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AP Chemistry Summer Assignment The summer assignment for AP Chemistry has two parts.
1. Complete the practice problems in this packet. You may use the resources listed below as well as any notes/worksheets from Accel. Chem that you may have.
2. You need to master the formulas, charges, and names of the common ions. On the first week of the school year, you will be given a quiz on these ions.
You will be asked to: • write the names of these ions when given the formula and charge • write the formula and charge when given the names I have included several resources in this packet. First, there is a list of the ions that you must know on the first day. This list also has, on the back, some suggestions for making the process of memorization easier. For instance, many of you will remember that most of the monatomic ions have charges that are directly related to their placement on the periodic table. There are naming patterns that greatly simplify the learning of the polyatomic ions as well. Also included is a copy of the periodic table used in AP Chemistry. Notice that this is not the table used in first year chemistry. The AP table is the same that the College Board allows you to use on the AP Chemistry test. Notice that it has the symbols of the elements but not the written names. You need to take that fact into consideration when studying for the afore‐mentioned quiz! I have included a sheet of flashcards for the polyatomic ions that you must learn. I strongly suggest that you cut them out and begin memorizing them immediately. Use the hints on the common ions sheet to help you reduce the amount of memorizing that you must do. Do not let the fact that there are no flashcards for monatomic ions suggest to you that the monatomic ions are not important. They are every bit as important as the polyatomic ions. If you have trouble identifying the charge of monatomic ions (or the naming system) then I suggest that you make yourself some flashcards for those as well. Doubtless, there will be some students who will procrastinate and try to do all of this studying just before the start of school. Those students may even cram well enough to do well on the initial quiz. However, they will quickly forget the ions, and struggle every time that these formulas are used in lecture, homework, quizzes, tests and labs. All research on human memory shows us that frequent, short periods of study, spread over long periods of time will produce much greater retention than long periods of study of a short period of time. I could wait and throw these at you on the first day of school, but I don’t think that would be fair to you. Use every modality possible as you try to learn these – speak them, write them, visualize them. I look forward to seeing you all at the beginning of the next school year. If you need to contact me during the summer, you can email me and I will get back to you quickly. Best of luck to you all, Mrs. Basile Email: [email protected] Resources:
1) NMSI- http://bit.ly/1fRGID3 2) Our Videos- http://youtube.com/flippinsciencevideos 3) Khan Academy Videos- http://bit.ly/1lF0uED 4) Bozeman Science Videos- http://www.bozemanscience.com/ap-chemistry/ 5) www.sciencegeek.net -you can use the many review activities in the AP chemistry section to
review 6) http://www.chemistrycoach.com/home.htm 7) http://www.collegeboard.com/ap/students/chemistry/index.html 8) http://www.wwnorton.com/college/chemistry/chemistry3/chemtours.aspx
AP Chem Summer Assignment Worksheet #1
Atomic Structure
1. a) For the ion 39K+ , state how many electrons, how many protons, and how many
19 neutrons are present?__________________________________________________________ b) Which of these particles has the smallest mass? ____________________________________________________________________________ 2. An atom has a net charge of -1.it has 18 electrons and 20 neutrons. Give a) its isotopic symbol b) its atomic number c) the charge on its nucleus d) the number of protons. a)_____________________________________________ b)______________________________________________ c)_____________________________________________ d)______________________________________________ 3. What is the number of electrons in 87Rb+?
37 ______________________________
4. Determine the number of protons, electrons, and neutrons in 80Br- and 79Se ? 35 34
________________________________________________________________________________________________________________________ 5. Complete the following table. Symbol Atomic
number Mass number
# of protons
# of electrons
# of neutrons
Net charge
90Sr+2
38
…Na…
11 10 12
….Br…
35 82 1-
6. Complete the following table. Isotopic Symbol
# of protons # of neutrons Atomic mass #
13C ….
