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CHEMISTRY 104 Rogue Community College HOMEWORK SHEETS to be used with General, Organic and Biochemistry, 2nd edition, by Janice Gorzynski Smith Classification of Matter (CH. 1) ….………………………………………………..... 3 Significant Figures (CH. 1) ……..….…………………..……………………………... 5 Unit Conversions (CH. 1) …………………..…..…..………………………………... 7 Temperature Scales (CH. 1) ……………………….………………………………….. 9 Atoms and Formulas (CH. 2) ………………….……...………………………………. 11 Atomic Structure (CH. 2) ………..…………………...………………………………. 13 Periodic Table (CH. 2) …………………………………….………………………….. 15 Chemical Bonding (CH. 3&4) ………...………………………..………...…………... 17 Naming and Formula Writing (CH. 3&4) ……………………………..……………... 19 Molecular Geometry (CH. 4) …………………………………….………..…………… 21 Balancing Equations (CH. 5) ………………..……………..………………………….. 23 Moles (CH. 5) ………………………………………………………………….……… 25 Stoichiometry (CH. 5) …….…………………………………………………………... 27 Energy (CH. 6) ………………….………………………………………...…………… 29 Reaction Rate (CH. 6) ………………………………………………………..……….. 31 Gas Laws (CH. 7) …………………………………………………………………….. 33 Intermolecular Forces (CH. 7) ……………………………………………...…….….. 35 Solutions (CH. 8) ….………………………………………………………………..... 37 Acids and Bases (CH. 9) ….…………………………………………………….…..... 39 Neutralization and Buffers (CH. 9) ….……………………...…………………..…..... 41 1 2 Chemistry 104 – Rogue Community College Classification of Matter Homework Name ___________________________ Distinguish between each of the following pairs of terms. Do not use examples! 1. mass and weight 2. element and compound 3. substance and mixture 4. physical change and chemical change 5. liquid and gas 3 6. Classify each of the following as an element, a compound or a mixture: water _______________ cheese _______________ mercury _______________ air _______________ sugar _______________ salt _______________ oxygen _______________ aluminum _______________ helium _______________ brass _______________ vinegar _______________ coffee _______________ steel _______________ iron _______________ steam _______________ ice _______________ ice cream _______________ seawater _______________ methane _______________ copper _______________ granite _______________ blood _______________ arsenic _______________ krypton _______________ 4 Chemistry 104, Rogue Community College Significant Figures Homework Name ___________________________ Part One. Record each of the following three measurements to the appropriate number of significant figures. Include the appropriate units. Centimeter Ruler: 1 2 3 5 4 6 5.5 5.0 3.96 4.00 5 Part Two. Rewrite the following measurements using scientific notation. Do not change the units. 1. 0.00573 g --------> 2. 0.45400 kg --------> 3. 12055 years --------> 4. 93,000,000 miles --------> Part Three. Write down the number of significant figures in each of the following measurements. 1. 0.00503 g --------> 2. 500 miles --------> 3. 1.75 yards --------> 4. 0.75 yards --------> 5. 1.00 x 10-10 m --------> 6. 93,000,000 miles --------> 7. 6.022 x 1023 atoms --------> Part Four. Perform each of the following calculations. Record each answer to the correct number of significant figures and in the correct units. 3.75 g = 2.24mL _______________ 2.75cm x 2.74cm = _______________ 2.05 g = _______________ 0.2900 g 11.29 g 1.4 g = _______________ 12.3 g = 5 11.29 g 1.4cg = _______________ _______________ 6 Chemistry 104, Rogue Community College Unit Conversions Homework Name ___________________________ Set up and solve the problem in the space provided. Show all of your work! 1. Convert the measurement 92.0 g into pounds. (1 lb = 453.6 g) 2. Convert the measurement 92.0 cm into inches. (2.54 cm = 1 in) 3. Convert the measurement 2.15 mi into kilometers. (1 mi = 1.609 km) 4. Convert the measurement 0.001065 metric tons into grams. (1 metric ton = 1 x 106 g) 5. Convert the measurement 0.0039 L into cm3. (1 cm3 = 1 mL) 7 6. Convert the measurement 45.0 mg into grams. 7. Convert the measurement 45.0 g into milligrams. 8. Convert the measurement 1.25 L into milliliters. 