CHEM 131 Introduction To Chemistry With Lab Test Questions And Answers

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Lesson 1 Quiz Part 1 of 4 - 8.0/ 8.0 Points Question 1 of 12 4.0/ 4.0 Points Who discovered the atomic theory? A. Antoine Lavoisier B. John Dalton C. John Dalton and Antoine La... voisier D. Albert Einstein E. none of the above Answer Key: B Feedback: Good! It was Dalton. Question 2 of 12 4.0/ 4.0 Points Who discovered the law of conservation of mass? A. Albert Einstein B. John Dalton and Antoine Lavoisier C. Antoine Lavoisier D. John Dalton E. none of the above Answer Key: C Feedback: Good. It was Lavoisier. Part 2 of 4 - 4.0/ 12.0 Points Question 3 of 12 4.0/ 4.0 Points A lead ball has a mass of 49.0 grams and a density of 11.3 g/cm3. What is the volume of the ball? A.0.0340 cm^3 B.554 cm^3 C.0.231 cm^3 D.4.34 cm^3 E.none of the above Answer Key: D Feedback: Good! This is simply an application of d = m/v. Question 4 of 12 0.0/ 4.0 Points What is the volume in mL of a cube of water with dimensions 11.0 cm × 11.0 cm × 11.0 cm ? A.1.33 × 103 B.1.3 × 103 C.1.33 × 10-3 D.1.331 × 10-3 E.none of the above Answer Key: A Feedback: This is discussed in section 2.8 in the text. Question 5 of 12 0.0/ 4.0 Points When the value 98.54 is rounded to two significant figures, the number should be reported as: A.98 B.98.5 C.99 D.100 E.none of the above Answer Key: C Feedback: Rounding associated with sig figs is discussed in section 2.4 of the text. Part 3 of 4 - 4.0/ 20.0 Points Question 6 of 12 4.0/ 4.0 Points `Given the sequence of temps below, which one represents the Fahrenheit boiling, room temp, and freezing points of water, in that order? A.0-75-100 B.212-75-32 C.0-25-100 D.0-298-373 E.none of the above Answer Key: B Question 7 of 12 0.0/ 4.0 Points `How should someone classify grape juice? A.mixture-homogeneous B.pure substance-compound C.mixture-heterogeneous D.pure substance-element E.none of the above Answer Key: A Question 8 of 12 0.0/ 4.0 Points `Gallium metal will melt in your hand. Which of the following is a true statement about this process? It represents a . A. physical change B. chemical property C. chemical change D.distillation E.none of the above Answer Key: A Question 9 of 12 0.0/ 4.0 Points `A solid that does not have a long range repeating order is called . A.fixed B.rigid C.amorphous D.crystalline E.none of the above Answer Key: C Question 10 of 12 0.0/ 4.0 Points `Please select the TRUE statement below. A.Mixtures may be composed of just one type of element. B.A pure substance may consist of two or more different compounds. C.A mixture cannot be homogeneous. D.Matter may be a pure substance or it may be a mixture. E.All of the above statements are true. Answer Key: D Part 4 of 4 - 0.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points `IN YOUR OWN WORDS, who was John Dalton, and why is he so important to chemistry? What did he "discover" that is so central to our study of chemistry? Explain why it is important. I believe that John Dalton discovered Law of Partial Pressures, Law of Stoichiometry, and Atomic Theory, but he did not invent anything that I know of. Feedback: See section 1.4 Question 12 of 12 0.0/ 5.0 Points `Human remains are typically cremated at a temperature of about 870.0 degrees C. (1) What is this temperature in F? (2) What is this temperature in K? All work must be shown, labeled, and explained in detail to receive credit. Note that where applicable, superscripts (X2) can be written as X^2 and subscripts (X2) can be written as X_2 if it saves you time. Feedback: See section 3.10 Lesson 2 Quiz Return to Assessment List Part 1 of 3 - 12.0/ 20.0 Points Question 1 of 12 0.0/ 4.0 Points `If a nickel atom formed an ion, what charge would it have? A.1+ B.1- C.2- D.2+ E.it cannot be determined based on the information given Answer Key: E Feedback: See section 4.7. Transition metals can have various charges, though they will all be positive. Question 2 of 12 4.0/ 4.0 Points `The elements located in groups 3B through 2B are known as A.halogens B.transition metals C.alkaline earth metals D.noble gases E.none of the above Answer Key: B Feedback: See section 4.6 Question 3 of 12 4.0/ 4.0 Points `Which of these can be found in the nucleus? A. protons and electrons. B. only protons C.electrons and neutrons D.protons, neutrons, and electrons. E.protons and neutrons. Answer Key: E Feedback: See section 4.3 Question 4 of 12 4.0/ 4.0 Points `If iodine were to form an ion, what would its charge be? A.2- B.1+ C.1- D.2+ E.none of the above Answer Key: C Feedback: See the periodic table and section 4.7 Question 5 of 12 0.0/ 4.0 Points `Of the scientists listed below, which one did not contribute to developing the model of the atom? A.Rutherford B.Thomson C.Democritus D.Mendeleev E.Dalton Answer Key: D Feedback: See sections 4.2 through 4.5 Part 2 of 3 - 12.0/ 20.0 Points Question 6 of 12 4.0/ 4.0 Points `What would be the proper way to write the ion formula for acetate? A.C3H2O - B.C2H3O - C.C2H3O- D.C2H3O 2- E.none of the above Answer Key: B Feedback: use naming rules and polyatomic ion list Question 7 of 12 0.0/ 4.0 Points `When naming Na3PO4 , it cannot be trisodium phosphate. Why? A. this compound should be called trisodium monophosphate. B. you cannot use a prefix for the first element of an ionic compound. C. you cannot use a prefix for the first element in a molecular compound. D. the sodium has a negative 3 charge. E. none of the above Answer Key: B Feedback: use naming mechanism Question 8 of 12 4.0/ 4.0 Points `We discussed diatomic molecules in this lesson. Which of these would NOT be classified in that category? A.nitrogen B.fluorine C.hydrogen D.neon E.all of these are diatomic Answer Key: D Feedback: see section 5.4 Question 9 of 12 4.0/ 4.0 Points `What would be the proper way to write the polyatomic ion formula for perchlorate? A.ClO- B.ClO4- C. ClO - D. ClO - E. none of the above Answer Key: B Feedback: use naming rules and polyatomic ion list Question 10 of 12 0.0/ 4.0 Points `How many oxygen atoms are in the formula Al2(CO3)3? A.1 B.6 C.3 D.9 E.none of the above Answer Key: D Feedback: use formula to count Part 3 of 3 - 0.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points `Chemistry really is another language sometimes. It abbreviates a lot, and chemical formulas are a way to write a little and still convey a lot of information. For example, consider the chemicals hydrogen, cadmium (III) acetate, Lead (II) Iodide, and tetranitrogen nonasulfide. Translate these names into chemical formulas using the appropriate procedure described in the course text and my lecture material. Answer the following: (1) What is the correct formula of each of these compounds? (2) Explain how exactly (i.e. the procedure used) you arrived at your answer...in other words, walk me through your thinking. You will not receive credit if you don't show your work in detail. Feedback: chapter 5 discusses naming Comment: :o( Question 12 of 12 0.0/ 5.0 Points `Describe, in detail, the "anatomy" of an atom. Include a discussion of all subatomic particles, any associated charges, their locations, how they interact with one another, and explain which of these particles actually identify the atom on the periodic table. Also include a discussion on which of these may change in number in the case of isotopes. Model Short Answer: this comes from chapter 4 Feedback: this comes from chapter 4 Comment: No answer Diane? Lesson 3 Quiz Return to Assessment List Part 1 of 4 - 0.0/ 8.0 Points Question 1 of 12 0.0/ 4.0 Points `I recently went to the dentist for a procedure that required me to have laughing gas (nitrous oxide, or N2O). I specified that I wanted EXACTLY 1.000 x 1025 molecules of this gas delivered to me. If he was going to be my dentist, he had to prove to me he knew a little chemistry. How many grams would he have to deliver? A.1.100 × 103 B.44.01 C.730.9 D.16.61 Answer Key: C Feedback: See section 6.3 Question 2 of 12 0.0/ 4.0 Points `When answering the question of what I would do for a Klondike bar, I said I would jump into the Nile river with a crocodile