Honors Chemistry Ms. K. Pages

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1 Name # Period Honors Chemistry Ms. K Pages Task Checklist: Look at Online Textbook Materials Look at Section 1 Visual Concepts Look at Section 2 Visual Concepts Look at Section 3 Visual Concepts Take Section 1 Self-Check Quiz Take Section 2 Self-Check Quiz Take Section 3 Self-Check Quiz Do the Periodic Table Concept Map Other Tasks Read Section 1 Read Section 2 Read Section 3 Review Chapter Packet Examine Class Website

2 Name ium Hour Elements of the Periodic Table What s in a Name? If you think naming a puppy is difficult, you should try naming a new element! First, you need to think of an appropriate name and then you need approval from the ACS (American Chemical Society) and the IUPAC (International Union of Pure and Applied Chemistry). Once these organizations agree on a name, that name is assigned to that element permanently. Elements have permanent names but elements are using their temporary systematic names until permanent names are assigned. Actually, element 117 has not even been discovered yet (but we know it s out there). Directions: Using your list of elements and the following clues, determine which element names were inspired by these famous people, places, and things. Famous People: Ernest Rutherford; British The Father of Nuclear Science. First to break the nucleus of an atom in Glenn Seaborg; American Part of a team which discovered the elements Plutonium, Americium, Curium, Berkelium, Californium, Einsteinium, and Mendelevium. Neils Bohr; Danish Designed the Bohr Model of the atom in Later advised the Atomic Bomb project. Lise Meitner; Austrian She worked with Otto Hahn to discover the process of nuclear fission in Pierre and Marie Curie French husband and wife team. Discovered the elements Radium and Polonium. Albert Einstein; Austrian One of the greatest scientists of all time. Known for his work with nuclear physics and for his theory of relativity (E=MC 2 ). Enrico Fermi; Italian Produced the first nuclear chain reaction in Worked on atomic bomb project. Ernest Lawrence; American Invented and developed the first particle accelerator in 1939 which led to the discovery of the subatomic particle called the Meson. Alfred Nobel; Swedish Made the use and handling of explosives safer by inventing dynamite. He established and funded the Nobel Prize to honor people who benefited society. Dmitri Mendeleev; Russian Developed the periodic law of elements from which the periodic table was made. Famous Places: University of California at Berkeley Many elements were discovered in the science laboratories here. Countries and Continents Some elements were named for countries and continents. Use an atlas if needed. Planets and planetoids Some elements were named for planets and planetoids. (Mercury, Venus, Earth, Mars, Jupiter, Saturn, Uranus, Neptune, Pluto).

3 Element Name Symbol Atomic # Clue Famous People Use this clue to find the element name. Write in a clue if none is given: Einsteinium Es 99 Named after one of the greatest scientists of all time. Famous for his theory of relativity (E=MC 2 ). Named after a Danish scientist who designed a model of the atom in Cm (write the clue here) Meitnerium Mt (write the clue here) Named for the Father of Nuclear Science. He was the first to break the nucleus of an atom. Named for the scientist who developed the first particle accelerator in Named after the American scientist who helped discover Plutonium, Americium, etc. Named after the Italian scientist who produced the first nuclear chain reaction in Md (write the clue here) Named after the inventor of dynamite. He also established and funded the Nobel prize. Famous Places Use this clue to find those elements named for famous places: Cf Discovered at the University of California at Berkeley. 97 Discovered at the University of California at Berkeley. Am 95 (write name of country here) Europe Francium (write name of country here) Germany 49 (write name of country here) Gonyoium Gy Just kidding I had an extra blank in this table that needed filling. Mercury (write the name of the planet/planetoid) Neptune Uranus Pu 94 (write the name of the planet/planetoid)

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8 It?s Elementary? March Madness Publication No March Madness is upon us! Your students are probably already working on their next assignment in bracketology, predicting the field for the NCAA Basketball Tournament. (Although the word doesn?t appear in Webster?s, there is an article on bracketology on Wikipedia, so it must be real.) Let?s apply the principles of bracketology to the properties of the elements. The compet ition among the 64 elements is stiff, and there is a wealth of information for students to research, in this?elementary? version of March Madness! Review of Element Properties Define each of the following properties of the elements and briefly describe any periodic trend in the property across a row or down a column in the periodic table.? Ionization energy? Atomic radius Tournament Rules Here are the rules for predicting the winners in each round of It?s Elementary?March Madness. In the event of a tie in the properties of two competing elements in any round of the tournament, the element with the larger atomic mass always wins.? First round: Research the date of discovery of each element. In each bracket, the element that was discovered earlier (in its free element form) wins and proceeds to the second round. If an element has been known since ancient times, assign it a discovery date of zero.? Second round: Compare the ionization energy of the elements in each bracket. The element with the higher ionization energy is the winner and advances to the Sweet 16.? Third round (Sweet 16): Compare the group numbers of the elements? the winner is the element with the larger group number using the international (IUPAC) system (Groups 1?18).? Fourth round: The element with the larger atomic radius wins this round and earns a trip to the Final Four. Use the atomic or covalent radius only, not the van der Waals radius.? Semifinals (Final Four): Solve the following riddles to determine the two elements that will compete for the championship. This?salt-maker? is also a rainmaker when its silver salt is scattered into clouds. Once a sedative and cure for nervous tension, the ion of this element is now a trite or commonplace expression.? Finals: It?s often said that there?s no in team, but it is the winner in this field! Connecting to the National Standards This laboratory activity relates to the following National Science Education Standards (1996): Unifying Concepts and Processes: Grades K 12 Systems, order, and organization Content Standards: Grades 9 12 Content Standard B: Physical Science, structure of atoms, structure and properties of matter References John Emsley, Nature?s Building Blocks, Oxford University Press: Oxford England (2001). WebElements Periodic Table, (accessed February 2008). Flinn Scientific Periodic Table of the Elements, Catalog No. AP9020. CHEM-FAX...makes science teaching easier

