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4 The Structure of the Atom ffi*sGi[i[:1 Write the Big ldea for this chapter. Use the "What I Know" column to list the things you know about the Big ldea. Then list the questions you have about the Big ldea in the "What I Want to Find Out" column. As you read the chapter, fill in the"What I Learned"column. Whot KWL Know I What t Wont to Find Out o E B g = @ o Science Notebook . The Structure of the Atom 53 What I Learned 4 The Structure of the Atom 1 Early ldeas About Matter t?fit3(F),6(A) rUAIN IDEA Write the Main ldea for this lesson. *strs=u, VocaeuLaxv Recall the definition of the Review Vocabulary term. theory theonl frlsw Voe*BUTARY Define each New Vocabulary term. Daltont atomic theory Dalton's alomictheonl Science Notebook. fhe Structure ofthe Atom 54 1 Early ldeas About Use with pages 102-104. Matter (continued) Summarize the effect that Aristotle had on the atomic theory proposed by Democritus. lnfer why it was hard for Democritus to defend his ideas. List the main points of Dalton's atomic theory. 1. 2. 3. 4. 5. . .'' : t': 'r' Compare and contrast Democritus' and Dalton's Science Notebook . The Structure of the Atom 55 ideas. 1 Early ldeas About Matter Use with page 104. (continued) Discuss Dalton's ideas by completing the following paragraph. studying accurately determine the , Dalton was able After years of reactions. His conclusions resulted in , of the elements involved in the the , in chemical reactions separate, explain that to which helped to ,ol ,ol but are not created, Compare and contrast the atomic theories of Democritus and Dalton. Mark an X under each name if a statement applies to that person's theory. Statement Democritus Dalton All matter is made of tiny pieces. Matter is made of empty space through which atoms move. Atoms cannot be divided. Atoms cannot be created. Atoms cannot be destroyed. Different atoms combine in whole-number ratios to form compounds. The properties of atoms vary based on shape, size, and movement. o :. @ Different kinds of atoms come in different sizes and shapes. @ 3 c { = m o n. I The experiments of the alchemists revealed the properties of some metals and provided the foundation for the science of chemistry. Although not successful, alchemy proved beneficial to science. Explain how this example can be applied to modern research. Science Notebook. The Structure ofthe Atom 56 1 Early ldeas Ahout Matter (continued) RTVIEW [T'! 1. MAINIDEA Contrast the methods used by the Greek philosophers and Dalton to study the atom. 2. Define atom using your own words. 3. Summarize Daltont atomic 4. theory. Explain how Dalton's theory of the atom and the conservation of mass are related. 5. Apply of Element A combine with eight atoms of Element B to produce six compound particles. How many atoms of Elements A and B does each particle contain? Are all of the atoms used to form compounds? Six atoms .F -t s6. E @ -a Design a concept map that compares and contrasts the atomic ideas proposed by Democritus and John Dalton. o Science Notebook. The Structure ofthe Atom 57 4 The Structure of the Atom 2 Defining the Atom IEl3(F),6(A) [vHAtFd it_rIA Write the Main ldea for this lesson. ilevrew Voceu*LsRc Recall the definition of the ReviewVocabulary term. model model Stlsw UceaBilrARY Define each New Vocabulary term. atom atorn cathode ray calhode ray electron nucleus proton electron neutron nucleus proton -9 =. o neutron = 6| il t = g Use with pages 106-107. , 6 Explain an atom by completing the following statements. The atom is the When a group of atoms , the result is known as a Science Notebook . The Structure of the Atom 58 and act as a 2 Defining the Atom Use with pages 107-'l 10, (continued) Summarize the information you learned about cathode ray experiments. Use Figure 7 for reference. Cathode Ray Experiment Altering the gas in the tube and the material used for the cathode have no effect. Proves: Cathode ray is deflected toward the positively charged plate by an electric field. Cathode ray is deflected in a magnetic field. Proves: lndicates: #ffifl !'tr=f Explain how the cathode ray was discovered. o E E i = ttl+r', --'fl-"hair*.i i, i Summarize howThomson discovered the electron. (, = @ 3 .9 Science Notebook. The Structure ofthe Atom 59 2 Defining the Atom Use with pages 1 10-114. (continued) ldentify the major discoveries about subatomic particles made by the 1 9th century. 