was a building material.
• Fire and Earth made Lava.
• If you are curious check out the Little Alchemy app (game) that can be found in Google Apps. It is a fun game.
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Jabir Ibn Haiyan (700? - 803 AD)
• Father of Chemistry
• Practiced Alchemy
• Discovered metals
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Antoine Lavoisier(1743 - 1794)
• Law of Conservation of Matter
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Joseph Louis Proust(1754-1826)
• Law of Constant Composition
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John Dalton (1766 - 1844)
• Atomic Theory
• This was the true start of our modern theory of matter.
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Dalton’s Theory
• Dalton’s ideas were a good start.
• However, we need to look at one of his postulates more closely.
• He stated that “All atoms of the same atom are identical…”
• He didn’t know about isotopes. The neutron wasn’t discovered for another 130 years.
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Atomic Theory
• Elements made of atoms• Atoms are identical of a given
type of element• Atoms neither created nor
destroyed• Compounds have fixed ratio of
atoms
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Ben Franklin (1706-1790)
• Two types of charge positive (+) and negative (-)
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Michael Faraday(1791-1867)
• Atoms are related to electricity
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J.J. Thomson(1856 - 1940)
• Cathode Ray Tube (CRT) stream of electrons
• Plum Pudding Model
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cathode ray tube
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Thomson’s Model
• This lead directly to the idea of electrons and was a major advancement in atomic theory.
• Sometimes this theory is called “Raisins in a Plum Pudding.”
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Robert Millikan(1838-1953)
• Determined charge & mass of electron
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Henri Becquerel(1852 - 1908)
• Uranium exposes film
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Marie (1867-1934) & Pierre Curie (1859-1906)
• Discovered radioactivity elements
• Radioactive decay
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Earnest Rutherford(1871 - 1937)
• Discovered radioactivity particles
• Discovered Nucleus
• Solar system model of atom
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Discovery of particles
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gold foil experiment
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Rutherford’s Gold Foil Experiment
• There are animations on the website so that you can get a better visual of the experiment.
• Rutherford’s experiment was truly a marvel.
• It answered a lot of questions and gave a good framework for future investigations.
• Remember that it was still a theory – there is a long way to go in understanding an atom.
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Early Atomic Theory• At this point, this completes our look at the
early contributors into Atomic Theory and Structure.
• You were given a lot of names, but here are the ones I want you to focus on:
• Democritus, Dalton, Thompson, Rutherford
• When we get to other topics, we will explore a few more of them in detail such as Becquerel and the Curies.
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Study Guide Help
• To assist you in your preparation, take note that I will not be asking much if anything about the following scientists:
• Ben Franklin, Joseph Proust, Michael Faraday
• Robert Millikan, Jabir Ibn Haiyan, and Antoine Lavoisier might get a short question or two on a test or quiz.
