AP CHEMISTRY SUMMER ASSIGNMENT - Ms....
30
Transcript of AP CHEMISTRY SUMMER ASSIGNMENT - Ms....
Future AP Chemistry Student,
Welcome to AP Chemistry! I am eagerly anticipating a great year of Chemistry. In order to ensure the best start for everyone next fall, I have prepared a summer assignment that reviews basic chemistry concepts. There is a multitude of tremendous chemistry resources are available via the Internet. With the ready access to hundreds of websites either in your home or at the local library, I am confident that you will have sufficient resources to prepare adequately for the fall semester. There are chemistry textbooks which can be picked up for your reference.
For those students who have already taken a high school chemistry course, much of the material in the summer packet will be familiar to you. For those students who will be taking AP Chemistry as your first high school chemistry course, the problems will help you build a foundation in chemistry and insure all students are on a relatively even plane. It will be important for everyone to come to class the first day prepared. While I review, extensive remediation is not an option as we work towards our goal of being 100% prepared for the AP Exam in early May 2018. There will be a test covering the basic concepts included in the summer packet during the first week of school. You can expect a quiz on the periodic table the first day of school. Make sure just completing assignment should not be the only objective but one should be confident enough to process the material for application during the school year. The sooner one realizes the easier the transition to the class.
The course grades are mainly depending on your assessment scores, although lab reports will also be assigned and evaluated. Assessments are administered and graded as if they are AP exams. Be aggressive in pursuit of knowledge not just the grades. Prioritize your learning process, do not procrastinate until the last minute, get help in class and at NEST, participate in class discussions and seek support before grades sink below one’s expectations.
You may contact me by email: ([email protected]) this summer. I will do my best to answer your questions ASAP. I hope you are looking forward to an exciting year of chemistry. You are all certainly fine students, and with plenty of motivation and hard work you should find AP Chemistry a successful and rewarding experience.Finally, I recommend that you spread out the summer assignment. Please do not try to complete it all in the final week of the summer. Chemistry takes time to process and grasp at a level necessary for success in AP Chemistry. Remember, AP Chemistry is an equivalent course to Introductory Chemistry in college. Taking a college level course in high school is difficult, requires dedication, and is a great investment in your education so prepare yourself and arrive ready to learn.
Have a great summer and enjoy learning chemistry.
Ms. Callahan
Required materials: 1. A 3 Ring Binder: 1 Inch, with Pockets – Any Color2. A Package of Lined Notebook Paper with 3-Holes3. Pencils, Erasers, and BLACK Pens4. A Set of Highlighters – 4 Different Colors 5. TI 30XII-S Calculator (Standard)6. Pocket Folder7. Set of Dry Erase Markers – 4 Different Colors8. Composition Notebook college rule or graph (not a spiral notebook)
AP Chemistry Summer Assignment
If you don’t have a user id for College Board, create one and explore website for the course. The website is: http://student.collegeboard.org/
Familiar yourself with the two pdf docments on site: AP Chemistry Course Overview AP Chemistry Course and Exam Description
Complete a laboratory safety contract, including student & parent signatures.If you have NOT passed a safety exam for me, then you will need to do so within the first week of school during your own time safety exam will be on the website.
Complete Worksheet 1 & 2 Due first day of school (last pages of the packet) Memorize the names of the elements and their corresponding symbols (quiz day
1) Memorize ions (polyatomic ion quiz 1st week) Memorize solubility rules Review concepts at the end of this packet Advised to watch crashcourse chemistry or similar video series to review on a
regular basis
Please have both completed forms (student id and safety contract) with you on first day of school.
Have a greatSummer!
