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Fall Final Exam Review

Fall Final Exam Review. Scientific Method. 1- Which of the following is the most important thing with regard to protecting your eyes while in a science laboratory? Never look directly into a light source.

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Fall Final Exam Review

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  1. Fall Final Exam Review

  2. Scientific Method 1- Which of the following is the most important thing with regard to protecting your eyes while in a science laboratory? • Never look directly into a light source. • If you get a chemical in your eyes, immediately go to an eyewash station and flush your eyes and eyelids for 15 minutes. • Always wear safety goggles while performing laboratory work, including cleanup • Do not wear contact lenses while in the lab.

  3. Scientific Method (Continue) 1- The observation that the sun sets in the west would be considered. a. a scientific law. c. a scientific model b. a scientific theory d. an inference (conclusion) 2- A series of orderly steps used to solve problems is a. the experimental process. c. the scientific theory. b. A procedure. d. the scientific method.

  4. Scientific Method (Continue) 1- Which question cannot be answered by experimentation? • Does penicillin kill Salmonella bacteria? • Is rabies caused by a virus? • Did a comet kill the dinosaurs? • Can radiation cause cancer?  2- Before beginning an experiment, you should always ______. a. mix all the solutions together c. weigh all substances b. read all instructions d. answer pre-lab questions 

  5. Scientific Method (Continue) Scientists wished to determine if a new type of antibiotic, called Antibiotic F, was effective against a particular type of bacteria that causes pneumonia. To test the antibiotic, the scientists enlisted 100volunteers, who were all suffering from pneumonia. The scientists gave 50 of the volunteers Antibiotic F for 10 days. The remaining 50 volunteers were given a sugar pill (called a placebo) that looked like the antibiotic. A volunteer was considered to be cured when their temperature remained normal (37oC) for three days.

  6. Scientific Method (Continue) 1- What problem was being investigated by the scientists? • Is pneumonia caused by bacteria? • Is Antibiotic F effective against pneumonia causing bacteria? • How many people can be cured of pneumonia? • How many days does it take to cure pneumonia?   2- What was the experimental group? • The bacteria. • The volunteers that received the antibiotic. • The volunteers that received the placebo. • The sugar pill.  3- Was there an experimental control (group)? • No • Yes, the bacteria. • Yes, the volunteers that received the antibiotic. • Yes, the volunteers that received the placebo (sugar pill).

  7. Scientific Method (Continue) 1- What type of observation is “The water temperature is 25oC”? • Subjective b. Qualitative c. Quantitative d. Vector 2- Scientist test a hypothesis by a. formulating questions. c. designing models. b. performing experiments. d. drawing conclusions.  3- The metric unit for volume of a fluid is • liters b. meters • c. grams d. cubic centimeters (cm3)

  8. Scientific Method (Continue) 1- The figures to the right represents a graduated cylinder before and after an object was placed in it. What is the volume of the object? • 14 cm3 • 15 ml • 20 ml • 24 cm3

  9. Scientific Method (Continue) 25 Graph #1 – The relationship between time and and the temperature of a sodium 20 bicarbonate solution. Temperature 15 10 5 0 2 4 6 8 10 12 Time 1- In a graph, the independent variable is • Temperature • Time • Sodium bicarbonate • Decreasing (going down) 2- An appropriate interpretation of the data in the graph is • As time decreases, the temperature decreases and then remains the same. • As time increases, the temperature goes down. • As the temperature goes down, the time increases. • As time increases, the temperature goes down and then remains the same.

  10. Density (Continue) 2- A block of maple wood with a volume of 405 cubic centimeters and a density of 0.67 g/cm3 is sawed in half. The density of the two smaller blocks is now — A one-fourth the original density B one-half the original density C two times the original density D the same as the original density

  11. Density 1- The density of a 10.0 gram liquid that has a volume of 5 ml is ________. a. 20 g/ml c. 5 g/ml b. 2 g/ml d. 0.5 g/ml 2- Methanol has the density of 0.79g/ml. How much would be the mass of 589ml of methanol?  mass = density x volume = 0.79 g/ml x 589 ml = 465.31g 3- Copper has the density of 8.90 g/ml. What would be the volume of 746g sample of copper?  volume = mass/density= 465.31g/(8.90g/ml)=52.28ml 4- Calculate the density of a solid, knowing that the mass is 123.4g and the volume is 14.3ml. Density= mass/volume = 123.4g/14.3ml = 8.63g/ml  5- the tendency of a less dense object to float in a more dense liquid is called • viscosity • density • sublimation • buoyancy

