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Name _____________________________ Mrs. Murray HONORS Chemistry, period____ Date ______________ UNIT4: Periodic Table Text Book Chapter 6 - The Periodic Table and Periodic Law, pages 174-194 A. ELEMENT PROJECT Instructions: This project is worth 1 test grade and divided into three parts. ELEMENT: DUE DATE: 1. Research 20 facts about your element. Information to include: The element name and symbol The origin of the name of the element The date the element was discovered The name of the discoverer of the element The atomic mass and atomic number of the element Chemical/physical properties of the element Interesting uses of the element/ compounds of the element A picture / pictures of the element Each fact must be submitted as a list (TYPED) on a sheet of paper. EACH fact gets neatly and creatively displayed on a circle ( 4 circle pages needed) Each circle can have a maximum of 5 words!!! 2. Write an info-mercial about the element. The ad may be a want ad, personal ad, sales ad etc...Be creative! In the ad, display some of the information about your element. The ad must be computer generated on a poster, pamphlet, moviemaker, animoto etc. 3. Create a new element square. The square must be done on paper provided. The square must contain: ON FRONT: Chemical Symbol Atomic Number Interesting Picture of something you learned about the element ON THE BACK: Explanation of the picture on front 1 HONORS B: Activity of the Elements Referring to a periodic table, circle the member of each pair of elements which is most chemically active. 1 . Li and Na 16. CI2 and Br2 2. CI2 and F2 17. Xe and I2 3. N2 and Ne 18. Fe and Ra 4. Rb and Ca 19. Sr and Mn 5. Ti and Ca 20. K and Na 6. K and Mg 21. Au and Mg 7. O2 and S 22. S and Rn 8. I2 and Br2 23. Li and Be 9. Na and Zn 24. Se and Br2 10. P and S 25. I2 and F2 11. N2 and O2 26. Rb and Sr 12. CI2 and Ar 27. Ba and Ra 13. Ba and Fr 28. Na and Mg 14. Rb and Cu 29. Te and I2 15. Be and Cr 30. Ca and Rn 31. What is the strongest metal on the periodic table? Strongest non-metal? 32. A characteristic of most nonmetallic solids is that they are 1. brittle 3. malleable 2. ductile 4. conductors of electricity 33. Which of the following period 3 elements has the least metallic character? 1. Na 3. Al 2. Mg 4. Si 34. The chemical properties of the elements are periodic functions of their atomic 1. masses 3. numbers 2. weights 4. radii 2 HONORS C: Periodic Table Place the letter of each of the above elements next to its description below. 1 . An alkali metal ______________ 2. An alkaline earth metal ______________ 3. An inactive gas _______________ 4. An active nonmetal ______________ 5. A metalloid (semimetal) _____________ 6. An transition element _________________ 7. Its most common oxidation state is -2 _________________ 8. A metal with more than one oxidation state ________________ 9. Metal with an oxidation number of +3 _________________ 10. Has oxidation numbers of + 1 and -1 _________________ 11. Which element is so active chemically that it occurs naturally only in compounds? 1. potassium 3. copper 2. silver 4. sulfur 12. Which element is not a semimetal? 1. arsenic 2. boron 3. silicon 4. sulfur 3 HONORS D: Ions: 1. What is an ion? 2. How does an atom become a positive ion? 3. How does an atom become a negative ion? 4. Complete the table. Element Name Ion Formed and Name Loss/ Gain how many electrons Ion Bigger or Smaller than Atom Protons, Neutrons and Electrons Lewis Dot Structure of the Atom Lewis Dot Structure of the ION Aluminum Bromine Sulfur Sodium Neon Nitrogen 4 HONORS E: Element Characteristics Use a periodic table to help you answer the following questions. 1. a. How many protons does an atom of bromine (Br) have? ____________ b. In which group is bromine found? ______________ c. What is the name of its chemical family? _________________ d. How many valence electrons does it have? _____________________ e. Draw the Lewis Dot structure for the atom_____________________ f. Is it a metal, a nonmetal, or a semimetal? _____________________ g. What ion is it most likely to form in compounds? __________________ h. Draw the Lewis Dot structure for the ion._____________________ 2. a. How many protons does an atom of magnesium (Mg) have? _______________________ b. In which group is magnesium found? ___________________ c. What is the name of its chemical family? _______________________ d. How many valence electrons does it have? __________________ e. Draw the Lewis Dot structure for the atom_____________________ f. Is it a metal, a nonmetal, or a semimetal? __________________ g. What ion is it most likely to form in compounds? _______________________ h. Draw the Lewis Dot structure for the ion._____________________ 3. a. How many protons does an atom of potassium (K) have? ___________________ b. In which group is potassium found? ________________ c. What is the name of its chemical family? _______________________ d. How many valence electrons does it have? __________________ e. Draw the Lewis Dot structure for the atom_____________________ f. Is it a metal, a nonmetal, or a semimetal? __________________ g. What ion is it most likely to form in compounds? _______________________ h. Draw the Lewis Dot structure for