AP Chemistry Information and Summer assignment
Overview of Course Expectations:
AP Chemistry is a college level course. Students can earn up to 8 hours college credit for successful completion of this course and a good score on the AP Exam. It is a time-consuming and challenging, yet extremely rewarding, course. This course moves at a very fast pace and classroom attendance is a MUST.
Students will be prepared to do college level work of any type upon completion of this course due to the thought processes used and the discipline/work habits required.
The course covers two semesters of college chemistry. We will complete many hours of lab work. To have success on the AP exam, students will need to spend on average five to ten additional hours per week outside of class working on AP chemistry. This time will be spent on homework assignments, pre-labs, lab reports, problem sets, etc. There will be times that students will be able to complete things during class if they use their time efficiently. These statements are not meant to discourage, but to point out and state the truth to avoid any misconceptions about the high expectations for this course. I will do my very best to provide a college level course/experience which not only prepares you for the AP exam, but provides a solid foundation in chemistry. I also intend for it to be fun!!
You are fortunate to be able to take this type of college level course in the high school setting as part of a small class.
Attached to this letter, you will find a list of things that you will need to review, memorize, and/or practice prior to school starting. The majority of the material required in this assignment is review material that students should have learned in their first year chemistry class. Some parts of the summer assignment are meant to stretch students' thinking and resourcefulness. (This means look it up if you don’t know it off the top of your head as you have so many resources available to you!) Students should not panic if they didn’t learn it in their first year – it is easily mastered.
Because this is a challenging problem-solving course, and for some of you, a year may have passed since you have had a chemistry course, it is imperative that you come to class the first day with some of the nomenclature, etc. second nature for you due to the pace at which this course progresses. Reviewing and committing to memory the topics in this summer assignment is not optional and completing the assignment in a thorough and focused manner will contribute to a student’s success in this course and on the AP Chemistry exam.
I look forward to getting to know each of you! We will have fun and we will work hard. Students will receive a detailed course syllabus when school resumes in the fall. AP Chemistry Required Materials and Summer Assignment
I. Required Materials for the AP Chemistry Course You will be provided with a digital textbook and a physical one if you want it.
Along with the internet resource for the textbook, students should also add the following sites to their internet favorites: http://www.khanacademy.org/#Chemistry http://www.brightstorm.com/science/chemistry
Other supplies for this course:
A sturdy three ring binder Pencils, pens, highlighters, etc. Scientific calculator
A great attitude and sense of humor. You will need it at times! Plan on forming study groups!
Please remember the following: To graduate from college, a student needs:
1) To understand learning is a continuous and uneven process 2) To understand that vocabulary and basic knowledge of the subject is the essential starting point. 3) To overcome the lack of immediate success (temporary failure). 4) To study and apply varying techniques: comparing and contrasting analysis and interpretation induction and deduction questioning skills problem solving skills rote memorization Part II. Summer Assignment The summer assignment consists of two parts –
Part A is the material you must have memorized by the first day of school.
Part B is practice with nomenclature, balancing equations, oxidation numbers, solubility rules, and practicing problem solving.
Summer Assignment - Part A– Material to be memorized by the 1st Day of School. NOTE: There will be quizzes during the first two weeks of school covering the topics in this assignment!! Memorization of material is not something that will be encouraged or emphasized in this course because this is a problem-solving course and it is impossible to memorize everything you will be asked to do. However, memorization of some topics/rules is necessary.
Master the memorization material listed in this assignment! DO whatever it takes to commit this information to memory for instant recall. Make flashcards, bingo games, etc. Have your friends and family quiz you, form study groups, etc. Again, this information needs to be second nature to you to ensure your success in this course.
I will be checking these assignments the first day of class to verify you have completed them so that you get off to a good start in this class. Topic/ Subject matter Where do I find it?
Specified element names and symbols Periodic table Element symbols 1 to 38 and Ag, Cd, I , Xe, Cs, Ba, W, Hg, Pb, Sn, Rn, Fr, U, Th, Pu, and Am written correctly. You should be able to locate these elements quickly because the periodic table provided on the exam does not include element names.
