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1 4 ATOMIC STRUCTURE NOTES __ /__ pts 6 electrons & 6 neutrons? Y N 2. Carb‐14 has 14 Neutron?Y N Anticipatory Response 1. Matter can be divided? Y N 2. Atoms are indivisible? Y N 3. Dalton tests showed that atoms were indivisible? Y N 4. Atoms of the same element are identical? Y N 5. Chemical reactions involve breaking & joining bonds? Y N Anticipatory Response 1.Carbon always has 6 protons, 3. Carbon‐13 has 6 e‐? Y N Small, dense & positive? Y N 5. Sodium has 11 protons? Y N Summary Section: 4.The Nucleus was found to be 1 First Last Name___Per__ Cornell Question & Ans Directions: Make 5 questions & answers that are different than the Anticipatory Response 1.Example: Why was Daltons theory better than Democritus’? Answer: Dalton had experimentation to back his theory. 2. 3. 4. 5. Double Bubble Compare & Contrast COMPARE What is the same about the two? 1__________________________ ___________________________ ___________________________ ___________________________ ___________________________ 1__________________________ ___________________________ ___________________________ ___________________________ ___________________________ What is different about the two? What is the same about the two? 2 What is different about the two? CONTRAST What is different about the two? 1__________________________ ___________________________ ___________________________ ___________________________ ___________________________ What is different about the two? 2__________________________ ___________________________ ___________________________ ___________________________ ___________________________ 2__________________________ ___________________________ ___________________________ ___________________________ ___________________________ 2__________________________ ___________________________ ___________________________ ___________________________ ___________________________ What is different about the two? What is the same about the two? What is different about the two? 3__________________________ ___________________________ ___________________________ ___________________________ ___________________________ 3__________________________ ___________________________ ___________________________ ___________________________ ___________________________ 3__________________________ ___________________________ ___________________________ ___________________________ ___________________________ 2 CONTRAST 05_CTR_ch04 7/9/04 3:26 PM Page 83 Name ___________________________ 4.1 3 Date ___________________ Class __________________ DEFINING THE ATOM Section Review Objectives • Describe Democritus’s ideas about atoms • Explain Dalton’s atomic theory • Describe the size of an atom Vocabulary • atom • Dalton’s atomic theory Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Elements are composed of tiny particles called 2 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Atoms of any one element are 1 . 1. _______________________ from those of any 2. _______________________ 3 3. _______________________ by combining in whole-number ratios. Chemical reactions 4. _______________________ other element. Atoms of different elements can form occur when atoms are 4 . Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 5. Atoms of one element change into atoms of another element during chemical reactions. ________ 6. Atoms combine in one-to-one ratios to form compounds. ________ 7. Atoms of one element are different from atoms of other elements. 3 Chapter 4 Atomic Structure 83 05_CTR_ch04 7/9/04 3:26 PM Page 85 Name ___________________________ 4 Date ___________________ Class __________________ STRUCTURE OF THE NUCLEAR ATOM 4.2 Section Review Objectives • Identify three types of subatomic particles • Describe the structure of atoms according to the Rutherford model Vocabulary • electrons • cathode ray • protons • neutrons • nucleus Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Dalton theorized that atoms are indivisible, but the discovery 1 of particles changed this theory. Scientists now know that 2 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. atoms are made up of electrons, which have a 3 4 ,which have a positive charge; and 6 nucleus, which has a 3. _______________________ , which are 4. _______________________ 5 5. _______________________ of the who discovered the nucleus of the atom. The 7 charge, occupies a very small volume of the atom. In contrast, the negatively charged 2. _______________________ charge; neutral. The latter two particles are found in the atom. It was 1. _______________________ 8 occupy 6. _______________________ 7. _______________________ 8. _______________________ most of the volume of the atom. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ______ 9. According to Dalton’s atomic theory, atoms are composed of protons, electrons, and neutrons. ______ 10. Atoms of elements are electrically neutral. ______ 11. The mass of an electron is equal to the mass of a neutron. ______ 12. The charge on all protons is the same. 4 Chapter 4 Atomic Structure 85 05_CTR_ch04 7/9/04 3:26 PM Page 86 Name ___________________________ 5 Date ___________________ Class __________________ Part C Matching Match each description in Column B to the correct term in Column A Column A Column B ________ 13. electrons a. stream of electrons produced at the negative electrode of a tube containing a gas at low pressure ________ 14. cathode ray b. the central core of an atom, which is composed of protons and neutrons ________ 15. protons c. negatively charged subatomic particles ________ 16. neutrons d. subatomic particles with no charge ________ 17. nucleus e. positively charged subatomic particles Part D Questions and Problems Answer the following questions in the space provided. 18. Which subatomic particles are found in the nucleus of an atom? 19. Which subatomic particles are charged? 86 Core Teaching Resources 5 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 20. Describe Rutherford’s model of the atom, including the location of protons, neutrons, and electrons with respect to the nucleus. How does this model explain the deflections of a beam of alpha particles aimed at a sheet of gold foil? 05_CTR_ch04 7/9/04 3:26 PM Page 87 Name ___________________________ 6 Date ___________________ Class __________________ DISTINGUISHING BETWEEN ATOMS 4.3 Section Review Objectives • Explain how isotopes differ from one another • Use the atomic number and mass number of an element to find the numbers of protons, electrons, and neutrons • Calculate the atomic mass of an element from isotope data Vocabulary • atomic number • mass number • isotopes • atomic mass unit (amu) • atomic mass • periodic table • period • group Key Equations • atomic number number of protons number of electrons • number of neutrons mass number atomic number © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Part A Completion Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. 1 The number of atomic 2 in the nucleus of an atom is the 1. _______________________ of that element. Because atoms are electrically 2. _______________________ 3 in an atom are equal. 3. _______________________ and neutrons in an atom is the mass 4. _______________________ neutral, the number of protons and The total number of 4 number. Atoms of the same element are identical in most respects, but they can differ in the number of 5 5. _______________________ in the nucleus. Atoms 6. _______________________ that have the same number of protons but different mass numbers 7. _______________________ are called The 6 7 . 8. _______________________ of an element is the weighted average of the 9. _______________________ masses of the isotopes of that element. Each of the three known isotopes of hydrogen has 8 proton(s) in the nucleus. The most common hydrogen isotope has mass number of 10 10. _______________________ 9 neutrons. It has a and is called hydrogen-1. 6 Chapter 4 Atomic Structure 87 05_CTR_ch04 7/9/04 3:26 PM Page 88 Name ___________________________ 7 Date ___________________ Class __________________ Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. ________ 11. The atomic number of an element is the sum of the protons and electrons in an atom of that element. ________ 12. The atomic number of an atom is the total number of protons in an atom of that element. ________ 13. An atom of nitrogen has 7 protons and 7 neutrons. ________ 14. Relative atomic masses are expressed in amus. ________ 15. The number of neutrons in the nucleus can be calculated by subtracting the atomic number from the mass number. Part C Matching Match each description in Column B to the correct term in Column A Column A Column B a. atoms that have the same number of protons but different numbers of neutrons ________ 17. periodic table b. weighted average mass of the atoms in a naturally occurring sample of an element ________ 18. mass number c. equals the number of neutrons plus the number of protons in an atom ________ 19. group d. ________ 20. isotopes e. the number of protons in the nucleus of an atom of an element ________ 21. atomic mass unit (amu) f. an arrangement of elements according to similarities in their properties ________ 22. atomic mass g. a vertical column of elements in the periodic table ________ 23. period h. a horizontal row of the periodic table 1 12 the mass of a carbon-12 atom Part D Questions and Problems Solve the following problem in the space provided. 