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Monday: Finish review. Receive reading guide for start of solutions unit
Tuesday: Test Chapter 3
Wednesday: Test Nomenclature and start Solutions Unit
Thursday: Continue with solutions unit. Homework: Page 566, #37,39, 41b, 43, 51 and then 31 & 33.
Friday: Colligative properties. Homework: Page 567, #67, 69, 71, 73
Posted at 01:53 AM in AP Chemistry | Permalink
Notes and Assignments
Reading Guide – Start Solutions
A. Read and define and understand terms in Introduction to Chapter 4 and Section 4.1:
aqueous solution, electrolyte, nonelectrolyte, dissociates, solvation, strong electrolyte, weak electrolyte, chemical equilibrium
B. Read and define and understand terms in Introduction to Chapter 13 and the beginning of Section 13.1 (pages 527-529): solution, component, solvent, solute, aqueous solution, solvation, hydration.
C. Recall: Molarity = moles solute per liter solution
Work through Samples 4.11 – 4.13 (pages 144-146)
D. See page 144, Figure 4.16. Know how to prepare a standard solution.
E. Read about dilution problems starting on page 146. Note that both the original and dilute solutions contain the same total amount of solute.
So: M1V1 = M2V2. See Sample 4.14 on page 148.
F. Page 156, #4, 5, 61, 67, 69, 73
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More vocabulary
hydrophobic – “water fearing” – will not mix with water
hydrophilic – “water loving” – will mix with water
miscible – two liquids that are mutually soluble in any proportion
immiscible – two liquids that will not dissolve in each other
ionization – creating ions where there were not ions before
(EX: HCl + H2O ® H3O+ + Cl-)
mass percent: (component mass / total mass) x 100
mole fraction (C): component moles / total moles
molality: moles solute / kg solvent
Master Chart
Solute Solvent Solution
mass
MM
moles
volume
Page 544, Sample 13.6 (and practice). Sample 13.7 (and practice)
Homework: Page 566, # 37, 39, 41b, 43, 51
Recall pressure units (atm, mm Hg, torr, kPa)
Effect of pressure on solubility of gas in a liquid
Henry's Law: the amount of a gas dissolved in a solution is directly proportional to the pressure of the gas above the solution. (page 540). Sg = kPg Sample 13.3
Effect of temperature on solubility of gas (or volatile solute) in a liquid: Figure 13.18 on page 541.
Homework: Page 566, #31, 33
Effect of pressure on nonvolatile solute in a liquid: None
Effect of temperature on a nonvolatile solute in a liquid:
Increased temperature always increases rate of solution but not necessarily solubility.
Figure 13.17 on page 541 (generalization?)
Section 13.5
Colligative properties: Properties of solutions that depend only upon the concentration of solute.
Colligative properties include lowering the vapor pressure of the solvent, boiling point elevation, freezing point depression, and osmotic pressure.
Raoult’s law – page 547.
Nonvolatile solute: Psoln = Xsolvent Posolvent
Volatile solute: For each component: PA = XA PoA
Sample 13.8 on page 547 and practice (whole class)
Homework: Pg 567, #59, 61
van't Hoff factor (i): the ratio of moles of particles in solution to moles of solute dissolved.
Ionic pair activity and effect on colligative properties: See Table 13.5 on p 554.
Boiling point elevation & Freezing point depression
DTb = i Kb msolute DTf = i Kf msolute Table 13.4 (page 549)
Sample 13.9
Can compare effects without actually calculating the DT. Sample 13.10 and practice
Homework: Page 567, #67, 69, 71
Define semipermeable membrane: solvent can pass through but solute can not.
Ex: cell membrane
Solvent will have net flow to even out the concentrations: osmosis
isotonic - same concentration solute
hypotonic - less concentration of solute
hypertonic - more concentration of solute
osmotic pressure (p) - pressure that must be supplied to stop osmosis
p = MRT = nRT x i Sample 13.11 on pg 553 and practice
V
Homework: Page 568, #73
Colligative properties to calculate molar mass.
Samples 13.12 and 13.13 (page 555-556)
and both practice problems
Homework: Page 568, #75 &77 and Prelab 8.
Note: for #75, black = carbon, red = oxygen, white = hydrogen
Experiment 11: Molecular Mass by Freezing Point Depression
regular, not microscale, foil sheet for steam shield
Step 10, 16, 17: Yes, repeat
Step 11-12: Use paradichlorobenzene (C6H4Cl2) instead of cetyl alcohol
Lab Report: no sources of error
Ksp: Read page 738. Sample problems 17.9
Homework: Page 761, #47b
ICE (initial, change, equilibrium) strategy for solving equilibrium problems
Sample 17.10 and 17.11 and practice 17.11
Homework: Page 761, #49ac
Common ion effect (page 741). Sample 17.12 and practice
Homework: Page 761, #53
Will it precipitate?
