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All Textbook Solutions for Chemistry for Today: General, Organic, and Biochemistry
A heavy steel ball is suspended by a thin wire. The ball is hit from the side with a hammer but hardly moves. Describe what you think would happen if this identical experiment were carried out on the moon.Explain how the following are related to each other: matter, mass, and weight.Tell how you would try to prove to a doubter that air is matter.1.4EThe attractive force of gravity for objetcs near Earths surface increases as you move toward Earths center. Suppose you are transported from a deep mine to the top of a tall mountain. a. How would your mass be changed by the move? b. How would your weight be changed by the move?Earths rotation causes it to bulge at the equator. How would the weights of people of equal mass differ when one was determined at the equator and one at the North Pole? See Exercise 1.5.Classify each of the following as a physical or chemical change, and give at least one observation, fact, or reason to support your answer. a. A plum ripens. b. Water boils. c. A glass window breaks. d. Food is digested.Classify each of the following as a physical or chemical change, and give at least one observation, fact, or reason to support your answer. a. A stick is broken into two pieces. b. A candle burns. c. Rock salt is crushed by a hammer. d. Tree leaves change color in autumn.Classify each of the following properties as physical or chemical. Explain your reasoning in each case. a. Iron melts at 1535C. b. Alcohol is very flammable. c. The metals used in artificial hip-joint implants is not corroded by body fluids. d. A 1-in. cube of aluminum weighs less than a 1-in. cube of lead. e. An antacid tablet neutralizes stomach acid.Classify each of the following properties as physical or chemical. Explain your reasoning in each case. a. Mercury metal is a liquid at room temperature. b. Sodium metal reacts vigorously with water. c. Water freezes at 0C. d. Gold does not rust. e. Chlorophyll molecules are green in color.A sample of liquid alcohol is frozen to a solid, then allowed to melt back to a liquid. Have the alcohol molecules been changed by the process? Explain your answer.Succinic acid, a white solid that melts at 182C, is heated gently, and a gas is given off. After the gas evolution stops, a white solid remains that melts at a temperature different from 182C. a. Have the succinic acid molecules been changed by the process? Explain your answer. b. Is the white solid that remains after heating still succinic acid? Explain you answer. c. In terms of the number of atoms contained, how do you think the size of succinic acid compares with the size of the molecules of the white solid produced by this process? Explain your answer. d. Classify molecules of succinic acid by using the term homoatomic or heteroatomic. Explain your reasoning.A sample of solid elemental phosphorus that is deep red in color is burned. While the phosphorus is burning, a white smoke is produced that is actually a finely divided solid that is collected. a. Have the molecules of phosphorus been changed by the process of burning? Explain your answer. b. Is the collected white solid a different substance from the phosphorus? Explain you answer. c. In terms of the number of atoms contained, how do you think the size of the molecules of the white solid compares with the size of the molecules of phosphorus? Explain your answer. d. Classify molecules of the collected white solid using the term homotatomic or heteroatomic. Explain your reasoning.Oxygen gas and solid carbon are both made up of homoatomic molecules. The two react to form a single substance, carbon dioxide. Use the term homoatomic or heteroatomic to classify molecules of carbon dioxide. Explain your reasoning.Under appropriate conditions, hydrogen peroxide can be changed to water and oxygen gas. Use the term homoatomic or heteroatomic to classify molecules of hydrogen peroxide. Explain your reasoning.Water can be decomposed to hydrogen gas and oxygen gas by passing electricity through it. Use the term homoatomic or heteroatomic to classify molecules of water. Explain your reasoning.Methane gas, a component of natural gas, is burned in pure oxygen. The only products of the process are water and carbon dioxide. Use the term homoatomic or heteroatomic to classify molecules of methane. Explain your reasoning.Classify each pure substance represented below by a capital letter as an element or a compound. Indicate when such a classification cannot be made, and explain why. a. Substance A is composed of heteroatomic molecules. b. Substance D is composed of homoatomic molecules. c. Substance E is changed into substance G and J when it is heated.Classify each pure substance represented below by a capital letter as an element or a