Irvington High School  AP Chemistry
Mr. Markic
Name _______________________________
Number ___ Date ___/___/___
2  Atoms, Molecules, and Ions
Station 1 – NAMING COMPOUNDS FROM FORMULAS
Name the following compounds:
Formula
Name
BF3
SF6
(NH4)2Cr2O7
PbCO3
NI3
Station 2 – WRITING FORMULAS FROM NAMES
Write the formulas for the following compounds:
Name
Dinitrogen pentoxide
Aluminum oxide
Stannic sulfate
Oxygen difluoride
Carbon tetrachloride
Formula
Station 3 – MINI MEGA-ION QUIZ
Fill in the symbol and charge for each of the following ions:
ferric
sulfite
hydronium
permanganate
silver
hydroxide
sulfide
thiosulfate
cupric
phosphate
hypoiodite
mercurous
calcium
nickel
cyanide
Station 4 – MYSTERY IONS
Use your knowledge of ions and a little logic to answer the following questions:
Sodium arsenide has the formula: Na3As. What is the formula for magnesium arsenide? _____________
Gold sulfide has the formula: Au2S3. What is the formula for gold chloride? __________
Calcium oxalate has the formula: CaC2O4. What is the formula for aluminum oxalate? ___________
Station 5 – % COMPOSITION
Use your periodic table and calculator to determine the % composition (by mass) of each element in:
Note: Give your answers to 1 decimal place.
Formula
%Ca
%C
%N
Ca(CN)2
Calculation Area:
Station 6 – EMPIRICAL FORMULA FROM % COMPOSITION
Determine the empirical formula of the compound from the following %composition (by mass) information:
A compound composed of carbon and hydrogen is found to contain 85.6% C and 14.4% hydrogen by mass.
What is the empirical formula of the compound? ____________
Calculation Area:
Station 7 – MOLE PROBLEMS
Solve the following problems. Show your work using dimensional analysis:
A 2.00 Liter bottle is filled with XeF4 gas. What is the mass of the gas sample? [MM XeF4 = 207.30 g/mol]
How many molecules of CO2 make up a 5.25 g chunk of dry ice? [MM CO2 = 44.01 g/mol]
Station 8 – IDENTIFY MYSTERY SUBSTANCE
When asked to identify a mystery compound, it is often useful to determine the molar mass of the substance.
Use the following information to identify the mystery substance:
A 1.25 Liter sample of a diatomic gas, measured at STP, has a mass of 3.96 grams.
What is the identity of the gas? ______
Station 9 – HYDRATE LAB
A student is assigned the task of determining the number of moles of water in one mole of MgCl2 · n H2O.
The student collects the data shown in the following table.
Mass of empty container
Initial mass of sample and container
Mass of sample and container after first heating
Mass of sample and container after second heating
Mass of sample and container after third heating
Determine the moles of water lost when the sample was heated.
Determine the formula of the hydrated compound.
22.347 g
25.825 g
23.982 g
23.976 g
23.977 g
3  Mass Relationships in Chemical Reactions
Station 1 – COMBUSTION EQUATIONS
Write balanced equations for the complete combustion of the following fuels:
Fuel
Combustion Equation
C3H8
C6H14
CH3OCH3
Station 2 – BALANCING EQUATIONS
Balance the following chemical equations:
__KClO3(s)  __KCl(s) + __O2(g)
__Fe(s) + __Cl2(g)  __FeCl3(s)
__Pb(NO3)2(aq) + __AlCl3(aq)  __PbCl2(aq) + __Al(NO3)3(aq)
Station 3 – PHASES
From the statement, decide whether each substance should be labeled with (s), (l), (g), or (aq):
Pure rubbing alcohol is C3H7OH( ).
Copper metal is Cu( ).
A solution of cupric chloride is CuCl2( ).
Melted iron is Fe( ).
Salt water is NaCl( ).
Helium is He( ).
Dry ice is CO2( ).
Steam is H2O( ).
