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05_CTR_ch04 7/9/04 3:26 PM Page 83 Name ___________________________ 4.1 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. Chapter 4 Atomic Structure 83 05_CTR_ch04 7/9/04 3:26 PM Page 84 Name ___________________________ Date ___________________ Class __________________ Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B ________ 8. atom a. an instrument used to generate images of individual atoms ________ 9. scanning tunneling microscope b. Greek philosopher who was among the first to suggest the existence of atoms ________ 10. John Dalton c. the smallest particle of an element that retains its identity in a chemical reaction ________ 11. Democritus d. English chemist and schoolteacher who formulated a theory to describe the structure and chemical reactivity of matter in terms of atoms Part D Questions and Problems Answer the following questions in the space provided. 12. In what type of ratios do atoms combine to form compounds? 84 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 13. How many copper atoms would you have to line up side by side to form a line 1 m long? 05_CTR_ch04 7/9/04 3:26 PM Page 85 Name ___________________________ 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 ,which have a positive charge; and 4 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. Chapter 4 Atomic Structure 85 05_CTR_ch04 7/9/04 3:26 PM Page 86 Name ___________________________ 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 © 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 ___________________________ 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. Chapter 4 Atomic Structure 87 05_CTR_ch04 7/9/04 3:26 PM Page 88 Name ___________________________ 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 © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 16. atomic number 05_CTR_ch04 7/9/04 3:26 PM Page 89 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 Actinium Atomic Number Mass Number 39 89 30 11 35 12 45 Yttrium Arsenic Number of Neutrons 33 75 227 Chapter 4 Atomic Structure 89 05_CTR_ch04 7/9/04 3:26 PM Page 90 Name ___________________________ Date ___________________ Class __________________ 3. How many neutrons are in each atom? a. 23 c. 81 11Na 35Br b. 238 92 U d. 19 9F 4. The two most abundant isotopes of carbon are carbon-12 (mass 12.00 amu) and carbon-13 (mass 13.00 amu). Their relative abundances are 98.9% and 1.10%, respectively. Calculate the atomic mass of carbon. 5. Element X has two isotopes: X-100 and X-104. If the atomic mass of X is 101 amu, what is the relative abundance of each isotope in nature? © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 90 Core Teaching Resources 05_CTR_ch04 7/9/04 3:26 PM Page 91 Name ___________________________ 4 Date ___________________ Class __________________ ATOMIC STRUCTURE Vocabulary Review Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line. Column A © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 1 Column B ________ 1. defined as 12 the mass of a carbon-12 atom a. isotopes ________ 2. central core of an atom, which contains most of the atom’s mass b. neutrons ________ 3. a vertical column of elements in the periodic table c. atom ________ 4. subatomic particles with no charge d. electrons ________ 5. positively charged subatomic particles e. atomic number ________ 6. the smallest particle of an element that retains its identity in a chemical reaction f. atomic mass unit ________ 7. the number of protons in the nucleus of an element g. group ________ 8. negatively charged subatomic particles h. nucleus ________ 9. atoms with the same number of protons but different numbers of neutrons i. periodic table ________ 10. an arrangement of elements according to similarities in their properties j. protons Chapter 4 Atomic Structure 91 05_CTR_ch04 7/9/04 3:26 PM Page 92 Name ___________________________ 4 Date ___________________ Class __________________ ATOMIC STRUCTURE Chapter Quiz Fill in the word(s) that will make each statement true. 1. Dalton’s atomic theory included the idea that the atoms of 1 different elements can chemically combine in ratios. 1. _______________________ 2. An atom is the smallest particle of an element that retains its 2 identity in a . 2. _______________________ 3. 