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AP Chemistry Summer Work 2016
You will need to obtain your textbook before summer break!
Chemistry, 9
th
edition, Raymond Chang
*****NOTE: There is no need to print any portion of this packet.*****
Part I: Memorization
AP Chemistry can be a difficult course. It is not all about memorization, but there are some things you simply must memorize. It is essential for success in learning the concepts covered in this course. It is to your advantage to memorize the material in this packet well before the first day of school and review it often. As I am sure you know, true learning (and retention) will come only from reviewing material regularly, as opposed to cramming. You will be quizzed on this material within the first full week of the school year, so plan ahead in order to be successful! Make flashcards, have friends and family quiz you, take this packet with you on vacation, or do whatever else it takes to get this information firmly planted in your head! Spending a mere five to ten minutes each day looking this over will be far more effective in the long run than attempting to cram the night before the quiz. DO NOT PROCRASTINATE!!! The topics of memorization are listed below, and the details are covered throughout this packet. Also, you may find much of this material outlined in your Honors Chemistry / first year course notes. If you still have them lying around somewhere dig them out and look them over. They will also be a valuable reference tool throughout the year.
- Solubility rules
- Rules for determining oxidation numbers
- Polyatomic ions (name, charge, symbol)
- Rules for naming ionic compounds
- Variable valences (charges) and colors for transition metal ions in solution
- Rules for naming acids, and the seven strong acids
- Element symbols and naturally occurring forms
- Units and conversions
- Common lab equipment (name - spelled correctly- and function)
Solubility Rules
- All compounds containing alkali metal cations and the ammonium ion are soluble.
All compounds containing NO 3
, ClO 4 - , ClO 3 - , HCO 3 - and C 2 H 3 O 2 - anions are **soluble**.
- All chlorides, bromides and iodides are soluble EXCEPT those containing Ag
- All sulfates are soluble EXCEPT those containing Ag+, Pb2+, Hg2+, Sr2+, Ca2+, or Ba2+.
- All hydroxides are insoluble EXCEPT compounds of the alkali metals, NH 4
- , Sr 2+ , or Ba 2+ . Ca 2+ is temperature dependent.
- All compounds containing PO 43 - , S^2 - , CO 32 -^ and SO 32 -^ ions are insoluble EXCEPT compounds of the alkali metals or NH 4 +. These are generalizations. We will learn later in the year that many compounds are slightly soluble, which will complicate things slightly. However, memorizing these generalizations now is essential for topics covered early in the year, and it will make our study of solubility later in the year easier.
Rules for determining Oxidation Number
Oxidation Number: A number assigned to an atom in a molecular compound or molecular ion that indicates the distribution of electrons among the bonded atoms.
- In free elements (including diatomic ones) each atom has an oxidation number of zero.
- For monatomic ions the oxidation number is equal to the charge of the ion.
- The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion.
- Fluorine has an oxidation number of – 1 in ALL of its compounds. Other halogens have negative oxidation numbers when they occur as halide ions in their compounds, but when combined with oxygen they have positive oxidation numbers.
- The oxidation number of oxygen is – 2 unless it is combined with fluorine (when it is +2) or in peroxides (when it is – 1).
- The oxidation number of hydrogen is +1 except when bonded to metals in binary compounds. In such cases its oxidation number is – 1.
- In compounds, the elements of groups one and two as well as aluminum have oxidation numbers of +1, +2, and +3 respectively.
- In a neutral molecule the sum of all the oxidation numbers must be zero.
- In a polyatomic ion the sum of all of the oxidation numbers in the ion must equal the net charge of the ion.
- Oxidation numbers do not have to be integers, though they typically are. (Ex: In O 2
- each O has an oxidation number of – 1/2.)