Monatomic ions (and ones with multiple oxidation states listed in this packet
Polyatomic ions and corresponding acids listed in this packet (If you master a system for naming acids, you do not have to memorize them- only the ions!)
6 Strong acids CBSPIN hydroChloric acid (HCl) hydroBromic acid (HBr)
Sulfuric acid (H2SO4) Perchloric acid (HClO4) hydroIodic acid (HI)
Nitric acid (HNO3) Strong bases Group 1 metal hydroxides (NaOH, KOH etc)
Group 2 metal hydroxides (Ba(OH)2, Sr(OH)2 Ca(OH)2, these are only slightly soluble- others are insoluble
Solubility rules listed in this packet
Colors of common ions listed in this packet Common Ions Ions Usually with One Oxidation State
Li+ Lithium ion N3- nitride
Na+ Sodium ion O2- oxide
K+ Potassium ion S2- sulfide
Mg2+ Magnesium ion F- fluoride
Ca2+ Calcium ion Cl- chloride
Sr2+ Strontium ion Br- bromide
Ba2+ Barium ion I- iodide
Ag+ Silver ion
Zn2+ Zinc ion
Cd2+ Cadmium ion
Al3+ Aluminum ion
Cations with more than One Oxidation State
+1 +2
Cu1+ Copper (I) or cuprous ion Cu2+ Copper (II) or cupric ion
Hg2+ Mercury (I) or mercurous ion Hg2+ Mercury (II) or mercuric on
+2 +3
Fe3+ Iron (II) or ferrous ion Fe3+ Iron (III) or ferric ion
Cr2+ Chromium (II) or chromous ion Cr3+ Chromium (III) or chromic ion
Mn2+ Manganese (II) or manganous ion Mn3+ Manganese (III) or manganic ion
Co2+ Cobalt (II) or cobaltous ion Co3+ Cobalt (III) or cobaltic ion
+2 +4
Sn2+ Tin (II) or stannous ion Sn4+ Tin (IV) or stannic ion
Pb2+ Lead (II) or plumbous ion Sn4+ Lead (IV) or plumbic ion Polyatomic Ions and Acids
Formula Name Ion Ion Name
2- H2SO4 Sulfuric acid SO4 sulfate
2- H2SO3 Sulfurous acid SO3 sulfite
- HNO3 Nitric acid NO3 nitrate
- HNO2 Nitrous acid NO2 nitrite
3- H3PO4 Phosphoric acid PO4 phosphate
2- H2CO3 Carbonic acid CO3 carbonate
- HMnO4 Permanganic acid MnO4 permanganate
HCN Hydrocyanic acid CN- cyanide ion
HOCN Cyanic acid OCN- cyanate ion
HSCN Thiocyanic acid SCN- thiocyanate ion
- HC2H3O2 Acetic acid C2H3O2 acetate ion
2- H2C2O4 Oxalic acid C2O4 oxalate ion
2- H2CrO4 Chromic acid CrO4 chromate ion
2- H2Cr2O7 Dichromic acid Cr2O7 dichromate ion
2- H2SrO5 Thiosulfuric acid SrO5 thiosulfate ion
3- H3AsO4 Arsenic ion AsO4 arsenate ion
3- H3AsO5 Arsenous acid AsO5 arsenite ion
Oxyhalogen acids
Formula Oxy name Ion Ion Name
HClO Hypochlorous acid ClO1- Hypochlorite ion
1- HClO2 Chlorous acid ClO2 Chlorite ion
1- HClO3 Chloric acid ClO3 Chlorate ion
1- HClO4 Perchloric acid ClO4 Perchlorate ion
Br, I, can be substituted for Cl. F may form hypoflourous acid and the hypofluorite ion Other ions
2- O2 peroxide ion
OH1- hydroxide ion
2- HSO4 Bisulfate ion or hydrogen sulfate ion
+ NH4 Ammonium ion
- O2 Superoxide ion
- HCO3 Bicarbonate ion or hydrogen carbonate ion
2- HPO4 Hydrogen phosphate ion
- H2PO4 Dihydrogen phosphate ion
Colors of common Ions in Aqueous Solutions
Most common ions are colorless in solution, however, some have distinctive colors. THese colors have appeared in questions on the AP exam
Fe2+ and Fe3+ Various colors
Cu2+ Blue to green
Cr2+ blue
Cr3+ Green or violet
Mn2+ Faint pink
Ni2+ green
Co2+ pink
2- MnO4 Dark purple
2- CrO4 yellow
2- Cr2O7 orange Organic functional groups: Be able to recognize the functional groups and the naming system associated with it
Summer Assignment Part B: Practice with Nomenclature, Balancing Equations, Oxidation Numbers, Solubility Rules and Problem Solving
Nomenclature: Simple Inorganic Formulas and Nomenclature – Complete Exercise 1 in the Appendix of this packet. Review the naming rules and commit the naming prefixes to memory!
