AP Chemistry Summer Assignment 2015‐2016 Mrs. Rankin Congratulations for choosing to take AP Chemistry in September. Enclosed is the summer assignment for this class. Over the summer, you will memorize several important tables that are needed for AP Chemistry. This information was in the Regents reference tables, but must be memorized for the AP class. You are responsible for this material, as it will not be covered in class. The summer assignment is due on the first day of class in September. No late or incomplete assignments will be accepted. If you have any questions regarding this assignment, feel free to see Mrs. Rankin in Room 201. Instructions 1. Memorize the tables and charts that follow. There will be a test on this the first week of school. 2. Complete the significant figures sheet. 3. Complete the compound naming sheet. Polyatomic Ions Name Ammonium Acetate Amide Bromate Bromite Chlorate Chlorite Cyanide Dihydrogen phosphate Hydrogen sulfate Hydroxide Hypobromite Hypochlorite Hypoiodate Iodate Iodite Nitrate Nitrite Perbromate Perchlorate Periodate Permanganate Thiocyanate Carbonate Chromate Dichromate Hydrogen carbonate Oxalate Peroxide Selenate Silicate Sulfate Sulfite Thiosulfate Phosphate Phosphite Formula NH4+ C2H3O2– NH2– BrO3– BrO2– ClO3– ClO2– CN– H2PO4– HSO– OH– BrO– ClO– IO– IO3– IO2– NO3– NO2– BrO4– ClO4– IO4– MnO4– SCN– CO32– CrO42– Cr2O72– HCO3– C2O42– O22– SeO42– SiO32– SO42– SO32– S2O32– PO43– PO33– Cations H+ Li+ Na+ K+ Rb+ Cs+ Be2+ Mg2+ Ca2+ Ba2+ Sr2+ Al3+ Fe3+ Fe2+ Cu2+ Cu+ Co3+ Sn4+ Sn2+ Pb4+ Pb2+ Hg2+ Hg22+ Ag+ Zn2+ Anions H– F– Cl– Br– I– O2– S2– Se2– N3– P3– As3– Name Hydrogen Lithium Sodium Potassium Rubidium Cesium Beryllium Magnesium Calcium Barium Strontium Aluminum Iron (III) Iron (II) Copper (II) Copper (I) Cobalt (III) Tin (IV) Tin (II) Lead (IV) Lead (II) Mercury (II) Mercury (I) Silver Zinc Name Hydride Fluoride Chloride Bromide Iodide Oxide Sulfide Selenide Nitride Phosphide Arsenide Tips for Learning the Ions From the Periodic Table These are ions can be organized into two groups. Their place on the table suggests the charge on the ion, since the neutral atom gains or loses a predictable number of electrons in order to obtain a noble gas configuration.  All Group 1 Elements (alkali metals) lose one electron to form an ion with a 1+ charge  All Group 2 Elements (alkaline earth metals) lose two electrons to form an ion with a 2+ charge  Group 13 metals like aluminum lose three electrons to form an ion with a 3+ charge  All Group 17 Elements (halogens) gain one electron to form an ion with a 1‐ charge  All Group 16 nonmetals gain two electrons to form an ion with a 2‐ charge  All Group 15 nonmetals gain three electrons to form an ion with a 3‐ charge Notice that cations keep their name (sodium ion, calcium ion) while anions get an “‐ide” ending (chloride ion, oxide ion). Metals that can form more than one ion will have their positive charge denoted by a Roman numeral in parenthesis immediately next to the name of the cation. Polyatomic Anions Most of the work on memorization occurs with these ions, but there are a number of patterns that can greatly reduce the amount of memorizing that one must do. Anions that end in “ate” have one more oxygen then the anions that end in “ite”, but the same charge. If you memorize the “ate” ions, then you should be able to derive the formula for the “ite” ion and vice‐versa.  Sulfate is SO42–, so sulfite has the same charge but one less oxygen (SO32–)  Nitrate is NO3 – , so nitrite has the same charge but one less oxygen (NO2– ) If you know that a sulfate ion is SO42– then to get the formula for hydrogen sulfate ion, you add a hydrogen ion to the front of the formula. Since a hydrogen ion has a 1+ charge, the net charge on the new ion is less negative by one. HPO42–  H2PO4 –  Example: PO43–  phosphate hydrogen phosphate dihydrogen phosphate Learn the hypochlorite  chlorite  chlorate  perchlorate series, and you also know the series containing iodite/iodate as well as bromite/bromate.  The relationship between the “ite” and “ate” ion is predictable, as always. Learn one and you know the other.  The prefix “hypo” means “under” or “too little” (think “hypodermic”, “hypothermic” or “hypoglycemia”) o Hypochlorite is “under” chlorite, meaning it has one less oxygen  The prefix “hyper” means “above” or “too much” (think “hyperkinetic”) o The prefix “per” is derived from “hyper” so perchlorate (hyperchlorate) has one more oxygen than chlorate.  Notice how this sequence increases in oxygen while retaining the same charge: ClO–  ClO2–  ClO3–  ClO4– hypochlorite chlorite chlorate perchlorate Rules for Determining Oxidation Number 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. 