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Academic Chemistry UNIT 3 BASIC ATOMIC STRUCTURE Monday September 22 29 Notes: Isotopes and Ions (p. 6-7) Tuesday 24 30 Average Atomic Mass (p. 10) October 1 Hwk: pg 11 Hwk: 8-9 6 Start 2nd 6 Weeks Radioisotopes and Nuclear Particles (p. 18) Hwk: pg. 19 Study Guide P. 22-28 13 Wednesday 23 7 Fission and Fusion (p. 21-22) Read Pg. 22 and complete P. 23 Hwk- Finish Study Guide P. 22-28 14 Student Holiday! Thursday Matter and Thermo TEST 6 weeks Cumulative TEST 8 Review Friday 26 History of the Atom (p.3-4) Atomic Structure Notes (p. 2) Hwk: pg 5 2 Lab – Average Atomic Mass (p.12) 3 EARLY DISMISSAL End of st 1 Six Weeks Hwk: pg 13-14 Nuclear Particles Notes (pg 15-16) Hwk- P. 17 9 10 UNIT 3 TEST Start Nomenclature Unit 16 17 Hwk- Study for the Test! 15 PSAT test Name: Class Period: Test Date: Thursday 10/9/14 1 Basic Atomic Structure WARM-UP: Label the following items on the atom at right: Nucleus Electrons Outside the Nucleus Protons Neutrons Complete the following Content Frame: Subatomic Particle Location Charge Mass Electron Proton Neutron NOTES: • Reading the periodic table: • Atomic Number: The number of _____________________________ in an atom. It also equals the number of ___________________________ in a neutral atom. • Mass Number = ______________________ + _______________________ • # of Neutrons = _____________________ – _______________________ • Atomic Mass: The _______________________ of all naturally occurring isotopes. • Use the acronym “APE MAN” to help you remember the above calculations: Atomic number = Protons = Electrons Mass number = Atomic number + Neutrons 2 APE MAN Democritus Dalton Thomson Rutherford Plum Pudding Model Bohr Electron Cloud Model 3 Dalton What year did he publish his atomic theory? Democritus (440 B.C.) What did he call the tiniest piece of matter? What did he propose? List the postulates of his theory. What was missing or wrong with his theory? Rutherford When did he make his discovery? Thomson When did he make his discovery? Describe his experiment. What subatomic particle did he discover? Draw his model. What TWO discoveries did he make about the atom? His model was different from Thomson’s model by thinking that the atom resembles our _________________. New Model View What is the basis of this new model? Bohr When did he make his discovery? He thought electron only traveled in _____________ paths around the nucleus. What is the name for this model? These electrons follow these orbits which he called ________________ _________________. Label the model with the # of electrons in each energy levels: What is the name of his model? 4 Homework: Atomic Models: Count the number of protons, neutrons, and electrons in each Model. Use the Atomic number and the Periodic Table to determine the true identity of the element. Element # of Protons # of Neutrons # of Electrons ATOMIC # MASS # NAME Symbol Zippy WoWie Tigerium 4 5 6 Answer the questions below. 1. How did you determine the name of the element?_____________________________________ 2. One subatomic particle adds no mass to the atom. Which one is it?(see background)___________ 3. Which subatomic particles added together equal the mass #? ____________________________ 4. Using the model of an atom, as in this lab, how do you find the Atomic # of an atom? __________ __________________________________________________________________________ 5. Using the model of an atom, as in this lab, how do you find the Mass # of an atom?____________ __________________________________________________________________________ 6. Conclusion: Write a rule concerning how to identify an atom from its parts. Review History of the Atom: 1. Thomson’s experiments with cathode ray tube led to the discovery of the _________________. 2. Who was the first person to suggest the idea of atoms in the fourth century B.C.? 3. Who stated that electrons do not move about an atom in definite paths but in large regions (clouds) determined by energy? 4. Consider the following selected postulates of Dalton’s atomic theory: Circle the statement(s) below that is (are) no longer considered to be true? i. Each element is composed of extremely small particles called atoms. ii. Atoms are indivisible. iii. Atoms of a given element are identical. iv. Atoms of different elements are different and have different properties. 