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CHEMISTRY-CP, PERIOD 4, MS. WACK CHAPTER 4, DAILY PLANNER, THE ATOM DAY 1 10/4 2 3 4 5 6 7 8 9 CLASSWORK HOMEWORK Finish Vocabulary Definitions Movie: Atoms Work on Vocabulary Definitions Notes: Atomic Models—Democritus to Dalton HW1: Read the article “SEARCHING FOR THE 6TH, TEVATRON REVEALS TRUTH ABOUT PARTICLES” and answer the questions on Worksheet A Finish today’s lab handout Vocabulary Quiz (20 Points) Indirect Evidence Lab (25 Points) Notes: Atomic Models—Franklin to Thomson HW2: Worksheet B Notes: Finish Models and Atom Basics Atomic Mass of Candium Lab (10 Points) Notes & Practice: Atomic Number, Mass Number, Isotopes, Protons, Electrons Neutrons Homework & Extra Credit Due (20 Points + EC) Finish Notes “Have you Met Objectives Worksheet” Go Over Review Worksheet & Homework Review for Test Test Chapter 4 (100 Points) HW3: Worksheet C HW4: Worksheet D Finish today’s review worksheet Study for Chapter 4 Test Top Group for Chapter 2: Carter Paules & Jenna Reid TOTAL POSSIBLE POINTS FOR CHAPTER 4: 175 POINTS + 19 POINTS EXTRA CREDIT EXTRA CREDIT: HOMEWORK GRADE A 20/20 B 17/20 C 15/20 D 12/20 F 10/20 No grade 0/50 ALL HW COMPLETE 4/4 HW 3.5/4 HW COMPLETE ¾ HW COMPLETE 2.5/4 HW COMPLETE 2/4 HW COMPLETE LESS THAN 2/4 HW COMPLETE 5 Points: Worksheet E 4 Points: Worksheet F 5 Points: Identify 10 elements that have symbols not directly related to their names. Research the origin of the name and symbol and display the information on an 8x11 poster board. The more creative you are with displaying the information, the more points you will get! 5 Points: Identify 10 elements named after either a person or place. Create a poster board illustrating the elements, their symbols and the person or place. The more creative you are, the more points you will get! Fermilab advances the understanding of the fundamental nature of matter and energy by providing leadership and resources for qualified researchers to conduct basic research at the frontiers of high energy physics. Searching for the Sixth: Tevatron Reveals Truth about Particles Meet the Quarks – a guide to their identities Millions of dollars worth of equipment, a four-mile ring buried in a maze of tangled wire, particles hurtling at one another, and scientists monitoring it all from their computer screens...What's all the commotion about? The answer to this question is simple: particles. Particles are the building blocks for all matter, from paper to primordial ooze. To better understand the forces of nature and the behavior of matter, scientists are attempting to learn all they can about particles using devices called accelerators. The Tevatron, although it sounds like some kind of doomsday robot, is the name of the superconducting particle accelerator at Fermilab. The Tevatron is a four-mile ring buried in a tunnel twenty feet underground. Inside this ring, protons whiz through the accelerator at nearly the speed of light. By crashing protons into antiprotons or into fixed targets, researchers can create new and different particles to study. Creating a new particle, however, requires an enormous amount of energy. The Tevatron is unique because it can accelerate particles to energies higher than those of any other accelerator in the world. The Tevatron's energy is essential in discovering the universe's heaviest particles, such as the top quark. No new particles could exist without some type of collision. Scientists control the speedy particles using magnets in the accelerator to steer the particles into each other or into a fixed target. Observing these particles is a difficult task because they are too small to be seen by the human eye. To do this, researchers have designed and built special detectors to monitor and record particle interactions. With these detectors, scientists hope to observe, among other things, particles called quarks (see box below). Physicists believe that there are six types of quarks, all of which can result from the proton-antiproton collisions that take place in accelerators like the Tevatron. The existence of the sixth quark was expected long before it was actually created because physicists believe that quarks come in pairs. After the discovery of the fifth quark, bottom, at Fermilab in 1977, the search for the sixth was the next logical step. The 1994 discovery of the top quark at Fermilab proved that physicists were on the right track with their theory about quarks, the Standard Model. Just as philosophers discover their own truths through self-examination, scientists discover universal truths through experimentation at Fermilab. That's what it's all about! Name Date Discovered General Information Up 1964 Down 1964 Strange 1964 Charm 1975 (Stanford Linear Accel.) Scientists readily accepted the data which indicated a fourth quark because they expected a partner for the strange quark. As a result of this data, the quark theory became more believable. (How charming!) Bottom 1977 (Fermilab) Leon Lederman and a Fermilab team discovered yet another! Because this quark and its expected partner were to be the object of intense scrutiny and searching, many wanted to name them Truth and Beauty. Top 1994 (Fermilab) Finally Fermilab found the last piece of the puzzle. To the scientists' surprise, the mass of this quark was very different from that of the others. Why? A researcher's work is never done... By the early '60's, physicists had gathered sufficient data to indicate the presence of these quarks. The first people to interpret this data in the form of a quark theory were Murray Gell-Mann and George Zweig. WORKSHEET A—BASED ON “SEARCHING FOR THE 6TH, TEVATRON REVEALS TRUTH ABOUT PARTICLES” 1. Are the protons, electrons and neutrons the only subatomic particles? Explain. 