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1. State the main ideas of Dalton’s Atomic Theory. 2. What experiments and theories regarding the atom came prior to Dalton? Explain these theories. a. b. c. d. Thomson Milliken Rutherford Chadwick 3. What did Rutherford’s gold foil experiment tell us about the structure of the atom? 4. Draw the Bohr Model of the atom for sodium. 5. Describe the composition of the nucleus of the atom. 6. What does the atomic number of each atom represent? Who is credited with the study of atomic numbers? 7. Distinguish between mass number and atomic number. 8. List the subatomic particles with charge, location, and approximate mass. 9. What is an amu? 10. How does the modern quantum mechanical atomic model differ from the atom of Dalton? 11. Why is there an average atomic mass on the periodic table? 12. Complete the following table. Nuclid Element # Mass e Proto # ns Hydrogen C-14 Carbon 14 19 # Electron s Atomic Number # Isotope, Neutrons Ion, or Neutral 17 37 Calcium 4 5 Uranium Neutral 235 10 12 13. Referring to the reference table for the Bohr model for the following questions a. For n = 1 an electron is at its ground state if it jumps up to level 4, what state is it? b. If the same electron drops back to its ground state, the light energy emitted is in which general region of the Electromagnetic spectrum c. Where is visible light located in the region of the electromagnetic spectrum in meters? 3. Dalton’s atomic theory and the Law of Multiple Proportions holds true with some major exceptions a. change mass to _______ _______ ________ b. subatomic particles found were_________, _________, _______ 4. Subatomic Particles: In the middle of the 19th century further experimentation led to the discovery of the ___________, ____________, and ________ Rays move from the ___________ to the ___________, therefore these rays were named ___________ rays and were composed of _____________. p.76 JJ Thomson discovered the _____________ and determined it’s charge to mass ratio. In addition, JJ Thomson discovered another subatomic particle, the ________. p.77_____________determined the first accurate measurement of an electron’s charge (-1) in his famous ________ __________experiment. Different drops had different charges but were all found to be multiples of one small _____. ________ ___________ predicted the presence of the neutron, however _____________ discovered the neutron. p. 80 Atoms of the same element that differ in mass are _________. Using X-rays, ___________found that the wavelength of the X-rays were characteristic of the particular metal being tested. He determined the ______ ______ of the element which is represented by the letter ____ p. 83. The number of ______ determines the identity of an element and the number of ____ determines the particular isotope of the elemtent. A particular kind of atom containing a definite number of protons and neutrons is called a ______. p.84 Any isotope of any element is called _______. The number of neutrons = _______ - _________ ______________ gold foil experiment determined that the nucleus is very very _______ and that most of the atom is occupied by __________ space p.78. p.809 ___________ are rays that are spontaneously emitted from unstable atomic nuclei. These rays can be particles or energy. This is no ordinary chemical reaction. __________ theorized that mass and energy are equivalent in the following equation ______= _________ (Energy is in ________, mass is in _______ and the speed of light is in ____________) Since the nucleus is composed of protons and neutrons, nuclear forces hold the nucleus together and are very powerful in order to overcome the repulsive forces of all the positive charges. Radiation p. 809 ________ particle is a helium nucleus composed of two _______ and two _________. A _______particle is a high speed __________ emitted from a radioactive ________. _________ _________ are very high energy X rays. Dalton’s Atomic Theory Dalton Today Matter is composed of very tiny or microscopic particles called “Atom”. Atom is an indivisible particle Atom can never be created nor it is destroyed. Atoms of an element are identical in size, shape, mass, and in other properties. Atoms of different elements are different in their properties. Atoms combine with each other in small whole numbers. _____1. Which of the following is NOT part of Dalton’s model of the atom? a. The atom is unchanged in chemical reactions. b. The atom is invisible. c. The atom has most of its mass in the center. d. The atom is indivisible. _____2. Which of the following statements was NOT part of Dalton’s hypothesis on the structure of matter? a. All matter is made up of atoms. b. Atoms of the same element are identical. c. Atoms are made of protons and electrons d. Atoms unite in definite ratios to form compounds. _____3. According to the law definite proportions, any