ftce chemistry sae preparation course session 1 lisa baig instructor
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FTCE Chemistry SAEPreparation Course
Session 1
Lisa BaigInstructor
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 OutlineSession 1
Review Pre TestCompetencies 6, 7 and 8
Competencies 1 & 2 Competency 5
Session 2Competency 3Competency 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.
MSDS
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 theNature of Matter
Differentiate between pure substances, homogeneous mixtures and heterogeneous mixtures
Knowledge of theNature 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 P1 = P2 V1 = V2
T1 T2 T1 T2
P1V1 = P2V2 PV= nRT Values for R are given
T1 T2 on your reference sheet
Knowledge of theNature of Matter
Apply units of mass, volume and moles to determine concentrations and
dilutions of solutions.
Molarity (M) = moles/LiterMolality (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 = 1.65 L of solution
0.200 M solution
Knowledge of theNature of Matter
Analyze the effects of physical conditions on solubility and the
dissolving process
How do changes in the following affect solubility?
pressureheat
agitation
Knowledge of theNature of Matter
Evaluate problems relating colligative properties, molar mass and solution
processPactual = 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 theNature 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 problemWhat is the Freezing Point Depression if
2.84 moles of a solute are added to 0.687 kg of benzene?
Normal F.P = 5.48oCKf = 5.12 DTt = -kf moles solute
kg solventDTt = -5.12(2.84/.687)
DTt = -21.16
5.48oC -21.16oC=-15.68oC
Knowledge of theNature 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=Q67.6J=Q
• Differentiate physical methods for separating the components of mixtures– Chromatography
• Combined liquids
– Extraction• Combined liquids
– Filtration• Solids within liquids
Knowledge of theNature of Matter
Lunch Time
We startAgain
InONE 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 Matter1) Gases consist of large numbers of tiny particles that
are far apart relative to their size2) Collisions between gas particles and between
particles and container walls are elastic collisions3) 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
Temperature
Pressure
Points on Diagram
A = Triple PointB = Normal Melting Point
C = Normal Vaporization PointD = 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!
Calculate the enthalpy change for:C (s) + 2H2 (g) CH4 (g)
Given the following equations:Equation DHC + O2 CO2 -393.5
H2 + 1/2 O2 H2O -285.8
CH4 + 2 O2 CO2 + 2 H2O -890.3
Knowledge of Energy and its Interaction with Matter
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
Yes@ low temps
+ +-
@ high 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 = h x vE = Energy of Quantum
h = 6.626 x 10-34 J•s (Planck’s Constant)v = frequency of the wave
C = l x vC = Speed of Light
3 x 108 m/s
l = wavelengthv= frequency
Break Time
Take a 10 minute
break!
73Li
42He 1
1H
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• 41
20Ca
• 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
SD-1
P
F-2
1s2s 2p3s 3p 3d4s 4p 4d 4f5s 5p 5d 5f6s 6p 6d7s 7p8s
This is the order used to
place electrons- follow 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
Tl
Sn
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 non-
metal 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 DecaySpontaneous disintegration of a nucleus into a
smaller sized nucleusNuclear RadiationParticles emitted by a decaying nucleus
All elements above #83 on the Periodic Table
Two Categories
FissionWhen a heavy nuclei splits into
more stable nuclei of intermediate mass
FusionWhen low mass nuclei combine to
form a heavier more stable nucleus
Types of Particle DecayParticle Symbol What stops this particle
Proton 11p A few sheets of paper
Neutron 10n A few centimeters of lead
Beta Particle(electron)
b-, 0-1b, 0
-1eA few sheets of aluminum foil
Positron b+, 0+1e
A few sheets of Aluminum Foil
Alpha Particle
42He, a, a2+ Skin or one sheet of paper
Gamma Ray
00g, g Several centimeters of lead
Nuclear Reactions42
19K 0
-1e + ?
4240
Ca239
94Pu ? + 235
92U
42He
2713
Al + 42He 30
15P + ?
10n
? + 10n 142
56Ba + 91
36Kr + 31
0n
23592
U
Half-Lives
Remaining Mass = half-life fractionTotal 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 Gold-198 remains after 8.10 days if its half life is 2.70 days?
12.5gA 50.0g sample of 14N decays to 12.5g in
14.4 seconds. What is its half-life?7.2 seconds
Calculating
C = l x v
C = Speed of Light3 x 108 m/s
l = wavelengthv= frequency
Practice
What is the frequency of a wave whose wavelength is 4.5x10-5m?
• C = l x v• 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 = h x vE = 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 = h x v• 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 = massC = 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
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