ftce chemistry sae preparation course session 1 lisa baig instructor

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)


• Erlenmeyer flasks– Receptacle for acid

during titrations– Ideal for mixing,

conical shape contains liquid


• Graduated Cylinder– Measuring specific

volumes for experimental use


• Beaker– Pouring liquids– Stirring liquids


• Crucible– Heating solids

• dehydration


• Clay Triangle– Holds crucible over

flame


• Bunsen burners– Heat source– Many experiments


• Test tubes– Small scale

mixtures that do not require agitation


• Hot plates– Heat source– More specific uses


• Micropipette wells– Small scale labs,

using pipetted liquids


• Vacuum Pump– Used to

demonstrate effects of Pressure on gas laws


• 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


• 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


• Goggle Cabinet– All students will

wear goggles in ANY experiment

– Goggle cabinets contain UV sterilization


• 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…


• 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


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


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


Analyze the effects of physical conditions on solubility and the

dissolving process

How do changes in the following affect solubility?

pressureheat

agitation


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


• 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


• 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


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


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


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


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


• 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


DH DS DG Spontaneous?

- + - Yes

- --

@ low temps

Yes@ low temps

+ +-

@ high temps

Yes@ high temps

+ - + No


DGo=DHo-TDSo

Temperature must be in KELVINS!!!DHo- • + = endothermic• - = exothermic


• 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

ftce chemistry sae preparation course session 1 lisa baig instructor

Documents

knowledge of measurement

knowledge of bonding

knowledge of energy

knowledge of atomic

data collection

scientific method parts

repeated experimental

close range