Memorize
Task 1: Memorize the names of the elements and their corresponding symbols
You need to know elements 1-56, plus Pt, Au, Hg, Pb, Rn, Fr, Ra, U, Pu Many of these elements you will already know Making flashcards is helpful! It’s important to know these elements because the periodic table you are
provided has only the symbols and not the names of the elements. All metals are solid except for mercury which is a liquid. All metalloids are solids. Nonmetals: carbon, phosphorus, sulfur, & selenium are solids; bromine is a liquid;
and the rest are gases. Elements with Subscripts: Br2, I2, N2, Cl2, H2, O2, F2, P4, S8
Task 2: Memorize the ionic charges of the basic ions
Think about the valance electrons! Think about the common elements/ions in that group
- All metals are solid except for mercury which is a liquid.
- All metalloids are solids.
- Nonmetals: carbon, phosphorus, sulfur, & selenium are solids; bromine is a liquid; and the rest are gases.
- Elements with Subscripts: Br2, I2, N2, Cl2, H2, O2, F2, P4, S8
Common Monatomic Ions
Metals with Multiple Oxidation States
Element Symbol Oxidation # Old System New System
Iron Fe +2 Ferrous Iron (II)+3 Ferric Iron (III)
Copper Cu +1 Cuprous Copper (I)+2 Cupric Copper (II)
Mercury Hg2 +2 Mercurous Mercury (I)Hg +2 Mercuric Mercury (II)
Lead Pb +2 Plumbous Lead (II)+4 Plumbic Lead (IV)
Tin Sn +2 Stannous Tin (II)+4 Stannic Tin (IV)
Task 3: Memorize the names, symbols, and charges of Polyatomic ions below:
Oxyanions – polyatomics containing oxygen, names end in –ate or –ite -ate is used for the most common form -ite is used for the form with the same charge, but one less oxygen
o Example: NO3- = nitrate NO2- = nitrite
Prefixes are also usedo Per- indicates one more oxygen than the –ate form (think “perfect =
overachieving”, ie = more)o Hypo- indicates one fewer oxygen than the –ite formo Example:
ClO4- = perchlorate (b/c it has one more O than the –ate form) ClO3- = chlorate (b/c it is the most common) ClO2- = chlorite (b/c it has one less oxygen than – ate form) ClO4- = hypochlorite (b/c it has one less oxygen than the –ite form)
o F, Cl, Br, I all behave the same Therefore, if chlorate is ClO3-, the bromate ion is… BrO3-!!!! Simply substitute one halogen for the other If you learn the chlorate series, you also automatically know the bromate, iodate, and fluorate series
Hydrogen can be added to -2 or -3 ions to make a “new ion” i.e. H2PO4 –1 is dihydrogen phosphate (note the – charge went up 1 for each H+ added)
+1 ammonium, NH4+
-1 -2 -3acetate, C2H3O2-, or CH3COO - carbonate, CO3 -2 phosphate, PO4 -3bromate, BrO3- chromate, CrO4 -2 phosphite, PO3 -3
chlorate, ClO3- dichromate, Cr2O7 -2Borate, BO33-
arsenate, AsO4 -3chlorite, ClO2- oxalate, C2O4 -2cyanide, CN- peroxide, O2 -2
Hypobromite, BrO-
hydrogen carbonate, HCO3-Silicate, SiO32-
sulfate, SO4 -2
(also called bicarbonate)sulfite, SO3 -2
hydroxide, OH-
hypochlorite, ClO-
iodate, IO3-
nitrate, NO3-
nitrite, NO2-
permanganate, MnO4-
perchlorate, ClO4-
thiocyanate, SCN -
Be able to name polyatomic ions using the rules above such as these below:HPO4-2 ________________________ HSO3-1 ________________________
FO3-1 ________________________ HCO3-1 ________________________
Be able to write formulas for polyatomic ions using the rules above such as these below:
Bromite __________________ periodate _________________
Dihydrogen phosphite _____________hydrogen chromate __________
Task 4: Memorize the solubility rules:
You will need to memorize the solubility rules! Start memorizing over the summer!
Part 1, Naming----------------------A) Metal- NonMetalThese compounds may be either ionic or covalent depending on the electronegativity of M and X. The metal of NH4
+ is always written first. These compounds are commonly referred to as salts.
