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Name ____________KEY______________________ Period ______________ Chemistry Final Exam STUDY/ Review Guide MATTER: Fill in the following chart for TYPICAL Solids, Liquids and Gases (not water) State of Particle Shape Density Rank Energy Rank Matter Arrangement Definite or 1 = highest 1 = highest Regular or Indefinite 3 = lowest 3 = lowest Irregular Compressibility Yes or No Gas irreg Indef 3 1 Y Liquid irreg Def 2 2 N Solid reg Def 1 3 N Atoms – draw a diagram of an atom of Lithium (mass number 7), labeling the following parts – nucleus, electron cloud, protons, neutrons, electrons Nucleus – center of atom Electron cloud – outside of nucleus Protons – in nucleus with (+) symbol Neutrons – in nucleus with no symbol Electrons – in energy levels outside of nucleus Label as: molecule, atom, compound, substance, homogeneous mixture, heterogeneous mixture Substance/Molecule - H2O Substance / atom - A single particle of pure potassium Heterogeneous mixture - A sample of sand scooped from a beach Substance / ionic compound - Sodium chloride Homogeneous mixture - Iced tea Atom - The smallest particle of an element that retains all of its chemical properties Heterogeneous mixture - Chicken soup PHYSICAL AND CHEMICAL CHANGES AND PROPERTIES Classify the following as a chemical or physical property or chemical or physical change ________ 1. PC - Liquid collects on the side of a cold drink glass ________ 2. CP - Hexane is flammable ________ 3. CC - Baking soda decomposes in the cake, releasing CO2 to make it fluffy. ________ 4. PP - Copper II sulfate is blue. ________ 5. PC - Ice is melting ________ 6. PP - Pure water has a density of 1 g/cm3 1 STATES OF MATTER: Mark the statements as true or false. If false, make changes to correct the statement. 1. Liquids have the greatest amount of kinetic energy among the phases of matter – FALSE, gases do. 2. In general, a solid is the densest phase of matter. - TRUE 3. Particles in a solid demonstrate rotation, vibration and translation. FALSE – no translation 4. The particles of liquids have low amounts of translation unless they are stirred. - TRUE 5. When a solid is melting, its temperature is still rising as it melts. – FALSE – holds steady 6. Both solids and liquids can flow. – FALSE – only liquids can flow 7. Translation is the type of kinetic energy in which a particle moves from place to place. - TRUE DENSITY CALCULATIONS Solve the following problems involving density calculations. Show all work. What is the formula for density? D= m/v A cube is 17 cm3 in volume with mass of 4.0 grams. Calculate its density. 0.24g/cm3 If a ball has a density of 27.5 g/cm3, determine its volume if its mass is 626 g. 22.8g METRIC UNITS Perform the following determinations. ________ 1. 1 kilometer (km) = _____1000____ meters (m) ________ 2. 1 milligram (mg)= _____.001___ grams (g) ________ 3. 1 liter (L) ________ 4. 2.3 kilograms (kg)= ____2300_______ grams (g) ________ 5. 12 meters (m) = ___________1200_______ centimeters (cm) = __1000____ milliliters (mL) ATOMIC STRUCTURE: Fill in the following table with the appropriate information Subatomic Charge Location Relative Mass Particle Nucleus or electron cloud Proton +1 Nucleus 1 amu Neutron O Nucleus 1 amu Electron -1 Electron cloud 1/1640th amu Order of Size 1= largest 3 = smallest 1 1 (same!) 3 2 PERIODIC TABLE: Answer the following questions What number of valence electrons indicates the most stable arrangement? Which group on the periodic table fits this description without forming ions? 8 valence e-; noble gases Elements on the periodic table are organized in order of increasing ____atomic number________.? Elements are identified by the number of ___protons_____ in their nucleus. The number of ___electrons_______ and ____neutrons_______ may vary. ORGANIZATION OF THE PERIODIC TABLE Label the following on the diagram below. Then, label the number of valence electrons inside the space for each group. s-block metals Aluminum group Halogens p-block non-metals Carbon group Noble Gases d-block alkali metals Nitrogen group transition metals f-block alkali earth metals Oxygen Group inner transition metals