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Niels Bohr (1885 – 1962)
• Electrons do not orbit like planets
• Described shells or energy levels
• Quantum theory
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H.G.J. Moseley (1887 - 1915)
• Discovered protons (+) in the nucleus
• Rearranged periodic table
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Sir James Chadwick (1891-1974)
• Discovered neutrons (0) in the nucleus
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Quarks, Quarks, Quarks (1950s – present)
• 6 quarks have been discovered that make up protons and neutrons
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Protons
• Make up the nucleus
• Charge +1.602 x 10 -19C
• Mass = 1.673 x 10 -24g
• Charge +1
• Mass = 1 amu
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Neutrons
• Make up the nucleus
• Charge 0
• Mass = 1.675 x 10 -24g
• Mass = 1 amu
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Electrons
• Occur in electron Clouds
• Charge -1.602 x 10 -19C• Mass = 9.109 x 10 -28g• Charge = -1• Mass = 0 amu
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• Atoms are small but nuclei are smaller
• Diameter of a penny has 810 million copper atoms
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Atomic Number
• Number of protons in an atom• Electrically neutral atoms have the
same number of electrons as protons
• Ions are formed by gaining or losing electrons
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Isotopes• Same number of Protons but
different numbers of neutrons• Mass number is the sum of the
protons and the neutrons• Isotopes have the same chemical
properties• Violates Dalton’s atomic theory
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Masses of Atoms• 1 amu = 1/12 mass of a 12C atom
• 99% Carbon 12C
• 1% Carbon 13C
• Average atomic mass of C is 12.01 amu
• Mass number is for one atom
• Listed as a decimal on the periodic table
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Nuclear Symbol
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Nuclear Reactions• Nuclear reactions involve the nucleus
of the atom
• Radioactivity is the spontaneous emission of radiation from an atom
• Nuclear reactions change elements involved
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Alpha Particle
• Alpha particle
– Helium nucleus with no electrons
– Will bounce off of paper and skin
– +2 charge
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Beta Particle• Beta particle
– High energy electron– Come from the decay
of a neutrons– Will penetrate skin– Blocked by
aluminum and Plexiglass
– -1 charge
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• Gamma Rays
– High energy wave
– No charge
– No mass
– Penetrates skin, damages cells and mutates DNA
– Blocked by lead
Gamma Radiation
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Nuclear Stability• Most elements have a
stable nucleus• A strong nuclear force
holds protons and neutrons together
• Neutrons act as the “glue” holding the protons together
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Nuclear Equations• Scientists use a nuclear equation when
describing radioactive decay
• The mass number and atomic number must add up to be the same on both sides of the equation
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Beta Decay• Beta decay results in an increase in
the atomic number
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Practice• Write the nuclear equation of the
alpha decay of Radon – 226• Write the nuclear equation of the
alpha decay of Gold - 185
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Practice• Write the nuclear equation of the
beta decay of Iodine - 131• Write the nuclear equation of the
beta decay of Sodium - 24
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Chapter 24Applications of Nuclear
Chemistry
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Half Life• Radioisotopes are radioactive
isotopes of elements (not all isotopes are radioactive)
• A half-life is the amount of time it takes for one half of a sample to decay.
• http://lectureonline.cl.msu.edu/~mmp/applist/decay/decay.htm
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Beta Decay of Phosphorous - 32
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Radiocarbon Dating• Carbon - 14 undergoes beta decay• Half life of 5,730 years• Used to approximate ages 100 –
30,000 years• Other radioisotopes are used to
measure longer periods of time
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Parent Daughter Half Change in...
Carbon-14 Nitrogen-14 5730 years
Uranium-235 Lead-207 704 million years
Uranium-238 Lead-206 4,470 million years
Potassium-40 Argon-40 1,280 million years
Thorium-232 Lead-208 14,010 million years
Rubidium-87 Strontium-87 48,800 million years
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Nuclear Bombardment• Nuclear scientists make nuclei
unstable by being bombarded with particles
• Also known as particle accelerators or “atom smashers”
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Radiation• SI units are in Curies (Ci)• One Curies is amount of nuclear
disintegrations per second from one gram of radium
• Also measured in rem (Roentgen equivalent for man
• Over 1000 rem is fatal• Detected by a Geiger counter
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Nuclear Power• Nuclear Reactors use fission of Uranium-
235 as source of energy• A large nucleus is split into two smaller
nuclei• A small amount of mass is converted to a
tremendous amount of energy• ~1 lb Uranium 235 = 1 million gallons of
gasoline• http://people.howstuffworks.com/nuclear-power2.htm
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Nuclear Fusion
• 2 atomic nuclei fuse releasing a tremendous amount of energy
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Nuclear Weapons• Source of
energy is Plutonium or Hydrogen
• Can be fusion or fission
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Gun-triggered fission bomb (Little Boy - Hiroshima),
Implosion-triggered fission bomb (Fat Man - Nagasaki),
http://people.howstuffworks.com/nuclear-bomb5.htm