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Unit 1 Atomic Structure, Periodic Properties and Nuclear Chemistry Chp 4 Atomic Structure Sec 1-2 Guided Reading Notes Chp 5 Electrons in Atoms Sec 1 (1st half) Guided Reading Notes Chp 4 Atomic Structure Sec 3 Guided Reading Notes Vocabulary 4.1 Defining the Atom Early Models of the Atom 1. Democritus, who lived in Greece during the fourth century B.C., suggested that matter is made up of tiny particles that cannot be divided. He called these particles _______________________________________________________________________ 2. List two reasons why the ideas of Democritus were not useful in a scientific sense. _______________________________________________________________________ _______________________________________________________________________ 3. The modern process of discovery about atoms began with the theories of an English schoolteacher named _____________________________________________________ 4. Summarize the four postulates of Dalton’s Atomic Theory. _______________________________________________________________________ _______________________________________________________________________ _______________________________________________________________________ _______________________________________________________________________ Sizing up the Atom 5. Suppose you could grind a sample of the element copper into smaller and smaller particles. The smallest particle that could no longer be divided, yet still has the chemical properties of copper, is the _________________________________________ 6. About how many atoms of copper when placed side by side would form a line 1 cm long? __________________________________________________________________ 4.2 Structure of the Nuclear Atom Subatomic Particles 1. How is the atomic theory that is accepted today different from Dalton’s Atomic Theory? _______________________________________________________________________ _______________________________________________________________________ 2. Which subatomic particles carry a negative charge? __________________________ 3. Thomson observed that the production of cathode rays did not depend on the kind of gas in the tube or the type of metal used for the electrodes. What conclusion did he draw from these observations? _______________________________________________________________________ _______________________________________________________________________ 4. What two properties of an electron did Robert Millikan determine from his experiments? _______________________________________________________________________ 5. What charge does a neutron carry? _______________________________________ 6. What is the positively charged subatomic particle called? ______________________ 7. What is the unit charge that remains when a hydrogen atom loses an electron? _______________________________________________________________________ 8. Complete the table. Particle Symbol Relative Relative Mass Electrical (mass of proton = 1) Charge Electron Proton Neutron The Atomic Nucleus 10. An alpha particle has a double positive charge because it has lost two of which subatomic particle? _______________________________________________________ 11. Explain why in 1911 Rutherford and his coworkers were surprised when they shot a narrow beam of alpha particles through a thin sheet of gold foil. _______________________________________________________________________ _______________________________________________________________________ _______________________________________________________________________ _______________________________________________________________________ 12. Based on Rutherford’s experimental results, what three nuclear theories of the atom can be suggested. 1. __________________________________________________________ 2. __________________________________________________________ 3. __________________________________________________________ 5.1 Models of the Atom The Development of Atomic Models 1. Complete the table describing the atomic models and the scientists who developed them. Scientist Model of Atom Dalton Thomson Rutherford Bohr Can electrons in an atom exist between energy levels? __________________________ The Bohr Model 3. What are the fixed energies of electrons called? _____________________________ 4. A quantum of energy is the amount of energy required to _______________________________________________________________________ 5. In general, the higher the electron is on the energy ladder, the __________ it is from the nucleus. 4.3 Distinguishing Among Atoms Atomic Number 1. Complete the table. Name Symbol Atomic # # of Protons # of Electrons Hydrogen Helium Lithium Boron Carbon Oxygen Mass Number 2. The total number of protons and neutrons in an atom is its ____________________ 3. What is the mass number of a helium atom that has two protons and two neutrons? _______________________________________________________________________ 4. How many neutrons does a beryllium atom have with four protons and a mass number of nine? _________________________________________________________ 5. Use the shorthand notation to symbolize neon-22. ___________________________ 6. How many protons, neutron, and electrons does neon-22 possess? _______________________________________________________________________ Isotopes 7. How do atoms of neon-20 and neon-22 differ? _______________________________________________________________________ 8. Neon-20 and neon-22 are called __________________________________________ Atomic Mass 9. Why is the atomic mass unit (amu), rather than the gram, usually used to express atomic mass? _______________________________________________________________________ 10. What isotope of carbon has been chosen as the reference isotope for atomic mass units? What is the defined atomic mass in amu of this isotope? _______________________________________________________________________ 11. Why is the atomic mass of an element not a whole number? _______________________________________________________________________ 12. What is the relationship between the weighted atomic mass of an element and the relative abundance of its isotopes? _______________________________________________________________________ _______________________________________________________________________ 13. When chlorine occurs in nature, there are three atoms of chlorine-35 for every one of chlorine-37. Which atomic mass number is closer to the weighted atomic mass of chlorine? 35 amu or 37 amu Vocabulary Define the following words and concepts atom Democritus’ atomic philosophy Aristotle atomic philosophy Dalton’s atomic theory JJ Thomson’s atomic theory electrons cathode ray RA Millikan’s atomic theory Oil drop experiment J Chadwick’s atomic theory neutrons E Rutherford’s atomic theory nucleus Gold Foil Experiment protons N. Bohr’s atomic theory energy levels quantum of energy atomic number mass number isotopes atomic mass unit (amu) weighted atomic mass