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Download ACS General Chemistry Study Guide Book in PDF, Epub and Kindle Test Prep Books' ACS General Chemistry Study Guide: Test Prep and Practice Test Questions for the American Chemical Society General Chemistry Exam [Includes Detailed Answer Explanations] Made by Test Prep Books experts for test takers trying to achieve a great score on the ACS General Chemistry exam Foreword You have in your hand the second edition of Preparingfor Your A CS Examination in General Chemistry, The Official Guide designed to help students prepare for examinations Details: ACS Study Guide - Free download as Word Doc .doc), PDF File .pdf), Text File .txt) or read online for free. Scribd is the world's largest social reading and publishing site. Open Download Free Acs Exam General Chemistry Study Guide Pdf Free Copy Ace General Chemistry I ACS General Chemistry Study Guide Study Guide General Chemistry The ACS Physical Chemistry Study Guide Pdf Free Download is a great book in terms of content and structure. It is written by some of the best authors in the field and updated regularly with ... read more

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Skip to main content. Acs General Chemistry Study Guide Free Home Acs general chemistry study guide free Listing Websites about Acs General Chemistry Study Guide Free Filter Type: All Education Study Learning. ACS General Chemistry Practice Test - mometrix. com Study Details: Exam Outline Overview. Equimolar amounts of nitrogen, hydrogen, and argon are placed in a reaction chamber. The amount of which substance s will determine the amount of ammonia produced in the reaction below if the reaction goes to completion? How many total molecules will be present when the reaction of 5, molecules of CS2 with 15, molecules of 0 2 goes to completion? What amount of the excess reagent remains when 0. What amount of Ab03 is produced from the reaction of3. The combustion ofC3H 80 with 02 is represented by this equation. Consider this reaction for the production of lead. What amount of excess reagent remains when 4.

Which representation shows what would be present after the reaction is complete? D C 8 55 Molar mass I g·mol- 1 Pb c Answers to Practice Questions-~~--~~ ~--~ l. B 56 Chapter 5- Solutions and Aqueous Reactions, Part 1 Chapter Summary: This chapter will focus on substances in solutions including qualitative and quantitative properties of solutions and reactions of substances in solution. Used in uestions related to Reactions, solution properties Where to find this in your textbook: The material in this chapter typically aligns to "Aqueous Reactions" in your textbook.

How this fits into the big picture: The material in this chapter aligns to the Big Idea oflntermolecular Interactions 4 and Reactions 5 as listed on page 12 of this study guide. Which compound is a weak electrolyte when dissolved in water? B KOH D NaN Knowledge Required: 1 Definition of an electrolyte. weak electrolyte. Thinking it Through: The definition of an electrolyte is a substance or solution that will conduct electricity. For this question, the solutes are all dissolved in water. You also know the reason the solutions conduct electricity is that the substance or solute produces ions when dissolved in water, creating an electrolytic solution. A strong electrolyte will dissociate or ionize completely in water while a weak electrolyte will only partially ionize in water. Considering the responses therefore, you are looking for a substance that would be classified as a weak acid or base as these substances would partially ionize in water.

Ammonia or NH 3 is a weak base, and therefore is a weak electrolyte. Nitric acid, HN03, is a strong acid and therefore a strong electrolyte, so choice A is incorrect. Potassium hydroxide, KOH, is a strong base and also a strong electrolyte, so choice B is incorrect. Potassium hydroxide is also ionic as is sodium nitrate, NaN0 3 or choice D. Ionic compounds when in solution are present as ions, so are strong electrolytes making choice D incorrect as well. Practice Questions Related to This: PQ-1 SQ What mass in g ofmagnesium nitrate, Mg N0 3 2, are required to produce Thinking it Through: The first thing you recognize when reading this question is that you are given a volume You know that "M" or molar concentration is:. mol solute 0. Then, given the volume, this allows you to determine the number of moles of solute Mg N03 2 : 0.

Choice A is not correct because the molar mass was not used this is the number of moles. Choice B is not correct because Choice C is not correct because the wrong molar mass was used for MgN03, not Mg N03 2. Na2S03 A O. Thinking it Through: Similar to SQ-2 previously, you will use the molar concentration and volume of the solution given in the problem to determine number of moles. Here, you are going to pay special attention to the substance:. I L solutiOn From here, if you used the molar mass ofNa2S0 3, you would determine the mass of sodium sulfite needed to make this solution, which is not what the question is asking. Choice C is the mass of sodium sulfite, Na2S0 3. Choice D uses the correct mole ratio but the wrong molar mass. Practice Questions Related to This: PQ-6 and PQ-7 SQ As water is being added to a concentrated NaOH solution ,. Thinking it Through: You start this question by evaluating the balanced equation for reactants and products.

s ~ ~ product Choice A omits the excess calcium ions. Choice C focuses on the other reactant counting the largest number of ions in solution the nitrate ions. Choice D represents all ions in solution and does not account for the product in solution or the spectator ions. Practice Questions Related to This: PQ, PQ, and PQ SQ Which reaction will result in a precipitate? Thinking it Through: You recall the criteria for a precipitation reaction to occur: I both reactants must be in solution and 2 at least one product must be insoluble or the precipitate. The choices show that the reactants are all soluble as noted by the "aq".

