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FINAL REVIEW Vella Name_______________ Period___ Date____________
2-1 1. How many molecules are there in each picture below ?
2. How many monatomic molecules are there ?
3. How many diatomic molecules are pictured ?
4. How many of the molecules are molecules of a compound ?
5. How many of the molecules are molecules of an element ?
6. How many atoms are in the picture ?
A B
1. molecules 1. molecules
2. monatomic 2. monatomic
molecules molecules
3. diatomic 3. diatomic
molecules molecules
4. molecules 4. molecules
of a compound of a compound
5. molecules 5. molecules
of an element of an element
6. atoms 6. atoms
2-2 Write the formulas and the names for the compounds formed between the
following elements / ions. ( The charges are provided for metals which form more than
one ion. )
FORMULA NAME
a. iodine and lead
+2
b. chlorine and ammonium
c. dichromate and potassium
d. carbonate and cobalt
+2
2-3. Write the formulas for the following chemical compounds
a. lead(IV) chloride d. phosphorus tribromide
b. dinitrogen monoxide e. copper(I) sulfide
c. aluminum chloride f. strontium hydroxide
2-4. Write the names for the following chemical compouds
a. CuSO4 d. CCl4
b. Cr2(C2O4)3 e. NaC2H3O2
c. CaBr2 f. SO3
2-5 Estimate measurements for the following as indicated
cm 9 10 11 12 13 14 15 16
ll l l l l l l l l Il l l l l l l l l Il l l l l l l l l ll l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l ABC C D E
1. Between & & &
2. Measurement 3. # of significant figures
cm 96 97 98 99 100 101 102 103
ll l l l l l l l l Il l l l l l l l l Il l l l l l l l l ll l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l D EF D E F
1. Between & & &
2. Measurement
3. # of significant figures
3-1. How many significant figures are in each of the following
measurements?
a. 834.71 g c. 33 km e. 0.00020 mm ____
b. 20.4 L d. 710,000,000 K f. 273.0 K ____
3-2. Convert the following quantities into scientific notation, showing the correct
number of significant figures.
a 840.00 kg b .000476 moles c 17.83 g d 0.27 cm e .00630 L
3-3. DENSITY
a. Find the density of a block of marble with a mass of 1.10 X 103 grams and a volume
of 4.00 X 102 cm3.
b. Diamond has a density of 3.26 g/cm3. What is the mass of 78 cm3 of a diamond?
c. 1.52 X 102 L of ethanol has a mass of g . ( density ethanol = .791 g/mL)
Look at each of the following formulas and identify what each represents. Writ
the correct letter in the space next to each symbol.
A = atom M = molecule P = polyatomic ion
I = ion F = formula unit
1. N2 3. AsO4-3 5. Mg3(PO4)2
2. Ca+2 4. NO2 6. Au
4-1. MOLE PARTICLE CALCULATIONS Show all work and use the factor-label method.
1. What is the molar mass of calcium bromide ? Formula =
2. What is the mass in grams of 2.83 moles of calcium bromide? Formula =
3. How many moles are in 4.13 x 10-5 grams of dinitrogen pentoxide? Formula =
4. How many atoms of sulfur are there in 45.5 grams of aluminum sulfide ? Formula
=
5. How many atoms are there in 88.0 grams of gold ?
4-2 MOLE PARTICLE CALCULATIONS/ PERCENT COMPOSITION PROBLEMS
1. How many molecules are in 3.75 moles of carbon tetrachloride?
2. Determine the mass of 2.89 x 1024 molecules of HCl.
3. Calculate the number of nitrogen atoms in 65.5 grams of nitrogen gas.
4. How many carbon atoms are in 7.46 x 1025 molecules of propane, C3H8?
5. What is the mass in grams of 12 atoms of arsenic?
6. Calculate the percent by mass of phosphorus and oxygen in P2O5.
7. Calculate the percent by mass of chlorine and copper in copper(II) chloride.
4-3 EMPIRICAL FORMULA / MOLECULAR FORMULA Solve the following calculations. Use significant figures and show all work.
1. A sample of a compound is composed of 1.19 grams of gold and 0.642 grams of
chlorine. Determine the simplest formula ( empirical formula ) for the compound
and name the compound.
2. A compound is composed of 30.4% nitrogen and 69.6 % oxygen. The compound is
known to have a molecular mass of 92.02.
a. Determine the empirical formula of the compound.
b. Determine the molecular formula of the compound.
4-4 SOLUBILITY RULES
Assume that each of the following compounds is placed in water.
1) Based on the solubility rules, indicate whether the
compound is SOLUBLE or INSOLUBLE in water.
2) Write the formula for the compound in waterand use the
appropriate phase symbol (s) = solid or (aq) = aqueous.
Ex. sodium chloride SOLUBLE NaCl(aq)
1. calcium hydroxide
2. iron(III) nitrate
3. ammonium oxalate
4. potassium sulfide
5. copper(I) fluoride
6. chromium(II) acetate
7. lead(II) sulfate
4-5 MOLARITY CALCULATION PROBLEMS
Solve the following calculations involving molarity. Use the factor-label method
when necessary.
1. What is the molarity of 2.20 liter solution containing 16.89g of HCl ?
2. How many moles of H3PO4 are in 2.85 liters of 3.00 M H3PO4 solution ?
3. A certain chemical reaction requires 3.00 moles of sodium iodide. How many liters of a .125 M NaI
solution would be needed?
4. Calculate the number of milliliters of 2.50 M H2SO4 solution that contains 0.490 grams of H2SO4 ?
5-1 CHEMICAL EQUATIONS: PREDICTING PRODUCTS AND BALANCING
Complete and balance the following chemical equations, then identify the TYPE OF
REACTION as either SYNTHESIS, DECOMPOSITION, SINGLE REPLACEMENT, DOUBLE
REPLACEMENT, COMBUSTION, or WATER - FORMING. Write N.R. if no reaction occurs.
