Physics Questionnaire-UNHS.

PHYSICAL SCIENCE 2 SCIH024055 Assignment Unit 3 Evaluation Print Page You’re Previewing This Assignment Your ability to start and submit this assignment is restricted by the sequencing policy. You must submit your previous graded assignment before you may start this assignment. More Information on Sequencing (https://highschool.nebraska.edu/forms-andpolicies/faq/courses) This computer-graded unit evaluation will help you check your understanding of the concepts presented in the lessons of this unit and will provide you with helpful feedback. You may refer to the course materials at any time while working on these evaluations. (Think of them as homework assignments.) Questions will reflect various levels of thinking skills: remembering, understanding, applying, analyzing, evaluating, and creating. You will be expected to apply and synthesize the information you have learned to answer these questions. You should print the evaluation(or save it to your computer) and take all the time you need to complete it, looking up the answers to any questions you are not sure about.You will not be able to submit this unit evaluation until it is available for submission within the sequencing of this course identified in your Student Progress Chart. Check your gradebook if you have any questions regarding when this may be submitted. Unit 3 Evaluation (in printable format) (/Files/Courses/SCIH 024055/Unit-3/Unit 3 Evaluation (in printable format).pdf) Multiple Choice Choose the answer that best completes the statement or answers the question. 1. Which of the following is not a good example of a solute and solvent in solution? A. a solution of a liter of water and a gram of salt B. a solution of a gram of silver and a milligram of copper C. solution of a liter of cold water and a liter of hot water 2. Michelle wants to quickly dissolve powdered drink mix in a pitcher of water. All of the following are ways in which she could increases the rate of dissolution except A. heating the mixture. B. stirring the mixture. C. adding more powdered drink mix. 3. Information about the amount of salt that will dissolve in a liter of water at 20 degrees Celsius would most likely be found in which kind of table? A. solubility B. polarity C. temperature 4. Jan added salt to a beaker of water until she could still see salt crystals, even after stirring. This type of solution is called A. an unsaturated solution. B. a saturated solution. C. a supersaturated solution. 5. Which of the following is not a solution? A. a mixture of nitrogen, oxygen, and argon B. a necklace made of copper and gold C. a liter of mercury 6. Which of these best describes the process of ionization? A. Molecules dissolve in water and form charged particles. B. Water mixes with oil to form nonpolar solutes. C. Positive and negative ions mix with a solved to form a solution. 7. Water is called the universal solvent. Which of these statements about water is false? A. water is a polar substance B. water is a nonpolar substance C. pure water is a nonelectrolyte 8. A student mixes a solution of sodium chloride and water. She finds that the solution conducts electricity. This means that sodium chloride must be A. a nonpolar substance. B. an electrolyte. C. a solvent. 9. Which of the following terms is used to describe a solution that results when both the solute and solvent are solids? A. alloy B. aqueous solution C. surface solution 10. Which of the following is not true for a solution? A. Solutions are homogeneous. B. The density at the top of the solution is the same as at the bottom. C. When two substances combine to form a solution, the dissolving always occurs at the same rate. 11. Since dissolving depends on collisions between the solute and solvent, increasing the surface area of a solute can increase the collisions between the solute and solvent. If a cube of sugar has the dimensions of 2 cm x 2 cm x 2 cm, how much surface area does it have? A. 2 cm B. 8 cm 3 2 C. 24 cm 2 12. If a sugar cube with the dimensions of 2 cm x 2 cm x 2 cm is cut down the middle to form two rectangular solids (as illustrated in the Applying Math section on page 651 in your textbook) how much new surface area is created? A. 4 cm B. 8 cm 2 2 C. 16 cm 2 13. Which of the following is not one of the drawbacks of nonpolar solvents? A. Many