Oxidation Numbers: Oxidation Numbers: Anions and Cations – Complete Exercise 2 in the Appendix of this packet. Review/Memorize the Rules for Oxidation Numbers
More Nomenclature: Ternary Nomenclature: Acids and Salts - Complete Exercise 3 in the Appendix of this packet.
Balancing Equations – Balancing Molecular Equations - Complete Exercise 4 in the Appendix of this packet.
Reaction Types and Reaction Prediction - Predict the products, write the equation and then balance, etc. – Complete Exercise 5 in the Appendix of this packet.
Solubility Rules – Using Solubility Rules Table – you must memorize these! –Complete Exercise 6 in the Appendix of this packet using the solubility rules listed in Part A of the summer assignment. Compare these rules to the ones in the reference packet for Honors Chemistry!!
Review Problem Sets – Complete the problems on attached Review Problem Sets – show your work and clearly mark your final answers!! Use correct significant figures for math answers and units where needed! Appendix
Exercises for Part B of the Summer Assignment
Nomenclature Review Forming binary ionic compounds A. In a binary ionic compound the total positive charges must equal the total negative charges. The best way to write correct formula units for ionic compounds is to use the “Criss Cross Method”. B. Sample problem: What ionic compound would form when calcium ions combine with bromide ions?
Steps to the Criss Cross Method: 1. Write the ions with their charges, cations are always first. Ca2+ Br1- 2. Cross over the charges by using the absolute value of each ion’s charge as the subscript for the other ion. Ca1 Br2 3. Check to make sure the subscripts are in the lowest whole number ratio possible. Then write the formula. CaBr2
Naming binary ionic compounds A. Combine the names of the cation and the anion.
B. Example: BaBr2 is named barium bromide. C. First write the ions formed for the following elements. Then use the Criss Cross method to determine the formula. Then name the compounds.
Naming binary ionic compounds that contain polyatomic ions A. The polyatomic ions on your common ions list should be memorized. B. The most common oxyanions – polyatomic anions that contain oxygen, end in –ate. Oxyanions with one less oxygen end in –ite. For example: -1 2- NO3 is nitrate SO4 is sulfate -1 2- NO2 is nitrite SO3 is sulfite
C. Anions with one less oxygen than the –ite ion are given the prefix hypo-. D. Anions with one more oxygen than the –ate ion are given the prefix per-. -1 -1 ClO is hypochlorite ClO3 is chlorate -1 -1 ClO2 is chlorite ClO4 is perchlorate
E. Naming compounds with polyatomics is the same as naming other compounds, just name the cation and then the anion. If there is a transition metal involved, be sure to check the charges to identify which ion (+1, +2, +3, +4….) it may be so that you can put the correct Roman numeral in the name. Name the following. Polyatomic ions ending with “ate”
3- 2- - BO3 CO3 NO3 O F
4- 4- 4- - SiO4 PO4 SO4 ClO3
3- 2- - AsO4 SeO4 BrO3
2- - TeO4 IO3
** The outside ions all have 3 oxygens
** The inside ions all have 4 oxygens
** Period 2 ions start with a -3 charge then increase by +1 from left to right
** Period 3-5 ions are the same charge as their “parent” ion Nomenclature- the language of chemistry
There are 5 different naming systems in general chemistry. The key to figuring out which one to use is to look at the 1st element!!!!
