Introduction To Chemistry Power Point

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Introduction To Chemistry Power Point

  1. 1. Introduction to Chemistry<br />Adam Rohde<br />
  2. 2. Particles<br />Protons: Positively charged particles<br />Neutrons: Neutral particles<br />Electrons: Negatively charged particles<br />
  3. 3. Nucleus<br />Dense center of the atom<br />Positively charged<br />Consists of protons and neutrons<br />Determines what the element is<br />Contains most of the mass<br />
  4. 4. Electron Cloud<br />Orbits the nucleus<br />Consists of electrons<br />Takes up most of the space<br />Does not contribute to atomic mass<br />
  5. 5. Atomic Mass<br />Number of protons and neutrons<br />Atomic mass units (amu)<br />4 protons + 3 neutrons = 7 amu<br />Electrons are not counted<br />
  6. 6. Nuclear Force<br />Protons repel each other<br />Held together by strong nuclear force<br />Have to be extremely close<br />Exchange mesons<br />
  7. 7. Atomic Charges<br />Relative to protons and electrons<br /># of protons &gt; # of electrons: + charge<br /># of electrons &gt; # of protons: - charge<br /># of protons = # of electrons: neutral<br />Neutrons are not counted<br />
  8. 8. Elements<br />Depend on # of protons<br /># of protons decides placement on the periodic table<br />Can have different charges<br />Can have different # of neutrons<br />
  9. 9. Ions<br />Same elements<br />Different charges<br />Hydrogen with 2 electrons: - 1<br />Hydrogen with 1 electron: neutral<br />Hydrogen with 0 electrons: + 1<br />
  10. 10. Isotopes<br />Same element<br />Different masses<br />Hydrogen with 1 neutron: 2 amu<br />Hydrogen with 0 neutrons: 1 amu<br />
  11. 11. Periodic Atomic Mass<br />Mass displayed on the periodic table<br />Average mass of the isotopes<br />Used when determining quantities of molecules<br />
  12. 12. Quantities<br />Mass (grams)<br />Moles<br />Molarity<br />
  13. 13. Avogadro’s Number<br />Used often if chemistry<br />Number of molecules in 1 mole<br />6.022 x 10e23<br />
  14. 14. Moles<br />Can be determined from mass<br />Grams / atomic mass<br />Ex: 28g of N / 14 amu = 2 moles<br />
  15. 15. Molarity<br />Concentration in a solution<br /># of moles / liters of solution<br />Ex: 2 moles of HCl / .5L = 4M<br />
  16. 16. Review<br />Structure of atoms<br />Charges of atoms<br />Mass of atoms<br />Quantities<br />
  17. 17. References<br />ion. (2009). In Merriam-Webster Online Dictionary. Retrieved October 1, 2009, from http://www.merriam-webster.com/dictionary/ion<br />isotope. (2009). In Merriam-Webster Online Dictionary. Retrieved October 1, 2009, from http://www.merriam- webster.com/dictionary/isotope<br />The Strong Nuclear Force. (n.d.). Retrieved October 1, 2009, from http://aether.lbl.gov/elements/ stellar/strong/strong.html<br />Weisstein, E. W. (n.d.). l. Retrieved October 1, 2009, from http://scienceworld.wolfram.com/physics/ AvogadrosNumber.html<br />

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