What do they have in common? - PowerPoint PPT Presentation

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What do they have in common?

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Title: What do they have in common?


1
What do they have in common?
2
Nuclear Chemistry
3
Nuclear Reactions
  • Involve the nucleus
  • Radioactivity is the spontaneous emission of
    radiation from an atom

4
Nuclear Stability
  • Most atoms have a stable nucleus
  • A strong nuclear force holds protons and neutrons
    together
  • Neutrons act as the glue holding the protons
    together

5
Belt of Nuclear Stability
There seems to be a ratio of protons to neutrons
that increase the chances that an atom will be
stable.
Figure 18.1 The Zone of Stability
6
Types of Radiation
  • The three main types of nuclear radiation are
    alpha radiation, beta radiation, and gamma
    radiation.

7
Radioactive Particles
  • Alpha particle - Helium nucleus with no
    electrons 2 charge
  • Beta particle - High energy stream of
    electrons -1 charge
  • Gamma Rays - High energy wave which are the
    strongest No charge
  • Refer to the radioactive particle sheet that can
    be found on the website for other particles.

8
A look at Alpha Decay
9
A look at Beta Decay
10
A look at Gamma Decay
11
Penetrating Powers
12
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

13
Balancing Nuclear Equations
  • Heres the equation from the previous slide.
  • The top numbers on the left side of the arrow
    the top numbers on the right side of the arrow.
  • The same holds for the bottom numbers.
  • USE A PERIODIC CHART for the atomic numbers if
    needed.

14
Beta Decay
  • Beta decay results in an increase in the atomic
    number.
  • Notice how the top numbers equal and the bottom
    numbers also equal

15
Nuclear Stability and Decay
For the equations on the right, the atomic
numbers are also shown but in many equations they
are omitted because they can be found on the
periodic chart. For example, carbon is often
written as 14C
16
Practice
  • Write the nuclear equation of the alpha decay of
    Radon 226
  • Write the nuclear equation of the alpha decay of
    Gold 185
  • The number after the element is the mass number.

17
Practice Answers
  • 226Rn ? 4He 222Po
  • 185Au ? 4He 181Ir

18
Practice
  • Write the nuclear equation of the beta decay of
    Iodine - 131
  • Write the nuclear equation of the beta decay of
    Sodium - 24

19
Practice Answers
  • 131I ? -1e-1 131Xe
  • 24Na ? -1e-1 24Mg

20
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.
  • The half-life is different for each element and
    isotope.
  • http//www.colorado.edu/physics/2000/isotopes/radi
    oactive_decay3.html

21
Beta Decay of Phosphorous - 32
Notice that every 14 days, the amount is cut in
half.
22
Radiocarbon Dating
  • Carbon - 14 undergoes beta decay to form stable
    nitrogen 14
  • Half life of 5,730 years
  • Used to approximate ages 100 30,000 years
  • Other radioisotopes are used to measure longer
    periods of time

23
Parent and Daughter Nuclides
  • The term parent nuclide refers to the original
    atom.
  • The term daughter nuclide refers to the particle
    that is produced after the radioactive decay is
    completed.

24
Some examples of Parent Daughter Nuclides
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
25
Practice
  • The half-life of Po-218 is three minutes. How
    much of a 2.0 gram sample remains after 15
    minutes?
  • Remember that the symbol for half life is t1/2

26
Practice Answer
  • It is often best to set up a simple table
    especially if the amount of time is a multiple of
    the half life like in this example.
  • Notice that 15 minutes is a multiple of the 3
    minute half life.
  • The next slide has the table that we need to
    create to solve the problem.

27
Practice Answer Half Life Table
Amount of Material Initially Time elapsed Amount of material remaining
2 grams 0 minutes 2 grams
2 grams 3 minutes 1 gram
1 gram 6 minutes .5 grams
.5 gram 9 minutes .25 grams
.25 grams 12 minutes .125 grams
.125 grams 15 minutes .0625 grams
So after 15 minutes, there is only .0625 grams
left.
28
Practice
  • Three grams of Bismuth-218 decay to 0.375 grams
    in one hour.
  • What is the half-life of this isotope?

29
Practice Answer Half Life Table
We can also create the table going backwards to
answer questions like this one. Notice it is
really a similar table.
Amount of Material Initially Number of half-lives Amount of material remaining
3 grams 1 1.5 grams
1.5 grams 2 .75 grams
.75 grams 3 .375 grams
It took 3 half-lives to get to the amount .375
grams. If 1 hour equals 3 half-lives, then each
half-life must be 20 minutes.
30
More on Half - Life
  • Sometimes the amount of time is not a multiple of
    number of half-lives.
  • We can use the following equation for all
    half-life problems.

