Week 2: Isotopes and Stellar Fusion. Part 1: Isotopes Part 2: Nucleosynthesis in Stars
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1 Week 2: Isotopes and Stellar Fusion Part 1: Isotopes Part 2: Nucleosynthesis in Stars
2 Part 1: Isotopes
3 Part 1: Isotopes After this lesson I can define isotopes. determine the number of protons & neutrons in isotopes. Write isotope names and symbols when given the number of protons and neutrons in an atom. explain & define the natural abundance of isotopes and how it is used to determine average atomic mass (students are not expected to calculate average atomic mass)
4 Isotopes Earlier it was noted that the number of protons in an atom s nucleus determines what element that atom is, but atoms can have a different number of neutrons and still be the same element. An isotope is the type or version of an element and is determined by the number of neutrons. Isotopes are different atoms of the same element. Isotopes have a mass number which indicates the total number of protons & neutrons. If the isotope is given by name, the mass number is written after the dash. If the isotope is given by symbol, the mass number is written as a superscript to the left of the symbol. Isotope examples: Carbon-12 = (6 protons, 6 neutrons) = 12 C Carbon-13 = (6 protons, 7 neutrons) = 13 C Carbon-14 = (6 protons, 8 neutrons) = 14 C
5 Additional Examples of Isotopes Nitrogen-14 = (7 proton, 7 neutrons) = 14 N Nitrogen-15 = (7 protons,8 neutrons) 15 N Oxygen-15 = (8 protons, 7 neutrons) = 15 O Oxygen-16 = (8 protons, 8 neutrons) = 16 O Oxygen-17 = (8 protons, 9 neutrons) = 17 O Krypton 71 = (36 protons, 35 neutrons) = 71 Kr Krypton 74 = (36 protons, 38 neutrons) = 74 Kr Krypton 76 = (36 protons, 40 neutrons) = 76 Kr Note that Nitrogen-15 & Oxygen-15 have the same mass number but are different isotopes and different elements.
6 Stable Isotopes of Carbon w/ Percent Abundance Image Credit: wordpress.mrreid.org/2011/03/23/potassium-iodide-pills-are-radioactive/
7 Two Isotopes of Iodine Image Credit
8 Further Examples of Isotopes Image Credit: kaffee.50webs.com/science/activities/chem/activity.isotopes.table.htm
9 Practice Problems: Isotopes and Mass Numbers Directions: Write the Number of Protons & Neutrons for each Isotope below... 1) 25 Al 2) 33 P 3) Silver ) Uranium ) 181 Au 6) 30 S 7) 122 Xe 8) Beryllium -9 9) 4 He 10) Nickel ) 56 Fe 12) 38 Ar 13) 73 As 14) Tellurium - 134
10 Practice Problems: Isotopes and Mass Numbers Directions: Write the Isotope Symbol and Isotope Name for the given atom 1) 15 protons, 16 neutrons 2) 27 protons, 32 neutrons 3) 79 protons, 100 neutrons 4) 79 protons, 102 neutrons 5) 31 protons, 36 neutrons 6) 8 protons, 8 neutrons 7) 100 protons, 165 neutrons 8) 78 protons, 99 neutrons 9) 34 protons, 42 neutrons
11 Natural Abundance Some isotopes are more common than others. For example 98.9% of all carbon atoms on planet earth are Carbon-12, only 1% are Carbon-13, & less than.1% are Carbon-14. The percentage of an isotope for a given element as it naturally occurs on earth is called it s natural abundance or percent abundance. Most elements have at least 2 isotopes that occur naturally, some have just 1, other have 5 or more. 10 is the highest (Tin if your curious) The natural abundance for the isotopes of any given element are available in tables on the internet.
12 Natural Abundance Examples Magnesium Magensium-24 = 79% Magnesium-25 = 10% Magnesium-26 = 11% Chromium 50 Cr = 4.3% 52 Cr = 83.7% 53 Cr = 9.5% 54 Cr = 2.5% Cobalt Cobalt-59 = 100% Bromine 79 Br = 50.7% 81 Br = 49.3%
13 Natural Abundance determines Average Atomic Mass For those of you wondering what the number below the element symbol on your periodic table means, it s entirely related to the naturally occurring isotopes of an element. The average atomic mass of an element is the average mass of the naturally occurring isotopes. The percent abundance figures into the average, just like your final exam counts for 20% of your final grade. An isotope that only accounts for 20% of the naturally occurring isotopes of an element would only count for 20% of the average atomic mass.