3 are subatomic particles with a negative charge. 4. The nucleus of an atom is composed of 4 3. _______________________ and protons. 5. A neutron has no charge, but its mass is almost the same as 5 that of a . 6. The number of protons in an atom is called its 7. There are 10 neutrons and oxygen-18. 7 6 5. _______________________ number. 6. _______________________ 7. _______________________ 8. Isotopes of an element have different numbers of neutrons. 8 They also have different numbers. 8. _______________________ 9. The total number of protons, neutrons, and electrons in an 9 atom of silver-109 (atomic number 47) is . 9. _______________________ 11. The horizontal rows of the periodic table are called 11 12. The elements in the periodic table are listed in order of 12 . increasing Core Teaching Resources 10. _______________________ . 11. _______________________ 12. _______________________ © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. electrons in an atom of 10. The mass number of an element with 14 electrons and 16 10 . neutrons is 92 4. _______________________ 05_CTR_ch04 7/9/04 3:26 PM Page 93 Name ___________________________ 4 Date ___________________ Class __________________ ATOMIC STRUCTURE Chapter Test A A. Matching Match each description in Column B with the correct term in Column A. Write the letter of the correct description on the line. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Column A Column B ________ 1. proton a. the total number of protons and neutrons in the nucleus of an atom ________ 2. atom b. the weighted average mass of the atoms in a naturally occurring sample of an element ________ 3. mass number c. ________ 4. atomic mass unit d. the number of protons in the nucleus of an element ________ 5. electron e. atoms with the same number of protons but different numbers of neutrons ________ 6. isotopes f. negatively charged subatomic particle ________ 7. atomic number g. the smallest particle of an element that retains its identity in a chemical reaction ________ 8. atomic mass h. a horizontal row of the periodic table 1 12 the mass of a carbon-12 atom ________ 9. period i. subatomic particle with no charge ________ 10. neutron j. positively charged subatomic particle B. Multiple Choice Choose the best answer and write its letter on the line. ________ 11. Which of the following is not a part of Dalton’s atomic theory? a. All elements are composed of atoms. b. Atoms of the same element are alike. c. Atoms are always in motion. d. Atoms that combine do so in simple whole-number ratios. ________ 12. The nucleus of an atom is a. negatively charged and has a low density. b. negatively charged and has a high density. c. positively charged and has a low density. d. positively charged and has a high density. Chapter 4 Atomic Structure 93 05_CTR_ch04 7/9/04 3:26 PM Page 94 Name ___________________________ Date ___________________ Class __________________ ________ 13. Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that a. Dalton’s theories are completely correct. b. atoms of an element can have different numbers of protons. c. atoms are all divisible. d. all atoms of an element are not identical but they all have the same mass. ________ 14. The number of neutrons in the nucleus of an atom can be calculated by a. adding together the numbers of electrons and protons. b. subtracting the number of protons from the number of electrons. c. subtracting the number of protons from the mass number. d. adding the mass number to the number of protons. ________ 15. The sum of the protons and neutrons in an atom equals the a. atomic number. c. atomic mass. b. number of electrons. d. mass number. ________ 16. All atoms of the same element have the same: a. number of protons. c. mass number. b. number of neutrons. d. mass. ________ 17. Which of these statements is false? a. Electrons have a negative charge. b. Electrons have a mass of 1 amu. c. The nucleus of an atom is positively charged. d. The neutron is found in the nucleus of an atom. ________ 19. How do the isotopes hydrogen-2 and hydrogen-3 differ? a. Hydrogen-3 has one more electron than hydrogen-2. b. Hydrogen-3 has two neutrons. c. Hydrogen-2 has three protons. d. Hydrogen-2 has no protons. ________ 20. The number 80 in the name bromine-80 represents a. the atomic number. b. the mass number. c. the sum of protons and electrons. d. none of the above ________ 21. Which of these statements is not true? a. Atoms of the same elements can have different masses. b. The nucleus of an atom has a positive charge. c. Atoms of isotopes of an element have different numbers of protons. d. Atoms are mostly empty space. 