General form = MyXz
Where M = any metal ion or ammonium ion, NH4+
X= any non metal element and OH- or CN-
y and z represent small integers
Steps in naming binary metal – nonmental compounds Use the full name of the metal, M, or ammonium if M is NH4
+
Follow metal name with a Roman numeral if (), to indicate the metal’s oxidation state (charge). This step is omitted if the metal has only one common oxidation state (see periodic chart)
Write the stem of the nonmetal’s name and add the suffix “-ide” to the stem of the nonmetal
Examples: NaCl = sodium chloride Fe2O3 = Iron (III) oxide Ag3N = silver nitride
Chemical Formulas helpful websites: http://www.wise.k12.va.us/jjk/Chemistry/formula.htmhttp://www.phs.princeton.k12.oh.us/departments/Science/ldusch/honorspdfs/namingchpt5/Flowcharts.pdf
B) NonMetal- NonMetalThese compounds are always covalently bonded. They are commonly referred to as covalent or molecular compounds. The least electronegative element (see periodic table) is usually written first.
General form= QyXz
Where Q= any nonmetal and X=a different nonmetal y and z are small integers
Steps in naming binary covalent compounds: Write the numerical prefix for y (unless it is one then no numerical prefix is used) Add the full name of the nonmetal Q Write the numerical prefix of z (unless it is one then no numerical prefix is used) Add the stem of the name for the second nonmetal, X, adding “-ide” at the end of the stem If the first element is hydrogen, no numerical prefixes are needed.
Most commonly used numerical prefixes:1=mono, 2=di, 3=tri, 4=tetra, 5=penta, 6=hexa, 7=hepta, 8=octa, 9=nono, 10=deca
Examples: ICl = iodine chloride ICl3 = iodine trichloride N2O4 = dinitrogen tetraoxide
C) Cation (Metal of NH4+) – polyatomic ions
Please note: From this point on, it is very important that you have memorized the correct name, formula, and charge for all the polyatomic ions listed at the end of this document.
General Form- cation written first, anion written second
D) Naming AcidsWhen the name of the anion ends in –ide, the acid name begins with the prefix hydro-, the stem of the anion has the suffix –ic and it is followed by the word acid.
-ide becomes hydro _____ic AcidExample: Cl- is the Chloride ion so HCl = hydrochloric acid
When the anion name ends in –ite, the acid name is the stem of the anion with the suffix –ous, followed by the word acid.
-ite becomes ______ous AcidExample: ClO2
- is the Chlorite ion so HClO2 = Chlorous acid.
When the anion name ends in –ate, the acid name is the stem of the anion with the suffix –ic, followed by the word acid.
-ate becomes ______ic AcidExample: ClO3
- is the Chlorate ion so HClO3 = Chloric acid.
**You will also need to learn which acids and bases are strong (CBSPIN) and which are weak.
A simple way to remember acids: all binary acids, except HF are strong.Oxyacids (contain polyatomic ions) are strong if there are two or more oxygen atoms than hydrogen atoms: H2SO4 = strongH2SO3 = weakPart 2, Determining Oxidation Numbers----------------------Rules for Determining Oxidation Number (this may be the one thing you did not learn in regular chemistry, but it’s very similar to charges, so it should be easy for you)
Oxidation Number: A number assigned to an atom in a molecular compound or molecular ion that indicates the general distribution of electrons among the bonded atoms. (these are a lot like charges, except they are assigned to covalent compounds in addition to ionic compounds. They just indicate the relative attractions for electrons.
5. The oxidation number of any uncombined or unbonded element is zero (0).6. The oxidation number of a monatomic ion is equal to the charge on the ion.7. The more electronegative element in a binary compound is assigned the number equal to the charge it
would have if it were an ion.8. The oxidation number of fluorine in a compound is always –19. Oxygen has an oxidation number of –2 unless it is combined with F, when it is +2, or it is in a
peroxide, when it is –1.10. The oxidation state of hydrogen in most of its compounds is +1 unless it combined with a metal, in
which case it is –1.11. In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation number of +1,
+2, and +3, respectively12. The sum of the oxidation numbers of all atoms in a neutral compound is zero (0).13. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the ion.