while wearing 5.50 x 1025 atoms of lead on my body. What would be the mass of this lead in kg? A.1.89 B.18.9 C.1.14 x 1025 D.1.60 x 1045 E.6.022 x 1023 Answer Key: B Part 2 of 4 - 0.0/ 16.0 Points Question 3 of 12 0.0/ 4.0 Points `In the image below, which reaction type is represented in equation 2? A.single displacement B.double-displacement C.decomposition D.synthesis/combination E.none of the above Answer Key: C Feedback: See section 7.10 Question 4 of 12 0.0/ 4.0 Points `If I ask you to write an equation representing a chemica reaction, you must first know A. the molar mass of all the reactants and products. B. the amount of moles of all compounds involved C. the atomic mass of each atom involved. D. the symbols and formulas of all reactants and products. E. none of the above. Answer Key: D Question 5 of 12 0.0/ 4.0 Points `Oxidation-reduction reactions are also known as redox reactions. We learned about their unique characteristics in this lesson. Which of the following would be a FALSE statement given what we learned about redox reactions? A. if an atom gains 1 or more electrons, it is "reduced" B. when a redox reaction occurs, either reduction happens or oxidation happens, but never both in the same reaction C. Redox reactions often involve elemental oxygen D. If an atom loses 1 or more electrons, it is "oxidized" E. All of the above statement are true. Answer Key: B Feedback: See section 7.9 Question 6 of 12 0.0/ 4.0 Points `There are many signs we can observe to tell us if a chemical reaction has taken place. Which of these would NOT be one of those signs? A.absorption of light B.absorption of heat C. release of heat D. release of light Answer Key: A Feedback: See section 7.2 Part 3 of 4 - 4.0/ 16.0 Points Question 7 of 12 0.0/ 4.0 Points `You have to be careful about pouring drano down your pipes since it is mainly hydrochloric acid--you can't do it if they are made of aluminum because it will dissolve them! You can't acid clean your aluminum auto parts for the same reasons: 2 Al + 6 HCl → 2 AlCl3 + 3H2. If you were able to dissolve 10.0 mol of Al, how many many moles of hydrogen gas could you make? NOTE: All numbers located immediately after elemental symbols should be considered subscripts. A.3.00 moles B.6.00 moles C.1.50 moles D.15.0 moles E.none of the above Answer Key: D Feedback: See section 8.6 Question 8 of 12 4.0/ 4.0 Points `Suppose you were tasked with producing some nitrogen monoxide (a.k.a. nitric oxide). I'm sure this is often requested of you. You can do it by combusting ammonia (be careful!). The equation would be as follows: 4NH3 + 5O 2→ 4NO + 6H2O. If you form 3.50 mol of water, how much NO forms? A.2.33 mol. B.4.00 mol. C.4.50 mol. D.6.75 mol. E. none of the above Answer Key: A Feedback: Good. See section 8.6 Question 9 of 12 0.0/ 4.0 Points `Sodium and chlorine are very dangerous by themselves. However, when we combine them together in a chemical reaction, we eat it--it's table salt: 2Na + Cl2 → 2NaCl. If I want to make 100.0 g of my own salt (because I can and that's how I roll), how much elemental chlorine would I need? NOTE: All numbers located immediately after elemental symbols should be considered subscripts. A.100.0 g B.50.0 g C.25.0 g D.60.67 g E.not enough information Answer Key: D Feedback: See section 8.6 Question 10 of 12 0.0/ 4.0 Points `Sodium and chlorine are very dangerous by themselves. However, when we combine them together in a chemical reaction, we eat it--it's table salt: 2Na + Cl2 → 2NaCl. If I want to make 50.0 g of my own salt (because I can and that's how I roll), how much elemental sodium would I need? NOTE: All numbers located immediately after elemental symbols should be considered subscripts. A.50.0 g B.100.0 g C.22.99 g D.19.67 g E.not enough information Answer Key: D Feedback: See section 8.6 Part 4 of 4 - 0.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points `Alkali metals are extremely reactive with water. Suppose I give you a 55.50 g chunk of cesium and you throw it into a lake. When it reacts with water to form cesium hydroxide and hydrogen gas, how much hydrogen in grams is theoretically produced? Write a balanced equation for the reaction and show all work clearly and in detail to receive credit. All numbers seen immediately following the elemental symbols are intended to be subscripts. Feedback: Use your limiting reactant to predict product formation. Comment: No solution...:o( Question 12 of 12 0.0/ 5.0 Points `Consider the solubility rules and identify all of the spectator ions when the following chemicals react: A) lead (II) nitrate and ammonium chloride B) Barium bromide and potassium carbonate. You must show all work (equations) clearly and in detail to receive credit. Feedback: This concerns net ionic reactions and the formations of precipitates. Comment: No solution Diane..? Lesson 4 Quiz Return to Assessment List Part 1 of 3 - 8.0/ 20.0 Points Question 1 of 12 0.0/ 4.0 Points `Having learned about electromagnetic radiation in this lesson, which of these statements about it is true? A. when wavelength increases, energy decreases B. when wavelength increases, frequency increases C. Red light wavelength is shorter than green light. D. when energy increases, frequency decreases E. none of the above Answer Key: A Feedback: See section 9.3 Question 2 of 12 4.0/ 4.0 Points `In terms of wavelength, which of these is the longest? A. Infrared Radiation B. Radio Waves C. Gamma Rays D.Microwaves E.X-rays Answer Key: B Feedback: Good. See section 9.3 Question 3 of 12 0.0/ 4.0 Points `Which of the following statements is true about atomic size? A.increases down a group and from right to left across a period. B.increases up a group and diagonally across the Periodic Table. C.increases down a group and from left to right across a period. D.increases up a group and from right to left across a period. E.increases up a group and from left to right across a period. Answer Key: A Question 4 of 12 0.0/ 4.0 Points `Write out the electron configurations of the ions below and determine which one is listed with an incorrect charge. (the numbers and charges written after the elemental symbol should be understood as superscripts) A.I- B.O2+ C.Al3+ D.Mg2+ E.none of the above Answer Key: B Feedback: See section 9.7 Question 5 of 12 4.0/ 4.0 Points `If I time the movement of waves for 1 second, and calculate that 100 waves passed through in that 1 second, what have I calculated? A.crest B.amplitude C.wavelength. D.frequency. E.none of the above Answer Key: D Feedback: Good. See section 9.3 Part 2 of 3 - 4.0/ 20.0 Points Question 6 of 12 0.0/ 4.0 Points `Geometrically linear means that the electron groups have what angle? A.90° B.120° C.109.5° D.180° E.not enough information Answer Key: D Feedback: See section 10.7 Question 7 of 12 0.0/ 4.0 Points `Geometrically trigonal planar means that the electron groups have what angle? A.120° B.90° C.180° D.109.5° E.not enough information Answer Key: A Feedback: See section 10.7 Question 8 of 12 0.0/ 4.0 Points `Some atoms are better at attracting electrons compared to others. Which term below best describes that? A. polar covalent B. nonpolar covalent C.electronegativity D.dipole moment E.coulombic attraction Answer Key: C Feedback: See section 10.8 Question 9 of 12 4.0/ 4.0 Points `According to the electronegativity table, the value for barium and sulfur is 0.9 and 3.5, respectively. What type of bond would you expect to form between these two elements? A.Polar covalent B.Ionic C. Pure covalent D. not enough information E. none of the above Answer Key: B Feedback: Good. See section 10.8 Question 10 of 12 0.0/ 4.0 Points `Regarding boron trifluoride, which of these is TRUE? A.the central atom does not obey the octet rule B. it is not polar C. it's molecular geometry is trigonal planar D. all of these are true E. None of these are true. Answer Key: D Feedback: See section 10.7 Part 3 of 3 - 0.