24. Given the relative abundance of the following naturally occurring isotopes of oxygen, calculate the average atomic mass of oxygen. oxygen-16: oxygen-17: oxygen-18: 88 99.76% 0.037% 0.204% Core Teaching Resources 7 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 16. atomic number 8 Identifying Elements & & Their Sub-Atomic Particles Complete the table Isotope Symbol Hydrogen-1 H Atomic # At. Mass 1 1 20 40 p+ n0 e 1 0 1 18 22 6 6 - 4 He Xenon-132 Tungsten-184 32 S 47 61 56 Fe Fluorine-19 41 79 52 197 85 Rb 37 Cl 35 195 15 30 117 31 17 O 14 7 8 9 Subatomic Particles & A.M.U.’s 1. What are the 3 sub-atomic particles? _____________ ______________ _______________ 2. Which of the 3 sub-atomic particles determines which element is present? 3. Which of the 3 sub-atomic particles when different, makes the atom an isotope? What is an isotope? 4. Which of the 3 sub-atomic particles when gained or lost, makes the atom become an ion with a charge? 5. Why is the Bohr model a FALSE picture of the atom? It describes the atoms similar to the pl_________ mo_________ rather a cl_______ or sph________ model. 6. Where is most of the mass of an atom found? 7 Why is there almost no mass found anywhere except in the nucleus? 8. What is the difference between Atomic Mass and Atomic Number? 9. What is an “a.m.u.?” 10. What is the average atomic mass of an element that is found to be 50%, In nature, 99.0 a.m.u.’s & 50% 100.0 a.m.u.’s. Method 1 (50/50) Transition Method 2 (all %’s) (99.0 + 100.0) = _____ ? (99+100) X 1 2 (99 + 100) x 0.5 11. What is Chlorine’s avg atomic mass which is 75% 35.0 amu. & 25% 37.0 12. What is Hydrogen’s average atomic mass if H-1 is 99.985%, H-2 is 0.015% & there is 0% Hydrogen -3? 9 05_CTR_ch04 7/9/04 3:26 PM Page 89 10 Name ___________________________ 4 Date ___________________ Class __________________ ATOMIC STRUCTURE Practice Problems In your notebook, solve the following problems. SECTION 4.1 DEFINING THE ATOM 1. According to Figure 5.2, 100,000,000 copper atoms would form a line 1 cm long. How long would a line formed by 1 107 copper atoms be? Express your answer in millimeters. SECTION 4.2 STRUCTURE OF THE NUCLEAR ATOM 1. A sulfur-32 atom contains 16 protons, 16 neutrons, and 16 electrons. What is the mass (in grams) of a sulfur-32 atom? 2. The mass of a neutron is 1.67 1024 g. Approximately what number of neutrons would equal a mass of one gram? 3. Which statement is consistent with the results of Rutherford’s gold foil experiment? a. All atoms have a positive charge. b. Atoms are mostly empty space. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. c. The nucleus of an atom contains protons and electrons. d. Mass is spread uniformly throughout an atom. SECTION 4.3 DISTINGUISHING BETWEEN ATOMS 1. How many protons are found in an atom of each of the following? a. boron c. neon b. sulfur d. lithium 2. Complete the table for the following elements. Element Number of Protons Manganese 25 Sodium Bromine Number of Electrons Atomic Number Mass Number 39 89 30 11 35 12 45 Yttrium Arsenic Number of Neutrons 33 Actinium 75 227 10 Chapter 4 Atomic Structure 89 11 Isotopes Quiz B 1. What is Carbon’s symbol 2. Write Carbon’s’ 2 smallest isotopes – ex: Li – 6 or Li - 7 3. List the 2 isotopes number of Protons, Electrons & Neutrons. Protons = Electrons = Neutrons = 4. Which isotope is more common? 5. How do you know # 4 above? 6. About what % of the Isotopes weigh 12. 7. Where is most of an atoms wt 8. What occupies most of the volume of an atom. Scientists Discoveries 1. What was Democritus known for? 2. What was John Dalton famous for? 3. What did JJ Thompson discover? 4. What ratio did Millikan find with his oil drop experiment? 5. What did Goldstein find? 6. With his gold foil experiment what did Rutherford conclude about the center of the atom? 7. What did Rutherford conclude about the rest of the atom? 8. What did Chadwick find? 9. What did Mendeleev find? 10. Which scientist in the room only wishes he would discover something important? 11 12Name Per ________ Date COMPLETE THE FOLLOWING TABLE Symbol 58 26 Atomic Number Mass Number 64 158 Number + of p 30 131 55 38 201 80 Number o n Fe 64 96 42 Number of e 52 Mo Hg 2. What sub-atomic particle determines which element is present? 3. In a neutral atom, which sub-atomic particles will always have equal numbers? 4. Where are electrons found? 5. Most of the mass of an atom is found in the …. 6. What is the difference between atomic mass and atomic number? 