Station 4 – EMPIRICAL FORMULAS
Determine the molecular formula given the following information:
Empirical Formula
Molecular Formula
Molar Mass
CH2
84.18 g·mol-1
NO2
92.02 g·mol-1
NaSO2
174.14 g·mol-1
PCl3
137.32 g·mol-1
Station 5 – STOICHIOMETRY
Solve the following general stoichiometry problems:
(Show work beautifully.)
N2(g) + 3H2(g)  2NH3(g)
[Molar Masses: 28.02 g·mol-1
2.02 g·mol-1
17.04 g·mol-1]
Calculate the mass of ammonia, NH3, formed when 45.0 L N2(g) reacts with excess H2(g) at STP.
What mass of H2 is needed to completely react with 10.0 grams of N2?
Station 6 – LIMITING REACTANT PROBLEMS
Solve the following problem:
N2(g) + 3H2(g)  2NH3(g)
[Molar Masses: 28.02 g·mol-1
2.02 g·mol-1
17.04 g·mol-1]
What mass of NH3 is formed when 135.00 g N2 reacts with 32.00 g H2?
Station 7 – LABORATORY PROBLEM
Using the following data, determine the best ratio of the chemical reaction:
___X + ___Y  Z + heat
Various mixtures of X and Y were mixed. A thermometer was used to record the temperature of the mixture.
The highest temperature reached for each mixture was recorded in the table below.
Circle the mixture in the data table that released the most heat.
Determine the stoichiometric ratio for X and Y (write in the coefficients in the equation above).
Volume X
(mL)
0
20
40
60
80
100
Volume Y
(mL)
100
80
60
40
20
0
Max Temp Measured
(°C)
20.0°C
25.0°C
30.0°C
35.0°C
27.5°C
20.0°C
In the mixture of 20 mL X and 80 mL Y, ______ was the limiting reactant.
Station 8 – PERCENT YIELD
Solve the following problem:
Hydrogen gas was generated according to the equation: Zn(s) + 2HCl(aq)  H2(g) + ZnCl2(aq)
When 25.00 grams of Zn metal reacted with excess HCl 7.50 L H2(g) was collected at STP.
The theoretical yield of H2(g) for this reaction is: (show work)
The percentage yield for this reaction is: (show set-up)
Station 9 – CHEMICAL ANALYSIS
Solve the following problem:
A compound composed of carbon and hydrogen is analyzed by combustion.
When a 4.297 g sample of the compound is burned, 12.57 g CO2 and 7.72 g H2O are formed.
What is the empirical formula of the compound? ________________
The molar mass of the compound is found to be about 30 g·mol-1.
The molecular formula for the compound is _________________
4  Chemical Equations and Stoichiometry
Station 1 – ACIDS, BASES, AND NEUTRALS
Classify each statement as talking about an [A]cid, [B]ase, or [N]eutral.
_____
feels slippery
_____
CH3OH
_____
tastes sour
_____
turns “phenol red solution” yellow
_____
KOH
_____
increases [OH-]
_____
turns cabbage juice red
_____
increases [H+]
_____
tastes bitter
_____
H2SO3
_____
cabbage juice stays purple
_____
NaHCO3
Hint: only one of these is neutral.