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points `On December 5, 1971, at the mere age of 35, the great composer Wolfgang Amadeus Mozart died after a three month long battle with illness. Rumor was that a rival musician had poisoned him, but it turned out that common consensus was that the antimony prescription that doctors had prescribed him was actually poisoning him. (a) What is the full and abbreviated electron configuration for this element? Explain how you arrived at this configuration. In other words, don't just give me the configuration, but walk me through and explain to me how exactly you arrived at your answer. (b) In this Lesson we talked about the relationship between frequency and wavelength. The relationship can actually be expressed as where f is the frequency, c is the speed of light (see below), and lambda (the symbol on the left of the equals sign that looks like an upside down y) is wavelength. The particle nature of light was first proposed by Einstein, who suggested that light could be described as a stream of particles called photons. A photon of a certain wavelength (lambda) has an energy (E) given by the equation: where E is the energy of the photon in J, h is Planck's constant (6.626 x 10-34 J*s), and c is the speed of light (3.00 x 108 m/s). If we determine the wavelength (lambda) of light emitted from a sample of antimony to be 206.8 nm, what is the energy (E) and frequency (f) that corresponds to this wavelength? You must show all work to receive credit. HINT: 1 nm = 1 x 10-9 m; be sure all units are able to cancel out as necessary HINT: Plug in the values you know. You can substitute values between these equations. Feedback: This is from chapter 9. Question 12 of 12 0.0/ 5.0 Points `Think about it--why is the line spectrum produced by excited barium atoms more complex than the line spectrum produced by excited sodium atoms? Be sure to base your answer on what we discussed in THIS class and use the terminology from the materials in THIS course. Your answer must be sufficiently detailed to receive credit. Feedback: Emission spectra are discussed in Chapter 9. Lesson 5 Quiz Return to Assessment List Part 1 of 3 - 12.0/ 20.0 Points Question 1 of 12 4.0/ 4.0 Points `Given the conversion factors and definitions discussed in the lesson, which of the following is equivalent to 2 atm? A. 1,520 torr. B. 1,520 mm Hg. C.29.4 psi. D.202,650 Pa. E.all of these choices Answer Key: E Feedback: Good. Gas law conversions are discussed in section 11.3 Question 2 of 12 4.0/ 4.0 Points `Which sentence below is NOT true about pressure? A. After creating a pressure difference, the atmospheric pressure can push liquid up a straw. B. The atmosphere has a pressure as the components of air collide with surfaces. C.A deep well dug in the ground must have the pump located at the bottom of well in order to have the water come to the surface. D.Pressure is caused by gas molecules colliding with surfaces. E.All of the above statements are true. Answer Key: E Feedback: Good. pressure is discussed in 11.3 Question 3 of 12 0.0/ 4.0 Points `You've got gas! A sample of it that, is. More specifically, a 350.0 mL sample in an flexible container that has a temperature of 293.15 K. Suppose you throw it on the stove and heat it to 373.15 K. What will the new volume be (in L)? A.2.75 L B.17.5 L C.0.224 L D.0.446 L Answer Key: D Feedback: This is Charles' Law, section 11.5 Question 4 of 12 0.0/ 4.0 Points `I have a cylinder sitting in my lab that contains 1.55 L of gas, and it's temperature is 305.15 K. If I compress the cylinder and change the volume to 0.755 L, what will be the new temperature in Celsius? A.149°C B.-124°C C.353°C D.273°C Answer Key: B Feedback: Charles' law is discussed in 11.5 Question 5 of 12 4.0/ 4.0 Points `I have a pressure cooker in my underground lair that is brewing a diabolical solution. I set everything up and went upstairs, but forgot to write down the initial temperature. When I came downstairs later to check on it, I see that the pressure gauge shows that the pressure has decreased by 10 times, while the volume increased by 5 times. The temperature now reads -123.15 °C. What was the starting temperature when I left (in °C)? A.-198 B.75 C.27 D.300 Answer Key: C Feedback: Good. Combined gas law is discussed in 11.6 Part 2 of 3 - 4.0/ 20.0 Points Question 6 of 12 0.0/ 4.0 Points `A liquid generally wants to decrease the area of its surface as much as possible. The natural tendency to do this is known as what? A.viscosity. B.vaporization. C.capillary action. D.surface tension. E.none of the above Answer Key: D Feedback: This action is discussed in 12.3 Question 7 of 12 0.0/ 4.0 Points `When you put water into an ice cube tray and stick it in the freezer to make ice, which of these is true? A. it is an exothermic process. B. the process is referred to scientifically as sublimation. C. it is an endothermic process. D. the heat of vaporization must be removed. E. none of the above Answer Key: A Feedback: Freezing is discussed in 12.5 Question 8 of 12 0.0/ 4.0 Points `Most people don't realize that once something starts to melt, cranking up the heat does't make the temperature of the substance higher, at least not until it is ALL melted. When you add lots of extra heat to a solid that is in the process of melting, what ends up happening to all of this extra energy you are adding? It is used to do what? A. expand the solid. B. change solid to liquid. C. change the liquid back to solid. D. overcome the intermolecular forces that hold the solid together. E. raise the temperature of the solid above its melting point. Answer Key: B Feedback: Melting is discussed in 12.5 Question 9 of 12 0.0/ 4.0 Points `We discussed intermolecular forces in this lesson. What would be the result if we increased these forces within a liquid? It would... A. decrease the vapor pressure B. decrease the evaporation rate C. increase the surface tension D. increase the viscosity E. all of the above Answer Key: E Feedback: This can be answered from the info in 12.1 and 12.2 Question 10 of 12 4.0/ 4.0 Points `As we learned, matter exists in different states--solid, liquid and gas. Which one of these could be described as having low density and easily compressible? A.gases B.solids C.liquids D.both solids and liquids E.none of the above Answer Key: A Feedback: Good. This is discussed in 12.2 Part 3 of 3 - 0.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points `Oxygen is a nonpolar gas, but it will dissolve a little bit in water (which is a polar solvent. Which intermolecular force(s) is/are responsible for the interaction between the two compounds? Explain in detail to receive credit. Feedback: Intermolecular forces are discussed in Ch. 12 Question 12 of 12 0.0/ 5.0 Points `What is the temperature of a 926 L compressed gas tank that contains 64.1 mol of carbon monoxide at a pressure of 38.1 atm? You must show all work to receive credit. Feedback: Gas laws are covered in Ch. 11 Comment: No solution Diane?...please check into how to solve these, then ask for help...I am here ...:o) Lesson 6 Quiz Part 1 of 3 - 12.0/ 20.0 Points Question 1 of 12 4.0/ 4.0 Points 'Which of these statements is true regarding a gas's ability to dissolve in water? It... A.is independent of temperature. B.decreases with increasing temperature. C.increases with increasing temperature. D.gases are not soluble in water. E.none of the above Answer Key: B Feedback: Good. Gas solutions are discussed in 13.4 Question 2 of 12 4.0/ 4.0 Points 'Suppose you have a 0.10 M solution of AlBr3. What is the concentration of each ion? A.0.10 M Al3+ ions and 0.30 M Br- ions B.0.30 M Al3+ ions and 0.10 M Br- ions C.0.10 M Al3+ ions and 0.033 M Br- ions D.0.033 M Al3+ ions and 0.033 M Br- ions Answer Key: A Feedback: Good. See 13.6 Question 3 of 12 0.0/ 4.0 Points `Suppose you want to prepare a 2.50 M solution of sodium chloride. If you only have 0.325 moles of sodium chloride, and you must use it all, how many mL must you prepare? A.0.130 mL B.0.813 mL C.130. mL D.7.69 mL Answer Key: C Feedback: Solution concentration is in 13.6 Question 4 of 12 4.0/ 4.0 Points 'Water can dissolve many compounds What happens when an ionic substance dissolves in it? A. the positive end of water dipoles attract the negative ions. B. the solvent-solute attractive forces overcome the solute-solute attractions. C. the negative end of water dipoles attract the positive ions. D. each of the above (A, B, and C) occurs. E. none of the above (A, B, or C) occurs. Answer Key: D Feedback: Good. This is discussed in 13.3 Question 5 of 12 0.0/ 4.0 Points 'We discussed how some solutions are electrolytes in this lesson. Which of these would be a strong one? A.HCl B.NH4Cl C.NaC2H3O2 D.NaCl E.all of the above Answer Key: E Feedback: Electrolytes are in 13.3 Part 2 of 3 - 8.0/ 20.0 Points Question 6 of 12 0.0/ 4.0 Points `Suppose you have a sample of HC2H3O2 with a concentration of 2.0 M. So, what would be the [H+]? A.2.0 M B.