31
Nuclear Bombardment
  • Nuclear scientists change elements by bombarding
    the nucleus with particles transmutation
  • 14N 4He ? 17O 1H
  • Leads to the creation of transuranium (after U)
    elements.

32
Transmutation Reactions
  • The first artificial transmutation reaction
    involved bombarding nitrogen gas with alpha
    particles.

33
Fermilab Particle Accelerator







34
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 (E mc)2
  • About 1 kg of Uranium-235 2.2 million gallons
    of gasoline
  • http//people.howstuffworks.com/nuclear-power2.htm

35
Nuclear Fission
  • Nuclear Fission

36
Fission Produces a Chain Reaction
37
Overview of a nuclear power plant
All power plants work on the same principal. It
needs to heat up water to make steam to run a
steam engine which produces the actual
electricity. The only difference between a coal
power plant and a nuclear power plant is that the
first burns coal to heat the water and the second
controls a nuclear reaction to heat the water.
38
Nuclear Power Plants 1
  • A nuclear plant has some differences of
    course compared to a coal burning plant.
  • The fuel is much more costly, though lasts
    much longer.
  • The heat can be controlled easily in a coal
    burning plant by simply controlling how much
    coal is added to the fire.
  • This is the primary difference and the biggest
    safety concern in a nuclear power plant as the
    next slide shows.

39
Nuclear Power Plants 2
  • Uranium fuel cant be removed or limited like a
    coal fired power plant.
  • The heat comes from the chemical reaction of the
    decay of a uranium atom.
  • The atom splits and the chain reaction keeps it
    going.
  • The way to control the heat released is by
    controlling the neutrons released
  • during the chain reaction.
  • This is done by using graphite rods that can be
    raised and lowered which controls the amount of
    neutrons absorbed at any time.

40
Nuclear Power Plants 3
  • This was the primary problem in developing the
  • atomic bomb during World War 2.
  • Both sides knew how to get the fission process of
    the uranium going, but the questions were on how
    to keep it under control so it wouldnt go off
    too early in the lab.
  • There were two teams. One team was working for
    Germany. The other team was a group of mostly
    German scientists who were able to flee Germany
    to the United States and were working for the
    Allied forces.

41
Nuclear Power Plants 4
The team working in Germany focused on using
heavy water to moderate the chain reaction.
Heavy water is regular water but with a
difference in the hydrogen isotope. Regular
water is mostly 1H but heavy water is 2H. This
extra neutron helps to absorb other neutrons and
control the reaction. Regular water is about
.0001 heavy water but the percentage needed is
about 98 so it took time to get enough heavy
water needed.
42
Nuclear Power Plants 5
The allied side, based in the United States
decided to use graphite rods which could be
raised and lowered and absorb the
neutrons. While both were acceptable ways to
moderate the reaction, the Allied side was able
to create the bomb first and force an end to the
war.
43
A Schematic Diagram of a Reactor Core
44
Gun-triggered fission bomb (Little Boy -
Hiroshima)Implosion-triggered fission bomb (Fat
Man - Nagasaki)
http//people.howstuffworks.com/nuclear-bomb5.htm
45







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46
Nuclear Power Plants 6
An interesting side note to all of this is how
nuclear energy in power plants came to be. The
scientists who were working on the bomb were
uneasy with this type of power and the US
government put out a survey to ask how can this
energy source by used peacefully. Some answers
such as to create a new Panama Canal were tossed
aside (too much residual radiation). Suggestions
were that if the reaction can be controlled it
can be used to run steam turbines in power
plants. This led to the start of the nuclear
power plant.
47
A schematic of a nuclear power plant







What the heat from the radioactive process does
is to heat water to run a turbine.
48
Nuclear Fusion
  • Atomic nuclei fuse releasing a tremendous
    amount of energy

49
Nuclear Weapons
  • The bombs dropped in World War 2 were fission
    bombs made of Uranium and getting their energy
    when the Uranium atoms split (fission) into
    smaller atoms.
  • This is called an Atomic Bomb.
  • Since then, the process of taking Hydrogen atoms
    and combining 4 of them to create a Helium atom
    (fusion) has been developed. This creates a more
    powerful bomb.
  • This is called a Nuclear Bomb.

50
Radiation and You
  • 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
  • The next slide gives a glimpse of the radiation
    we receive. NOTE that the units are MILLIREMS,
    which is 1/ 1,000 of a REM.

51
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52
Radon Gas
53
Figure 18.2 A Decay Series
54
Detecting Nuclear Radiation
  • You cannot hear or feel nuclear radiation.
  • Geiger Counter
  • Film badges
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