compound. Indicate when such a classification cannot be made, and explain why. a. Two elements when mixed combine to form only substance L. b. An element and a compound when mixed form substances M and Q. c. Substance X is not changed by heating.Consider the following experiments, and answer the questions pertaining to classification: a. A pure substance R is heated, cooled, put under pressure, and exposed to light but does not change into anything else. What can be said about classifying substance R as an element or a compound? Explain your reasoning. b. Upon heating, solid pure substance T gives off a gas and leaves another solid behind. What can be said about classifying substance T as an element or compound? Explain your reasoning c. What can be said about classifying the solid left in part b as an element or compound? Explain your reasoning.Early scientists incorrectly classified calcium oxide lime as an element for a number of years. Discuss one or more reasons why you think they might have done this.Classify each of the following as homogeneous or heterogeneous: a. a pure gold chain b. liquid eyedrops c. chunky peanut butter d. a slice of watermelon e. cooking oil f. Italian salad dressing g. window glassClassify each of the following as homogeneous or heterogeneous: a. muddy flood water b. gelatin dessert c. normal urine d. smog-filled air e. an apple f. mouthwash g. petroleum jellyClassify as pure substance or solution each of the materials of Exercise 1.22 that you classified as homogeneous.Classify as pure substance or solution each of the materials of Exercise 1.23 that you classified as homogeneous.1.26EIn the distant past, 1in. was defined as the length resulting from laying a specific number of grain kernels such as corn in a row. Discuss the disadvantages of such a system.1.28EWhich of the following quantities are expressed in metric units? a. The amount of aspirin in a tablet: 5grains b. The distance between two cities: 55km c. The internal displacement of an auto engine: 5L d. The time for a race: 4min, 5.2s e. The area of a field: 3.6acres f. The temperature on a hot day: 104FWhich of the following quantities are expressed in metric units? a. Normal body temperature: 37C b. The amount of soft drink in a bottle: 2L c. The height of a ceiling in a room: 8.0ft d. The amount of aspirin in a tablet: 81mg e. The volume of a cooking pot: 4qt f. The time for a short race to be won: 10.2s1.31E1.32EReferring only to Table 1.2, answer the following questions: a. A computer has 12megabytes of memory storage. How many bytes of storage is this? b. A 10-km race is 6.2mi long. How many meters long is it? c. A chemical balance can detect a mass as small as 0.1mg. What is this detection limit in grams? d. A micrometer is a device used to measure small lengths. If it lives up to its name, what is the smallest metric length that could be measured using a micrometer?Referring only to Table 1.2, answer the following questions: a. Devices are available that allow liquid volumes as small as one microliter (L) to be measured. How many microliters would be contained in 1.00liter? b. Electrical power is often measured in kilowatts. How many watts would equal 75kilowatts? c. Ultrasound is sound of such high frequency that it cannot be heard. The frequency is measured in hertz vibrations per second. How many hertz correspond to 15megahertz? d. A chlorine atom has a diameter of 200picometers. How many meters is this diameter?One inch is approximately equal to 2.54cm. Express this length in millimeters and meters.Cookbooks are going metric. In such books, 1 cup is equal to 240mL. Express 1 cup in terms of liters and cubic centimeters.Two cities in Germany are located 25km apart. What is the distance in miles?The shotput used by female track and field athletes has a mass of 4.0kg. What would be the weight of such a shotput in pounds?Referring to Table 1.3, answer the following questions: a. Which is longer, a centimeter or an inch? b. How many milliliters are in a quart? c. How many grams are in an ounce?1.40E1.41EUsing appropriate values from Table 1.3, answer the following questions: a. One kilogram of water has a volume of 1.0dm3. What is the mass of 1.0cm3 of water? b. One quart is 32floz. How many fluid ounces are contained in a 2.0-L bottle of soft drink? c. Approximately how many milligrams of aspirin are contained in a 5-grain tablet?1.43E1.44E1.45EWhich of the following numbers are written using scientific notation correctly? For those that are not, explain what is wrong. a.02.7103 b.4.1102 c.71.9106 d.103 e..0405102 f.0.119Which of the following numbers are written using scientific notation correctly? For those that are not, explain what is wrong. a.4.2103 b.6.84 c.202103 d.0.026102 e.102 f.74.5105Write each of the following numbers using scientific notation: a. 14 thousand b. 365 c. 0.00204 d. 461.8 e. 0.00100 d. 9.11 hundredWrite each of the following numbers using scientific notation: a.three hundred b.4003 c.0.682 d.91.86 e.six thousand f.4001.50EA sheet of paper is 0.0106cm, or 0.0042in., thick. Write both numbers using scientific notation.1.52E1.53EDo the following multiplications, and express each answer using scientific notation: a.