The element farthest left on the periodic table will ALWAYS be written first
Ionic compounds: METAL + Non-metal (cation and anion)
How to write the formulas How to name the compound
Binary compounds (only 2 elements) Binary Compounds (Only 2 elements) + + ***Exception is NH4 **Exception is NH4 ● Write the symbol and the oxidation ● Name the cation (+ ion) number for each element. The cation ● Use the root of the anion (- ion) will be first ● Change the ending to ___ide ● Cross the value of the oxidation ● If there is a transition metal, place the number but not the sign to the other charge of the metal as roman element. numerals after the cation name. ● Transition metals charge will be indicated by roman numerals in the name ● Reduce the subscript if possible. +1 -2 Ex. Na + S → Na2S Ca+2 + O-2 → CaO
Ternary compounds (anion is polyatomic) Ternary compounds (anion is polyatomic) ● Write the symbol and the oxidation ● Name the cation number for each element. ● Name the anion. DO NOT change the ● Cross the value of the oxidation ending number but not the sign to the other ● If there is a transition metal, place the element/ polyatomic ion charge of the metal as roman ● If there is an additional subscript on numerals after the cation name. the polyatomic ion you MUST put the ion in parenthesis. ● Transition metals charge will be indicated by roman numerals in the name ● Reduce the subscript if possible. +2 -3 Ex. Ca + PO4 → Ca3(PO4)2 Molecular compounds: Non-metal + Non-metal
Prefix’s
1 Mono
2 Di
3 Tri
4 Tetra
5 Penta
6 Hexa
7 Hepta
8 Octa
9 Nona
10 deca
How to write the molecular compound How to name molecular compounds
All will be Binary (only two elements) All will be Binary (only two elements) ● Use the prefix’s given in the name as ● Name the 1st element using the prefix the subscript for each element. to indicate the number of atoms ● DO NOT REDUCE ● ****Do not use Mono for 1st element ● Do not worry about the oxidation ● Name the 2nd element using a prefix numbers to indicate the number of atoms
Ex. diphosphorous pentoxide: P2O5 Acids: (H+ + Anion)
How to write the formulas How to name the compound (*** Always name acids using the anion)
Binary acids (hydrogen + monatomic ion) Binary acids (hydrogen + monatomic ion) ● Write hydrogen first ● Use the prefix hydro ● Write the anion from the periodic ● Use the root name of the anion table ● Add a suffix ___ic ● Whatever the oxidation number is for ● Add the name acid
the anion will be the subscript Ex. H2S: hydrosulfic acid (number of) for hydrogen + -2 Ex. H + S → H2S
Ternary acids (H+ + Polyatomic ion) Ternary acids (H+ + Polyatomic ion) ● Write hydrogen first ● If the anion suffix is ___ate: Use the ● Write the polyatomic anion root and change the suffix to ____ic ● Whatever the oxidation number is for acid
the anion will be the subscript Ex. H2SO4: hydrogen and sulfate= sulfuric (number of) for hydrogen acid + -2 Ex. H + SO4 → H2SO4 ● If the suffix ends in ___ite: Use the root and change the suffix to ___ous acid
Ex. H2SO3 : hydrogen and sulfite = sulfurous acid
Hydrates (Metal + non-metal with water attached)
Ionic compound● H2O
How to write the formulas How to name the compound
● Follow the rules of ionic compound ● Name as an ionic compound ● Write a ● symbol after ● Use the molecular compound prefix ● Use the prefix stated in front of system as the prefix before hydrate hydrate as the coefficient for water.
