FTCE Chemistry SAE
Preparation Course
Session 1
Lisa Baig
Instructor
Session Norms
• Respect
– No side bars
– Work on assigned materials only
– Keep phones on vibrate
– If a call must be taken, please leave the
room to do so
Course Outline
Session 1
Review Pre Test
Competencies 6, 7 and 8
Competencies 1 & 2
Competency 5
Session 2
Competency 3
Competency 4
Post Test
Required Materials
• Scientific Calculator
• 5 Steps to a 5: AP Chemistry
– Langley, Richard, & Moore, John. (2010).
5 steps to a 5: AP chemistry, 2010-2011
edition. New York, NY: McGraw Hill
Professional.
• Paper for notes
• State Study Guide
Chemistry Competencies
1. Knowledge of the nature of matter (11%)
2. Knowledge of energy and its interaction with
matter (14%)
3. Knowledge of bonding and molecular structure
(20%)
4. Knowledge of chemical reactions and
stoichiometry (24%)
5. Knowledge of atomic theory and structure (9%)
6. Knowledge of the nature of science (13%)
7. Knowledge of measurement (5%)
8. Knowledge of appropriate laboratory use and
procedure (4%)
Pre-Test
• Your homework coming into this
session was to complete the pre-test
and bring in to this session.
• We will now go over your test
answers.
• You will receive a listing of
competencies covered by each
question, to better review the
information you need further
assistance in
Pre-Test Review
The Scientific Method
Parts Of An Experiment
• Constant
– The elements of an experiment that remain
unchanged throughout the duration of the
trials
• Control
– A part of the experiment that does not have
the independent variable applied to it. (Think
Comparison)
• Independent Variable
– The variable that is applied to the experiment,
causes a change in the dependent variable
• Dependent Variable
– The variable that is measured in the
experiment.
Types of Data
• Qualitative Data
– Qualities
– Descriptive
• Quantitative Data
– Numbers
– Counted or Estimated
Scientific Data
• Accurate
– Data collected are within a close range of an
accepted or correct value
• Precise
– Data collected are within a close range of
each other
• Systematic Error
– Differences in data collection that can be
predicted theories, laws or technology
application
• Random Error
– Differences in data collection that result from
human error or environmental variances
Parts of an Experiment
• Experimental evidence
– Data collected from an experiment that
can be used to validate results from
repeated trials
• Models
– A visual or mathematical aid created
using repeated experimental data to
predict or represent items in nature
Parts of Scientific Methodology
• Observations
– Data collected using the senses during or before an
experiment
• Assumptions
– Similar to Hypotheses, a guess about a situation in
nature
• Hypotheses
– An educated guess about a problem based upon
observations and background information
• Theories
– A statement that consistently predicts a pattern in
nature
• Laws
– A mathematical statement that consistently
predicts a pattern in nature
Areas of Scientific Study
• Basic scientific research
– No particular goal in mind
– Research to learn more about nature
• Applied research
– Specific goal or desired product
– Research to acquire desired results
• Technology
– Tools used within scientific study to gain
insight and collect further data
Chemistry Lab Clean Up
• After any experiment you
should consult your
school’s MSDS reference
sheets to determine the
safest/legal way to dispose
of any chemical waste.
Chemistry Lab Equipment
• Micropipette
– Used to dispense
small amounts of
liquid (<1mL)
Chemistry Lab Equipment
• Erlenmeyer flasks
– Receptacle for acid
during titrations
– Ideal for mixing,
conical shape
contains liquid
Chemistry Lab Equipment
• Graduated Cylinder
– Measuring specific
volumes for
experimental use
Chemistry Lab Equipment
• Beaker
– Pouring liquids
– Stirring liquids
Chemistry Lab Equipment
• Crucible
– Heating solids
• dehydration
Chemistry Lab Equipment
• Clay Triangle
– Holds crucible over
flame
Chemistry Lab Equipment
• Bunsen burners
– Heat source
– Many experiments
Chemistry Lab Equipment
• Test tubes
– Small scale
mixtures that do
not require
agitation
Chemistry Lab Equipment
• Hot plates
– Heat source
– More specific uses
Chemistry Lab Equipment
• Micropipette wells
– Small scale labs,
using pipetted
liquids
Chemistry Lab Equipment
• Vacuum Pump
– Used to
demonstrate
effects of Pressure
on gas laws
Chemistry Lab Equipment
• Buret
– Titrations
• Buret Clamp
– Hold the Buret to
the ring stand
• Ring Stand
– To hold any variety
of clamp or ring in
an experiment
Chemistry Lab Facilities
• Fume hood
– Used to
temporarily house
chemicals which
may have noxious
or toxic fumes
associated with
them
Chemistry Lab Facilities
• Gas Jets
– Attach to bunsen
burners
– In the system
shown here, both
jets are off
– Teacher should
have control of
flow of gas within
classroom
Chemistry Lab Facilities
• Goggle Cabinet
– All students will
wear goggles in
ANY experiment
– Goggle cabinets
contain UV
sterilization
Chemistry Lab Facilities
• Safety Shower
– Rapid release of
large volume of
liquid
– Designed to quickly
wash away caustic
chemicals from
entire body
• Eye Wash Stand
– Washes eyes in case
of exposure
• But if they wore the
proper goggles…
Chemistry Lab Facilities
• Fire Blanket
– Flame retardant
material
– Drape and hold
tightly over
affected area
Break Time
Take a
10 minute
break!