Reactions quotient (Q) = equilibrium expression evaluated at current conditions.
Q > Ksp Yes, it will precipitate
Q = Ksp No precipitate. At equilibrium.
Q < Ksp No precipitate. Solution is not saturated and could absorb more solute.
Sample 17.15 and 17.16 and both practice problems
Homework: Page 762, #67
Exp 18:Do all post lab calculations and questions
Lab report: Sources of Error is not required.
Assign AP solutions worksheet
Worksheet answers: #1a(62 g/mol), 1b(C2H6O2), #2a(C6H5), #2b(0.666 molal), #2c(6.8oC/m), #2d(150 g/mole), #2e(C12H10), #3(0.20 moles), #4a(2.6 x 10-13), #4b(8.0 x 10-7 M), #4c(Q=0.003364 which is less than Ksp. So yes it will ppt.)
Posted at 01:47 AM in AP Chemistry | Permalink
Monday & Tuesday: Time line construction and notes. Homework - Read section 3.3A
Wednesday: Rutherford penny lab (no prelab)
Thursday: Element Quiz 2. Extra-credit (5 test points) due one week from date of assignment.
Other particles carry or mediate the four forces. Find out the names of the force particles. Write one paragraph for each force and discuss these "messenger" particles.
Posted at 11:18 PM in Honors Chemistry | Permalink
(Sections 3.2, 3.3, 19.1, 19.2)
Notes and Assignments
GPS:
SCSh1. Students will evaluate the importance of curiosity, honesty, openness, and skepticism in science.
SCSh3. Students will identify and investigate problems scientifically.
SCSh4. Students will use tools and instruments for observing, measuring, and manipulating scientific equipment and materials.
SCSh5. Students will demonstrate the computation and estimation skills necessary for analyzing data and developing reasonable scientific explanations.
SCSh6. Students will communicate scientific investigations and information clearly.
SCSh7. Students will analyze how scientific knowledge is developed.
CSh8. Students will understand important features of the process of scientific inquiry.
SC3 Students will use the modern atomic theory to explain the characteristics of atoms.
c. Explain the relationship of the proton number to the element’s identity.
d. Explain the relationship of isotopes to the relative abundance of atoms of a particular element.
Atomic Theory History (How did we get here?)
Need to know: 5 historical models (Who made them, their order, descriptions in words and pictures) and types of radiation
Two Greek ideas: Democritus(Ultimate particle = “atom”) and Aristotle (Continuous matter)
John Dalton: First atomic theory, Five parts (page 56)
1. Elements are made of tiny particles called atoms.
2. All atoms of a given element are identical.
3. The atoms of a given element are different from those of any other element.
4. Atoms of one element can combine with atoms of other elements to form compound. A given compound always has the same relative numbers and types of atoms.
5. Atoms are indivisible. That is, atoms are not created or destroyed. In chemical reactions, atoms are combine, separated or rearranged. (my #5 different from book)
MODEL = cue ball
Explained Law of Conservation of Matter and Definite Composition.
atom - smallest particles of an element that retain the chemical identity of the element
J.J. Thomson: Using cathode ray tube (Text page 60), discovers and names “electron” = Small negative particle in all atoms)
Plum pudding model (page 61)
Ernest Rutherford’s 3 types of radiation:
name, symbol, charge, mass
alpha, a, positive, same as helium
beta, b, negative, very small
gamma, g, no charge, no mass (energy wave)
Ernest Rutherford’s Gold foil experiment (page 62)
1. Most of mass and all of charge in small dense region - nucleus
2. Most of total volume = empty space.
3. There must be enough electrons to equal charge of nucleus.
J.J. Thomson: Mass spectrometer(Charge/mass ratio): Discovers isotopes
isotopes = atoms of the same element with different masses
Henry Moseley - atomic # (x-ray diffraction)
Niels Bohr - Quantum Theory of atoms (planets around sun, quantized energy)
quantum - a package of mass or energy
1919
1932 James Chadwick – isolates neutrons (Why did it take so long?)
Homework: Read Sections 3.3A (The importance of “read behind”), Flashcards anyone?
Essential Question: What is the modern model of the atom?
atom - smallest particle that retains all the characteristics of an element
Size of atoms requires new units:
atomic mass unit (amu) - 1/12th the mass of a carbon-12 atom = 1.66 x 10-24 g
angstrom (capital A with a little circle on top ) = 10-10m
Subatomic particles of the Current model (Quantum Mechanical model)
|
Particle |
Charge |
Location |
Mass |
Symbol |
|
proton |
positive |
nucleus |
1 amu |
p+ |
|
neutron |
none |
nucleus |
1 amu |
no |
|
electron |
negative |
electron cloud |
tiny |
e- |
electron cloud: Can never tell where an electron is. Only where it was or probably will be.