6 7
Cl
17 18
Fe
26 56
H
1 3
Sn
70 120
7. Which of the following statements is wrong for structure of an atom? A) Protons and neutrons are in the center. B) Electrons are moving around the nucleus. C) Electrons are negatively charged particle. D) Neutrons are positively charged particles. E) Mass of one proton is equal to mass of one neutron. 8. Which of the following statements is (are) true for structure of an atom? I . Volume of a nucleus is smaller than volume of its atom. I I . The atomic mass number is the sum of proton and neutron numbers. I I I . The atomic number is the sum of protons and electrons. A) I B) II C) II I D) I , I I E) I , I I , I I I 9. 1) Proton number 2) Neutron number 3) Chemical properties 4) Physical properties Which of the above is (are) different for isotopes? A) II B) III C) I , IV D) II , I I I E) II , IV 10. If X+ 2 has 28 electrons and 35 neutrons, what is the atomic mass number of X? A) 68 B) 67 C) 65 D) 63 E) 60 11. If atomic mass number of 24X is 51, what is the number of neutrons of X? A) 27 B) 24 C) 51 D) 75 E) 40
12. If X+ 2 has 28 electrons and 35 neutrons, what is the atomic mass number of X? A) 68 B) 67 C) 65 D) 63 E) 60 13. If atomic mass number of 24X is 51, what is the number of neutrons of X? A) 27 B) 24 C) 51 D) 7 5 E) 40
14) What is the atomic mass number of 23692U?
a) 92 b) 144 c) 236 d) 328
15) What is the neutron number of 236
92U?
a) 92 b) 144 c) 236 d) 328
16. The element F has 10 neutrons and a mass number = 19. How many electrons are in its outermost shell?
A) 10 B) 3 C) 9 D) 7 E) cannot tell from the information given
17. Which one is a stable isotope of 17
35Cl.
A) 1734X B) 18
33X C) 1937X D) 20
36X
18. The most common form of iron has 26 protons and 30 neutrons in its nucleus. State its atomic number, atomic mass, and number of electrons if it's electrically neutral. Atomic number: _______ Atomic mass: ________ # of electrons: __________
19. Consider the following three atoms: Atom 1 has 7 protons and 8 neutrons; atom 2 has 8 protons and 7 neutrons; atom 3 has 8 protons and 8 neutrons. Which two are isotopes of the same element?
_ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _ _
20. Consider fluorine atoms with 9 protons and 10 neutrons. What are the atomic number and atomic mass of this fluorine? Suppose we could add a proton to this fluorine nucleus. Would the result still be fluorine? Explain. What if we added a neutron to the fluorine nucleus? Atomic number: ____________ Atomic mass: _____________ 21. How many neutrons are in the nucleus of an atom of tungsten-184 which has an atomic number of 74? # of neutrons:_________________ 22. Which of the following combinations of particles represents an ion of net charge -1 and of mass number 82? (A) 46 neutrons, 35 protons, 36 electrons (B) 46 neutrons, 36 protons, 35 electrons (C) 46 neutrons, 36 protons, 36 electrons (D) 47 neutrons, 35 protons, 35 electrons (E) 47 neutrons, 35 protons, 36 electrons 23. One species of element M has an atomic number of 10 and a mass number of 20; one species of element N has an atomic number of 11 and a mass number of 20. Which of the following statements about these two species is true? (A) They are isotopes. (B) They are isomers. (C) They are isoelectronic (D) They contain the same number of neutrons in their atoms. (E) They contain the same total number of protons plus neutrons in their atoms. 24. A neutral atom has an atomic number of 30 and a mass number of 62, the atom must contain: (A) 92 neutrons (B) 62 electrons (C) 29 neutrons (D) 30 electrons 25. Atom X has 12 protons, 12 electrons, and 13 neutrons. Atom Y has 10 protons, 10 electrons, and 15 neutrons. It can therefore be concluded that: (A) atoms X and Y are isotopes. (B) atom X is more massive than atom Y. (C) atoms X and Y have the same mass number. (D) atoms X and Y have the same atomic number. 26. A neutral atom which has 42 electrons and a mass number of 93 has (A) an atomic number of 51. (B) a nucleus containing 51 neutrons. (C) a nucleus containing 40 neutrons. (D) a nucleus containing 51 protons. 27. A sodium ion, Na + , contains the same number of electrons as (A) a sodium atom, Na. (B) a magnesium atom, Mg. (C) a potassium ion, K+ . (D) a neon atom, Ne.
