Elements Atoms and Nuclear Discovery of Atom & Atom Structure Periodic table and trends Electrons Fission and Fusion Isotopes and Nuclear Decay

Elements Look for these: Here’s the BIG Picture Topic When The Good Stuff Homework Discovery & Atom Class 1 Building an atom Proof of electrons Organizing the Elements Crash Course Chem ∞ Dissecting the PT ∞ Read 6.1-6.2 pp155-167, do 6.1-6.2 Odds Periodic Trends Class 2 Electron Arrangements Class 3 Reinforcement Small Scale Lab/Other Look for these: Most Important Real World Evidence

Elements Atoms and Nuclear Discovery of Atom & Atom Structure Periodic table and trends Electrons Fission and Fusion Isotopes and Nuclear Decay

What is an isotope? Not every atom is exactly the same We know that different elements have different number of protons. However even atoms of the same element are not exactly the same. Atoms of the same element can have different number of neutrons. These are called Isotopes.

It’s all about the Mass Number Because Isotopes differ in their number of neutrons, the mass of the atom also changes. Isotopes are identified by their mass numbers. Remember, mass number is the sum of what two particles? Protons and Neutrons!

1 Proton 1 Proton 1 Proton 0 Neutrons 1 Neutron 2 Neutrons Mass # = 1 Mass # = 2 Mass # = 3

Isotopic Notation Isotopic Notation is generally how isotopes are written. Mass number on top Atomic number on bottom This format makes it easy to calculate number of Neutrons How do we calculate neutrons?

Isotopes have different mass numbers and also different numbers of neutrons. Mass Number – Atomic Number = Neutrons

Identify the number of Protons, Neutrons, and Electrons for each of the following: A) Carbon-12 B) Carbon-14 C) 104Be D) Phosphorus-32

Radioactive Isotopes and Half Life

What is a Radioactive Isotope? What is Radioactive Decay? What is Half Life?

Radioactive Isotopes Radioactive elements are unstable. They decay, and change into different elements over time. Not all elements are radioactive. Those that are listed below are the most useful for geologic dating of fossils are: U-238 Half-life = 4.5 Billion Years K-40 Half-life = 1.25 Billion Years C-14 Half-life = 5, 730 Years

Radioactive Decay and Half Life Here are some facts to remember: The half-life of an element is the time it takes for half of the material you started with to decay. 2. Each element has it’s own half-life.

Radioactive Decay and Half Life Each element decays into a new element - C14 decays into N14 4. The half-life of each element is constant. It’s like a clock keeping perfect time. Now let’s see how we can use half-life to determine the age of a rock, fossil or other artifact.

The blue grid below represents a quantity of C14. Each time you click, one half-life goes by and turns red. C14 – blue N14 - red Half lives % C14 %N14 Time elapsed 100% 0% 0 years As we begin notice that no time has gone by and that 100% of the material is C14

The grid below represents a quantity of C14. Each time you click, one half-life goes by and you see red. C14 – blue N14 - red Half lives % C14 %N14 Time Elapsed 100% 0% 0 years 1 50% 5,730 years After 1 half-life (5730 years), 50% of the C14 has decayed into N14. The ratio of C14 to N14 is 1:1. There are equal amounts of the 2 elements.

The blue grid below represents a quantity of C14. Each time you click, one half-life goes by and you see red . C14 – blue N14 - red Half lives % C14 %N14 Time Elapsed 100% 0% 0 years 1 50% 5,730 years 2 25% 75% 11,460 years Now 2 half-lives have gone by for a total of 11,460 years. Half of the C14 that was present at the end of half-life #1 has now decayed to N14. Notice the C:N ratio. It will be useful later.

The blue grid below represents a quantity of C14. Each time you click, one half-life goes by and you see red. C14 – blue N14 - red Half lives % C14 %N14 Time Elapsed 100% 0% 0 years 1 50% 5,730 years 2 25% 75% 11,460 years 3 12.5% 87.5% 17,190 years After 3 half-lives (17,190 years) only 12.5% of the original C14 remains. For each half-life period half of the material present decays. And again, notice the ratio, 1:7

Band of Stability Stable, naturally occurring isotopes For low atomic numbers the stable nuclei are those with a ratio of protons to neutrons approx. 1:1 As the atomic # increases, the stable ratio increases to about 1.5: 1. 1

Band of Stability Stable, naturally occurring isotopes If an isotope falls above the band, then it needs to lose neutrons and gain more protons to become stable. How would it achieve that? If an isotope had too many protons and too many neutrons, how would it become stable? Alpha Decay Beta Decay Positron Emission 1

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