14 Average Atomic Mass Examples Magnesium and Bromine Magensium-24: natural abundance is 79% (24.79 = 18.96) Magnesium-25 = natural abundance is 10% (25.10 = 2.50) Magnesium-26 = natural abundance is 11% (26.11 = 2.86) = Average Atomic Mass of Mg Bromine 79 = natural abundance is 50.7% ( = 40.05) Bromine 81 = natural abundance is 49.3% ( = 39.93) = Average Atomic Mass of Br
15 Video! Show the Video: CCC #1 - The Nucleus Note: Start at around 7:40 and play till the end Video Credit:
16 Part 1 Additional Resources Tyler Dewitt s Youtube Video on Isotopes Tyler Dewitt s Youtube Video on Isotope Practice Problems Isotopes interactive simulator program from the University of Colorado.
17 Part 2: Nucleosynthesis in Stars
18 Part 2: Nucleosythensis in Stars After this lesson I can explain fusion inside of stars. explain stellar equilibrium. Categorize elements on the periodic table as being in 1 of 3 categories: 1) Left over from the big bang 2) Formed during the lifespan of small to large stars 3) Formed in supernovae explosions Draw a model of nuclear fusion inside the sun and annotate it, Draw a model of a given step in the nucleosynthesis of an element when provided the equation.
19 A Brief History of the Universe The universe began 13.4 Billions years ago, in a massive expansion of space and time and called the Big Bang. How do we know this? 3 reason you might get: There are no stars in the universe older than 13 billion years. This is despite the fact that certain types of stars we have observed can live to be 100 billion years old or older. Cosmic Background radiation is the heat that is still left over from the big bang and we can see it with special cameras just like we use infrared cameras to see living things at night. We know the universe is expanding because we see galaxies getting farther apart from each other. We can observe this using the same type of doppler radar you often hear about on the news. If it s expanding now, it stands to reason that they were together at some point in the past.
20 Timeline of the Universe Image Credit:
21 Video! Show the Video: The Green s on the Big Bang Video Credit: Crash Course
22 Fusion The early universe was composed almost entirely of Hydrogen, in addition to some very small amounts of Helium & Lithium. None of the other elements on the periodic table existed in the early universe. The process by which the larger elements on the periodic table were (and still are) created is called fusion. Fusion is when two or more atoms fuse together to form one larger atom. Through Fusion inside of stars, almost all of the other elements on the periodic table are created. First hydrogen is combined to make helium, then two heliums combine to make Beryllium, and so forth Fusion is a type of nuclear change, because the nucleus of the atom is changing. When studying any type of nuclear change, the electrons are ignored. In fact fusion happens inside the very center of stars where it s so hot that the electrons separate from the rest of the atom.
23 Model of Step 3 for Fusion inside the Sun Image Credit: Image credit: clipart.dk.co.uk
24 Model of Step 3 for Fusion inside the Sun Image Credit: Wikipedia
25 Videos! Show the Video: Fusion & Atoms Show the Video: Life and Death of a Star
26 Stellar Fusion The concept behind fusion inside of stars is simple but the step-wise process by which elements are created gets more and more complicated as you move up in the atomic number. To make things even more complicated, sometimes more than one pathway is taken to form an Isotope! Here is one set of steps for the formation of Helium-4. These are some of the most common reactions in our sun. Step 1: 1 H + 1 H 2 H (this step also happens twice) Step 2: 2 H + 1 H 3 He (this step also happens twice) Step 3: 3 He + 3 He 4 He + 1 H + 1 H A couple of things to note about the equations above: Protons turn into neutrons Types of radiation like gamma rays and positrons are produced by these reactions but left out of the equation for simplicity These reactions release a tremendous amount of energy. Just 1 gram of 1 H could power 250,000 homes for an entire day!
27 Model Showing All Three Steps for Fusion inside the Sun Image Credit: Wikipedia
28 Part 2 Additional Resources Reading from the American Chemical Society Where do the elements come from Crash Course Big History Video: #1 The Big Bang
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