7. What is an “amu?” 12 13 How Many Protons, Neutrons and Electrons are in Common Elements Classzone.com activity http://www.classzone.com/books/earth_science/terc/content/investigations/es0501/es0501page01.cfm?chapter_no=05 Go to classzone.com. Then go to the earth science book for California and the investigations for Chapter 5 or search ES0501. Answer the questions below. 1. What elements are in these common items? Diamonds –Carbon ________________ ________________ _________________ _______________ ________________ 2. . Give the mass,charge and location (nucleus or orbit) of each particle in the atom. Name Location Mass Charge Pr______ El_____ Ne______ 3. Fill out the chart for these elements. Name Hydrogen Helium Lithium Beryllium Symbol Atomic # Electrons Neutrons +Protons = Mass # of The isotope Boron Carbon Nitrogen Directions: Forward through the “Next” and “Skip” prompts. Then experiment with the program to answer the questions below: 4. Which particle controls what element an atom is (hint: See which particle when added changes the element name in the info box)?_________ 5. What do you get when you change the number of neutrons in the nucleus? 6. What 2 particles control the mass of an atom(hint: Look at which particle doesn’t change the mass)?_____________________________________________________________________ 7. What happens when you cluster the electrons or move them into another level? They r______. Why do they behave the way they do?____________________________________________ 8. What do you get if the # of protons and electrons in your model differ? An un_________ _____. 9. Fill out the chart for these elements, Name Symbol Atomic # Electrons Neutrons +Protons Oxygen Flourine Neon Alumimum Iron Gold = Mass # of The isotope Bonus -AvgAtomicMass 15.9994 _________ ________ ___________ 13 ___________ ___________ 14 _________________ Cartoon Lab Safety Questions 1. 3. List 3 unsafe activities shown in the picture and explain why each is unsafe. a. ________________________________________________________________ __________________________________________________________________ b.________________________________________________________________ __________________________________________________________________ c.________________________________________________________________ __________________________________________________________________ List 3 correct lab procedures in the picture. a. ________________________________________________________________ __________________________________________________________________ b.________________________________________________________________ __________________________________________________________________ c.________________________________________________________________ __________________________________________________________________ What should Bob do after the accident? 4. What should Sue have done to avoid an accident? 5. 8. Compare Luke and Duke’s lab techniques. Who is following the rules and how? a. Luke -______________________________________________________ ____________________________________________________________ b. Duke -______________________________________________________ ____________________________________________________________ What are 3 things shown in the lab that should not be there and why? a. ________________________________________________________________ __________________________________________________________________ b.________________________________________________________________ __________________________________________________________________ c.________________________________________________________________ __________________________________________________________________ Compare Joe & Carl’s lab techniques. Explain who is doing it correctly and why? a. Joe -______________________________________________________ ____________________________________________________________ b. Carl -_______________________________________________________ ____________________________________________________________ What will happen to Ray and Tim when the teacher catches them? 9. List 3 items in the picture that are there for the safety of the students in the lab. 10. What is Betty doing wrong? 11. Which one of the good actions in the picture will be easy for you to do correctly? 12. Honestly, which one do you think you may not follow correctly? 2. 6. 7. 