(8.2103)(1.1102) b.(2.7102)(5.1104) c.(3.3104)(2.3102) d.(9.2104)(2.1104) e.(4.3106)(6.1105)1.55E1.56EExpress each of the following numbers using scientific notation, then carry out the multiplication. Express each answer using scientific notation. a.(538)(0.154) b.(600)(524) c.(22.8)(341) d.(23.6)(0.047)1.58E1.59E1.60E1.61EIndicate to what decimal position readings should be estimated and recorded nearest 0.1,0.01,etc. for measurements made with the following devices: a. A ruler with a smallest scale marking of 0.1cm b. A measuring telescope with a smallest scale marking of 0.1mm c. A protractor with a smallest scale marking of 1 d. A tire pressure gauge with a smallest scale marking of 1lb/in2.Indicate to what decimal position readings should be estimated and recorded nearest 0.1,0.01,etc. for measurements made with the following devices: a. A buret with a smallest scale marking of 0.1mL b. A graduated cylinder with a smallest scale marking of 1mL c. A thermometer with a smallest scale marking of 0.1C d. A barometer with a smallest scale marking of 1torrWrite the following measured quantities as you would record them using the correct number of significant figures based on the device used to make the measurements. a. Exactly 6mL of water measured with a graduated cylinder that has a smallest scale marking of 0.1mL b. A temperature that appears to be exactly 37 degrees using a thermometer with a smallest scale marking of 1C c. A time of exactly nine seconds measured with a stopwatch that has smallest scale marking of 0.1 second d. Fifteen and one-half degrees measured with a protractor that has 1- degree scale markings1.65E1.66E1.67EDetermine the number of significant figures in each of the following: a. 0.0400 b. 309 c. 4.006 d. 4.4103 e. 1.002 f. 255.021.69EDo the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements. a. (3.71)(1.4) b. (0.0851)(1.2262) c. (0.1432)(2.81)(0.7762) d. (3.3104)(3.09103) e. (760)(2.00)6.0210201.71EDo the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements. a. 0.208+4.9+1.11 b. 228+0.999+1.02 c. 8.5437.954 d. (3.2102)+(5.5101) HINT: Write in decimal form first, then add. e. 336.86309.11 f. 21.660.023871.73EDo the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements. In calculations involving both addition/subtraction and multiplication/division, it is usually better to do additions/subtractions first. a. (0.0267+0.0019)(4.626)28.7794 b. 212.621.8886.37 c. 27.9918.074.630.88 d. 18.872.4618.070.88 HINT: Do divisions first, then subtract. e. (8.462.09)(0.51+0.22)(3.74+0.07)(0.16+0.2) f. 12.0611.840.271Do the following calculations and use the correct number of significant figures in your answers. Assume all numbers are the results of measurements. In calculations involving both addition/subtraction and multiplication/division, it is usually better to do additions/subtractions first. a. 132.1532.1687.55 b. (0.0844+0.1021)(7.174)19.1101 c. (2.780.68)(0.42+0.4)(1.058+0.06)(0.22+0.2) d. 27.6521.714.970.36 e. 12.476.97203.4201.8 HINT: Do divisions first, then subtract. f. 19.3718.490.8221.76EDetermine a single factor derived from Table 1.3 that could be used as a multiplier to make each of the following conversions: a.3.4lb to kilograms b.3.0yd to meters c.1.5oz to grams d.40.cm to inches1.78E1.79E1.80E1.81EA metric cookbook calls for 250mL of milk. Your measuring cup is in English units. About how many cups of milk should you use? Note: You will need two factors, one from Table 1.3 and one from the fact that 1cup=8floz.1.83EYou have a 40-lb baggage limit for a transatlantic flight. When your baggage is put on the scale, you think you are within the limits because it reads 18.0. But then you realize that weight is in kilograms. Do a calculation to determine whether your baggage is overweight.You need 3.00lb of meat that sells for 3.41/lb i.e., 1lb=$3.41. Use this price to determine a factor to calculate the cost of the meat you need using the factor-unit method.During a glucose tolerance test, the serum glucose concentration of a patient was found to be 131mg/dL. Convert the concentration to grams per liter.1.87E1.88E1.89E1.90E1.91EImmunoglobulin antibodies occur in five forms. A sample of serum is analyzed with the following results. Calculate the percentage of total immunoglobulin represented by each type. Type:IgGIgAIgMIgDIgEAmount(mg):987.1213.399.714.40.1Calculate the density of the following materials for which the mass and volume of samples have been measured. Express the density of liquids