TYPE OF REACTION
1. Al + ZnCl2
2. C4H10 + O2
3. HNO3 + Mg(OH)2
4. MgCl2
5. Al + CaCl2
6. Na + O2
5-2 STOICHIOMETRY CALCULATIONS WITH MOLES, MOLAR MASS, AND
MOLARITY
For the following calculation problems, first write and balance the appropriate
chemical equation for the reaction described. Then, perform all necessary calculation
steps. Express all answers using the correct number of SIGNIFICANT FIGURES.
1. Acetylene, C2H2 , is a fuel used in the process of welding. Acetylene combines with oxygen in the
following combustion reaction:
2C2H2 + 5O2 4CO2 + 2H20
a. How many moles of oxygen gas are needed to completely burn 3.75 moles of acetylene?
b. Calculate the mass of carbon dioxide gas produced when 1.62 moles of oxygen react with acetylene.
2. In a combustion reaction aluminum reacts with oxygen to produce aluminum oxide. Write the balanced
equation for this reaction below.
a. Calculate the number of moles of aluminum oxide that can be produced from 17.4 grams of aluminum.
b. What mass (in grams) of aluminum oxide can be produced from 78.3 grams of oxygen gas ?
3. In a replacement reaction, magnesium reacts with hydrogen chloride (hydrochloric acid) to produce
magnesium chloride and hydrogen gas.
Mg + 2HCl MgCl2 + H2
a. How many milliliters of 3.00 M HCl are required to produce 5.37 g of magnesium chloride ?
b. Calculate the number of moles of hydrogen gas that can be formed using 65.0 milliliters of 2.75 M HCl .
4. a. What volume in milliliters of .25 M sodium chromate will react with 75.0 mL of .100 M copper (II)
chloride to form copper(II) chromate and sodium chloride ?
b. What mass (in grams) of sodium chloride can be produced from 75.0 mL of .100 M copper(II)
chloride ?
5. Hydrogen sulfate (sulfuric acid) reacts completely with aqueous sodium hydroxide. Write and balance
the equation for this double replacement reaction.
a. What volume in milliliters of 3.25 M sodium hydroxide is required to completely react with 75.0 mL of
4.38 M hydrogen sulfate ?
b. Calculate the mass in grams of sodium sulfate that can be produced when 75.0 grams of sodium
hydroxide reacts with 115.0 g of hydrogen sulfate. What is the percent yield if 125.0 g are produced?
5-3 LIMITING REAGENT / PERCENT YIELD
6. In a combustion reaction, 125 g of oxygen are combined with 85.0 g of ethane, C2H4.
a. Determine which reactant is in excess and which reactant is the limiting reagent.
b. Calculate the mass in grams of water that can be produced.
c. The experiment above is conducted and 45.0 grams of water is produced. Calculate the percent
yield.
6-1 TEMPERATURE / PRESSURE UNIT CONVERSION AND DALTON’S LAW
I. Convert the following quantities using the factor-label method as applicable.
Express all answers by using the correct number of significant figures.
a. Mercury boils at 629.7 K , what is this temperature on the Celsius (centigrade) scale ?
b. 96.8 degrees Fahrenheit = degrees Celsius
c. 625.4 degrees Fahrenheit = K
II. Solve the following problems according to Dalton’s law of partial pressures.
1. A mixture of gases (X,Y, and Z) has a total pressure of 378.3 kPa. If the pressure of gas A = 64.31 kPa
and the pressure of gas C = 2.804 atm, then what is the pressure of gas B in kilopascals ?
2. Nitrogen gas is collected over water at a temperature of 40 degrees Celsius ( v.p. of H2O = 7.38 kPa).
The water levels inside and outside the collecting bottle are equal at the end of the experiment.
Calculate the pressure of the nitrogen gas if the atmospheric pressure = 97.3 kPa.
6-2 THE GAS LAWS OF CHARLES, BOYLE, AND GAY-LUSSAC
Solve the following calculation problems.
1. Express all answers by using the correct number of significant figures.
2. Indicate the name of the gas law that applies to each problem. ( CHARLES’S
LAW, BOYLES’S LAW, GAY-LUSSAC’S LAW, OR COMBINED GAS LAW )
1. A sample of gas occupies a volume of 225 cm3 when a pressure of 478.1 mmHg is applied to it. What
will be the volume (in cubic centimeters) of the gas when the pressure is increased to 575.0 mmHg ?
Temperature of the gas is held constant.
GAS LAW
2. A 2.25 L sample of air collected at 30.0 º C has a pressure of .743 atm. Calculate the new pressure of
the gas if the temperature of the gas is raised to 65.7 º C and the volume expands to 3.15 L.
GAS LAW
3. 358 mL of nitrogen gas at standard temperature is heated to a temperature of 95.0 º C. Find the new
volume of the gas if the pressure is held constant.
GAS LAW
4. A sample of hydrogen gas at 48.5 º C has a pressure of 275.0 torr. If the gas is heated to 115.0 º C
what will be its new pressure ? (Volume is held constant.)
GAS LAW
6-3 THE IDEAL GAS EQUATION AND DETERMINING THE MOLAR MASS OF GASES
I. Use the ideal gas equation to solve the problems below. Express all answers using
the correct number of significant figures. Values for R are provided below.
R = .0821 L atm
R = 8.314 L kPaR =
62.4 L mmHg
mol K mol K mol K
1. How many moles of neon gas are there in a 54.85 L sample of gas at 46.2 ºC and 78.30 kPa ?
2. Calculate the volume of 2.58 g of chlorine gas at 1.140 atm pressure and standard temperature.
3. What is the mass in grams of 175.94 cm3 of dinitrogen monoxide gas at a temperature of 6.9 ºC and
at a pressure of 727.5 mmHg ?
II. Calculate the molar mass / molecular mass of the gases described in the problems
below.
4. A collecting bottle is known to contain 4.670 moles of gas “ X.” If the mass of the gas is 131 grams,
calculate the molecular mass of the gas.