2. What is the Tevatron? Why is it important for the development of the atom? 3. How does a particle accelerator allow you to “see” the particles in an atom? 4. How is the motion of the particles in a particle accelerator controlled? 5. How many quarks do physicists believe there are? 6. Who were the first scientists to develop the quark theory? 7. What are the names of the quarks? 8. When was the last quark discovered? 9. Have scientists discovered all there is to know about the atom? Explain. WORKSHEET B (© Prentice Hall) MATCHING (Each letter may be used once, more than once or not at all.) A. Democritus B. Lavoisier C. Proust D. Dalton E. Franklin F. Faraday _____ 1. Matter is neither created nor destroyed in chemical reactions. _____ 2. A given compound always has the same relative numbers and kinds of atoms. _____ 3. All atoms of a given element are identical, but they differ from those of any other element. _____ 4. A given compound always contains the same elements in the same proportions by mass. _____ 5. Each element is composed of extremely small particles called atoms. _____ 6. The scientist who discovered that the structure of the atom was somehow related to electricity _____ 7. Atoms are neither created nor destroyed in chemical reactions. TRUE/FALSE _____ 8. There are about 5000 elements, which combine to form the vast number of different substances in the world around us. _____ 9. Like other well-known Greek philosophers of the time, Aristotle agreed with Democritus’ ideas about atoms. _____ 10. The study of atoms has led to technological advances such as televisions and computers. _____ 11. Ancient philosophers regularly performed controlled experiments. _____ 12. Both Democritus and Dalton suggested that matter is made up of atoms. _____ 13. Dalton was correct in thinking that atoms could not be divided into smaller particles. _____ 14. The smallest particle of an element that retains the properties of that element is called an atom. LAW OF CONSTANT COMPOSITION Tanya wanted to verify Proust’s law of constant composition. She heated different masses of magnesium powder in the presence of oxygen. Tanya then recorded the mass of each product in the table below. Original Mass of Total Mass of Calculated Mass of Magnesium (grams) Product-Magnesium Oxygen % Magnesium % Oxygen oxide (grams) 2.00 3.34 2.40 3.98 2.80 4.64 3.20 5.30 Tanya concluded that the product she had made was a magnesium oxide. She used the following formulas to calculate the percent composition of magnesium and oxygen by mass. Mass of magnesium 100% = percent magnesium Mass of product Mass of oxygen 100% = percent oxygen Mass of product Tanya also concluded that the product, magnesium oxide, always contained 60% magnesium and 40% oxygen. 9. Calculate the mass of oxygen in each compound and write your answers in the data table. 10. Evaluate Tanya’s conclusion by calculating the percent composition of each product (Record it in the data table). correct? Why or why not? 11. How did Tanya’s investigation support Proust’s law of constant composition? Was she WORKSHEET C TRUE/FALSE _____ 1. There are no instruments powerful enough to magnify atoms so that they can be seen. _____ 2. The submicroscopic world of the atom includes exotic particles called quarks and gluons. _____ 3. The neutron was the first subatomic particle discovered. _____ 4. According to Rutherford, the whole atom is dense. _____ 5. Millikan determined the charge and mass of an electron in his oil-drop experiment. MATCHING A. Thomson B. Millikan C. Rutherford D. Becqueral E. The Curies _____ 6. Proposed the nuclear atomic model. _____ 7. Determined that cathode rays were made of negatively charged particles. _____ 8. Discovered radioactivity while working with a sample of uranium. _____ 9. Calculated the mass of an electron. _____ 10. Disproved Thomson’s model of the atom. DRAW and label a diagram of each atomic model below. 11) Plum-Pudding Model 12) Nuclear Atomic Model 13. Why was the discovery of radioactivity important to the development of the atom? CONCEPT MASTERY In 1897, J.J. Thomson constructed a Cathode Ray Tube (like the one pictured on the front of your note packet) filled with gas at very low pressure. When a high voltage is applied to the electrodes, a glowing beam is projected toward the fluorescent screen, creating a pinpoint glow. The position of the glow shows that the beam is deflected down when the magnet is put in place and up when a charge is applied to the plates near the fluorescent screen. 