nonpolar solvents are flammable. B. Some nonpolar solvents are toxic and hazardous if inhaled. C. Nonpolar solvents are used to dissolve oils. 14. Use the graph in Figure 9 on page 655 of your textbook to determine the solubility of potassium nitrate at 50°C (how many grams would be dissolved in 100 g of water). A. 120 grams B. 40 grams C. 80 grams 15. Which of the following is not an acid? A. Mg(OH)2 B. H2 C6 H6 O6 C. H2 SO4 16. Solution A has HCl dissolved with a pH value of 5. Solution B also has HCl dissolved, but has a pH value of 4. Which of the following makes a valid comparison of the two solutions? A. Solution A is more acidic than solution B. B. Solution B contains twice as much HCl as solution A. C. Solution B contains ten times more HCl than solution A. 17. Acetic acid (CH3 COOH) is the weak acid found in vinegar. Which of the following statements is not true about this acid? + A. It can produce H3 O in water solutions. B. Most solutions of acetic acid will have pH values above 7. C. Equations that show the reaction of acetic acid in water will have both a forward and a reverse arrow. 18. Which of the following instruments could tell you how acidic a sample of stream water is? A. anemometer B. oscilloscope C. pH meter 19. According to the pH scale, which of the following pH measurements is basic? A. 7.0 B. 9.5 C. 1.2 20. An aqueous solution of which of the following compounds will change universal indicator paper to red? A. HCl B. NaCl C. NaOH 21. Lye, a substance used in making soap, has a pH of 13. A substance with a pH of 13 is best described as A. acidic. B. basic. C. neutral. 22. An unknown substance in solution is slippery to the touch, dissolves easily in water, and makes red litmus paper turn blue. The substance is most likely A. an acid. B. a base. C. a salt. 23. At the instant of neutralization, what is in the beaker besides water? A. acid only B. base only C. salt only 24. Which item is a solution of hydrochloric acid and water? A. vitamin C B. stomach acid C. vinegar 25. A change in what property permits certain materials to act as indicators? A. acidity B. color C. concentrations 26. What is the pH of pure water at 25°C? A. 5.2 B. 7 C. 14 27. Which of the following is not a solution? A. mud in a water tank B. glass of flat soda C. air in a scuba tank 28. What can a polar solvent dissolve? A. any solute B. a polar solute C. a nonpolar solute 29. Which of the following is the best definition of an organic compound? A. most compounds containing the element carbon B. a compound composed of only carbon and hydrogen atoms C. compounds that have the same chemical formulas but different molecular structures 30. Proteins have all the following characteristics except that they are A. inorganic compounds. B. able to fold into different shapes. C. found in hemoglobin. 31. Mixing alcohols and organic acids will form A. water and salt. B. water and an ester. C. a foul smelling thiol. 32. A substituted hydrocarbon has one or more of its _________ atoms replaced by atoms, or groups of atoms of other elements. A. carbon B. hydrogen C. oxygen 33. There are over four million organic compounds. The element carbon forms so many compounds because A. it is easy for carbon to gain four electrons. B. carbon atoms readily form ionic bonds with other carbon atoms. C. carbon atoms readily form four covalent bonds with other atoms. 34. Butane and isobutane are isomers. Isomers are compounds with A. identical chemical formulas but different molecular structures. B. identical molecular structures but different chemical formulas. C. identical chemical formulas and molecular structures. 35. There are so many different kinds of organic materials because carbon A. is a very light element. B. has a low melting point. C. forms many types of bonds. 36. Sugars and starches are part of the group of organic compounds called A. lipids. B. carbohydrates. C. amino acids. 37. Which crude oil fractions are collected at the bottom of a fractionating tower? A. high boiling point, many carbon atoms B. low boiling point, few carbon atoms C. high boiling point, few carbon atoms 38. Small molecules from petroleum that can combine with themselves repeatedly to form long chains are A. monomers. B. polymers. C. polystyrenes. 