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The Structure of the AtomThe Structure of the Atom - Weebly

CHAPTER 4 SOLUTIONS MANUAL. The Structure of the Atom Concept maps will vary, but should reflect the Section Early Ideas About following summary. Both believed: matter Matter composed of extremely small particles called pages 102 105 atoms; all atoms of a given element are identical, but differ from the atoms of other elements;. Section Assessment atoms could not be created, divided, or destroyed;. page 105 apparent changes in matter result from changes in the groupings of atoms. Democritus further 1. Contrast the methods used by the Greek philos- believed that matter is composed of empty space ophers and Dalton to study the atom. through which atoms move, that different kinds Greek philosophers could not conduct of atoms come in different sizes and shapes, and experiments to verify their hypothesis, whereas that the differing properties of atoms are due Dalton could make careful measurements.

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Transcription of The Structure of the AtomThe Structure of the Atom - Weebly

1 CHAPTER 4 SOLUTIONS MANUAL. The Structure of the Atom Concept maps will vary, but should reflect the Section Early Ideas About following summary. Both believed: matter Matter composed of extremely small particles called pages 102 105 atoms; all atoms of a given element are identical, but differ from the atoms of other elements;. Section Assessment atoms could not be created, divided, or destroyed;. page 105 apparent changes in matter result from changes in the groupings of atoms. Democritus further 1. Contrast the methods used by the Greek philos- believed that matter is composed of empty space ophers and Dalton to study the atom. through which atoms move, that different kinds Greek philosophers could not conduct of atoms come in different sizes and shapes, and experiments to verify their hypothesis, whereas that the differing properties of atoms are due Dalton could make careful measurements.

2 To the size, shape, and movement of the atoms. Dalton further specified that different atoms 2. Define atom using your own words. combine in simple whole number ratios to form An atom is the smallest component of an element compounds. that exhibits all of the characteristic properties of that element. Section Defining the Atom 3. Summarize Dalton's atomic theory. pages 106 114. Matter is composed of small particles called atoms that are indivisible. Atoms of an element are Section Assessment identical in size, mass, and chemical properties. page 114. Atoms of a specific element are different from 7. Describe the Structure of a typical atom. atoms of another element. Different atoms copyright glencoe / mcgraw - hill , a division of the mcgraw - hill companies , Inc. Identify where each subatomic particle is combine in simple whole-number ratios to form located.

3 Compound. In a chemical reaction, atoms are separated, combined, or rearranged. A typical atom consists of a central, small, dense nucleus containing protons and neutrons. The 4. Explain how Dalton's theory of the atom and nucleus is surrounded by a cloud of negatively the conservation of mass are related. charged electrons. Dalton explained that atoms are not created 8. Compare and contrast Thomson's plum or destroyed in chemical reactions, but only pudding atomic model with Rutherford's rearranged. nuclear atomic model. 5. Apply Six atoms of Element A combine with Thomson's plum pudding model describes atoms 8 atoms of Element B to produce six compound as spherical particles with uniformly distributed particles. How many atoms of Elements A and positive charge in which individual, negatively B does each particle contain?

4 Are all atoms charged, electrons are located in fixed positions. used to form compounds? In contrast, Rutherford's model states that an atom is mostly empty space, with a small, Each compound contains 1 atom A and 1 atom B. dense, central nucleus containing all of an 2 atoms of element B are not used. atom's positive charge and most of its mass. The negatively charged electrons move through the 6. Design a concept map that compares and empty space and are held in the atom by their contrasts the atomic theories proposed by attraction to the positively charged nucleus. Democritus and John Dalton. Solutions Manual Chemistry: Matter and Change Chapter 4 53. CHAPTER 4 SOLUTIONS MANUAL. 9. Evaluate the experiments that led to the conclu- 15. Challenge Do the atoms shown in the figure sion that electrons are negatively charged to the right have the same atomic number?

5 Particles found in all matter. The deflection toward positively charged plates 9e- demonstrated the negatively charged nature 9p of electrons; the fact that changing the type of 10n 9n electrode or the type of gas used in the cathode ray tube did not affect the ray produced led to the conclusion that electrons are present in all matter. Yes. 9. 10. Compare the relative charge and mass of each 16. Determine the number of protons, electrons, and of the subatomic particles. neutrons for isotopes b through f. in the table above. Name each isotope, and write its symbol. Particle Relative charge Relative mass Protons Electron 21 1/1840. and Proton 11 1 Electrons Neutrons Isotope Symbol b. 20 26 calcium-46 46Ca Neutron 0 ~1 20. c. 8 9 oxygen-17 17O. 8. 11. Calculate What is the difference expressed in 57Fe d.