>2.0 M C.< 2.0 M D.1.0 M Answer Key: C Feedback: Weak acids discussed in 14.7 Question 7 of 12 4.0/ 4.0 Points `We discussed many properties and characteristics of acids in this lesson. Which of the following is NOT one that was mentioned? A. Acids have a slippery feel. B. Acids have a sour taste. C. Acids dissolve many metals. D. Acids turn litmus paper red. E. All of the above are properties of acids. Answer Key: A Feedback: Good. Acid properties are discussed in 14.2 Question 8 of 12 4.0/ 4.0 Points `In this lesson we learned about Kw, which is known as the the ion product constant for water. What is this value? A.0.0 B.1.0 x 1014 C.1.0 x 10-7 D.1.0 x 10-14 E.1.0 x 107 Answer Key: D Feedback: Good. Water is discussed in 14.8 Question 9 of 12 0.0/ 4.0 Points `Bases have many useful properties that can be exploited for our own benefit. They are commonly used to make many things that we use. For example, which of these is associated with making fertilizer? A.NaHCO3 B.NH3 C.KOH D.NaOH E.all of the above Answer Key: B Feedback: Base properties and examples are discussed in 14.3 Question 10 of 12 0.0/ 4.0 Points `If a solution is acidic, which of the following is true? A.[H3O+] > [OH-] B.[H3O+] = [OH-] C.pH = pOH D.[H3O+] < [OH-] E.none of the above Answer Key: A Feedback: This is discussed in 14.7 Part 3 of 3 - 0.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points PART 1: How many milliliters of concentrated HCl (12.1 M) are needed to make the following amounts of acid? You must show all work in detail to receive credit. (a) 5.00 L of 0.100 M, (b) 1.00 L of 6.00 M, (c) 2.00 L of 3.00 M, (d) 100 mL of 0.100 M. PART 2: Explain, in detail, how you would go about making the solution in letter (a) above. Include all detail and terminology as discussed in the Lesson materials. Feedback: Solutions are discussed in Ch. 13 Question 12 of 12 0.0/ 5.0 Points **(PART 1) Calculate the boiling points of these solutions: 0.1 m Na2P 0.2 m NaBr 0.16 m C12H22O11 POTENTIALLY USEFUL INFORMATION: Kb for water = 0.512 C*kg solvent/mol solute ---You must show all work in detail to receive credit.--- (PART 2) Place the above solutions in order of boiling point from lowest to highest. You must show all work in detail to receive credit. Feedback: Colligative properties are discussed in Ch. 13 Comment: No solution Diane...:o( Lesson 7 Quiz Return to Assessment List Part 1 of 3 - 8.0/ 20.0 Points Question 1 of 12 0.0/ 4.0 Points `We discussed several different types of hydrocarbons in this lesson. Which one is saturated? A.alkynes B.alkenes C.alkanes D.all of these E.none of the above Answer Key: C Feedback: Saturation is discussed in 18.5 Question 2 of 12 0.0/ 4.0 Points `We discussed different types of organic reactions in this lesson, one of which was addition. Which if these will undergo this type of reaction? A.C2H6 B.C3H8 C.C2H4 D.all of the above E.none of the above Answer Key: C Feedback: reactions are discussed in 18.9 Question 3 of 12 4.0/ 4.0 Points `Endings (suffixes) in the naming process can tell us a lot about a chemical. For example, a compound named "butanal" would be categorized as a(n): A.ether. B.amine. C.aldehyde. D.alcohol. E.none of the above Answer Key: C Feedback: Good. This chemical group is discussed in 18.4 Question 4 of 12 0.0/ 4.0 Points `Consider the BLUE carbon atom in the formula shown below. What is its molecular geometry? A.bent B.linear C.trigonal planar D.tetrahedral E.none of the above Answer Key: B Feedback: This geometry is discussed in 18.8 Question 5 of 12 4.0/ 4.0 Points `We discussed benzene rings in this lesson. So, consider the compound chlorobenzene. How many carbon atoms would it have? A.5 B.1 C.7 D.6 E.none of the above Answer Key: D Feedback: Good. Benzene rings are discussed in 18.10 Part 2 of 3 - 12.0/ 20.0 Points Question 6 of 12 4.0/ 4.0 Points `We discussed different structures of proteins (primary, secondary, etc.). When considering the secondary structure, what is the repeating pattern that is commonly found along this chain? A.β-pleated sheet. B.β-turn. C.α-helix. D.random coil. E.none of the above Answer Key: C Feedback: Good. Protein structure is discussed in 19.6 Question 7 of 12 0.0/ 4.0 Points `Of the different protein structures discussed in this lesson, which actually gives the short-range repeating patterns? A.Primary Structure B.Secondary Structure C.Tertiary Structure D.Quaternary Structure E.Pental Structure Answer Key: B Feedback: Protein structure is discussed in 19.6 Question 8 of 12 0.0/ 4.0 Points `Of the different protein structures discussed in this lesson, which actually gives the arrangement of polypeptides? A.Primary Structure B.Secondary Structure C.Tertiary Structure D.Quaternary Structure E.Pental Structure Answer Key: D Feedback: Protein structure is discussed in 19.6 Question 9 of 12 4.0/ 4.0 Points `What joins the two strands of the twisted ladder of DNA together? A. ester linkages. B. peptide bonds. C. covalent bonds. D. hydrogen bonds. E. none of the above Answer Key: D Feedback: Good. DNA structure is discussed in 19.8 Question 10 of 12 4.0/ 4.0 Points `Which of these would NOT be categorized under under the category of "lipds"? A.phospholipids. B.steroids. C.glycolipids. D.carboxylic acids. E.All of the above are lipids. Answer Key: E Feedback: Good.Lipids are discussed in 19.4 Part 3 of 3 - 3.0/ 10.0 Points Question 11 of 12 0.0/ 5.0 Points *(1) How are the aldehyde functional group and the carboxylic acid functional group similar? How are they different? (2) How are ketone, ether, and ester functional groups similar? How are they different? Be sure you provide detailed answers according to the info form the course materials. Feedback: Organic chemistry is discussed in Ch. 18 Comment: No answer? Check out the think well 13.2.2 Question 12 of 12 3.0/ 5.0 Points *(1) Why is DNA classified as a polymer? What are the monomers? (2) What force holds together the strands of DNA? Why would covalent bonding be problematic? You must provide sufficient detail in your answer and incorporate information from the course materials to receive credit. DNA is comprised of a chain of nucleotides. The nucleotides are added together in a linear fashion forming a polymer Monomer are molecule that attach chemically to other molecules and forms polymer. Hydrogen bonds Feedback: Biochemistry is discussed in Ch. 19 Comment: A nice start, what is the monomer in this picture? Why would covalent bonding be problematic? Midterm Examination Part 1 of 4 - Short Answer 6.0/ 15.0 Points Please show as much work as possible for full credit. Question 1 of 13 3.0/ 5.0 Points `IN YOUR OWN WORDS, who was John Dalton, and why is he so important to chemistry? What did he "discover" that is so central to our study of chemistry? Explain why it is important. John Dalton was the first to atom. John Dalton is the person who invented atom for the first time. The bases of chemistry is the atom that is why John Dalton is considered the most important person in chemistry. Feedback: See section 1.4 Comment: I am not so sure he invented the atom? Question 2 of 13 3.0/ 5.0 Points `Human remains are typically cremated at a temperature of about 870.0 degrees C. (1) What is this temperature in F? (2) What is this temperature in K? All work must be shown, labeled, and explained in detail to receive credit. Note that where applicable, superscripts (X2) can be written as X^2 and subscripts (X2) can be written as