5. Complete the History of the Atom Timeline 1 Date: 2 3 4 440 BC 5 1831 Inventor: Bohr 5 6 NOTES: Isotopes and Ions WARM-UP: 1. Complete the labels below and fill in the blanks in the statements to the right. NOTES: Isotopes and Ions • Isotopes – Have the same number of __________________________ but a different number of __________________________. – If an atom is an isotope you name it using the element name followed by the ________________________________________. Ex: – Writing Isotope Symbols: 1. Write the atomic symbol for the element. 2. To the top left of the symbol write the mass number of the isotope. 3. Beneath that (to the bottom left of the symbol), write the atomic number of the element. Ex: Label the following: Mass number (protons + neutrons) Element symbol Atomic number (protons) Example of Isotopes: 14 𝐶 6 and 12 𝐶 6 How many protons does Carbon-14 have? How many protons does Carbon-12 have? How many neutrons does Carbon-14 have? How many neutrons does Carbon-12 have? 6 Atoms as a rule are all _______________ in charge, meaning that the number of protons and electrons in the atoms are equal. Ions: Ions are __________________________________ that can only form when an atom ________________________________________________________. Cations Examples: 7 + 3Li Lithium-7 Protons: Neutrons: Electrons: Charge: = Anions Examples: Sulfur-32 Protons: Neutrons: Electrons: Charge: 32 2- = 16S Lab: Beanium Lab: STATE THE PROBLEM: How can you identify an element? BACKGROUND: Atoms are made of the subatomic particles protons, neutrons, and electrons. The atomic number, atomic mass, name, and symbol are on the periodic table . The electrons are so small that they add no mass to the atom. The mass # is the rounded atomic mass from the periodic table, also determined by adding protons and neutrons. HYPOTHESIS: (Answer the problem question above.) ____________________________________ __________________________________________________________________________________ Materials: 10 zip lock baggies, Black beans = Protons, White beans = Neutrons, Popcorn = Electrons PROCEDURE: 1. Count the number of protons, neutrons, and electrons in the bags and record. 2. Return to your assigned seat to complete the data table and answer the questions. 7 DATA TABLE: Complete the data table and then answer the questions below. Bag # # of Protons # of Neutrons # of Electrons ATOMIC # MASS # NAME with mass # Isotope Symbol Neutral atom, Isotope or Ion 1 2 3 4 5 6 7 8 9 10 11 12 1. Which particle did you use to determine the name of the element?_________________________ 2. One subatomic particle adds virtually no mass to the atom. _________________________ 3. Which subatomic particles added together equal the mass #? ___________________ and ____________________ 4. Using the model of an atom, as in this lab, how do you determine if an atom is the neutral version or an ion? ______________________________________________________________ ______________________________________________________________________________ 5. Using the model of an atom, as in this lab, how do you determine if an atom is an Isotope? ______________________________________________________________________________ 6. Conclusion: Write a rule concerning how to identify an atom from its parts. 8 Homework: Isotope, Ion and Atomic Structure 1. What subatomic particle remains the same among isotopes of the same element? 2. What subatomic particle changes among isotopes of the same element? 3. Complete the following table for the neutral atoms: Complete Symbol Element name (including mass #!) Lead-206 Atomic number Mass number 7 # protons #neutrons # electrons 82 7 Use the information below to determine if the pair of elements is a set of isotopes or different elements. Indicate your answer in the space provided: Isotope or different element? 1. Element D has 6 protons and 7 neutrons. Element F has 7 protons and 7 neutrons. 2. Element J has 27 protons and 32 neutrons. Element L has 27 protons and 33 neutrons. 