Mrs. Cook's Blog

Honors Chemistry: Week of September 28

GPS:

SC3 Students will use the modern atomic theory to explain the characteristics of atoms.

b. Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical properties.

SC4. Students will use the organization of the Periodic Table to predict properties of elements.

b. Compare and contrast trends in the chemical and physical properties of elements and their placement on the Periodic Table.

SCSh7. Students will analyze how scientific knowledge is developed. Students recognize that:

a. The universe is a vast single system in which the basic principles are the same everywhere.

b. Universal principles are discovered through observation and experimental verification.

c. From time to time, major shifts occur in the scientific view of how the world works. More often, however, the changes that take place in the body of scientific knowledge are small modifications of prior knowledge. Major shifts in scientific views typically occur after the observation of a new phenomenon or an insightful interpretation of existing data by an individual or research group.

d. Hypotheses often cause scientists to develop new experiments that produce additional data.

e. Testing, revising, and occasionally rejecting new and old theories never ends.

SCSh8. Students will understand important features of the process of scientific inquiry. Students will apply the following to inquiry learning practices:

b. Scientific researchers are expected to critically assess the quality of data including possible sources of bias in their investigations’ hypotheses, observations, data analyses, and interpretations.

c. Scientists use practices such as peer review and publication to reinforce the integrity of scientific activity and reporting.

d. The merit of a new theory is judged by how well scientific data are explained by the new theory.

 

Monday: Introduction to Periodic Table

Tuesday: Mendeleev lab (No prelab.  No need to dress for lab.) 

Wednesday: Work on review

Thursday: Review assignment (including the back of the assignment sheet) due

Friday:  Test

 

Special Reminder:  Portfolio #2 is due Monday, October 5

AP Chemistry: Week of September 28

College Board Course Description

II. States of Matter

A. Gases

1. Laws of ideal gases

a. Equation of state for an ideal gas

b. Partial pressures

2. Kinetic molecular theory

a. Interpretation of ideal gas laws on the basis of this theory

b. Avogadro’s hypothesis and the mole concept

c. Dependence of kinetic energy of molecules on temperature

d. Deviations from ideal gas laws

 

Chapter 10 homework previously assigned:  #23, 23, 33, 39, 41, 75, 45, 49ab

First period also assigned #53, 55

Monday:  Chapter 10 problems: #53, 55, 59, 63, 65, 57, 75b, 82 (answer = 370 g/mol) and Read pages 418-420

Tuesday: Prelab 9 due  (We will do one trial only.)

Wednesday: AP problems worksheet.

Thursday: Lab 9 due

Friday: Test Chapter 10 (Gases)

AP Chemistry; Adjusted schedule for 9/24 & 9/25

9/24: Continue with notes and practice problems for Chapter 10

9/25:  Solutions unit homework due.  Second part of solutions test will be this date.

Honors Chemistry: Adjusted schedule for Electron Unit

Please see the link at the top of my blog for the adjusted due dates for this unit.

Honors Chemistry: Week of Sept 21

GPS: SC3 Students will use the modern atomic theory to explain the characteristics of atoms.

b. Use the orbital configuration of neutral atoms to explain its effect on the atom’s chemical properties.

 

Monday, 9/21: Homework: electron configuration of O(#8) to Ca(#20) & Co, Br, Kr, Hg and orbital notation for O to Ca, Br

 

Tuesday, 9/22: Bohr diagrams for Be(#4) to Ca(#20) & Co, Br, Kr, Hg.  Study for orbital quiz tomorrow

 

Wednesday, 9/23: Lewis dot for O(#8) to Ca(#20) & Co, Br, Kr, Hg and noble gas short-cut for Be, F, Na, P, Co, Bi

 

Thursday, 9/24: Quantum numbers for Be, F, Na, P, Co

 

Friday, 9/25: No homework

AP Chemistry: Week of September 21

College Board AP Chemistry Course Description:

II. States of Matter

A. Gases

1. Laws of ideal gases

a. Equation of state for an ideal gas

b. Partial pressures

2. Kinetic molecular theory

a. Interpretation of ideal gas laws on the basis of this theory

b. Avogadro’s hypothesis and the mole concept

c. Dependence of kinetic energy of molecules on temperature

d. Deviations from ideal gas laws

 

C. Solutions

1. Types of solutions and factors affecting solubility

2. Methods of expressing concentration (use of normalities is not tested)

3. Raoult’s law and colligative properties (nonvolatile solutes); osmosis

III. Reactions

C. Equilibrium

b. Equilibrium constants for reactions in solution

(2) Solubility product constants and their application to precipitation and the

dissolution of slightly soluble compounds

(3) Common ion effect; buffers; hydrolysis

 

 

Monday, 9/21: Detailed write-up for Solutions Worksheet #4.  Describe how to solve the problem with words.  Use the calculation as an illustration.

