Test 2 Chapter 4 & 24 review sheet
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Name_______________________________ Block_____ Test 2 Chapter 4 & 24 - REVIEW SHEET Use prior worksheets and your book to answer and understand the following information. 1. Compare and contrast Thompson’s plum pudding atomic model with Rutherford’s nuclear atomic model. 2. Discuss the experiments and scientists that led to the conclusion that electrons are negatively charged particles found outside the nucleus in all matter. 3. Draw the evolution of atomic theory by filling the boxes below with the model accepted by the scientist.    
Dalton’s atom Plum Pudding Model Rutherfords Model Electron Cloud Model 4. How many protons electrons and neutrons are in the following: a. Aluminum-27 cation (charge = 1) b. Magnesium – 24 atom c. Rhenium – 186 cation (charge = 2) d. Selenuim – 79 anion (charge = 2) e. Gold – 197 atom f. Bromine – 80 anion (charge = 1) g. Neon – 20 atom h. Germanium – 73 atom i. Phosphorous – 31 anion (charge = 3) 5. Put the elements in #4 in shorthand notation. 6. Where are metals located on the periodic table? Where are the nonmetals? Name some differences between metals and nonmetals. 7. What is the name of the elements in group 18 (farthest to the right of the table)? What makes these elements unique? 8. Gallium has two isotopes, 69Ga and 71Ga. Ga-69 has a percent abundance of 60.3% and Ga-71 has a percent abundance of 39.7%. What is the atomic mass of Ga? 9. Silver has two naturally occurring isotopes, Ag-107 and Ag-109. The atomic mass of Ag is 107.868 amu. Calculate the percent abundances of the two isotopes. (Remember that R.A.1+R.A.2 = 1). 10. What are the three radioactive particles? List their charges and how the change atomic number and atomic mass. 11. What is the relationship between a neutron and a beta particle? 12.
a) _____ He + _____ b) ______ + _____ 2 77 44
c)  U → ______ +  He d) 47Ca
247 221 4 i) _____ Cm + j) _______ Fr + He 96 87 2 95 0 h) 240Am + 2 1n Write a sentence that describes the nuclear process in (h) 12. Write balanced equations for each of the following decay processes. a. Alpha decay of curium – 244
h. What is the neutron to proton ratio of curium–244, bismuth-210, arsenic-70, antimony-116, seaborgium-271, and mendelevium-258. 13. If a basement air sample contains 3.64 m of radon-222, how much radon will remain after 19 days. The half life of radon-222 is 3.8 days.
15. The half life of polonium-218 is 3 min. If you start with 26 g, how long will it be before only 2 g remains? 16. How much time has passed if 1/10 of an original sample of phosphorous-32 is left? The half life of phosphorous is 14.28 days. 17. Strontium-90 has a half life of 28 years. It is produced during nuclear weapons testing and when ingested, it is assimilated into the bones of the body where it damages healthy tissue. In 1963, several countries signed a treaty banning above ground nuclear testing. Using 1963 as time zero (start time), when the maximum amount of Sr-90 existed in the environment (100%), what percentage existed in 1991? What percentage will exist in 2075? 2159? 2215? Sr-90 levels are considered safe after 10 half lives. What year are we considered safe from radioactive Sr-90? 18. What is a chain reaction? Give an example of a nuclear chain reaction. 19. Describe nuclear fission. Include the ideas of particle accelerators, critical mass, chain reaction, methods of control, pollution, and how it differs from nuclear fusion. Draw a diagram (for example neutrons + large nucleus…) to show the mechanism. |