Name: Chemistry SOL Review Test PROPER SCIENTIFIC

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Name:Chemistry SOL Review TestDirections: Read each question and write a brief answer. Use your notes,diagrams, etc. to help you. SHOW ALL WORK (no work no credit) Your work and writing must be neat & legible (unreadable no credit)Unit 1: Measurement (Ch. 3)1) Define the followingaccuracy reflects how close a measurement is toa) Accuracya known or accepted valueb) Precisionc) Quantitative Datad) Qualitative Dataprecision reflects how reproduciblemeasurements are, even if they are far from theaccepted valuequantitative analysis is used to tell 'how much' isin a sampledata that determine the characteristics of asubstance chemical constituents.2) Number of Significant Figuresa) 1.23 X 1073b) 100.10107c) 33,0002d) 0.0000413) Perform the calculations indicated. Round your answer to thecorrect number of significant figures.1500a) 632,000 410b) 100.0 45.0 35180.c) 98.012 16114d) 891.000 * 1.08904) Put the following numbers in proper scientific notation.-5a) 0.00003303.30 x 10b) 95,200,0009.52 x 1075) Take the following numbers out of scientific notation.a) 3.458 X 10-110.000 000 000 0345810b) 2.4 X 1024,000,000,0006) Answer the following: Be sure to put your answers inPROPER SCIENTIFIC NOTATIONa) (3.10 x 103) (1.68 x 102)3.27 x 103b) (1.11 x 108) – (1.1 x 103)1.1 x 1085-9c) (8.00 x 10 ) / (4.00 x 10 )2.00 x 1014d) (600 x 1025)*(0.00020 x 10-10)1 x 10147) Use the solving problems method to answer the followingquestions. SHOW ALL OF YOUR WORK.a) How many micrograms are in 3.00 grams?3.00g1,000,000 μg 3.00 x 106 μg1gb) How many seconds are in 24 days?24 days 24 hrs 60 min 60 sec 1 day1 hr1 minc) How many grams are in 9.42 mL ofpentane (C5H12)?(Density 0.0980 g/mL)9.42 ml0.0980 g 1 mLd) How many milligrams are in 85kilograms?85 kg 1,000 g 1,000,000 μg 1 kg1g2,073,600 sec2,100,000 sec0.923g C5H128.5 x 1011 μgUnit 2: Matter & Energy (Ch. 2)8) Classify the following as either a physical or chemical changea) Pizza is slicedPhysical changeb) Paper is tornPhysical changec) NaCl is dissolvedPhysical changed) Wood burnsChemical change9) ID the following as either a heterogeneous mixture or ahomogeneous mixture.a) Italian dressingheterogeneous mixtureb) NaHCO3 solutionhomogeneous mixturec) Muddy solutionheterogeneous mixture

10) Predict whether the element is a metal, nonmetal, or metalloid.nonmetala) seleniummetal,b) magnesiumnonmetalc) chlorined) antimonymetalloid11) List four different characteristics of metals & nonmetalsNonmetalMetalNot Ductile (Brittle)DuctileLow MP and BPHigh MP and BPTend to be volatileLuster (shiny)InsulatorsConductors12) Describe the following changes of statea) SublimationSolid to Gasb) FreezingLiquid to solidc) VaporizationLiquid to Gasd) CondensationGas to Liquide) MeltingSolid to Liquid13) Differentiate between gases, liquids, & solids.solidsliquidsgasesSlowFasterFastestParticle speedclose together no Far apart noParticle spacing entFixedregulararrangementVariable(fixed or variable)ShapeDefiniteNotNot(definite or not)Most denseSomewhat denseLeast denseDensityNoNoteasilyYesCompressible?14) Identify the group/family number/s for the following:a) Noble gases18b) Halogens17c) The Alkali Metals1d) Alkaline Earth Metals2e) Transition Metals3-12Unit 3: Atomic Structure and Theory (Ch. 4)15) Describe the Dalton’s atom model. Atoms are indivisible andindestructible. (Billiard ball model)16) Describe Thomson’s atom model. Electron are like raisinssurrounded by a soup of positive charge to balance the electrons'negative charges (Plum Pudding Model).17) What experiment did Thomson do? The cathode rays tube18) What was his model called?Plum Pudding Model19) Describe Rutherford’s model. Atoms have a center nucleus andthe rest of the atom is mostly empty space20) What experiment did Rutherford do? He shot alpha particlesthrough a thin film of gold and to his amazement a few alphaparticles rebounded almost directly backwards.21) What was his model called? “gold foil" experiment22) Describe Bohr’s model. He proposed his quantized shell model ofthe atom, electrons orbits around the nucleus23) What was his model called? Planetary Model24) What is the difference between an isotope and an ion?IsotopeIonDifferent number of NeutronsDifferent number of Electrons25) Use your periodic table to fill in the following table.(HINT: These are isotopes)Protons Neutrons Electrons Atomic Massnumber number3344333377a) As -77153745453127b) I3035303065c) Zn2 2630242656d) Fe565511e) boron-1126) A cation is positive “ ” in chargea anion is negative “‒“ in charge.27) A horizontal row in the periodic table is called a Periods28) A vertical column is called a Groups or FamiliesH29) protonBFG30) isotope31) electron32) neutronD33) nuclear pullE34) shieldinga. the smallest particle of an element that retains theproperties of that elementb. atoms of the same element with different massesc. the number of protons in the nucleus of an atomd. attraction of positive nucleus for the outer negativeelectronse. electrons in between the outer electrons and the nucleusshield the positive nucleus from the negative outer electrons.f. the first subatomic particle discovered