Non-metals Metalloids Border stairstep s - block Metals p - block d – block Transition Metals f – block Inner Transition Metals 3 ELECTRON CONFIGURATION: Write the full electron configuration for the following elements. Circle the valence electrons. Strontium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 Helium 1s2 Oxygen Barium 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 1s2 2s2 2p4 5p6 6s2 Neon 1s2 2s2 2p6 Fluorine 1s2 2s2 2p5 BONDING Draw the covalent structure for the following chemical formulas. Name the shape of the molecule. a) PBr3 c) SO3 b) SO2 d) PO43- Indicate the correct word(s) to complete each sentence. ________ 1. Ionic bonds are formed between metals and non-metals ________ 2. Covalent bonds are formed between non-metals and other non-metals. ________ 3. Metals do not form bonds with other metals ________ 4. The transition metals lose electrons to form ions. ________ 5. When comparing degree of polarity between two bonds, the bond with the greatest polarity has the largest difference between the two atoms in the bond. ELECTRON DOT STRUCTURES Draw the electron dot structure of the valence electrons for the following elements. Indicate which, if any, fulfill the “octet rule” when neutral. If they do not fulfill the octet rule when neutral, indicate the number of electrons gained or lost for the atom to fulfill the rule. Sodium Silicon Magnesium Mg Phosphorus Aluminum Al Sulfur Si P Chlorine Cl Argon Ar S 4 ION FORMATION Fill in the following table regarding ions Element Group Name Ion Type cation/anion Sodium Alkali metals cation Charge # and +/+1 Metal / Non-Metal Metal Selenium Oxygen group anion -2 Non-metal Boron B/Al group cation +3 Metalloid Phosphorus Nitrogen group anion -3 Non-metal Calcium Alkaline Earth cation +2 Metal Fluorine Halogens anion -1 Non-metal Radon Noble Gases none none Non-metal Phosphorus Nitrogen group anion -3 Non-metal BONDING Fill in the following table regarding ionic bonding Cation Charge Anion Charge Calcium +2 Sulfur -2 Balanced Formula CaS Strontium +2 Chlorine -1 SrCl2 Aluminum +3 Iodine -1 AlI3 Cesium +1 Nitrogen -3 Cs3N Magnesium +2 Oxygen -2 MgO Boron +3 Phosphorus -3 BP Sodium +1 Fluorine -1 NaF Chemical Name Calcium sulfide Strontium chloride Aluminum iodide Cesium nitride Magnesium oxide Boron phosphide Sodium fluoride 5 POLYATOMIC IONS Fill in the following chart Cation Formula and Anion Charge Calcium Ca +2 Hydroxide Formula and Balanced Charge Formula -1 OH Ca(OH)2 Strontium Sr +2 Nitrate NO3 -1 Sr(NO3)2 Ammonium NH4 +1 Acetate C2H3O2 -1 NH4C2H3O2 Cesium Cs +1 Chlorate ClO3 -1 CsClO3 Magnesium Mg +2 Cyanide CN -1 Mg(CN)2 Boron B +3 Sulfate SO4 -2 B2(SO4)3 Sodium Na +1 Nitrite NO2 -1 NaNO2 Chemical Name Calcium hydroxide Strontium nitrate Ammonium acetate Cesium chlorate Magnesium cyanide Boron sulfate Sodium nitrite BALANCING EQUATIONS AND REACTION SYMBOLS Balance all equations. Label reaction type for all reactions. 1. N2(g) + 3H2(g) 2. 2KClO3(s) ∆ 3. 2NaCl(s) + 4. 2AgNO3(aq) + MgCl2(aq) 2AgCl↓ + Mg(NO3)2(aq) DOUBLE REP. 5. C3H8(l) + 2NH3(g) SYNTHESIS 3O2(g) DECOMPOSITION 2KCl(aq) + F2(g) 2NaF(aq) 5O2(g) 3CO2(g) + + Cl2(g) SINGLE REP. 4H2O(l) COMB. Answer the following questions based upon the formulas above. 1. Rewrite #4 as a word equation. Dissolved silver nitrate and dissolved magnesium chloride react to form solid solver chloride and dissolved magnesium nitrate. 2. What does the subscript “(g) “in #1 and subscript “(s)” indicate in equation 2? Gas; solid 3. Does equation 3 take place in water? How do you know? Yes; the NaF is dissolved 6 4. Write the formula for the precipitate in equation 4. Rewrite its name in word format. AgCl↓, silver chloride 5. Write the 3 criteria for identifying a combustion reaction. Hydrocarbon and oxygen are reactants; products are always CO2 and H2O 6. What does “∆” indicate in equation 2? How can you indicate a catalyst in a reaction? Heat; symbol will be written over the arrow. REACTIONS STOCHIOMETRY and Limiting Reactants: Perform the following stochiometric calculations. Make sure you have a balanced equation first! CH4 + 2O2 CO2 + 2H2O How many grams of O2 are needed to react with 9.02 g of CH4? 