9. Convert the measurement 15.0 cm into mm. 10. Convert the measurement 125 g into g. 11. Convert the measurement 0.0058 m into cm. 8 Chemistry 104, Rogue Community College Temperature Scales Homework Name ___________________________ There are three common temperature scales: Fahrenheit (F), Celsius (C) and kelvins (K). It is easiest to convert between kelvins and Celsius: TK = Tc + 273.15 or Tc = TK 273.15. It is also straightforward to convert between Celsius and Fahrenheit: TF = 1.8(Tc) + 32 or Tc = (TF 32)(5/9). To convert between kelvins and Fahrenheit, it is easiest to do it in two steps: first convert from kelvins to Celsius and then from Celsius to Fahrenheit, or first convert from Fahrenheit to Celsius and then from Celsius to kelvins. Practice using the above equations on the following temperature conversions: 1. Convert normal body temperature (98.6F) into Celsius. 2. Convert the freezing point of water (0C exactly) into kelvins. 3. Convert room temperature (25C) into Fahrenheit. 4. Convert absolute zero (0 K exactly) into Celsius. 9 5. Convert the temperature of liquid nitrogen (77 K) into Celsius and Fahrenheit. 6. Convert the temperature of dry ice (78.5C) into Fahrenheit and kelvins. 7. Convert the temperature of the surface of Venus encountered by Soviet spacecraft (about 465C) into Fahrenheit and kelvins. 8. Choose a temperature that is of interest to you for some reason. What makes this temperature interesting? Express this temperature in C, F and K. 10 Chemistry 104, Rogue Community College Atoms and Formulas Homework Name ___________________________ 1. 2. Classify each of the following elements as a metal, nonmetal or metalloid. (a) lithium (Li) ____________________________ (b) beryllium (Be) ____________________________ (c) boron (B) ____________________________ (d) carbon (C) ____________________________ (e) nitrogen (N) ____________________________ (f) oxygen (O) ____________________________ (g) fluorine (F) ____________________________ Fill in the blanks to accurately complete the following statements about the structure of the atom. (a) All atoms of the same element have the same number of ________________ in the ________________. (b) The subatomic particle with no electrical charge is called the ________________. (c) When an atom has no overall electrical charge, it has the same number of ________________ and ________________. (d) Atoms of the same element that have different weights are called ________________ of that element. 11 3. Distinguish between the terms atomic number and mass number. Do not use examples! 4. Write the chemical formula for a compound that contains: 5. (a) two atoms of hydrogen and one atom of oxygen (b) one atom each of carbon and oxygen (c) two atoms of hydrogen, one atom of carbon and three atoms of oxygen (d) two atoms of potassium, one atom of sulfur and four atoms of oxygen (e) three atoms of sodium, one atom of phosphorus and four atoms of oxygen How many of each kind of atom are present in each of the following formulas? (a) KOH K= (b) Cl = Mg3(PO4)2 Mg = (d) H= AlCl3 Al = (c) O= P= O= H= S= (NH4)2SO3 N= 12 O= Chemistry 104, Rogue Community College Atomic Structure Homework Name ___________________________ 1. How many protons, neutrons and electrons are there in each of the following species? (a) (d) 2. 12 6 C 238 92 U p+ (b) 14 6 C+ p+ (c) 1 1 H- p+ n0 n0 n0 e- e- e- p+ (e) 23 11 Na + p+ (f) 32 16 S2- p+ n0 n0 n0 e- e- e- Give one example of (a) an isotope of carbon-12, (b) an ion that is isoelectronic with neutral carbon-12, (c) an atom that has the same number of protons as carbon-12, (d) an atom that has the same number of neutrons as carbon-12, and (e) an atom that has the same number of nucleons as carbon-12. 13 3. Write the complete symbol ( ZA E chg ) for an atom that contains 15 protons, 17 neutrons and 15 electrons. (Write the correct atomic symbol in your answer, not E!!) 4. Write the complete symbol ( ZA E chg ) for an atom that contains 1 proton, no neutrons and no electrons. (Write the correct atomic symbol in your answer, not E!!) 5. Write the complete symbol ( ZA E chg ) for an atom that contains 82 protons, 125 neutrons and 80 electrons. (Write the correct atomic symbol in your answer, not E!!) 6. Write the electronic configuration for each element. 