in g/mL, the density of solids in g/cm3, and the density of gases in g/L. a. 250mL of liquid mercury metal (Hg) has a mass of 3400g. b. 500.mL of concentrated liquid sulfuric acid (H2SO4) has a mass of 925g. c. 5.00L of oxygen gas has a mass of 7.15g. d. A 200-cm3 block of magnesium metal (Mg) has a mass of 350g.Calculate the density of the following materials for which the mass and volume of samples have been measured. Express the density of liquids in g/mL, the density of solids in g/cm3, and the density of gases in g/L. a. A 50.0-mL sample of liquid acetone has a mass of 39.6g. b. A 1.00-cup(236-mL) sample of homogenized milk has a mass of 243g. c. 20.0L of dry carbon dioxide gas (CO2) has a mass of 39.54g. d. A 25.0-cm3 block of nickel metal (Ni) has a mass of 222.5g.Calculate the volume and density of a rectangular block of metal with edges of 5.50cm, 12.0cm, and 4.00cm. The block weighs 929.5g.Calculate the volume and density of a cube of lead metal (Pb) that has a mass of 718.3g and has edges that measure 3.98cm.The volume of an irregularly shaped solid can be determined by immersing the solid in a liquid and measuring the volume of liquid displaced. Find the volume and density of the following: a. An irregular piece of the mineral quartz is found to weigh 12.4g. It is then placed into a graduated cylinder that contains some water. The quartz does not float. The water in the cylinder was at a level of 25.2mL before the quartz was added and at 29.9mL afterward. b. The volume of a sample of lead shot is determined using a graduated cylinder, as in part a. The cylinder readings are 16.3mL before the shot is added and 21.7mL after. The sample of shot weighs 61.0g. c. A sample of coarse rock salt is found to have a mass of 11.7g. The volume of the sample is determined by the graduated-cylinder method described in part a, but kerosene is substituted for water because the salt will not dissolve in kerosene. The cylinder readings are 20.7mL before adding the salt and 26.1mL after.The density of ether is 0.736g/mL. What is the volume in mL of 280.g of ether?Calculate the mass in grams of 100.0mL of chloroform (d=1.49g/mL).Do the following metric system conversions by changing only the power of 10. For example, convert 2.5L to mL: 2.5L=2.5103mL a. Convert 4.5km to mm b. Convert 6.0106mg to g c. Convert 9.861015m to km d. Convert 1.91104kg to mg e. Convert 5.0ng to mgA single water molecule has a mass of 2.991023g. Each molecule contains two hydrogen atoms that together make up 11.2 of the mass of the water molecule. What is the mass in grams of a single hydrogen atom?1.102ECooking oil has a density of 0.812g/mL. What is the mass in grams of 1.00quart of cooking oil? Use Table 1.3 for any necessary factors.1.104EAt 4.0C, pure water has a density of 1.00g/mL. At 60.0C, the density is 0.98g/mL. Calculate the volume in mL of 1.00g of water at each temperature, and then calculate the percentage increase in volume that occurs as water is heated from 4.0C to 60.0C.The following pairs of substances represent heterogeneous mixtures. For each pair, describe the steps you would follow to separate the components and collect them. a. wood sawdust and sand b. sugar and sand c. iron filings and sand d. sand soaked with oilExplain why a bathroom mirror becomes foggy when someone takes a hot shower. Classify any changes that occur as physical or chemical.1.108ELiquid mercury metal freezes to a solid at a temperature of 38.9C. Suppose you want to measure a temperature that is at least as low as 45C. Can you use a mercury thermometer? If not, propose a way to make the measurement.1.110EShow how the factor-unit method can be used to prepare an oatmeal breakfast for 27 guests at a family reunion. The directions on the oatmeal box say that 1 cup of dry oatmeal makes 3 servings.1.112ERefer to Chemistry Around Us 1.2 and explain what is meant by the following statement: All matter contains chemicals.1.114EWhich of the following properties is considered a physical property? a.flammability b.boiling point c.reactivity d.osmolarityWhich of the following properties depicts a chemical process? a.Helium is combined with neon b.Iron forms rust c.Water causes soil erosion d.Ice meltsWhich of the following is a mixture? a.sodium chloride b.rice and beans c.magnesium sulfate d.water1.118E1.119EThe correct formula for converting Fahrenheit to Celsius is given by: C=59(F32). Convert 72F into temperature in Celsius. a.72C b.40C c.25C d.22C1.121E1.122E1.123EHow many millimeters are there in one centimeter? a.10,000 b.1000 c.100 d.10Convert 4.50102nm into pm. a.4.50102pm b.4.50102pm c.4.501011pm d.4.50105pm1.126EConvert 4.50102nm into m. a.4.50102m b.4.501011m c.4.50107m d.4.50108mThe quantity 6185meters can be rewritten as: a. 6.185103meters. b. 6185kilometers. c. 6185103meters. d. 185103meters.The number 1,000,000 is what