9 Hydrogen Promethium Copper Arsenic Chlorine Rhodium Aluminum Indium Scandium Niobium Fluorine Iodine Manganese Rubidium Boron Lanthanum Beryllium Gadolinium Germanium Krypton Calcium Cadmium Sulfur Tellurium Chromium Ruthenium Magnesium Barium Nickel Zirconium Oxygen Neodymium Helium Samarium Zinc Selenium Argon Palladium Silicon Tin Titanium Molybdenum Neon Xenon Iron Strontium Carbon Cerium Lithium Europium Gallium Bromine Potassium Silver Phosphorus Antimony Vanadium Technetium Sodium Cesium Cobalt Yttrium Nitrogen Praseodymium It?s Elementary?March Madness! 2008 Flinn Scientific, Inc. All Rights Reserved

10 Hydrogen Promethium Copper Arsenic Chlorine Rhodium Aluminum Indium Scandium Niobium Fluorine Iodine Manganese Rubidium Boron Lanthanum Beryllium Gadolinium Germanium Krypton Calcium Cadmium Sulfur Tellurium Chromium Ruthenium Magnesium Barium Nickel Zirconium Oxygen Neodymium Hydrogen Copper Chlorine Aluminum Niobium Iodine Manganese Boron Beryllium Germanium Calcium Sulfur Chromium Magnesium Nickel Oxygen Hydrogen Chlorine Iodine Boron Beryllium Sulfur Magnesium Oxygen It?s Elementary?March Madness! Answers Chlorine Zinc Iodine* Zinc Iodine Iodine Xenon Iodine Sulfur Bromine Bromine Sulfur Bromine Oxygen Nitrogen *This?salt-maker? (halogen) is also a rainmaker in the form of AgI seed crystals.?bromide salts were used as a sedative in the 1800s. Zinc Palladium Xenon Carbon Bromine Antimony Vanadium Nitrogen Samarium Zinc Palladium Tin Molybdenum Xenon Iron Carbon Lithium Bromine Silver Antimony Vanadium Sodium Cobalt Nitrogen Helium Samarium Zinc Selenium Argon Palladium Silicon Tin Titanium Molybdenum Neon Xenon Iron Strontium Carbon Cerium Lithium Europium Gallium Bromine Potassium Silver Phosphorus Antimony Vanadium Technetium Sodium Cesium Cobalt Yttrium Nitrogen Praseodymium 2008 Flinn Scientific, Inc. All Rights Reserved

11 Attention Honors Chemistry Students: enter the All-School Competition for the Periodic Table Objective: to bring in the most items with the periodic table on them that also have another function. Each item must have all or part of the real periodic table on it. All items must be submitted by 3:03pm on Monday, November 23, Example? periodic table tie Example? periodic table coffee cup Winners and Prizes: The class that brings in the most qualifying items will win an after school pizza party, a mystery prize, and a chance to see the?bes t Demonstration Ever?. The individual who brings in the most qualifying items will win a periodic table beach towel.

12 K Mrs. Name # Chemistry Date Period Chapter 5 Internet Research Johann W. Dobereiner 1. What was his birthyear & deathyear? 2. In what country was he born? 3. What is a triad? 4. Why did he group these elements like this? 5. Explain the law of triads. 6. What did he notice about the atomic mass of the middle element in a triad? John Newlands 7. What was his birthyear & deathyear? 8. In what country was he born? 9. What did he do with the elements? 10. Explain the law of octaves? 11. Why did some scientists dispute his work as coincidence? Dimitri Mendeleev 12. What was his birthyear & deathyear? 13. In what country was he born? 14. He proposed arranging the elements in order of increasing. 15. In what year did he arrange the first periodic table? 16. Why did Mendeleev leave?gaps? in his table? 17. What elements were later discovered that Mendeleev predicted would exist? Henry Moseley 18. What was his birthyear & deathyear? 19. In what country was he born? 20. He proposed revising Mendeleev s periodic table so that the properties of the elements varied periodically when arranged in order of increasing. 21. What is the periodic law?