Ex. MgSO4 ● 7H2O = magnesium sulfate hepta hydrate Organic compounds (CxHy…) Simplest are alkane’s (CnH2n+2)
Name is determined by the number of carbon atoms Prefix’s 1 meth 2 eth 3 prop 4 but 5 pent 6 hex 7 hept 8 oct 9 non 10 dec
How to write the formulas of alkanes How to name the compound
● Use the prefix for the number of ● Identify how many carbon atoms are carbon atoms present and use the prefix ● Multiply the carbon atom number by 2 ● Add the suffix ____ ane and add 2 for the number of hydrogen **** If an additional functional group is atoms present the suffix will change
Ex. C3H8 : propane Exercise 1: Nomenclature: Simple binary formulas and nomenclature
In the first column, classify each as a molecular or ionic compound. Then name the compound:
Formula M Name Formul M or I a or I
NaCl Mg3N2
SrO CCl4
K2S AzAt2
CO2 PCl5
Al2Se3 Na2S
N2O5 FeCl3
Exercise 2: In the first column, write the chemical formula, and in the second wrote the name of the formula,
Elements Chemical formula Name
Magnesium and iodine
Potassium and sulfur
Zinc and bromine
Chlorine and aluminum
Strontium and oxygen
Calcium and nitrogen
Calcium and oxygen
Copper (I) and oxygen
Copper (II) and chlorine
Mercury (II) and oxygen Rules for Assigning Oxidation Numbers
1. The convention is that the cation is written first in a formula, followed by the anion. For example, in NaH, the H is H-; in HCl, the H is H+. 2. The oxidation number of a free element is always 0. The atoms in He and N2, for example, have oxidation numbers of 0. 3. The oxidation number of a monatomic ion equals the charge of the ion. For example, the oxidation number of Na+ is +1; the oxidation number of N3- is -3. 4. The usual oxidation number of hydrogen is +1. The oxidation number of hydrogen is -1 in compounds containing elements that are less electronegative than hydrogen, as in CaH2. 5. The oxidation number of oxygen in compounds is usually -2. Exceptions include OF2 because F is more electronegative than O, and BaO2, due to the structure of the peroxide ion, which is [O-O]2-. 6. The oxidation number of a Group IA element in a compound is +1. 7. The oxidation number of a Group IIA element in a compound is +2. 8. The oxidation number of a Group VIIA element in a compound is -1, except when that element is combined with one having a higher electronegativity. The oxidation number of Cl is -1 in HCl, but the oxidation number of Cl is +1 in HOCl. 9. The sum of the oxidation numbers of all of the atoms in a neutral compound is 0. 10. The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion. For example, the sum of the oxidation numbers for SO42- is -2.
Determine the oxidation number for each of the underlined atoms:
K2S S8 C60 NaClO4
Mg ZrO2 BrCl K2W4O15
K2Cr2O7 Li2CO3 Mg(BF4)2 OF2
Au2O3 Ce2TeF3 NO2 FeS2 Mixed NOMENCLATURE Practice Molecular Compounds, Ionic Compounds, & Acids
NAME THE FOLLOWING COMPOUNDS:
1. BaSO3 2. (NH4)3PO4
3. PBr5 4. MgSO4
5. CaO 6. H3PO4
7. Na2Cr2O7 8. MgO
9. SO3 10. Cu(NO3)2
11. HI 12. N2O
13. MnO 14. AgNO3
15. As2O5 16. Fe2O3
17. HClO 18. N2O3
19. HF 20. H2C2O4
21. NaHCO3 22. SiBr4
23. CuCl2 24. HNO2
25. SnO2 26. BaCrO4
WRITE FORMULAS FOR THE FOLLOWING COMPOUNDS:
27. hydrobromic acid 28. chromium(III) carbonate
29. magnesium sulfide 30. iodine trichloride
31. lithium hydride 32. ammonium hydroxide
33. calcium chloride 34. hydroselenic acid
35. iron(II) nitride 36. aluminum hydroxide
37. tin(II) fluoride 38. sulfur tetrachloride
39. mercury(II) iodide 40. diphosphorus pentoxide
41. sulfurous acid 42. lead(II) nitrate
43. dihydrogen monoxide 44. sodium oxalate Practice with Acids:
____ic from _____ate ____ous from _____ite Hydro___ic from _____ide
Complete the following table
Name of acid Formula of acid Name of anion
hydrochloric HCl chloride
Sulfuric acid H2SO4 sulfate
HI
sulfite
Chlorous acid
nitrate
HC2H3O2 or CH3COOH
Hydrobromic acid
sulfide
HNO2
Chromic acid
phosphate Balancing Equations: Practice Problems 1. Balance each of the following equations.