power of 10? a. 106 b. 106 c. 16 d. 0.000001What exponent or power of ten would you use to express how many meters are in a kilometer? a. 105 b. 103 c. 104 d. 102Express 0.0562 in exponential notation. a. 0.0562103 b. 56103 c. 562104 d. 5.62102Write the correct answer correct number of significant figures for the following calculation: (27+93)5.1558. a. 618.697 b. 618.7 c. 619 d. 618.69701.133EThe percentage of oxygen by weight in Al2(SO4)3 atomic weights: Al=27, S=32, O=16 is approximately: a. 19. b. 21. c. 56. d. 92.1.135EThe density of gold (Au) is 19.3g/cm3 and that of iron (Fe) is 7.9g/cm3. A comparison of the volumes (V) of 50gram samples of each metal would show that: a. VAu=VFe b. VAuVFe c. VAuVFe d. There is no predictable relationship between volumes.Draw a formula for each of the following molecules using circular symbols of your choice to represent atoms: a. A diatomic molecule of an element b. A diatomic molecule of a compound c. A triatomic molecule of an element d. A molecule of a compound containing one atom of one element and four atoms of another element2.2EWrite formulas for the following molecules using elemental symbols from Table 2.1 and subscripts. Compare these formulas with those of Exercise 2.1. a. A diatomic moelcule of chlorine gas. b. A diatomic molecule of hydrogen fluoride one hydrogen atom and one fluorine atom c. A triatomic molecule of ozone a molecular form of the element oxygen d. A molecule of carbon tetrachloride oneatom of carbon and four atoms of chlorineWrite formulas for the following molecules using elemental symbols from Table 2.1 and subscripts. Compare these formulas with those of Exercise 2.2. a. A molecule of water two hydrogen atoms and one oxygen atom b. A molecule of hydrogen peroxide two hydrogen atoms and two oxygen atoms c. A molecule of sulfuric acid two hydrogen atoms, one sulfur atom, and four oxygen atoms d. A molecule of ethyl alcohol two carbon atoms, six hydrogen atoms, and one oxygen atomDetermine the number of each type of atom in molecules represented by the following formulas: a. ammonia (NH3) b. acetic acid (C2H4O2) c. boric acid (H3BO3) d. ethane (C2H6)Determine the number of each type of atom in molecules represented by the following formulas: a. sulfur dioxide (SO2) b. butane (C4H10) c. chlorous acid (HClO2) d. boron trifluoride (BF3)Tell what is wrong with each of the following molecular formulas and write a correct formula: a. H3PO3 phosphorous acid b. SICI4 silicon tetrachloride c. SOO sulfur dioxide d. 2HO hydrogen peroxide-two hydrogen atoms and two oxygen atomsTell what is wrong with each of the following formulas and write a correct formula: a. HSH hydrogen sulfide b. HCLO2 chlorous acid c. 2HN2 hydrazine-two hydrogen atoms and four nitrogen atoms d. C2H6 ethane2.9E2.10EDetermine the number of electrons that would have to be associated with each nucleus described in Exercise 2.9 to produce a neutral atom.Determine the number of electrons that would have to be associated with each nucleus described in Exercise 2.10 to produce a neutral atom.Determine the number of electrons and protons contained in an atom of the following elements: a. sulfur b. As c. element number 24Determine the number of electrons and protons contained in an atom of the following elements: a. silicon b. Sn c. element number 742.15E2.16EWrite symbols like those given in Exercises 2.15 and 2.16 for the following isotopes: a. cadmium -110 b. cobalt -60 c. uranium -235Write symbols like those given in Exercises 2.15 and 2.16 for the following isotopes: a. silicon -28 b. argon -40 c. strontium -882.19E2.20EWrite isotope symbols for neutral atoms with the following characteristics: a. Contains 20 electrons and 20 neutrons b. Contains 1 electron and 2 neutrons c. A magnesium atom that contains 14 neutronsWrite isotope symbols for neutral atoms with the following characteristics: a. Contain 17 electrons and 20 neutrons b. A copper atom with a mass number of 65 c. A zinc atom that contains 36 neutronsWrite the symbols and names for two elements whose average atoms have masses that are within 0.3u of each other. Dont look beyond element number 83.Round atomic weights to the nearest whole number, and determine how many helium atoms would balance one carbon atom on a seesaw.Round atomic weights to the nearest whole number, and determine how many lithium atoms would balance two nitrogen atoms on a seesaw.What are the symbol and name for an element whose average atoms have a mass that is 77.1 of the mass of an average chromium atom?In the first 36 elements, 6 elements have atoms whose average mass is within 0.2u of being twice the atomic number of the element. Write the symbols and names for these 6 elements.What are the symbol and name of the element whose average atoms have a mass very nearly half the mass of an average silicon atom?2.29E2.30EThe molecular