13 Ms. K Chemistry Name # Date Period Trends Worksheet 1. Circle the more reactive of the pair. a. K, Ga b. Rb, Si c. Mg, Ba d. F, Br e. S, Ar f. N, F g. Ne, Br 2. Circle the larger atom. h. K, Ga i. Rb, Si j. Mg, Ba k. P, Ra 3. Circle the larger of the pair. l. Li, Li + m. B, B +3 n. F, F - o. P, P Circle the more electronegative element of the pair. p. K, Se q. N, As r. F, Ne s. Se, Ne 5. Circle the element with the greater ionization energy. t. Rb, I u. N, Sb v. N, O 6. Circle the element with a more negative electron affinity. w. C, F x. C, Ne 7. Explain why atomic radii gets larger as one moves down a group. 8. Explain why atomic radii gets larger as one moves left in a period. 9. Explain why anions are larger than their respective atoms. 10. Explain why atoms are larger than their respective cations.

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15 Ms. K Chemistry Name # Date Period Reactivity metals (within a period) Metals increase in activity from right to left on the periodic table. This leaves the alkali metals being the most reactive metals. (within a group) Metals increase in activity from top to bottom. This leaves francium being the most reactive alkali metal What is the most metallic element? nonmetals - (within a period) Nonmetals increase in activity from left to right on the periodic table with the exception of the noble gases. This leaves the halogens being the most reactive nonmetals. (within a group) Nonmetals increase in activity from bottom to top. This leaves fluorine being the most reactive halogen. What is the most nonmetallic element? Atomic Radius atomic radius ½ the distance between the nuclei of identical atoms that are bonded together GROUP TRENDS: In general, the atomic radii of the main-group elements increase from top to bottom in a group. WHY? - The number of energy levels increases as you move down a group as the number of electrons increases. Each subsequent energy level is further from the nucleus than the last. Therefore, the atomic radius increases as the group and energy levels increase. PERIOD TRENDS: In general, the atomic radii decreases from left to right on the table due to the increasing positive charge of the nucleus. WHY? - As you go across a period, electrons are added to the same energy level. At the same time, protons are being added to the nucleus. The concentration of more protons in the nucleus creates a "higher effective nuclear charge." In other words, there is a stronger force of attraction pulling the electrons closer to the nucleus resulting in a smaller atomic radius. What element has the largest atomic radius? What element has the smallest atomic radius?

16 Ionic Radius ionic radius the radius of an ion CATIONS: Positive ions are smaller than their respective atoms. WHY? - If the electron that is lost is the only valence electron so that the electron configuration of the cation is like that of a noble gas, then an entire energy level is lost. In this case, the radius of the cation is much smaller than its respective atom. Na Na + ANIONS: Negative ions are larger than their respective atoms. WHY? - Electron-electron repulsion forces them to spread further apart. Electrons outnumber protons; the protons cannot pull the extra electrons as tightly toward the nucleus. Cl Cl - Electronegativity electronegativity? a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound (This scale was devised by Linus Pauling, one of America?s most famous chemists.) GROUP TRENDS: Electronegativities tend to increase going up a group or remain about the same. PERIOD TRENDS: Electronegativities tend to increase across each period, although there are exceptions. NOBLE GASES: Since some noble gases do not form compounds (He, Ne, Ar), some do not have electronegativity values. When a noble gas does form a compound (Kr, Xe, Rn), it follows the group and period trends.

17 Ionization Energy ionization energy? the energy required to remove one electron from a neutral atom of an element (An electron can be removed from any atom if enough energy is supplied.) Why is there is a jump in IE between N and O? 1 st IE 2 nd IE Remember: Full or ½ full orbitals lend more stability to the atom. Why does Na has a large 2 nd IE and not a large 1 st IE? What element would you expect to have a large 3 rd ionization energy compared to its other IEs? Electron Affinity electron affinity? the energy change that occurs when a neutral atom takes an electron A + e - A - (an anion) + energy - Most atoms release energy when they acquire an electron. If energy is released, the electron affinity value if negative (- kj mol ). A + e - + energy A - (an anion) - Some atoms must be forced to take an e - by adding energy. If energy is absorbed, the electron affinity value is positive (+ kj mol ). Why does nitrogen have a positive electron affinity compared to carbon and oxygen?s negative values? Remember: Full or ½ full orbitals lend more stability to the atom.

18 Attention Honors Chemistry Students: enter the All-School Competition for the Periodic Table Objective: to bring in the most items with the periodic table on them that also have another function. Each item must have all or part of the real periodic table on it. All items must be submitted by 3:03pm on Monday, November 23, Example? periodic table tie Example? periodic table coffee cup Winners and Prizes: The class that brings in the most qualifying items will win an after school pizza party, a mystery prize, and a chance to see the?bes t Demonstration Ever?. The individual who brings in the most qualifying items will win a periodic table beach towel.

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20 Ms. Meer Chemistry Atomic Radii & Ionic Radii Worksheet Name # Date Period 1. Circle the larger atom. a. K, Ga b. Rb, Si c. Mg, Ba d. P, Ra 2. Circle the larger of the pair. a. Li, Li + b. B, B +3 c. F, F - d. P, P Explain why atomic radii gets larger as one moves down a group. 4. Explain why atomic radii gets larger as one moves left in a period. 5. Explain why anions are larger than their respective atoms. 6. Explain why atoms are larger than their respective cations.