39. Which name would be used for a straight-chained hydrocarbon containing 2 carbon atoms? A. methane B. ethane C. butane 40. An alloy is a mixture of one or more elements with what kind of properties? A. plastic B. ceramic C. metallic 41. Most ceramics have all the following properties except A. the ability to withstand high temperatures. B. brittleness. C. malleability. 42. Plastics are usually made of what kind of materials? A. polymers B. ceramics C. alloys 43. Many modern materials are combinations of other materials. What does doping do? A. It changes the electrical conductivity of a metalloid. B. It changes the malleability of polymers. C. It changes the hardness of alloys. 44. Synthetic polymers are usually made from A. hydrocarbons found in fossil fuels. B. chemically treated natural fibers. C. composites such as fiberglass. 45. Joe needs to classify a substance. Through experimentation, he finds that the material is lustrous, malleable, and conducts electricity. Joe therefore identifies the substance as a A. polymer. B. ceramic. C. metallic alloy. 46. What property allows brass to be shaped into a musical instrument? A. ductility B. luster C. malleability 47. Which property of metals and alloys makes a French horn appear shiny? A. conductivity B. luster C. malleability 48. Which group of materials is not classified as synthetic? A. ceramics B. metal ores C. composites 49. What class of materials is made from clay, silica, and feldspar? A. hydrocarbons B. fiberglass C. ceramics 50. Ceramics are not generally used for making A. fireproof clothing. B. crystal glassware. C. tooth replacements. PHYSICAL SCIENCE 2 SCIH024055 Assignment Unit 2 Evaluation Print Page You’re Previewing This Assignment Your ability to start and submit this assignment is restricted by the sequencing policy. You must submit your previous graded assignment before you may start this assignment. More Information on Sequencing (https://highschool.nebraska.edu/forms-andpolicies/faq/courses) This computer-graded unit evaluation will help you check your understanding of the concepts presented in the lessons of this unit and will provide you with helpful feedback. You may refer to the course materials at any time while working on these evaluations. (Think of them as homework assignments.) Questions will reflect various levels of thinking skills: remembering, understanding, applying, analyzing, evaluating, and creating. You will be expected to apply and synthesize the information you have learned to answer these questions. You should print the evaluation(or save it to your computer) and take all the time you need to complete it, looking up the answers to any questions you are not sure about.You will not be able to submit this unit evaluation until it is available for submission within the sequencing of this course identified in your Student Progress Chart. Check your gradebook if you have any questions regarding when this may be submitted. Unit 2 Evaluation (in printable format) (/Files/Courses/SCIH 024055/Unit-2/Unit 2 Evaluation (in printable format).pdf) Part A: Matching Match each of the following with the correct definition. WORDBANK A. noble gas E. sodium chloride B. chemical bond C. water D. molecule 1. table salt 2. H2 O 3. a neutral particle that forms as a result of electron sharing 4. the force that holds atoms together in a compound 5. almost never forms compounds because they are extremely stable Part B: True/False Choose whether the following statements are True or False. 6. Metals tend to lose electrons and nonmetals tend to gain electrons when they form ions. A. True B. False 7. In ionic compounds, the oxidation number is the same as the charge on the ion. A neutral ionic compound can only contain ions with identical charges. A. True B. False 8. A crystalline substance that contains water is called a polyatomic molecule. A. True B. False 9. Copper(II) sulfate pentahydrate has five water molecules. A. True B. False 10. Different parts of the atom form new substances during both chemical reactions and nuclear reactions. A. True B. False 11. In chemical equations, coefficients act as the unit mangers, representing the number of units of each substance taking part in a reaction. A. True B. False 12. In a synthesis reaction, substances break down into two or more substances. A. True B. False 13. Glow sticks contain three different chemicals that release energy in the form of light when they are mixed. This is called an endothermic reaction. A. True B. False 14. The rate of reaction can be affected by a chemical’s temperature and concentration, the level of agitation or pressure, and the amount of surface area exposed. A. True B. False 15. Food preservatives act as catalysts to slow down the rates of the chemical reactions that cause certain foods to spoil. A. True B. False Part C: Multiple Choice Choose the answer that best completes the statement or answers the question. 