5. Calculate the molar mass of a gas if an 8.06 x 10-2 gram sample of it occupies .0650 L at 574 ºC and
70.5 kPa .
6-4 MEASUREMENT UNIT CONVERSIONS S.I. / METRIC SYSTEM / BRITISH SYSTEM
Complete the following conversions using the factor-label method. Show all work and
express all answers using the correct number of significant figures.
Exact Conversions Conversions/ Not Exact
1 km = 1000 m 1 min = 60 s 1 mi = 5280 ft
1 m = 100 cm 1 h = 60 min 1 mi = 1.61 km
1 m = 1000 mm 1 h = 3600 s 1 m = 3.28 ft
1 yd = 3 ft 1 in = 2.54 cm
1 ft = 12 in
1. 38.4 cm2 = m2
2. 940.0 m3 = km3
3. 720 mm3 = nm3
4. 26.5 km/s = km/h
5. 233 mi/h = m/s
6. 9760 kJ/mol = J/cmol
7. 68.10 mi/h = km/h
6-5 KINETIC ENERGY
1. A molecule of dinitrogen tetroxide is moving at 638 m/s. The molecule has 1.05 x 10-17 J of energy. What is the
mass in kilograms of the molecule?
2. A single molecule of xenon tetrafluoride is moving at 125 m/s. Calculate the kinetic energy in joules of the
molecule.
6-6 CALCULATING TEMPERATURE AND vrms OF GASES
Solve the following calculations. Use the correct number of significant figures.
Boltzmann’s constant k = 1.38 x 10-23 kg m2
s2 K
1. For a lab sample of fluorine gas, the vrms is determined to be 16.3 m/s. Calculate the
temperature in degrees Celsius of the gas.
2. What is the root mean speed in m/s of the carbon dioxide molecules in the atmosphere on a day when
the temperature is 72.0 º F ?
6-7 GRAHAM’S LAW OF EFFUSION AND DIFFUSION
Solve the following calculations. Use the correct number of significant figures.
1. In an experiment, a sample of phosphorus pentachloride gas diffuses .844 times as fast as an unknown
gas. Calculate the molar mass of the unknown gas.
2. Which gas should effuse faster at the same temperature and pressure, carbon dioxide gas or oxygen
gas? How do you know ? Calculate the relative rate of effusion for carbon dioxide gas and
oxygen gas. State the answer in this sentence. ( “ gas effuses times as fast as
gas.”)
6-8 THE VAN DER WAALS EQUATION
(P + ) ( V - nb ) = n RTn2 a
V2
Gas van der Waals constants
nitrogen dioxide a = 5.284 b = 0.04424
1. At a pressure of 3.000 atm, a 2.00 mole sample of nitrogen dioxide gas occupies a volume of 6.00 L.
Use the Van der waals equation to calculate the temperature of the gas a) in kelvins and b) in
Celsius. c) When is the van der waals equation most applicable for a gas?
6-9 STANDARD MOLAR VOLUME AND GAS DENSITY
I. Solve the following calculation problems. Show all work and express answers
by using the correct number of significant figures.
1. A sample of carbon dioxide has a volume of 8.4 L at STP. Calculate the number of moles of carbon
dioxide in the sample.
2. What is the volume in dm3 of 22.13 grams of fluorine gas at STP ?
3. Calculate the mass of 15.73 L of krypton gas at STP.
II. Calculate the density of the gases below under the stated conditions.
1. Calculate the density in g / L of oxygen gas at standard temperature and standard pressure ?
2. What will be the density ( in g / L ) of neon gas at 98.51 kPa and 75.5 ºC ?
3. Calculate the density of ethene gas, C2H4 , at 50.0 ºC and 765 torr.
6-10 GAS STOICHIOMETRY
I. For each of the following chemical reactions, write and balance the chemical
equation and solve by using the factor-label method. Use the correct number of
significant figures in the answers.
1. In a combustion reaction at standard temperature and standard pressure, C2H6 reacts completely with
17.9 L of oxygen. What mass in grams of water vapor is produced?
2. In a replacement reaction at STP, solid iron reacts with aqueous hydrogen chloride to produce
aqueous iron (II) chloride and hydrogen gas. What volume in mL of 3.50 M hydrogen chloride is
required to produce 2.75 L of hydrogen gas at STP ?
3. Calcium chlorate decomposes to form calcium chloride and oxygen. What mass in grams of calcium
chlorate is required to produce 6.28 L of oxygen gas at STP ?
II. Reactions under nonstandard conditions
1. What volume in liters of carbon monoxide gas at 22.8 ºC and 121.6 kPa would be required to produce
18.36 grams of iron in the reaction below ?
Fe2O3 (s) + 3CO (g) 2Fe (s) + 3CO2 (g)
2. In a replacement reaction, aqueous potassium iodide reacts with chlorine gas to produce aqueous
potassium chloride and iodine gas. What mass in grams of potassium iodide is required to produce
7.48 dm3 of iodine gas at 35 ºC and 105.3 kPa ?
3. Aqueous hydrogen phosphate combines with aqueous sodium carbonate to produce aqueous sodium
phosphate, liquid water, and carbon dioxide gas. What mass in grams of hydrogen phosphate will
produce enough gas to fill a 854.2 mL container at 50.5 ºC and 765.0 mmHg ?
6-11 INTERPRETING A PHASE DIAGRAM
D
C
B
G
A
E
F
Temperature (in oC)
H
0 10 20 30 40 50 60 70 80 90 100 110
Identify the name for these points on the phase diagram
D = H = What is the normal boiling point?
I. Each statement below describes a point (A-H) that is found in the phase diagram
on the next page. Match the correct letter with its description. Use each answer
once.
1) This substance must be in the gas state at this point on the phase diagram
2) This substance can exist in the solid, liquid, and gas states at this point on the phase diagram
3) This substance must be in the liquid phase at this point
4) This substance exists as a liquid and as a gas but not as a solid under these conditions of
pressure and temperature
5) This combination of temperature and pressure is unique. Here, this substance exists as a
liquid and as a gas (not as a solid.) But, the temperature value of the substance at this point
represents the highest temperature point at which the substance can exist as a liquid.
