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CHEM 100-002 Study guide CH 1-3

by: Carly Holliday

CHEM 100-002 Study guide CH 1-3 Chem 100

Marketplace > Indiana State University > Chem 100 > CHEM 100 002 Study guide CH 1 3
Carly Holliday
GPA 3.3

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I have provided 50 practice questions and all 50 answers to them to help you study for the exam on Friday! Enjoy!
Chemistry 100
Dr. Jeewandara
Study Guide
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This 7 page Study Guide was uploaded by Carly Holliday on Friday February 12, 2016. The Study Guide belongs to Chem 100 at Indiana State University taught by Dr. Jeewandara in Summer 2015. Since its upload, it has received 79 views.


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Date Created: 02/12/16
PRACTICE QUESTIONS EXAM 1 CHEM 100­002 Is the following a physical or chemical reaction? 1. Sugar melting in coffee 2. Wood burning 3. Ice melting  4. Hydrogen and oxygen combining to form water Are the following pure substances or mixtures 5. Soda (Coca­Cola)  6. Sugar 7. Copper 8. Water 9. What is an element? ________________________________________________________________________ 10. What is an atom? ________________________________________________________________________ 11. What is a compound? ________________________________________________________________________ 12. What is a molecule? ________________________________________________________________________ 13. Give an example of a homogeneous mixture: ________________________________ 14. Give an example of a heterogeneous mixture:________________________________ 15.  Determine whether each of the following is an element, a compound, or a mixture. If it is a  mixture, classify it as homogeneous or heterogeneous. a. copper wire b. water c. salt water d. Italian salad dressing 16. Identify the three states of matter. ________________      _________________________      __________________________ 17. What is a physical change? 18. What is a chemical change? 19. What does the law of constant composition say? 20. What does the law of conservation of mass say? ______________________________________________________________________________ ____________________________________________________________________________. 21. A match is weighed and then burned. The ashes are found to weigh much less. How can this  be consistent with the conservation of mass? ______________________________________________________________________________ ______________________________________________________________________________ _______________________________________________________________. 22. What are the three subatomic particles found in a single atom? a.  b.  c.  23. What are the charges of the three subatomic particles? a.  b.  c. 24. In order for an atom to have a neutral charge it must have  __________________________________________________________? 25. Which substance is a pure substance? a. Sea water b. Orange soda c. Nitrogen gas d. Air 26. Which substance is an element? a. table salt b. water c. sugar d. oxygen 27. Which state of matter has both a fixed volume and a fixed shape? a. solid b. liquid c. gas d. none of the above 28. In a chemical reaction, A and B combine to form AB. A reaction mixture contains 11 g of A  and  21g of B. After the reaction, A was completely consumed, but 6 g of B remained. What is  the mass of the AB that formed? a. 11g b. 21g c. 26g d. 32g 29. 6 grams of hydrogen react with 48 grams of oxygen to form how many grams of water? 30. A chemist combines 22 grams of sodium with 28 grams of chlorine. A spectacular reaction  occurs and produces sodium chloride. After the reaction, the chemist finds that all the chlorine  was used up by the reaction, but 4 grams of sodium remained. How many grams of sodium  chloride were formed? a. 40g b. 22g c. 95g d. 46g 31. What is Uncertainty in measurements? ______________________________________________________________________ 32. What is the unit for Temperature? __________________________ 33. What is the unit for Mass? __________________________ 34. What is the unit for Time? __________________________ 35. What is Slope on a graph? ____________________________________ 36. How do you find Density? _____________________________________ 37. What’s the difference between Weight and Mass? ______________________________________________________________________________ ____________________________________________________________________________ 38. What is in the nucleus of an atom? ___________________________________ 39. What is an Ion? __________________________________________ 40. What is an Isotope? ___________________________________________ 41. How do you calculate the average atomic mass? ____________________________________________________________________________ 42. What gives an atom its identity? ___________________________________ 43. What determines reactivity? _____________________________________ 44. How many Electrons can orbit 1 hold until it’s full?  _____________________ 45. How many Electrons can orbit 3 hold until it’s full?  _______________________ 46. What group is the Alkali earth metal family in? _____________________________ 47. What group is the Noble gas family in?  ________________________________ 48. How many Copper atoms are in 1 Mole of copper? ______________________________ 49. How many aluminum atoms are in 2 moles of aluminum? ___________________________ 50. What is the mass of one Mole of Sulfur? ______________________________________ ANSWER KEY: 1. Physical Change 2. Chemical Change 3. Physical Change 4. Chemical Change 5. Mixture  6. Pure 7. Pure  8. Pure 9. A pure substance that exists in nature or has been made by scientists 10. The smallest identifiable single unit of an element  11. When two or more elements join together they form a compound (H O is 2ne example) 12. One single unit of a compound 13. Salt water, coffee and sugar mixture, Air 14. Oil and water 15.       A. Copper is listed in the table of elements. It is an element. B. Water is not listed in the table of elements, but it is a pure substance; therefore, it is a  compound. C. Salt water is composed of two different substances, salt and water; it is a mixture.  Different samples of salt water may have different proportions of salt and water, a  property of mixtures. Its composition is uniform throughout; thus, it is a homogeneous  mixture. D. Italian salad dressing contains a number of substances and is therefore a mixture. It  usually separates into at least two distinct regions—each with a different composition— and is therefore a heterogeneous mixture. 16. Solid,  Liquid,  Gas 17. A change in matter in which it changes it appearance, but not its composition. 18. A change in which a sample of matter changes its composition. (*hint* if you can change the  substance back into what you started with, it is a physical change. If you cannot, it is a chemical  change) 19. If you take any mixture of the same substance, its chemical composition will always be the  same. The ratios between the atoms that make it up will always be the same.  20. In a chemical reaction matter is neither created nor destroyed. Your reactant and product will  always be equal in mass. 21. Much of the match’s mass was converted to a gas and lost into the air. If the gain in mass of  the surroundings was somehow measured, it would exactly equal the missing mass. 22. Protons, neutrons, electrons 23.       Protons + Neutrons 0  Electrons ­ 24. Equal # of protons and electrons. 25. (C) Nitrogen gas 26. (D) Oxygen 27. (A) solid  28. (C) 26g 29. 54 Grams 30.  (D) 46 Grams with 4g sodium left over 31. The last digit in a decimal measurement. The one digit you guess because your tool has  certain limitations (ten’s place or hundredth place).  32. Kelvin 33. Kilograms 34. Seconds 35. Change in y/change in x  or  (rise/run) 36. Density = Mass/Volume 37. Mass: the measure of quantity of matter (the same everywhere in the universe)       Weight: how strong gravity pulls on an object (different on earth and on the moon) 38. Protons and Neutrons 39. An atom or molecule that has an unequal number of electrons and protons. (it is not neutral is it is an ion) 40. Atoms having the same number of protons but different numbers of neutrons 41. Isotope1 %isotope2 %Isotope3 Average Atomicmass= 100 xmassIsotope1+ 100 xmassisotope2+ 100 xmass Isotope3 (Also Located in my CH 3 Notes) 42. Protons  43. Valence electrons  44. 2 Electrons  45. 8 Electrons  46. Group 2 47. Group 8 48.  6.022x1023 49. 12.044x10 23 50. 32.06 grams (Found on the periodic table)


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