  12. Density (Continue) 1- Swimmers find that they can float more easily in the ocean than in a freshwater pond. The most likely reason for this phenomenon is that the — A viscosity of pond water is greater than that of ocean water B density of ocean water is higher than that of pond water C temperature of pond water is lower than that of ocean water D mass of ocean water is greater than that of pond water

  13. Density (Continue)

  14. Viscosity 1- The resistance of a fluid to flow is referred to as a. Pressure b. energy c. Viscosity d. shape

  15. Heating Curve of water

  16. Bonding 1.  What kind of chemical bond is formed when electrons are transferred from one atom to another? • Covalent b. ionic c. metalllic d. transition 2. In the formula Fe2O3, what is the oxidation number for iron? a. 3+ b. 4+/- c.3- d. 2+ 3. A group of atoms that acts as one charged atom is a ______. a. Molecule c. positive ion b. negative ion d. polyatomic ion  4. The formula for Calcium Carbonate is ________ . a. CCa4 b. C2CO3 c. CaCO3 d. Ca3OH

  17. Bonding (Continue) 1- The name for Ca(OH)2 is ________. a. calcium hydroxide c. hydroxide calcium b. calcium oxygen hydrogen d. calcium dihydroxide 2- The name for CCl4 is ________. a. carbon tetrachloride c. carbon chloride b. carbon chlorine d. chlorine carbon 3- What type of bond does the chemical compound KCl contain? a. ionic c. both ionic and covalent b. covalent d. polar 

  18. Bonding (Continue) 1- Water is a polar molecule because it ______. • shares electrons • shares electrons unequally • transfers electrons • transfers electrons unequally

  19. Periodic table

  20. Periodic Table (Continue) 1-The element Magnesium is classified as a • Nobel gas b. Transition metal c. Alkaline-Earth metal d. Halogen 2- What do elements H, Na, and Li all have in common? a. They have one valence electron. c. They belong in same period. b. They commonly form covalent bonds. d. They take electrons during bonding. 3- Elements in groups 3 – 12 on the periodic table are called ______. a. metalloids c. nonmetals b. transition metals d. ions 4- Hydrogen is grouped with the alkali metals because it ______. a. is a metal c. is a gas b. has one valence electron d. does not easily form compounds

  21. Periodic Table (Continue) 1- Atoms of the same element with different numbers of neutrons are called ______. a. groups c. clusters b. Isotopes d. ions 2- Antimony (Sb) is a ______. a. metal c. metalloid b. nonmetal d. transition meta

  22. Periodic Table (Continue) • 1- Substances that conduct electric current under certain conditions are most likely ______. • metals b. metalloids • c. nonmetals d. noble gases  • 2-What is the oxidation number for Silicon? • 3+ b. 4+/- c. 3- d. 2+ • 3- Where are metals found on the periodic table? • a. left side c. along the staircase • b. right side d. at the bottom • 4- Horizontal rows on the periodic table are called ______. • a. groups c. clusters • b. families d. periods • 5- What kind of chemical bond occurs when atoms share electrons? • a. covalent b. metallic c. ionic d. mixed

  23. Periodic Table (Continue) 1- Which element has 35 protons? a. chlorine c. argon b. bromine d. iodine  2- A certain atom has 92 protons, 92 electrons and 146 neutrons. Its mass number is ______. a. 184 c. 238 b. 146 d. 54  4- How many electrons are needed in the outermost energy level of most atoms to be chemically stable? a. 2 b. 6 c. 8 d. 10 5- Group 17 on the periodic table is known as the ______. a. alkaline earth metals c. halogens b. alkali metals d. noble gases

  24. Periodic Table (Continue) • Which of the following is NOT a property of nonmetals? • can be solids, liquids or gases c. dull • conduct electricity d. brittle • The nucleus of an atom contains the ______. • protons only c. protons and neutrons • neutrons only d. protons and electrons  • The chemical symbol for Potassium is ______. a. P b. K c. Po d. Pt • Which of the following is NOT a characteristic of metals? • are shiny c. brittle • are malleable d. conduct electricity 

  25. Chemical Reactions 1- What type of reaction is 2KCl  2K + Cl2? a. synthesis c. single replacement b. decomposition d. double replacement 2- What type of reaction is 3NaOH + FeCl3 NaCl + Fe(OH)3? a. Synthesis c. single replacement b. Decomposition d. double replacement 3- What type of reaction is 2KCl  2K + Cl2? a. Synthesis c. single replacement b. Decomposition d. double replacement