X_2 if it saves you time. 1) 870 degrees Celsius =1598 degrees Fahrenheit 2) 870 degrees Celsius = 1143.15 kelvin Feedback: See section 3.10 Comment: Yes, you are correct, but need to show your work for these conversions Question 3 of 13 0.0/ 5.0 Points `The general public's definition of "theory" does not match the scientific definition of "theory." For example, non-scientists often say, "But it's JUST a theory!" What is wrong with this line of thinking? What is implied by this statement, and how does it reflect an improper definition of the term? What word from the course material thus far may perhaps be a better choice for the general public to use here instead of the word "theory"? Feedback: See section 1.4 Comment: No solution...at least write down your known's and unknows, with units to get some points...and you never know, something might jump out Part 2 of 4 - 9.0/ 10.0 Points Question 4 of 13 4.0/ 5.0 Points `Chemistry really is another language sometimes. It abbreviates a lot, and chemical formulas are a way to write a little and still convey a lot of information. For example, consider the chemicals hydrogen, cadmium (III) acetate, Lead (II) Iodide, and tetranitrogen nonasulfide. Translate these names into chemical formulas using the appropriate procedure described in the course text and my lecture material. Answer the following: (1) What is the correct formula of each of these compounds? (2) Explain how exactly (i.e. the procedure used) you arrived at your answer...in other words, walk me through your thinking. You will not receive credit if you don't show your work in detail. The chemical symbol for hydrogen is H2. cadmium (III) acetate Cd(CH 3 CO 2)2 Lead (II) Iodide Pb(I)2 tetranitrogen nonasulfide N4s4 Feedback: chapter 5 discusses naming Comment: Almost all correct, just that in Cadmium III you would have 3 acetates... Question 5 of 13 5.0/ 5.0 Points `Describe, in detail, the "anatomy" of an atom. Include a discussion of all subatomic particles, any associated charges, their locations, how they interact with one another, and explain which of these particles actually identify the atom on the periodic table. Also include a discussion on which of these may change in number in the case of isotopes. Matter is anything that has mass and occupy space. The smallest particle of matter is referred to as the atom. An atom is the basic substance of the matter. An atom consist of; tiny subatomic substance. These substances are; proton, electron, and neutron. The protons are positively charged, electrons are negatively charged, and neutrons have no charge. The atom is divided into two parts, the center which consists of the neutrons and proton and the outer part which consist of the electrons. An atom has different properties; a physical property can be seen and observed without changing its composition chemically. A chemical property of the matter describes how the substance reacts. An atom forms an ion by either losing or gaining an electron in the outer most energy level. Model Short Answer: this comes from chapter 4 Feedback: this comes from chapter 4 Comment: Nice Part 3 of 4 - 5.0/ 30.0 Points Question 6 of 13 2.5/ 5.0 Points `Alkali metals are extremely reactive with water. Suppose I give you a 55.50 g chunk of cesium and you throw it into a lake. When it reacts with water to form cesium hydroxide and hydrogen gas, how much hydrogen in grams is theoretically produced? Write a balanced equation for the reaction and show all work clearly and in detail to receive credit. All numbers seen immediately following the elemental symbols are intended to be subscripts. 2Cs(s)+2H2O- 2CsOH(aq)+H2(g) From the balanced equation the mass of hydrogen gas produced is 55.5 grams Feedback: Use your limiting reactant to predict product formation. Comment: Perfectly balanced equation but then you need to convert each to moles, and use the conversion 1moleH2/2mole Cs and back you grams Question 7 of 13 2.5/ 5.0 Points `Consider the solubility rules and identify all of the spectator ions when the following chemicals react: A) lead (II) nitrate and ammonium chloride B) Barium bromide and potassium carbonate. You must show all work (equations) clearly and in detail to receive credit. A) 2NH4CI(aq) + Pb(NO3)2 (aq)> PbC12(s)+2NH4NO3(aq) From the equation above we can observe that ammonium ion and nitrate ions are spectator ions. B) BaBr2(aq) +K2CO4(aq)+BaCO4(s) From the equation potassium ion and barium ion are spectator ions. Feedback: This concerns net ionic reactions and the formations of precipitates. Comment: Here you needed to show your work... Question 8 of 13 0.0/ 5.0 Points Let's acidify some phosphorous. Figure out how many grams of SO2 you could theoretically produce if you start with 2.3 moles of P and 3.6 moles of H2SO4. Reaction: 2P + 5H2SO4 --> 2H3PO4 + 5SO2 + 2H2O. You must show all work clearly and in detail to receive credit. All numbers seen immediately following the elemental symbols are intended to be subscripts. Feedback: Theoretical yield found in Chapter 8 Comment: No solution...at least write down your known's and unknows, with units to get some points...and you never know, something might jump out Question 9 of 13 0.0/ 5.0 Points If I give you an unknown acid that has a molar mass of 90.03 g/mol, and I tell you that the percent composition is 26.68%C, 2.24% H, 71.08% O, what would be the molecular formula? You must show all work to receive credit. Comment: No solution...at least write down your known's and unknows, with units to get some points...and you never know, something might jump out Question 10 of 13 0.0/ 5.0 Points With the current push for alternative energy sources, hydrogen certainly offers one possibility. It can be obtained from other compounds such as water. Water can be decomposed into oxygen and hydrogen using an electric current. How much hydrogen in grams can be obtained from 2.1 kg of water? You must show all work clearly and in detail to receive credit. Question 11 of 13 0.0/ 5.0 Points Knowing the following masses determined from decomposition in the laboratory, calculate the empirical formulas for each compound: A) 0.871 g Zn, 0.213 g O; B) 2.41 g Fe, 2.77 g S. You must show all work to receive credit. Feedback: Please see Chapter 6 for empirical formulas Part 4 of 4 - 10.0/ 30.0 Points Question 12 of 13 0.0/ 15.0 Points Bornite (Cu3FeS3) is a copper ore used in the production of copper. When heated, the following (unbalanced) reaction occurs: Cu3FeS3 (s) + O2 (g) → Cu(s) + FeO (s) + SO2 (g). If 3.70 kg of bornite is reacted with excess O2 and the process has a 60.2% yield of copper, how much copper is produced (in kg)? Feedback: The problem requires many steps from chapters 6-8. Comment: No solution...at least write down your known's and unknows, with units to get some points...and you never know, something might jump out Question 13 of 13 10.0/ 15.0 Points A sample was decomposed in the laboratory and found to have 38.67g C, 16.22g H, and 45.11g N. a) Find the molecular formula of this compound if the Formula mass is 62.12 g/mole. b)Determine how many H atoms would be in a 3.50g sample of this compound. a) Element-------C---------H N No.of mol--3.222---16.22 3.222 Ratio = 1: 5: 1 Empirical formula: CH5N n: 62.12/ (12+5+14) = 2 Molecular formula = C2H10N2 b) Mass of H = fraction of H x mass of sample So, (10x1)/62.12 x 3.50g = 0.563g (3s.f.) Feedback: This problem uses many concepts learned in Lessons 1 - 3. Comment: Nicely done, but again, you need to show your conversions (ALL work) and then you needed to get the number of molecules Midterm Review (graded) Return to Assessment List Part 1 of 8 - 4.0/ 4.0 Points Question 1 of 22 2.0/ 2.0 Points Who discovered the atomic theory? A. Antoine Lavoisier B. John Dalton C. John Dalton and Antoine Lavoisier D. Albert Einstein E. none of the above Answer Key: B Feedback: Good! It was Dalton. Question 2 of 22 2.0/ 2.0 Points Who discovered the law of conservation of mass? A. Albert Einstein B. John Dalton and Antoine Lavoisier C. Antoine Lavoisier D. John Dalton E. none of the above Answer Key: C Feedback: Good. It