(a) Fe+ Cl2 → FeCl3
(b) Fe+ O2 → Fe2O3
(c) FeBr3 + H2SO4 → Fe2(SO4)3 + HBr
(d) C4H6O3 + H2O→ C2H4O2
(e) C2H4 + O2 → CO2 + H2O
(f) C4H10O+ O2 → CO2 + H2O
(g) C7H16 + O2 → CO2 + H2O
(h) H2SiCl2 + H2O→ H8Si4O4 + HCl
(i) HSiCl3 + H2O → H10Si10O15 + HCl
(j) C7H9 + HNO3→ C7H6 (NO2)3 + H2O
(k) C5H8O2 + NaH+ HCl → C5H12O2 + NaCl
Predict the products for the reactions:
Combustion:
1. C4H9OH + oxygen →
2. C7H14 + oxygen →
Synthesis:
1. Sodium + oxygen → 2. Calcium + nitrogen → 3. Potassium + bromine →
Decomposition
1. Strontium carbonate → 2. Mercury (II) oxide → 3. Aluminum chlorate → Double replacement
1. Iron (III) sulfate + calcium hydroxide → 2. Sodium hydroxide + sulfuric acid → 3. Sodium sulfide + manganese (VI) acetate → 4. Chromium (III)bromide + sodium sulfite → 5. Barium hydroxide + chlorous acid →
Single replacement
1. Nickle + steam → 2. Chlorine + aluminum iodide → 3. Potassium + water → 4. Lead + copper (II) chloride → 5. Zinc + hydrochloric acid →
Predict the products and write the complete net ionic equations:
Include the molecular equation, complete ionic equation, and the net ionic equation
1. Iron (III) sulfate + calcium hydroxide → 2. Sodium hydroxide + sulfuric acid → 3. Calcium nitrate + lithium phosphate → 4. Chlorine gas + aluminum iodate (aq) 5. Potassium metal + water → 6. Zinc metal + hydrochloric acid (aq) → Solubility rules: For the compounds, write the formula for each compound then indicate if it is soluble (aq) or insoluble (i). Include the reason why for solubility.
Name Formula (aq) or (i)
Silver nitrate AgNO3 (aq)- nitrate
Cobalt (II) sulfate
Zinc hydroxide
Iron (III) iodide
Nickel (II) chloride
Lead (II) iodide
Sodium carbonate
Barium sulfate
Lead (II) sulfide
Silver phosphate
Lithium phosphate
Nickel (II) carbonate
Copper (II) hydroxide
Tin (IV) sulfate
Lead (IV) nitrate
Density: Complete the following calculation:
1. Calculate the mass of a sample of copper that occupies 5.3 x 10-2 cm3 if the density of copper is 8,4 g/cm3
2. A 9.46 g sample of a solid is placed in a 25.00 mL flask. THe remaining volume in the flask is filled with benzene in which the slid is insoluble THe solid and the benzene together weigh 26.83 g. The density of benzene is 0.879 g/mL. What is the density of the solid? Atomic Theory: The atomic number is the same as the number of protons, the electrons for a neutral atom will be the same as the protons. If the symbol has a charge then it is an ion. Add or subtract electrons accordingly. To find the number of neutrons subtract the atomic number from the atomic mass.
Element/ ion # protons # neutrons # electrons
Fe
Na+
27 25
S2-
Cr3+