6) This substance must be in the solid state under these conditions of pressure and temperature
7) Under these conditions of pressure and temperature, this substance exists as a solid and as
a gas but not as a liquid
8) When this combination of temperature and pressure conditions exists, this substance can
exist as a solid and as a liquid but not as a gas
II. Match the descriptions below with the process (a-g) they describe
a) evaporation c) deposition e) freezing g) boiling
b) condensation d) melting f) sublimation
1. What process occurs if the substance is at a constant pressure of 200 kPa
and the temperature is changed from 40 oC to 15 oC ?
2. What process occurs if the substance is at a constant temperature of 70 oC
and the pressure is changed from 150 kPa to 50 kPa ?
3. What process occurs if the substance is at a 100 oC and 50 kPa
and changes to 10oC ad 60kPa ?
4. What process occurs if the substance is at a 50 kPa and 40 oC
and changes to 35oC ad 150kPa ?
PHASE CHANGES AND INTERPRETING A PHASE DIAGRAM
III. Each of the two graphs below illustrates the change in temperature of a pure
substance over time. During the temperature changes, the substance is
undergoing phase changes. Answer the questions that follow the graphs.
Time (in min)
a
b c d
e
f g h
i
Time (in min)
j
k l m
n
o p q
r
In this graph, energy is being added released In this graph, energy is being added released
The temperature is increasing decreasing over time The temperature is increasing decreasing over time
1. the substance is in the solid state and its temperature is decreasing
2. substance is changing from a liquid to a gas and about half of it is converted
3. the substance is starting to melt
4. the substance is in the liquid state and its temperature is starting to increase
5. at this point the substance is beginning to condense
6. the substance is in the gaseous state and its temperature is starting to increase
7. the substance is a solid and its temperature is increasing
8. the substance is starting to boil at this point
9. at this point the substance is beginning to freeze
10. the substance is in the liquid state and its temperature is starting to decrease
7-1 IDENTIFICATION OF ATOMS AND IONS BY THEIR SUBATOMIC PARTICLES
I. Complete the following the following chart by filling in the appropriate word, symbol,
or number.
ELEMENT SYMBOL ATOMIC # OF PROTONS TOTAL NUCLEAR
NAME NUMBER IN THE NUCLEUS CHARGE
a. 16
b. + 74
c. 52
II. Complete the following by circling the appropriate underlined choice from each
pair of words and by filling in the correct number of electrons.
To change from Name of process
a. N to N-3 the atom / ion must gain / lose electrons. oxidation / reduction
b. O-2 to O the atom / ion must gain / lose electrons. oxidation / reduction
c. Fe+2 to Fe+3 the atom / ion must gain / lose electrons. oxidation / reduction
d. S-1 to S-2 the atom / ion must gain / lose electrons. oxidation / reduction
7-3 CALCULATING WEIGHTED AVERAGE ATOMIC MASS
1. Calculate the weighted average atomic mass of silver given the following data:
Isotope Natural Abundance Mass
107Ag 51.82 % 106.90509 amu
109Ag 48.18 % 108.9047 amu
2. Naturally occurring silicon is composed of the following three isotopes:
92.21% silicon-98 ( mass = 27.97693 amu) ; 4.70% silicon-29 ( mass = 28.97649 amu );
and 3.09% silicon-30 ( mass 29.97376 amu).
7-4 THE SUBATOMIC PARTICLES : NUCLIDES AND ISOTOPES
I. Complete the following chart by filling in the appropriate word(s), symbol,or number.
Assume that all particles are neutral in charge.
A B C D
Name
of carbon-14
Nuclide
Nuclear
Symbol
Atomic
Number 36
Z
Mass
Number 92
A
Number
of 9
protons
Number
of 144
neutrons
Number
of 92
electrons
Number
of 19
nucleons
element
name
II. THE NUCLIDES HAVE THE SAME NUMBER OF
a. 14C and 13C electrons protons neutrons nucleons
e. 39K and 39K+1 electrons protons neutrons nucleons
g. 80Sr+2 and 80Br -1 electrons protons neutrons nucleons
h. 108Sn and 105Ag electrons protons neutrons nucleons
i. 34P-3 and 34Cl -1 electrons protons neutrons nucleons
j. 22F-1 and 24Na+1 electrons protons neutrons nucleons
7-5 RADIOISOTOPES AND NUCLEAR EQUATIONS
I. Write the complete nuclear equation for each reaction below, including the mass
number and the atomic number for all reactants and products.
1. In a nuclear reaction, uranium-238 decomposes into thorium-234 and an alpha particle.
Which nuclide in your equation is the parent nuclide ? Which is the daughter nuclide ?
2. Write the nuclear equation for the alpha decay of protactinium-227.
3. Write the equation for the beta emission of neptunium-238.
4. Write the nuclear equation for the positron emission of arsenic-68.
5. Write the equation for the K electron capture by mercury-195..
6. Write the equation that represents the bombardment a magnesium-25 nucleus by an alpha particle. A
proton is released as one of the products.
What is the short form for this nuclear equation ?
7. Write the equation for the bombardment of the nucleus of sulfur-33 by a neutron if there are two
protons released from the nucleus as products.
What is the short form for this nuclear equation ?
8. Write the nuclear equation for 54Fe ( ! , 2p )
7-6 HALF-LIFE, ACTIVITY AND THE RADIOACTIVE DECAY LAW
Complete the following calculations. Show all work and use signficant figures.
1. a. The half-life of tin-121 is 27.0 hours. Calculate the decay constant for tin-121 (in h-1).
b. What is the activity ( in disintegrations/hour) of a 155 gram sample of tin-121?