36.1 g O2 2. N2 + 3H2 2NH3 How many grams of NH3 are formed when 11.7 g of H2 react? 65.9 g H2 3. 2C + O2 2CO How many grams of carbon are needed to produce 0.98 g of CO? 0.82 g C 4. Silicon dioxide (quartz) reacts with hydrogen fluoride to produce silicon(IV)fluoride and water by the reaction SiO2 + 4HF SiF4 + 2H2O. Determine which is the limiting reactant if 2.0 mol HF is combined with 4.5 mol SiO2? 2.0 mol HF is limiting 5. Using the reaction above, determine which is limiting and which is excess when 46.3 g of SiO2 react with 25.0 g of HF. 25.0 g HF is limiting 7 GRAPH OF TEMPERATURE VS. TIME FOR A SUBSTANCE BEING HEATED T E M P E R A T U R E (°C) 180 170 160 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 0 E D B C A TIME (seconds) Phase Changes – temperature vs. time: Phase changes (step diagram) Indicate the following on the graph above. melting, vaporization, solid being heated, liquid being heated, gas being heated, freezing, condensation Answer the following questions based upon the diagram above. 1. Which interval(s) on the graph above indicate a change in kinetic energy? A—B; C-D and E above 2. Which intervals on the graph above indicate a change in potential energy? B-C and D-E 3. At lines A-B and C-D the graph shows plateaus - the temperature is not changing while heat energy is still being added. Describe what the heat is doing to particles of the substance. Breaking bonds 4. Explain the difference between vaporization and evaporation. Give an example for each. Vaporization (boiling) is where the substance becomes liquid from inside and the surface. Evaporation is vaporization from the surface only. 8 GASES: Name and describe the three types of particle motion. Indicate the phases of matter that exhibit each. Rotation (spinning in place) – all phases Vibration (shaking in place) – all phases Translation (moving from place to place) – Liquid and Gas only Describe the “Kinetic Theory of Gases” and list the three assumptions associated with it. What volume does one mole of any gas occupy at STP? 22.4 L Kinetic theory states that all matter is composed of particles and the particles are in constant motion. Particles are small hard spheres which are not attracted or repelled from each other. They move in straight lines until they impact with something. Between the particles is empty space. Define “phase change.” This is a physical change which involves changes in the bonds between particles, types of particles, and the types of particle motion. No chemical bonds are made or broken. Define these types of phase changes. Give an example of where you might experience each. Melting - solid to liquid Vaporization - liquid to gas Freezing - liquid to solid Condensation - gas to liquid Evaporation - liquid to gas (surface only) Sublimation - Solid to gas GAS LAWS: Solve the following problems using the gas laws 1. A gas with volume of 5.3 L at 17°C decreases to -3°C. Find the new volume. 2. A 2.1 L sample of gas a standard pressure is moved to a 5.2 L container. Find the new pressure. 3. An aerosol can contains gas at 15 atm and 25°C. Find the pressure inside the can at 100.°C 4. Find the number of moles of gas in a container at the following conditions – 6.0 atm, 3.6 L, and 118°C. 5. A gas at 742 mmHg and -18°C occupies 1.7 L. Find the volume of the gas at STP. 6. Define absolute zero. Give the temperature for it in both °C and K. -273°C and 0K; temp at which all particle motion ceases 7. A mixture of four gases is stored at 1187.3 mmHg. H2 is 127 mmHg, O2 is 350 mmHg and CO2 is 642 mmHg. Find the partial pressure of the Helium in the mixture. 68.3 mmHg 9 8. Under what conditions does a gas stop acting “ideal” and begin acting “real?” low temps / high pressure 9. What volume does one mole of any gas occupy at STP? 22.4L CONVERSIONS Perform the following conversions. 1. 26C to K 299K 5. 23.5 atm to mmHg 2. -52C to K 325K 6. 89 kPa to Torr 3. 89 K to C 184°C 7. 768 mmHg to atm 4. 304 K to C 31°C 8. 