Station 2 – SOLUBILITY RULES
Circle the ionic compounds that are Insoluble (i.e. circle the precipitates):
MgF2
CuSO4
NH4Cl
Fe(OH)3
CsF
AgCl
CdS
CuF2
PbSO4
Ba(OH)2
Na2SO4
NH4OH
Sr(NO3)2
Hg2I2
Na2CrO4
BaCO3
PbBr2
CaC2O4
HC2H3O2
MgO
Station 3 – WRITE THE IONIC EQUATION
For the following molecular equations, write the ionic equation and underline out the spectators:
HF + NaOH  NaF + H2O
CuSO4 + Sr(NO3)2  Cu(NO3)2 + SrSO4
2HCl + BaSO3  BaCl2 + H2O + SO2
Station 4 – PREDICT THE PRODUCTS
Predict the products in these molecular equations. Indicate (s), (l), (g), or (aq):
CuSO3 + HF
Ca(NO3)2
HCl

+ (NH4)2SO4
+ Zn(C2H3O2)2


Station 5 – NAMING ACIDS
Fill in this chart:
Anion name
Anion formula
Acid formula
Acid name
cyanide
chlorate
hypochlorite
sulfide
sulfate
sulfite
nitrate
acetate
Station 6 – RECOGNIZING OXIDATION-REDUCTION
For each statement, classify the change of the underlined element as [O]xidation, [R]eduction, or [N]either:
_____ `Cu°  Cu2+ + 2e_____ Al3+ + 3e-  Al°
_____ CH4  CO2
_____ NaOH + HCl  NaCl + H2O
_____ gaining electrons
_____ oxidation number increases
_____ Zn° + 2HCl  ZnCl2 + H2
_____ Mg + ½O2  MgO
Station 7 – OXIDATION NUMBERS
Determine the oxidation number of the underlined element:
MgF2
CuSO4
NH4+
CO2
AgCl
Cr2O72-
ClO3-
SiH4
Station 8 – MOLARITY PROBLEMS
Solve the following problems:
A 2.00 mole sample of NaOH is dissolved in enough water to make 500. mL of solution. What is the
concentration of the solution?
60.0 grams of NaOH (MM = 40.00 g·mol-1) is dissolved in enough water to make 0.750 L of solution. What is
the concentration of the solution?
A 250. mL sample of a 0.125 M solution of NaOH contains ________ grams of NaOH.
Station 9 – DILUTIONS AND STOICHIOMETRY
Show your work for these problems:
You need to make 2.00 L of 0.200 M HCl.
What volume of concentrated HCl (11.65 M) should you dilute? ___
Given the equation: Al2O3(s) + 6 HCl(aq)  3 H2O(l) + 2 AlCl3(aq)
What volume of 0.250 M HCl is needed to completely react with 25.0 grams Al2O3 (MM =101.96 g·mol-1).
STOICHIOMETRY
Balance these equations and classify their type (single replacement, double replacement, etc.)
__C5H12 + __O2  __CO2 + __H2O
Classify this reaction: ______________________
__H2O2  __H2O + __O2
Classify this reaction: ______________________
__AgNO3 + __K2CO3  __Ag2CO3 + __KNO3
Classify this reaction: ______________________
Solve the following mole problems:
How many grams of CO2 (MM = 44.01) are produced when 11.0 grams of C5H12 (MM = 72.17) burn?
Consider the balanced equation: N2(g) + 3 H2(g)  2 NH3(g)
molar masses:
(28.02)
(2.02)
(17.04)
How many grams of NH3(g) is formed when 10.0 grams of H2(g) reacts with 50.0 grams of N2?
5  Gases
Review Topic 1: Pressure
and
Partial Pressure
1 atm = 760 mmHg = 760 torr = 14.7 psi = 101.3 kPa
Make the following conversions: (Show your work)
550 mmHg x ____________ =
325 kPa x ____________ =
kPa
atm
55 psi x ____________ =
2284 torr x ____________ =
mmHg
kPa
125.0 g of CH4 and 15.00 g of He are placed in a rigid container. The total pressure of the gas mixture is 1.45
atm. What is the partial pressure of each gas?
Review Topic 2: Root Mean
Square
Calculate the root mean square velocity of a sample of SF6 gas at room temperature (21.0 °C).
Review Topic 3: Graham’s Law
1 mole each of He gas and CO2 gas are in a rigid container at the same temperature.
The kinetic energy of He is ________________ (greater than, less than, the same as) the kinetic energy of CO2?
The velocity of He is ________________ (greater than, less than, the same as) the kinetic energy of CO2?
Calculate the ratio of the velocities of He/CO2.
When HCl(g) and NH3(g) come in contact, they form a white solid, NH4Cl(s).
If samples of the two gases are placed at the ends of a tube, the white solid will appear closest to point ___?
HCl
a
b
c
d
e
NH3
Review Topic 5: Gas Law Problems
Solve the following problems:
___________ 1. A balloon at 35.0C and 0.980 atm has a volume of 12.5 L.
What is its volume at 75.0C and 150. kPa?
