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DAILY QUESTION October 2, 2008

DAILY QUESTION October 2, 2008. The rows on the periodic table are called _________. The columns on the periodic table are called__________. Agenda 10/2/08. Daily Question Chapter 4 Section 2 Notes Assignments: 1. No assignment tonight. Organization of the Periodic Table (pg. 111).

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DAILY QUESTION October 2, 2008

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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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