two samples of potassium chloride have a. The same mass. b. Slightly different molecular structures. c. The same melting point. d. The same ratio of elements. _____4. According to the law of conservation of mass, when sodium, hydrogen, and oxygen react to form a compound, the mass of the compound is _________ the sum of the masses of the individual elements. a. Equal to. b. Greater than. c. Less than. d. Either greater than or less than. _____5. According to Dalton’s atomic theory, atoms a. Are destroyed in chemical reaction b. Can be divided c. Of each element are identical in size, mass, and other properties d. Of different elements cannot combine _____6. Which of the following is NOT part of Dalton’s atomic theory? a. Atoms cannot be divided, created, or destroyed b. The number of protons in an atom is its atomic number c. In a chemical reaction atoms are combined. d. All matter is composed of extremely small particles called atoms _____7. According to Dalton’s atomic theory, atoms a. Of different elements combine in simple whole-number ratios to form compounds b. Can be divided into protons, neutrons, and electrons c. Of all elements are identical in size and mass d. Can be destroyed in chemical reactions _____8. Dalton’s theory essentially agreed with the present atomic theory EXCEPT for the statement that a. All matter is made up of small particles called atoms b. Atoms are not divided in chemical reaction c. Atoms of the same element are chemically alike d. All atoms of the same element have the same mass _____9. Which concept in Dalton’s atomic theory has been modified? a. All matter is composed of atoms b. Atoms of different elements have different properties and masses c. Atoms can combine in chemical reaction d. Atoms cannot be divided _____10. When electrical current passed through a glass tube, a paddle wheel placed between the anode and the cathode moved. Scientists concluded that a. A magnetic field was produced b. Particles were passing from the cathode to the anode c. There was gas in the tube d. Atom were indivisible _____11. The ray produced in a cathode tube in early experiment were a. Unaffected by a magnetic field b. Deflected away from a negative plate c. Found to carry a positive charge d. Striking the cathode _____12. The behavior of cathode rays produced in a glass tube containing gas at low pressure led scientists to conclude that the rays a. Were not composed of matter b. Were composed of positively charged particles c. Were composed of negatively charged particles d. Were composed of uncharged particles _____13. Experiments with cathode rays led to discovery of the a. Proton b. Nucleus c. Neutrons d. Electron _____14. Millikan’s experiments a. Demonstrated that the electron carried no charged b. Demonstrated that the electron carried the smallest possible positive charge c. Measured the charge on the electron d. Atoms carried a negative charged _____15. By analyzing the data from hundreds of experiments, Millikan found that oil droplets carried an electric charge a. that was not related to other oil droplets. b. that was attracted to the negatively charge plate. c. that was equal to a fundamental unit of charge. d. that caused it to be attracted to other oil droplets. _____16. In Rutherford’s experiment very few positively charged alpha particles a. Were slightly deflected as they passed through the metal b. Were used to bombard a cathode plate c. Collided with electrons d. Were used to bombard thin metal foil _____17. In Rutherford’s experiment, most of the particles a. Bounced back b. Passed through the foil c. Were absorbed by the foil d. Combined with the foil _____18. Because most particles fired at metal foil passed straight through, Rutherford concluded that a. Atoms were mostly empty space b. Atoms contained no charged particles c. Electron formed the nucleus d. Atoms were indivisible _____19. Because a few positively charged particles bounced back from the foil, Rutherford concluded that such particles were a. Striking electrons b. Indivisible c. Repelled by dense regions of positive charge d. Magnetic _____20. Rutherford’s experiment led to the discovery of the a. Electron b. Cathode ray c. Nucleus d. Neutron _____21. Rutherford’s experimental results led him to conclude that atoms contain massive central regions that have a. A positive charge b. A negative charge c. No charge d. Both protons and electrons _____22. Rutherford’s fired positively charged particles at metal foil and concluded that most of the mass of an atom was a. In the electrons b. Concentrated in the nucleus c. Evenly spread throughout the atom d. In rings around the atom _____23. The Greek philosopher that first proposed the idea of atoms was a. Aristotle b. Dalton c. Plato d. Democritus _____24. The Greek philosopher that first came up with the Four Element Theory of Matter was a. Aristotle b. Dalton c. Plato d. Democritus