was Lavoisier. Part 2 of 8 - 4.0/ 6.0 Points Question 3 of 22 2.0/ 2.0 Points A lead ball has a mass of 49.0 grams and a density of 11.3 g/cm3. What is the volume of the ball? A.0.0340 cm^3 B.554 cm^3 C.0.231 cm^3 D.4.34 cm^3 E.none of the above Answer Key: D Feedback: Good! This is simply an application of d = m/v. Question 4 of 22 0.0/ 2.0 Points What is the volume in mL of a cube of water with dimensions 11.0 cm × 11.0 cm × 11.0 cm ? A.1.33 × 103 B.1.3 × 103 C.1.33 × 10-3 D.1.331 × 10-3 E.none of the above Answer Key: A Feedback: This is discussed in section 2.8 in the text. Question 5 of 22 2.0/ 2.0 Points When the value 98.54 is rounded to two significant figures, the number should be reported as: A.98 B.98.5 C.99 D.100 E.none of the above Answer Key: C Feedback: Good. Rounding associated with sig figs is discussed in section 2.4 of the text. Part 3 of 8 - 4.0/ 6.0 Points Question 6 of 22 0.0/ 2.0 Points `Given the sequence of temps below, which one represents the Fahrenheit boiling, room temp, and freezing points of water, in that order? A.0-75-100 B.212-75-32 C.0-25-100 D.0-298-373 E.none of the above Answer Key: B Question 7 of 22 2.0/ 2.0 Points `How should someone classify grape juice? A.mixture-homogeneous B.pure substance-compound C.mixture-heterogeneous D.pure substance-element E.none of the above Answer Key: A Question 8 of 22 2.0/ 2.0 Points `Gallium metal will melt in your hand. Which of the following is a true statement about this process? It represents a . A. physical change B. chemical property C. chemical change D.distillation E.none of the above Answer Key: A Part 4 of 8 - 6.0/ 6.0 Points Question 9 of 22 2.0/ 2.0 Points `If a nickel atom formed an ion, what charge would it have? A.1+ B.1- C.2- D.2+ E.it cannot be determined based on the information given Answer Key: E Feedback: See section 4.7. Transition metals can have various charges, though they will all be positive. Question 10 of 22 2.0/ 2.0 Points `The elements located in groups 3B through 2B are known as A.halogens B.transition metals C.alkaline earth metals D.noble gases E.none of the above Answer Key: B Feedback: See section 4.6 Question 11 of 22 2.0/ 2.0 Points `Which of these can be found in the nucleus? A. protons and electrons. B. only protons C.electrons and neutrons D.protons, neutrons, and electrons. E.protons and neutrons. Answer Key: E Feedback: See section 4.3 Part 5 of 8 - 6.0/ 6.0 Points Question 12 of 22 2.0/ 2.0 Points `What would be the proper way to write the ion formula for acetate? A.C3H2O - B.C2H3O - C.C2H3O- D.C2H3O 2- E.none of the above Answer Key: B Feedback: use naming rules and polyatomic ion list Question 13 of 22 2.0/ 2.0 Points `When naming Na3PO4 , it cannot be trisodium phosphate. Why? A. this compound should be called trisodium monophosphate. B. you cannot use a prefix for the first element of an ionic compound. C. you cannot use a prefix for the first element in a molecular compound. D. the sodium has a negative 3 charge. E. none of the above Answer Key: B Feedback: use naming mechanism Question 14 of 22 2.0/ 2.0 Points `We discussed diatomic molecules in this lesson. Which of these would NOT be classified in that category? A. nitrogen B. fluorine C.hydrogen D.neon E.all of these are diatomic Answer Key: D Feedback: see section 5.4 Part 6 of 8 - 4.0/ 6.0 Points Question 15 of 22 2.0/ 2.0 Points `I recently went to the dentist for a procedure that required me to have laughing gas (nitrous oxide, or N2O). I specified that I wanted EXACTLY 1.000 x 1025 molecules of this gas delivered to me. If he was going to be my dentist, he had to prove to me he knew a little chemistry. How many grams would he have to deliver? A.1.100 × 103 B.44.01 C.730.9 D.16.61 Answer Key: C Feedback: Good. See section 6.3 Question 16 of 22 2.0/ 2.0 Points `When answering the question of what I would do for a Klondike bar, I said I would jump into the Nile river with a crocodile while wearing 5.50 x 1025 atoms of lead on my body. What would be the mass of this lead in kg? A.1.89 B.18.9 C.1.14 x 1025 D.1.60 x 1045 E.6.022 x 1023 Answer Key: B Question 17 of 22 0.0/ 2.0 Points `I have some aliens in my basement who have developed a chemical weapon in an attempt to escape. I was able to survive the first attack and capture a sample of the dangerous gas. I analyzed it to find that it had a molar mass of 648.52 grams, and its empirical formula is C5H11N2O2P. What is its molecular formula? A.C20H44N8O8P4 B.C5H11N2O2P C.C10H22N4O4P2 D.CH2.2N0.4O0.4P0.2 E.cannot be determined from the information given Answer Key: A Feedback: See section 6.9 Part 7 of 8 - 6.0/ 6.0 Points Question 18 of 22 2.0/ 2.0 Points `In the image below, which reaction type is represented in equation 2? A.single displacement B.double-displacement C.decomposition D.synthesis/combination E.none of the above Answer Key: C Feedback: Good. See section 7.10 Question 19 of 22 2.0/ 2.0 Points `If I ask you to write an equation representing a chemica reaction, you must first know A. the molar mass of all the reactants and products. B. the amount of moles of all compounds involved C. the atomic mass of each atom involved. D. the symbols and formulas of all reactants and products. E. none of the above. Answer Key: D Question 20 of 22 2.0/ 2.0 Points `Oxidation-reduction reactions are also known as redox reactions. We learned about their unique characteristics in this lesson. Which of the following would be a FALSE statement given what we learned about redox reactions? A. if an atom gains 1 or more electrons, it is "reduced" B. when a redox reaction occurs, either reduction happens or oxidation happens, but never both in the same reaction C. Redox reactions often involve elemental oxygen D. If an atom loses 1 or more electrons, it is "oxidized" E. All of the above statement are true. Answer Key: B Feedback: Good. See section 7.9 Part 8 of 8 - 4.0/ 4.0 Points Question 21 of 22 2.0/ 2.0 Points `You have to be careful about pouring drano down your pipes since it is mainly hydrochloric acid--you can't do it if they are made of aluminum because it will dissolve them! You can't acid clean your aluminum auto parts for the same reasons: 2 Al + 6 HCl → 2 AlCl3 + 3H2. If you were able to dissolve 10.0 mol of Al, how many many moles of hydrogen gas could you make? NOTE: All numbers located immediately after elemental symbols should be considered subscripts. A.3.00 moles B.6.00 moles C.1.50 moles D.15.0 moles E.none of the above Answer Key: D Feedback: Good. See section 8.6 Question 22 of 22 2.0/ 2.0 Points `Suppose you were tasked with producing some nitrogen monoxide (a.k.a. nitric oxide). I'm sure this is often requested of you. You can do it by combusting ammonia (be careful!). The equation would be as follows: 4NH3 + 5O 2→ 4NO + 6H2O. If you form 3.50 mol of water, how much NO forms? A.2.33 mol. B.4.00 mol. C.4.50 mol. D.6.75 mol. E.none of the above Final Exam Review Assessment Return to Assessment List Part 1 of 8 - 6.0/ 6.0 Points Question 1 of 23 2.0/ 2.0 Points `Having learned about electromagnetic radiation in this lesson, which of these statements about it is true? A. when wavelength increases, energy decreases B. when wavelength increases, frequency increases C. Red light wavelength is shorter than green light. D. when energy increases, frequency decreases E. none of the above Answer Key: A Feedback: Good. See section 9.3 Question 2 of 23 2.0/ 2.0 Points `In terms of wavelength, which of these is the longest? A. Infrared Radiation B. Radio Waves C. Gamma Rays D.Microwaves E.X-rays Answer Key: B Feedback: Good. See section 9.3 Question 3 of 23 2.0/ 2.0 Points `Which of the following statements is true about atomic size? A. increases down a group and from right to left across a period. B. increases up a group and diagonally across the Periodic Table. C.increases down a group and from left to right across a period. D.increases up a group and from right to left across a period. E.increases up a group and from left to right across a period. Answer Key: A Part 2 of 8 - 6.0/ 6.0 Points Question 4 of 23 2.0/ 2.0 Points `Geometrically linear means that the