___________ 2. A balloon has a volume of 1.00 L at 21.0C and 750. mmHg.
What is the balloon’s volume at STP?
Review Topic 6: Kinetic Molecular Theory
Explain the following observations in terms of the “kinetic molecular theory” (that is, what do the gas particles
look like?)
A balloon of gas is placed in a car on a hot day. The balloon gets larger. Explain.
A syringe is squeezed so the gas sample changes from 10 cc to 5 cc. The pressure doubles. Explain.
Review Topic 7: Ideal Gas Law
A 0.00195 mole sample of CO2 has what volume (in Liters) measured at 27.0C and 740 mmHg?
P=
V=
n=
R=
T=
How many moles of CO2 gas will fit into a 2.00 Liter soda bottle at 35.0°C and 0.990 atm?
P=
V=
n=
R=
T=
Review Topic 8: Molar Mass
Calculate the molar mass of a gas sample if 3.00 grams of the gas in a 2.00 L container at 25.0C has a pressure
of 2.294 atm.
What mass of chlorine gas, Cl2, is needed to fill a 10.0 L container at 100.°C and 775 torr?
PROPERTIES OF GASES
What is the mass of a 84.50-Liter sample of helium (MM= 4.00) measured at 20.0C and 700. mmHg?
How much faster does a molecule of He travel than a molecule of SO2 (MM = 64.07)?
A balloon with a volume of 2.50 L at 20.0 and 745 mmHg would have what volume at STP?
Review Topic 9: Molar Volume Lab
Information:
volume of gas at room conditions: 45.0 mL
length of Mg used: 4.65 cm
mass of 1.00 m of Mg: 0.958 g
room temperature: 22.0°C
room pressure: 751 mmHg
water vapor pressure at 22.0°C = 19.8 mmHg
How many moles of magnesium were used? Show work.
What is the molar volume of this hydrogen gas sample under room conditions? Show work.
What is the molar volume of this hydrogen gas sample at STP? Identify the variables and show work.
P1=
P2=
V1=
V2=
T1 =
T2=
6  Thermochemistry
Station 1 – EXOTHERMIC AND ENDOTHERMIC
Classify each statement as talking about an [EXO]thermic or [ENDO]thermic reaction:
_____
surroundings get hot
_____
H is negative
_____
PE diagram is uphill
_____
PE diagram is downhill
_____
energy is a product
_____
surroundings get cold
_____
H is positive
_____
products have more energy
_____
reactants have more energy
_____
energy is a reactant
Station 2 – HEAT CALCULATIONS
A 45.0 mL sample of water is heated from 15.0°C to 35.0°C. How many joules of energy have been absorbed
by the water? (Show work)
If 5430 J of energy is used to heat 1.25 L of room temperature water (23.0°C), what is the final temperature of
the water?
Station 3 – HOT AND COLD OBJECTS
A 100. gram sample of aluminum (specific heat = 0.900 J·g-1·°C-1) in boiling water is added to an insulated cup
containing 50.0 grams of water at 5.00°C. What will the final temperature of the mixture be? The specific heat
of water is 4.184 J·g-1·°C-1.
ENERGY & HESS’S LAW
Calculate the standard enthalpy of the reaction for the process
3NO(g)  N2O(g) + NO2(g)
using the standard enthalpies of formation (Hf): NO = 90 kJ/mol; N2O = 82.1 kJ/mol; NO2 = 34.0 kJ/mol
How much energy is required to change the temperature of 2.00 g aluminum from 20.0C to 25.0C?
The specific heat of aluminum is 0.902 J/gC.
Station 5 – HEATS OF FUSION & VAPORIZATION
Knowing that the Hfus for water is 6.02 kJ·mol-1, calculate the following:
How much energy (in kJ) is absorbed by 45.0 g or ice as it melts?
What mass of ice can be melted with 75.0 kJ of energy?
Station 6 – H FROM DATA
When 10.0 grams of C5H12 is burned, 453 kJ of energy is released.
What is the Hcombustion for C5H12?
When 10.0 grams of aluminum melts, 3.929 kJ of energy is required. What is the Hfus of Al?
