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ACS Study Guide Solutions for Practice QuestionsAtomic Structure D – definition of a neutral atomD – can identify based on atomic number (number of protons) which is the bottom left number. Top left number is the mass number (protons + neutrons)D – protons and neutrons occupy next to no volume, they are concentrated in the nucleus. Only electrons have volume/take up space in the atom.B – mass number minus the atomic number = number of neutronsC – isoelectronic means to have the same number of electronsA – same as 6C – remember that positively charged ions lost electrons from neutral atom and negatively charged ions gained electronsB – definitionA – inert means unreactive noble gas configuration. Ions always have noble gas configurations.A – sodium ion is positively chargedC – deuterium is an isotope of hydrogen that has 1 proton and 2 neutrons. Also, you can eliminate the other choices based on the fact that you have never heard those terms before. C – use weighted average isotope formulaB – isoelectronic means same number of electrons, isotopic means same element but different mass number A – an alpha particle is a helium nucleus (2 protons, 2 neutrons), so the mass number should decrease by 4 and the number of protons (atomic number) should decrease by 2B – like charges repel, so nucleus will only attract the alpha particles at high speeds; A doesn’t make sense since that would naturally happen without extra speed, C is wrong because speed doesn’t affect accuracyC – experiments are found in first chapter of your textbook. A few to know: Thomson discovered the electron, Millikan discovered the charge on an electron, and Rutherford discovered the proton through a gold foil experimentA – valence electrons are those in the highest energy level (highest n value)B – 2d does not existD – use your periodic table and s, p, d, and f blocks to determine ground-state electron configurationsD – missing the 4s shell tells you this is an ion with a +2 chargeB – maximum 2 electrons in ANY orbitalD – draw orbital box diagram, remember that every orbital must have one electron before they can be pairedA – paramagnetic means that the species has unpaired electronsD – fill all positive spins before pairing and filling negative spinsD – definition A – highest frequency means highest energy jump, remember that lower energy level transitions have larger energy values on the Bohr diagramA – last quantum number must be +/- ?, ml value ranges from – to + lD – electropositive is a fancy term for a positively charged ion, these lose electrons and become smallerC – definitionA – the helium ion has 1 proton and 1 electron, exactly the same composition as the hydrogen atomMolecular Structure and Bonding A – draw the Lewis structure for the final compound and use your knowledge of molecular geometries to determine this. FOR THE ACS, geometry or shape ALWAYS refers to the molecular geometry. If they want the electronic geometry, they will specify. In other words, always take lone pairs into account.D – draw structureC – draw Lewis structureD – draw the Lewis structures and see two have the same geometryC – planar means flat, that all atoms are in the same plane anything with tetrahedral geometry has one atom sticking out of the plane and cannot be planarD – draw Lewis structureA – use molecular geometriesA – draw Lewis structureA – draw Lewis structures and remember that lone pairs on the central atom compress bond angles the more lone pairs or more lone electrons something has, the more the bond angles are compressedC – draw the Lewis structuresD – this is the definition of resonance, which is the concept being tested. Look always for the MOST CORRECT answer, and not just the one that is correct on its own.B – theory that explains covalent bonding is hybridizationA – hybridization + Lewis structureB – lone pairs = polar, larger dipole momentC – tricky because this is a coordinate covalent compound. All of the individual SiO2 molecules are bonded to other ones, making the geometry tetrahedral and the angles about 109. CB – only answer that is true and pertains to the idea of polarityC – add all valence electronsB – draw Lewis structuresC – only difference between all of the molecules B – molecule needs to have lone pairs to shift or isomerize between two formsD – look for the polyatomic ions (those are connected within by covalent bonds, but to other ions by ionic bonds)D – single bonds are longer than double bonds ethane has single bonds, benzene has a mix of double and single bonds, ethene has all C-C double bondsC – we want formal charge to be as close to zero as possible (formal charge = valence electrons – lone pair electrons - # of bonds)C – know through practiceA – isomers have same molecular formula (# of atoms) but different connectivity A – single bonds have one sigma bond, double bonds have one sigma and one pi, triple bonds have one sigma and two piB – cubes have six faces, so an atom in the middle of the cube would be in contact with 6 facesD – definitionB – complete the Lewis structure they have started for youStoichiometryA – follow the steps to find an empirical formula (assume 100 grams, turn percentages into grams, convert grams to moles, divide by the smallest number of moles to get subscripts)C – follow steps to find empirical