Knowledge of the
Nature of Matter
Differentiate between pure substances, homogeneous
mixtures and heterogeneous mixtures
Knowledge of the
Nature of Matter
Determine the effects of changes in
temperature, volume, pressure or quantity
on an ideal gas
(Work with the various gas laws and their constants.)
P1V1=P2V2
P1V1 = P2V2
T1
T2
P1 = P2
V1 = V2
T1 T2
T1 T2
PV= nRT Values for R are given
on your reference sheet
Knowledge of the
Nature of Matter
Apply units of mass, volume and
moles to determine concentrations
and dilutions of solutions.
Molarity (M) = moles/Liter
Molality (m) = moles/kilogram
How many liters of solution are
needed to make a 0.200M solution
with 36.7g of Calcium chloride?
How many liters of solution are needed to
make a 0.200M solution with 36.7g of
Calcium chloride?
Molarity = moles/Liter
36.7g CaCl2
= 0.331 moles CaCl2
110.984 g/mol
0.331 moles CaCl2
0.200 M solution
= 1.65 L of solution
Knowledge of the
Nature of Matter
Analyze the effects of physical
conditions on solubility and the
dissolving process
How do changes in the following
affect solubility?
pressure
heat
agitation
Knowledge of the
Nature of Matter
Evaluate problems relating colligative
properties, molar mass and solution
process
Pactual = POXsolvent
If 18g of Sucrose (C12H22O11) are used
in a 250mL cup of coffee. (80oC),
What is the vapor pressure of the
sugared coffee?
• How many moles of Sucrose? (C12H22O11)
– Molar mass = 342 g/mol
– Moles = 0.105 mol
• 1 mL = 1g of water, so 250g of water
– 13.89 mol H2O
13.89 mol H2O
=X
13.89 mol H2O+ 0.105 mol C12H22O11
X = 0.992
• Vapor pressure of water at 80oC = 355.1
(reference sheet)
• P = (355.1)(0.992)
• P = 352 mmHg
Knowledge of the
Nature of Matter
• Analyze the effects of forces between
chemical species on properties (eg, melting
point, boiling point, vapor pressure,
solubility, conductivity of matter)
– ie- boiling point elevation, freezing point
depression
DT =kbm
DTt = -kf moles solute
kg solvent
Practice problem
What is the Freezing Point Depression if
2.84 moles of a solute are added to
0.687 kg of benzene?
Normal F.P = 5.48oC
Kf = 5.12 DTt = -kf moles solute
kg solvent
DTt = -5.12(2.84/.687)
DTt = -21.16
5.48oC -21.16oC=-15.68oC
Knowledge of the
Nature of Matter
• Solve problems involving an intensive
property of matter
– Density
– Specific Heat
D = m/V
Cp= . Q .
m*DT
Practice problem
What is the energy absorbed by an
8.32g sample of Gold that goes from
37oC to 100oC? (Specific Heat of Gold
= 0.129)
Cp= . Q .
m*DT
0.129 = Q/(8.32•63)
0.129•8.32•63=Q
67.6J=Q
Knowledge of the
Nature of Matter
• Differentiate physical methods for
separating the components of
mixtures
– Chromatography
• Combined liquids
– Extraction
• Combined liquids
– Filtration
• Solids within liquids
Lunch Time
We start
Again
In
ONE HOUR
Knowledge of Energy and its
Interaction with Matter
• Distinguish between different forms
of energy
– Thermal
– Electrical
– Nuclear
– Mechanical
– Potential
– Kinetic
Knowledge of Energy and its
Interaction with Matter
The Kinetic Molecular Theory of Matter
1) Gases consist of large numbers of tiny particles
that are far apart relative to their size
2) Collisions between gas particles and between
particles and container walls are elastic
collisions
3) Gas particles are in continuous, rapid random
motion. They therefore possess kinetic energy,
which is energy of motion
4) There are no forces of attraction between gas
particles
5) The temperature of a gas depends on the
average kinetic energy of the particles of the
gas EK= ½ mv2
Phase Diagram
Points on Diagram
A = Triple Point
B = Normal Melting Point
C = Normal Vaporization Point
D = Critical Pressure Boiling Point
E = Critical Point
Knowledge of Energy and its
Interaction with Matter
Wood, A. (2006, May). CO2 info. Retrieved from
http://www.teamonslaught.fsnet.co.uk/co2_info.htm
As substance is heated, temperatures
do NOT rise when it reaches a
melting/boiling point. Temperatures
remain constant until all matter
reaches next state!
