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APPLIED CHEMISTRY, MS. WACK UNIT B—ATOMIC STRUCTURE DAILY PLANNER DAY 1 10/26 2-4 5 6-7 8 9 10 Tent. 11/8 CLASSWORK Indirect Observation and the Atom Activity (10 Points) Atomic Models (12 Points for Classwork) -10 Points Possible for Atom Poster -10 Points Possible for Technology Connection Daily Quiz Atomic Structure (4 Points for Classwork) Daily Quiz Isotopes and Atomic Mass (8 Points for Classwork) -15 Points for Atomic Mass Lab Homework Packets Due (50 Points) Daily Quiz (25 Points) Review for Test Review for Test HOMEWORK Do definitions for vocabulary terms HW1: Worksheet A HW2: Worksheet B HW3: Worksheet C HW4: Worksheet D Unit B Test (100 Points) Homework Grades 20/20 (A) 4/4 Homeworks Complete 15/20 (B) 3/4 Homeworks Complete 10/20 (C) 2/4 Homeworks Complete 0/20 (F) Less than 2/4 Homeworks Complete Congratulations to the following top pairs for Chapter 1: Period 1: Kile Vierling & Ben Rhodes Period 2: Levi McCord & Ben Uhl Period 8: Johnny Watson & Micah Fick Total Possible Points this Chapter: 244 Points + 15 Extra Credit Points 1st Quarter Ends November 9, 2011 Extra Credit 5 Points: Worksheet E 5 Points: Workhseet F 5 Points: Read the article “Searching for the 6th, Tevatron reveals truth about particles” and answer the questions on Worksheet G WORKSHEET A Thomson’s Experiment Revisited While Fred was babysitting his younger brother, Phil, he noticed that Phil was trying to stick a magnet on the screen of their black-and-white television. The magnet did not stick to the glass, but the picture seemed to be distorted. The closer he held the magnet to the screen, the more the images bent. Fred asked Phil if he could try an experiment with the magnet. When Fred touched the magnet to the screen, the image curved away from the magnet in one direction. When he turned the magnet around and tried again, the image curved away in the other direction. When he waved the magnet back and forth across a part of the screen, the distortion in the images followed the magnet. (CAUTION: Do not try this activity on your own television screen at home.) 1. The image on a television screen is produced when electrons hit the phosphorus coating and cause it to glow. Why did Fred’s magnet affect the image on the screen? __________________________________________________________________________________________________ __________________________________________________________________________________________________ __________________________________________________________________________________________________ 2. Why did the image curve away from the magnet in a different direction when the magnet was reversed? __________________________________________________________________________________________________ __________________________________________________________________________________________________ __________________________________________________________________________________________________ 3. If Fred had two bar magnets, could he have placed them near the screen without causing any distortion in the image? Explain. __________________________________________________________________________________________________ __________________________________________________________________________________________________ __________________________________________________________________________________________________ 4. Describe the effects a stronger magnet would have had on the television image. __________________________________________________________________________________________________ __________________________________________________________________________________________________ __________________________________________________________________________________________________ 5. How is this experiment similar to the experiment J.J. Thomson did to discover the electron? __________________________________________________________________________________________________ __________________________________________________________________________________________________ __________________________________________________________________________________________________ WORKSHEET B MATCHING Match the following with the definitions/ideas/theories given. Write the letter which corresponds to the answer on the line. The same answer may be used more than once. _____ 1. He said that electrons can be found in energy levels. A. Dalton _____ 2. The word atom came from him (“atomos”) B. Thomson _____ 3. He found that cathode ray particles are negatively charged particles C. Bohr called electrons _____ 4. He said that each atom contains a small, dense, positively charged D. Rutherford central portion or nucleus E. Democritus _____ 5. He said that electrons around the nucleus like planets move around the sun _____ 6. He gave the Plum-Pudding Model _____ 7. He did the gold foil experiment. _____ 8. These two scientists said that the atom is indivisible and indestructible. _____ 9. Stated that all atoms of a given element are identical, but they differ from every other element 10-11 DIAGRAMS: Draw a diagram of 2 of the 4 models described in the table below. Thomson’s Plum Bohr’s Planetary Model Rutherford’s Model Bohr’s Model Pudding Model Diagram of Model 12. Above is a Cathode Ray Tube like that used in J.J. Thomson’s experiment. The black lines in the cathode ray tube seen above represent beams of light in that cathode ray tube. What charge does this beam of light have? Why? 13. Choose two models of the atom and describe how they differ from each other. WORKSHEET C 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 Atomic # Mass # How Many? Protons 26 56 16 32 6 Fluorine Neutrons 6 19 61 Iodine Electrons 127 238 146 47 WORKSHEET D Complete the following chart Element/Ion Atomic # Atomic Mass H Mass Number # of Protons # of Neutrons # of Electrons 