AP Chem Summer Assignment Worksheet #2
Electronic Configuration
Write the electron configurations using arrows of the following elements: 1) Magnesium _________________________________________________
2) Cobalt __________________________________________________
3) Krypton ___________________________________________________
4) Beryllium ___________________________________________________
5) Scandium ___________________________________________________
Write the electron configurations of the following elements: 6) Nickel ______________________________________________________
7) Cadmium______________________________________________________
8) Selenium ______________________________________________________
9) Strontium______________________________________________________
10) Lithium ______________________________________________________
Determine what elements are denoted by the following electron configurations:
11) 1s22s22p63s23p5 ____________________
12) 1s22s22p63s23p64s23d104p65s2 _____________________
13) [Kr] 5s24d105p4 ___________________
14) [Xe] 6s24f145d7 ___________________
15) [Rn] 7s25f12 ___________________
Determine whether the following electron configurations are or are not valid:
16) 1s22s22p63s23p64s24d104p6 __________________
17) 1s22s22p63s33d6 _________________
18) [Rn] 7s25f9 __________________
19) [Xe] __________________
20) [Ne] 3p5 3s2 __________________
AP Chem Summer Assignment Worksheet #3
Periodic Table 1. A gaseous ion X2 + has two unpaired electrons in its most stable state. If X is a representative element, to which groups could the element X belong?
a) IA and VIA b) IVA c) VA and VIIA d) IA and IIIA e) VIA and VIIA
2. In the fourth period of the Periodic Table, how many elements have one or more 4p electrons?
a) 2 b) 6 c) 10 d) 18 d) 32 3. A horizontal row in the periodic table containing a sequence of elements is a: a) Group b) family c) subgroup d) period 4. The modern periodic table has the elements arranged in order of : a) their date of discovery. b) increasing radii of the atoms. c) increasing number of neutrons. d) increasing number of protons. e) number of isotopes. 5. Which of the following electron configurations is correct for chromium, (atomic number 24)?
a) [Ar]4s24p4
b) [Ar]3d54s1 c) [Ar]3d45s2 d) [Kr]4d55s1 e) [Ar]4s14p5
6. The electron configuration of Pt is [Xe]4f145d96s1. How many unpaired electrons are in this atom?
a) 1 b) 2 c) 7 d) 8 e) 9 7. Which of the following statements is false?
a) The s orbital is spherical. b) There are 10 d orbitals in a d subshell. c) The third energy level has no f orbitals. d) The fifth energy level has a set of f orbitals. e) A set of p orbitals can have a maximum of 6 electrons.
8. For a group in the periodic table, the elements have in common: a) the same number of electrons. b) the same number of electrons in all subshells. c) the same number of filled subshells. d) the same number of electrons in the highest energy subshell containing electrons. e) the same number of orbitals. 9. Which of the following electron configurations belong to an element that is the most chemically reactive? a) 1s2 b) 1s2 2s2 2p6 c) 1s22s22p5 (d) 1s22s22p63s23p6
10. How many valence electrons does the element with the electron configuration 1s22s22p63s23s64s1 have? a. 0 b) 1 c) 9 d) 19 11. How is the electron configuration similar for each element in a group?