AC35) Atom36) atomicnumberg. subatomic particle with no chargeh. .the kind of subatomic particle with a positive charge37) The element iron is made up of the isotopes 58Fe (2.45%), 56Fe(80.3%), 54Fe (10.2%), and 57Fe (7.05%). Calculate the averageatomic mass (weight) of iron.Answer: 58 (0.0245) 56(0.803) 54(0.102) 57(0.0705) 55.92Unit 4: Electrons in atoms (Ch. 5)38) Describe the following prop39) erties and their periodic trend (you may draw a picture forthe trend)DefinitionTrenda) electron affinity increasesDHACFEBG40) 1st quantum #41) p orbital42) Atomic spectrum43) Electromagneticspectrum44) 3rd quantum #45) 2nd quantum #46) d orbital47) 4th quantum #a) the characteristic spectrum of an elementb) complex shapedc) A listing of all known forms of radiationd) describes how far the electrons is from the nucleuse) describes the shape of the orbitalf) describes the orientation of the orbitalg) describes the direction the electron is spinning inh) dumbbell shaped48) Whichcolor has the shortest wavelength? ROY G BIV (longest to shortestso Violet)b) electronegativity increases49) Define the following terms.FrequencyThe amount of time it takes for one cycle to completeAmplitudeThe distance from the equilibrium to the crest or to the troughWavelength The distance from Crest to Crest or Trough to Troughc) ionization energy increases50) Write the complete electron configuration for the following :2262622a) Titanium (Ti). 1s , 2s 2p , 3s 3p , 4s , 3dd) atomic radius increasese) ionic size (cations, anions)f) Atomic numberg) valence electronsh) atomic massi) electron configuration (s, p, d, f blocks) increases increases increases increases22626b) Si-4 1s 2s 2p 3s 3p normally it would be 3p2 but there are 4-4additional electrons Sigiving it a noble gas configurationUnit 5: Nomenclature (Ch. 9)51) Name the following compounds: (molecular or ionic)HINT: Molecular 2 nonmetals – use prefixes; Ionic anything else – just statethe name of the cation then anion (use roman numerals if it is a cation w/multiple charges)a) CaSb) PO3Calcium SulfidePhosphorus trioxidec) N2O6d) (NH4)3CO3Dinitrogen hexoxideAmmonium carbonatee) C2I4f) Fe2O3Dicarbon tetraiodideIron (III) oxide52) Write the formulas for the following compoundsb) rubidium carbonatea) lead (IV) chlorideRb2CO3PbCl4c) silicon monoxided) sodium arsenideSiONa3As