3. Element X has 17 protons and 18 neutrons. Element Y has 18 protons and 17 neutrons. 4. 14 6 X 14 7 and X 5. Element P has an atomic number of 92 and a mass number of 238. Element S has 92 protons and 143 neutrons. Use the information below to determine if the element is an ion or neutral atom. Indicate your answer in the space provided: Ion or neutral atom? 6. Element Z has 6 protons and 6 electrons. 7. Element N has 17 electrons and 18 protons. 8. 9. Element P has 12 protons, 12 neutrons and 10 electrons. 10. Element K has atomic # 7 and 7 electrons. 9 ISOTOPES AND AVERAGE ATOMIC MASS • Compare & contrast Mass Number and Atomic Mass: Elements come in a variety of isotopes, meaning they are made up of atoms with the same atomic number but different atomic masses. These atoms differ in the number of neutrons. The average atomic mass is the weighted average of all the isotopes of an element. Formula for Atomic Mass: Practice Problems: 1. A certain element has two naturally occurring isotopes. Determine the atomic mass given the following data and identify the element. Isotope Atomic Mass Abundance X-35 34.969 amu 75.53% X-37 36.966 amu 24.47% a. Show your work in calculating the average atomic mass of this isotope: b. What element is this? (hint: compare this atomic mass to ones on the periodic table to determine its identity!) 2. Given the following data, calculate the average atomic mass of magnesium. Isotope Atomic Mass Abundance Magnesium-24 23.985 amu 78.70% Magnesium-25 24.986 amu 10.13% Magnesium-26 25.983 amu 11.17% a. Show your work in calculating the average atomic mass of Mg (Magnesium): 10 Homework - Atomic Mass Calculations: 133 132 Example: A sample of cesium is 75.0 % 55 Cs, 20.0% 55 Cs and 5.0% 134 55Cs. What is its average atomic mass? Answer: .750 x 133 = 99.75 .200 x 132 = 26.4 .050 x 134 = 6.70 Total = 132.85 a.m.u. (average atomic mass) Determine the average atomic mass of the following mixtures of isotopes. 1. 80.0% 127 53 I , 17.0% 126 53 I , 3.0% 128 53 I _____________ 2. 50.0% 197 79 Au , 50.0% 198 79 Au _____________ . 3. 15.0% 55 26 Fe , 85.0% 56 26 Fe _____________ . 4. 99.0% 1 1 H , 0.8% 2 1 H , 0.2% 3 1 H _____________ . 5. 95.0% 14 7 N , 3.0% 15 7 N , 2.0% 16 7 N _____________ . 6. 98.0% 12 6 C , 2.0% 14 6 C _____________ . 11 LAB: Average Atomic Mass WARM-UP: Test Average Quiz Average Homework Average 74 82 84 Grading policy is that tests are worth 55%, quizzes worth 30%, and homework worth 15% of your average. 1. Look over the data before you begin the problem. Estimate this student’s average before you begin the calculation. Will his average be closer to 74, 82, or 84? 2. Now, calculate this student’s average according to our grading policy. LAB: AVERAGE ATOMIC MASS Background Information: Mass number is the sum of the protons and neutrons in an atom. The electrons are so small that they do not really contribute to the atom’s mass. Isotopes are atoms of the same element with the same number of protons but a different number of neutrons. The mass you see on the periodic table is the average atomic mass. It takes into account the mass of each isotope of an element and the percent abundance in nature. Procedure: 1. Determine the average atomic mass of fictitious elements. Note: At each station you will see bags. Each little bag represents an atom. DO NOT OPEN THE LITTLE BAGS! 2. Count the total number of bags (atoms) for the element. 3. Separate the bags based on isotope name (labeled on the front of the bag). 4. Count how many bags (atoms) of each isotope. 5. Calculate the percent abundance. (# atoms for each isotope/total atoms) 6. Determine the average atomic mass for the element. (Mass # of the isotope x percent abundance. Add up the total) 7. Determine the number of protons for each element. For Example: Sica-11 Sica-11 Sica-12 Sica-13 Sica-13 1. There are six atoms of the element Sica. 2. I’ve separated them based on the isotope name. 12 Sica-13 3. The data table below was filled in based on the example from the previous page: Isotope Name Sica-11 Sica-12 Sica-13 #3 How many atoms of each isotope? 