Knowledge of Energy and its
Interaction with Matter
Calculate the enthalpy change for:
C (s) + 2H2 (g)  CH4 (g)
Given the following equations:
Equation
DH
C + O2  CO2
H2 + 1 / 2 O 2  H2 O
CH4 + 2 O2  CO2 + 2 H2O
-393.5
-285.8
-890.3
We want C (s) + 2H2 (g)  CH4 (g), so:
C + O2  CO2
-393.5
CO2 + 2 H2O  CH4 + 2 O2
+890.3
2(H2 + ½ O2  H2O)
2(-285.8)
-74.8
Knowledge of Energy and its
Interaction with Matter
• Predicting Entropy changes
• Look at States of Matter
– Solids- LOW entropy
– Liquids- Medium entropy
– Gases- HIGH entropy
• Look at compounds-vs-elements
– The more items in combination, the
more entropy
Knowledge of Energy and its
Interaction with Matter
DH
DS
DG
Spontaneous?
-
+
-
Yes
-
-
+
+
+
-
@ low
temps
@ high
temps
+
Yes
@ low temps
Yes
@ high temps
No
Knowledge of Energy and its
Interaction with Matter
DGo=DHo-TDSo
Temperature must be in KELVINS!!!
DHo• + = endothermic
• - = exothermic
Knowledge of Energy and its
Interaction with Matter
• Relate regions of the electromagnetic spectrum
to the energy, wavelength and frequency of
photons
E=hxv
E = Energy of Quantum
h = 6.626 x 10-34 J•s (Planck’s Constant)
v = frequency of the wave
C=lxv
C = Speed of Light
3 x 108 m/s
l = wavelength
v= frequency
Break Time
Take a
10 minute
break!
7 Li
3
4 He 1 H
2
1
Atomic Number
Mass Number
Element Symbol
Two Key Numbers
• Atomic Number
– # of Protons in an atom
– This determines the type of
element you have!
– If atom is electrically neutral,
then the number of electrons
is also equal to this number
• Mass Number
– # of protons + neutrons in an
atom’s nucleus
– Mass # - atomic # = # of
neutrons
How many protons, neutrons
and electrons?
• Iodine-128
• 4120Ca
• 20882Pb4+
• 8135Br1• Cobalt-60
S Orbital
• Orbital that can contain
2 electrons
• Spherical in Shape
P Orbitals
• Orbital that can contain
up to 6 electrons
• Contains 3 sub-orbitals,
each holding 2
electrons
• “Peanut” or “Dumbbell”
shaped
D Orbital
• Orbital that can contain
up to 10 electrons
• Contains 5 sub-orbitals
that can each hold 2
electrons
F Orbital
• Orbital that can contain up to
14 electrons
• Contains 7 sublevels each
holding 2 electrons
S
D
P
-1
F
-2
1s
2s
3s
4s
5s
6s
7s
8s
2p
3p
4p
5p
6p
7p
3d
4d 4f
5d 5f
6d
This is the
order used to
place
electronsfollow the
arrows to
their “end”,
then move to
the next
arrow
Find the Arrangements for:
•
•
•
•
•
Sulfur
Strontium
Copper
Lead
Radon
Alkali Metals
• HIGHLY Reactive Metals
• 1 valence electron
– Filling their “S” orbital
• Do not occur naturally in nature as
elements
– ALWAYS found in compounds
• React with water with increasing
violence as atomic number increases
Alkaline Earth Metals
• 2 valence electrons
• Fill their “S” orbitals
• Do not occur in nature as elements
– ALWAYS in compounds
• Less reactive than the Alkali Metals
Al
Ga
In Sn
Tl
Pb Bi
Transitional Metals
• Most have 2 valence electrons
– These fill their “D” sublevels
• Harder and more brittle than the other
metals
• High melting and boiling points
• Good heat and electrical conductors
• Hg- the ONLY metal to be in the liquid
state at room temperature
• Often have colored compounds
Lanthanide Series
•
•
•
•
Elements Ce thru Lu
Once called the “Rare Earth Metals”
Fill their 4f orbitals
All elements within this section have