1. The oxidation number of any uncombined element is zero. 2. The oxidation number of a monatomic ion equal the charge on the ion. 3. The more electronegative element in a binary compound is assigned the number equal to the charge it would have if it were an ion. 4. The oxidation number of fluorine in a compound is always –1 5. 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. 6. The oxidation state of hydrogen in most of its compounds is+1 unless it combined with a metal, in which case it is –1. 7. In compounds, the elements of groups 1 and 2 as well as aluminum have oxidation number of +1, +2, and +3, respectively 8. The sum of the oxidation numbers of all atoms in a neutral compound is zero. 9. The sum of the oxidation number of all atoms in a polyatomic ion equals the charge of the ion. Solubility Rules 1. Most nitrate (NO3–) salts are soluble. 2. Most salts containing the alkali metal ions (Li+, Na+, K+, Cs+, Rb+) and the ammonium ion (NH4+) are soluble. 3. Most chloride, bromide, and iodide salts are soluble. Notable exceptions are salts containing the ions Ag+, Pb2+, and Hg22+. 4. Most sulfates are soluble. Notable exceptions are BaSO4, PbSO4 ,Hg2SO4, and CaSO4. 5. Most hydroxide salts are only slightly soluble. The important soluble hydroxides are NaOH and KOH. The compounds Ba(OH)2, Sr(OH)2, and Ca(OH)2. 6. Most sulfide(S2–), carbonate (CO32–), chromate (CrO42–), and phosphate (PO43–) salts are only slightly soluble. Rules for Making and Naming Ionic Compounds 1. 2. 3. Balance Charges (charges should equal zero). Cation is always written first ( in name and in formula). If the cation has more than one charge, indicate the charge used in the name with a Roman numeral. Change the ending of the anion to –ide. Rules for Naming Covalent Compounds 1. 2. 3. The less electronegative element gets written first. The first element does not need the prefix mono if there is only one atom. The more electronegative element gets written second and always needs a prefix. Rules for Naming an Acid 1. 2. 3. When 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 acid  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 acid  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 acid  ClO3– is the chlorate ion so HClO3 = chloric acid Significant Figures in M
Measuremen
nt and Calcu
ulations A successful chemistry stude
ent habitually labels all n
numbers, beecause the u
unit is importtant. Also off great impo
ortance is th
he number ittself. Any number used in a calculatiion should contain only figures that are conssidered reliable; otherwiise, time and
d effort are w
wasted. Figuures that aree considered
d reliable aree called signiificant figure
es. Chemical calculationss involve numbers repreesenting actu
ual measureements. In a measurement, significant figgures in a nu
umber consisst of figures (digits) definitely known plus one eestimated figurre (digit) Recording Measurem
ments Wheen one readss an instrument (ruler, th
hermometer, graduate, buret, barometer, balan
nce), he exp
presses the read
ding as one w
which is reassonably reliable. For example, in thee accompanyying illustration, note the reading markked A. This rreading is de
efinitely beyo
ond the 7 cm
m mark and also beyond the 0.8 cm mark. We read tthe 7.8 with certainty. mate that the reading is five‐tenths tthe We ffurther estim
distaance from th
he 7.8 mark tto the 7.9 m
mark. So, we estimate the length as 0.0
05 cm more than 7.8 cm. All of these
e have meaning and are
e therefore ssignificant. W
We express tthe reading as 7.85 cm, accurate to
o three signifficant figures. All of these figurres, 7.85, can
n be used in calculationss. In readingg B we see th
hat 9.2 cm iss definitely kknown. We can iinclude one estimated d
digit in our re
eading, and we estimatee the next diigit to be zerro. Our reading is repo
orted as 9.20
0 cm. It is acccurate to thrree significant figures. es for Zeros Rule
If a zzero represe
ents a measu
ured quantityy, it is a significant figuree. If it merelly locates the decimal po
oint, it is nott a siggnificant figu
ure.  ZZero Within a
a Number: In reading th
he measurem
ment 9.04 cm
m, the zero rrepresents a measured q
quantity, just as 9 and 4, and is, th
herefore, a significant nu
umber. A zerro between any of the o
other digits in a number is a significant figure. umber: In reaading the measurementt 0.46 cm, th
he zero doess not represeent a  ZZero at the FFront of a Nu
m
measured qu
uantity, but merely locattes the decim
mal point. Itt is not a sign
nificant figurre. Also, in th
he m
measuremen
nt 0.07 kg, th
he zeros are used merely to locate tthe decimal point and arre, thereforee, not ssignificant. ZZeros at the first (left) off a number aare not significant figurres. mber: In read
