5 Steps to a 5 AP Chemistry (2010-2011 Edition)

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Look at the following descriptions, and see which best describes you.


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This will help you pick a prep mode. You are the kind of person who likes to plan for everything very far in advance. You arrive very early for appointments. You like detailed planning and everything in its place. You feel that you must be thoroughly prepared. You hate surprises. If you fit this profile, consider Plan A.

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You are always on time for appointments. You are willing to plan ahead to feel comfortable in stressful situations, but are OK with skipping some details. You feel more comfortable when you know what to expect, but a surprise or two is good. If you fit this profile, consider Plan B. You get to appointments at the last second. You work best under pressure and tight deadlines.

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You feel very confident with the skills and background you learned in your AP Chemistry class. You decided late in the year to take the exam. You like surprises. If you fit this profile, consider Plan C. Look now at the following calendars for plans A, B, and C. Choose the plan that will best suit your particular learning style and timeline. For best results, choose a plan and stick wish it.

Table 2. However, this book is capable of filling other roles. It can broaden your study of Chemistry, help your analytical skills, and aid you scientific writing abilities. These will aid you in a college course in Chemistry.

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Use this plan to organize your study during the coming school year. You should highlight material that applies specifically to you. Reviewing the topics covered in this section will be part of your year-long preparation. You need to get some idea of the layout, and break it in. Highlight important points.

You may wish to retake part of the Diagnostic Exam. MARCH 30 weeks have now elapsed.

Thank you!

Read and study Chapter 15, Equilibrium. Read and study Chapter 16, Electrochemistry. Review Chapters 5— Review the appropriate chapters to correct any weaknesses. Take Practice Exam 2. Score your exam. Fall asleep knowing you are well prepared. This calendar begins in mid-year, and prepares you for the mid-May exam. MARCH 10 weeks to go. The best use of this book for you is as a specific guide towards the AP Chemistry exam. There are time constraints to this approach, as the exam is only a short time away.

This is not the best time to try to learn new material. Fall asleep knowing that you are well prepared. Skim Chapters 1—4. Go over Chapter 5. Skim Chapters 6—9. Carefully go over the Rapid Review sections of Chapters 5—9. It will let you know where you need to spend the majority of your study time. Do not make the mistake of studying only those parts you missed; you should always review all topics. It may be to your advantage to take the diagnostic exam again just before you begin your final review for the exam. This exam has only multiple-choice questions. It will give you an idea of where you stand with your chemistry preparation.

The questions have been written to approximate the coverage of material that you will see on the AP exams and are similar to the review questions that you will see at the end of each chapter. Once you are done with the exam, check your work against the given answers, which also indicate where you can find the corresponding material in the book. We also provide you with a way to convert your score to a rough AP score.

It is not important whether you get the correct answers. If you have a problem with one or more questions from a chapter, review the chapter. You may use a calculator and the periodic table. For each question, circle the letter of your choice. Chapter 5 1. In most of its compounds, this element exists as a monatomic cation.

Which of the following groups has the species correctly listed in order of decreasing radius? Which of the following elements has the lowest electronegativity? Which of the following represents the correct formula for hexaamminecobalt III nitrate? The discovery that atoms have small, dense nuclei is credited to which of the following? Choose the strongest Lewis acid from the following. This ion will form a precipitate when added to a sodium sulfate solution. This ion gives a deep blue color when excess aqueous ammonia is added to a solution containing it.

Aqueous solutions of this ion give a reddish precipitate when excess hydroxide ion is added. Which of the following best represents the net ionic equation for the reaction of calcium hydroxide with an aqueous sodium carbonate solution? A student mixes A green precipitate forms, and the concentration of the hydroxide ion becomes very small. Which of the following correctly places the concentrations of the remaining ions in order of decreasing concentration? What volume of hydrogen gas, at standard temperature and pressure, is produced from 0.

What is the concentration of the iron solution if it takes Manganese, Mn, forms a number of oxides. A particular oxide is What is the simplest formula for this oxide? A sample of chlorine gas is placed in a container at constant pressure. The sample is heated until the absolute temperature is doubled.

This will also double which of the following? A B C D E potential energy moles density number of molecules volume A balloon contains 2. A second balloon contains 4.

trigtenlade.tk Both balloons are at the same temperature and pressure. Pick the false statement from the following list. A The number of hydrogen molecules is the same as the number of helium atoms in each balloon. B The density of the helium in its balloon is greater than the density of the hydrogen in its balloon. C The volume of each balloon is the same. Determine Your Test Readiness The volume and pressure of a real gas are not the same as those calculated from the ideal gas equation, because the ideal gas equation does NOT take into account: A the attraction between the molecules and the speed at which the molecules are moving B the volume of the molecules and the mass of the molecules C the attraction between the molecules and the mass of the molecules D the volume of the molecules and variations in the absolute temperature E the volume of the molecules and the attraction between the molecules Aluminum metal reacts with HCl to produce aluminum chloride and hydrogen gas.

What volume of hydrogen gas, at STP, is produced when A sample containing the gases carbon dioxide, carbon monoxide, and water vapor was analyzed and found to contain 4. The mixture had a total pressure of 1.

5 Steps to a 5 AP Chemistry, 2010 2011 Edition 5 Steps to a 5 on the Advanced Placement Examinations

What was the partial pressure of the carbon monoxide? An ideal gas sample weighing 0. Determine the molar mass of the gas. A B C D E free energy lattice energy kinetic energy activation energy ionization energy The energy required to produce a gaseous cation from a gaseous atom in the ground state The maximum energy available for useful work from a spontaneous reaction The energy required to completely separate the ions from a solid is Choose the reaction expected to have the greatest increase in entropy.

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A certain reaction is nonspontaneous under standard conditions, but becomes spontaneous at lower temperatures. What conclusions may be drawn under standard conditions? The exact position of an electron is not known. Nitrogen atoms, in their ground state, are paramagnetic.

An atomic orbital can hold no more than two electrons. The 4s orbital fills before the 3d.