1. Chapter 6 notes The Periodic Table

2. Dobereiner – attempted to classify the elements in 1817. Triad – three elements with similar properties The middle element has an atomic mass about halfway between the other two.

3. Newlands in 1863 arranged the elements in order of increasing atomic masses Appeared to be a repetition every eighth element 7 elements into 7 groups Law of Octaves

4. Mendeleev – properties of elements were a function of atomic masses Left blank spots Correctly predicted properties and masses of unknown elements Mendeleev, the “Father of the periodic table”

5. Moseley– Found atomic number and problem solved!!! Periodic Law – properties of the elements are a periodic function of their atomic numbers Periodic table from 1930 This is how our table is organized today

6. Periodic Table Groups or families are columns that have elements with the same number of valence electrons Periods or series are rows on the chart. The properties vary. 8 main groups Transition elements Rare earth elements

7. Metals Tend to Lose electrons General rule–3 or fewer electrons in the outer level Left side of table Alkali metals group 1 Alkali earth metals group 2

8. Nonmetals tend to Gain electrons 5 or more electrons in the outer level Right on the table Halogens and Noble gases

9. Metalloids Have properties of both metals and nonmetals Located on ladder like line on table (not Al)

10. Examples of periodic law Metallic vs. nonmetallic character Size of atoms

11. Periodic Table Each time a new energy level is started, a new row in the table begins

12. Transition elements – inner building Columns 3-12

13. Lanthanoid series Z = 57 to Z = 70 2 electrons in outer level 4f sublevel

14. Actinoid Series Z = 89 to Z = 102 5f sublevel

16. Ionization Energy To form a cation (a positively charged ion) an electron must be removed from the atom Ionization Energy—the energy needed to remove an electron from a gaseous atom A higher ionization energy means that an atom likes to hold onto its valence electrons Group 1 elements (Li, Na, K, Rb) have low ionization energies, while the noble gases (He, Ne, Ar, Kr, Xe) have high ionization energies

17. Ionization Energy After removing one electron, it is possible to remove another. This is called second ionization energy. Each successive removal of an electron has a higher ionization energy.

18. Ionization Energy Trends: –Within a period: ionization energies generally increase across a row. –Within a group: ionization energies generally decrease down the columns. Octet Rule: atoms tend to gain, lose, or share electrons to get a full set of 8 electrons

19. Electronegativity Liking for electrons when bonded