  26. Rock Cycle

  27. Rock Cycle (Continue)

  28. Rock Cycle (Continue)

  29. Chemical Reactions (Continue)

  30. Chemical Reactions (Continue) 1- A chemical reaction in which energy is released is ______. a. exothermic c. flammable b. endothermic d. decomposing  2- Each substance on the left side of the arrow in a chemical equation is a ______. • reactant b. catalyst c. product d. inhibitor  3- Coefficients (the numbers in front of) the chemical formulas in a chemical equation show • the number of atoms of each element. • the number of molecules. • the number of reactants. • the number of products.  4- Subscripts represent • the number of atoms of each element. • the number of molecules. • the number of reactants. • the number of products

  31. Chemical Reactions (Continue) 1- Which of the following shows a correctly balanced chemical equation for the following reaction? a. 2 Mg + O2 MgO c. Mg + 2 O2 MgO b. 2 Mg + O2 2 MgO d. 2 Mg + 2 O2 2 MgO 2- When one element displaces another element in a compound, this reaction is a ______. a. synthesis c. single replacement b. decomposition d. double replacement 

  32. Chemical Reactions (Continue) 1- According to the law of conservation of mass, how much zinc was present in the zinc carbonate? A 40 g B 88 g C 104 g D 256 g

  33. Properties of Matter 1- The image that represents a solid is _____ . a. A b. B c. C d. None of the above. 2- The phase that possesses the greatest amount of energy would be ______. a. A b. B c. C d. None of the above 3- Most matter ______ when heated. a. condenses b. expands c. contracts d. solidifies

  34. Properties of Matter (Continue) 1- As a sample of matter is cooled, its particles ______. a. move more slowly c. do not change b. move more quickly d. stop moving 2- The change of state in which a gas changes into a liquid is ______. a. melting b. sublimation c. freezing d. condensation 3- Vaporization refers to the phase change from a. liquid to gas. c. solid to liquid. b. gas to liquid. d. liquid to solid. 4- All matter is made up of tiny particles that are in constant motion is known as ______. a. law of conservation of mass c. kinetic theory of matter b. law of conservation of energy d. archimedes’ principle 

  35. Properties of Matter (Continue) 1- Which of the following is not a physical property of matter? a. mass b. color c. density d. flammability 2- Ice (solid water) floats because a. it is more dense than water. b. it is less dense than water. c. it is the same density as water. d. it has fewer total particles than water.

  36. Properties of Matter (Continue) E D   B C A Heat Energy 1- What portion of the diagram represents a solid? a. A b. B c. C d. D e. E  2- What line segment represents vaporization? a. A b. B c. C d. D e. E  3- If heat energy were being removed from the substance in the diagram, Line Section “B” would represent a. a solid. b. condensation c. melting. d. freezing.

  37. Properties of Matter (Continue) • What happens to the temperature of a substance while it is undergoing a phase change? • it increases c. it stays the same until the change is complete • it decreases d. nothing  • The particles in a solid move ______ than particles in a gas (at the same temperature). • more quickly c. the same • more slowly d. depends on the substance

  38. Properties of Matter (Continue) • Which of the following is a CHEMICAL property? • Color c. density • melting point d. ability to rust  • Which of the following is a PHYSICAL change? • rusting b. evaporating • c. burning d. corroding • Which of the following is a homogeneous mixture? a. water. c. isopropyl (rubbing) alcohol. b. italian salad dressing. d. grape kool-aid 4. Which one of the following represents a correctly balanced equation for the following equation? KI + Br2 KBr + I2 • 2 KI + 2 Br2 2 KBr + I2 c. 2 KI + Br2 2 KBr + I2 • 2 KI + Br2 2 KBr + 2 I2 d. 3 KI + Br2 3 KBr + I2

  39. Properties of Matter (Continue) • The change of state in which a liquid changes into a solid is ______. • Evaporation c. melting • Freezing d. sublimation 2. The color of ink is a ______. • chemical property c. chemical change • physical property d. physical change 3. Smoke is an example of a ______. • colloid b. suspension c. solution d. molecule  4. Temperature is a measure of a. how hot or cold something is. c. degrees Celsius b. particle motion. d. cubic centimeters (cm3) 

  40. Properties of Matter (Continue) • Which of these is NOT homogeneous? a. a compound c. a solution b. an element d. a suspension • the law of the conservation of mass states that mass cannot be • Burned b. changed in form • created or destroyed d. heated or cooled   • during a chemical or physical change, energy may be a.created c. destroyed b. greatly increased in strength d.converted into another form 4. all changes of the state of matter require • Water b. vibration c. Energy d. sublimation