13. How might you plan or prepare yourself so that you will do the above correctly? ________________________________________________________________________ ________________________________________________________________________ ________________________________________________________________________ 14 Cartoon on Lab Safety 2 of 3 15 http://www.biologycorner.com/worksheets/safety.html Questions: 15 8/16/2010 8:33 AM 16 4 & 25 Jeopardy 1-100 DALTONS THEORY OF INDIVISIBLE ATO MS STOOD THE TEST OF TIME. 1-200 Who DID THE GOLD FOIL EXPERIMENTAND FOUND THAT ATOMS HAVE POS+TIVE CEN+ERS SURROUNDED BY MOSTLY E M P T Y S P A C E! a. J. J. Thompson b. Robert Millikin 1-300 Who discovered the electron. c. Rutherford d. Heisenberg e. Bohr 1-400 Who used the equation E = m C 2 to calculate the amount of energy released in nuclear reactions. 2-100 Which is an element?_______ Which is an element and molecule? _______ Which is a compound.____ 2-200 Which is the most accurate to describe the mass and charge of the proton electron & neutron a. 1 +1 0 -1 0 1 b. 1 -1 1 -1 1 0 c. 1 1 2 -1 0 0 d. 1 +1 0 -1 1 0 2-300 What particles are in the nucleus? 2-400 What particles are added to make the mass number? 2-500 How many neutrons does Sodium usually have? Why is the atomic mass not a whole number like 23? 3-100 Fission or Fusion Which happens on the sun? 3-200 Fission or Fusion Splitting of the atom, like Uranium in the 2 bombs on Japan in WWII. 3-300 Fission & Fusion Hydrogen changing into Helium 3-400 An element is 50% with a mass of 35 a. m. u. and 50% with a mass of 36 a. m. u. What should it’s atomic mass be listed as?_________What element is it? ________ 3-500 The mass number is: a) The number of protons + neutron b) Th # of protons + electrons c) The number of electrons + neutrons d) The atomic number + protons 4-100 The isotopes of Hydrogen each have 1 proton but differ in their number of electrons. 4-200 When Iodine release an electron (or beta particle), its atomic mass a. increases b. Remains the same c. decreases d. Can’t be determined 4-300 Elements have different isotopes.This is why on P.Table average ________ ______ has decimals. 4-400 Using the 2 Atomic Mass numbers, explain why the particle released must be an electron. 4-500 Looking at Sulfur on the Periodic Table, if Sulfur-32 is the most abundant form, what other 2 forms are more likely. a. 28, 29 b.30, 31 c. 32, 33 d. 63, 64 5-100 The # of Protons electrons & neutrons for the smaller Potassium Isotope is a. 20, 19, 19 b. 19, 19, 20 c. 19, 19, 19 d. none correct 5-200 If the atomic number is 50 & mass number125,whats the # of Protons, Electrons & Neutrons?What element? 5-300 The mass & charge of gamma is: ______ ______ 5-400 The change in atomic mass when beta is released is? +4, -4, +2, or -2 5-500 What is the least and most penetrating form and radiation?______ _______ Explain Why? 6-100 What particle is released w/ alpha? A. proton B. neutron C. 2 neutrons & 2 electrons D. helium nucleus 6-200 What unit is used to measure the average atomic mass of an element’s isotopes? 6-300 What is the symbol for tritium or Hydrogen – 3? ____ (ex: 6 C) 6-400 What is the difference between mass number and average atomic mass? 6-500 Alpha Decay changes the atomic mass & atomic number by A. Increase by 2 increase by 2 B. Increase by 4 Decrease by 2 C. Decrease by 4 Decrease by 2 D. Decrease by 0 Increase by -1 7-100 Chlorine -35 & C1-37 are the 2 Isotopes. Which isotope is more abundant? How do you know? 7-200 All atoms of the same element must have the same A. mass B. electrons & protons C. mass number 7-300 What is the smallest particle of an element that retains the properties of that element? a.electron b.Atom c.element d.proton e.electron 7-400 Which 2 ideas of Daltons’ Atomic Theory had to be revised and explain why for each reason? 7-500 Lithium – 6 is 10.0% of the total Lithium found. Lithium – 7 is 90.0%. What is the avg. atomic mass of Lithium? 8-100 How many protons has: Carbon-14? Carbon-13? Carbon-12? 8-200 After 2 half-lives how much radioactive material is left (in %) and explain? 8-300 How many neutrons does Uranium give off in a nuclear chain reaction? 8-400 Why doesn’t a Uranium bomb go off early. 10-500 Why would Uranium be a bad radio Isotope for medicine? How to get the best score on the test? 1. Take the above info & study it. 2. Highlight it. 3.Write the info on test help sheet.Review packet. 4. Do practice test on my website: http://staff.hartdistrict.org/bscott/PracticeTests/practicetests.htm 5. Ask teacher about anything you don’t understand, read over in Chapters 4 & 25 in the textbook. 16 17 18 F 9 20 19 F F 9 Combined Isotopes 21 9 F 9 9 F 4 Different Flourine Isotopes ___________________________ First Name, Last ________ Period SCORE: ___/10 pts 18.998 4 Atomic Structure Formal Assessment 3 Directions: Circle the best answer for each question. 