e) strontium nitrateSr(NO3)2Unit 6: The Mole (Ch. 10)f) silver nitrideAg3NUse the solving problems method to answer the following questions.SHOW ALL OF YOUR WORK and use significant figures.53) Find the molar mass of Sr3(PO3)2Sr 87.62(3) P 30.97(2) O 16.00(6) Answer: 420.8054) How many formula units are in 2.84 moles of potassium oxide(K2O)?2.84 mol K2O 6.02 x 1023 fu Answer: 1.71 x 1024 fu K2O1 mol K2O55) How many moles are in 8.50 X 1023 molecules of water?8.50 x 1023 mlcs H2O1 mol H2O Answer: 1.41 mol H2O6.02 x 1023 mlcs H2O56) How many grams are in 4.42 moles of methane (CH4)?4.42 mol CH416.05 g CH4 Answer: 67.4 g CH41 mol CH457) How many moles are in 1.2 X 104 liters O2 gas at STP?1.2 x 104 L O21 mol O222.4 L O2 Answer: 540 mol O258) How many grams are in 0.9500 liters F2 (Fluorine Gas)?1 mol F238.00 g F2 Answer: 1.612 g F20.9500 L F222.4 L F21 mol F259) How many atoms of nitrogen are in 56.652 grams of nitrogen?56.652 g N2 1 mol N2 6.02 x 1023 mlc N2 Answer: 1.2171 x1023 mlc N228.02 g N2 1 mol N260) Find the percentage composition of a compound that contains19.5 g of iron and 5.8 g or sulfur. The total mass of the compoundis 20.3 g.Answer: omit61) 11.66 g iron, 5.01 g oxygen. Find the empirical formula.11.66 g Fe 1 mol Fe55.85 g Fe5.01 g O 1 mol O16.00 g O 0.20877 / 0.20877 1 x 2 2 3.13125 / 0.20877 1.5 x 2 3So the empirical formula is Fe2O362) What is the molecular formula? empirical formula NO2,molar mass 92.02 g/molN 14.01(1) 16.00(2) 46.0192.02/46.01 2So there are 2 (NO2); so the molecular formula is N2O463) What is used to convert molecules to moles?a) Name: Avogadro’s numberb) Number: 6.02 x 1023 mlcs/moleUnit 7: Chemical Equations (Ch. 11)64) Use the activity series of metals to determine which of thefollowing reactions will occur. If a reaction will take place,complete and balance the equation. If the reaction will not occur,write no reaction.a) 2 Al 3 CuSO4 3 Cu Al2(SO4)3b) 6 Ag 2 H3PO4 3 H2 2 Ag3PO465) Determine the products of the following double replacementreactions.a) 3 Ag2CO3 2 Na3PO4 2 Ag3PO4 3 Na2CO3b) Pb(NO3)2 CoCl2 PbCl2 Co(NO3)266) What are the meanings of the following symbols?a) (aq)aqueousb) given off (gas)c) Precipitate (solid)d) heat67) Directions: Balance the following reactions. To the right ofeach equation, write the type of reaction each represents. (Use S,D, S-R, D-R, C rather than the name)a) Zn HCl ZnCl2 H2Single Replb)C7H6O2 O2 CO2 H2Oc) Sb O2 Sb4O6CombustionSynthessisd) H2O2 H2O O2Decompostione) Al2(SO4)3 Ca(OH)2 Al(OH)3 CaSO4Double Repla

Unit 8: Stoichiometry (Ch. 12)68) Define the following:It is the reactant that is completely used upa) Limiting Reagentb) Actual Yieldc) Percent Yieldd) Theoretical Yieldin a reactionThe experimental yield, what you actuallyget.(Actual yield/Theoretical yield) x 100.Percent yield measures how efficient thereaction is under certain conditions.The amount of product that could possiblybe produced in a given reaction.Answer:73) Sodium chloride can be prepared by the reaction of sodiummetal with chlorine gas. 2Na (s) Cl2 (g) 2 NaCl (s)a) When 6.70 mol of Cl2 reacts with 3.20 mole of Na, what isthe limiting reactant?Answer:b) How many moles of NaCl are produced?Problems: Make sure that your chemical equation is balanced. Set up a proportion under the substances in the equation that you areinterested in.Divide by the coefficient to cancel out moles, the (coefficient * molarmass) to cancel out grams, or the (coefficient * 22.4) to cancel outliters 69) How many moles of aluminum oxide are needed to reactcompletely with 5 moles of SnO?2Al 3SnO 3Sn Al2O35 mol SnO 1 mol Al2O3 1.7 mol Al2O33mol SnO70) How many moles of sodium are needed to react with 18.3 g ofSodium chloride?2 Na Cl2 2 NaCl18.3g NaCl 1 mol NaCl 2 mol Na 0.313 mol Na58.44 g NaCl 2mol NaClAnswer:c) How much of the excess reagent remains unreacted?Answer:74) Calcium carbonate is decomposed by heating.CaCO3 CaO CO2What is the percent yield of this reaction if 27.8 g of CaCO3 isheated to actually produce 13.6 g of CaO?Answer:71) If 48.3 g of Fe2O3 react with Aluminum in a singledisplacement reaction, how many grams of aluminum are needed?2 Al Fe2O3 Al2O3 2 Fe48.3g Fe2O3 1 mol Fe2O3 2 mol Al 0.605 mol Al159.7 g Fe2O3 1mol Fe2O375) 2 Al 2 H3PO4 2AlPO4 3H2What is the percent yield if 6.6 g of Al is reacted to produce 1.85 gof H2?72) If 40 L of oxygen combine with oxygen to synthesize water,how many grams of water are produced? 2H2 O2 2 H2OUnit 9: GASES (Ch. 14 &Ch 13)(don’t forget to change C to K)76) What do moles tell you? What is the unit for n?Answer:77) What is volume? What are the units of volume?