ding the meaasurement 111.30 cm, the zero is an estimate an
nd  ZZero at the EEnd of a Num
rrepresents a measured q
quantity. It iss therefore ssignificant. A
Another wayy to look at tthis: The zero is not n
needed as a placeholderr, and yet it w
was included
d by the perrson recordin
ng the meassurement. It must have b
been recorde
ed as a part of the meassurement, m
making it signnificant. Zero
os to the rigght of the deecimal point, aand at the end of the nu
umber, are ssignificant figures. hole Numberr: Zeros at th
he end of a w
whole numb
ber may or m
may not be siignificant. If  ZZeros at the End of a Wh
aa distance is reported ass 1600 feet, o
one assumes two sig figss. Reportingg measuremeents in scien
ntific n
notation rem
moves all dou
ubt, since all numbers w
written in scieentific notattion are considered sign
nificant. 1 600 feet 1.6
6 × 103 feet Twoo significant ffigures 3
1 600 feet 1.6
60 × 10 feett Threee significant figures 1 600 feet 1.6
600 × 103 fee
et Fourr significant figures Sample Problem #1: Underline the significant figures in the following numbers. (a) 0.0420 cm answer = 0.0420 cm (e) 2 403 ft. answer = 2 403 ft. (b) 5.320 in. answer = 5.320 in. (f) 80.5300 m answer = 80.5300 m (c) 10 lb. answer = 10 lb. (g) 200. g answer = 200 g (d) 0.020 mL answer = 0.020 mL (h) 2.4 x 103 kg answer = 2.4 x 103 kg Rounding Off Numbers In reporting a numerical answer, one needs to know how to "round off" a number to include the correct number of significant figures. Even in a series of operations leading to the final answer, one must "round off" numbers. The rules are well accepted rules: 1. If the figure to be dropped is less than 5, simply eliminate it. 2. If the figure to be dropped is greater than 5, eliminate it and raise the preceding figure by 1. 3. If the figure is 5, followed by nonzero digits, raise the preceding figure by 1 4. If the figure is 5, not followed by nonzero digit(s), and preceded by an odd digit, raise the preceding digit by one 5. If the figure is 5, not followed by nonzero digit(s), and the preceding significant digit is even, the preceding digit remains unchanged Sample Problem #2: Round off the following to three significant figures. (a) 3.478 m answer = 3.48 m (c) 5.333 g answer = 5.33 g (b) 4.8055 cm answer = 4.81 cm (d) 7.999 in. answer = 8.00 in. Multiplication In multiplying two numbers, when you wish to determine the number of significant figures you should have in your answer (the product), you should inspect the numbers multiplied and find which has the least number of significant figures. This is the number of significant figures you should have in your answer (the product). Thus the answer to 0.024 x 1244 would be rounded off to contain two significant figures since the factor with the lesser number of significant figures (0.024) has only two such figures. Sample Problem #3: Find the area of a rectangle 2.1 cm by 3.24 cm. Solution: Area = 2.1 cm × 3.24 cm = 6.804 cm2 We note that 2.1 contains two significant figures, while 3.24 contains three significant figures. Our product should contain no more than two significant figures. Therefore, our answer would be recorded as 6.8 cm2 Sample Problem #4: Find the volume of a rectangular solid 10.2 cm x 8.24 cm x 1.8 cm Solution: Volume = 10.2 cm × 8.24 cm × 1.8 cm = 151.2864 cm3 We observe that the factor having the least number of significant figures is 1.8 cm. It contains two significant figures. Therefore, the answer is rounded off to 150 cm3 . Division In dividing two numbers, the answer (quotient) should contain the same number of significant figures as are contained in the number (divisor or dividend) with the least number of significant figures. Thus the answer to 528 ÷ 0.14 would be rounded off to contain two significant figures. The answer to 0.340 ÷ 3242 would be rounded off to contain three significant figures. Sample Problem
m #5: Calculaate 20.45 ÷ 2
2.4 So
olution: 20.4
45 ÷ 2.4 = 8.52083 We n
note that thee 2.4 has few
wer significan
nt figures th
han the 20.45. It has o
only two significant figures. Therefoore, our answ
wer should h
have no morre than two siignificant figgures and should be repo
orted as 8.5.. Addition and Subtra ction dding (or sub
btracting), se
et down the numbers, b
being sure too keep like decimal placees under eacch other, In ad
and add (or subttract). Next, note which column con
ntains the fir st estimated
d figure. Thiss column determines e answer. Aftter the answ
wer is obtain ed, it should
d be rounded off in this column. In the last decimal place of the
und to the le
east numberr of decimal places in you data. otheer words, rou
