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AP Chem Summer Assignment:
Independent Study Chapters 1 and 2 of textbook
Read Chapters 1 and 2 of text book, these are a review of Chem 1
We will not be discussing these chapters in class.
Answer the questions in this packet to accompany Chapters 1 and 2
The answers to the questions in the packet will be posted on my website
during the last week of August. You can check your answers then
Do the following questions from your text: These will be turned in and
graded on Friday, September 7th
.
Pages 31-35 : # 5,15,16,24,25,28,29,35,39,41,45,57,60,65,70
Pages 71-76 : # 1,9,27,29,31,33,39,41,59,61,63,64,65,68,69,71,73,75,
84,94,96
There will be a test on Chapters 1 and 2 on Friday, September 7.
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AP Chemistry Unit I Chemical Foundations
Chapters 1 Matter and Measurement , Chapter 2-Atoms Molecules and Ions
Objectives
Chapter 1 Matter and Measurement
Recall a definition of chemistry
Understand the stages and process of scientific problem solving
List the states of matter, defining and listing characteristics of the common states
Compare and contrast physical and chemical changes
Differentiate among elements, mixtures and compounds
Differentiate between homogeneous and heterogeneous mixtures
Understand and use scientific notation
Define and convert among SI units and prefixes
Understand the concept of derived units and use relationships relating to density
Define uncertainty in a measurement and recall the rules for significant digits in
calculations
Compare and contrast accuracy and precision
Interconvert between Celsius, Kelvin and Fahrenheit temperature scales
To state the fundamental chemical Laws of Conservation of Mass, Definite Proportions,
and Multiple Proportions
Chapter 2 Atoms, Molecules and Ions
To Summarize Dalton’s Atomic Theory
To explain how the Experiments of Thomson, Millikan, and Rutherford led to the
Modern view of Atomic Structure
Define isotope, and describe how mass spectrometers determine the mass of an isotope
Calculate the Average atomic mass
Distinguish among terms chemical formula, empirical formula, molecular formula and
structural formula
Determine the oxidation numbers of monatomic ions
State the formula and oxidation numbers of a variety of polyatomic ions
Distinguish among three types of inorganic substances: ionic compounds, acids, and
binary molecular compounds
Name and write formulas for some simple Organic compounds
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Classify the following as element, compound, homogeneous mixture , heterogeneous
mixture:
1. Aqueous solution of sodium chloride ________________________
2. Air_____________________________________________________
3. Granite_________________________________________________
4. Sodium chloride _________________________________________
5. White Gold (gold and palladium in differing amounts) ____________
States of matter
Properties described on the macroscopic level:
•gas (vapor)_________________________________________.
•liquid: _______________________________________________
•solid: ________________________________________________
Properties described on the molecular level:
•gas: ___________________________________________________.
•liquid: ___________________________________________________
•solid: ___________________________________________________
Physical vs. Chemical Properties A physical property is observed with the senses and can be determined without destroying the object. For
example, color, shape, mass, length, and odor are all examples of physical properties
A chemical property indicates how a substance reacts with something else. The original substance is
fundamentally changed in observing a chemical property. For example, the ability of iron to rust is a
chemical property. The iron has reacted with oxygen, and the original iron metal is changed. It now exists
as iron, a completely different substance.
Intensive properties do not depend on the amount of substance (for example, alcohol is flammable).
Extensive properties do depend on the amount (for example, the mass of the alcohol).
Classify the following properties as either chemical or physical by putting a check in the appropriate
column. Also indicate if it is an intensive or extensive property.
Property
Ph
ysi
cal
Ch
emic
al
Inte
nsi
ve
Ex
ten
siv
e
1. weight
2. blue color
3. density
4. flammability
5. volume
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Physical vs Chemical Changes
In a physical change, the original substance still exists, it has only changed in form. In a chemical
change, a new substance is produced. Energy changes always accompany chemical changes.
Classify the following as being a physical or chemical change by writing a C or a P.