13. William Crookes had already demonstrated the deflection of the beam caused by the magnet. The deflection established an important fact about the glowing beam. Why was the deflection significant? _____________________________________________________________________________________________ 14. After passing the magnet, the beam is redirected by the field between the charged plates. What is the significance of the fact that the beam is deflected up toward the positively charged plate? _____________________________________________________________________________________________ _____________________________________________________________________________________________ 15. The model of the atom proposed by John Dalton had to be considerably altered to account for the discoveries of J.J. Thomson. What is the major difference between Dalton’s model and the model proposed by Thomson? _____________________________________________________________________________________________ _____________________________________________________________________________________________ 16. Thomson’s model of the atom allows an atom to gain a net electrical charge. What is a charged atom called, and how is it different from a neutral atom? _____________________________________________________________________________________________ _____________________________________________________________________________________________ WORKSHEET D Use the periodic table to identify each element described below. 1. atomic number 65 _______________________________________________ 2. 78 protons _______________________________________________ 3. 44 protons and 44 electrons _______________________________________________ 4. atomic number 24 _______________________________________________ 5. 21 protons _______________________________________________ 6. atomic number 55 _______________________________________________ Answer the following questions. 7. Lead has an atomic number of 82. How many protons and electrons does lead have? _____________________________________________________________________________________________ 8. Oxygen has 8 electrons. How many protons does oxygen have?__________________ 9. Zinc has 30 protons. What is its atomic number?______________________________ 10. Astatine has 85 protons. What is its atomic number?___________________________ 11. Nobelium has an atomic number of 102. How many protons and electrons does it have? _____________________________________________________________________________________________ TRUE/FALSE For each statement below, write true or false. _______________ 16. The number of neutrons in an atom is referred to as its atomic number. _______________ 17. The periodic table is arranged by increasing atomic number. _______________ 18. Atomic number is equal to the number of electrons in an atom. _______________ 19. The number of protons in an atom identifies it as an atom of a particular element. _______________ 20. Most atoms have either a positive or negative charge. COMPLETE Complete the following table. Element Symbol Atomic # Mass # How Many? Name Protons 26 S Neutrons 56 32 7 7 146 6 F Electrons 6 19 92 Have You Met Objectives Review Sheet Identify and give the chemical symbols of the elements 1) Give the symbol for a) Silicon _________ b) Copper ________ c) Tin ________ Create a timeline of the development of the atomic model 2) Write the name of the scientist on the left of the line associated with each contribution to the atomic model. 400 BC--Atomos 1803 Atomic Theory 1897 Electron Discovered 1918 Proton Discovered 1938 Neutron Discovered Describe the development and models of the atom over time. Describe in detail the experiments of Democritus, Thomson & Rutherford and how each experiment altered the model of the atom 3) Complete the following table. An example has been done for you. Scientist Experiment(s) How he altered the atomic model Democritus Dalton Franklin/Faraday Thomson Rutherford Describe a cathode ray tube and how it relates to modern times 4) Explain how the anode works to move the electron beam in the following cathode ray tube. Define the laws of conservation of mass and constant composition. 5) Law of Conservation of Mass states: 6) Law of Constant Composition states: 7) If you began a reaction with 15 grams of reactants, how many grams of product would form? Define, locate and determine the charge and relative mass of electrons, protons and neutrons. 