Thinking it Through: You start this problem by first determining the molecular equation. soluble soluble insoluble The next step will be to determine the total ionic equation. Choice B is the molecular equation and choice D is the total ionic equation. Use the standard enthalpies of formation in the table to calculate for this reaction. Calculate the enthalpy of combustion of ethylene, C2H4, at 25 atmosphere of pressure. Use the given heats of formation to calculate the enthalpy change for this reaction. Using the given thermochemical data, what is the! What is the! What is the enthalpy of formation ofhydrazine, N 2H4 1? ww· Exams~~~~~~- PQ What is the standard enthalpy change for this reaction? B Answers to Practice Questions l. A 80 Chapter 7- Structure and Bonding Chapter Summary: This chapter will focus on concepts related to chemical bonding. This includes both ionic and covalent bonding extending into bonding theories and applications.

Although this chapter is traditionally included in firstterm chemistry, the concepts in this chapter are critical to your understanding of other concepts throughout general chemistry. Used in questions related to Structures, formal charge, resonance, bond enthalpy, shape, polarity, valence bond theory Valence bond theory, molecular orbital theory Atomic orbitals Molecular orbital diagrams Molecular orbital theory ,,. Choice ~ was incorrectly determined by not considering the carbon-carbon bond neither breaking the double bond nor n aking the single bond. A longer and stronger B longer and weaker C shorter and stronger D shorter and weaker Knowledge Required: 1 Understanding of covalent bonds. Thinking it Through: You could approach this by knowing facts about bonds, but you also know that you can approach this by considering a single versus a double bond in the context of valence bond theory.

What is not immediately obvi us from this is that double bonds are shorter than single bonds and stronger bonds are typically shorter or ch tee C. uestions Related to This: PQ and PQ What is the molecular geometry of C0 ? B A bent C trigonal bipyramidal Thinking it Through: The first thing you notice when you read this is that you are going to need to determ shape, and the next thing you notice is that this is for an ion. Earlier, you walked through the process to de the Lewis dot structure for a molecule, now you will walk through this with an ion including using formal to "place" the charges. Following this, bond all of the terminal atoms t o the central atom with sin le bonds. rmine harge viii Structure and Bonding.. Next, complete the octets of each atom by adding lone pairs of electrons. For en h oxygen atom, you will add three lone pairs and for carbon, you will add one.

Now, you count the number of electrons shown in your structure so far. Forth ; one, you now have 26 which is more than You can add the doubl1 bond between carbon and any oxygen. Then you will again complete the octets for all atoms. The form1' charges you determine will be the charges on the ion here a net of -2, so for this io t, there are two atoms with a negative one formal charge. You start this by evaluating the central atom in simple molecules or ions 1 :atom of focus in more complex molecules or ions and asking yourself how many atoms are bonded to the cf: tral atom and how many lone pairs are on the central atom. You recall that it is not the type ofbonding between :o: the at1 ns, but only the number that matters so no difference for the three oxygen atom!

Because there are no lone pairs o: on th1: ~entral atom, this is also the shape of the ion. Drawn more consistently with this shape ,nd bond angle shown to the right which is choice D. Choice A may be selected if the formula were read incorrectly. II uestions Related to This: PQ and PQ SQ Which species contains a bond angle less than °? of lone of electron Molecule or ion of bonded atoms ~airs grou~s [:·1·-. When a molecule or ion has one or more lone pairs on the central atom, it can change the bond ar. There are exceptions to this including the linear ion shown here and square planar molecules. Considering the results of your evaluation above, you see choice D is correct. A C02 B so2 C D Knowledge Required: 1 Lewis dot structures. Thinking it Through: You know to determine polarity you need to start with the Lewis dot structure. Now, you add the bond moment arrows to each structure, placing these on all bonds between aton ; of different elements.

From here you can see that 0 2 or choice C does not contain polar bonds, so this is not correct. F r m here you can evaluate the molecular polarity of the remaining three choices. However, because l1e two polar bonds in C02 cancel, the electron density distribution remains even, and C02 is nonpolar. The correc1 ::hoice A. Practice uestions Related to This: PQ, PQ and PQ 88 ~.. Think· 'lg it Through: As you notice from the question, you need to determine hybridization. To do this, there are anum er of steps you will follow: 1. Draw the Lewis dot structure already provided to you in the question 2. Evaluate the t es of bonds made b eted atom: C1 C2 makes 1 sin le bond and 1 tri makes 4 sin le bonds 3.

