2. Orbital's ___________ - are areas around the nucleus that contain electrons. Depicted as rings.

3. Valence Electrons The valence electrons are the electrons in the last shell or energy level of an atom. Valence electrons

4. Rules for Orbital's Electrons must fill the orbital closest to the nucleus before moving to the next one Each orbital holds a specific number of electrons e- Orbital 1: Orbital 2: Orbital 3: Orbital 4: Orbital 5:

5. Atoms to Draw

6. Friday Feb. 3, 2012 Objectives: IWBAT know the periodic Table. Agenda: Catalyst Periodic Table Independent Practice Homework: Topic for the science fair Research your topic HW2 Catalyst Draw a Lewis Dot Structure for the followings: Ca Ar Na

7. Mike Turner, Jan. 2004 Elements, Molecules and Compounds Some elements, such as the noble gases, exist as individual atoms. Often, elements consist of two or more atoms joined together. We call these molecules. If more than one type of atom is in a molecule, we call it a compound. Click to move on

8. Friday 01/25/13 Objectives: IWBAT show mastery on atomic structure Agenda: Catalyst Collecting HW2 quiz Independent Practice Homework: Binder check Memorize the first 20 elements in PPT Project due Tuesday Catalyst Draw a Lewis Dot Structure for the followings: Ca ; Ar ;Na Write the symbol for the followings: Sulfur Helium Zinc Sliver

9. Monday 01/28/13 Objectives: IWBAT be familiar with periodic table. Agenda: Catalyst Binder check Quiz on the element symbol Periodic table Independent Practice Homework: Project due tomorrow/page 2 Catalyst Write the electron configuration for Oxygen and argon. 2- Write the symbol of the following elements: Sodium, Silver, Iron, Carbon, Oxygen, Hydrogen, Helium, Potassium, & Calcium

10. Elements The elements, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe. Each elements has its own color

11. When a metal is heated in a flame, the flame has a distinctive color. This information was eventually extended to the study of stars because A the color spectra of stars indicate which elements are present. B a red shift in star color indicates stars are moving away. C star color indicates absolute distance. D it allows the observer to determine the size of stars. Think critically

12. The most abundant element in the earth’s crust is oxygen.

13. Periodic Table The periodic table organizes the elements in a particular way. A great deal of information about an element can be gathered from its position in the period table. For example, you can predict with reasonably good accuracy the physical and chemical properties of the element. You can also predict what other elements a particular element will react with chemically. Understanding the organization and plan of the periodic table will help you obtain basic information about each of the 118 known elements.

14. Key to the Periodic Table Elements are organized on the table according to their atomic number, usually found near the top of the square. –The atomic number refers to how many protons an atom of that element has. –For instance, hydrogen has 1 proton, so it’s atomic number is 1. –The atomic number is unique to that element. No two elements have the same atomic number.

15. Mike Turner, Jan. 2004 Arranging the Elements : Metals and Non-Metals Most of the elements are metals. The non-metals are found to the top right of the periodic table. The metals and non-metals are separated by a sort of ‘stair case’. Click to move on

16. Mike Turner, Jan. 2004 Arranging the Elements : Groups and Periods The columns of the periodic table are called Groups. Elements in a group have similar properties. Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 Group 0 Group 1 : Alkali metals Group 2 : Alkaline earth metals Group 7 : Halogens Group 0 : Noble gases Transition metals The horizontal rows are called Periods. Click to move on

17. Metal: Elements that are usually solids at room temperature. Most elements are metals. Non-Metal: Elements in the upper right corner of the periodic Table. Their chemical and physical properties are different from metals. Metalloid: Elements that lie on a diagonal line between the Metals and non-metals. Their chemical and physical properties are intermediate between the two.

18. Periodic Patterns –The chemical behavior of elements is determined by its electron configuration –Energy levels are quantized so roughly correspond to layers of electrons around the nucleus. –Each period begins with a new outer electron shell

19. Elements are arranged: Vertically into Groups Horizontally Into Periods

20. Why?

21. If you looked at one atom of every element in a group you would see…

22. Each atom has the same number of electrons in it’s outermost shell. An example…

23. The group 2 atoms all have 2 electrons in their outer shells Be (Beryllium) Atom Mg (Magnesium) Atom

24. The number of outer or “valence” electrons in an atom effects the way an atom bonds. The way an atom bonds determines many properties of the element. This is why elements within a group usually have similar properties.

25. If you looked at an atom from each element in a period you would see…

26. Each atom has the same number of electron holding shells. An example…

27. The period 4 atoms each have 4 electron containing shells K (Potassium) Atom Fe (Iron) Atom Kr (Krypton) Atom 4 th Shell

28. Each group has distinct properties The periodic Table is divided into several groups based on the properties of different atoms.

29. Alkali Metals Soft, silvery colored metals Very reactive!!! http://www.lyon. edu/webdata/U sers/DMcDowel l/GenChem/alka lishow.html

30. Alkali Metals reacting with water: Li (Lithium) Na (Sodium) K (Potassium) Rb (Rubidium) Cs (Cesium) What would you expect from Francium?!?!

31. Alkaline Earth Metals Silvery-White Metals Fairly reactive Many are found in rocks in the earth’s crust

32. Transition Metals Malleable (easily bent/hammered into wires or sheets) Most are good Conductors of electricity

33. How many things can you think of that have Transition Metals in them?

35. Metalloids lie on either side of these “stairsteps” They share properties with both metals and non-metals Si (Silicon) and Ge (Germanium) are very important “semi-conductors”

36. What are semiconductors used in?

37. Nonmetals Brittle Do not conduct electricity

38. Most are Poisonous Fairly reactive Halogens

39. Chlorine Gas was used as a chemical weapon during World War I. It was used by the Nazis in World War II.

40. Unreactive Gases at room temperature Noble Gases

41. Jellyfish lamps made with noble gases artist- Eric EhlenbergerEric Ehlenberger

42. Colors Noble Gases produce in lamp tubes: Ne (Neon): orange-red Hg (Mercury): light blue Ar (Argon): pale lavender He (Helium): pale peach Kr (Krypton): pale silver Xe (Xenon): pale, deep blue

43. Lanthanide Series Actinide Series

44. http://www.bookrags.com/periodictable/

45. Quiz The symbol Au represents which element on the periodic table? A. silver B. gold C. mercury D the element of surprise

46. Exit Slip 1- Write the symbol of the following elements: Sodium, Silver, Iron, Carbon, Oxygen, Hydrogen, Helium, Potassium, & Calcium What is the name of group 1A, 2A,8A