1. 3. QeT [T.? Explain whyThomson's model was called the plum pudding model. Describe Rutherford's model of the atom by completing the following statements. 1. Most of an atom consists of moving through 2. The electrons are within the atom by their to the positively charged 3. of many times The volume deT [T? through which the electrons move than the volume of Describe Rutherford's model of the the is S .: g atom. a ; ,= I + E o 9' Science Notebook . The Structure of the Atom 60 2 Defining the Atom Use with pages 1 10-1 14. (continued) Organize the properties of subatomic particles by completing the table below. Use Table 3 for reference. Proton Electron Neutron Symbol in nucleus Location Relative 1+ electrical charge Summarize what you have learned about subatomic particles by completing the following paragraph. Atoms have of of an atom is made up shape. The a that have a positive charge and of the mass of an atom. .The nucleus makes up Most of the area of an is made up of negatively charged traveling around the are held in place by their the that have no charged nucleus.The to the positive charge of of the protons and neutrons are almost .The to each other while the o f T 3 g \, = @ 'E o Science Notebook . The Structure of the Atom 61 of the electrons is 2 Defining the Atom (continued) REVIEW IT! 7. MAINIDEA Descibe the structure of a typical atom. ldentify where each subatomic particle is located. 8. Compare and contrastThomsont plum pudding atomic modelwith Rutherfordt nuclear atomic model. 9. Evaluate the experiments that led to the conclusion that electrons are negatively charged particles found in all matter. n ao 1O. Compare the relative charge and mass of each of the subatomic particles, E @ 3 o il I- h = c G o 1 1. Calculate What is the difference expressed in kilograms between the mass of a proton and the mass of an electron? Science Notebook. The Structure ofthe Atom 62 4 The Structure of the Atom 3 How Atoms Differ EtB6(D) IVEAIN iL]EA Write the Main ldea for this lesson. Rrvrrw llocnsurnns Recall the definition of the ReviewVocabulary term. periodic table periodictable Nsw VocnsuLARY Define each New Vocabulary term. atomic number alomic number isotope mass number atomic mass unit (amu) isolope atomic mass mass number atomic mass unrl (amu) .9 f ! U atornic mass T i g g = @ E _9 ' o Ae*trgmrc€$eABUt**Y Define the following term. specific specitic Science Notebook . The Structure of the Atom 63 3 How Atoms Differ ( continued) Use with pages 1 l5-'l 16. Explain how to use an atomic number to identify an element by completing the paragraph below. Each of an element has a unique number the overallcharge of an atom the number of of . lf . is of the number Atomic number : number . of equals : of Since number you know how many one of the three an atom contains, you also know the other the . Once you know the , can be used to find the name of the Solve Read Example Problem 1 in your text. Problem Given the following information about atoms, determine the name each atom's element and its atomic number. a. Atomt has1l protons of b. Atom2has2Oelectrons 1. Analyze the Problem Apply the relationship among atomic number, number of protons, and number of electrons to determine the name and atomic number of each element. 2. Solve for the Unknown a. Atom 1 : Atomic number : : electrons : number of electrons The element with an atomic number of 1 is Atomic number number of protons number of 1 b. Atom 2 : : Atomic number = number of protons : The element with an atomic number of Atomic number 3. number of protons number of electrons is Evaluate the Answer The answers agree with and element given in the periodic table. Science Notebook. The Structure ofthe Atom 64 ,g ,E, 6 F i E I g 3 How Atoms Differ (continued) Use with pages 1 17-118. Review your understanding of isotopes and mass number by completing the following paragraph. lsotopes are elements with but with . The number of neutrons can be determined by the atomic numberfrom the The mass number . Solve is Read Example Problem 2 in your text. Problem You are given two samples of carbon. The first sample, carbon-12, has a mass number of 12, the second sample, carbon-l3, has a mass number of 1 3. Both samples have an atomic number of 6. Determine the number of protons, electrons, and neutrons in each sample. 