(molar mass of tin-121 = 120.90 g/mole)
2. A 285.0 gram sample of neon-24 is prepared in a lab. What mass in grams of neon-24 will
remain in 22.0 minutes? (The radioactive decay constant for neon-24 is 0.205 min-1)
3. What fraction (percentage) of a sample of technetium-95 will remain after 155 days? (The half-life
of technetium-95 is 61.0 days.)
4. How long will it take for 57.0 % of a radioactive sample of phosphorus-32 to decay? (The half-life
of phosphorus-32 is 34.0 minutes .)
5. How long will it take for a radioactive sample of phosphorus-32 to decay down to the point that only
36.0% of the original sample remains? (The half-life of phosphorus-32 is 34.0 minutes .)
6. Imagine that the following reaction occurs. In a nuclear reaction, lead-204 is bombarded with 1
neutron. The daughter nuclides produced are zirconium-101 and molybdenum-104.
a. Write the balanced nuclear equation for the reaction below.
b. How much energy (in joules) is released in this nuclear reaction? (Assume that one mole is used)
Mass data : 1 neutron = 1.0087 amu molybdenum-104 = 103.91 amu
zirconium-101 = 100.92 amu lead-204 = 203.97 amu.
7-7 THE LINE EMISSION SPECTRA OF THE ELEMENTS
When electricity is passed through hydrogen gas, the gas glows with a lavender color.
This lavender color seen is actually a mixture of the many different wavelengths of
light emitted by the excited atoms. If this lavender “light” is viewed through a prism or
through diffraction grating, the light will break up (diffract ) into these different
wavelengths. ( " is given in nanometers ) Planck’s constant h = 6.626 x 10-34 J s
LINE EMISSION SPECTRUM FOR HYDROGEN
400 450 500 550 600 650 700 750
l l l l l l l l
l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l
l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l l
l l l l l l l l
400 450 500 550 600 650 700 750
I. Look at the four lines above. From left to right refer to the lines as LINE 1, LINE 2,
LINE 3, and LINE 4. Estimate the wavelength of each line (in nanometers )
LINE 1 LINE 3
LINE 2 LINE 4
2. Calculate the energy in kilojoules that was necessary to excite ELECTRON 1.
What amount of energy was released by ELECTRON A when it returned to ground state?
3. Calculate the frequency of the light seen in LINE 3
7-8 CALCULATING ENERGY OF PHOTONS : PLANCK’S THEORY
1. A photon of light has an energy of 2.780 x 10-19 J.
a. Calculate the frequency (in hertz)of the light.
b. Determine the wavelength (in meters) of the light.
8-1 ENERGY LEVEL DIAGRAMS AND ELECTRON CONFIGURATION
I. For each of the following atoms or ions, write the ground state electron
configuration and draw the energy level diagram.
a. carbon b. phosphorus
d. manganese f. zinc ion in zinc(II) phosphate
II. Identify the elements that have the following short form electron configurations.
1. [Ar] 4s2 3d6 3. [Ne] 3s2 3p3
2. [He] 2s2 2p5 4. [Xe] 6s2 4f14 5d10
III. For each of the following electron configurations identify the element symbol for
the atom represented, then classify the energy state of the atom as either “ground
state” or “excited state.” If the configuration is not possible write “impossible.”
1. 1s2 2s2 2p8 3s2 3p4 4s2
2. 1s2 2s2 2p6 3p4
3. [Xe] 6s2 4f14 5d10 6p4
4. [Ar] 4s2 3d14 4p2
8-2 QUANTUM NUMBERS
I. Write the symbol for the orbital (e.g. 5f, 3s, 9i, ...) that is described by the
following sets of principal and azimuthal quantum numbers. If an orbital is impossible
write IMPOSSIBLE.
a. n = 5 l = 0 orbital c. n = 5 l = 6 orbital
b. n = 3 l = 3 orbital d. n = 6 l = 3 orbital
II. Write the principal and azimuthal quantum numbers for these orbitals. Also,
indicate the maximum number of electrons that can have these quantum numbers in
one atom. # of # of electrons electrons
a. 3s n = l = c. 5p n = l =
b. 4d n = l = d. 6g n = l =
III. For each of the following atoms, indicate the number of valence electrons, the
principal quantum number for the energy level(s) in which the valence electrons are
located, and the letter that corresponds to the shell(s) in which they are located.
valence
short form # of valence energy shell
atom electron configuration electrons level(s) letter(s)
Ex. lithium [ He ]2s1 1 2 L
a. fluorine
b. cobalt
c. barium
d. lead
IV. Identify these categories of the Periodic Chart
a. alkali metals h. first transition series
b. alkaline earth metals i. second transition series
c. chalcogens j. third transition series
d. halogens k. fourth transition series
e. noble gases l. first inner transition series
f. lanthanide series m. second inner transition series
g. actinide series n.transuranium elements
V. Write possible quantum numbers for the following.
a. the electrons b. the valence electrons c. the electrons in the
of carbon of manganese 5p orbitals of antimony
VI. Indicate which of the following sets of quantum numbers are impossible by writing
IMPOSSIBLE next to it.Then, briefly state the reason why the set is impossible.
a. n = 6 l = 3 ml = -4 ms = - 1/2
b n = 5 l = 2 ml = -2 ms = + 1/2
c. n = 4 l = 0 ml = 1 ms = + 1/2
8-3 PERIODIC TRENDS: COVALENT AND IONIC RADII / IONIZATION ENERGY
I. Circle the atom in each pair that has the larger covalent radius.
a. potassium or calcium c. tellurium or oxygen e. tungsten or iron
b. chlorine or silicon d. fluorine or phosphorus f. copper or gold
1 . For the section above, State the periodic trend and explain why the trend is true.