formula, remember if you end up with fractions in your subscripts you must multiply through by a factor to get rid of them (multiply anything with .25 and .75 by 4, .5 by 2, and .33 and .66 by 3)D – empirical formula, since you are missing percentages you must find those first before you can follow the steps in #1C – percent by mass formula = (mass of element * how many of that element is present) / total mass of compoundC – same as 4B – convert grams to moles using the molar mass, multiply by the percentage of carbon in the sampleC – convert grams to moles using molar mass, then moles to atoms using Avagadro’s numberC – this is a tricky one. Convert molecules given to moles using Avagadro’s number. Anytime you are have both grams and moles values for the same compound, you can divide grams by moles to get the molar mass. Subtract the mass of xenon from this molar mass, then divide by the mass of fluorine. C – convert molecules to moles. For every 1 mole of compound, there are 12 moles of carbon, so you can find the moles of carbon in the same. Convert those moles to grams of carbon. D – write a balanced equation for this reaction (4 M + 3 O2 2 M2O3). Convert from moles of metal oxide to moles of metal using mole to mole ratios. Calculate the molar mass by dividing grams given by moles calculated and use calculated molar mass to determine identity of metal.A – convert molecules to moles, then divide grams by moles to get molar mass to identify compound.D – definitionA – convert grams to moles and moles to atoms for each value given and compare.D – convert molecules to moles, then divide grams by molesC – write balanced equation (2 KClO3 2 KCl + 3 O2). Convert grams to moles, use molar ratios, then convert back from moles to grams.C – use molar ratios to covert to aluminum chloride then covert from moles to grams.A – convert from grams to moles, use molar ratios to convert to oxygen gas, then convert from moles to molecules.A – use value of S moles and molar ratios to calculate how much fluorine was used during the reaction, then subtract this value from the amount that you started with.B – this is a tricky one. Write balanced equation (M2O + H2 2 M + H2O). Substitute x for the molar mass in all of your conversions, but use the same conversions as any other problem above. Convert from grams of metallic oxide to moles, then use molar ratios to convert to metal, then convert from moles to grams – all conversions should equal 1.054 grams, then solve for x.C – use molar ratios to convert oxygen gas to ironD – definition of limiting reagentC –limiting reagent problem, so follow steps. First convert both reactants all the way to grams of product – whichever one produced less is the limiting reagent and the maximum yield from the reaction.C – reaction has a 1:1 molar ratio, so you can use M1V1 = M2V2 hereA – solution stoichiometry. First multiply molarity by volume to get moles. Convert from moles to moles using molar ratio, then use molarity given and moles calculated to get the volume. Remember that molarity is equal to moles of solute / L of solution.C – gas stoichiometry. Trick here is that at STP, 1 mole of gas is equal to 22.4 L. Use this to convert L to moles, then use mole to mole ratios, then convert from moles to grams.A – determine which is the limiting reagent using steps in 22, then use the technique to find out how much excess is remaining from 18A – asking for the actual yield produced. Determine the theoretical yield by converting moles of ammonia to moles of product, then multiple by the percent yield.D – definitionB – calculate theoretical yield by converting antimony to grams to product. Remember that percent yield = actual/theoretical *100. A – same as 29States of Matter/SolutionsB – in phase diagrams like this, the section to the far left is solid, the section at the bottom is gas, and the section in the middle is liquid ALWAYS D – same as 1 B – molecular solids don’t conduct electricity and are soft, ionic solids conduct electricity, metals are hardBC – melting point is the same thing as freezing point. The colligative property that deals with this is freezing point DEPRESSION, so the temperature at this point decreases when the compound has more impurities or solute particles.B – partial pressures law. Multiply each pressure by the mole fraction, then add them together to get the total pressureB – a body-centered cube has a total of 2 atoms in it. Use dimensional analysis to convert these two atoms to grams of lithium. A – in a face centered cubic solid, the formula to calculate the radius is r = (2)1/2(edge length)/ 4. This is not a formula we talked about in lecture, but plug in the edge length and it should give you the radius of the atom in question. A – definitionD – point between a gas and a liquid is called the critical temperature, liquification occurs at bottom, so at lower temperaturesA – look at graphC – use PV = nRT to solve for moles, then divide grams by moles to get molar mass. Remember to make sure everything is in the right units first!C – gas deviates from ideal behavior at low temperatures and high pressures ALWAYSB – using combined gas law to solve for the final volume. Only trick is that you must subtract the vapor pressure of water from the original pressure since the gas was collected over water.C – most solute particlesB – molarity