1. Analyze the Problem Known: Carbon-l2 Mass number is Atomic number is Carbon-I3 Mass number is Atomic number is Unknown: o I ! - The number of protons, electrons, and neutrons in each sample. 2. Solve for the Unknown Number of protons : I number of electrons : - Number of neutrons : The number of neutrons for carbon-l3 : .9 o o mass number atomic number : atomic number E 3 o : The number of neutrons for carbon -12 13 12 : 6: 6 3. Evaluate the Answer The number of neutrons does equal the , or the number of protons. Science Notebook . The Structure of the Atom 65 the minus 3 How Atoms Differ (continued) Use with pages 1 19-121 I .i I r' , ,' Explain how to calculate atomic mass. Summarize Fill in the blanks to help you take notes while you read Example Problem 3. Problem in the table in the left Given the lsotope Abundance for Element X lsotope Mass Percent (amu) abundance 6x 7x 6.015 7.016 of unknown element , margin, the the unknown X. Then, to treat some which is used 1. Analyze the problem Unknown: Known: 7.59o/o For isotope 92.41o/o 6X: ofX:?amu of element X MASS: : abundance: For isotope 7X: mass: abundance : 2. Solve for the unknown Masscontribution:( 6X: For Mass contribution : 7X: For Mass contribution : )( : : o ! @ =. Sum the mass contributions to find the atomic mass. of X: { = [' to identify the element. Use the The element with an atomic mass of 6.939 amu 3. o = 6' is Evaluate the answer The number of neutrons does equal the the , or number of Science Notebook. The Structure ofthe Atom 66 MINUS 3 How Atoms Differ (continued) AFr.l#rlr ld:u.vt&w il 'fg ! 20. MAINIDEA Explain howthe type of an atom is defined. 2I. Recall Which subatomic particle identifies an atom as that of a particular element? 22. Explain how the existence of isotopes is related to the fact that atomic masses are not whole numbers. 23. Calculate Copper has two isotopes:Cu-63 (abundance and Cu-65 (abundance :3A.8a/o, mass : -- 69.20/o, mass : 62.930 amu) 64.928 amu). Calculate the atomic mass of copper. 24. Calculate Three magnesium isotopes have atomic masses and relative abundances 23.985 amu (78.99o/o),24.986 amu (10.00o/o), and 25.982 amu (1 1.01o/o), Calculate the atomic mass of magnesium. o I g = u = @ .E1 d o Science Notebook. The Structure ofthe Atom 67 of 4 The Structure of the Atom 4 Unstable Nuclei and Radioactive DecaY ffi3(F),12(A) Mse$tW i*i:A Write the Main ldea for this lesson. #svrcre €*<e+a:a**v Reca!lthe definition of the ReviewVocabulary term' element elemenl H=*r W*cs=sL&eY Define each New VocabularY term. radioactivity radioactivity radiation radiation nuclear reaction nuclear reaction radioactive decay alpha radiation alpha particle radioaclive decay nuclear equation beta radiation alpha radiation beta particle gamma ray alpha pavticle nuclear equafion bda radiation beta particle gamma raY Science Notebook . The Structure of the Atom 68 4 Unstable Nucleiand Radioactive Decay (continued) REVIEW tri 25. MAINIDEA Explain how unstable atoms gain stability. 26. State what quantities are conserved when balancing 27. Classify a nuclear reaction. each of the following as a chemical reaction, a nuclear reaction, or neither. a. Thorium emits a beta particle. b. Two atoms share electrons to form a bond. c. A sample of pure sulfur emits heat energy as it slowly cools. d. A piece of iron rusts. 28. Calculate How much heavier is an alpha particle than an electron? Create a table showing how each type of radiation affects the atomic number and the mass number of an atom. ( a c Science Notebook . The Structure of the Atom 70 4 Unstable Nuclei and Radioactive Decay (continued) Use with pages 122-124. Explain radioactivity by completing the paragraph below. ln chemical reactions, atoms maY be do not change. The the , but their rearrangement only of the atoms, not the reactiohs are different. In nuclear reactions, gain stability by emitting . As a result change. in the nuclei, the atoms' will continue emitting called , of , until stable nuclei, often of in a process a formed. , are Sequence the steps of a nuclear reaction. A stable, nonradioactive atom is formed. Radiation is emitted. The process of radioactive decay continues until the nucleus stable. is An atom has an unstable nucleus. Distinguish between alpha, beta, and gamma radiation by completing the table below Radiation Type Alpha symbot Mass " (amu) (l Beta Gamma H") 1 Charge /1840 0 Discuss why some elements are radioactive while most elements are not. Science Notebook.The Structure ofthe Atom 69