II. Circle the atom or ion in each pair that has the smaller ionic radius.
a. Ca+2 or K+1 c. In+3 or Sb+5
b. N-3 or F-1 d. O-2 or Te-2
2. For the section above, state the trend and explain why the trend is true.
III. Circle the atom or ion in each pair which has the smaller radius.
a. Be or Be+2 c. Al+2 or Al+3
b. O or O-2 d. As-2 or As-3
3. For the section above, state a trend and explain why the trend is true.
IV. Circle the atom in each pair which has a higher first ionization energy.
a. Sr or Rb c. Rn or Ar b. O or In d. Ba or Zn
4. For the section above, state the periodic trend and explain why the trend is true
V. Circle the atom in each pair which has a higher electron affinity.
a. Sb or I d. Br or O
b. Rb or K e. Si or S
c. F or I f. S or Cl
6. Arrange the following sets of atoms in order of increasing first ionization energy.
ex. C F N C < N < F
a. O B C
b. Se F Zn
c. Sr Zr Cs
7. The data listed below provides the first, second, third, and fourth ionization
energies for five different elements:Elements from Group 1, Group 2, Group 13,
Group 17, and Group 18. Write the Group Number for each element in the
appropriate space.
symbol IE1 IE2 IE3 IE4
a. 577 kJ 1820 kJ 2740 kJ 19290 kJ
b. 417 kJ 3070 kJ 4440 kJ 5880 kJ
c. 1520 kJ 2660 kJ 3950 kJ 5770 kJ
d. 900 kJ 1760 kJ 14800 kJ 21000 kJ
e. 1140 kJ 2080 kJ 3560 kJ 4560 kJ
8. The electron affinities (in kJ/mol) for each of the following sets of atoms are given
in brackets. First, arrange each set of atoms in order of increasing electron
affinity. Then , write the correct electron affinity value above each atom.
-183 -185 -200
ex. {-200, -183, -185 } Se Te S Te < Se < S
a. {-116, -123, -120 } Si Ge C
b. {-53, -47, -83 } Na B Rb
8-4 ELECTROCHEMICAL CELLS AND ELECTROLYTIC CELLS
Based on the activity series, indicate which metal in each set would be metal
#1 and which would be metal #2 for the electrodes in thiselectric cell.
- +
M1 M2
electrochemical cell
ACTIVITY SERIES
Metals Nonmetals
Zn F
Cr Cl
Fe Br
Pt I
Au
a. zinc gold b. platinum chromium
Imagine that the diagram below represents an eletrolytic cell. Draw wires to
connect the battery terminals to the electrodes. Connect the positive terminal to T1.
T1 is the cathode / anode
T2 is the cathode / anode
electrolytic cell
+ - BATTERY
T1 T2
VI.Write equations for the electrolysis of the following compounds and indicate where
each product will form in the electrolytic cell pictured above. (at T1 or T2)
a. molten magnesium nitride
b. water
8-5 pH and pOH FOR STRONG ACIDS AND STRONG BASES
1. Calculate the hydronium ion concentration of a solution that has a pH of 4.11.
2. In a solution (at 25.0 degrees Celsius) the hydroxide ion concentration [OH-] = 3.16 x 10-11 M.
a) Calculate the [H3O+]
b) Calculate the pOH .
5. 0.575 grams of hydrogen chloride is dissolved in water. The total volume of the solution is 472.0 mL.
Calculate the pH of the acid.
6. In a titration experiment, perchloric acid is added to aqueous barium hydroxide. What volume
in milliliters of 3.50 M perchloric acid is required to neutralize 88.0 mL of 2.10 M strontium
hydroxide? (Be sure to write and balance the equation. Include the phase symbols)
9-1 LEWIS DOT DIAGRAMS : ATOMS AND IONIC COMPOUNDS
I. Write the, formulas, names, and Lewis dot diagrams for the ionic compounds formed
from the following elements.
ELEMENTS FORMULA NAME OF COMPOUND LEWIS DOT DIAGRAM
a. nitrogen and calcium
b. rubidium and sulfur
II. For each of the following atoms / ions write the short form electron configuration,
then draw the 3-D orbital diagram and draw the Lewis dot diagram.
1. calcium 2. boron 3. nitrogen
3-D diagram 3-D diagram 3-D diagram
1 Lewis dot diagram 2 Lewis dot diagram 3 Lewis dot diagram
9-2 ELECTRONEGATIVITY : PREDICTING BOND TYPES AND DIPOLES
I. Use the Pauling electronegativity values below to predict the type of bond that is
likely to form between atoms of the following pairs of elements, ( ionic, covalent,or
nonpolar covalent .) Then, when necessary, label the dipoles with the symbols
#+ and #-
B 2.0 H 2.1
Br 2.8 N 3.0
C 2.5 O 3.5
F 4.0 S 2.5
Fe 1.8 Li 1.0
1. B -------- F 2. Br -------- C 3. O -------- Li 4. H -------- HII. Circle the atom in each pair that has the greater electronegativity. ( Do not use the
Pauling values.)
a. aluminum or chlorine d. nitrogen or bromine
b. phosphorus or fluorine e. iodine or oxygen
c. iodine or chlorine
III. Label the dipole for the following covalent bonds by using the symbol .
If a bond is nonpolar then write “nonpolar” above it.
1. Al -------- Cl 2. F -------- P 3. Br -------- C 4. I -------- O
9-3 LEWIS DOT DIAGRAMS : MOLECULAR COMPOUNDS Draw Lewis dot
diagrams for the following molecules.
1. CH4 2. HCl 3. F2 4. CO2
5. O2 6. N2 7. NH3
# of bonds # of bonds # of bonds
# of lone pairs # of lone pairs # of lone pairs
Draw Lewis dot diagrams for the following polyatomic ions, then label the formal
charge for each atom.
8. sulfate 9. ammonium
IV. Draw resonance structures for the following molecules / ions and label the formal
charge for each atom.
a. sulfur dioxide b. nitrate ion
9-4 MOLECULAR GEOMETRY On another sheet of paper, draw the Lewis dot diagrams for the
following then complete the chart.