11.2 atm to kPa 17900 mmHg 670 Torr 1.01 atm 1130 kPa WATER AND SOLUTIONS: Draw a picture of a water molecule. Indicate the poles on this polar molecule. Write a definition and example for each of the following. Polar – charges on the water molecules (O is slight negative while H is slight positive) Specific heat – amount of energy required to raise Surface tension – “skin” on water (water strider) Hydrogen bonds – bond b/w adjacent water molecules b/w – O and + H (drops on a penny) one g of water by 1°C (1 cal) Surfactant - breaks H-bonds (soap) a) Why does solid ice float on liquid water? H-bonds hold water molecules apart; increases spaces between molecules b) How does soap help to clean dirty dishes? Soap is a surfactant which breaks Hbonds and allows the soap and oil to mix 10 MOLAR MASS AND PERCENT COMPOSITION Find the gram formula mass for the following formulas BaCl2 208.236 g/mol CuSO4 159.608 g/mol NaNO3 84.994 g/mol Ba(OH)2 171.3438 g/mol Determine the percent composition of the following S in CuSO4 20.1% NO3 in NaNO3 72.9% H2O in CuSO4 * 5 H2O 36.1% Empirical and Molecular Formulas A compound sample is made of 40.68 g C, 5.08 g H and 54.24 g O. Its molar mass is 118.1 g/mol. Determine the empirical and molecular formula. A compound sample contains 174.86 g iron and 75.14 g oxygen. Molar mass is 160.0 g mole. Determine the molecular formula. Acids and Bases What helps you to recognize an acid when you look at a chemical formula? What are the general characteristics of acids? H (hydrogen) ion; smell strongly, corrosive, react with bases and metals; conduct electricity What helps you to recognize a base when you look at a chemical formula? What are the general characteristics of bases? OH (hydroxide) ion; slippery corrosive; react with acids What two products are always formed from the neutralization of an acid and base? Water and salt Write the chemical equation for the neutralization of hydrochloric acid and sodium hydroxide HCl + NaOH NaCl + H2O Write the chemical equation for the neutralization of sulfuric acid and potassium hydroxide H2SO4 + 2 KOH K2SO4 + 2 H2O 11 Data Analysis, Significant Figures and Sources of Error: Students want to determine the percent of water in a compound. They heat the substance in a watch glass in order to drive off the water. The raw data they collected is found below. Use this information to answer the questions. Item CuSO45H2O Mass of Empty Watch Glass 46.25 g Mass of Watch Glass and Compound before 70.65 g heating CuSO45H2O Mass of Watch Glass and Compound after 63.33 g heating CuSO4 a. What is the mass of the sample of CuSO45H2O they started with? 24.40g b. What is the mass of the water lost? 7.32g c. From the given data, calculate the percent water in the compound. 30.% d. What is the mass of one mole of this entire compound? 249.684 g/mol e. What is the mass of just the water that is trapped in 1 mole of this compound? 90.074 g/mol f. From the two previous questions, determine the actual percent (accepted value) of water that makes up this compound. 36.1% g. Assuming that the accepted value of % water should be 36.1%, determine the % error for this lab group’s results. 16.9 % h. If their experiment showed the percentage of water to be too low, how might this error have occurred? Incomplete evaporation 12 Determine the number of significant figures in each of the following numbers. a. 13,000 2 b. 13,000. 5 c. 0.00013 2 d. 9.0 x 109 2 Solve the following correctly, and include the correct label and number of significant figures in your response. a. A box measures 1.613 m by 6.213 m by 5.15 m. Determine the volume of the box. 51.6 m3 b. You measured the mass of a beaker as 16.255 g. When you added water to the beaker, you measured the mass as 36.04g. Determine the mass of the water in the beaker. 19.79g c. In B above, what should you have done to allow you to record the mass of the water to the thousandth of a gram? Read your mass decimal measurement to a thousandth of a gram. (0.001g) State the rules for use of significant figures within calculations: For addition and subtraction? Round to the same number of decimal places as the addend with the fewest decimals For multiplication and division? Round to the same number of significant figures as the multiplicand or divisor with the fewest significant figures. That’s it! If you would like additional practice for any of the topics covered on this exam – see me! 13