1. Starter: Atomic Particle Copy and complete the following statements with the following terms you will use one of them twice. Protons, Electrons, Neutrons 1. ___ identify the element. 2. ___ have no charge and mass equal to another particle. 3. ___ have a negative charge and basically no mass. 4. ___ have a positive charge and mass equal to another particle.

2. Day 55 and 56

3. Subatomic Particles  Copy the table and fill in the blanks. ParticleProtonElectronNeutron Symboln Relative Charge 1+

4. Review Complete the following table for the Bohr model using your periodic table. element name # electrons# protons # neutronsatomic #atomic mass Protons Neutrons Electrons

5. Using the periodic table, find the following information: The number of protons for: 1. Aluminum 2. Fluorine 3. Beryllium 4. Neon The symbol for: 1. # 18 2. # 15 3. # 7 4. # 12 The average atomic mass for: 1. Chlorine 2. Argon 3. Calcium 4. Hydrogen The name for: 1. # 2 2. # 5 3. # 14 4. # 19

6. Periodic Table Groups Period

7. Energy Levels Period = rows (left to right) Period # = # EL (energy levels) Periods 7 periods on Periodic Table 1920212223242526 KCaScTiVCrMnFe

8. Valence Electrons  Groups = columns (up/down down/up)  Groups = chemical properties  Group # = # V.E. (valence electrons)  Charge of the atom (+ or -) 5B5B 13 Al 31 Ga 49 In 81 Tl

9. Periodic Table Trdends

10. Family Foldable  You will need 3 sheets of legal paper.  Fold the paper in half horizontally so that you will have six flaps.  Then fold cut the five bottom flaps in half exactly.  In the end you should have 10 separate flaps.

11. Family Foldable Directions: Each Flap will have one of the following titles in bold. For each title you will write the answer to what is being asked.  Group 1: Hydrogen and Alkali Metals Identify hydrogen and alkali metals. List this group’s properties.  Group 2: Alkaline Earth Metals Identify the alkaline earth Metals. Describe alkaline Earth metals.  Groups 3-12: Transition Metals List properties of transition metals.  Metalloids Name the metalloids and their properties. Identify which group each metalloid is in.  Group 3: Boron Family Describe the properties of this group  Group 4: Carbon Family Describe the properties of this group  Group 5: Nitrogen Family Describe the properties of this group  Group 6: Oxygen Family Describe the properties of this group  Group 7: Halogens Give properties of halogens.  Group 8: Noble Gases Describe noble gases. List their properties.

12. Alkali Metals  Has one valence electron.  Extremely reactive, most reactive of all elements.  The reactivity increases from top of to the bottom.  Softer than group 2 elements.  Lower melting and boiling points.  Reacts violently with water and oxygen.  Oxidizes very fast.  Only found in compounds in nature.  Hydrogen is NOT a member of this group, it is a non-metal.

13. Alkaline Earth Metals  Have two valence electrons.  Metals in group 2A are harder than metals in group 1A.  Higher melting and boiling points than group 1A.  Only found in compounds in nature.  Less reactive than group 1A metals but more reactive than remaining groups.

14. Transition Metals  Form compounds with distinctive colors  Will have several oxidation numbers  Label the columns

15. Metalloids  Metalloids are elements with properties that fall between those of metals and non-metals.  The metalloids in the remaining groups will be colored green.  They include: (list them)

16. The Boron Family  Have three valence electrons.  Boron is a metalloid and the remaining elements are metals.  Aluminum is strong, lightweight, malleable, and a good conductor of electric current.  Aluminum is the most abundant element in the earth’s crust.

17. The Carbon Family  Group 4A contains a nonmetal (Carbon), two metalloids (silicon and germanium), and two metals (tin and lead).  Has four valence electrons.  Except for water, most of the compounds in your body contain carbon.  Silicon is the second most abundant element in the Earth’s crust.  As you go down the family the elements become better conductors.

18. The Nitrogen Family  Group 5A contains two nonmetals (nitrogen and phosphorous), two metalloids (arsenic and antimony), and one metal (bismuth).  Nitrogen is nonmetal gas, phosphorous is a solid nonmetal, and bismuth is a dense metal.  Properties vary greatly.  Has 5 valence electrons.

19. The Oxygen Family (Chalcogens)  Group 6A has three nonmetals (oxygen, sulfur, and selenium), and two metalloids (tellurium and polonium).  Have six valence electrons.  Oxygen is the most abundant element in Earth’s crust.

20. The Halogens  Has 7 valence electrons.  Fluorine and Chlorine are gases, bromine is a liquid that evaporates quickly, and iodine is a solid that sublimes.  Despite their physical differences, the halogens have similar chemical properties.  They are highly reactive nonmetals, with fluorine being the most reactive and chlorine a close second.

21. The Noble Gases  Helium has two valence electrons  They remaining has eight valence electrons. [8 electrons in the outer shell = Full Helium (He) has only 2 electrons in the outer shell = Full]  The noble gases are colorless and odorless and extremely unreactive.  Exist as gases  Non-metals

22. Exit Slip  Which particle is NOT found in the nucleus? Proton, neutron, electron, or neither  What is the process of changing a liquid to a gas called? Evaporation, condensation, sublimation, neither