1 H 1 12 C 6 7 Li 3 35 Cl 17 As 75 Ag 24 61 Mg 12 MATCHING _____ 1. Mass Number A. atoms that have the same number of protons but different numbers of neutrons _____ 2. Atomic Mass B. Weighted average of the masses of the isotopes of an element _____ 3. Atomic Number C. The total number of protons and neutrons in an atom _____ 4. Isotopes D. The number of protons in the nucleus of an atom ISOTOPES OR DIFFERENT ELEMENTS In each of the following statements, you are given a pair of elements and important information about each. Use this information to determine if the pair of elements are isotopes or different elements. Put a check mark in the correct box Isotopes Different Elements Element D has 6 protons and 7 neutrons Element F has 7 protons and 7 neutrons Element J has 27 protons and 32 neutrons Element L has 27 protons and 33 neutrons Element X has 17 protons and 18 neutrons Element Y has 18 protons and 17 neutrons Determine the number of protons, electrons and neutrons for each isotope described below. 5. An isotope has atomic number 19 and mass number 39. Protons = __________ Electrons = _________ Neutrons = ________ 6. An isotope has 14 electrons and a mass number of 28. Protons = __________ Electrons = _________ Neutrons = ________ 7. An isotope has 21 neutrons and a mass number of 40. Protons = __________ Electrons = _________ Neutrons = ________ 8. Which of the atoms in problems 5-7 are isotopes of the same element? Identify the element.___________________________________ WORKSHEET E—EXTRA CREDIT Write the correct answer on the line. _____ 1. What was concluded about the structure of the atom as a result of the gold-foil experiment? a) A positively charged nucleus is surrounded by positively charged particles b) A positively charged nucleus is surrounded by mostly empty space c) A negatively charged nucleus is surrounded by positively charged particles d) A negatively charged nucleus is surrounded by mostly empty space _____ 2. An atom is electrically neutral because the a) Number of protons equals the number of electrons b) Number of protons equals the number of neutrons c) Ratio of the number of electrons to the number of neutrons is 1:1 d) Ratio of the number of neutrons to the number of protons is 2:1 _____ 3. Which two particles make up most of the mass of a hydrogen-2 atom? a) electron and neutron c) electron and proton b) proton and neutron d) proton and positron _____ 4. Which two particles each have a mass of approximately one atomic mass unit? a) electron and neutron c) electron and positron b) proton and electron d) proton and neutron _____ 5. What is the total number of neutrons in an atom of a) 26 b) 31 c) 57 _____ 6. a) b) c) d) 57 26Fe? d) 83 A positive charge will attract another positive charge repel another positive charge repel a negative charge neither attract nor repel a negative charge _____ 7. Electrons were discovered by a) Thomson, in his studies of magnetic and electric fields on cathode rays b) Franklin, in his kite-flying experiment c) Rutherford, in his experiments with alpha-particle beams and gold foil d) Becquerel, in his oil-drop experiment _____ 8. Isotopes contain different numbers of a) electrons b) protons c) neutrons d) nuclei _____ 9. Who first proposed that matter is composed of tiny, indivisible particles? a) Aristotle b) Democritus c) Franklin d) Rutherford _____ 10. Which scientist developed the atomic theory of matter? a) Antoine Lavoisier b) John Dalton c) Aristotle d) J.J. Thomson WORKSHEET F—EXTRA CREDIT In this activity you will explore the concept of weighted averages. Procedure 1. Examine the chemistry test scores listed for Students A & B below. 2. Find the average grade for each student by adding together each student’s scores and dividing by the number of test scores. Place this value in the space provided. Test Student A Student B 1 95 89 2 74 88 3 95 87 4 95 88 5 74 88 6 95 88 Average Grade QUESTIONS 1. If you know a student’s average grade, can you tell what that person’s individual scores were? Explain. __________________________________________________________________________________________________ __________________________________________________________________________________________________ 2. Suppose that student C had an average grade of 88. The student’s individual scores on each test were either 92 or 68. Which score do you think occurred more often. Why? __________________________________________________________________________________________________ __________________________________________________________________________________________________ 3. Suppose that the students’ chemistry teacher decided that Test 6 would count for 50 percent of each student’s final grade and each of the other tests would count for 10 percent of the final grade. Calculate the weighted average for students A and B based on the chemistry teacher’s formula. How do these averages compare to the averages you entered into the table in Step 2. Weighted Average of Student A = _____________ Weighted Average of Student B = ________ __________________________________________________________________________________________________ __________________________________________________________________________________________________ 4. The mass given for each element on the periodic table is also a weighted average. Based on this information answer the following question: There are two isotopes of chlorine, chlorine-35 and chlorine-37. The atomic mass of chlorine given in the periodic table is 35.45. Which of these isotopes of chlorine is most abundant? Explain. __________________________________________________________________________________________________ __________________________________________________________________________________________________ WORKSHEET G EXTRA CREDIT 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.