2 1 3 #4 Calculate Percent abundance 2/6= 33% 1/6= 17% 3/6= 50% Total atoms = 6 #5 Average Atomic Mass 11 x .33 = 3.63 12 x .17 = 2.04 13 x .50 = 6.5 Total = 3.63 +2.04 +6.5 = 12.17 amu GATHER DATA: Sciencetopium Isotope Name How many atoms of each isotope? Calculate Percent abundance Total atoms = Tigerium Isotope Name How many atoms of each isotope? Total = Calculate Percent abundance Total atoms = Katyum Isotope Name How many atoms of each isotope? Average Atomic Mass Average Atomic Mass Total = Calculate Percent abundance Total atoms = Average Atomic Mass Total = 13 Championodium Isotope Name How many atoms of each isotope? Calculate Percent abundance Total atoms = Average Atomic Mass Total = Safarium Isotope Name How many atoms of each isotope? Calculate Percent abundance Total atoms = Superdupium Isotope Name How many atoms of each isotope? Average Atomic Mass Total = Calculate Percent abundance Total atoms = Average Atomic Mass Total = QUESTIONS: (look at the background info for this lab and notes on previous pages to help with these questions) 1. What is an isotope? 2. Why did you have to find the percent abundance? 3. What is the difference between a mass number and an atomic mass? Cumulative Test Tomorrow...Study Units 1 and 2 14 Notes over Radiation What causes nuclear decay? Terms to know: Radioisotopes: Nuclear Reactions: Radiation: Transmutation: Radioactive Decay: 3 Types of Radiation alpha radiation – __________________________________________________________________ __________________________________________________________________ o symbol : beta radiation – __________________________________________________________________ __________________________________________________________________ __________________________________________________________________ o Symbol: gamma radiation – _________________________________________________________________ __________________________________________________________________ o Symbol: 15 Types of Radiation Property Alpha radiation Beta radiation Gamma radiation Composition Symbol Charge Mass (amu) Common Source 1/1837 Radium – 226 Carbon-14 Cobalt - 60 Penetrating power Shielding Review 1. Label the following statements as alpha, beta, or gamma radiation. ____the most dangerous type of radiation ____the largest of the radiation particles ____have a positive charge ____have no mass (multiple answers) ____a helium nucleus ____cannot penetrate paper or clothes ____harmful only when ingested 16 Writing Nuclear Equations A nuclear equation will look like this: 1. 2. Examples: Nuclear Reactions using symbols and word equations. 1. 𝟐𝟑𝟗 𝟗𝟒𝑷𝒖 2. 𝟑𝟕 𝟏𝟗𝑲 3. ______ 𝟔𝟒𝑩𝒆 + 4. Write the equation of lead-210 undergoing alpha decay. 5. Write the equation where lead-210 emits a beta particle. 6. 𝟒𝟐𝑯𝒆 + ______ _____ + Type: ___________ Type: ___________ 𝟑𝟕 𝟏𝟖𝑨𝒓 Type: ___________ 𝟎 −𝟏𝒆 Show the transmutation of uranium-237 as it undergoes alpha decay. What is the nuclide that is produced? 17 Homework Nuclear Reactions 1. Write the nuclear decay equation for the alpha particle decay of 231 91 2. Write the nuclear decay equation for the alpha particle decay of 146 62 3. Write the nuclear decay equation for the beta particle decay of 152 54 Pa . Sm . Xe . 4. Write the nuclear decay equation for the beta particle decay of cesium-120. 5. Write the nuclear decay equation for the gamma particle decay of 142 60 Nd . 6. Which type of nuclear decay is NOT a transmutation reaction? 7. Find the missing part of the equation and label the type of transmutation (alpha, gamma or beta). a. b. 222 86 Rn ____ He 4 2 Type: ______ c. 209 85 At ____ 24He Type: ______ d. 87 37 Rb Sr ____ 87 38 Type: ______ 14 6 C ____ 10 e Type: ______ 18 Fission and Fusion Fission Picture Fusion Picture 19 Nuclear Fission vs. Nuclear Fusion Nuclear f“i”s s i o n (Spl“ i ”tting an atom into two new ones) In nuclear fission reactions (also called radioactive decay), a neutron is aimed at the nucleus of a large, unstable atom, like uranium, thorium, or other radioactive elements. The extra mass of the neutron causes the radioactive nucleus to split apart, forming lighter elements, free neutrons, and great quantities of energy. This process causes convection currents that move Earth’s tectonic plates, and generate earthquakes and volcanic eruptions. Nuclear Fission: Nuclear Source of energy in the core of the Earth that produces heat from the decay of radioactive elements. Produces vast quantities of energy. Does not produce particulate air pollution like fossil fuels and coal. Involves the splitting of harmful radioactive elements. Loss of control leads to harmful radiation exposure. Produces a radioactive waste product that will need to be stored. f“u”s i o n (combining/fusing two atoms together into one new atom) During fusion reactions, nuclei collide and fuse, eventually forming nuclei of heavier elements and producing enormous amounts of energy. Fusion of hydrogen to helium occurs in the sun and is the source for all external weather related events. Nuclear Fusion: Source of energy in the Sun that produces heat from the fusing of elements like hydrogen. Produces unsurpassed quantities of energy. Does not produce particulate air pollution like fossil fuels and coal. Does not produce a radioactive waste product that will need to be stored. Currently, we lack the technology to maintain reactions as a viable energy source. 20 **Write Fission or Fusion next to each of the descriptions below:** 1. Generates a large volume of solid radioactive waste. 2. Occurs in the core of the Earth. 3. The reaction occurs only at extremely high temperatures. 4. Earth’s source in internal energy. (volcanoes, plate motion, geothermal, etc.) 5. The products of this reaction are not radioactive. 6. Occurs only in the core of the Sun. 7. Earth’s source of external energy (atmosphere, oceans, weather, plants, etc.). 8. Also called radioactive decay. 9. Responsible for providing heat for the convection in the interior of the Earth. 10. A potential power source but we lack the technology to maintain the reactions so we are unable to perform these reactions on Earth. 11. The one with a “u” in it._ 12. The one with two “i’s” in it. 13. The one that sounds like “fuse” 14. The one that almost rhymes with “split.” 15. Creates enough energy for the whole Earth (inside and out) 16. Which one you love the most now . 21 and . Atomic Structure and Nuclear Unit 3 Test Review TEST on Thursday 10/9 Parts of the atom: Learning Goals Describe the three subatomic particles: protons, neutrons electrons. Determine the atomic number for any element using the periodic table. Using given information, determine one or more of the following for a neutral atom or ions. o Number of Protons o Atomic Number o Number of Neutrons o Mass Number o Number of Electrons o Complete Atomic Symbol Identify pairs of isotopes. Identify ions. Calculate atomic mass. Determine the most abundant isotope for each element based on its atomic mass. Explain how the theory of the atom has changed over time especially from the contributions of the following scientists. o Democritus o Dalton o Thomson o Rutherford o Bohr Describe major experiments and their effects on the atomic model. o Thomson o Rutherford Describe the current atomic model. Example Questions 1. What quantity identifies an element? A) atomic number B) mass number C) number of neutrons D) number of valence electrons 2. Chlorine-37 can be represented as A) 17 37 B) 37 17 C) 35 20 D) 37 35 Cl Cl Cl Cl 22 3. Which isotope is the basis of the atomic mass unit (amu)? A) hydrogen-1 B) carbon-12 C) carbon-14 D) oxygen -16 4. Which total mass is the smallest? A) the mass of 2 electrons B) the mass of 2 neutrons C) the mass of 1 electron plus the mass of 1 proton D) the mass of 1 neutron plus the mass of 1 electron 5. The diagram below represents the nucleus of an atom. Key Proton = Neutron = What are the atomic number and mass number of this atom? A) The atomic number is 9 and the mass number is 19. B) The atomic number is 9 and the mass number is 20. C) The atomic number is 11 and the mass number is 19. D) The atomic number is 11 and the mass number is 20. 6. Which represents the most abundant isotope of sodium? A) sodium-11 B) sodium-22 C) sodium-23 D) sodium-24 7. What is the total number of electrons in a Mg ion if it loses 2 electrons? A) 2 electrons B) 10 electrons C) 12 electrons D) 14 electrons 8. Which two notations represent different isotopes of the same element? A) 6 4 Be and 49 Be B) 14 6 C) 6 3 D) 31 15 C and 14 7 N Li and 36 Li P and 32 16 S 23 9. What is the total number of neutrons in an atom of 26 Fe ? 