6 26 31 iron-57 26. kilograms between the mass of a proton and the mass of an electron? e. 30 34 zinc-64 64Zn 30. 3 10224 g 2 3 10228 g 5 3 f. 80 124 mercury-204 204Hg 80. 10224 g 3 1 kg/1000 g 5 3 10227 kg copyright glencoe / mcgraw - hill , a division of The mcgraw - hill companies , Inc. 17. Challenge An atom has a mass number of 55. Its number of neutrons is the sum of its atomic Section How Atoms Differ number and 5. How many protons, neutrons, pages 115 121 and electrons does this atom have? What is the identity of this atom? Practice Problems 25 protons, 25 electrons, 30 neutrons. manganese pages 116 121. 12. How many protons and electrons are in each 18. Boron (B) has two naturally occurring isotopes: atom? boron-10 (abundance 5 , mass 5. amu), boron-11 (abundance 5 , a. radon, 86 protons and 86 electrons mass 5 amu).

7 Calculate the atomic mass b. magnesium, 12 protons and 12 electrons of boron. 13. An atom of an element contains 66 electrons. B-10 amu 3 5 amu Which element is it? B-11 amu 3 5 amu dysprosium Atomic mass amu 1 amu 5 amu 14. An atom of an element contains 14 protons. 19. Challenge Nitrogen has two naturally occur- Which element is it? ring isotopes, N-14 and N-15. Its atomic mass silicon is Which isotope is more abundant? Explain your answer. N-14 is more abundant because the atomic mass is closer to 14 than 15. 54 Chemistry: Matter and Change Chapter 4 Solutions Manual CHAPTER 4 SOLUTIONS MANUAL. Section Assessment 26. State what quantities are conserved when page 121 balancing a nuclear reaction. 20. Explain how the type of an atom is defined. mass number and atomic number by the atomic number 27.

8 Classify each of the following as a chemical 21. Recall Which subatomic particle identifies an reaction, a nuclear reaction, or neither. atom as that of a particular element? a. Thorium emits a beta particle. the proton nuclear 22. Explain how the existence of isotopes is b. Two atoms share electrons to form a bond. related to the fact that atomic masses are not chemical whole numbers. c. A sample of pure sulfur emits heat energy as Atomic masses aren't whole numbers because it slowly cools. they represent weighted averages of the masses of the isotopes of an element. neither 23. Calculate Copper has two isotopes: Cu-63 d. A piece of iron rusts. (abundance 5 , mass 5 amu) and Chemical Cu-65 (abundance 5 , mass 5 amu). Calculate the atomic mass of copper. 28. Calculate How much heavier is an alpha Cu-63 amu 3 5 amu particle than an electron?

9 Cu-65 amu 3 5 amu 3 10227 kg 2 3 10231 kg 5 3. 10227 kg Atomic mass amu 1 amu 5 amu 29. Create a table showing how each type of radia- 24. Calculate Three magnesium isotopes have copyright glencoe / mcgraw - hill , a division of The mcgraw - hill companies , Inc. tion affects the atomic number and the mass atomic masses and relative abundances of number of an atom. amu ( ), amu ( ), and ( ). Calculate the atomic Particle Atomic number Mass Number mass of magnesium. a 22 24. Mg-24 amu 3 5 amu b 11 no change Mg-25 amu 3 5 amu g no change no change Mg-26 amu 3 5 amu Atomic mass 1 1 amu 5. amu ( amu). Chapter 4 Assessment pages 128 131. Section Unstable Nuclei and Section Radioactive Decay pages 122 124 Mastering Concepts 30. Who originally proposed the concept that Section Assessment matter was composed of tiny indivisible, page 124.

10 Particles? 25. Explain how unstable atoms gain stability. Democritus They undergo a series of radioactive decays until they reach a stable element. Solutions Manual Chemistry: Matter and Change Chapter 4 55. CHAPTER 4 SOLUTIONS MANUAL. 31. Whose work is credited with being the begin- 37. Conservation of Mass Explain how Dalton's ning of modern atomic theory? atomic theory offered a convincing explanation John Dalton of the observation that mass is conserved in chemical reactions. 32. Distinguish between Democritus's ideas and Mass is conserved because atoms cannot be Dalton's atomic theory. created, divided, or destroyed. Chemical reactions involve only the separation, combination, and Democritus's ideas Dalton's atomic theory rearrangement of atoms. Atoms move through Matter is composed of empty space composed small particles called 38.


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