electron groups have what angle? A.90° B.120° C.109.5° D.180° E.not enough information Answer Key: D Feedback: Good. See section 10.7 Question 5 of 23 2.0/ 2.0 Points `Geometrically trigonal planar means that the electron groups have what angle? A.120° B.90° C.180° D.109.5° E.not enough information Answer Key: A Feedback: Good. See section 10.7 Question 6 of 23 2.0/ 2.0 Points `Some atoms are better at attracting electrons compared to others. Which term below best describes that? A. polar covalent B. nonpolar covalent C.electronegativity D.dipole moment E.coulombic attraction Answer Key: C Feedback: Good. See section 10.8 Part 3 of 8 - 4.0/ 6.0 Points Question 7 of 23 2.0/ 2.0 Points `You have been given a 0.325 L canister containing a gas. The pressure gauge on the canister reads 721 mmHg, and the temperature gauge reads 305.15 K. The piston on the canister was pushed to compress the gas to 0.286 L, thereby increasing the pressure to 901 mmHg. What is the new temperature in Celsius? Remember sig figs. A.62.4°C B.215°C C.35.2°C D.335°C Answer Key: A Feedback: Good. This is the combined gas law, section 11.6 Question 8 of 23 2.0/ 2.0 Points `I have a pressure cooker in my underground lair that is brewing a diabolical solution. I set everything up and went upstairs, but forgot to write down the initial temperature. I know the starting volume was 1.00 L. When I came downstairs later to check on it, I see that the volume increased to 1.10 L, and thermometer read that the temperature was now 528.15 K. What was the starting temperature when I left (in °C)? A.-41°C B.207°C C.232°C D.480°C Answer Key: B Feedback: Good. Charles' law is in section 11.5 Question 9 of 23 0.0/ 2.0 Points `Think back to Lesson one when we talked about density. Now think about it--my kids love balloons, and then are always laying around the house. Suppose one was laying by the window at night when they went to bed, but the next day, when the sun came up, it warmed the gas (air) that was in the balloon. What would be true about the density of the air in the balloon? A. It will increase. B. It will remain the same. C. It will decrease. D. it will decrease for a while, then increase E. none of the above Answer Key: C Feedback: See KMT in section 11.2 Part 4 of 8 - 6.0/ 6.0 Points Question 10 of 23 2.0/ 2.0 Points `A liquid generally wants to decrease the area of its surface as much as possible. The natural tendency to do this is known as what? A.viscosity. B.vaporization. C.capillary action. D.surface tension. E.none of the above Answer Key: D Feedback: Good. This action is discussed in 12.3 Question 11 of 23 2.0/ 2.0 Points `When you put water into an ice cube tray and stick it in the freezer to make ice, which of these is true? A. it is an exothermic process. B. the process is referred to scientifically as sublimation. C. it is an endothermic process. D. the heat of vaporization must be removed. E. none of the above Answer Key: A Feedback: Good. Freezing is discussed in 12.5 Question 12 of 23 2.0/ 2.0 Points `Most people don't realize that once something starts to melt, cranking up the heat does't make the temperature of the substance higher, at least not until it is ALL melted. When you add lots of extra heat to a solid that is in the process of melting, what ends up happening to all of this extra energy you are adding? It is used to do what? A. expand the solid. B. change solid to liquid. C. change the liquid back to solid. D. overcome the intermolecular forces that hold the solid together. E. raise the temperature of the solid above its melting point. Answer Key: B Feedback: Good. Melting is discussed in 12.5 Part 5 of 8 - 6.0/ 6.0 Points Question 13 of 23 2.0/ 2.0 Points 'Which of these statements is true regarding a gas's ability to dissolve in water? It... A.is independent of temperature. B.decreases with increasing temperature. C.increases with increasing temperature. D.gases are not soluble in water. E.none of the above Answer Key: B Feedback: Good. Gas solutions are discussed in 13.4 Question 14 of 23 2.0/ 2.0 Points 'Suppose you have a 0.10 M solution of AlBr3. What is the concentration of each ion? A.0.10 M Al3+ ions and 0.30 M Br- ions B.0.30 M Al3+ ions and 0.10 M Br- ions C.0.10 M Al3+ ions and 0.033 M Br- ions D.0.033 M Al3+ ions and 0.033 M Br- ions Answer Key: A Feedback: Good. See 13.6 Question 15 of 23 2.0/ 2.0 Points `Suppose you want to prepare a 2.50 M solution of sodium chloride. If you only have 0.325 moles of sodium chloride, and you must use it all, how many mL must you prepare? A.0.130 mL B.0.813 mL C.130. mL D.7.69 mL Answer Key: C Feedback: Good. Solution concentration is in 13.6 Part 6 of 8 - 6.0/ 6.0 Points Question 16 of 23 2.0/ 2.0 Points `Suppose you have a sample of HC2H3O2 with a concentration of 2.0 M. So, what would be the [H+]? A.2.0 M B.>2.0 M C.< 2.0 M D.1.0 M Answer Key: C Feedback: Good. Weak acids discussed in 14.7 Question 17 of 23 2.0/ 2.0 Points `We discussed many properties and characteristics of acids in this lesson. Which of the following is NOT one that was mentioned? A. Acids have a slippery feel. B. Acids have a sour taste. C. Acids dissolve many metals. D. Acids turn litmus paper red. E. All of the above are properties of acids. Answer Key: A Feedback: Good. Acid properties are discussed in 14.2 Question 18 of 23 2.0/ 2.0 Points `In this lesson we learned about Kw, which is known as the the ion product constant for water. What is this value? A.0.0 B.1.0 x 1014 C.1.0 x 10-7 D.1.0 x 10-14 E.1.0 x 107 Answer Key: D Feedback: Good. Water is discussed in 14.8 Part 7 of 8 - 6.0/ 6.0 Points Question 19 of 23 2.0/ 2.0 Points `We discussed several different types of hydrocarbons in this lesson. Which one is saturated? A.alkynes B.alkenes C.alkanes D.all of these E.none of the above Answer Key: C Feedback: Good. Saturation is discussed in 18.5 Question 20 of 23 2.0/ 2.0 Points `We discussed different types of organic reactions in this lesson, one of which was addition. Which if these will undergo this type of reaction? A.C2H6 B.C3H8 C.C2H4 D.all of the above E.none of the above Answer Key: C Feedback: Good. reactions are discussed in 18.9 Question 21 of 23 2.0/ 2.0 Points `Endings (suffixes) in the naming process can tell us a lot about a chemical. For example, a compound named "butanal" would be categorized as a(n): A.ether. B.amine. C.aldehyde. D.alcohol. E.none of the above Answer Key: C Feedback: Good. This chemical group is discussed in 18.4 Part 8 of 8 - 4.0/ 4.0 Points Question 22 of 23 2.0/ 2.0 Points `We discussed different structures of proteins (primary, secondary, etc.). When considering the secondary structure, what is the repeating pattern that is commonly found along this chain? A.β-pleated sheet. B.β-turn. C.α-helix. D.random coil. E.none of the above Answer Key: C Feedback: Good. Protein structure is discussed in 19.6 Question 23 of 23 2.0/ 2.0 Points `Of the different protein structures discussed in this lesson, which actually gives the short-range repeating patterns? A.Primary Structure B.Secondary Structure C.Tertiary Structure D.Quaternary Structure E.Pental Structure Answer Key: B Feedback: Good. Protein structure is discussed in 19.6 Final Exam Return to Assessment List Comment: Diane, what happened? There are no answers in here...:o( Part 1 of 5 - 0.0/ 10.0 Points Please show as much work as possible for full credit. Question 1 of 16 0.0/ 5.0 Points `On December 5, 1971, at the mere age of 35, the great composer Wolfgang Amadeus Mozart died after a three month long battle with illness. Rumor was that a rival musician had poisoned him, but it turned out that common consensus was that the antimony prescription that doctors had prescribed him was actually poisoning him. (a) What is the full and abbreviated electron configuration for this element? Explain how you arrived at this configuration. In other words, don't just give me the configuration, but walk me through and explain to me how exactly you arrived at your answer. (b) In this Lesson we talked about the relationship between frequency and wavelength. The relationship can actually be expressed as