is moles of solute / L of solution. Convert grams to moles, then divide by volumeD – multiply molarity by volume to get moles, then convert to grams. Remember you always need to dissolve your solute and then dilute it.C – use M1V1 = M2V2D – use solubility guidelinesB – definition of supersaturated is when a solution prepared, then cooled and the solid stays in solution fitting more in the solution than should be possible based on the solubility.D – only answer choice that, according to the graph, will not dissolve in 100 g of waterA – remember that molality = mol of solute/kg of solvent. We are solving for kg of solvent. First convert grams to moles of solute, then divide moles of solute by the molality and you will be left will kg. B – the formula for mole fraction is X = mol of solute / mol of total solution. In this case, X = moles of water / moles of water + ethanol. There are 200 grams of total solution and 95% of that is ethanol, so the solution must be 190 g ethanol and 10 g water. Convert those to moles and plug into mole fraction expression.B – formula for freezing point depression is T = ikm. Calculate m by converting grams of ethanol to moles and dividing by kg of solvent (water) in the solution. Plug and chug to get change in temperature. C – use dimensional analysis here. Cube the edge value given to convert the units to cm3. Then use the density given to convert this value to grams. Since you know that the unit cell contains 2 atoms, then you can use Avagadro’s number to convert this 2 atoms into moles. To find the molar mass, divide the grams value by moles. B - definitionC D C – using PV = nRT, see that if both pressure and temperature are doubled, it will not change anything else since they are directly proportional. Final system should look exactly the same as initial system.D – 29.2 cm = 292 mmHg, then add the pressure in the manometer to the air pressure to get total pressure. Energetics B – using thermal equilibrium (heat that the metal lost is equal to heat that water gained, final temperature is the same for both). Expand heats to mcT and solve for missing variable.A – use q = mcT to solve for mass, then covert mass to volume using density givenD – not changing the specific heats or the reaction that is taking place will not change the temperature changeC – going up our phase diagram (from solid to gas) requires energy, while going down it releases energyA – dissolving something breaks bonds, which requires energy and enthalpy should increase at a semi-constant rateB – when using bond energies, add up all the bonds in the reactants and subtract all the bonds of the products. You’ll need to draw Lewis structures to see the number and types of bonds. REACTANTS – PRODUCTSD – steam to water requires a change in state of matter, which involves using the heat of condensation, vaporization, or fusionC –same as 6C – same as 6A – to calculate the heat released by a bomb calorimeter, use the formula: Q = CT (multiply the calorimeter constant and the change in temperature). Since we are asked for molar heat, you have to divide the heat released by the number of moles of ammonium nitrate in the system. B - definitionB – definitionB – when using heats of formation to calculate enthalpy, add up all the heats for the products multiplied by molar coefficients and subtract the reactants from that. PRODUCTS – REACTANTSA – exothermic released heat (negative), endothermic absorbs heats (positive) D – same as 13C – use Hess’ Law. Remember whatever changes you make to the reactions, you must also make to the heats before you add them together. C – same as 13D – Hess’ LawA – same as 13C – same as 13C – same as 13C – same as 13C – look for process that becomes more ordered (a decrease in disorder or entropy)B – solid to a gas skips 2 states of matter, so will have more of an entropy change than liquid to gas to solid to liquid. D – changes from liquid to solid increasing orderA – going from a liquid to gas, so entropy will be positive for sure. Heat needs to be added to get a liquid to condense, so enthalpy is positive also. D – use G = H – TS formula chartC – heat was removed so enthalpy is positive – there was more heat in the solution to begin with. Dissolution process always gives a positive entropy change.B – entropy should be positive since we are gaining moles of gas, use Gibbs free energy formula to predict the spontaneityC – for the reaction to drive in the same direction, enthalpy and entropy changes must have opposite signs (think of your Gibbs free energy formula) the only reaction where this is true is C, entropy is negative and enthalpy is positive.DynamicsD – since this is a bimolecular reaction, you can read the rate law straight off of the balanced equation. Both reactants are first order, so if you double each, the rate should increase by 4.C – must be first order in chlorine, since changing its concentration has the same effect on the rate. Doubling both increases rate by 8 – chlorine doubled the rate, so the other reactant must have quadrupled the rate, making it second order.A – write rates of appearance and disappearance expressions and set them equal to each other to solve for the disappearance of the O3B – activation energy is the difference between the reactants and the top of the hill. Heat of reaction is difference between reactants and