57 A) 26 electrons B) 31 electrons C) 57 electrons D) 83 electrons 10. If an element loses or gains electrons, it will form a(an) A) Neutral atom B) Isotope C) Ion D) fluorine 11. How many protons are found in an atom of fluorine? A) 7 B) 9 C) 10 D) 19 12. Which isotope of magnesium is the most abundant? A) magnesium-12 B) magnesium-24 C) magnesium-25 D) magnesium-26 13. In the Modern wave mechanical model of the atom, the orbitals are regions of the most probable locations of the A) protons B) electrons C) neutrons D) positrons 14. Which scientist was the first to indicate that electrons exist in distinct energy levels? A) Thomson B) Rutherford C) Millikan D) Bohr 15. Who discovered the electron? A) Dalton B) Thomson C) Rutherford D) Bohr 24 16. Which A) B) C) D) phrase describes an atom? a positively charged electron cloud surrounding a positively charged nucleus a positively charged electron cloud surrounding a negatively charged nucleus a negatively charged electron cloud surrounding a positively charged nucleus a negatively charged electron cloud surrounding a negatively charged nucleus 17. Complete the following table. Complete Symbol 41 19 23 11 Atomic Number Mass Number Protons Neutrons Electrons Charge K 12 14 30 18 Na -3 18. Showing all your work, calculate the atomic mass for the following element. Identify this element. Isotope Isotope #1 Isotope #2 Isotope #3 Mass (amu) 27.98 28.98 29.97 Percent Abundance 92.22% 4.69% 3.09% 19. Neon-20 accounts for 94.3% of naturally occurring neon. Neon-23 accounts for the remaining 5.7%. Calculate the atomic mass of neon. SHOW ALL WORK! 25 20. Rutherford led to two important discoveries about the atom using his gold foil experiment. For each observation, indicate what he was able to conclude about the atom. A) Observation #1: Rutherford noticed that about 1 in 10,000 of the positively charged particles was deflected. He discovered the _______________________. B) Observation #2: Rutherford noticed that a majority of the positively charged particles went straight through the gold foil and were not deflected. He discovered the _______________________. 21. Complete the labels below and fill in the blanks in the statements to the right. Stop at the directions. DIRECTIONS: Fill in the blank in each box as well as the 6 blanks below it. Use the information provided in each box as well as the isotope name above it. Oxygen-16 Zinc-67 Lithium-6 22. An isotope of an element has an atomic number of 8 and a mass number of 15. How many protons, neutrons, and electrons does this atom have and which element is this? 26 23. If hydrogen has two naturally occurring isotopes, H-1 and H-2 and the atomic mass of hydrogen is 1.0079, then which of these two isotopes of hydrogen is more abundant? Study Guide for Nuclear Chemistry 1. What determines if an atom will be radioactive or unstable? 2. The three principle types of radioactive decay are , , and Use the following answer choices for question 4-16 a. alpha particles b. beta particles c. gamma rays d. alpha and beta particles e. beta particles and gamma rays f. all of the above 3. Described as a fast moving electron 4. Has a positive charge 5. Has no mass or atomic number 6. Changes both the mass number and atomic number in radioactive decay 7. A helium nucleus 8. Electromagnetic radiation 9. Cannot be stopped by human skin or a piece of paper 10. Largest type of radioactive decay 11. Transmutation reaction 12. Most damaging and most penetrating 13. Particle released when carbon-14 changes to nitrogen-14 14. Emission increases the stability of the nucleus 15. Not deflected by any magnetic or electrical fields 16. Write the nuclear decay equation for thorium-230 undergoing alpha decay. 17. Write the nuclear decay equation for 8 3 Li emitting a beta particle. 18. Thorium-234 can undergo beta particle production. What is the other product? 27 . 19. List three positive uses of nuclear chemistry. 20. Identify the following as fission or fusion: Label Type:_______________________ Type: ______________________ 21. List properties of fusion and fission. 28