weight was determined for a gas that is known to be an oxide of nitrogen. The value obtained experimentally was 43.98u. Which of the following is most likely to be the formula of the gas? NO, N2O, NO2.A flammable gas is known to contain only carbon and hydrogen. Its molecular weight is determined and found to be 28.05u. Which of the following is the likely identity of the gas? Acetylene (C2H2), ethylene (C2H4), ethane (C2H6).Glycine, an amino acid found in proteins, has a molecular weight of 75.07u and is represented by the formula C2HxNO2. What number does x stand for in the formula?Serine, an amino acid found in proteins, has a molecular weight of 105.10u and is represented by the formula CyH7NO3. What number does y stand for in the formula?Naturally occurring sodium has a single isotope. Determine the following for the naturally occurring atoms of sodium: a. The number of neutrons in the nucleus. b. The mass in u of the nucleus to three significant figures.Naturally occurring aluminum has a single isotope. Determine the following for the naturally occurring atoms of aluminum: a. The number of neutrons in the nucleus. b. The mass in u of the nucleus to three significant figures.Calculate the atomic weight of lithium on the basis of the following percent composition and atomic weights of the naturally occurring isotopes. Compare the calculated value with the atomic weight listed for lithium in the periodic table. lithium-6=7.42(6.0151u)lithium-7=92.58(7.0160u)Calculate the atomic weight of boron on the basis of the following percent composition and atomic weights of the naturally occurring isotopes. Compare the calculated value with the atomic weight listed for boron in the periodic table. boron-10=19.78(10.0129u)boron-11=80.22(11.0093u)Calculate the atomic weight of silicon on the basis of the following percent composition and atomic weights of the naturally occurring isotopes. Compare the calculated value with the atomic weight listed for silicon in the periodic table. silicon-28=92.21(27.9769u)silicon-29=4.70(28.9765u)silicon-30=3.09(29.9738u)Calculate the atomic weight of copper on the basis of the following percent composition and atomic weights of the naturally occurring isotopes. Compare the calculated value with the atomic weight listed for copper in the periodic table. copper-63=69.09(62.9298u)copper-65=30.91(64.9278u)Refer to the periodic table and determine how many grams of sulfur contain the same number of atoms as 3.10 grams of phosphorus.Refer to the periodic table and determine how many grams of fluorine contain the same number of atoms as 1.60 grams of oxygen.Write three relationships equalities based on the mole concept for each of the following elements: a.beryllium b.lead c.sodiumWrite three relationships equalities based on the mole concept for each of the following elements: a.phosphorus b.aluminum c.kryptonUse a factor derived from the relationships written in Exercise 2.43 and the factor-unit method to determine the following: a.The number of moles of beryllium in a 10.0g sample of beryllium b.The number lead atoms in a 2mol sample of lead c.The number of sodium atoms in a 50.0g sample of sodiumUse a factor derived from the relationships written in Exercise 2.44 and the factor-unit method to determine the following: a.The mass in grams of one phosphorus atom b.The number of grams of aluminum in 1.65mol of aluminum c.The total mass in grams of one-fourth Avogadros number of krypton atoms2.47ERefer to the periodic table and calculate the molecular weights for the compounds BF3 and H2S. Then, determine how many grams of BF3 contain the same number of molecules as 0.34g of H2S.2.49E2.50EAnswer the following questions based on the information contained in the statements you wrote for Exercise 2.49. a.How many moles of oxygen atoms are contained in 1 mol of CO2 molecules? b.How many grams of carbon are contained in 1.00 mol of C2H6? c.What is the mass percentage of oxygen in C6H12O6?Answer the following questions based on information contained in the statements you wrote for Exercise 2.50. a. How many moles of hydrogen atoms are contained in 0.50mol of ethyl ether? b. How many carbon atoms are contained in 0.25mol of C2H3O2F. c. How many grams of hydrogen are contained in 2.00mol of C6H7N?How many moles of N2O5 contain the same number of nitrogen atoms as 3.0mol of NO2.How many grams of C2H6O contain the same number of oxygen atoms as 0.75mol of H2O.2.55EDetermine the mass percentage of hydrogen in CH4 and C2H6.2.57E2.58EUrea (CH4N2O) and ammonium sulfate (N2H8SO4) are both used as agricultural fertilizers. Which one contains the higher mass percentage of nitrogen?2.60E2.61E2.62E2.63EThe mass of a single carbon 12 atom is 1.991023g. What is the mass in grams of a single carbon 14 atom?2.65E2.66Ea. Explain how atoms of different elements differ from one another. b. Explain