1. How many protons does Flourine – 18 have? 9 18 19 2. How many protons does Flourine – 19 have? 9 X X 3. What is the atomic number of Flourine -19? 9 18 19 4. What is the average Atomic Mass of Flourine? 18 19 neither 5. How many positive charges does Oxygen have in its’ nucleus? 8 18 it varies 6. How many Atomic Mass Units (a.m.u.) is the heaviest Flourine Isotope? 18 19 20 21 7. Atomic Mass Units are made up of: 8. How many electrons does the lightest Flourine have? Protons Neutrons Both 8 18 9 True or False 9. The name of the heaviest shown Flourine Isotope is Flourine 18.998. 10. In Flourine – 18, the 18 stands for how many particles (protons and neutrons) are in the nucleus), while the 9 stands for how many protons it has in the nucleus. Bonus (circle the best answer). 11. What is the difference between atomic mass and atomic number? a. Atomic Number is a whole number. b. Atomic Mass is an average of the masses of all the isotopes. c. Atomic Mass is a decimal because it is an average d. All above answers are correct 17 18 15 O 8 17 16 O O 8 18 8 Combined Isotopes O 8 8 O 4 Different Oxygen Isotopes ___________________________ First Name, Last ________ Period SCORE: ___/10 pts 15.999 4 Atomic Structure Formative Assessment 2 Directions: Circle the best answer for each question. 1. What is the average Atomic Mass of Oxygen? 8 15.999 Neither 2. How many protons does Oxygen have? 8 15.999 It varies 3. How many positive charges does Oxygen have in its’ nucleus? 8 15.999 It varies 4. What is the Atomic Number of Oxygen? It varies 5. How many Atomic Mass Units (a.m.u.) is the heaviest Oxygen Isotope? 8 16 18 6. How many neutrons does the lightest Oxygen Isotope have? 7 8 9 7. How many electrons does the heaviest Oxygen have? 7 8 16 8. How many electrons does the lightest Oxygen have? 7 8 16 8 15.999 True or False 9. The name of the heaviest shown Oxygen Isotope is Oxygen -18. 10. The name of the lightest Oxygen Isotope shown is Oxygen -8. *Bonus 11.__Atomic Mass is the average mass of the 3 isotope, resulting in a decimal but Mass Number is the mass of one of the isotopes, resulting in a whole number. 18 19 ___________________________ First Name, Last ________ Period SCORE: ___/10 pts Atomic Structure Formal Assessment 1 Circle the correct answers 1. How many protons does Carbon – 12 have? 3 6 12 13 14 2. How may protons does Carbon – 13 have? 3 6 12 13 14 3. What is the atomic number of Carbon -12? 3 6 12 13 14 4. What is the atomic number of Carbon-13? 3 6 12 13 14 5. How many neutrons does Carbon – 12 have? 6 7 8 13 14 6. How many neutrons does Carbon – 13 have? 6 7 8 13 14 Write True or False in the blank 7. Carbon has 3 isotopes which differ in their number of neutrons. The Carbon – 12 has 12 – 6 = 6 neutrons. Carbon – 13 has 13 – 6 = 7 neutrons. 8. Most of the mass of all the isotopes are in the center or nucleus because the electrons almost weigh zero. 9. Protons and Electrons have the same positive charge while neutrons have a neutral charge. 10. The nucleus is filled with negative charges which hold together because of The stronger nuclear forces between all the nuclear particles. 19 20 ___________________________ Name ________ Period SCORE: ___/10 pts Science Rules Formal Assessment 1 Multiple Choice – Circle one or more as directed 1. Circle 3 things that shouldn’t be out/visible in class and will be taken away. a. gum b. food/drink c. water d. phones e. ipod/mp3… f. calculator 2. Circle 3 things that will cause loss of points. a. Being out of seat when bell rings. b. Not covering answers during a test. c. Using a calculator on a test d. Turning in homework a few minutes late or forgetting to write name. e. Raising ones’ hand before speaking or answering a question. 3. What times can one make up tests & quizzes? (pick 1) a. anytime b. Tuesday intervention c. Wednesday and Friday Lunch d. ASAP (in the following days) during the above b & c answers e. 2-5 weeks after the assignment was due during Tues/Wed./Friday lunches Write True or False 4. Extra point quizzes are only given on the day of correcting homework. 5. Mr. Abouaf will drop the lowest “Zero” earned. If none he will drop the lowest other grade. 6. Absent students are responsible for finding out missing work, quizzes, tests from others. 7. Students can talk to Mr. Abouaf or be out of their seat during roll call, as long as they are in the class room. 8. Intervention will be Tuesdays after school from 3:05 to 4:05 for 1 point extra credit. 9. Students are allowed to complain about food or drink being thrown in the trash because They forgot, didn’t know or were never told. 10. Test help sheets can be used on make up tests. 20