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Atoms Unit Matter’s Building Blocks “Nothing exists except atoms and empty space; everything else is opinion” Democritus Greek Philosopher, 460-370bc Section 1A – Atoms Must Know Vocabulary! Below is a list of the vocabulary terms used in this unit. By the end of the unit, you should be able to write a working definition of each term and correctly use each term in a sentence. alchemy amu atom atomic mass atomic mass number atomic mass unit atomic number cathode ray chemical symbol Dalton's atomic theory Democritus Dmitri Mendeleev electron Ernst Rutherford gram group Henry Mosely isotope J J Thompson James Chadwick John Dalton mass number neutron nucleus period periodic table plum pudding model proton scientific notation subatomic particle Section 1B –– Mastery Objectives and Critical Skills Describe the historical evolution of the atomic model from early Greek to modern times. List the three subatomic particles that make up atoms and describe their location and 3 key facts about each. Explain how atoms of different elements differ from each other List and explain 3 key properties that can be used to sort elements into different groups. Give one example of how each subatomic particle influences the properties of the element. Describe the subatomic differences between the isotopes of atoms of the same element. Determine the atomic mass of an element based on its isotopes and their relative abundance Using the scientific method, build and test a model that explains another objects’ internal organization. Version 3 – summer 2009 Atoms Unit Section 2A –Required Readings covered on Tests and Quizzes 1) Wilbraham, Staley, Matta and Waterman, Chemistry, pp 107-113; 115-121. 2) John Godfrey Saxe “The Blind Men and the Elephant” Section 2B –Websites to help with OCAs and Extend Your Knowledge see the wiki for current listings of key URLS Section 3 –Anticipated In Class Activities 1) Lecture / slides 2) Demonstrations a) Atomic Size b) Scattering demo c) Cathode Rays and Electrons 3) Student Labs and Activities a) Black Box Investigation b) Isotopes and the Atomic Mass of Pennium c) Patterns and Periodicity 4) Student Project –Representative Elements – Part I 5) Videos a) “The Elements” with Roger McGough Section 4 –– Outside Class Assignments Thoughtfully answer each of the following questions or comments. Include all your reasoning and show all your work wherever it is appropriate. To receive any credit for a question, your answer must be a correctly numbered restatement of the question or statement followed by a series of complete sentences. No phrases, partial answers or isolated numbers will be given credit! Your answer must stand alone without the reader knowing the question asked or statement made. Due dates for each assignment will be given in class. (Please remember - homework that is passed in late – not when collected during class) is automatically discounted 15% of total possible points.) 1. Create a concept map for the following set of terms: atom, electron, neutron, proton, isotope, atomic mass, atomic mass number, atomic number, amu, nucleus, and mass number. Version 3 – summer 2009 Atoms Unit 2. Each scientist bases his/her work on that of their predecessors. Using the presentation s and the readings list five main contributors to the atomic theory and explain what and how each contributed to the modern atomic theory. 3. Read the attached poem “The Blind Man and the Elephant” by John Godfrey Saxe. a. Why did the blind men have such different impressions of the elephant? b. Why didn’t the blind men look further for the truth? c. Describe a time when you jumped to a conclusion about something and later found out you only had part of the story or truth. d. How does this poem reflect the history of atomic theory? 4. Why is an atom considered a basic building blocks of matter even though smaller particles such as protons and neutrons make them up? 5. Imagine “standing” on top of a carbon 14 nucleus, a. Describe the numbers and kinds of subatomic particles you would see looking straight down at your feet. b. Describe the numbers and kinds of subatomic particles you would see looking out from where you are standing. c. If the bulk of an atom is empty space, why don’t we fall through the seat of a chair when we try to sit down or slip through walls when we lean against them? 6. You are already familiar with the law of conservation of mass. Explain this law using Dalton’s atomic theory. 7. Diamond and graphite are both composed only of carbon atoms. The density of diamond is 3.52 g/cm3. The density of graphite is 2.25 g/cm3. a. Use modern atomic theory and your imagination to explain how carbon can have two different densities. b. Which would weigh more, a cubic inch of graphite or a cubic inch of diamond? Explain your answer by showing your reasoning. 8. Complete the attached “Table of Elements” at the back of the packet. 9. What data must you know about the isotopes of an element in order to calculate the atomic mass of the element? 10. Calculate the atomic mass of bromine. One isotope of bromine has an atomic mass of 78.62 amu and makes up about 50.7% of all naturally occurring bromine. The second isotope of bromine has an atomic mass of 80.92 amu. Version 3 – summer 2009 Atoms Unit 11. Uranium has three common isotopes. If the abundance of 234U is 0.01%, the abundance of 235U is 0.71% and the reminder is 238U, what is the atomic mass of uranium? 12. The periodic table has been called the central tool of modern chemists. a. Why is it called the periodic table? b. How are the periodic table and the periodic law related? c. You are expected to memorize the symbols and locations of 50 elements in the periodic table. The names for those fifty elements are given below. Fill in the attached periodic table with the correct symbols and locations for each of these fifty elements. Version 3 – summer 2009 Atoms Unit The Table of Elements Atomic Mass Number Number 20 196 Number of Protons Humber of neutrons 20 14 14 Number of Electrons 117 17 Version 3 – summer 2009 Symbol of Element Atoms Unit The First Fifty Elements Element Symbol Element Aluminum Phosphorus Antimony Platinum Argon Potassium Arsenic Radon Astatine Selenium Barium Silicon Beryllium Silver Boron Sodium Bromine Stron tium Calcium Sulfur Carbon Tantalum Cesium Tin Chlorine Tungsten Chromium uranium Cobalt Vanadium Copper Zinc Fluorine Francium Germanium Gold Helium Hydrogen Iodine Iron Lead Lithium Magnesium Manganese Mercury Molybdenum Neon Nickel Nitrogen Oxygen Version 3 – summer 2009 Symbol