___________________ 12. How is the electron configuration similar for each element in a period?
___________________ 13. Refer to a periodic table. In which period is calcium? a. Period 2 b. Period 4 c. Period 6 d. Period 8 14. Refer to a periodic table. In which group is calcium? a. Group 1 b. Group 2 c. Group 17 d. Group 18 15. An element that has the electron configuration [Ne]3s23p5 is in which period? a. Period 2 b. Period 3 c. Period 5 d. Period 7 16. An element that has the electron configuration [Ne]3s23p5 is in which group? a. Group 2 b. Group 5 c. Group 7 d. Group 17
AP Chem Summer Assignment Worksheet #4
Mole Concept Complete the following problems showing all work and with answers using the correct significant digits.
1) How many grams does 0.500 moles of NaCl weigh?
____________________ 2) How many molecules are there in 0.655 moles of C6H14?
____________________ 3) How many moles are there in 1.204 x 1025 molecules of water?
____________________ 4) How many grams does2.408 x 1023 molecules of SiO2 weigh?
____________________ 5) How many molecules are there in 21.6 grams of CH4?
____________________ 6) Calculate the molecular mass for the following: A. KOH ______________ B. N2O2 ___________________ C. Cu2SO3 ______________ D. Sr3 (PO4)2_________________ 7) Convert each of the following from grams to moles. A. 15.O g C2H6 _________________ C. 80 g NaOH__________________ B. 36 g H2O ____________________ D. 50 g CaCO3___________________________
8) Convert moles to grams in each of the following: A. 2 mole NH3_____________________________ B. 0.5 mole H2SO4_____________________________ 9) Convert the following to moles: A. 3.01 X 1023 atoms Na ____________________ B. 6.02 X 1024 molecules CO2 _____________________ 10) Calculate the molecular mass of the following compounds: a. acetone, CH3COCH3 _________________________ b. ethyl ether, C4H10 ____________________________ 11) How many moles of hydrogen atoms are there in 1 mole of following molecules? a. C3H8____________________ b. C2H5OH_____________________________ 12) How many moles of atoms are there in 2 moles of following molecules? a. C10H22 ___________________ b. CH3COOH__________________________
AP Chem Summer Assignment Worksheet #5
Chemical Formula /Percent Composition Complete the following problems showing all work and with answers using the correct significant digits. 1. A 0.941 gram piece of magnesium metal is heated and reacts with oxygen. The resulting oxide weighed 1.560 grams. Determine the percent composition of each element in the compound.
___________________
2. Determine the empirical formula given the following data for each compound: (a) Fe = 63.53%, S = 36.47% (b) Fe = 46.55%, S = 53.45%
(a)___________________(b)______________
3. A compound contains 21.6% sodium, 33.0% chlorine, 45.1% oxygen. Determine the empirical formula of the compound.
__________________
4. A 2.500 gram sample of uranium was heated in air. The resulting oxide weighed 2.949 gram. Determine the empirical formula of the oxide. {Hint: Carry out the calculations to four decimal places}.
__________________
5. When 1.010 g of zinc vapor is burned in air, 1.257 grams of the oxide is produced.
a) What elements are present in the oxide?
b) Determine the percent composition of each element in the oxide.
c) Determine the empirical formula of the compound.
(a)_________________ (b)________________ (c)_______________
6. A compound has the empirical formula of CH3Br and a vapor density of 6.00 g/L,
at 375 K and 0.983 atm. Using these data, determine the following:
a) The molar mass of the compound. b) The molecular formula of the compound.
(a)________________ (b)_______________
7. A compound containing the elements C, H, N, and O is analyzed. When a 1.2359 gram is burned in excess oxygen, 2.241 g of CO
2
(g) is formed. The combustion analysis showed that the sample contained 0.0648 g of H.
a) Determine the mass, in grams, of C in the 1.2359 g sample of the compound.
b) When the compound is analyzed for N content only, the mass percent of N is found to be 28.84%. Determine the mass, in grams, of N in the original 1.2359 g sample of compound.
c) Determine the mass, in grams, of O in the original 1.2359 g sample of the compound.
d) Determine the empirical formula of the compound.
