2. Learning Target: Classify elements according to their location on the Periodic Table

3.  Identify the following as being an alkalai metal, alkaline earth metal, transition metal, semi-conductor, halogen, or noble gas:  Germanium  Tungsten  Potassium  Radon  Strontium  Uranium  Silicon  Beryllium  Palladium

4.  Which of the following are main-group elements?  Magnesium  Vanadium  Antimony  Lead  Neptunium  Cesium  Rutherfordium  Boron  Indium

7. Section 1: Who’s Who??? Learning Target: Explain the development of Periodic Law

8.  1817 – Dobereiner Grouped elements in TRIADS… Three elements with similar properties  1865 – Newlands Arranged by increasing atomic MASS. Law of Octaves = Similar properties over EIGHT elements

9.  1870 – Mendeleev Created an 8 Column table based on ATOMIC MASS Elements with similar properties were in the same column

10. Problems w/ Mendeleev’s table: 1. Some elements did not fit the order. Ex: Tellurium (Te) and Iodine (I) 2. There were gaps in the table BUT he was able to predict the properties and masses of the unknown elements very accurately.

12.  1913 – Mosley Studied X-ray spectra of elements and noticed they correlated with atomic number Arranged elements with increasing ATOMIC NUMBER  PERIODIC LAW: Properties of the elements are a (periodic) function of their atomic number

13.  1944 –Glenn Seaborg  Last rearrangement of the periodic table – created the actinide series

14. Dobereiner Triads Newlands Law of Octaves Mendeleev First 8 column table Mosley Periodic Law 1817 1913187018651944 Seaborg Actinide Series

15. Section 2

17.  Atomic properties are determined by ELECTRON CONFIGURATION.  Ex. 1s 2 2s 2 2p 6 3s 2 3p 3  Therefore…the table is designed on the basis of electron configuration…

18.  Valence Electrons: Electrons that are found in an atom’s outer most shell  Determines chemical properties of an atom  These are the electrons that can be gained, lost or shared when forming compounds

21.  OCTET RULE… 8 electrons in the outer energy level renders an atom UNREACTIVE Unreactive = Very Stable So…which elements are considered unreactive?

22. A: The Noble Gases

23.  Atoms react with other atoms so all atoms end up with FULL OUTER ENERGY LEVELS (i.e. compounds) 1. They may add electrons 2. They may lose electrons 3. They may share electrons

24. Section 3 Learning Target: Identify properties of metals, nonmetals and metalloids

25.  Don’t forget your color-coded periodic table…  It identifies the… Groups Periods Main Group Elements

26.  It also classifies elements as… Metals:  Alkali metals  Alkaline Earth metals  Transition metals  Lanthanide Series  Actinide Series  Other Metals Nonmetals:  Noble gases  Halogens  Other nonmetals Metalloids:  semiconductors

27.  Metals –On the LEFT of the stairs  Nonmetals – On the RIGHT of the stairs  Metalloids – Attached to stairs (not shown here)

28. METALSNONMETALS 1. Typically Solids1. Gasses or BRITTLE solids 2. Shiny2. Dull 3. Conduct Heat and Electricity 3. Insulators 4.Tendency when forming compounds to lose outer electrons 4.Tendency when forming compounds to GAIN or SHARE electrons

29. RULE of THUMB  Metals: 3 or fewer outer energy level electrons  Nonmetals: 5 or more outer energy level electrons  Metalloids: Properties of both Metals and Nonmetals Semiconductors

30. Section 4 Learning Target: Describe element trends on the Periodic Table

31.  What is a trend?  A predictable change in a particular direction  (FOCUS ON MAIN GROUP ELEMENTS)

32. Atomic Radii  ½ the distance between the nuclei of identical atoms that are bonded together  Atomic Radii increase from top to bottom and from right to left on the periodic table Radius = d/2

33. Periodic Table Increases

35.  Increases as you move down due to electron shielding electrons in the inner energy levels are between the nucleus and the outer electrons and therefore are shielded from being pulled away

36.  Decrease as you go right due to increasing charge of the nucleus (means increases as you go left due to decreasing charge of nucleus) although more electrons are also present they are at the same distance from the nucleus b/c they are in the same energy level

37.  Gallium  Yttrium  Helium  Hafnium  Thallium  Strontium  Neon  Vanadium

38. Ions  Atom or group of atoms that has a positive or negative charge Positive charge occurs when atom loses electrons Ex: Na + : Sodium that has lost an electron, and now has 10 e - Negative charge occurs when atom gains electrons Ex: Cl - : Chlorine that has gained an electron, and now has 18 e -  This process that results in an ion requires energy—this process is referred to as ionization

39. Ionization Energy  Energy required to remove one electron from a neutral atom of an element This happens when compounds form  Ionization energy tends to increase from bottom to top and left to right

40. Periodic Table Increases

42.  As you move across, the nucleus gets larger and holds the electrons more tightly THEREFORE harder to remove  Requires MORE energy (higher ionization energy)

43.  As you move down, the outer most electrons are farther away from the nucleus THEREFORE easier to remove  Requires LESS energy (lower ionization energy)

44.  Iron  Cesium  Sulfur  Iodine  Cobalt  Rhenium  Tin  Bismuth

45. Electron Affinity  Energy change that occurs when an electron is acquired by a neutral atom (The ability to attract and hold an electron.)  Electron affinity follows the same trend as Ionization Energy (Bottom to Top/Left to Right generally more exothermic)

46. Periodic Table Increases

47.  Gold  Platinum  Barium  Fluorine  Osmium  Cadmium  Beryllium  Aluminum