where f is the frequency, c is the speed of light (see below), and lambda (the symbol on the left of the equals sign that looks like an upside down y) is wavelength. The particle nature of light was first proposed by Einstein, who suggested that light could be described as a stream of particles called photons. A photon of a certain wavelength (lambda) has an energy (E) given by the equation: where E is the energy of the photon in J, h is Planck's constant (6.626 x 10-34 J*s), and c is the speed of light (3.00 x 108 m/s). If we determine the wavelength (lambda) of light emitted from a sample of antimony to be 206.8 nm, what is the energy (E) and frequency (f) that corresponds to this wavelength? You must show all work to receive credit. HINT: 1 nm = 1 x 10-9 m; be sure all units are able to cancel out as necessary HINT: Plug in the values you know. You can substitute values between these equations. Feedback: This is from chapter 9. Question 2 of 16 0.0/ 5.0 Points `Think about it--why is the line spectrum produced by excited barium atoms more complex than the line spectrum produced by excited sodium atoms? Be sure to base your answer on what we discussed in THIS class and use the terminology from the materials in THIS course. Your answer must be sufficiently detailed to receive credit. Feedback: Emission spectra are discussed in Chapter 9. Part 2 of 5 - 0.0/ 20.0 Points Question 3 of 16 0.0/ 5.0 Points `Oxygen is a nonpolar gas, but it will dissolve a little bit in water (which is a polar solvent. Which intermolecular force(s) is/are responsible for the interaction between the two compounds? Explain in detail to receive credit. Feedback: Intermolecular forces are discussed in Ch. 12 Question 4 of 16 0.0/ 5.0 Points `What is the temperature of a 926 L compressed gas tank that contains 64.1 mol of carbon monoxide at a pressure of 38.1 atm? You must show all work to receive credit. Feedback: Gas laws are covered in Ch. 11 Question 5 of 16 0.0/ 5.0 Points `Pentaerythritol tetranitrate, a.k.a., PETN, is one of the most powerful explosives known. It has a density of 1.77 g/cm3. Find (1) the volume of a 227 g (about 1/2 pound) quantity of the explosive before the explosion and (2) the volume of total gas produced after the explosion. Assume STP conditions: C(CH2ONO2)4 (s) → 2CO(g) + 4H2O(g) + 3CO2(g) + 2N2(g) All numbers immediately following elemental symbols are subscripts. You must show all work to receive credit. (HINT: You can use density to find the initial condition for volume of the solid. You can then use the mol of gaseous products to determine volume of final condition since you know molar volume at STP.) Feedback: Gas laws are in Ch. 11 Question 6 of 16 0.0/ 5.0 Points `Nitrogen monoxide can be formed according to the equation: N2 (g) + 2O2 (g) → 2NO2 (g) If 8.0 L of nitrogen is reacted at STP, exactly how many liters of oxygen at STP would be needed to allow complete reaction? All numbers following elemental symbols are subscripts. You must show all work to receive credit. Feedback: Gas Laws are found in Chapter 11 Part 3 of 5 - 0.0/ 20.0 Points Question 7 of 16 0.0/ 5.0 Points PART 1: How many milliliters of concentrated HCl (12.1 M) are needed to make the following amounts of acid? You must show all work in detail to receive credit. (a) 5.00 L of 0.100 M, (b) 1.00 L of 6.00 M, (c) 2.00 L of 3.00 M, (d) 100 mL of 0.100 M. PART 2: Explain, in detail, how you would go about making the solution in letter (a) above. Include all detail and terminology as discussed in the Lesson materials. Feedback: Solutions are discussed in Ch. 13 Question 8 of 16 0.0/ 5.0 Points **(PART 1) Calculate the boiling points of these solutions: 0.1 m Na2P 0.2 m NaBr 0.16 m C12H22O11 POTENTIALLY USEFUL INFORMATION: Kb for water = 0.512 C*kg solvent/mol solute ---You must show all work in detail to receive credit.--- (PART 2) Place the above solutions in order of boiling point from lowest to highest. You must show all work in detail to receive credit. Feedback: Colligative properties are discussed in Ch. 13 Question 9 of 16 0.0/ 5.0 Points *Calculate the molarity (M) for each of these solutions--you must show all work in detail to receive credit: (a) 31.45 g of NaCl in 1.50 L, (b) 14.41 g of MgS in 0.750 L, (c) 0.4567 g of CuSO4 in 825 mL, (d) 25.5 mg of NaCN in 5.00 mL Feedback: Concentrations are discussed in Ch. 13 Question 10 of 16 0.0/ 5.0 Points *Calculate the number of grams of calcium carbonate in the following solutions--you must show all work in detail to receive credit: (a) 25.0 mL of 0.997 M CaCO3, (b) 10.0 mL of 2.50 M CaCO3, (c) 525.0 mL of 0.501 M CaCO3, (d) 1.25 L of 3.42 M CaCO3 Feedback: Concentrations of solutions is discussed in Ch. 13 Part 4 of 5 - 0.0/ 20.0 Points Question 11 of 16 0.0/ 5.0 Points *(1) How are the aldehyde functional group and the carboxylic acid functional group similar? How are they different? (2) How are ketone, ether, and ester functional groups similar? How are they different? Be sure you provide detailed answers according to the info form the course materials. Feedback: Organic chemistry is discussed in Ch. 18 Question 12 of 16 0.0/ 5.0 Points *(1) Why is DNA classified as a polymer? What are the monomers? (2) What force holds together the strands of DNA? Why would covalent bonding be problematic? You must provide sufficient detail in your answer and incorporate information from the course materials to receive credit. Feedback: Biochemistry is discussed in Ch. 19 Question 13 of 16 0.0/ 5.0 Points *Discuss the historical origins of the terms "organic" and "inorganic" for classifying chemical compounds. What was the difference between the terms then versus now--what does "organic" mean now in terms of chemical compounds? Be sure to include the terminology and content from this Lesson, and include a discussion on vitalism in your response. Feedback: Organic chemistry is discussed in Ch. 18 Question 14 of 16 0.0/ 5.0 Points *Name the following compounds according to what you learned in this Lesson. You must spell all names correctly and explain how you arrived at your answers in order to receive credit: Feedback: Organic chemistry is discussed in Ch. 18 Part 5 of 5 - 0.0/ 30.0 Points Question 15 of 16 0.0/ 15.0 Points (1) Write and balance the full chemical equation for the reaction between lead (II) nitrate and manganese (IV) chloride. (2) How much 0.175 M lead (II) nitrate solution, in liters, is required to completely precipitate all the chloride ions (in other words, react completely with) in 0.075 L of 0.125 M manganese (IV) chloride solution? All work must be shown, labeled, and explained in detail to receive credit. Note that superscripts (X2) can be written as X^2 and subscripts (X2) can be written as X_2 if it saves you time. Feedback: This is a cumulative problem that incorporates chemical naming, chemical equations, reaction types and product formation, solution concentrations, as well as stoichiometry. Question 16 of 16 0.0/ 15.0 Points `Vinegar, which is just a dilute acetic acid solution, is very common and versatile. The concentration of store-bought vinegar around a 5.0 % solution by mass, and its density is approximately 1.01 g/mL. (a) Suppose I dilute this vinegar into a bottle to 3 parts water + 1 part vinegar (in other words, I make a solution that is 25% as strong as it was) . Determine the molarity of this new vinegar solution. (b) If I use 2 cups (473.2 mL) of this new vinegar solution from part (a) to help create a cleaning solution for my windows, how many molecules of acetic acid is this? (c) How many atoms of carbon are in 2 cups of this new vinegar you made in part (a)? All work must be shown, labeled, and explained in detail to receive credit. Note that superscripts (X2) can be written as X^2 and subscripts (X2) can be written as X_2 if it saves you time. Be careful to account for significant figures in your final answers. Feedback: This is a cumulative problem involving concentration of solutions, percent composition, percent mass, conversions, and chemical nomenclature. [Show More]

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