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1 4.1 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 Atoms of any one element are 2 from those of any 2. other element. Atoms of different elements can form by combining in whole-number ratios. Chemical reactions 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
2 Part C Matching Match each description in Column B to the correct term in Column A. Column A Column B atom scanning tunneling microscope John Dalton a. an instrument used to generate images of individual atoms b. Greek philosopher who was among the first to suggest the existence of atoms c. the smallest particle of an element that retains its identity in a chemical reaction 11. Democritus 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? d. English chemist and schoolteacher who formulated a theory to describe the structure and chemical reactivity of matter in terms of atoms 13. How many copper atoms would you have to line up side by side to form a line 1 m long? 84 Core Teaching Resources
3 4.2 STRUCTURE OF THE NUCLEAR ATOM 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 1 particles changed this theory. Scientists now know that 2. atoms are made up of electrons, which have a 2 charge; 3. 3,which have a positive charge; and 4, which are 4. neutral. The latter two particles are found in the 5 of the 5. atom. It was 6 who discovered the nucleus of the atom. The 6. nucleus, which has a 7 charge, occupies a very small volume 7. of the atom. In contrast, the negatively charged 8 occupy 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
4 Part C Matching Match each description in Column B to the correct term in Column A Column A Column B electrons cathode ray protons neutrons nucleus a. stream of electrons produced at the negative electrode of a tube containing a gas at low pressure b. the central core of an atom, which is composed of protons and neutrons c. negatively charged subatomic particles d. subatomic particles with no charge 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? 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? 86 Core Teaching Resources
5 4.3 DISTINGUISHING BETWEEN ATOMS 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 Key Equations atomic number number of protons number of electrons number of neutrons mass number atomic number periodic table period group 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. The number of 1 in the nucleus of an atom is the 1. atomic 2 of that element. Because atoms are electrically 2. neutral, the number of protons and 3 in an atom are equal. 3. The total number of 4 and neutrons in an atom is the mass 4. number. Atoms of the same element are identical in most respects, 5. but they can differ in the number of 5 in the nucleus. Atoms 6. that have the same number of protons but different mass numbers 7. are called The 7 of an element is the weighted average of the 9. masses of the isotopes of that element. Each of the three known 10. isotopes of hydrogen has 8 proton(s) in the nucleus. The most common hydrogen isotope has 9 neutrons. It has a mass number of 10 and is called hydrogen-1. Chapter 4 Atomic Structure 87
6 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 atomic number periodic table a. atoms that have the same number of protons but different numbers of neutrons b. weighted average mass of the atoms in a naturally occurring sample of an element mass number group isotopes atomic mass unit (amu) atomic mass 23. period 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: 99.76% oxygen-17: 0.037% oxygen-18: 0.204% c. equals the number of neutrons plus the number of protons in an atom d the mass of a carbon-12 atom e. the number of protons in the nucleus of an atom of an element f. an arrangement of elements according to similarities in their properties g. a vertical column of elements in the periodic table h. a horizontal row of the periodic table 88 Core Teaching Resources
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