Evaluate the bonds made in terms of overlap of atomic orbitals or hybrid atomic orbitals you also know 1 single bond is often 1 a bond, 1 double bond is often 1 a bond and 1 n bond, and 1 triple bond is 1 a bond and 2 n bonds : CI C2 makes 4 a bonds makes 2 a bonds and 2 n bonds c onsi'der the nee 4 or 1yt n atomic orb. Structure and Bonding ACS Exams - - - - - - - - - - H How many sigma cr and pi n bonds are in one molecule of benzoic acid? Thinking it Through: As discussed in the previous study question, you know that a single bond is often I i gma bond, a double bond is often I sigma and I pi bond, and a triple bond is 1 sigma bond and 2 pi bonds.

c~ Number of bonds: 11 single bonds II sigma bonds , Choice A omits the sigma bonds from the double bonds. Choice B counts the double bonds as 2 pi bonds rather than I sigma and I pi bond. Choice D counts the doubl bonds as 2 sigma and I pi bond. Thinking it Through: You start this question by interpreting the molecular orbital diagram: anti bonding molecular orbital. The electrons fill these orbitals based on the Au· 1au principle or lowest to highest energy noted in the diagraJ Choice A reflect:; :he electrons; choice B omits the antibonding electrons; and choice C omits the one-half Practi. Practice Questions PQ I {'. Arrange CsBr, NaCI, and RbBr in increasing magnitude oflattice energy. Which ionic compound has the largest magnitude lattice energy? Which statement best describes ionic bonding in lithium fluoride?

What is the formal charge on the phosphorous atom in the phosphate ion as shown? Which molecule contains carbon with a negative fonnal charge? How many valence electrons are in the carbonate ion, C0 ? Which is the best Lewis structure for nitrogen monoxide? The best Lewis structure ofN2H2 shows A a nitrogen-nitrogen triple bond. B a nitrogen-nitrogen single bond. C each nitrogen with one nonbonding electron pair. D each nitrogen with two nonbonding electron pairs. W~~t is the corr. e9" GO.. I : F: PQ The resonance structures for benzene indicate that the H H I I H' B benzene molecule exists as two unique structures. C benzene molecule alternates between forms I and II. H C I H D carbon-carbon single bonds are longer than the double bonds. e9" H' C I H II PQ What is the bond order of the C-0 bond in the acetate ion? The Lewis dot structure of ethanol is given below.

Estimate the enthalpy of combustion of ethanol C2H 5 0H using the bond enthalpies in the table. e~~ c,o~ For the nitrate ion, N0 3-, predict the bond energy between nitrogen and the oxygen labeled "A". A kJ-mol- 1 o:; D kJ·mol- C III B II.. H C--N--N--CH 3 3 II. C kJ·mol- 1 B klmol- 1 PQ Which molecule has the strongest nitrogen-nitrogen bond? Bond entha! Ethinyl estradiol EE is widely used in oral contraceptive pills. Which arrow points to the shortest carbon-carbon bond in EE? H PQ What is the molecular geometry around theN atom in the molecule depicted? H 0 I I II H-N--C--CH I H A t-shaped B tetrahedral C trigonal planar D trigonal pyramidal PQ A central atom has two lone pairs and three single bonds. What is the molecular geometry?

A T-shaped B tetrahedral C trigonal planar D trigonal pyramidal PQ According to VSEPR, what are the approximate values of the bond angles X andY? Which molecule has a ° bond angle? C IF3 B NH3 A C02 IC. What are the polarities of the indicated molecules? Which molecule is polar? What is the hybridization of the indicated nitrogen atoms? What is the hybridization on the central atom in the molecule GeC]z? A sp PQ How many a and 11 H bonds are shown? I~'~ A 5 Structure and Bonding ···Exams PQ How many a and n bonds are in the molecule shown? According to MO theory, F2 would. B have a bond order of 1 and be paramagnetic. C have a bond order of 2 and be diamagnetic. D have a bond order of 2 and be paramagnetic. Using the MO diagram given to the right, what is c.

o~'efl the bond order for [N2t? J ~ D Answers to Practice Questions l. Chapter Summary: This chapter will focus on concepts related to gases including single gases, mixtures of gases and kinetic molecular theory. Additionally, this chapter includes concepts related to liquids and solids such as intermolecular forces and phase diagrams. The names of your chapters may vary. How this fits into the big picture: The material in this chapter aligns to the Big Idea oflntermolecular Forces 4 as listed on page 12 of this study guide. A gas behaves most ideally at A high pressures and low temperatures.

