lecture3 - Monday Sept. 8, 2003 Todays Lecture 2.6 Atomic...

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Unformatted text preview: Monday Sept. 8, 2003 Todays Lecture 2.6 Atomic Structure 2.7 Molecules and Ions 2.8 The Periodic table 2.9 Naming Compounds Modern View of Atomic Structure: Chemist perspective: an important feature of an atom is its electrons since they dictate the chemical properties of an element Simple view of an atom: small nucleus ~ 10-13 cm in diameter electron cloud 10-8 cm across Atoms are made of: Mass Charge electrons 9.11 x 10-31 kg-1 protons 1.67 x 10-27 kg +1 neutrons 1.67 x 10-27 kg nucleus is very small and very dense If atoms are made of the same components, why do different atoms have different chemical properties? The chemical properties are due to the # and arrangement of electrons different elements have have different # of p and e- different chemical properties Notation for atoms: X = element symbol (Na, H, He, Li, Cl) A = atomic mass number = # of protons + # of neutrons Z = atomic number = # of protons = # of electrons in a neutral atom A-Z is the # of neutrons Example: X A Z Na 23 11 e- = 11, p = 11, n = 12 Atoms with the same atomic # (Z) but different mass # (A) are called: isotopes Example 1: hydrogen deuterium Tritium Proton # 1 1 1 Neutron # 1 2 Electron # 1 1 1 H H H 3 1 2 1 1 1 Example 2: Proton # 6 6 6 Neutron # 6 7 8 Electron # 6 6 6 C C C 14 6 13 6 12 6 Many Isotopes Exist Pt atomic number 78 mass number 195-33.8% mass number 194- 32.9% mass number 196- 25.3% mass number 198- 7.21% mass number 190- 0.0127% t 1/2 =6x10 11 Tc atomic number 43 no stable isotopes mass numbers- 92, 93, 93m, 94, 94m, 95, 95m, 96, 96m, 97, 97m, 98, 99m, 99, 100, 101, 102, 102m, 103, 104, 105, 106, 107 Atomic Mass Units atomic massed units - amu based the mass of a specific isotope of an element defined as 12 amu for 12 6 C Electrons, Protons and Neutrons...
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lecture3 - Monday Sept. 8, 2003 Todays Lecture 2.6 Atomic...

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