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Section 2 – A Guided Tour of the Periodic Table

Section 2 – A Guided Tour of the Periodic Table. Chapter 4 Study Guide. Definitions. Periodic law:. The law stating that repeating chemical and physical properties of elements change periodically with the atomic numbers of the elements. Period:. Horizontal rows of elements. Group:.

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Section 2 – A Guided Tour of the Periodic Table

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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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