8) Complete the following table: Particle Location Relative Charge Relative Mass 0 +1 Neutron List radioactive elements 9) Name two radioactive elements: Explain how scanning tunneling microscopy works 10) Can you see, with your eyes, an atom using scanning tunneling microscopy? Define and use atomic number Define isotopes 11) Match the term with its definition _____ Mass Number A. atoms that have the same number of protons but different numbers of neutrons _____ Atomic Mass B. Weighted average of the masses of the isotopes of an element _____ Atomic Number C. The total number of protons and neutrons in an atom _____ Isotopes D. The number of protons in the nucleus of an atom Write isotopic symbols and isotopic names Use atomic number Calculate mass number 12) Complete the following chart Element/Ion Atomic # Atomic Mass Mass Number H 1 H 2 12 C 6 # of Protons # of Neutrons # of Electrons Element/Ion 7 Atomic # Atomic Mass Mass Number # of Protons # of Neutrons # of Electrons Li 3 35 Cl 17 As 74 Ag 24 60 Mg 12 13) Are any of the atoms in the above table isotopes of each other? If so, which? Determine the atomic mass of an element 14) Calculate the atomic mass of the elements described below. Then use the periodic table to identify each element. Isotope Mass Number Percent Isotope Mass Number Abundance 63 X 63 65 65 X Percent Abundance 69.17 35 X 35 75.77 30.83 37 37 24.23 X Atomic Mass = _________________________ Atomic Mass = ______________________ Element = _____________________________ Element = __________________________ WORKSHEET E--EXTRA CREDIT—ATOMIC DIMENSIONS WORKSHEET © PRENTICE HALL The following examples are designed to help you become more familiar with the size of atoms, which are very, very small! By working through these examples, you may better understand how the parts of the atom are related to one another. What is the size of one atom? 1. It is estimated that about 1 trillion (1,000,000,000,000) atoms would fit into a period at the end of this sentence. If all the atoms were carbon atoms of the same size, and if the period had an approximate volume of 0.000,000,06 cm 3, what would be the approximate size in cubic centimeters of just 1 atom? Now just think how many atoms it would take to make a colon! Answer:_________________________________________________________________ 2. If you inhaled 1000 cm3 of air with one breath, about 200 cm3 would be oxygen. The rest is mostly nitrogen. One molecule of oxygen is about 0.000,000,000,000,000,000,04 cm3 in volume. About how many molecules of oxygen did you just inhale? Answer: ___________________________________________________ (This is not just a lot of hot air!) 3. A nucleus occupies a very small amount of space inside the atom. From the nucleus to an electron is approximately 10,000 times the radius of the nucleus. Imagine the nucleus of an atom to be a ball 10 cm in diameter. How far away from this ball would the nearest hypothetical electron be? Could you throw the ball that distance so it reaches the electron? 4. The atomic mass unit, amu, represents a very small amount of mass and is actually 0.000,000,000,000,000,000,000,001,67 g. Calculate your mass in grams, and then convert your mass to amu. 5. An electron is only 1/1836 the mass of a proton. If your mass was 50 kg, what would be the mass of something 1836 times smaller than you? Try it the other way. What would be the mass of something 1836 times larger than you? WORKSHEET F—EXTRA CREDIT _____ 1. An atom of carbon-12 and an atom of carbon-14 differ in a) atomic number b) mass number c) nuclear charge d) number of electrons _____ 2. Hydrogen has 3 isotopes with a mass number of 1, 2 and 3 and has an average of atomic mass of 1.01. This information indicates that a) equal numbers of each isotope are present b) more isotopes have a mass of 2 or 3 than 1 c) more isotopes have a mass of 1 than 2 or 3 d) isotopes only have an atomic mass of 1 _____3. What is the total charge of the nucleus in a carbon-12 atom? a) -6 b) 0 c) +6 d) +12 c. phosphorus d. silicon _____4. Which substance can be decomposed by chemical means? a. ammonia b. oxygen _____ 5. A dilute, aqueous potassium nitrate solution is best classified as a a. homogeneous compound b. homogeneous mixture c. heterogeneous compound d. heterogeneous mixture _____ 6. Which two substances can not be broken down by chemical change? a. C and CuO b. C and Cu c. CO2 and CuO d. CuO and Cu _____ 7. In 1820, Hans Christian Oersted was presenting a demonstration on electric currents in wires. He was surprised to notice that the current produced a magnetic field around the wire. What is true about his observations? a. His observations were not important because he did not first develop a hypothesis about them b. Other scientists should not consider his observations because they were unexpected. c. Although the observations were unexpected, they could be the basis of future experiments. d. Only expected observations that were part of his demonstrations should be reported. Base your answers to question 8 on the information below. In living organisms, the ratio of the naturally occurring isotopes of carbon, Carbon-12 to Carbon-13 to Carbon-14, is fairly consistent. When an organism such as a woolly mammoth died, it stopped taking in carbon, and the amount of Carbon-14 present in the mammoth began to decrease. For example, one fossil of a woolly mammoth is found to have of the amount of Carbon-14 found in a living organism. 8 State in terms of subatomic particles how an atom of Carbon-13 is different from an atom of Carbon-12.