products. C – add individual orders to get overall orderC – can use common sense and definition of half-life. Or use first order integrated rate law to solve for k. Then use t = .693/k formula to solve for the half-life.B – use common sense and definition of half-life. Or use t = .693/k to solve for k and then plug into integrated rate law (first order) to solve for time. A – definition/graphs of ordersB – initial rates method hold concentration of one reactant constant and observe how the other reactant has changed the rate. When [water] doubled, rate quadruples, so must be second order. When [CH3Cl] is doubled, rate doubles, so must be first order.B – same as 9D – A, B, and C have to do with kinetics (making a reaction faster or slower). D will not change the rate of the reaction but will only shift the direction of the reaction (equilibrium not kinetics)B – graph that plots a straight line corresponds to the order of the reaction.A – to calculate initial rate = change in concentration / change in time. Pick any two points on graph and plug into formula.D – definitionA – definition, reactions that have smaller activation energies will happen faster than those with higher energiesA – increasing temperature increases rate, increases temperature also increases K for endothermic reactions (Le Chatelier’s principle)D – definition, look at Boltzmann plots in book or lecture notesB – increases, but doesn’t depend on whether reaction is exothermic or endothermicA – rule about activation energies from #15 flip flops when two reactions are not at the same, constant temperatureA – definitionA – remember that the slow step determines rate if it is the first step, the rate law for the overall mechanism can be read straight off of the slow stepD – draw the potential energy diagram B – definitionC – definitionB – same as 9B – analyze the graph to see how much time it took for the partial pressure to decrease by halfC – same as 3D – definition, look for activation energy from reverse reactionA – definition, made in one step and consumed in the nextC – definition EquilibriumD – definition of equilibrium, rates of forward and reverse reactions are the sameC – K = products over reactants raised to their molar coefficients, omit solids and liquidsA – same as 2D – same as 2D – write K expression like 2, then plug and chug the values given for concentrationsA – same as 5D – cannot be used to predict how fast a reaction happens that is kinetics, not equilibriumD – definition C – temperature does change the equilibrium constant, and if the constant changes the concentrations must change as wellD – only temperature will change the equilibrium constantB – Le Chatelier’s principle decreasing pressure shifts to side with more moles of gasB – Le Chatelier’s principle adding products shifts to reactantsA – same as 12B – same as 12A – Le Chatelier’s principle increasing temperature for an endothermic reaction will shift reaction to make more productsB – same as 15D – same as 10B – same as 15D – set up ICE chart and plug into K expressionC – use Kw = [H3O+][OH-] to solve for the amount of hydronium in solution and then take the –log to solve for pH.A – definitionA – set up K expression for this salt and plug in its solubility for the concentrations of the ions B – same as 22 (“saturated” value is just giving you the value for its molar solubility)B – solve for Q using the concentrations given and compare it to K. The ions left over in solution are simply the ones that you have more of to start off with C – common ion effectC – set up ICE chart and plug in values for H+ and HA [A-] = [H+]. Plug these concentrations into K expression.B – same as 15D – remember that % ionization = [HA] change / [HA] initial. Use this formula to find change value. Set up ICE chart to find equilibrium values to plug into K expression. C – G = -RTlnK plug and chugA – Use equation from #29 to find K for this reaction at 298 K. Then use the derived Arrhenius equation to solve for the K at 1000 K. Then use equation from #29 again to solve for G at 1000 K. Electrochemistry and Redox A – assign oxidation numbers for each of the elements referenced. Remember rules for assigning them (oxygen is always -2 except in peroxide, hydrogen is always +1, anything in elemental state is 0, anything with a charge is just that number, all oxidation numbers must add up to charge on compound). D – same as 1B – same as 1C – transition metals fit this definition C – copper goes from +2 to 0 oxidation state gained electrons reduction is gain of electronsA – an oxidation process will require an oxidizing agents, so look for one that is oxidation (loss of electrons)A – zinc goes from 0 to +2 oxidation state, so it is oxidized which makes it the reducing agentC – lead is PbO2 goes from +4 to +2, which is reduction must be reducing agentD – definitionD – trick here is balancing electrons first. Mn half-reaction uses 5 electrons, while Fe half-reaction only uses 1 would need to multiply Fe by 5 to get those electrons balanced.B – same as 10 ALWAYS balance electrons first.D – reducing agents are more likely to be oxidized, so they have to be a product in these standardized reactions. Also, remember the higher the E value, the more likely the reaction proceeds as a reduction. Since we want something more likely oxidized, pick the lower E value. D – same