1. When placed in water, a sodium pellet catches on fire as hydrogen gas is liberated
and sodium hydroxide forms Sodium hydroxide dissolves in water.
2. Sugar dissolves in water
3. Hydrochloric acid reacts with potassium hydroxide to produce salt, water, and hat.
4. Leaves change color.
5. Potassium chlorate decomposes into potassium chloride and oxygen gas.
6. Iron rusts.
7. Distillation of a liquid
8. Ice melting.
9. Milk sours.
10. evaporation
Counting Significant Digits
Quantities in chemistry are of two types:
Exact numbers – These result from counting objects such as desks (there are 24
desks in this room), occur as defined values (there are 100 cm in 1 m), or as
numbers in formulas (area of a right triangle = ½ B x H). They (24, 100, 1, and ½
for these examples) all have an infinite(∞) number of significant digits. B and H
are measurements and do not have an infinite number of digits.
Inexact numbers – These are obtained from measurements and require judgment.
Uncertainties exist in their values.
When making any measurement, always estimate one place past what is actually known.
For example, if a meter stick has calibrations to the 0.1 cm, the measurement must be
estimated to the 0.01 cm. When making a measurement with a digital readout, simply
write down the measurement. The last digit is the estimated digit.
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Significant digits are all digits in a number which are known with certainty plus one
uncertain digit. The following rules can be used when determining the number of
significant digits in a number:
Rule Example Sig Digs
1. All nonzero numbers are significant. 132.54 g 5
2. All zeros between nonzero numbers are significant. 130.0054 m 7
3. Zeros to the right of a nonzero digit but to the left of an
understood decimal point are not significant unless shown
by placing a decimal point at the end of the number.
190 000 mL
190 000. mL
2
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4. All zeros to the right of a decimal point but to the left of
a nonzero digit are NOT significant.
0.000 572 mg 3
5. All zeros to the right of a decimal point and to the right
of a nonzero digit are significant.
460.000 dm 6
A good way to remember which side to start on is:
decimal point present, start at the Pacific
decimal point absent, start at the Atlantic
How many significant digits do each of the following numbers have?
1. 2.3000 x 106_____________________ 6. 500. _____________________
2. 45.1 _____________________ 7. 970 _____________________
3. 800000.103 _________________ 8. 0.002 _____________________
4 0.000000001500_________________ 9. 0.007 80 _____________________
5. 600 _____________________ 10. 145.55 _____________________
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Rounding Rules Calculators often give answers with too many significant digits. It is often necessary to round off the answers to the correct number of
significant digits. The last significant digit that you want to retain should be rounded up if the digit immediately to the right of it is (Each of the examples are being rounded to four sig digs):
Rule Example 4 sig digs
….. greater than 5 532.79 532.8
….. 5, followed by a nonzero digit 17.255 1 17.26
….. 5, not followed by a nonzero, but has an odd digit directly in front of it. 3 213.5 3214
The last significant digit that you want to retain should stay the same if the digit immediately to the right of it is:
Rule Example 4 sig digs
….. less than 5 5 454.33 5 454
….. 5, not followed by a nonzero digit, but has an even digit directly in front of it. 0.007 85 0.007 8
Round the following numbers to 3 sig digs.
1. 279.3 ___________ 3. 32.395 ___________ 5. 18.29 ___________
2. 42.353 ___________ 4. 32.25 ___________ 86 5 001 ___________
Applying significant digits to arithmetic operations
Addition and Subtraction – Look at the numbers being added or subtracted and identify which one has the lowest number
of decimal places. Calculate the answer. Round the answer to the lowest number of decimal places.
14.565 + 7.32 = 21.885 7.32 has only 2 decimal places, so the answer should be rounded to 21.88
143.52 – 100.6 = 42.92 100.6 has only 1 decimal place, so the answer should be rounded to 42.9
Multiplication and Division – Look at the numbers being multiplied or divided and identify which one has the lowest number of significant digits. Calculate the answer. Round the answer to the lowest number of significant digits.
