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Understanding the Organization of the Periodic Table

This lesson focuses on the structure of the periodic table, explaining the terminology used in its organization. The rows of the periodic table are referred to as periods, while the columns are known as groups. Each element is represented by its symbol, and their arrangement is determined by the atomic number, which signifies the number of protons. This arrangement reveals patterns in elemental properties. Additionally, we explore the concepts of ions, isotopes, atomic number, mass number, and atomic mass units, enhancing our understanding of atomic structure and interactions.

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Understanding the Organization of the Periodic Table

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  1. DAILY QUESTION October 2, 2008 • The rows on the periodic table are called _________. • The columns on the periodic table are called__________.

  2. Agenda 10/2/08 • Daily Question • Chapter 4 Section 2 Notes Assignments: 1. No assignment tonight.

  3. Organization of the Periodic Table (pg. 111) • Groups similar elements together • Elements are represented by their symbols • Order is based on the number of protons (The Atomic Number of the atom) • Hydrogen has 1 proton, so it is first in the table

  4. Periodic Law • Order of periodic table is based on this • States: when elements are arranged by the number of protons, similarities in their properties will occur in a regular pattern

  5. Periods • Horizontal rows in the periodic table • Can determine the number of electrons based on the element’s location

  6. Groups • Columns in the periodic table • Atoms of elements in the same group have the same number of valence electrons; therefore they have similar properties

  7. Ions • Atoms that have a net electric charge • Have either lost or gained electrons • Cation = a positive ion (lost electrons) • Anion = a negative ion (gained electrons)

  8. Ions continued • Having just 1 valence electron makes the atom highly reactive • Having a full energy level makes the atom less reactive

  9. Atomic Number • Atomic # = # of protons of an atom • In a “happy atom”, it also = # of electrons • Each element has a different atomic number • Atomic number never changes

  10. Mass Number • Mass number = # of protons + # of neutrons • Elements can have a different mass # • Isotopes of an atom

  11. Isotopes • An atom with the original number of protons and electrons, but a different number of neutrons (Therefore a different mass number) • Example: Hydrogen Isotopes: Protium, Deuterium, and Tritium

  12. Calculating the # of Neutrons in an Atom • # of neutrons = mass # – atomic #

  13. Atomic Mass Unit (amu) • Is equal to one-twelfth of the mass of a carbon-12 atom

  14. Average Atomic Mass • A weighted average of the isotopes, so the more commonly found isotopes have a greater effect on the average than rare isotopes

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