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Chapter 5 Atomic Structure & The Periodic Table

Chapter 5 Atomic Structure & The Periodic Table. Atoms. The smallest particle of an element that retains the properties of that element. Dalton’s Atomic Theory (1808). Each element is made up of tiny particles called atoms. The atoms of a given element are identical .

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Chapter 5 Atomic Structure & The Periodic Table

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  1. Chapter 5 Atomic Structure & The Periodic Table

  2. Atoms • The smallest particle of an element that retains the properties of that element.

  3. Dalton’s Atomic Theory (1808) • Each element is made up of tiny particles called atoms. • The atoms of a given element are identical. • Chemical compounds are formed when atoms combine with each other. • Chemical reactions involve reorganization of the atoms

  4. J. J. Thomson • Cathode Ray Tube • Discovered the electrons • Cathode rays bent towards the positive plate

  5. Deflection of cathode rays by an applied electric field.

  6. Plum Pudding Model of an Atom

  7. A schematic representation of the apparatus Millikan used to determine the charge on the electron.

  8. Rutherford’s Gold Foil Experiment

  9. (a) The expected results of the metal foil experiment if Thomson's model were correct. (b)Actual results.

  10. Building Blocks of Atoms Subatomic particles • Protons, electrons, and neutrons Nucleus • Protons & neutrons Where are the electrons? • They surround the nucleus.

  11. Periodic Table • Atomic Number = # of protons • Element Symbols (1-2 letters) • Groups / Families = columns • Similar properties • Periods = rows

  12. Distinguishing Between Atoms • Atomic # = # protons = # electrons • Isotopes: # of protons remains the same, but # of neutrons vary • Example: 3 isotopes of hydrogen • Protium (0 neutrons) • Deuterium (1 neutron) • Tritium (2 neutrons) • Mass # = protons + neutrons

  13. Two isotopes of sodium.

  14. Mass # A Element Symbol ZX Atomic #

  15. Atomic Mass • Elements occur in nature as mixtures of isotopes • Carbon = 98.89% 12C 1.11% 13C <0.01% 14C • Carbon atomic mass = 12.01 amu

  16. Copper has two naturally occurring isotopes: copper-63 and copper-65 69.17% of copper-63; the mass is 62.94 amu 30.83% of copper-65; the mass is 64.93 amu Calculate the average atomic mass.

  17. Average atomic mass of copper = (.6917 x 62.94 amu) + (.3083 x 64.93 amu) = 63.55 amu

  18. Periodic Table (cont.) • METALS: cover the largest region of the periodic table • Good conductors of heat and electricity, ductile, and malleable • NONMETALS: most of them are gases • Poor conductors of heat and electricity • METALLOIDS: elements that have some properties of metals and nonmetals • NOBLE GASES: extremely unreactive or inert

  19. Classification of elements as metals, nonmetals, and metalloids.

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