78) What are the units for pressure and how are they related?1 atm 101.325 kPa 760 mmHg 760 torrs79) Fill in the following tableGayAvogadro’s Charles’ Boyle’sLussac’sFormulaV1 V2 P1V1 P2V2P1 P2 V1 V2T1T2 n1 n2T1T2Inverse or Direct DirectlyDirectlyDirectlyInverselyGraphR 8.31 L*kPamol*K; 0.0821 L*atmmol*K;62.4 L*mmHgmol*K80) Many gases are available for use in the laboratory incompressed gas cylinders, in which they are stored at highpressures. Calculate the number of moles of O2 that could bestored at 24.0 C and 0.935 atm, in a cylinder with a volume of16.5 liters?PV nRTAnswer:81) A balloon contains 2.5 mol of helium at a pressure of 1.06 atmand a temperature of 274. K. What is the volume of the balloon?PV nRTAnwer:82) A helium balloon with a volume of 22.5 L, a pressure of101.3.kPa, and a temperature of 328 K is put into an environmentwhere the pressure is 25.0 kPa and the temperature is 25.0 C.What is the new volume of the balloon?Answer:83) The gas balloon has a volume of 4.8 L at 330 K. At whattemperature will the balloon expand to 8.50 L?Answer:84) A 2.43 L balloon contains 0.35 moles of He. How muchHelium must be added in order for the balloon to be 5.2 L?Assume constant temperature and pressure.Answer:85) Calculate the temperature ( C) of 2.65 g of I2 if it occupies 50.mL at 676 mm Hg.PV nRT676 mmHg 0.050 L (2.56g/253.8 g/mol) (62.364 L mmHg mol-1 K-1) T53 K or -219 CAnswer:Unit 10: Liquids (Ch. 15&16)86) The solubility of most liquids increases as temperatureincreases. (increases/decreases)87) The solubility of gases in liquids increases as temperaturedecreases.88) Three colligative properties are:1. Vapor pressure depression2. Boiling point elevation3. Melting point depression4. Osmotic pressure89) Four factors which affect solubility.a)b)c)d)TemperaturePressureSolvent – Solute interaction (like and unlike)Size

90) What is the molarity of a 1500 mL solution made with 7.5moles of KCl?7.5 mol KCl 1.6 M1.5 L91) How many mL of a 0.01 M solution of NaCl would you needin order to have 1.4 moles?1.4 mol 0.01 M NaClx 140,000 mLxL92) How could you make a 2.5 M NaOH dilute solution in a 250mL volumetric flask, from a 3 M concentrated solution of NaOH.M1V1 M2 V2 2.5 M 250 ml 3 M x x 208 mLSo place 208 mL of the 3M solution in a flask and add 42 mL of H2Ofor 250 mL of 2.5 M solution.102) Fill in the following chartLewis DotDiagramCO# of lone # of Molecular BondVSEPRpairsbonds Geometry Angles Structure(name)skipskipH2Se93) If NaCl dissolves in water? Is NaCl POLAR or nonpolar?Unit 11: Bonding (Ch. 8 & 7.3)94) Write electron dot structures for the following ATOMSa) siliconb) S95) Write electron dot structures for the IONS of the followingatomsa) S-2GeH4AlF3b) Mg 296) Use the electronegativity table to determine what type of bond(IONIC, VERY POLAR COVALENT, MODERATELYPOLAR COVALENT, OR NONPOLAR COVALENT) willform between the atoms of the following elements.IONIC97) Mg and FMODERATELY POLAR COVALENT98) C & HPOLAR COVALENT99) C and OIONIC100) Na & FMODERATELY POLAR COVALENT101) H and BrUnit 12: RATES OF REACTION & CHEMICAL EQUILIBRIUM (Ch.18)103) Using the following equations for complex ions, draw anarrow to show how each system would change under thefollowing conditions. (In which direction will the equilibriumshift?)[Zn(H2O)4]2 H2O [Zn(H2O)3(OH)] H3O a. Removing waterb. Adding H3O