Station 7 – HESS’S LAW—LONG VERSION
Iron ore can be converted to iron metal with CO gas.
FeO (s)  CO (g)  Fe (s)  CO2 (g)
Calculate the standard enthalpy change for this reaction from these reactions
of iron oxides with CO :
(1) 3 Fe2O3 (s)  CO (g)  2 Fe3O4 (s)  CO2 (g)
(2) Fe2O3 (s)  3 CO (g)  2 Fe (s)  3 CO2 (g)
H  - 47 kJ
H  - 25 kJ
(3) Fe3O4 (s)  CO (g)  3 FeO (s)  CO2 (g)
H  19 kJ
Station 8 – HESS’S LAW--SHORTCUT
CO2(g)
H2O(g)
chemical
-1
-393.5
kJ·mol
-241.8
kJ·mol-1
Hf
C5H12(l)
-173.1 kJ·mol-1
C2H5OH(l)
-277.6 kJ·mol-1
Given the above Hf°’s, calculate the Hcombustion of pentane, C5H12.
Calculate the Hcombustion of ethyl alcohol, C2H5OH(l)
Station 9 – MORE HESS’S LAW
CO2(g)
chemical
-393.5 kJ·mol-1
Hf
H2O(g)
-241.8 kJ·mol-1
C8H18(l)
??? kJ·mol-1
Knowing that the Hcombusion of octane, C8H18, is -5508.9 kJ·mol-1 calculate the Hf of octane.
7  Electronic Structure of Atoms
Station 2 – VIEWING SPECTRA
Using the triangular spectrometers, look at the provided light source.
The wavelength of light viewed ranges from 400 nm to 700 nm.
What is the wavelength of the GREEN light? _______________
Calculate the frequency of the green light.
Consider the spectrum below. It is an _____________________ (emission/absorption) spectrum.
Explain what the electrons are doing to produce the black lines:
Station 3 – ENERGY CALCULATIONS
H-O-O-H
The energy required to break the O - O bond in hydrogen peroxide, H2O2(g), is 139 kJ mol-1.
How much energy is needed to break one peroxide bond (in Joules)? (Show work)
Blue light has a wavelength of about 475 nm. Does this light have enough energy to break the bond? _____
Justify your answer with calculations.
Station 4 – SHELLS, SUBSHELLS & ORBITALS
Circle the subshells that do NOT exist:
4p 1p 2f 5s
_____ The number of orbitals in a 4d subshell.
_____ The number of orbitals in the n=2 shell.
_____ The number of subshells in the n =5 shell.
_____ The number of orbitals in a 4f subshell.
_____ The number of subshells in the n =3 shell.
3d
7p 2d 3s
Station 5 – WAVE CALCULATIONS
c = 2.998 x 108 m/s
h = 6.626 x 10-34 J·s
The color orange has a wavelength of 615 nm.
Calculate the frequency of this light.
Calculate the energy of a photon this light.
A radio station broadcasts at a frequency of 590 KHz (590 x 103 Hz).
What is the wavelength of the radio waves?
Station 6 – THE BOHR ATOM
c = 2.998 x 108 m/s
h = 6.626 x 10-34 J·s
Sketch the Bohr atom from levels n=1 to n=5.
Rhc = 2.18 x 10-18 J
R = 1.0974 x 107 m-1
Show the transition that would give off blue-green light.
Calculate the energy of level n=4.
Calculate the energy change of an electron that drops from
level 4 to level 2.
An electron that moves from n=1 to n=5 would _________
(gain / lose) energy and produce an _______________
(absorption / emission) spectrum.
Station 10 – Electron Configurations
Fill in the orbital diagram for S.
Fill in the orbital diagram for Cu.
Write the short form and long form electron configurations for S and Cu.
e CONFIGURATION &
Fill in this chart:
PERIODICITY
Fill in the orbital diagram for As (#33)
atom
mass
# p+
# n
# e4s
Na
23
3s
24
12
4p
3d
3p
2p
2s
9
10
1s
Mg
2+
24
What energy is needed to move an electron in a
hydrogen atom from level 1 to level 5?
Which element has the largest ionization energy?