16. How many electrons are found in the outer level of an atom of sulfur? (Hint: refer to Figure 3 in Chapter 18 of your text.) A. 16 B. 8 C. 6 D. 2 17. Which of the following best describes the term “ion”? A. An ion is an atom that has lost a neutron. B. An ion is an atom that has gained a proton. C. An ion is an atom that has either lost or gained an electron. D. An ion is an atom that has either lost or gained a quark. 18. Of the following statements, which is not true of a covalent chemical bond? A. In covalent bonding, the sharing of electrons must always be equal. B. In covalent bonding, the outer electrons are shared. C. Covalent bonds usually form between nonmetals. D. A compound that is held together by covalent bonding is called a covalent compound. 19. Which of the following is the most accurate statement about a polar covalent bond? A. The charge is balanced. B. The attraction for electrons between two atoms with a polar covalent bond is equal. C. The bond will have one side that is slightly positive and another side that is slightly negative D. CCl4 is an example of a molecule with polar covalent bonds. 20. What is the formula of the ionic compound that forms between Mg and Cl? (Hint: use Figure 9 in Chapter 18 of the text for assistance, if needed.) A. MgCl B. MgCl2 C. Mg2 Cl2 D. Mg2 Cl 21. Sulfur dioxide is a common air pollutant that is a concern near coal burning power plants. What is the chemical formula of this covalent compound? A. SO B. SO2 C. S2 O2 D. SOS 22. Which of the following statements provides an accurate comment about the following balanced chemical equation? NiCl2 (aq ) + 2NaOH(aq ) → Ni(OH)2 (s ) + 2NaCl(aq ) A. The product side contains one unit of nickel(II) chloride. B. The reactant side contains a solid. C. The reactant side contains more atoms of oxygen than the product side. D. The product side contains sodium chloride. 23. Suppose you saw 3Ni(OH)2 in a balanced chemical equation. How many atoms of oxygen are represented in this expression? A. 3 B. 2 C. 6 D. 5 24. One way to obtain hydrogen that may potentially be used for future fuel supplies is to split water molecules—as shown in the unbalanced chemical equation that follows. Which coefficients would you need to insert to balance the equation? __ H2 O (l ) → __H2 (g ) + __O2 (g ) A. 2, 2, 1 B. 1, 1, 2 C. 2, 4, 1 D. 1, 1, 1 25. Using the list of active metals shown in Figure 10 in Chapter 19 of your textbook, which of the following metals would displace zinc ions from a solution? A. aluminum B. copper C. silver D. gold 26. The minimum amount of energy needed to start a chemical reaction is A. endothermic energy. B. exothermic energy. C. activation energy. D. catalytic energy. 27. How does a catalyst affect the rate of a chemical reaction? A. It affects the pressure. B. It can increase the temperature, thereby increasing the rate of reaction. C. It can lower the activation energy needed. D. It can cause the reaction to be exothermic. 28. What causes the attractions between protons and neutrons in the nucleus of an atom? A. electrostatic attractions B. the strong force C. radioactivity D. fission 29. Which of the following statements about neutrons, alpha particles, beta particles, and gamma rays is true? A. Alpha particles are the only ones with a charge greater than one. B. All those listed move at the same speed. C. Only gamma rays carry a negative charge. D. Beta particles have the highest penetrating ability of all those listed. 