Sample Problem
m #6: Add 42
2.56 g + 39.460 g + 4.1g So
olution: Since th
he number 44.1 only exteends to the first decimal place, the answer must be rouunded to thee first decim
mal place, yieelding the answer 86.1 g. Averaage Readinggs The average of aa number of successive rreadings will have the saame numberr of decimal places that are in their sum. Sample Problem
m #7: A gradu
uated cylind
der was weigghed three tiimes and thee recorded w
weighings w
were 12.523 g
g, 5 g. Calculate
e the averagge weight. 12.497 g, 12.515
In ord
So
olution: der to find thhe average, tthe sum is divided by 3 tto give an answe
er of 12.51167. Since eaach number extends to tthree decim
mal places, thhe final answ
wer is rounded to three decimal placess, yielding a final answer of 12.512 gg. Notice thaat the divisor of 3 does not afffect the roun
nding of the final answer. This is beccause 3 is an
n exact number, known to an infinite number of decimal p
places. Name __________________________________ AP Chemistry Summer Assignment Sheet #1 Mrs. Rankin Give the number of significant figures in each of the following. ____ 402 m ____ 34.20 lbs ____ 0.03 sec ____ 0.00420 g ____ 3 200 liters ____ 0.0300 ft. ____ 5.1 × 104 kg ____ 0.48 m ____ 1 400.0 m ____ 78 323.01 g ____ 1.10 torr ____ 760 mm Hg Multiply each of the following, observing significant figure rules. 17 m × 324 m = ________________ 1.7 mm × 4 294 mm = __________________ 0.005 in × 8 888 in = _____________ 0.050 m × 102 m = ____________________ 0.424 in × .090 in = ______________ 324 000 cm × 12.00 cm = _______________ Divide each of the following, observing significant figure rules. 23.4 m ÷ 0.50 sec = ______________ 12 miles ÷ 3.20 hours = ________________ 0.960 g ÷ 1.51 moles = ____________ 1 200 m ÷ 12.12 sec = __________________ Add each of the following, observing significant figure rules 3.40 m 102.45 g 102. cm 0.022 m 2.44 g 3.14 cm 0.5 m 1.9999 g 5.9 cm ________________ ______________ _______________ Subtract each of the following, observing significant figure rules. 14.33 g 234.1 cm 42.306 m 1.22 m 3.468 g 62.04 cm ________________ ______________ _______________ Work each of the following problems, observing significant figure rules. Three determinations were made of the percentage of oxygen in mercuric oxide. The results were 7.40%, 7.43%, and 7.35%. What was the average percentage? A rectangular solid measures 13.4 cm × 11.0 cm × 2.2 cm. Calculate the volume of the solid. If the density of mercury is 13.6 g/mL, what is the mass in grams of 3426 mL of the liquid? A copper cylinder, 12.0 cm in radius, is 44.0 cm long. If the density of copper is 8.90 g/cm3 , calculate the mass in grams of the cylinder. (assume pi = 3.14) Name ____________________________________ AP Chemistry Summer Assignment Sheet #2 Mrs. Rankin Write formulas for the following substances. 1. barium sulfate _______________________ 2. ammonium chloride ___________________ 3. chlorine monoxide ____________________ 4. silicon tetrachloride ___________________ 5. magnesium fluoride ___________________ 6. sodium oxide ________________________ 7. sodium peroxide _____________________ 8. copper (I) iodide _____________________ 9. zinc sulfide _________________________ 10. potassium carbonate __________________ 11. hydrobromic acid _____________________ 12. perchloric acid _______________________ 13. lead (II) acetate ______________________ 14. sodium permanganate _________________ 15. lithium oxalate _______________________ 16. potassium cyanide ____________________ 17. iron (III) hydroxide ____________________ 18. silicon dioxide ________________________ 19. nitrogen trifluoride ____________________ 20. chromium (III) oxide ___________________ 21. calcium chlorate ______________________ 22. sodium thiocyanate ___________________ Name each of the following compounds/acids. 23. CuSO4 ___________________________ 24. PCl3 _____________________________ 25. Li3N _____________________________ 26. BaSO3 ____________________________ 27. N2F4 _____________________________ 28. KClO4 ____________________________ 29. NaH _____________________________ 30. (NH4)2Cr2O7 _______________________ 31. HNO2 _____________________________ 32. Sr3P2 _____________________________ 33. Mg(OH)2 __________________________ 34. Al2S3 _____________________________ 35. P4O10 ____________________________ 36. HC2H3O2 _________________________ 37. CaI2 ______________________________ 38. MnO2 _____________________________ 39. Li2O ______________________________ 40. FeI3 ______________________________ 41. Cu3PO4 ____________________________ 42. PCl3 _______________________________ 43. NaCN ______________________________ 44. Cs3N ______________________________