172.6 x 24.1 = 4159.66
24.1 has only 3 significant digits, so the answer should be rounded to 4160
172.6 ÷ 24.1 = 7.161 82
234.1 only has 3 significant digits, so the answer should be rounded to 7.16
Express each answer with the correct number of significant digits.
1. 320 x 24.9
0.080
2. 432.7 x 6.5 x .002300
62 x 0.103
3. 32.44 + 4.9- 0.304
82.94
4. 8.002 + 0 .3040
13.4 - 0.066 + 1.02
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Temperature is defined as the average kinetic energy of the particles in a sample of
matter. The units for this are oC and Kelvin (K). Note that there is no degree symbol for
Kelvin. Absolute zero is ) Kelvin. This is the coldest possible temperature where all
molecular motion ceases
Heat is a measurement of the total kinetic energy of the particles in a sample of matter.
The units for this are the calorie (cal) and the Joule (J).
The following equation can be used to convert temperatures from Celsius (t) to Kelvin
(T) scales and fahrenheit to celsius and celsius to fahrenheit
T(K) = t(oC) + 273.15
t(oC) = T(K) - 273.15
You are simply subtracting 273.15 from your Kelvin temperature.
Convert the following:
1. 335C = _______________K
2 50.0 K = _______________C
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SI Fundamental Units
http://wpscms.pearsoncmg.com/wps/media/objects/3661/3749680/Aus_content_01/Table01-03.jpg
SI Derived Units- calculated from fundamental units
http://cornellchem.wikispaces.com/Unit+2+-+Measurements+and+Calculations
SI Prefixes
http://wpscms.pearsoncmg.com/wps/media/objects/3661/3749680/Aus_content_01/Table01-03.jpg
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Using Dimensional Analysis to convert among metric units
1. Convert 1.09 ng to g
2. Convert 90.1 ms to s
3. Convert 145 pm to m
4. Convert 1.55 kg/m3 to g/L
5. Determine the number of L in a box that measures 4cm x 8cm x 10cm.
(1 ml= 1 cm3)
6. If a car has an EPA mileage rating of 30 miles per gallon, what is this rating in
km/L?
7.
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Accuracy versus Precision
Percent Error – Measures accuracy of measurement.
Calculate the percent error for the following problems. Show your work and use the
correct number of significant digits in your answer.
1. A student measures a rectangular piece of metal. According to the student, it has
a length of 1.98 cm, a width of 5.15 cm, and a height of 1.03 cm and a mass of
77.89 g. The metal is iron, which has a density of 7.80 g/cm3. What is the
percent error?
2. A technician is making a 0.500 M salt solution for an experiment. The
experiment will work as long as the solution is within 2.00 % of the accepted
0.500 M. In actuality, the solution was 0.522 M. Will the experiment work?
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Density
The formula for density is d=m/v
The density of wáter at 22 C is 1 g/ml
1 cm3= 1 ml
1. An irregularly shaped piece of metal with a mass of 125g is placed into a
graduated cylinder that contains 25.00mL of water. This raises the water level to
56.00mL. What is the density of the metal?
2. Calculate the mass of a block of iron (density = 7.86g/ml) with dimensions of
528mm x 67.4mm x 37.3mm.
3. The volume of a red blood cell is about 9.00x10-11
cm3. Assuming that red blood
cells are spherical, what is the diameter of a red blood cell in inches?
4. A fertilizer contains 21% nitrogen by mass. What mass of this fertilizer, in
kilograms, is required for an application of 775g of nitrogen?
5. A column of mercury is contained in a cylindrical tube. The tube has a diameter
of 8.0 mm, and the height of the mercury column is 1.20 m. Given that the
density of mercury is 13.6 g/mL and that the volume of mercury in the tube can
be calculated by the relation V = πr2h (r = the radius of the tube and h = the height
of the mercury column), calculate the mass of mercury present in the cylindrical
tube.
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Fundamental Chemical Laws and Dalton’s Atomic Theory
What Laws do Dalton’s atomic theory explain?