94 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 18. An atom of an element with atomic number 48 and mass number 120 contains a. 48 protons, 48 electrons, and 72 neutrons. b. 72 protons, 48 electrons, and 48 neutrons. c. 120 protons, 48 electrons, and 72 neutrons. d. 72 protons, 72 electrons, and 48 neutrons. 05_CTR_ch04 7/9/04 3:26 PM Page 95 Name ___________________________ Date ___________________ Class __________________ ________ 22. Relative atomic masses are measured in a. nanograms. c. angstroms. b. grams. d. amus. ________ 23. If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? 1. 24 12E 2. 24 13E a. 1 and 2 b. 3 and 4 3. 25 11E 4. 25 12E c. 1 and 4 d. 2 and 3 C. Problems Solve the following problem in the space provided. Show your work. 24. There are five naturally occurring isotopes of the element zinc. The relative abundance and mass of each are as follows. 64 30Zn 48.89%, 63.929 amu 66 30Zn 27.81%, 65.926 amu 67 30Zn 4.11%, 66.927 amu 68 30Zn 18.57%, 67.925 amu 70 30Zn 0.62%, 69.925 amu © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Calculate the average atomic mass of zinc. Chapter 4 Atomic Structure 95 05_CTR_ch04 7/9/04 3:26 PM Page 96 Name ___________________________ Date ___________________ Class __________________ 25. Complete this table. Atomic Number Mass Number Number of Protons 9 Number of Neutrons Number of Electrons 10 14 7 21 13 20 27 56 26 26. List the number of protons, neutrons, and electrons in each of the following atoms. Protons Neutrons Electrons 13 6C 10 4Be 20 10Ne 11 5B D. Essay Write a short essay to answer the following. 27. Explain how the atoms of one element differ from those of another element. Then explain how the atoms of one isotope differ from those of other isotopes of the same element. 96 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 33 16S 05_CTR_ch04 7/9/04 3:26 PM Page 97 Name ___________________________ 4 Date ___________________ Class __________________ ATOMIC STRUCTURE Chapter Test B A. Matching Match each term in Column B with the correct description in Column A. Write the letter of the correct term on the line. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. Column A Column B ________ 1. the number of protons in the nucleus of an element a. electron ________ 2. the smallest particle of an element that retains its identity in a chemical reaction b. mass number ________ 3. the total number of protons and neutrons in the nucleus of an atom c. atomic number ________ 4. a positively charged subatomic particle d. atomic mass ________ 5. atoms with the same number of protons but different numbers of neutrons e. neutron ________ 6. a negatively charged subatomic particle f. atomic mass unit ________ 7. 1 12 g. proton the mass of a carbon-12 atom ________ 8. an arrangement of elements in which the elements are separated into groups based on a set of repeating properties h. isotopes ________ 9. a subatomic particle with no charge i. atom ________ 10. the weighted average of the mass of the atoms in a naturally occurring sample of an element j. periodic table B. Multiple Choice Choose the best answer and write its letter on the line. ________ 11. Which of these statements is included in Dalton’s atomic theory? a. Chemical reactions occur when atoms are separated, joined, or rearranged. b. Some but not all elements are composed of atoms. c. Atoms of the same element can have different numbers of protons. d. Atoms are divisible. ________ 12. Which of the following statements is correct? a. Electrons are positively charged. b. Protons are negatively charged. c. Neutrons have no charge. d. Atoms are positively charged. Chapter 4 Atomic Structure 97 05_CTR_ch04 7/9/04 3:26 PM Page 98 Name ___________________________ Date ___________________ Class __________________ ________ 13. Which of the following correctly lists the particles in order from least massive to most massive? a. proton, electron, hydrogen atom, helium