7. (a) lithium _______________________________________________ (b) carbon _______________________________________________ Name the element with each of the following electronic configurations. (a) [He] 2s2 ______________________________ (b) [Ne] 3s23p1 ______________________________ (c) [Ar] 4s1 ______________________________ 14 Chemistry 104, Rogue Community College Periodic Table Homework Name ___________________________ 1. Distinguish between a group and a period on the periodic table. 2. Give one example of each of the following: alkali metal = halogen = noble gas = metalloid = alkaline earth metal = transition metal = lanthanide = an element used by the thyroid gland to make thyroxine = an element whose forms include diamond, graphite and buckminsterfullerene = an element in the p-block of the periodic table that is not a halogen, noble gas or metalloid = 15 3. How many electrons can the first energy level (or shell) in an atom hold? 4. How many electrons can the fifth energy level in an atom hold? (hint: use 2n2) 5. How many valence electrons are there in a neutral oxygen atom? 6. How many valence electrons are there in a neutral sodium atom? 7. How many valence electrons are there in a neutral carbon atom? 8. How many valence electrons are there in a potassium ion, K+? 9. How many valence electrons are there in a calcium ion, Ca2+? 10. Which group of atoms has a stable octet of valence electrons? 11. Distinguish between an s-orbital and a p-orbital. 12. Comparing C and F, which atom has the larger radius? Which has the higher ionization energy? 13. Comparing N and P, which atom has the larger radius? Which has the higher ionization energy? 16 Chemistry 104, Rogue Community College Chemical Bonding Homework Name ___________________________ 1. 2. Draw the electron-dot symbol for each of the following atoms: arsenic, As iodine, I rubidium, Rb beryllium, Be gallium, Ga silicon, Si helium, He radon, Rn oxygen, O nitrogen, N Draw electron-dot symbols for the ions in each of the following binary ionic compounds: sodium chloride, NaCl magnesium oxide, MgO 17 3. Explain the octet rule in your own words. 4. Briefly explain why hydrogen does not follow the octet rule. 5. Distinguish between ionic and covalent bonds. 6. What is a polyatomic ion? What makes it different from a molecule? What makes it different from a monatomic ion? (Include an example of each in your answer.) 7. Draw a valid Lewis structure for each of the following molecules: oxygen, O2 iodine, I2 water, H2O methane, CH4 phosphorus trichloride, PCl3 oxygen dichloride, OCl2 18 Chemistry 104, Rogue Community College Naming and Formula Writing Homework Name ___________________________ Name each of the following compounds: H2CO3 ______________________________________________ NaHCO3 ______________________________________________ CO2 ______________________________________________ SCl2 ______________________________________________ Zn3(PO4)2 ______________________________________________ AgI ______________________________________________ TiF4 ______________________________________________ Cr(ClO3)3 ______________________________________________ Al2S3 ______________________________________________ H2O ______________________________________________ NBr3 ______________________________________________ Fe(OH)2 ______________________________________________ CBr4 ______________________________________________ H2SO4 ______________________________________________ 19 Write the correct formula for each of the following compounds: hydrochloric acid ______________________________ magnesium chloride ______________________________ aluminum phosphate ______________________________ ammonium hydroxide ______________________________ ammonium carbonate ______________________________ dinitrogen trioxide ______________________________ dinitrogen tetroxide ______________________________ dinitrogen pentoxide ______________________________ sulfur dioxide ______________________________ sulfuric acid ______________________________ potassium bicarbonate ______________________________ ammonium cyanide ______________________________ calcium hydrogen phosphate ______________________________ iron (III) cyanide ______________________________ silver oxide ______________________________ nitric acid ______________________________ 20 Chemistry 104, Rogue Community College Molecular Geometry Homework Name ___________________________ Molecular Formula Number of v.e. Lewis Structure H2O NH3 CH4 CH2F2 HCN CO2 21 Shape Polar or Nonpolar? Molecular Formula Number of v.e. Lewis Structure Cl2O BF3 H2CO (formaldehyde, C in the center) NF3 H2S C2H4 (ethylene, H2C=CH2) 22 Shape Polar or Nonpolar? Chemistry 104, Rogue Community College Balancing Equations Homework Name ___________________________ Balance each of the following equations by placing an integer coefficient on each of the blank lines: ___ KNO3 ----------> ___ NH4NO2 ----------> ___ O2 ___ KNO2 + ___ N2 ___ H2O + ___ MgO + ___ H2O ----------> ___ Mg(OH)2 ___ Fe2O3 + ___ CO ----------> ___ Fe + ___ CaO + ___ P2O5 ----------> ___ Ca3(PO4)2 ___ MgCl2 + ___ AgNO3 ----------> ___ Mg(NO3)2 ___ Cu ___ H2SO4 + ___ K2CO3 + ---------> ___ BaCl2 ___ CuSO4 ----------> + ___ KCl ___ Mg(OH)2 + ___ (NH4)3PO4 ----------> 23 ___ CO2 + ___ SO2 + + ___ AgCl ___ H2O ___ BaCO3 ___ Mg3(PO4)2 + ___ NH3 + ___ H2O Note: Be very careful about writing chemical formulas! If your formulas are wrong, you may come up with an equation that is impossible to balance!! methane + oxygen --------> carbon dioxide + water magnesium oxide + carbon dioxide --------> magnesium carbonate magnesium oxide --------> magnesium + oxygen water + carbon dioxide --------> carbonic acid water + diphosphorus pentoxide --------> phosphoric acid water + sodium oxide --------> sodium hydroxide 24 Chemistry 104 – Rogue Community College Mole Homework Name ______________________________ 1. Calculate the number of moles of O2 in 100.0 g of O2 gas. 2. Calculate the number of O2 molecules in 100.0 g of O2 gas. 3. Calculate the number of moles of Ti in 38.2 g of titanium metal. 4. Calculate the number of Ti atoms in 38.2 g of titanium metal. 25 5. Calculate the mass of 2.08 moles of CO2. 6. Calculate the mass of 0.064 moles of C6H12O6. 7. Calculate the mass of 1 hundred trillion water molecules. (By definition, 1 hundred trillion = 1 x 1014.) Do you think you could see a sample of water this small? 8. Proteins can have extremely high molecular weights, up into the thousands and millions of grams/mole. Calculate the mass of 1 hundred trillion protein molecules if the protein has a molecular weight of 10,000,000 g/mol. Do you think you could see a sample of protein this small? 26 Chemistry 104, Rogue Community College Stoichiometry Homework Name ___________________________ 1. Balance the following chemical equation, and use it to answer the following questions: _____ Al (s) + _____ O2 (g) -----> _____ Al2O3 (s) (a) What mass of oxygen will react with 2.75 g of aluminum? (b) What mass of aluminum oxide will be formed when 2.75 g of aluminum reacts completely with oxygen? (c) Show how your results are consistent with the Law of Conservation of Mass. 27 2. Hydrogen gas reacts with oxygen gas to form liquid water. How many grams of O2 are required in order to produce 10.0 g of H2O? 3. Sodium metal reacts with chlorine gas to form sodium chloride. How many grams of sodium chloride can be produced from 10.0 g of Cl2? 4. Methane reacts with oxygen to form carbon dioxide and water. How many grams of oxygen are required in order to react completely with 10.0 g methane? 28 Chemistry 104, Rogue Community College Energy Homework Name ___________________________ 1. 2. Use Table 6.2 on p. 171 to help you answer these questions. (a) Which bond is stronger, H-H or F-F? (b) Which bond is stronger, H-H or H-F? (a) Bond __________________ is always endothermic. (making or breaking) (b) Bond __________________ is always exothermic. (making or breaking) 3. In the reaction H2 + F2 2HF, one H-H bond is broken, one F-F bond is broken and two H-F bonds are formed. Is the reaction exothermic or endothermic? Explain your reasoning. (Use the bond dissociation energies in Table 6.2 to help you answer this question.) 4. (a) Slow reactions have __________________ activation energies. (high or low) (b) Fast reactions have __________________ activation energies. (high or low) 5. Catalysts speed up chemical reactions by ________________ the activation energy. 