N, O, P, S
8  Periodic Properties of Elements
STATION 1 – ORBITALS AND ELECTRONS
1. The number of electrons that can occupy a 3d orbital is _____.
2. The highest energy orbital in boron, B, is _____.
3. The orbital farthest from the nucleus in Cr is _____.
4. The number of orbitals when n=3 is _____.
5. The number of electrons that have n=2 is _____.
6. The orbital that fills after the 6s is _____.
7. Circle the orbital representations that could exist: 4s3
5g18
3p4
2p8
8. When Zn becomes an ion, it loses its electrons from the _____ orbital.
6d3
1s1
7f15
STATION 3
– THE PERIODIC TABLE
Write in the last orbital filled in each zone of the periodic table.
1
18
2
13
Circle the following element(s) that would be paramagnetic: Zn
STATION 4
– IONIZATION
The Period 3 Elements are:
Na
Mg
Al
Mg
14
Mn2+
N
15
16
17
O2- Co2+
ENERGY
Si
P
S
Cl
Ar
Which Period 3 element has the following five ionization energies? _____
IE1
IE2
IE3
IE4
736 kJ
1445 kJ
7730 kJ
10,600 kJ
IE5
13,600 kJ
Which Period 3 element has the following five ionization energies? _____
IE1
IE2
IE3
IE4
787 kJ
1575 kJ
3220 kJ
4350 kJ
IE5
16,100 kJ
Which period 3 element has the largest 3rd ionization energy? ______
STATION 5
–
TRENDS IN IONIZATION
ENERGY
For each pair of elements, circle the element with the larger ionization energy:
F & Cl
Na & Be
Mg & Al
N&O
C&O
Which element, Mg or Ca has the larger first ionization energy? _____ Explain.
Write the equation for the first ionization of Mg: _________________________________________
Write the equation for the first ionization of Cl: _________________________________________
STATION 6
–
GRAPHED
IONIZATION ENERGIES
This is a graph of the ionization energies for the
first 20 elements by atomic number.
Determine which families are W, X, and Y:
W is the ____________________ family and the
____________________ family.
X is the ____________________ family.
Y is the ____________________ family.
STATION 7 – ELEMENTS & ELECTRON CONFIGURATIONS
Identify the elements with the following electron configurations:
1s2 2s2 2p6 3s2 3p6 4s2
[Ne] 3s1
[Ar] 4s2 3d6
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p5
[Kr] 4d7 5s2
[Xe] 6s2 4f4
1s2 2s2 2p6 3s2 3p6 3d5 4s1
Write the long form electron configuration for Fe3+:
STATION 9 – TRENDS IN SIZE
For each pair of elements, circle the element with the larger atomic radius:
Mg & Ca
N&O
Sn & As
K & K+
I and I
As you move down a family (column) of elements, the atomic radius _____________ (increases, decreases)
because ____________________________________________________________________________.
As you move across a period (horizontal row) of elements, the atomic radius __________ (increases, decreases)
because ____________________________________________________________________________.
Put these five elements in order from smallest atomic radius to largest atomic radius. F Br Ca K Cs
Smallest
Largest
10  Molecular Geometry & Bonding Theories
Station 1 – BOND TYPES
State the type of bond (covalent, ionic, or metallic) that will form from each pair of elements:
Type
Type
Mg F
Ag Cu
K Na
Xe F
S
Cl
H
Li
O
Br
Cl
I
Match the statement with the type of bonding:
____
Electrons are close to two nuclei, lowering the energy of the system
I.
Ionic
____
Electrons are transferred, the two oppositely charged atoms attract
M.
Metallic
____
Electrons are delocalized and move from atom to atom
C.