30. Some radioactive isotopes take millions of years to decay. What is the nucleus that is left after the isotope decays called? A. unstable nucleus B. beta particle C. daughter nucleus D. alpha particle 31. In which method of radiation detection are the vapor trails of alpha and beta particles visible as they travel? A. electroscope B. bubble chamber C. positron emission tomography D. cloud chamber 32. A Geiger counter functions by A. producing an electric current when radiation is present. B. detecting radioactive isotopes present in organisms. C. responding to ionization of the surrounding air. D. responding to ionization of the radioactivity in the soil. 33. Using Figure 14 in Chapter 20 of your textbook, determine which of the following sources of background radiation contributes the highest amount to the average background radiation in the United States. A. cosmic rays B. X-rays C. radon gas D. radiation inside the body 34. If 100 g of radioactive material has a half-life of 10 years, how much of the material will remain after 30 years? A. 50 g B. 33 g C. 25 g D. 12.5 g 35. The process by which hydrogen and oxygen form water can be classified as a A. decomposition reaction. B. synthesis reaction. C. precipitate reaction. D. single-displacement reaction. 36. Which of the following may be classified as a binary compound? A. H2 SO4 B. NH4 Cl C. Hg(OH)2 D. NaCl 37. Ionic compounds are usually formed by ionic bonding between metals and nonmetals. Which of the following is not an ionic compound? A. NaBr B. MgCl2 C. HCl D. KI 38. In the following equation, which are the reactants? HCl + NaOH → NaCl + H2 O A. HCl + NaOH B. NaCl + H2 O C. HCl + H2 O D. NaOH + NaCl 39. Which of these is a reason a catalyst is added to a chemical reaction? A. to stabilize a substance B. to speed up a reaction C. to produce a greater amount of the catalyst D. to prevent a compound from forming 40. Some reactions require an input of energy in order to occur. Photosynthesis, the process in which plants use light to make sugars, requires an energy input. This reaction would be classified as A. endergonic. B. exergonic. C. synthetic. D. exothermic. 41. Which of these processes is endothermic? A. iron rusting B. burning wood C. exploding dynamite D. mixing Epsom salt in water 42. A double-displacement reaction occurs if water, gas or a precipitate forms when two ionic compounds in solution are combined. Which of the following is the generalized formula for this type of reaction? A. AB + CD → AD + CB B. A + BC → AC + B C. D + BC → BD + C D. A + B → AB 43. Which of these is not evidence of a chemical reaction? A. An iron nail changes to a brownish-orange color. B. An ice cube melts into liquid water. C. An antacid table produces bubbles of gas when placed in water. D. A piece of zinc raises the temperature of an acid as it reacts with it. 44. Metal corrosion and the formation of rust are often the result of which type of reaction? A. decomposition B. synthesis C. redox D. combustion 45. The positive or negative number that indicates how many electrons an atom has gained, lost, or shared to become stable is always the A. oxidation number. B. elemental charge. C. ionic charge. D. polarity. 46. Which statement best describes what happens to sodium and chlorine atoms when they combine to form sodium chloride? A. the sodium atom becomes a positive sodium ion, and the chlorine atom becomes a negative chloride ion. B. the sodium atom becomes a negative sodium ion, and the chlorine atom becomes a positive chloride ion. C. the sodium atom becomes a positive chloride ion, and chlorine atom becomes a negative sodium ion. D. the sodium atom becomes a negative chloride ion, and the chlorine atom becomes a positive sodium ion. 47. Which of these would penetrate a car door made of aluminum? A. alpha particles B. beta particles C. gamma rays D. helium nuclei 48. Which of these is not a type of nuclear radiation dangerous to human tissue? A. alpha particles B. beta particles C. gamma rays D. microwaves 49. Which statement provides the best description of transmutation? A. change in genetic material due to radiation B. change of one element to another through nuclear decay C. nuclear reactors are the cause of all transmutations D. can be speeded up or slowed down by chemical intervention 50. In Einstein’s famous equation, E = mc 2, what does m represent in a nuclear reaction? A. the mass of the starting materials in a nuclear reaction B. the total mass of starting materials plus ending materials in a nuclear reaction C. the small mass of light needed to begin a nuclear reaction D. the mass that is converted to energy in a nuclear reaction