6. When the forward and reverse rates of a chemical reaction are equal, we say that the reaction is at _________________________. 29 7. Distinguish between the terms endothermic reaction and exothermic reaction. 8. Distinguish between the terms potential energy and kinetic energy. 9. Distinguish between the terms calorie and Joule. 10. According to Le Chatelier’s Principle, adding reactants (or removing products) drives the equilibrium to the __________, adding products (or removing reactants) drives the equilibrium to the __________, increasing temperature favors the ___________________ reaction, decreasing temperature favors the ____________________ reaction, increasing pressure shifts the reaction toward _______________ gas molecules, decreasing pressure shifts the reaction toward ________________ gas molecules, and adding a catalyst has no effect on equilibrium position whatsoever. (Choices: left/right, endothermic/exothermic, more/fewer) 30 Chemistry 104, Rogue Community College Reaction Rate Homework Name ___________________________ 1. According to molecular collision theory, only collisions that have sufficient energy and proper orientation lead to a reaction. (a) In your own words, explain why sufficient energy is necessary for a reaction to occur. (b) In your own words, explain why proper orientation is necessary for a reaction to occur. 2. The transition state is the point of ________________ energy in a molecular collision. (maximum/minimum) 3. Sketch a labeled energy diagram for an endothermic reaction with H = 10 kcal/mol and and Ea = 30 kcal/mol. Be sure to label the axes (energy and reaction coordinate), the reactants, products, transition state, H and Ea. 31 4. For a given chemical reaction, state whether each of the following changes will result in a faster or a slower reaction (circle your answer). Then, explain each answer in terms of molecular collision theory (collision rates, collision energies and activation energy). (a) The concentrations of reactants is decreased. Faster Slower (b) The temperature is decreased. Faster Slower (c) A catalyst is added. Faster Slower (d) The volume of a gas-phase reaction is decreased. Faster Slower (e) Any solid reactants are crushed. Faster Slower 32 Chemistry 104 – Rogue Community College Gas Law Homework Name ___________________________ Ideal Gas Law: PV = nRT, where R = 0.08206 Latm/molK Boyle's Law: P1V1 = P2V2 (n, T constant); Charles' Law: V1/T1 = V2/T2 (n, P constant) Gay-Lussac’s Law: P1/T1 = P2/T2 (n, V constant) Avogadro’s Law: V1/n1 = V2/n2 (T, P constant) 1. What is the volume of 3.25 moles of ideal gas at 25.0C and 0.759 atm pressure? 2. What pressure is exerted by 0.25 moles of ideal gas at 50.0C and a volume of 1.75 L? 3. How many moles of ideal gas will occupy a volume of 20.0 L at 100.C and 0.275 atm? 33 4. At what temperature (in C) will 1.25 moles of ideal gas occupy a volume of 10.0 L with a pressure of 0.500 atm? 5. A fixed quantity of gas at 25.00C occupies 3.75 L. If the gas is heated at constant pressure to 50.00C, what will its new volume be? 6. A fixed quantity of gas at 2.75 atm occupies 3.75 L. If the gas is compressed at constant temperature to 1.75 L, what will its new pressure be? 7. A 1.25-mol sample of gas occupies 25.0 L at a certain temperature and pressure. What volume will a 2.25-mol sample occupy at the same temperature and pressure? 8. A fixed quantity of gas at 300.0 K exerts a pressure of 1.45 atm. If the gas is heated at constant volume to 350.0 K, what will its new pressure be? 34 Chemistry 104, Rogue Community College Intermolecular Forces Homework Name ___________________________ ______ ______ ______ ______ ______ ______ ______ ______ 1. Which of the following molecules exhibits hydrogen bonding? (A) CH4 2. Which of the following are intermolecular forces? (A) dipole-dipole interactions (B) London forces (C) hydrogen bonding (D) all of the above 3. Which of the following will tend to increase intermolecular forces? (A) increased molecular weight (B) increased polarity (C) increased hydrogen bonding (D) all of the above 4. Choose the substance with the highest boiling point: (A) H2O 5. Choose the substance with the highest boiling point: (A) F2 6. Which state of matter has both definite shape and definite volume? (A) solid 7. Which state of matter has neither definite shape nor definite volume? (A) solid 8. Which state of matter has definite shape but not definite volume? (A) solid (B) (B) (B) (B) (B) (B) PH3 Ne Cl2 liquid liquid liquid 35 (C) (C) (C) (C) (C) (C) H2S O2 Br2 gas gas gas (D) H2O (D) Ar (D) I2 (D) (D) (D) none none none 9. Can nonpolar molecules experience London dispersion forces? Why or why not? 10. Which types of intermolecular forces are present in HCN? Explain your reasoning. 