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Ch 4

Ch 4. ATOMIC STRUCTURE. All about the ATOM. The Structure of Atom’s Subatomic Particles. Electrons are TINY compared to a Proton or Neutron. All elements are on the periodic table of elements!. GET OUT YOUR PERIODIC TABLE REFERENCE SHEET. Atomic Number is # of p+ & e- in atom

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Ch 4

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  1. Ch 4 ATOMIC STRUCTURE

  2. All about the ATOM

  3. The Structure of Atom’sSubatomic Particles

  4. Electrons are TINY compared to a Proton or Neutron

  5. All elements are on the periodic table of elements! GET OUT YOUR PERIODIC TABLE REFERENCE SHEET

  6. Atomic Number is # of p+ & e- in atom Atomic Mass # is average of all of isotopes of atom (decimals) Mass number (atomic mass rounded)is sum of the p+ & nO in atom 1 H 1.0079 round 1.0079 to 1, 1 is mass #

  7. A P E M A N To find # of p+, use Atomic # To find # of e-, use Atomic # To find # of no, subtract Atomic # from Mass # (round & subtract) 9 F 18.988 n0= p+= e-=

  8. 16 ____________

  9. Mass # =__________ Mass # = ___________ Mass # = ____________

  10. Isotopes have same atomic # but different mass # b/c they have different #s of neutrons

  11. Different ways to write isotopes: Carbon-12, 126C, C-12 Atomic # Mass #

  12. Sample chart

  13. Neils Bohr model stated e- move w/ constant speed in fixed orbits around the nucleus, like planets orbiting the sun

  14. Bohr Model

  15. The possible energies e- in atom can have are called energy level (orbital, shell) • e- in atom can move from one energy level to another when atom gains or loses e-

  16. Atomic Orbitals & max e- in each orbital

  17. Practice drawing Bohr models

  18. STAR Questions • How many neutrons does Lithium have? • How many electrons can go in the second orbital? • Draw a Bohr model of Al.

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