# OF # OF HYBRID-
ATOMS LONE IZATION NUMBER
BONDED PAIRS OF OF POLAR
TO CENTRAL (CENTRAL CENTRAL HYBRID SHAPE BOND OR
MOLECULE ATOM ATOM) ATOM ORBITALS NAME ANGLE(S) NONPOLAR
1 phosphate
2 H2O
3 IF7
4 CH3Br
5 CO2
6 XeF2
7 BCl3
8 ICl4-
9 chlorate
10 BeF2
11 SeCl4
12 BrF5
13 SF5I
14 PCl5
I. Identify the hybridization for each carbon atom in this diagram
F H H
Br C C C C C H
Cl O H
.
.
.
.
.
..
. C1 C2 C3 C4 C5
a)What type(s) of bond overlap exists for the C - F ?
b)What type(s) of bond overlap exists for the C2 to C3 ?
c)What is the bond angle for C3 to C4 to O ?
d) What is the bond angle for F to C1 to C2 ?
II. Draw energy level diagrams for the following. (Some of them were
already done in part 8-1 of this review)
carbon sulfur scandium manganese
magnesium ion zinc ion phosphide bromide
1) Which of the atoms or ions in PART I exhibit magnetic properties to some degree?
2) Which of the atoms or ions in PART I contain unpaired electrons?
How many unpaired electrons does each have?
3) Which of the atoms or ions in PART I are paramagnetic?
4) Which of the atoms or ions in PART I are diamagnetic?
Name
Write net ionic equations for the follow mixturesof aqueous solutions)
1. lead(II) chlorate + iron(II) sulfate
List the the spectator ions
2. chromium(II) iodide + barium acetate
List the the spectator ions
3. lithium hydroxide + calcium chloride
List the the spectator ions
I. Complete and balance these advanced equations.
1. N2O3 + H2O
2. H3PO3 heat
3. Ba(OH)2 heat
4. BeH2 + H2O
5. K + H2O
6. CaCO3 + HNO3
7. SrO + H2O
Final Exam Review Chemistry Answers to calculation problems and some others.
2-1 A) 8; 0; 5; 3; 5; 20 B) 9; 2; 5; 5; 4; 1
2-2 PbI2 lead(II) iodide NH4Cl ammonium chloride K2Cr2O7 potassium dichromate CoCO3 cobalt(II) carbonate
2-3 a) PbCl4 b) N2O c) AlCl3 d) PBr3 e) Cu2S f) Sr(OH)2
2-4 a) copper(II) sulfate b) chromium(III) oxalate c) calcium bromide
d) carbon tetrachloride e) sodium acetate f) sulfur trioxide
3-1 a) 5 b) 3 c) 2 d) 2 e) 2 f) 4
3-2 a) 8.4000 x 102 kg b) 4.76 x 10-4 mol c) 1.783 x 101 g d) 2.7 x 10-1 cm e) 6.30 x 10-3 L
3-3 a) 2.75 g/cm3 b) 250 g C (diamond) c) 1.20 x 105 g ethanol
3-4 1) molecule 2) ion 3) polyatomic ion 4) molecule 5) formula unit 6) atom
4-1 1) 199.88 g CaBr2 2) 566 g CaBr2 3) 3.82 x 10-7 mol N2O5 4) 5.47 x 1023 atoms S 5) 2.69 x 1023 atoms Au
4-2 1) 2.26 x 1024 molecules CCl4 2) 175.0 g HCl 3) 2.82 x 1024 atoms N 4) 2.24 x 1026
atoms C 5) 1.493 x 10-21 g As 6) 43.6% P ; 56.4% O 7) 52.7 % Cl; 47.3 % Cu
4-3 1) AuCl3 2) a. NO2 b. N2O4
4-4 1) soluble Ca(OH)2(aq) 2) soluble Fe(NO3)3(aq) 3) soluble (NH4)2C2O4(aq) 4) soluble
K2S(aq) 5) insoluble CuF(s) 6) insoluble Cr(C2O3O2)2 (s) 7) insoluble PbSO4 (s)
4-5 1) 0.210 M HCl 2) 8.55 mol H3PO4 3) 24 L NaI solution 4) 2.00 mL H2SO4 solution
5-2 1. a) 9.38 moles O2 b) 57.0 g CO2 2. a) 0.322 moles Al2O3 b) 166 g Al2O3
3. a) 37.6 mL HCl solution b) 8.94 x 10-2 moles H2 4. a) 30. mL Na2CrO4 solution
b) 0.877 g NaCl 5. a) 202 mL NaOH solution b) 133.6 g Na2SO4 93.56% percent yield
5-3 6. a) O2 is the limiting reagent b) 46.9 g H2O c) 95.9 %
6-1 a) 356.6 oC b) 36.0 oC c) 602.9 K 1) 29.9 kPa 2) 89.9 kPa
6-2 1) 187 cm3 Boyle’s Law 2) 0.593 atm Combined Gas Law 3) 483 mL Charles Law
4) 331.8 torr Gay-Lussac’s Law
6-3 1) 1.617 moles Ne 2) 0.716 L Cl2 3) 0.322 g N2O 4) 28.1 g/mole 5) 124 g/mole
6-4 1) 3.84 x 10-3 m2 2) 9.400 x 10-7 km3 3) 7.2 x 1020 nm3 4) 95400 km/h 5) 104 m/s
6) 97600 J/cmol 7) 110. km/h
6-5 1) 5.16 x 10-23 kg 2) 2.69 x 10-21 J
6-6 1) -272.75 oC 2) 409 m/s
6-7 1) 149 g/mole 2) 1 17 oxygen gas effuses 1.17 times as fast as carbon dioxide.