11. (a) Which of the phase changes are endothermic? (b) Which of the phase changes are exothermic? 12. Higher vapor pressures are found in liquids with __________________ temperatures and ____________________ intermolecular forces. (higher/lower, stronger/weaker) 13. Distinguish between the terms viscosity and surface tension. 14. Distinguish between the bonding in ionic, molecular, network and metallic solids. 36 Chemistry 104 – Rogue Community College Solutions Homework Name ___________________________ 1. A solution is prepared by dissolving 10.0 g of (solid) naphthalene (C10H10) in 500.0 mL of (liquid) chloroform (CHCl3). The resulting solution is liquid. Identify the solute and the solvent. 2. Calculate the molarity of the solution from #1. 3. Calculate the weight/volume percent concentration of C10H10 in the solution from #1. 4. What volume of the solution from #1 contains 2.7 g of naphthalene? 5. How many grams of naphthalene are contained in 25.0 mL of the solution from #1? 37 Remember that for dilution calculations c1V1 = c2V2. 6. Calculate the final concentration obtained when 150.0 mL of a 0.757 M solution of CaCl2 is diluted to a final volume of 1.000 L. 7. What volume of 6.00 M HCl should be diluted to a final volume of 500.0 mL in order to obtain a 1.50 M solution of HCl? 8. Determine the number of “particles” contained in one mole of each solute, and then rank the solutions in order of increasing vapor pressure. 0.10 M sucrose (C12H22O11) 0.08 M NaCl 0.03 M MgCl2 9. Rank the solutions from #8 in order of increasing boiling point. 10. Rank the solutions from #8 in order of increasing freezing point. 11. Rank the solutions from #8 in order of increasing osmotic pressure. 38 Chemistry 104 – Rogue Community College Acids & Bases Homework Name___________________________________ 1. 2. 3. Write the formula for the conjugate base of each of the following acids: HC2H3O2 __________ H2O __________ HCO3− __________ H3PO4 __________ NH4+ __________ H3O+ __________ Write the formula for the conjugate acid of each of the following bases: NH3 __________ H2O __________ HCO3− __________ F− __________ PO43− __________ OH− __________ Give one example each of a strong acid, a strong base, a weak acid and a weak base. 39 4. How many grams of H2SO4 are present in 250.0 mL of 0.175 M solution? 5. What volume of 0.1073 M NaOH contains 0.0250 moles of NaOH? 6. What is the pH of 0.100 M HCl? 7. What is the pH of 0.100 M NaOH? 40 Chemistry 104 – Rogue Community College Neutralization and Buffer Homework Name___________________________________ Write the net ionic equation for each of the following neutralization reactions. 1. HCl reacts with NaOH in a neutralization reaction. 2. H2SO4 reacts with NaOH in a neutralization reaction. 3. HCl reacts with NaHCO3 in a neutralization reaction. 4. H2SO4 reacts with NaHCO3 in a neutralization reaction. 41 5. State whether each of the following salts is acidic, basic or neutral. sodium chloride ________________ sodium acetate _________________ ammonium chloride ______________ potassium nitrate _______________ sodium phosphate _______________ lithium fluoride ________________ For questions #6 and 7, use the equation [H3O+] = Ka[HA]/[A−] or pH = pKa – log[HA]/[A−]. 6. Find the pH of a buffer that contains 0.15 M acetic acid and 0.10 M sodium acetate. 7. Find the pH of a buffer that contains 0.20 M sodium carbonate and 0.10 M sodium bicarbonate. 8. What is the property of a buffer that makes it different from a non-buffer solution? 9. Why are buffers important in the environment and in the human body? 42