the ion._____________________ 5 HONORS F: Periodic Table Trends 1. Where are the most active metals located? __________________________ 2. Where are the most active nonmetals located? ___________________________ 3. As you go from left to right across a period, the atomic size ( decreases / increases). Why? ___________________________________________________________ 4. As you travel down a group, the atomic size (decreases /increases). _________________________________________________________________ 5. A negative ion is ( larger / smaller) than its parent atom. 6. A positive ion is ( larger / smaller) than its parent atom. 7. As you go from left to right across a period, the first ionization energy generally ( decreases / increases). ________________________________________ 8. As you go down a group, the first ionization energy generally ( decreases / increases) ____________________________________________________________ 9. Where is the highest electronegativity found? _____________________________ 10. Where is the lowest electronegativity found? ______________________________ 11. Elements of Group 1 are called ____________________________ 12. Elements of Group 2 are called ____________________________ 13. Elements of Group 3-11 are called __________________________________ 14. As you go from left to right across the periodic table, the elements go from ( metals / nonmetals) to ( metals / nonmetals ). 15. Group 17 elements are called _________________________________ 16. The most active element in Group 17 is _____________________________ 17. Group 18 elements are called _____________________________________ 18. Can lose electrons from valence and sub-valence electrons _______________________ 19. Elements within a group have a similar number of _______________________ 20. Elements across a period have the same number of ______________________ 21. A colored ion generally indicates ____________________________________ 22. As you go down a group, the elements generally become (more / less) metallic. 23. The majority of elements in the periodic table are (metals / nonmetals). 24. Elements in the periodic table are arranged according to their ___________________ 25. An element with both metallic and nonmetallic properties is called a _________________ 6 HONORS G: More Periodic Trends Complete the following tables: Periodic Trend Going Across the Periodic Table Element Atomic Radius (pm) Electronegativity First Ionization Energy (kJ/mole) Electron Affinity* Calcium Selenium Trend Explanation of Trend Periodic Trend Going Down the Periodic Table Element Atomic Radius (pm) Electronegativity First Ionization Energy (kJ/mole) Electron Affinity* Fluorine Iodine Trend Explanation of Trend * online information…not on Table S! 7 HONORS H: Multiple Choice ___1. The elements from which two groups of the periodic table are most similar in their chemical properties? (1) 1 and 2 (2) 1 and 17 (3) 2 and 17 (4) 17 and 18 ___2. Elements in the modern periodic table are arranged according to their (1) atomic number (2) atomic mass (3) relative activity (4) relative size ___3. As elements of Group 15 of the periodic table are considered in order from top to bottom, the metallic character of the atoms of each successive element generally (1) decreases (2) increases (3) remains the same ___4. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? (1) nonmetal metalloid metal (2) metalloid metal nonmetal (3) metal metalloid nonmetal (4) metal nonmetal metalloid ___5. Which statement is true about the properties of the elements in anyone period of the periodic table? (1) They are determined by the number of neutrons. (2) They are determined by the number of electrons in the first principal energy level. (3) They change in a generally systematic manner. (4) They change in a random, unpredictable manner. ___6. Which statement describes the elements in Period 3? (1) Each successive element has a greater atomic radius. (2) Each successive element has a lower electro negativity. (3) All elements have similar chemical properties. (4) All elements have valence electrons in the same principal energy level. ___7. Which noble gas has the highest first ionization energy? (1) radon (3)neon (2) krypton (4) helium ___8. Which of these metals loses electrons most readily? (1) calcium (2) magnesium (3) potassium (4) sodium ___9. In which area of the periodic table are the elements with the strongest nonmetallic properties located? (1) lower left (2) upper left (3) lower right (4) upper right 8 HONORS I: SAT II Questions 1-4 refer to the following atoms in the ground state. (A) Ar (B) O (C) S (D) Ti (E) U 1. Has the electron configuration 1s2 2s22p63s23p4 _______________ 2. Has the same number of electrons as Ca2+ _______________ 3. Has electrons in f orbitals _________________ 4. Is the LEAST chemically reactive ________________ ____5. For elements in the left-most column of the periodic table, properties that have increasing values as the atomic number increases include which of the following? I. Ionization energy (potential) II. Atomic radius III. Atomic mass (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III ____6. Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having A. a greater charge on the nucleus. B. a smaller charge on the nucleus. C. more principal energy levels. D. fewer principal energy levels. ____7. As the elements in Period 3 are considered from left to right, they tend to A. lose electrons more readily and increase in metallic character. B. lose electrons more readily and increase in nonmetallic character. C. gain electrons more readily and increase in metallic character. D. gain electrons more readily and increase in nonmetallic character. 9 HONORS ____8. Which diagram correctly shows the relationship between electronegativity and atomic number for the elements of Period 3? ___9. A sulfur ion is represented as S2-. How is the sulfide ion different from a sulfur atom? A. The sulfide ion has gained two electrons. B. The sulfide ion has gained two protons. C. The sulfide ion has lost two electrons. D. The sulfide ion has lost two protons. ___10. When an atom of aluminum forms an ion, the resulting ionic symbol is correctly written as A. Al3+ B. Al2+ C. Al2D. Al3___11. Which element has properties most like those of oxygen? A. nitrogen B. fluorine C. sulfur D. chlorine 10 HONORS J. DBQ DRY ICE Dry ice is frozen carbon dioxide. It has a unique feature. Under normal atmospheric conditions, it sublimes; changes from a solid to a gas. If you ever have to handle dry ice, you want to be sure to wear heavy gloves, because a block of dry ice has a surface temperature of 78.5 ° C. The super-cold surface temperature can easily damage your skin if you touch it directly. While dry ice looks like it would be cold, it's extremely dangerous to the touch and can cause severe burns. It's actually a lot like if you were to touch the handle of a hot pot or pan without an oven mitt. If you did this for less than a second -- so that you simply felt the heat and quickly pulled your hand away -- then at most your skin would be a little red. However, if you were to grab a hold of the handle tightly for a couple of seconds or more, chances are you would get a pretty nasty burn. The heat kills the skin cells. It's the same with dry ice. Dry ice actually freezes your skin cells. The resulting injury is very similar to a burn and should be treated with the same medical attention. For the same reason you never want to taste or swallow dry ice. This would be like drinking something that was scalding hot and you would risk damaging your mouth, throat and part of your esophagus. 1. What is sublimation? 2. What other chemical sublimes? 3. Is sublimation a chemical or physical change? Explain. 4. What is the surface temperature of dry ice? Convert this temperature to Kelvin. 5. What is the oxidation state of oxygen in carbon dioxide? 6. What happens when you touch dry ice? 11 HONORS 12 HONORS UNIT 4 Periodic Table: 1. Periodic Table was originally developed by Dmitri Mendeleev. 2. It is arranged according to increased atomic number. 3. The Periodic Law states that the chemical properties of elements are periodic functions of their atomic number. 4. Elements are classified as metals, non-metals and metalloids. Metals make up more than 2/3 of the periodic table found on the left side of the staircase on the periodic table lose electrons to form positive ions which are smaller than the metal atom solids at room temperature except Mercury (Hg) which is a liquid most active metals found on lower left of table (Francium) good conductors of heat and electricity malleable, ductile and have luster Non-Metals found on the right of the staircase on the periodic table gain electrons to form negative ions which are larger than the atom Bromine is the only liquid non-metal most active non-metal found upper right of table (Fluorine) brittle and dull poor conductors of electricity Metalloids found on the staircase on the periodic table have properties of both metals and non-metals 5. Vertical columns on the Periodic Table are called groups or families. Atoms in the same group have the same number of valence electrons, therefore reacting very similarly. Elements of the same group have the most in common. Group 1 = Alkali Metals. Very reactive metals-found in nature in compound form only Group 2 = Alkaline Earth Metals. Reactive metals mostly found in nature in compound form Group 17 = Halogens (all diatomics) - this group contains all three phases of matter at room temperature. F2, Cl2 - gases, Br2 - liquid, I2 - solid). These are very reactive elements that are found in nature in compound form only. Group 18 = Noble Gases (monatomics) have 8 valence electrons in the outer PEL, except He which only has 2. 13 HONORS Group 3-11 – Transition Metals - found in the middle of the periodic table. can have electrons from two outermost shell involved in bonding they have multiple oxidation states form colored ions in compounds or in solution 6. Horizontal rows on the Periodic Table are called periods or rows. Atoms in the same row have the same number of occupied principal energy levels. 7. General trends of the periodic table: Metallic character increases Increasing PELs Atomic radius increases Ionization energy decreases Electronegativity decreases Electron Affinity decreases Metallic character decreases Increased Effective nuclear charge Atomic radius decreases Ionization energy increases Electronegativity increases Electron Affinity increases 14