  41. Properties of Matter (Continue) 1- you burn a log of wood and only a small pile of ashes is left, what has happened? • a large amount of mass has been lost • a small amount of mass has been turned into a large amount of heat energy • the total amount of wood and oxygen is the same as the amount of ash and gases • the total amount of energy is less than before  2- knowing the chemical properties of a substance will tell you how the substance • Looks c. can be broken down into atoms • Smell d. reacts with other substances 3- which of the following is an example of physical change • dissolving salt in water c. cooking an egg • burning wood into charcoal d. rusting iron  4- ice floats in water because it is • more dense than water c. colder than water • less dense than water d. warmer than water

  42. Properties of Matter (Continue) 1- which of the following is not an example of a physical property? • freezing point c. reactivity • boiling point d. density  2- which of the following is an example of chemical change? • ice melting c. pounding gold into a coin • paint fading d. a puddle of water evaporating  3- digesting food is an example of • physical change c. chemical change • change of state d. physical change  4- grinding quartz crystals down to produce sand is an example of a • change in state c. chemical reaction • chemical change d. physical change

  43. Properties of Matter (Continue) 1- The smallest unit of a substance that behaves like a substance is • an element c. a molecule • an atom d. a compound 2- The kinetic theory states that the higher the temperature, the faster the • the particles that make up the substance move • bonds between atoms break • molecules of gas rush together • the lighter particles within a substance clump together 3- you put on gram of salt in one liter of water and stir the resulting liquid is an example of • pure substance c. a homogeneous • a heterogeneous mixture d. immiscible

  44. Acids & Bases 1- Coffee has a pH of about 5. Coffee is a ______. a. strong acid c. strong base b. weak acid d. weak base  2- Lye has a pH of 13.8. Lye is a ______. a. strong acid b. strong base c. weak acid d. weak base  3- Red litmus paper turns blue in a ______. • acid b. base c. either acid or base d. neither acids nor bases 4- The terms dilute and concentrated refer to the ______ of a solution. a. acidity c. pH b. concentration d. strength  5- A substance that produces OH- ions in solutions is a ______. a. acid c. salt b. base d. water

  45. Acids & Bases (Continue) 1- A substance that produces H+ ions in a solution is a ______. a. acid b. salt c. base d. soap  2- OH- represents _____. a. the hydroxide ion c. oxygen hydride b. hydrochloric acid d. sodium hydroxide  3- Blue litmus paper turns red in a ______. a. acid c. either acid or base b. base d. neither acids nor bases 4- A reaction between an acid and a base that produces salt and water is a ______ reaction. a. Synthesis c. neutralization b. Decomposition d. combustion

  46. Solutions 1- The terms dilute and concentrated refer to the ______ of a solution. a. acidity c. pH b.concentration d. strength 2- When a gas is dissolved in a liquid, the gas dissolves faster if the liquid is ______. a. heated c. under low pressure b. cooled d. none of the above 3- Increasing the surface area of a solid ______. a. slows the rate of dissolving. c. has no effect on the rate of dissolving. b. speeds up the rate of dissolving d. increases the amount that can be dissolved. 4. The concentration of a solution that contains a small amount of solute in a solvent can be described as ______. a. saturated c. concentrated b. polar d. dilute

  47. Solutions (Continue) 1- A solution with a bitter taste and slippery feel is most likely a ______. • acid c. salt • base d. water  2- A solution that contains all the solute is can normally hold at a given temperature is ______. • saturated c. supersaturated • Unsaturated d. dilute  3- Sugar dissolved in water is an example of a ______. • homogeneous mixture • suspension • heterogeneous mixture • d. colloid

  48. Solutions (Continue) 1- Which of the following will NOT speed up the dissolving of a solid solute in water? • stirring the solution • heating the solution • crushing the solute • increasing pressure   2- A solution that contains less solute than it can hold at a given temperature is ______ a. saturated c. supersaturated b. unsaturated d. dilute  3- In a solution, the substance that is being dissolved is the ______. • solute c. liquid • solvent d. solid

  49. Solutions (Continue) 1- How much potassium nitrate is present in a saturated solution at 30oC? a. 35 grams b. 45 grams c. 65 grams d. 95 grams  2- At what temperature will 20 grams of potassium chlorate (KClO3) produce a saturated solution? a. 30 degrees b. 44 degrees c. 53 degrees d. 80 degrees 3- Will 80 grams of sodium nitrate (NaNO3) dissolve completely in 100 grams of water at 10oC? a. Yes b. No c. Maybe d. Not enough information

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