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Periodic Table Organization and Atomic Structure Study Guide

Understand the periodic law, atomic numbers, isotopes, ions, and more. Learn how elements are arranged in the periodic table and relate it to electron configurations. Discover why atoms gain or lose electrons to form ions, and how isotopic abundance impacts average atomic mass calculations.

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Periodic Table Organization and Atomic Structure Study Guide

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  1. Section 2 – A Guided Tour of the Periodic Table Chapter 4 Study Guide

  2. Definitions

  3. Periodic law: • The law stating that repeating chemical and physical properties of elements change periodically with the atomic numbers of the elements

  4. Period: • Horizontal rows of elements

  5. Group: • Vertical columns of elements • Elements in the same group have similar properties

  6. Ion: • Atoms that either lose electrons or gain electrons • Have positive or negative charge

  7. Atomic number: • The number of Protons an element has • Determines the sequence of the periodic table

  8. Mass number: • The total number of subatomic particles • Mass # = Protons + Neutrons

  9. Isotope: • Atoms of an element that have different numbers of neutrons • Carbon-12, Carbon-14

  10. Atomic mass unit (amu): • Standard unit of atomic mass, equal to one-twelfth the mass of a Carbon-12 atom

  11. Average atomic mass: • A weighted average of the masses of all naturally occurring isotopes. More common isotopes count more than less common ones.

  12. Questions?

  13. Objecive 1: Relate the organization of the periodic table to the arrangement of electrons in an atom.

  14. Objective 1 • (1) The order of elements in the periodic table is based on the number of protons in the nucleus.

  15. Objective 1 • (2) Atoms of elements that are in the same group have the same number of valence electrons.

  16. Objective 1 • (3) Valence electrons determine an atom’s chemical properties.

  17. Objective 1 • (4) The periodic table organizes elements into groups that have similar properties.

  18. Objective 1 • (5) Magnesium (Mg) is located to the right of sodium (Na) because Mg has more electrons and more protons.

  19. Objective 1 • (6) Elements that have one valence electron tend to be highly reactive, form ions, and become charged.

  20. Objective 1 • (7) The order of elements in the periodic table is based on the number of protons in the nucleus.

  21. Objective 1 • (8) Because atoms of elements in the same group of the periodic table have the same number of valence electrons, they have similar properties.

  22. Objective 1 • (9) The periodic law states that when elements are listed in order of atomic number, similarities in their properties will emerge in a regular pattern.

  23. Questions?

  24. Objective 2: Explain why some atoms gain or lose electrons to form ions.

  25. Objective 2 • (10) Ionization refers to the process of losing or gaining electrons.

  26. Objective 2 • (11) A lithium ion is much less reactive than a lithium atom because it has a full outermost energy level.

  27. Objective 2 • (12) Some elements are highly reactive because their outermost energy levels are only partially filled.

  28. Objective 2 • (13) The valence electron of a lithium atom is easily removed to form a lithium ion or cation with a charge of 1+.

  29. Questions?

  30. Objective 3: Determine how many protons, neutrons, and electrons an atom has, given its symbol, atomic number, and mass number.

  31. Objective 3 • (14) Oxygen’s atomic number is 8. This means that an oxygen atom has eight protons in its nucleus.

  32. Objective 3 • (15) An atom’s mass number equals the number of protons plus the number of neutrons.

  33. Objective 3 • (16) An element’s atomic number is equal to its number of protons.

  34. Objective 3 • (17) Two different isotopes of an element have different number of neutrons.

  35. Objective 3 • (18) The mass number of an element that has 19 protons, 19 electrons, and 20 neutrons is 19 + 20 = 39.

  36. Objective 3 • (19) As you move left to right across the periodic table, elements have more protons and higher mass numbers.

  37. Objective 3 • (20) An iron atom has an atomic mass of 56. Its atomic number is 26. This iron atom has 56 – 26 = 30 neutrons.

  38. Objective 3 • (21) An atom of potassium has an atomic mass of 39 amu and an atomic number of 19. It therefore has 39 – 19 = 20 neutrons in its nucleus.

  39. Questions?

  40. Objective 4: Describe how the abundance of isotopes affects an element’s average atomic mass.

  41. Objective 4 • (22) An element’s average atomic mass is a weighted average, so common isotopes have a greater effect than uncommon ones.

  42. Objective 4 • (23) An atomic mass unit is equal to one-twelfth the mass of a carbon-12 atom.

  43. Objective 4 • (24) More abundant isotopes will have more effect on the average atomic mass of an element.

  44. Objective 4 • (25) An element’s average atomic mass refers to the weighted average of the masses of all of its naturally occurring isotopes.

  45. Objective 4 • (26) Isotopes of an element have the same atomic number but different atomic mass.

  46. Questions?

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