how atoms of different isotopes of the same element differ from one another.The atomic weight of aluminum is 26.98u and the atomic weight of nickel is 58.69u. All aluminum atoms have a mass of 26.98u, but not a single atom of nickel has a mass of 58.69u. Explain.Answer the question in the caption of Figure 2.3 see page 57. Would you expect any orange in the bowl to have the exact mass you calculated as an average? Explain.Answer the question in the caption of Figure 2.5 see page 60. Use your answer and the fact that an average jelly bean has a mass of 1.18g to calculate the number of beans in each jar.2.71E2.72E2.73E2.74E2.75EWhich one of the following substances is a chemical compound? a.blood b.water c.oxygen d.airWhich of the following is true about compounds? a.Compounds are pure substances that are composed of two or more elements in a fixed proportion. b.Compounds can be broken down chemically to produce their constituent elements or other compounds. c.Both A and B are correct. d.Neither A nor B is correct.C1734l has a.17 protons, 17 electrons, and 17 neutrons. b.17 protons, 19 electrons, and 17 neutrons. c.17 protons, 18 electrons, and 17 neutrons. d.34 protons, 34 electrons, and 17 neutrons.If two atoms are isotopes, they will a.have same number of protons and neutrons. b.have the same number of neutrons, but different numbers of protons. c.have the same number of protons, but different numbers of neutrons. d.have same number of neutrons and electrons.Copper (Cu) has an atomic number of 29 and a mass number of 64. One copper atom, therefore, has how many protons? a.27 b.29 c.31 d.35Atoms are electrically neutral. This means that an atom will contain a.more protons than neutrons. b.more electrons than protons. c.an equal number of protons and electrons. d.None of the above.The negative charged particle found within the atom is the a. proton. b. electron. c. nucleus. d. neutron.2.83E2.84EThe mass of an atom is almost entirely contributed by its a. nucleus. b. protons. c. electrons and protons. d. neutrons.Which of the following is the chemical symbol for the species that has 16 protons, 17 neutrons, and 18 electrons? a. 1633S b. 1733Cl c. 1735Cl d. 1633S22.87EWhat is the mass number of an atom with 60 protons, 60 electrons, and 75 neutrons? a. 120 b. 135 c. 75 d. 195Which of the following represents Avogadros number? a. 1.661024 b. 1.01024 c. 6.0221023 d. 3.0111023Which of the following has the greatest number of atoms? a. 1.0molN b. 1.0gN c. 1.0molNO2 d. 0.5molNH3The formula of carbon dioxide is CO2. Its molecular weight is 44u. A sample of 11grams of CO2 contains a. 1.0mole of carbon dioxide. b. 1.5grams of carbon. c. 3.0grams of carbon. d. 6.0grams of oxygen.What is the molar mass of calcium oxide, CaO? a. 56 b. 28 c. 640 d. 320How many grams are contained in 0.200mol of calcium phosphate, Ca3(PO4)2? a. 6.20 b. 62.0 c. 124 d. 31.0How many moles are contained in a 54.0g sample of Al? a. 1.0 b. 2.0 c. 0.5 d. 4.0Identify the group and period to which each of the following elements belongs: a. Si b. element number 21 c. zinc d. element number 35Identify the group and period to which each of the following elements belongs: a. element number 27 b. Pb c. arsenic d. BaWrite the symbol and name for the elements located in the periodic table as follows: a. Belongs to group VIA (16) and period 3 b. The first element reading down in group VIB (6) c. The fourth element reading left to right in period 3 d. Belongs to group IB (11) and period 5Write the symbol and name for the elements located in the periodic table as follows: a. The noble gas belonging to period 4 b. The fourth element reading down in group IVA (14) c. Belongs to group VIB (6) and period 5 d. The sixth element reading left to right in period 6a. How many elements are located in group VIIB (7) of the periodic table? b. How many elements are found in period 5 of the periodic table? c. How many total elements are in groups IVA (14) and IVB (4) of the periodic table?a. How many elements are located in group VIIB (7) of the periodic table? b. How many total elements are found in periods 1 and 2 of the periodic table? c. How many elements are found in period 5 of the periodic table?The following statements either define or are closely related to the terms periodic law, period, and group. Match the terms to the appropriate statements. a. This is a vertical arrangement of elements in the periodic table. b. The chemical properties of the elements repeat in a regular way as the atomic numbers increase. c. The chemical properties of elements 11, 19, and 37 demonstrate this principle. d. Elements 4 and 12 belong to this arrangement.The following statements either define or are closely related to the terms periodic law, period, and group. Match the terms to the appropriate statements. a. This is a horizontal arrangement of elements