Covalent
Station 2 – ELECTRONEGATIVITY
WITHOUT LOOKING AT THE CHART, fill in the following values for electronegativity:
H
F
O
N
Cl
S
For each pair of elements, state whether the bond is Ionic (I), Polar Covalent (PC), or Nonpolar Covalent(NC)
H
2.1
Li
1.0
Na
0.9
K
0.8
Rb
0.8
Cs
0.7
Fr
0.7
Electronegativity Values
Be
1.5
Mg
1.2
Ca
1.0
Sr
1.0
Ba
0.9
B
2.0
Al
1.5
Ga
1.6
In
1.7
Tl
1.8
C
2.5
Si
1.8
Ge
1.8
Sn
1.8
Pb
1.8
N
3.0
P
2.1
As
2.0
Sb
1.9
Bi
1.9
O
3.5
S
2.5
Se
2.4
Te
2.1
Po
2.0
F
4.0
Cl
3.0
Br
2.8
I
2.5
At
2.2
He
--Ne
--Ar
--Kr
--Xe
--Rn
---
Type
S
Cl
Li
C
N
O
Br
Cl
O
Cl
Station 3 – BOND ENERGIES
From this diagram,
the bond distance is ________________ nm and
the bond energy is _________ joules.
Some Useful Bond Energies:
C-H 413 kJ/mol
C-C 346 kJ/mol
C-O 358 kJ/mol
O=O 498 kJ/mol
Calculate the enthalpy of combustion, Hcombustion, for ethanol, C2H5OH.
O-H 463 kJ/mol
C=O 799 kJ/mol
Station 4 – LEWIS SYMBOLS
Draw the Lewis structures of the following:
Al (ground state)
S2-
CaH2
H2O
Al3+
Cl2
Station 5 – MORE LEWIS SYMBOLS
Draw the Lewis structures of the following:
N2
SO2
CO2
SF6
XeF2
IF3
Station 6 – SHAPES / HYBRIDIZATION / POLARITY
State the steric number, the hybridization used by the central atom, the shape of the molecule and polarity:
SN = _____ hybridization: ______
Polar? __
molecular shape: _____________________
SN = _____ hybridization: ______
Polar? __
molecular shape: _____________________
SN = _____ hybridization: ______
Polar? __
molecular shape: _____________________
SN = _____ hybridization: ______
Polar? __
molecular shape: _____________________
Station 7 – MULTIPLE BONDS / SIGMA & PI BONDS
Consider the gas, hydrogen cyanide, HCN:
This molecule contains ___ sigma bonds and ___ pi bonds.
The steric number for H = ___ C = ___ N = ___.
The hybridization for H = ____ C = ____ N = ____.
Draw the “balloon diagram” for HCN.
Station 8 – RESONANCE & BOND ORDER
Draw the Lewis Structures for NO2+, NO2, and NO2-:
NO2+
NO2
Station 9 – FORMAL CHARGE
Consider these two possible Lewis structures for the thiocyanate ion, SCN-:
Determine the formal charges of each atom and circle the best structure.
What is wrong with the structure you did not circle.
NO2-
SHAPES & POLARITY
Draw the Lewis structure for the following molecules. State their steric number and shape. Are they polar?
Formula
ClF3
XeF4
SO2
XeF2
PF3
Lewis
Stucture
Steric
Number
Shape
Polar?
11  IMF's, Liquids, & Solids
Station 1 – PHASE DIAGRAMS
Label the “triple point” on the diagram.
Label the “critical point” on the diagram.
Boiling liquid would be found at Point ___.
The name of the phase change that occurs by increasing temperature
at Point D is ___________________.
Which two phases are in equilibrium at Point B? ________ & ________
Indicate the region where the gas can no longer be liquefied by increasing the pressure.
Is this a phase diagram of H2O? ______ Explain.
Station 2 – IMF’s
Match the statement with the IMF:
A Dipole-Dipole B. Covalent network
_____
_____
_____
_____
_____
_____
1.
2.
3.
4.
5.
6.
C. Hydrogen-bonding
D. Ionic
E. Metallic
Is used to explain why BP of Xe > Kr > Ar > Ne > He
Is present in C(graphite) but not in C(diamond)
Is used to explain why Cu is a good conductor
Is used to explain why NaCl(l) is a good conductor
Is used to explain why ICl has a higher BP then Br2
Is used to explain why vapor pressure of CH3OH is less than CH4.
F. London Dispersion Forces
Match the IMF with its description:
___ 1. hydrogen bonding
___ 2. dipole-dipole attractions
___ 3. London dispersion forces
___ 4. ionic interactions
___ 5. metallic bonding
A.
