1. Nucleons
Protons: +1 each, determines identity of element, mass of 1 amu, determined using atomic number, nuclear charge
Neutrons: no charge, determines identity of isotope of an element, 1 amu, determined using mass number - atomic number (amu = atomic mass unit)
3216S and 3316S are both isotopes of S
S-32 has 16 protons and 16 neutrons
S-33 has 16 protons and 17 neutrons
All atoms of S have a nuclear charge of +16 due to the 16 protons.

3. Isotopes
Atoms of the same element MUST have the same number of protons.
Atoms of the same element can vary in their numbers of neutrons. therefore have different atomic masses and are called isotopes.
The atomic mass on the Periodic Table is the weight-average atomic mass, taking into account the different isotope masses and their relative abundance.
Rounding off the atomic mass on the Periodic Table will tell you what the most common isotope of that element is.

4. Weight-Average Relative Atomic Mass
RAM = ((% A of A/100) X Mass of A) + ((% A of B/100) X Mass of B) + …
What is the RAM if its isotope masses and abundances are:
X-200: Mass = amu, % abundance = 20.0 %
X-204: Mass = amu, % abundance = 80.0%
ANSWER: (from X-204) + 40 = g/mol
amu = atomic mass unit (1.66 × kilograms/amu) , thus FACT: one atomic mass unit (1.66 × kilograms) is defined as 1/12 of the mass of an atom of C-12.

5. Natural Radioactivity
Isotopes of atoms with unstable nuclei are called radioisotopes.
Unstable nuclei emit radiation to attain more stable atomic configurations in a process called radioactive decay.
The three most common types of radiation are alpha, beta, and gamma.

6. Alpha Decay
Alpha radiation is not very penetrating—a single sheet of paper will stop an alpha particle.

7. Balancing Equations Alpha Decay

8. Beta Decay
Beta radiation is a stream of fast moving particles with greater penetrating power—a thin sheet of foil will stop them.

9. Gamma Decay
The nucleus has energy levels just like electrons, but the involve a lot more energy.
When the nucleus becomes more stable, a gamma ray may be released.
This is a photon of high-energy light, and has no mass or charge.
Gamma rays are highly penetrating because they have no charge and no mass.

10. Beta Decay

11. Positron Decay Positron decay is like a mirror image of beta decay.
A proton is converted into a neutron and a positron, thus the
Atomic Number goes down.
Since the proton becomes a neutron and they weigh approx same,
the mass stays same
The positron is ejected by the nucleus.

12. Positron Decay

13. Band of Stability All radioactive nuclei are found outside the band
Atoms can undergo different types of decay—beta decay, alpha decay, and positron emission.
At close distances, a strong nuclear force exists between nucleons. This attractive force comes from the neutrons.
More protons in the nucleus need more neutrons to bind the nucleus together.
 1:1 is stable only below Z=20
Uranium-238  has the one of the highest N/Z ratios d 1.596, respectively, 

14. Going Forwards in Time
A half-life is the time required for one-half of a radioisotope to decay into its products.
How many grams of a 10.0 gram sample of I-131 (half-life of 8 days) will remain in 24 days?
#HL = 24/8 = 3
Cut 10.0g in half 3 times: 5.00, 2.50, 1.25g

15. Going Backwards in Time
How many grams of a 10.0 gram sample of I-131 (half-life of 8 days) would there have been 24 days ago?
#HL = t/T = 24/8 = 3
Double 10.0g 3 times: 20.0, 40.0, 80.0 g

16. Radioactive Dating
A sample of an ancient scroll contains 50% of the original steady-state concentration of C-14. How old is the scroll?
50% = 1 HL
1 HL X 5730 y/HL = 5730y

17. Nuclear Transmutation
New elements or isotopes can be created by adding particles to elements or splitting atoms.
These are generally done using particle accelerators.
These speed particles at each other near the speed of light to overcome electrostatic repulsion.

18. Nuclear Transmutation
Most of the “artificial elements” have been created by adding particles to large atoms. Cf 98 C 6 Rf
104 4N
Californium
Carbon
Rutherfordium
249 12
257

19. Magnets Are Used to Move Particles

20. Fusion The combination of two smaller atoms into one larger one.
Hydrogen
Helium
Lithium
Beryllium
The combination of two smaller atoms into one larger one.

21. Fusion Makes Larger Elements

22. Fusion is Hard!
Because the protons repel each other, getting two atoms close enough to fuse is hard.
It takes temperatures approaching 10 million degrees to have them travel fast enough to overcome the electrostatic repulsion

23. Strong Nuclear Force It only acts within the nucleus
Fusion can only occur if protons are brought within the nucleus.
One approach is to shoot particles at each other at near the speed of light.

24. Fusion Releases Energy
When fusion occurs, some of the matter is converted to energy and that energy is released as heat.

25. Stars are Element Makers
Medium stars like our sun mostly convert
Hydrogen to Helium.
Later, it will convert Helium to Carbon.
Giant stars can fuse higher atoms to larger elements.

26. Human Induced Fusion
Hydrogen Bomb

27. Fission When an atom splits into two smaller atoms.
The release of the strong nuclear force releases energy in the form of heat.