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Atomic # = # of Protons Atomic Mass = # of Protons + # of Neutrons

17 Cl 35.453. Atomic # = # of Protons Atomic Mass = # of Protons + # of Neutrons Charge = # of Protons - # of electrons. Atomic Mass                    Charge                Element                Symbol Atomic #              # of Atoms. 35   -1    Cl 17       2.

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Atomic # = # of Protons Atomic Mass = # of Protons + # of Neutrons

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  1. 17 Cl 35.453 Atomic # = # of Protons Atomic Mass = # of Protons + # of Neutrons Charge = # of Protons - # of electrons Atomic Mass                    Charge                Element                Symbol Atomic #              # of Atoms 35   -1    Cl 17       2

  2. On line Activity • BUILDING ATOMS AND ISOTOPES • http://www.kscience.co.uk/animations/atom.swf • 1. 31H • 2. 94Be 2+ • 3. 2010 Ne • 4.3517Cl – • 5. 3919 K + • 1) Which of the above are cations?  Which are anions?  Which are neutral atoms? • 2) What is the relationship between mass number and atomic number?  Is this relationship the same for small atoms as it is for larger atoms? • 3) Why does 3919 K + have a positive charge?  Why does 3517Cl–  have a negative charge?

  3. Nuclear video • practice counting protons, neutrons and electrons:http://science.widener.edu/svb/tutorial/protonscsn7.htmltypes of radiation: http://www.glencoe.com/sites/common_assets/science/cmc/cim/animations/ch4_3.swf1/2 life: http://einstein.byu.edu/~masong/HTMstuff/Radioactive2.html & http://www.colorado.edu/physics/2000/isotopes/radioactive_decay3.htmlfission: http://www.kscience.co.uk/animations/fission_final.swffusion: http://www.kscience.co.uk/animations/fusion_final.swf

  4. 17 Cl 35.453 Atomic # = # of Protons Atomic Mass = # of Protons + # of Neutrons Charge = # of Protons - # of electrons Atomic Mass                    Charge                Element                Symbol Atomic #              # of Atoms 35   -1    Cl 17       2

  5. There are three naturally occurring isotopes of carbon on Earth: 99% of the carbon is carbon-12, 1% is carbon-13, and carbon-14 occurs in trace amounts, i.e. making up as much as 1 part per trillion (0.0000000001%) of the carbon in the atmosphere. The half-life of carbon-14 is 5,730±40 years. Carbon-14 decays into nitrogen-14 through beta decay.[3] The primary natural source of carbon-14 on Earth is cosmic ray action upon nitrogen in the atmosphere, and it is therefore a cosmogenic nuclide. However, open-air nuclear testing between 1955-1980 contributed to this pool.

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