in the periodic table. b. Element 11 begins this arrangement in the periodic table. c. The element nitrogen is the first member of this arrangement. d. Elements 9, 17, 35 and 53 belong to this arrangement.According to the Bohr theory, which of the following would have the higher energy? a. An electron in an orbit close to the nucleus b. An electron in an orbit located farther from the nucleusWhat particles in the nucleus cause the nucleus to have a positive charge?What is the maximum number of electrons that can be contained in each of the following? a. A 3d orbital b. A 3d subshell c. The third shellWhat is the maximum number of electrons that can be contained in each of the following? a. A 2p orbital b. A 2p subshell c. The second shellHow many orbitals are found in the fourth shell? Write designations for the orbitals?How many orbitals are found in the second shell? Write designations for the orbitals?3.15EHow many orbitals are found in a 4f subshell? What is the maximum number of electrons that can be located in this subshell?Identify the subshells found in the fourth shell; indicate the maximum number of electrons that can occupy each subshell and the total number of electrons that can occupy the shell.Look at the periodic table and tell how many electrons are in the valence shell of the following elements: a. element number 54 b. the first element reading down in group VA (15) c. Sn d. The fourth element reading left to right in period 3Look at the periodic table and tell how many electrons are in the valence shell of the following elements: a. element number 35 b. Zn c. strontium d. the second element in group VA (15)What period 6 element has chemical properties most like sodium? How many valence-shell electrons does this element have? How many valence-shell electrons does sodium have?3.21E3.22E3.23EWrite an electronic configuration for each of the following elements, using the form 1s22s22p6, and so on. Indicate how many electrons are unpaired in each case. a. element number 37 b. Si c. titanium d. Ar3.25EWrite electronic configuration and answer the following: a. How many total s electrons are found in magnesium? b. How many unpaired electrons are in nitrogen? c. How many subshells are completely filled in Al?Write electronic configuration and answer the following: a. How many total electrons in Ge have a number designation before the letters of 4? b. How many unpaired p electrons are found in sulfur? What is the number designation of these unpaired electrons? c. How many 3d electrons are found in tin?3.28E3.29E3.30E3.31E3.32E3.33EClassify each of the following elements into the s,p,d, or f area of the periodic table on the basis of the distinguishing electron: a. lead b. element 27 c. Tb d. RbClassify each of the following elements into the s,p,d, or f area of the periodic table on the basis of the distinguishing electron: a. Kr b. tin c. Pu d. element 403.36E3.37EClassify the following as metals, nonmetals, or metalloids: a.argon b.element 3 c.Ge d.boron e.Pm3.39E3.40E3.41EUse trends within the periodic table and indicate which member of each of the following pairs has the larger atomic radius: a.Ga or Se b.N or Sb c.O or C d.Te or S3.43EUse trends within the periodic table and indicate which member of each of the following pairs gives up one electron more easily: a.Li or K b.C or Sn c.Mg or S d.Li or N3.45EHow would you expect the chemical properties of isotopes of the same element to compare to each other? Explain your answer.3.47EWhat would be the mass in mg of 3.01020atoms that all have the same electronic configuration of 1s22s22p4.3.49EA 10.02-g sample of an element contains 0.250mol of the element. Classify the element into the correct category of the representative, transition, inner-transition, or noble gas. Will the element conduct electricity?3.51E3.52E3.53ECalcium metal reacts with cold water as follows: Ca+2H2OCa(OH)2+H2 Magnesium metal does not react with cold water. What behavior toward cold water would you predict for strontium and barium? Write equations to represent any predicted reactions.3.55E3.56EThe arrangement of the modern periodic table is based on atomic: a. mass b. number c. radius d. electronegativityThe horizontal rows of the periodic table are called: a. families b. group c. representative elements d. periods3.59EWhich two elements have chemical properties that are similar? a. H and He b. Fe and W c. Li and Be d. Mg and Ca3.61E3.62EWhat does the number 36 represent on the periodic table entry for krypton? a. atomic number b. relative atomic mass c. group number d. electron configuration3.64E3.65E3.66EFrom the periodic table, which of K and Br is larger? a. K is larger. b. Br is larger. c. They are the same size. d. We cannot know which one is larger.3.68E3.69EWhich of the following has the largest first ionization energy? a. Cs b. Rb c. Ba d. Sr