B high pressures and high temperatures. C low pressures and low temperatures. D low pressures and high temperatures. Knowledge Required: I Ideal gas properties. Thinking it Through: You know you need to consider properties of ideal gases. One ofthe primary properties of an ideal gas is that there are no attractions between particles, and all interactions between particles are totally elastic. You know that these attractions are minimized by maintaning a sufficiently high temperature, which keeps the average energy of the particles sufficiently high.

Coordinating with this you also know that ideal gases are assumed to have no volume. Therefore, to minimize the volume of the gas particles, the number of gas particles is sufficiently low bymaintaining either a low pressure or low density. Therefore, combining these, a gas behaves most ideally at low pressures and high temperatures or choice D. All other combinations are incorrect. Finally, you also know that "sufficiently" high temperature or "sufficiently" low pressure or density varies depending on the gas. For a noble gas, this could be relatively low temperature and high pressure which would not be true for a heavier gas.

For most gases the ideal gas law will be adequate at or near conditions of Standard Temperature and Pressure STP. These conditions are 0 oc and 1 bar ~Iatm of pressure. Practice Questions Related to This: PQ-1 and PQ-2 SQ What is the density of Xe gas at 70 A 1. Thinking it Through: You start this problem by defining density, which you know is mass per volume or g·L- 1. As you read the problem, you notice that you are not given either the mass or the volume of the gas. However, you also know that density is an intensive property, so you can use any sample size. Two logical sample sizes would be either 1. You do the question first with 1. You now have temperature 70°C or K , pressure 2. C acuatmgt I I · h edens1ty: · · h mce · C. IC h ISC Choice D is incorrectly determined by 70 oc rather K. Practice uestions Related to This: PQ-3, PQ-4, PQ-5, and PQ-6 98 '"··A C S States of Matter ~~~~. What is the final temperature of the gas? Thinking it Through: The first thing you notice for this question is that you have one ideal gas in two conditions.

Choice D 2 is the temperature in kelvin. uestions Related to This: PQ-7 and PQ-8 What volume ofC0 2 g , measured at 0. Thinking it Through: You start this problem by considering what you are given: a mass Secondly, what you need to find is the volume of the other reactant COz. So, your approach will be: mass of Al uscmolarma"iS nAI O; uscthcmolratio nco'2 uscP. T VCO Choice C is incorrectly determined by omitting the mole ratio of 1 mol Ab03 to 3 mol COz. Choice B uses 28 "C rather than K and Choice A uses 28 "C as well as omits the mole ratio. If the diagram shown is representative of B B has the largest partial pressure. C C has the largest partial pressure. D All partial pressures are equal. Thinking it Through: For this question, you see that you first are going to interpret the particulate diagram. For this problem, there are 4 particles of A g , 5 particles of B g and 3 particles of C g which you can equate to number of moles so 4 mol A g , 5 mol B g and 3 mol C g.

Then you realize that you need to determine which gas has the highest partial pressure. Partial pressure is defined as the pressure an ideal gas would exert if it occupied the container alone. Therefore, the greatest number of moles corresponds to the largest partial pressure or gas B , which is choice B. Choices A and C correspond to selecting smaller number of moles of gas possibly inverting Avogadro's law. Choice D would be true only ifthere were equivalent number of particles of all gases. Finally, it is important to remember that it is either the number of moles of particles or number of particles which can be atomic gases like what is shown in the figure or molecules such as N2 or CH4. Which are the correct label for curves I-IV? The reaction between acetone and bromine Exp IM M in acidic solution is represented by the equation: I 0.

What is the rate law for the reaction? B -fi. Doubling the concentration of both reactants increases the rate of reaction by a factor of eight. The reaction is A first order in both NO and Cb. B first order on NO and second order in Cb. C second order in NO and first order inCh. D second order in both NO and Cb. A PQ The activity of a radioisotope is counts per minute at one time and counts per minute 48 hours later. What is the half-life, in hours, of the radioisotope? After 55 years, what mass in g remains of a time PQ If you are looking for a guide, I highly recommend this one! you can also download other ACS Physical Chemistry Study Guide PDF book on this same book site. All you need in one place with easy access and no cost attached. What more could you ask for? ACS Physical Chemistry Study Guide Pdf Free Download is a great guide book for students to better understand the chemistry behind physical chemistry.

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What is the fommla ofhydroiodic acid? Page Chapter 10 - Kinetics Choice D has a charge, but it is the wrong charge should be III not II. The correc1 ::hoice A. C low pressures and low temperatures. You know that these attractions are minimized by maintaning a sufficiently high temperature, which keeps the average energy of the particles sufficiently high. How many atoms are in 1.

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