Particle-wave duality
But even smaller sub-subatomic particles.
"The Generations of Matter" website: http://particleadventure.org/frameless/generations.html
Note: heavier across row. (last quark found = top (heaviest) in 1995 at Fermilab
If protons and neutrons are made of 3 quarks (up/down) determine the collection of quarks for each particle.
All particle also have anti-matter opposites. EX: positron (positron emission tomography)
annihilation: matter and antimatter collide - matter destroyed, energy released.
Homework: Are you making vocabulary flashcards?
Extra-credit (5 test points) due one week from date of assignment.
Other particles carry or mediate the four forces. Find out the names of the force particles. Write one paragraph for each force and discuss these "messenger" particles.
Essential Question: How many subatomic particles in a specific atom?
Recall atom: smallest unit of an element that retains all the characteristics of the element
But even elements have different types of atoms.
Recall isotopes: atoms of the same element with different masses.
atomic number = # protons = # e- (Find on periodic table)
atomic mass number = # protons + # neutrons
isotope: Atoms of the same element with different masses.
Same atomic number, different atomic mass number
Same number of protons, different number of neutrons
Know all three ways of naming an isotope.
Example and Practice 3.2 on page 66. (Answers in green section in back of book.)
Homework: Read Section 3.3C. Page 67, #3, 4, 5, 7
Essential Question: What is the other number on the periodic table?
atomic mass: mass of an isotope reported in amu's
atomic weight: average atomic mass - the weighted average of the masses of the naturally occurring isotopes of an element
Homework: Average atomic mass problems on unit assignment sheet.
Essential Question: What is half-life?
Classwork and Homework: “Half-life of an Element”
Essential Question: How do you write nuclear equations?
Page 668. Recall nuclear symbols (center of page)
nuclide: a unique atom (an isotope)
Page 669: “In a nuclear equation both the atomic number and the mass number must be conserved.”
See examples on page 669 and 670.
See example 19.2 on page 674. Students do practice problems.
Homework: Review assignment for unit.
Essential Question: What evidence do we have for subatomic particles?
Classwork and Homework: “Particle Contrails” lab
Review due Sept 14 (Monday)
Test Sept 15 (Tuesday)
Homework on test day for next unit:
Read sections 11.1A&B. Define wavelength, frequency, photon. Copy the table part of Figure 11.4
Posted at 11:10 PM in Honors Chemistry | Permalink
Don't forget to complete your portfolio #1 project. (see link on left side of blog).
Time line activity (Come to class with whatever information you can find)
Atomic Theory Time Line
Find out about these scientists and their advances in chemistry.
Row 1
400 BC Democritus
1780-1790 Antione Lavoisier
1799 Joseph Proust
1803-1808 John Dalton
1834 Michael Faraday
1869 Dmitri Mendeleev
Row 2
1896 Henri Becquerell (& Curies)
1897 J.J. Thomson
1900 Max Planck
1902 Pierre and Marie Curie
1903 Ernest Rutherford
1905 Albert Einstein
Row 3
1909 Robert Millikan
1909-1910 Ernest Rutherford
1912 J.J. Thomson
1913 Niels Bohr
1913 Henry Mosely
1919 Ernest Rutherford
1932 James Chadwick
Posted at 09:48 AM in Honors Chemistry | Permalink
The meeting for AP parents has been relocated to the cafeteria.
See you there Thursday, 8/27 at 6:30 PM
Posted at 10:48 AM in AP Chemistry | Permalink
Monday, 8/24: Comtinue with lab 2.
Tuesday, 8/25: Final mass for lab 2. Lab report due Friday, August 28 (This is a change.) Include all lab post calculations and questions. Homework: Nomenclature worksheet due Wednesday along with problems on Page 115, #88, 89, 97
Wednesday, 8/26: Nomeclature worksheet and Page 115 problems due. Homework: Review worksheet due Friday, August 28 along with your lab report.
Thursday, 8/27: Prelab 5 due.(This is a change.) Lab report due on Monday, 8/31. (This is a change.)
Friday, 8/28: Review worksheet due. Lab report 2 due.
Monday, 8/31: Lab 5 report due
Tuesday, 9/1: Test Chapter 3
Posted at 01:29 PM in AP Chemistry | Permalink
Thursday, August 27 (Open House night)
6 PM in the gym.
Hope to see you there!
Posted at 05:06 PM in AP Chemistry | Permalink
Correct: Page 115, #88, 89, 97
Incorrect: Page 127, #anything
Posted at 12:13 PM in AP Chemistry | Permalink
The rubric is not posting correctly on TypePad. So I have loaded the file here:
