PART I: ATOM SCREEN Build an Atom simulation ( ) Positive ions have protons than electrons.
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1 PART I: ATOM SCREEN Build an Atom simulation ( ) 1. Explore the Build an Atom simulation with your group. As you explore, talk about what you find. 2. a) List two things your group observed in the simulation. b) What particle(s) are found in the center of the atom? 3. Play until you discover which particle(s) determine(s) the name of the element you build. What did you discover? 4. What is the name of the following atoms? a) An atom with 3 protons and 4 neutrons: b) An atom with 2 protons and 4 neutrons: c) An atom with 4 protons and 4 neutrons: 5. Play with the simulation to discover which particles affect the charge of an atom or ion. a) Fill in the blanks below to show your results: Neutral atoms have the same number ofprotons and electrons. Positive ions have protons than electrons. Negative ions have protons than electrons. b) Develop a relationship (in the form of a single sentence or equation) that can predict the charge based on the number and types of particle. 6. Play with the simulation to discover what affects the mass number of your atom or ion. a) What is a rule for determining the mass number of an atom or ion? 7. Practice applying your understanding by playing 1 st and 2 nd levels on the game screen. 1
2 PART II: SYMBOL SCREEN 8. Using the Symbol readout box, figure out which particles affect each component of the atomic symbol. a) In the atomic symbol below, label each letter ( a, b, c, and d ) with: the particle(s) used to determine the letter, and how the value of each letter is determined. 9. Create a definition (using a complete sentence) for each of these items based on your labels from the atomic symbol above. a) Element Symbol b) Charge c) Atomic Number d) Mass Number 10. Practice applying your understanding by playing the 3 rd and 4 th game levels. Play until you can get all the questions correct on the 4 th level. 11. In addition to atomic symbol, we can represent atoms by name and mass number. a) Complete the table below: Symbol Name Carbon-12 b) Each representation (Symbol and Name) in the table above provides information about the atom. Describe the similarities and differences between the Symbol and Name representations. 2
3 PART III: ISOTOPES 12. Play with the simulation to determine: a) Which particles affect the stability of the atom? b) Which particles do not affect the stability of the atom? 13. What are the names of the stable forms of oxygen? a) Oxygen-16 b) Oxygen- c) Oxygen- d) List all of the things that are the same about these atoms (ignore the electrons). e) List all of the things that are different about these atoms (ignore the electrons). 14. The atoms in the previous question are isotopes of each other. Based on this information, list the requirements for two atoms to be isotopes of each other. 15. Test your understanding of isotopes by examining the relationships between the pairs of atoms listed below: Atom 1 Atom 2 Relationship between atom 1 and atom 2 Different Element Carbon-12 Different Element Argon-40 Argon-41 Different Element Boron-10 An atom with 13 protons and 13 neutrons An atom with 14 protons and 13 neutrons Different Element Different Element 3
4 4
5 EXERCISES 16. The periodic table has a great deal of information about every atom. Using your periodic table, answer the following questions: a) What is the atomic number of chlorine (Cl)? b) What is the atomic number of tungsten (W)? c) How many protons are there in any Cl atom? d) How many protons are there in any Te atom? e) Can you tell from the periodic table exactly how many neutrons are in an atom? 17. Complete the following table: Atomic Mass Number of Number of Name Symbol Charge number Number neutrons Electrons 2 hydrogen-2 H H sodium Na Ti Ag 19 F carbon-12 6 carbon-13 6 carbon-14 6 carbon-12 7 carbon He argon Ga 70 Ga
6 18. To test your knowledge of isotopes, draw arrows between all pairs of atoms in the table above that are isotopes of each other. 6
TITLE Build an Atom. AUTHORS Timothy Herzog (Weber State University) Emily Moore (University of Colorado Boulder) COURSE General Chemistry I
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