(a)_________________ (b)__________________ (c)_________________ (d)______________
AP Chem Summer Assignment Worksheet #6
Stoichiometry Balance all of the equations that need to be balanced. The answers are given in parenthesis at the end of each problem. 1. In the decomposition of sodium hydroxide, how many moles of sodium hydroxide are needed to produce 30.0 moles of water? (60.0 moles NaOH)
__________________ 2. In the single replacement reaction of lithium and magnesium nitrate, what mass of lithium combines with 75.0 grams of magnesium nitrate? (7.02 g Li)
_________________
3. How many grams of lead (II) nitrate are needed to produce 60.0 grams of potassium nitrate in the double replacement reaction of potassium iodide and lead (II) nitrate. (98.3 g lead (II) nitrate)
_________________
4. In the synthesis reaction of zinc(II) and sulfur, what mass of zinc (II) sulfide is produced from 100.0 grams of sulfur? (303.9 g ZnS)
________________
5. A synthesis reaction of calcium and oxygen was completed in a lab and 234.9 grams of calcium oxide were produced from 75.00 grams of oxygen. What is the percent yield? (89.36%)
_______________ 6. In the single replacement reaction of magnesium and aluminum phosphate, if 7.00 moles of magnesium react, how many moles of aluminum phosphate would be needed? (4.67 mol AlPO
4)
_______________
7. When methane and oxygen react (complete combustion reaction) how many grams of water would be produced from 25.0 grams of methane? (56.1g water)
_______________ 8. A 26.3 gram sample of potassium chlorate decomposed and produced 9.45 grams of oxygen. What is the percent yield for oxygen? (91.7%)
______________
9. If 7.40 grams of calcium hydroxide react with nitric acid to produce 2.01 grams of water, what is the percent yield? (55.8%)
______________
10. Lime, CaO, reacts with hydrochloric acid to form calcium chloride and water. How many moles of HCl would be required to react with 7.5 moles of lime? How many moles of water would be formed? (15 mol HCl; 7.5 mol water)
______________
For each of the following write balanced chemical equations and then solve the problem. 11. What is the maximum number of grams of PH3 that can be formed when
6.2 g of phosphorus reacts with 6.0 g of hydrogen to form PH3?
______________ 12. Copper is formed when aluminum reacts with cupric sulfate in a single-replacement reaction. How many grams of copper can be obtained when 29.0 g of Al reacts with 156 g or cupric sulfate?
______________
13. If you begin with 1250 g of N2 and 225 of H2 in the reaction that forms
ammonia gas (NH3), how much ammonia will be formed? What is the limiting
reagent? How much of the reagent is left when the maximum amount of ammonia is formed?
______________
Common Ions and Their Charges
A mastery of the common ions, their formulas and their charges, is essential to success in AP Chemistry. You are expected to know all of these ions on the first day of class, when I will give you a quiz on them. You will always be allowed a periodic table, which makes indentifying the ions on the left “automatic.” For tips on learning these ions, see the opposite side of this page. From the table: Ions to Memorize Cations Name Cations Name H+ Hydrogen Ag+ Silver Li+ Lithium Zn2+ Zinc Na+ Sodium Hg2
2+ Mercury(I) K+ Potassium NH4
+ Ammonium Rb+ Rubidium Cs+ Cesium Be2+ Beryllium Anions Name Mg2+ Magnesium NO2
- Nitrite Ca2+ Calcium NO3
- Nitrate Ba2+ Barium SO3
2- Sulfite Sr2+ Strontium SO4
2- Sulfate Al3+ Aluminum HSO4
- Hydrogen sulfate (bisulfate) OH- Hydroxide Anions Name CN- Cyanide H- Hydride PO4
3- Phosphate F- Fluoride HPO4
2- Hydrogen phosphate Cl- Chloride H2PO4
- Dihydrogen phosphate Br- Bromide NCS- Thiocyanate I- Iodide CO3
2- Carbonate O2- Oxide HCO3
- Hydrogen carbonate (bicarbonate) S2- Sulfide ClO- Hypochlorite Se2- Selenide ClO2
- Chlorite N3- Nitride ClO3
- Chlorate P3- Phosphide ClO4
- Perchlorate As3- Arsenide BrO- Hypobromite Type II Cations Name BrO2
- Bromite Fe3+ Iron(III) BrO3
- Bromate Fe2+ Iron(II) BrO4
- Perbromate Cu2+ Copper(II) IO- Hypoiodite Cu+ Copper(I) IO2
- iodite Co3+ Cobalt(III) IO3
- iodate Co2+ Cobalt(II) IO4
- Periodate Sn4+ Tin(IV) C2H3O2
- Acetate Sn2+ Tin(II) MnO4
- Permanganate Pb4+ Lead(IV) Cr2O7
2- Dichromate Pb2+ Lead(II) CrO4
2- Chromate Hg2+ Mercury(II) O2
2- Peroxide C2O4
2- Oxalate NH2
- Amide BO3
3- Borate S2O3
2- Thiosulfate
Tips for Learning the Ions “From the Table” These are ions can be organized into two groups.