Part 3, Identifying Types of Reactions----------------------
Synthesis:Metal oxide + water metal hydroxide MgO + H2O Mg(OH)2Nonmetal oxide + water acid (polyatomic) CO2 + H2O H2CO3Metal + oxygen → metal oxide 2Mg(s) + O2(g) → 2MgO(s)Nonmetal + oxygen → nonmetallic oxide C(s) + O2(g) → CO2 (g)Metal + nonmetal → salt 2 Na(s) + Cl2 (g) → 2NaCl(s)
A few nonmetals combine with each other. 2P(s) + 3 Cl2 (g) → 2PCl3(g)
Decomposition:Metal carbonate metal oxide + carbon dioxide Cs2CO3 Cs2O + CO2Metal hydroxide metal oxide + water 2LiOH Li2O + H2OMetal chlorate metal chloride + oxygen gas 2LiClO3 2LiCl + 3O2Some acids, when heated, decompose into nonmetallic oxides and water.
H2SO4 → H2O(l) + SO3 (g)Some oxides, when heated, decompose. 2HgO(s) → 2Hg(l) + O2 (g)Some decomposition reactions are produced by electricity. 2H2O(l) → 2H2(g) + O2 (g) and
Acid/Base Reactions2NaCl(l) → 2Na(s) + Cl2(g)
acid + base salt + water H2SO4 + NaOH Na2SO4 + H2Ometal + acid salt + hydrogen gas 3Mg + 2H3PO4 Mg3(PO4)2 + 3H2metal oxide + acid salt + water CaO + HCl CaCl2 + H2Ocarbonate + acid salt + carbon dioxide + water BaCO3 + H2SO4 BaSO4 +CO2 + H2O
(The carbonate ion breaks apart. The other negative ion becomes part of the salt)nonmetal oxide + hydroxide salt + water CO2 + Ba(OH)2 BaCO3 + H2O
metal oxide + nonmetal oxide salt Na2O + SO3 Na2SO4
Part 4, Stoichiometry----------------------Helpful websites:http://www.chemtutor.com/mols.htmhttp://www.chem.tamu.edu/class/majors/tutorialnotefiles/limiting.htmhttp://www.ausetute.com.au/idealgas.html
Rules10. Always start with a balanced equation11. Write what you know underneath the chemical that is known (5.23grams)12. Place a question mark (?) underneath what you are looking for.13. Use dimensional analysis to convert to the chemical you are trying to find information about. Note that
you will most likely need to use the mole-mole ratio (also called the stoichiometric ratio) to convert from one chemical to another.
Limiting Reactant ProblemsRules2. Convert all reactants to moles3. Divide by the coefficient in the balanced equation4. The chemical with the lowest number of moles is the limiting reactant (LR)5. Use the LR for all further calculations
Percent Yield1. Balanced Equation2. Write amount given under the reactant that has a value3. You will be given an amount of product (write this under the product) this is the actual amount produced4. Convert given reactant amount to same product (and units) that was given
Percent Error
Name:Date:
AP Chemistry Summer Assignment
Worksheet #1 – Math SkillsSignificant Figures (Sig Figs)
1. How many sig figs are in the following numbers?
a) 0.0450 ____________
b) 790 ____________
c) 32.10 ____________
2. Solve the following problems. Round your answer to the correct number of sig figs (and use
the correct unit on your answer).a) 825 cm x 32 cm x 0.248 cm _____________________b) 15.68 g
2.885 mL _____________________
Density (round your answers to correct number of sig figs and show all work with units)
3. A cube of ruthenium metal 1.5 cm on a side has a mass of 42.0 g. What is the density in g/cm3? Will ruthenium metal float on water?