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
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Thomson’s Cathode Ray Tube
Experiments
Describe Thomson’s Cathode ray tube experiment and describe the major conclusions of
this experiment:
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
Describe this picture in terms of Thomson’s model
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Millikan’s Oil Drop Experiment
What was Milikan able to determine from his oil drop experiment?
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
Radioactivity
Explain the behavior of alpha, beta and gamma rays as illustrated in the diagram above
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
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Rutherford’s Gold Foil Experiment
Describe Rutherford’s Gold Foil Experiment and describe the major conclusions of this
experiment:
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
__________________________________________________________________
Atomic theory Summary
Scientist Experiment Knowledge gained Relating to
Thomson
Millikan
Rutherford
Chadwick
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Modern view of Atomic Structure
Atomic number & the number of electrons, protons, and neutrons.
XAZ
is the general symbol for an isotope where A is the mass number (number of
protons + number of neutrons), X is the element’s symbol, and Z is the atomic
number (number of protons). This information can also be found on the periodic
table. Use this information to fill in the chart for the following elements
Symbol Atomic
Number
Atomic
Mass Protons Electrons Neutrons Element Name
Gold
copper
nickel
lead
zinc
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Average Atomic Mass
Directions:
1. Write the isotopes.
2. Write the masses.
3. Multiply the masses by the decimal equivalent of the relative abundance.
4. Add the products. This is the average atomic mass.
Example:
A sample of cesium is 20.0 % 132
Cs ,75.00 % 133
Cs, and 5.0 % 134
Cs
132
Cs = 132 x 0.200 = 26.4 133
Cs = 133 x 0.7500 = 99.75 134
Cs = 134 x 0.050 = _6.7_
132.8
Determine the average atomic mass of the following mixtures of isotopes:
1. 80.0 % I-127, 17.0 % I-126, and 3.00 % I-128.
2. 50.0 % Au-197, 50.0 % Au-198.
3. Naturally occurring chlorine molecules (chlorine is diatomic) have masses of
70, 72 and 74. They occur in the percentages of 56.25%, 37.50% and
6.250%. What is the average atomic mass of chlorine atoms?
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Chemical Nomenclature Flowchart
Case 1: Ionic compounds containing monatomic ions (i.e. ions that can only have one charge)
Name of Compound = name of metal + name of non-metal w/ide suffix or name of polyatomic ion. No
prefixes are used!
e.g. NaF = sodium fluoride; Na3PO4 = sodium phosphate; (NH4)3PO4 = ammonium phosphate
Case 2: Ionic compounds containing a metal that can form more than one ion
Name of Compound = name of metal, followed by charge of metal in Roman numerals in parentheses,
followed by name of non-metal w/ -ide suffix or name of polyatomic ion. No prefixes are used!
e.g. PbCl2 = Lead (II) chloride; Cu(NO3)2 = copper (II) nitrate
Case 3: Binary molecular compounds:
Name of Compound = name of first element + name of second element with -ide suffix.
Use prefixes (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, nona-, deca-) to indicate the number of atoms.
The mono prefix is not used with the first element.
e.g. CO = carbon monoxide; NO2 = nitrogen dioxide; N2O = dinitrogen monoxide; P2O5 = diphosphorus
pentoxide
Case 4: Binary acid solutions (i.e. binary acids dissolved in water = binary acids in aqueous solution)
Name of Compound = hydro + name of halogen w/ -ic suffix e.g. HF(aq) = hydrofluoric acid; HCl(aq) =
hydrochloric acid
Unless stated otherwise assume the formula of a binary acid is for the acid dissolved in water. E.g.
assume HCl = HCl(aq)
Naming Oxoacids (i.e. compound with the general formula HxMOy, where M = nonmetal)
The name of an oxoacid is based on the name of the polyatomic ion from which the acid is derived.
Case 5: -ate -ic
If the name of the polyatomic ion ends in “-ate,” the name of the corresponding acid ends in “-ic acid.”
Polyatomic ion (-ate) Acid (-ic)
sulfate = SO42- H2SO4 = sulfuric acid
Chlorate = ClO31- HClO3 = chloric acid
Case 6: -ite -ous
If the name of the polyatomic ion ends in “-ite,” the name of the corresponding acid ends in “-ous acid.”