Variable Valences for Transition Metals
Name Symbol Charge Stock Name Chromium Cr +
Chromium (II) Chromium (III) Manganese Mn +
Manganese (II) Manganese (III) Iron Fe +
Iron (II) Iron (III) Cobalt Co +
Cobalt (II) Cobalt (III) Copper Cu +
Copper (I) Copper (II) Lead Pb +
Lead (II) Lead (IV) Mercury Hg +
Mercury (I) Mercury (II) Tin Sn +
Tin (II) Tin (IV) Gold Au +
Gold (I) Gold (III) Silver Ag + +2 (rare) Silver (I) Silver (II) Bismuth Bi +
Bismuth (III) Bismuth (V) Antimony Sb +
Antimony (III) Antimony (V) Cadmium Cd +2 Cadmium Zinc Zn +2 Zinc
Common Ion Colors in Aqueous Solution
Ion Color Ion Color
Cu
2+
Blue-green Fe
2+
Light blue-green
Cr
2+
Blue Fe
3+
Yellow-brown
Co
2+
Pink Ni
2+
Green
Mn
2+
Faint pink CrO 4
2 -
Yellow
MnO 4
Dark purple Cr 2 O 7
2 -
Orange
Rules for Naming an Acid
- When the name of the anion ends in – ide, the acid name begins with the prefix hydro- and the stem of the anion has the suffix – ic. This is followed by the word acid. Pattern: hydro _____ ic acid Examples: HCl = hydrochloric acid HCN = hydrocyanic acid
- When the name of the anion ends in – ite, the acid name is the stem of the anion with the suffix – ous. This is followed by the word acid. Pattern: _____ ous acid Example: HNO 2 = nitrous acid
- When the name of the anion ends in – ate, the acid name is the stem of the anion with the suffix – ic. This is followed by the word acid. Pattern: _____ ic acid Example: HNO 3 = nitric acid
Strong Acids
Hydrochloric acid Hydrobromic acid Hydroiodic acid Perchloric acid Chloric acid Nitric acid Sulfuric acid *A few others are debatable, but these are certain.
Common Elements and Symbols:
See page 12 (Table 1.1) of Chang textbook The periodic table used in AP Chemistry does not include element names, only symbols!
Diatomic Molecules: H, O, F, Br, I, N, Cl
These seven elements exist as diatomic molecules in their natural state, while phosphorus exists as P 4. Memorize them!
SI Units and Conversions:
See pages 16-17 (Tables 1.2-1.3) of Chang textbook
Common Lab Equipment:
Attached to the end of this document
AP Chemistry Unit I Text Assignments
Not all of this is summer work, only the reading assignments with embedded practice exercises. However, if you are comfortable with the material and wish to complete some of the end-of- chapter problems you will be ahead when school begins. That is up to you. Chapter 1 - Chemistry: The Study of Change § Read, take notes, and complete all practice exercises § Focus on vocabulary and tables § Make note of Tables 1.1, 1.2 1. § Know how to do temp conversions (use 2 decimal places with K) and density calculations § Practice scientific notation and rules for sig figs Additional resources: Honors Chemistry Unit I End of chapter problems: (10) 12, 16, 22, 26, 30, 32, 36, 52, 54, 62 Chapter 2 - Atoms, Molecules, and Ions § Read, take notes, and complete all practice exercises § Focus on vocabulary and figures § Make note of Figures 2.3- 2 .8 and 2. § Know all components of the atomic theory and contributions of named scientists § Know all information about subatomic particles § Know rules for naming all types of compounds Additional resources: Honors Chemistry Units II and III There are more detailed chapters coming on topics such as the periodic table; do not feel the need to go above and beyond what you find in this particular chapter at this time. End of chapter problems: (12) 16, 26, 36, 46, 50, 58, 60, 62, 66, 68, 72, 76 Chapter 3 - Mass Relationships in Chemical Reactions § Read, take notes, and complete all practice exercises § Focus on vocabulary and mass calculations/terms § Focus on spectrometry, as it is relatively new to you and will be used in lab § Know how to calculate percent composition and empirical formulas § Know how to balance equations § Know how to utilize mole ratios in various applications § Know how to calculate and utilize limiting reagents § Know how to calculate percent yield and percent error Additional resources: Honors Chemistry Unit V End of chapter problems: (24) SHOW YOUR WORK FOR ALL CALCULATIONS! 1, 4, 9, 10, 14, 16, 18, 20, 22, 30, 32, 34 42, 50, 57, 60, 66, 74, 78, 86, 90, 100, 110, 112
Chapter 24 - Organic Chemistry Organic chemistry is merely glossed over on the AP exam. It is not worth taking tremendous class time to cover this material, as the payoff on the exam will be minimal. On the 2002 exam, for example, there were no questions directly involving organic chemistry. However, there are usually a few questions that mention organic compounds by name. It might be beneficial if you actually knew what those compounds were. § Read, take notes, and complete all practice exercises § Focus on nomenclature and functional groups, but read all Additional resources: Honors Chemistry Unit III End of chapter problems: (9) 1, 3, 14, 26 (omit d), 32, 36, 42, 58, 60 Optional: While the end-of-chapter problems are included along with the information about each chapter, they are not required as part of the summer assignment. If you feel confident with the material and want to get ahead, feel free to start them. Answers to end of chapter problems numbered in red are in the back of the book. Check your answers when you finish and redo those that are incorrect. If you get stuck, try working backwards from the answer given. You will gain far more from going through this process than you will from asking someone to present the solution to you, and it will save valuable class time when we are going over homework. Also, I am not assigning Chapter 24 as part of the summer assignment. However, you can expect to have this reading assigned within the first few days of school. So, if you want to do more work over the summer so that you have less work during the first week, then read this chapter.