4. The density of bismuth metal is 9.8 g/cm3. What is the mass of a sample of bismuth that displaces 65.8 mL of water?
Conversions (round answers correctly and show work with units)
14. Make the following conversions:a) 16.2 m to km
b) 5.44 nL to mL
c) 45.7 mL/s to kL/hr
Reactions
6. Balance the following and equations and tell what type of reaction it is (synthesis, decomposition, single replacement, double replacement, or combustion)
a) ___ KNO3 ___ KNO2 + ___ O2 Type: __________b) ___ AgNO3 + ___ K2SO4
___ Ag2SO4 + ___ KNO3 Type: __________
c) ___ CH3NH2 + ___ O2 ___ CO2 + ___H2O + ___ N2 Type: __________d) ___ N2O5 + ___ H2O ___HNO3 Type: __________e) ___ Na +
___ Zn(NO3)2
___ Zn + ___ NaNO3 Type: __________
7. What are diatomic molecules? List the 7.
Average Atomic Mass
8. Magnesium consists of 3 naturally occurring isotopes with the masses 23.98504, 24.98584, and 25.98259 amu. The relative abundances of these three isotopes are 78.70%, 10.13 %, and 11.17% respectively. Calculate the average atomic mass.
Percent Composition
9. Calculate the percent composition of C12H22O11 (sugar). (Give Percent of each element.) Show all work.
Moles
14. Calculate the number of moles of the following: (SHOW WORK)
a) 42.8 g of KNO3
b) 155.7 L of CO2 at STP
c) 9.25 x 1026 molecules of CaCl2
Stoichiometry
11. Using the following equation:
2 NaOH + H2SO4 2 H2O + Na2SO4
How many grams of sodium sulfate will be formed if you start with 200 grams of sodium hydroxide and you have an excess of sulfuric acid?
12. Using the following equation:
Pb(SO4)2 + 4 LiNO3 Pb(NO3)4 + 2 Li2SO4
How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate, assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?
13. Using the following equation: Fe2O3 + 3 H2 2 Fe + 3 H2OCalculate how many grams of iron can be made from 16.5 grams of Fe2O3.
Limiting Reactant & Percent Yield
1. Determine the grams of sodium chloride produced when 10.0 g of sodium react with 10.0 g of chlorine gas according to the equation: 2 Na + Cl2 2 NaCl
6. Determine the mass of lithium hydroxide produced when 50.0g of lithium are reacted with 45.0g of water according to the equation: 2 Li + 2 H2O 2 LiOH + H2
3. Determine the percent yield of water produced when 68.3 g of hydrogen reacts with 85.4g of oxygen and 86.4g of water are collected. 2 H2 + O2 2 H2O
Worksheet #2: Practice Naming Compounds
5. Provide names for the following ionic compounds:a. AlF3
b. Fe(OH)2
c. Cu(NO3)2
d. Ba(ClO4)2
e. Li3PO4
f. Hg2Sg. Cr2(CO3)3
h. (NH4)2SO4
6. Write the chemical formulas for the following compounds:a. Copper(I) oxideb. Potassium peroxidec. Iron(III) carbonated. Zinc nitratee. Sodium hypobromitef. Aluminum hydroxide
7. Give the name or chemical formula for each of the following molecular substances:a. SF6
b. XeO3
c. Dinitrogen tetroxided. Hydrogen cyanidee. IF5
f. Dihydrogen monoxideg. Tetraphosphorous hexasulfide _______
4. Give the name or chemical formula for the following compounds:a. Ammonium oxalateb. Manganese(III) dichromatec. Ti(OH)4
d. Ni(ClO2)3
e. Dinitrogen pentoxidef. Aluminum oxideg. Fe2S3
5. Name the following acidsa. H2C2O4
b. HBrO3
c. HBrd. HNO2
e. H2SO4
f. HClO6. Write formulas for the following acids.
a. hydrochloric acidb. sulfuric acidc. nitric acidd. phosphoric acide. carbonic acidf. acetic acid