Polyatomic ion (-ite) Acid (-ous)
sulfite = SO32- H2SO3 = sulfurous acid
Chlorite = ClO21- HClO2 = chlorous acid
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Write the formula.
1. Ammonium Nitrate
2. Calcium Bicarbonate or Calcium
Hydrogen Carbonate
3. Barium Chlorate
4. Dimercury (I) Iodide
5. Hydronitric acid
6. Plumbic Oxide or Lead (IV) Oxide
7. Potassium Thiocyanide
8. Perchloric acid
9. Sulfur hexafluoride
10. Zinc Hydroxide
11. Potassium Sulfite
12. Copper (I) Sulfide
13. Potassium bisulfate
14. Zinc Bromide
15. Ferric Chromate
16. Sodium Perchlorate
17. Potassium Hypochlorite
18. Magnesium Nitride
19. Sodium Permanganate
20. Potassium Permanganate
Write the name.
21. Hg2(CN)2
22. H2SO4
23. Fe(C2H3O2)2
24. KClO3
25. PbF2
26. HBr
27. N2O4
28. HgCrO4
29. Ag3PO4
30. K2Cr2O7
31. Ba3N2
32. NF3
33. CuBr2
34. (NH4)2S
35. Ca(NO3)2
36. Zn(OH)2
37. NaHCO3
38. PbO2
39. KClO4
40. Hg2I2
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Mixed Practice
Write the correct formula, Write I, A, or M to the left to state what type of compound it is
1. ______calcium fluoride _________________________
2. _______ferrous carbonate _________________________
3. _______aluminum hydroxide __________________________
4. _______dinitrogen pentaoxide ___________________________
5. _______chromic acid ___________________________
6. _______nitrogen monoxide ___________________________
7. _______plumbic sulfate ___________________________
8. _______hydrophosphoric acid _____________________________
9.________tetraphosphorus decoxide ____________________________
Write the correct name. IF THERE ARE TWO WAYS TO NAME A COMPOUND
USE BOTH!!
9. ______ LiS ___________________________________________
10. ______NH4Cl _______________________________________
11. _______SnSO4 ____________________________________________
12. _______ H3PO3 _____________________________________________
13. ________ P2O5 ____________________________________________
14. ________ CO ______________________________________________
15. _______H3N ______________________________________________
16. _______ CuS ________________________________________________
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Naming Acids
“ate” becomes “____ic acid” I ate something icky
“ite” becomes “____ous acid”
“ide” becomes hydro ___ic acid
**in sulfur acids add “ur” in phosphorous acids add “or”
Write formula and oxidation number of anion, write correct formula
for acid, name the acid:
anion Anion
formula
/ox #
Acid
formula
Acid name
bromate
periodate
carbonate
sulfide
chloride
chloric
thiosulfate
dichromate
chromate
permanganate
bromate
iodite
iodide
perchloride
phosphate
hyporchlorite
phosphide
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Simple Organic Compounds
Alkanes
Most basic type of hydrocarbon
Carbón bonded to 4 other atoms
General fromula is CnH2n+2
End in suffix –ane
Name derived from number of carbons in hydrocarbon chain. KNow the
following:
Part of name derived from # carbons # carbons in hydrocarbon chain
Meth- 1
Eth- 2
Prop- 3
But- 4
Pent- 5
Hex- 6
Hept- 7
Oct- 8
Non- 9
Dec- 10
Write the molecular formula for the following:
1. Propane___________________
2. Hexane ____________________
3. Octane _____________________
4. Methane _____________________
5. Butane _______________________
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Alcohols
Some hydrogen atoms in an alkane chain replaced with hydroxyl -OH
Name is derived from its parent alkane
Name ends with –ol
WHen there is more tan one carbón upon which the hydroxyl group can be
present, a number is placed in front of the name to inducate which carbón in the
hydrocarbon chain has the –OH group attached