1. 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. This was a focus in first year chemistry, so if you are unsure what this means, get help BEFORE the start of the year.
a. All Group 1 Elements (alkali metals) lose one electron to form an ion with a 1+ charge b. All Group 2 Elements (alkaline earth metals) lose two electrons to form an ion with a 2+
charge c. Group 13 metals like aluminum lose three electrons to form an ion with a 3+ charge d. All Group 17 Elements (halogens) gain one electron to form an ion with a 1- charge e. All Group 16 nonmetals gain two electrons to form an ion with a 2- charge f. 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).
2. 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
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.
1. “ate” anions have one more oxygen then the “ite” ion, 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.
a. sulfate is SO42-, so sulfite has the same charge but one less oxygen (SO3
2-) b. nitrate is NO3
-, so nitrite has the same charge but one less oxygen (NO2-)
2. If you know that a sufate ion is SO4
2- 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.
a. Example: PO4
3- Æ HPO42- Æ H2PO4
- phosphate hydrogen phosphate dihydrogen phosphate
3. Learn the hypochlorite Æ chlorite Æ chlorate Æ perchlorate series, and you also know the series containing iodite/iodate as well as bromite/bromate.
a. The relationship between the “ite” and “ate” ion is predictable, as always. Learn one and you know the other.
b. The prefix “hypo” means “under” or “too little” (think “hypodermic”, “hypothermic” or “hypoglycemia”)
i. Hypochlorite is “under” chlorite, meaning it has one less oxygen c. The prefix “hyper” means “above” or “too much” (think “hyperkinetic”)
i. the prefix “per” is derived from “hyper” so perchlorate (hyperchlorate) has one more oxygen than chlorate.
d. Notice how this sequence increases in oxygen while retaining the same charge:
ClO- Æ ClO2- Æ ClO3
- Æ ClO4-
hypochlorite chlorite chlorate perchlorate
Sulfite
Sulfate
Hydrogen
sulfate
Phosphate
Dihydrogen Phosphate
Hydrogen Phosphate
Nitrite
Nitrate
Ammonium
Thiocyanate
Carbonate
Hydrogen carbonate
Borate
Chromate
Dichromate
Permanganate
Oxalate
Amide
Hydroxide
Cyanide
Acetate
Peroxide
Hypochlorite
Chlorite
Chlorate
Perchlorate
Thiosulfate
HSO4
-
SO4
2-
SO3
2-
HPO4
2-
H2PO4-
PO4
3-
NH4
+
NO3
-
NO2-
HCO3
-
CO3
2-
NCS- SCN-
Cr2O7
2-
CrO42-
BO3
3-
NH2
-
C2O4
2-
MnO4-
C2H3O2
-
CH3COO-
CN-
OH-
ClO2
-
ClO-
O22-
S2O3
2-
ClO4
-
ClO3
-