104) For the following reaction, equilibrium is established at acertain temperature when the following concentrations are present:[CO] 0.10 mol/L, [H2O] 0.80 mol/L, [CO2] 0.012 mol/L,and [H2] 0.012 mol/L. Calculate the Keq value for this reaction.HINT: Write the equilibrium expression for the reactions, then fillin the values and solve for KeqCO (g) H2O (g) CO2 (g) H2 (g)Answer:Unit13: Acids, Bases, & Neutralization (Ch. 14)105) In a neutralization reaction the products are always and .106) An acid turns litmus paper and a base turns litmus paper .107) Water is amphoteric because it can108) pH [H ]109) Label the Bronsted-Lowry acid, base, conjugate acid, andconjugate base in the following reactions.a) H2O H3PO4 H2PO4-1 H3O b) H2O H2SO4 H3O HSO4-1110) Name each of the following acids and their anionsFormulaName of anionName of acida) HBrb) H2CO3c) H3PO3d) H2SO3111) Write the formulas for the following acids.NameCationAnionFormulaa) Chloric acidb) Phosphorous acidc) hydronitric acid112) Complete and balance the following neutralization reactions.a) H2SO4 Ca(OH)2 b) HI NH4OH 113) Determine the pH for the aqueous solutions with the following[H ]. Is the solution acidic, basic or neutral?[H ]pHAcid, base, orneutrala) 1 X 10-6 Mb) 1 X 10-7 M114) Determine the [H ] for aqueous solutions that have thefollowing pH values. Is the solution acidic, basic, or neutral?pH[H ]Acid, base, orneutrala) 11b)8115) Determine the pH of the following solutions that have thefollowing [OH-]. Is the solution acidic, basic, or neutral?[OH-]pHAcid, base, orneutrala) 3.8 X 10-3b)0.000001116) Would a stronger acid have a large or a small Ka?117) In a titration, a 15 mL solution of hydrochloric acid isneutralized by 6 mL of 2.5 M sodium hydroxide, usingphenophthalein as an indicator. What is the concentration of thehydrochloric acid solution?Answer:

Unit 14: REDOX(Ch. 20)O.I.L.R.I.G.118) Oxidation is the loss / gain of electrons & increase/decrease of oxidation #.119) Reduction is the loss / gain of electrons & increase/decrease of oxidation #.120) Show the oxidation numbers for all of the atoms in thefollowing equation.Al(OH)3 H2SO4 --- Al2(SO4)3 HOH121) In the following equation, which chemical is oxidized?Reduced? Oxidizing agent? Reducing agent?Zn HCl --- ZnCl2 H2Oxidizing Agent:Reducing Agent:Oxidized:Reduced:129) Write the half reactions for the oxidized and reducedchemicals in previous problem.Oxidation ½ reaction :Reduction ½ reaction:Unit 15: Thermochemistry (Phase Changes)(Ch. 17)Heat energy mc T (WITHIN A PHASE)Heat Energy m H (TO CHANGE PHASE)4.18 J 1 Cal & specific heat of liquid water 1 cal/g C130) A 16.3 gram water sample in a calorimeter has its temperatureraised 8.0 C while an exothermic chemical reaction is takingplace. How much heat is generated in the calorimeter? (solve forcalories and for joules)Answer:Answer:131) How many joules would be needed to raise 20.0 grams of waterforms 10.0 C to 98 C?Answer:132) If 5.0 grams of water at 45 C gains 5600.0 Joules of heat,what is the final temperature of the water? (Hint - solve for T)Answer:133) 98.7. grams of a material is melted at it’s freezing point.Heat of fusion 472 J/gAnswer:134) 16.3 grams of a material is heated from 100oC to 200oCSpecific heat 2.34 J/goCHow much heat is absorbed?122) the energy required to melt of mole of asubstance123) the energy required to change one mole of asubstance from a liquid to a gas.124) a measure of the randomness or disorder of asystem125) The total energy content of a system126) A substance that increases the rate of achemical reaction and that is not changed by thereaction.127) The system gains energy128) The system releases energya. entropyb. heat ofvaporizationc. heat of fusiond. endothermice. exothermicf. enthalpyg. catalystAnswer:Match the following:135) Decide which of these reactions are endothermic andexothermic,Your DONE!!a. BCl3 3 H2O H3BO3 3 HCl H -112kJb. 2 Fe 3 CO2 26.8 kJ Fe2O3 3COc. C2H4 2 H2 52.3kJd. S2Cl2 CCl4 CS2 3 Cl2 H 112kJ

c) Quantitative Data quantitative analysis is used to tell 'how much' is in a sample d) Qualitative Data data that determine the characteristics of a substance chemical constituents. 2) Number of Significant Figures a) 1.23 X 107 3 b) 100.1010 7 c) 33,000 2 d) 0.00004 1 3) Perform the calculations indicated. Round your answer to the