B.
C.
D.
E.
a lattice of positive ions in a sea of delocalized electrons
positive ends of polar molecules attract negative ends of other polar
molecules
lattice of alternating positively and negatively charged particles
polar interactions in molecules with especially polar intramolecular
attractions
polarized electron clouds induce dipoles in their neighboring atoms
Station 3 – MORE IMF’s
Here are the attractive forces in order from weakest to strongest:
London
Dipole-Dipole
HydrogenDispersion
Metallic Bonding
Interaction
Bonding
Forces
Ion-Ion
Interaction
Covalent
Network
Indicate the strongest IMF in each of the following:
SO2
NH3
Xe
CO2
KOH
XeF4
CH3OH
K2S
SF4
Na
H2S
CH4
List the 8 substances that are covalent network solids:
Station 4 – BOILING
A liquid will boil when it’s ___________ _____________ is equal to the _______________ above the liquid.
Here is a graph of the vapor pressures of two liquids, A and B.
Which compound has the greater IMF’s? ______
Could A or B be H2O? _____ Justify your answer.
What is the normal boiling point of A? _______
What is the normal boiling point of B? _______
If beakers of liquids A and B were placed in a bell jar connected to a vacuum pump at room temperature (20°C),
which liquid would begin to boil first when the vacuum pump was turned on? _____ At what pressure would
this occur? __________mmHg.
Station 5 – PROPERTIES OF SUBSTANCES
In each case, circle the choice with the HIGHER value for the property listed:
Boiling Point:
Cl2
or
Br2
Melting Point:
Si
or
S
Melting Point:
KBr
or
LiF
Hvaporization:
HF
or
HCl
Vapor Pressure:
C3H8
or
CH4
Boiling Point:
H2O
or
NH3
Vapor Pressure:
CH3OH
or
C2H5OH
Hvaporization:
HCl
or
HBr
Station 6 – EXPLAINING TRENDS
This graph shows the BP’s of analogous compounds using elements from
periods 2, 3, 4, and 5.
Explain why the BP of Xe > Kr > Ar > Ne:
Explain why the BP of H2Te > H2Se > H2S:
Why is the BP of H2O > the others in its group?
Station 7 – ENERGY OF PHASE CHANGES
1. The heat of vaporization of methane, CH4, at its boiling point is 9.20 kJ/mol.
How much heat energy is required to vaporize 100. G of methane at its boiling point?
2.
Methanol, CH3OH, (molar mass 32.04 g/mol) has a heat of vaporization of 39.2 kJ/mol and a density of
0.7914 g/mL. How much energy is needed to vaporize 350. mL of methanol?
3.
The greatest change in energy for a substance is seen with which process? _____
a) vaporization
b) condensation
c) fusion
d) sublimation
e) melting
Station 8 – EQUILIBRIUM VAPOR PRESSURE
Which of the following has the lowest equilibrium vapor pressure? _____
a) F2
b) H2O
c) HF
d) NaCl
e) Br2
Liquid “X” is at equilibrium with its vapor in a cylinder and piston apparatus. When the
volume of the space above the liquid is 100 mL and the temperature 25°C, the vapor
pressure of “X” is 120 torr.
What will the vapor pressure of “X” be when the volume above the liquid is 50 mL and
the temperature is 25°C? _____
a) 240 torr
b) 120 torr
c) 60 torr
Station 9 – VISUALIZING SOLIDS
For each image, name the type of solid and the IMF(s) illustrated.
d) 480 torr
e) 30 torr
IMF’s and PHASE DIAGRAMS
Circle the chemical with the weakest IMF? H2O, H2S, H2Se, H2Te
Write these chemicals in order of increasing boiling point: SO2, CH3OH, O2, SiO2
Substance
Type of IMF
Fill in the phases (s, l, g) on the phase diagram.
What is the normal boiling point of this substance. _____
Which phase is more dense, the liquid or the solid? ____
What change occurs as the substance is heated from 10C
to 50C at a pressure of 0.4 atm. ___________________