atom b. proton, helium atom, hydrogen atom, electron c. hydrogen atom, electron, helium atom, proton d. electron, proton, hydrogen atom, helium atom ________ 14. Which of the following statements is not consistent with the results obtained in Rutherford’s gold foil experiment? a. The nucleus of an atom is positively charged. b. The nucleus of an atom contains almost all the mass of the atom. c. Atoms are composed mainly of empty space. d. Electrons are contained in the nucleus of an atom. ________ 15. The identity of an element can be determined on the basis of which of the following? a. the number of protons in an atom of the element b. the number of neutrons in an atom of the element c. the mass number of the element d. the atomic mass of the element ________ 16. What is the atomic number and the mass number of an atom with 11 protons and 12 neutrons? a. atomic number 11 and mass number 12 b. atomic number 12 and mass number 11 c. atomic number 11 and mass number 23 d. atomic number 23 and mass number 12 ________ 18. Which of the following statements is correct? a. Each vertical column of elements in the periodic table is called a period. b. The elements in any group of the periodic table have similar physical and chemical properties. c. Group 1A contains the elements hydrogen and helium. d. In the modern periodic table, elements are listed in order of increasing atomic mass. ________ 19. Isotopes of the same element have a. the same number of protons but different numbers of neutrons. b. the same number of protons but different numbers of electrons. c. the same number of neutrons but different numbers of protons. d. the same number of neutrons but different numbers of electrons. ________ 20. Which symbol correctly represents an element (D) whose atoms contain 15 protons and 20 neutrons? a. 20 c. 35 15D 15D 15 b. 20D d. 15 35D 98 Core Teaching Resources © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. ________ 17. An atom of hydrogen-2 contains a. 2 protons, 2 electrons, and 2 neutrons. b. 2 protons, 2 electrons, and 4 neutrons. c. 1 proton, 1 electron, and 1 neutron. d. 1 proton, 1 electron, and 2 neutrons. 05_CTR_ch04 7/9/04 3:26 PM Page 99 Name ___________________________ Date ___________________ Class __________________ ________ 21. If Z is the symbol for an element, which pair among the following represents isotopes of the same element? 51 50 a. 51 c. 50 25Z and 26Z 25Z and 27Z 51 50 51 b. 25Z and 25Z d. 26Z and 50 25Z ________ 22. The relative abundance of each isotope of an element determines its a. atomic number. c. number of electrons. b. atomic mass. d. number of protons. ________ 23. Three isotopes of oxygen occur in nature: oxygen-16, oxygen-17, and oxygen-18. If the atomic mass of oxygen is 15.9994, which of the three isotopes, if any, is the most abundant? a. oxygen-16 c. oxygen-18 b. oxygen-17 d. All are equally abundant. ________ 24. Element Z has two naturally occurring isotopes: Z-20 and Z-22. If the atomic mass of Z is 21.5 amu, what is the relative abundance of each isotope in nature? a. one Z-20 to one Z-22 c. two Z-20s to one Z-22 b. one Z-20 to two Z-22s d. one Z-20 to three Z-22s C. Problems Solve the following problems in the space provided. Show your work. 25. The element argon contains three naturally occurring isotopes: © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 36 18Ar 38 18Ar 40 18Ar The relative abundances and atomic masses are 0.337% (mass 35.978 amu), 0.063% (mass 37.963 amu), and 99.600% (mass 39.962 amu), respectively. Calculate the average atomic mass of argon. 26. List the numbers of protons, neutrons, and electrons in each of the following atoms. Protons Neutrons Electrons 19 9F 27 13Al 40 18Ar 65 30Zn 108 47 Ag Chapter 4 Atomic Structure 99 05_CTR_ch04 7/9/04 3:26 PM Page 100 Name ___________________________ Date ___________________ Class __________________ 27. Complete the following table. Atomic Number Mass Number Number of Protons Number of Neutrons Number of Electrons Symbol 24 12Mg 12 39 20 30 26 80 35Br 79 118 D. Essay Write a short essay for the following. 28. Explain how the isotopes of one element are alike and how they are different. Give at least two examples of each. © Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reserved. 100 Core Teaching Resources