amazingly similar chemical and physical
properties
– This lead to the difficulty in identification of
the elements in this section
Actinide Series
•
•
•
•
Elements Th thru Lr
Fill their 5f orbital
All elements are radioactive
Beyond Uranium, these elements
have been artificially created
B
Si
Ge As
Sb Te
Po At
Metalloids/Semi-Metals
• All are solids at room temperature
• Semi-conductors of heat and
electricity
• Some metal properties and nonmetal properties
• Fill their “P” level electrons
Non-Metals
• Poor (Non) Conductors of heat and
electricity
• Reactive
• Diatomic Elements
• Gas
– Nitrogen, Oxygen, Hydrogen
• Solid
– Carbon, Phosphorus, Sulfur, Selenium
Halogens
• Diatomic Elements or found in
compounds
• HIGHLY Reactive
• Gases= Fluorine, Chlorine
• Liquid = Bromine
• Solid = Astatine, Iodine
Noble Gases
• Non-Reactive
• We have FORCED it to react and form
compounds with Fluorine
• Uses:
– Neon, Argon, Krypton and Xenon are
used for lighting
– Helium is used in balloons
Break Time
Take a
10 minute
break!
Unstable Nuclei
Radioactive Decay
Spontaneous disintegration of a nucleus into a
smaller sized nucleus
Nuclear Radiation
Particles emitted by a decaying nucleus
All elements above #83 on the Periodic Table
Two Categories
Fission
When a heavy nuclei splits into
more stable nuclei of
intermediate mass
Fusion
When low mass nuclei combine to
form a heavier more stable
nucleus
Types of Particle Decay
Particle
Symbol
Proton
1 p
1
1 n
0
Neutron
Beta
Particle
b- , 0
A few sheets of paper
A few centimeters of lead
0
A few sheets of aluminum
foil
+1e
A few sheets of Aluminum
Foil
-1b, -1e
(electron)
b+, 0
Positron
Alpha
Particle
Gamma
Ray
4
2+
He,
a,
a
2
0
What stops this particle
0g,
g
Skin or one sheet of paper
Several centimeters of lead
Nuclear Reactions
42
K
19
 0-1e + ?
42
Ca
40
239
235
Pu

?
+
U
94
92
4
He
2
27
4
30
Al + 2He  15P + ?
13
1
n
0
? + 10n  14256Ba + 9136Kr + 310n
235
U
92
Half-Lives
Remaining Mass = half-life fraction
Total Mass
1=½
2=¼
3 = 1/8
4 = 1/16
5 = 1/32
6 = 1/64
7 = 1/128 8 = 1/256
# h.l = time elapsed
time of 1 h.l
Amount remaining = (original)(1/2)#h.l
Practice
How much of a 100.0g sample of Gold198 remains after 8.10 days if its half
life is 2.70 days?
12.5g
14
A 50.0g sample of N decays to 12.5g in
14.4 seconds. What is its half-life?
7.2 seconds
Calculating
C=lxv
C = Speed of Light
3 x 108 m/s
l = wavelength
v= frequency
Practice
What is the frequency of a wave whose
wavelength is 4.5x10-5m?
• C=lxv
• 3x108m/s= 4.5x10-5m •v
• 3x108m/s =
4.5x10-5m
= 6.7 x 1012 Hz
What’s a Quantum??
The amount of energy that can be
gained or lost by an atom
E=hxv
E = Energy of Quantum
h = 6.626 x 10-34 J•s (Planck’s Constant)
v = frequency of the wave
Practice
• What is the energy of a wave whose
frequency is 2.5x10-4Hz?
• E=hxv
• E= (6.626 x 10-34 J•s)(2.5x10-4Hz)
• E=1.65x10-37J
Conversions of Mass and Energy
E = mC2
E = Energy m = mass
C = Speed of Light
(3 x 108 m/s)
Practice
• What is the mass of a particle whose
energy is 2.41x10-27J?
• E = mC2
2.41x10-27J = m
(3 x 108 m/s)2
2.68x10-44kg
Homework
• Diagnostic Exam in your AP chem Prep
book- Page 17-26
• Only answer the questions for these
Chapters & Questions
– Ch 5 #1, 3, 5
– Ch 8 #21, 22
– Ch 9 #25, 28, 29, 30
– Ch 10 #32-35
– Ch 12 #55
– Ch 13 #60
– Ch 17 #81-84