6-8 1) -144 oC
6-9 1) 0.38 moles CO2 2) 13.1 dm3 F2 3) 58.85 g Kr II. 1) 1.43 g/L 2) 0.6857 g/L 3) 1.07 g/L
6-10 I. 1) 12.3 g H2O 2) 70.2 mL HCl solution 3) 19.3 g Cu(ClO3)2
II. 1) 9.979 L CO 2) 102 g KI 3) 2.12 g H3PO4
7-3 1) 107.87 amu 2) 28.09 amu
7-5 Only the product (daughter nuclide) is listed for each reaction:
1) thorium-234 2) actinium-223 3) plutonium-238 4) germanium-68 5) gold-195
6) aluminum-28 7) silicon-32 8) iron-56
7-6 1. a) 0.0257 h-1 b) 1.98 x 1022 dis/h 2) 3.13 g Ne-24 3) 10.8 %
4) 41.1 minutes 5) 50.0 minutes 6 b) 1.4 x 1013 joules
7-7 2) 4.82 x 10-22 kJ 3) 6.15 x 1014 Hz
7-8 1) 4.20 x 1014 Hz 2) 7.14 x 10-7 m
8-5 1) 7.76 x 10-5 M 2. a) 3.16 x 10-4 M b) pOH = 10.5 5) pH = 1.48
OXIDATION - REDUCTION (REDOX) STOICHIOMETRYName
Date Period
Complete the following, showing all work and using significant figures.
1. A 75.00 mL solution containing I- ions is titrated with 0.550 M NaClO3 solution. It required
35.00 mL to reach the equivalence point, oxidizing all the iodide ions to iodine by the following reaction:
6H+ (aq) + ClO3
-1(aq) + 6I- (aq) ===> Cl- (aq) + 3I2 (aq) 3H2O (l)
b) How many moles of chlorate, ClO3-1, reacted at the equivalence point? . .0193
b) How many moles of iodide, l-1, reacted at the equivalence point? .116
c) What was the concentration of the I- ions in the solution that was titrated? 1.55 M
d) What is the concentration of the iodine solution that is produced? .526 M
c) Identify the following:
the oxidized substance the oxidizing agent
the reduced substance the reducing agent
2. 0.500 g oxalic acid reacts with 50.0 mL of 0.0200 M KMnO4 solution in acidic solution in the following equation: #54 p 178
acid
6H+(aq) + 2MnO4
-1(aq) + 5H2C2O4 (aq) ===> 2Mn+2
(aq) + 10CO2 (g) + 8H2O (l)
a) Identify the limiting reactant and the reactant that is in excess in this reaction.
LR = MnO4-
b) What is the amount of the excess in moles? 3.05 x 10-3 moles
c) What mass in grams of carbon dioxide will be produced? .220 g
d) What will be the concentration of the aqueous substances remaining in the final solution after the reaction has occurred? .0610 M & .0100 M
BALANCING REDOX EQUATIONS
i) In the unbalanced equation, label the oxidation numbers above each element symbol.
ii) Beneath each appropriate element, label the following terms: “oxidized” , “reduced” , “oxidizing agent” and “reducing agent”.
iii) Below each unbalanced equation, balance each equation by the half reaction method.2. Assume that the following reactions occur in acidic solution.
a) Cr2O7-2(aq) + Cl- (aq) Cr+3 (aq) + Cl2 (g)
(Ans 14 H+ + 6 Cl- + Cr2O72- ===> 2 Cr+3 + 3Cl2 + 7 H2O)
b) MnO4-1(aq) + S-2(aq) MnS (s) + S (s)
(Ans 8 H2O + 5S-2 + 2MnO4- ===> 5S + 2 Mn+2 + 16 OH-)
DETERMINING HEAT OF REACTION BY CALORIMETRY
3.000 L (3000. kg) of 2.00 M calcium hydroxide solution at 25 oC is neutralized by
4.000 L (4000. kg) of hydrochloric acid at 25 oC in a calorimeter and the temperature
increases to 60.0 oC.
*Assume that the calorimeter only absorbs a negligible amount of heat and assume that the specific heat capacity of the solution(s) is 4.18 J/ oC.g, and that the densityof the solution(s) is 1.0 g/mL.
Ca(OH)2 + 2HCl ===> 2H2O + CaCl2
i. Calculate the heat that is released by this reaction.
ii. What is the limiting reagent in this reagent...How do you know?
Calculate the number of moles of product produced in this reaction.
iii. Calculate the enthalpy change in kJ mol-1 of product formed in this reaction.
iii. Calculate the enthalpy change in kJ mol-1 of calcium hydroxide for his reaction.
iii.Calculate the value of the molar enthalpy of neutralization !Hneut for this reaction kJ/mol.
Ca(OH)2 + 2HCl ===> 2H2O + CaCl2 !H ° =
BOMB CALORIMETRY
11. A 12.0 gram sample of gasoline is burned in a bomb calorimeter, releasing 250 kJ of heat. The temperature of the calorimeter increases from 25.0 to 80.0 degrees Celsius.
a) What is the heat capacity (the calorimeter constant) for this bomb calorimeter? 4.5 kJ/oC
b) What is the energy of combustion for gasoline in kJ per gram ? - 21 kJ/g
12. A 0.1964 g sample of quinone (C6H4O2; molar mass is 108.1 g/mol) is burned in a bomb
calorimeter
that has a heat capacity of 1.56 kJ oC-1. The temperature of the calorimeter increases by 3.2 oC.
a (i) Calculate the quantity of heat that is absorbed by the calorimeter in this experiment. 5.0 kJ
(ii) Calculate the energy of combustion per gram of quinone. -25 kJ/g
(iii) What is the enthalpy change if 2.5 moles of quinone is burned? -6800 kJ
CALCULATIONS INVOLVING GIBBS FREE ENERGY !G
Name________________
Date_______ Period ___ 1)
(a) -2 x 103 J
(b) 1 x 104 J
(c) 5050 J
(a) 10000 J
2)
HESS!S LAW Name________________
Date_______ Period ___
For each of the following calculation problems show all work and express all answers by using the correct number of significant figures.
1.
"H = -58.0 kJ
2.
"H = 226 kJ
STANDARD ENTHALPIES OF FORMATION Name________________
Date_______ Period ___
For each of the following calculation problems show all work and express all answers by using the correct number of significant figures.
1.
(a)"H = -1235 kJ/mol(b)"H = -20. kJ/mol