reasoning as 12D – same as 12B – remember to find the total voltage, we add the voltage from each half-reaction together, but we have to flip the sign of one E value to make it an oxidation reaction. Flip the most negative one and add it to the most positive one to get the highest voltage.B – voltaic cell = positive E value flip the reaction that is most negative and add values togetherC – same as 16 except given balanced equation tells you which reaction to flipA – same as 16, except you are solving for one of the half-reaction potentials rather than the total voltageA – same as 18C – cathode is where reduction takes place, so this is where metal will be plated and mass will be gainedD – half-reaction for oxygen can be found lower down the table (more easily oxidized, less easily reduced) than fluorine remember fluorine is the most easily reduced and will never be oxidizedD – look at half-reactions to see products of this reaction A – use dimensional analysis. Some conversions to remember: current (A) = C/s; Faraday’s constant = 96,500 C/ mole of electron. B – same as 23C – same as 23D – higher molar mass = less moles of electrons transferred per gram less electricity neededB – same as 23B – plug and chug into Nernst equationA – B, C, and D are all wrong so use process of elimination C – Le Chatelier’s principle we want to increase value of E, so make the reaction go forward. Increasing the concentration of reactants will make the reaction go in the direction written. Descriptive Chemistry/PeriodicityA – uses the activity seriesB – always want a solvent that will be as similar as possible to the metal but not exactly the sameC – all other choices will create another molecule or ion when they are dissolved in water (ammonia will produce the ammonium ion, carbon dioxide will produce bicarbonate, hydrogen chloride will make the chloride ion) need one that will be collected in isolationA – like dissolves like, so looking for something polar like waterC – definition D – want to use something inert (unreactive) so balloon wont explodeD – all others are traits that transition metals have that you should know use process of eliminationC – lab experienceD – lab experienceA - definitionB – combustion reaction definitionD – definition, what makes up hard waterCD – remember elements will share characteristics with other elements in their period other elements in gallium’s period have a charge of +3, other elements in selenium’s period have a charge of -2B – needs a charge of +2 to form the oxideA – Y has a charge of +2, X has a charge of +4, so Z has a charge of -2 YZA – atomic radii trendA – atomic radii trendB – Z is effective nuclear charge, but that doesn’t really matter. Still use your atomic radii trendB – effective nuclear charge is the amount of pull the nucleus has on electrons increases with increasing positive chargeA – anions are largest, then neutral atoms, then cationsA – cations are smallest with highest chargeC – anions larger than neutral atomsA – atomic radii trend + anions are largerA – electronegativity trendB – electronegativity trendD – electronegativity trendB – ionization energy trendB – ionization energy trendB – huge jump in energy from 2nd to 3rd energy harder to ionize a third timeLaboratory Chemistry – omit 1, 10, 11, 13A – II would give you a higher percentage of water, I would cause you to lose more water and give a percentage that is too lowD – we are looking specifically for a problem with the use of a buret, the other answer choices have to do with other parts of the titration B – use M1V1 = M2V2 to solve for volume needed remember to add extra to dilute, don’t dump it all in at onceB – subtract the two and watch significant figures use the number in the value with the least amount, so two decimal places neededC – when measuring, we can extrapolate out one decimal place further than what can be seen on the instrument. This instrument reads to the tenths place, so we can report a value to the hundredths place.B – the more demarcations and smaller an instrument is, the more precise it isA – average the first three values, leave out the third one because it is an outlierA – accuracy is how close the reported numbers are to the actual value (given as 1.0000) and precision is how close the reported numbers are to each otherC – A, C, and D will all work but C provides the most detailed procedureB – ammonia is basic and will turn litmus paper blueD – reaction took carbon dioxide out of solution. Carbon dioxide has acidic properties, so must be a base in the solution for it to react with. C – graph shows us we need 2 moles of base for every one mole of acid B – chlorine needs to oxidize something else. Br- Br2 is an oxidation reaction. A would mean that chlorine was oxidized, which is wrong. C is not an experiment. D has nothing to do with redox reactions. C- purple indicates a positive displacement reaction has occurred D D – must have strontium since it forms a white precipitate with acid. Must have magnesium or calcium as well since there was no reaction with dichromate. Barium reacted with dichromate, so it can’t be present. C – safety rulesB – use wider tongsD – ALWAYS add acid to water, not the other way around otherwise reaction will combustD – danger sign, look in safety rules ................
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