Tuesday, 9/22: Part 2 of Solutions test today.  Homework packet (including assignment on 9/21) due today.

Wednesday, 9/23: Homework: Page 428, #25, 33, 39, 41, 75, 45, 49ab.  Prelab 9

Thursday, 9/24 and Monday, 9/28: Lab 9.  Lab report due Thursday, Oct 1

Friday, 9/25:  Guided reading worksheet

AP Chemistry: Gases (Chapter 10)

Notes and assignments

Define:

pressure – force per unit area

pressure units:  1 atm = 760 mm Hg = 760 torr = 101.3 kPa

barometer – measures atmospheric pressure

manometer – measures pressure in a closed container

Homework: Page 428, #23  (Assigned 9/18)

 

Define:

STP – standard temperature and pressure = 0 ^oC and 1 atm

Ideal gas law:   PV = nRT

Boyle’s law: P₁V₁ = P₂V₂ (Figure 10.7 on page 399)

Charles’s law: V₁/T₁ = V₂/T₂  (See Figure 10.7 on page 400:  How to determine absolute zero)

Gay-Lussac:  P₁/T₁ = P₂/T₂

Combined gas law: P₁V₁/T₁ = P₂V₂/T₂

Avogadro’s law:  Equal volumes of gases and constant temperature and pressure contain the same number of particles.

Homework: Page 428, #25, 33, 39, 41

 

Why? Kinetic Molecular Theory - Assumptions on 414

Real gases do not conform to all assumptions, Read derivation. Page 421.

    KE avg = 3/2 RT  So temperature is a measure of KE.  At same temp, same KE.

 

    KE per molecule = 1/2 mv2   See balloons on pg 401, Which faster?  heavier?

 

Homework: page 431, #75

 

 

Density of gas:  Sample 10.7  Homework: Page 429, #45, 49a

 

Molar mass of gas from density: D = mass/V, n = mass/MM

Can derive: MM = DRT/P     Sample 10.8 and practice.

Homework: Page 430, #49b

 

Molar Mass of a Volatile Liquid (#9)

 

 

Reactions with Gases

A) All gasses at same T & P (Avogadro’s Law):  Treat volume like moles.  Only need reaction coefficents.

B) Reactions with gases at STP: Use 1 mole = 22.4 L

C) Other reactions:  Use the ideal gas law to go from Quantity Given A ® Mole Given
OR Mole Requested ® Quantity Requested

 

    Sample 10.9 on page 409 and practice

Homework: Pg 430, #53, 55

 

 

Dalton's Law of Partial Pressures:  See page 410 and Sample 10.10 on page 411.

Note: if only asked for total pressure:  P = nRT/V where n = n O2 + n CH₄

Homework: page 430, #59, 63

   

Mole fraction of gases: Xgas =  n gas / n total =  Pgas / P total.  See Sample 10.11

    Homework: page 431, #65

 

Collection by displacing water:  See Fig 10.16 on page 413 (start with the collection jar completely filled with water.  Note: Pressure in jar = atmosphere (barometric)

    Sample 10.12 on page 413

Homework: Page 430, #57

 

Root mean square velocity: urms = square root of (3RT/M)  where M is the molar mass in kilograms and R = 8.3145 J/K mol

    Rarely shows up in multiple choice as a problem with numbers

    If on free-response, you will have equations.

 

    See Figure 10.19 on page 417    Sample 10.14 on page 417

    Homework: Page 431, #75b

 

Diffusion and effusion: Read pages 418-420

    Effusion: passage of gases through tiny orifice (hole) into evacuated (empty) chamber

    Graham's law (page 418).  Sample and practice 10.15 (page 419)

Homework: Page 432, #82   (Answer: 370 g/mol)

 

 

Homework:  GAS LAWS WORKSHEET

 

Answers to Gases Worksheet

1a) 74 torr

1b) 35 torr & 0.52 or 0.54

2a) 0.640 atm

2b) PCl₃ = 0.36 atm, PCl₅ = 0.28 atm

3) 88.1 g/mol

5a) 0.00750 mol excess O₂

5b) 868 mm Hg

5c) 0.0116 mol H₂O vapor

6a) 3.49 x 10^-3 mol

6b) 6.93 x 10¹⁹ molecules

6c) V of H₂ = 3 x V of H₂O

7) 72.08%

8) 0.135g or 0.14g

14-C

15-B

16-B

Honors Chemistry: Week of September 14

Monday: Study for Atomic Theory Test

Tuesday: Read sections 11.1 A& B.  Define wavelength, frequency, photon.  Copy the table part of Figure 11.4

Wednesday: Flame test prelab (due 9/17) and Light problems worksheet (due 9/18)

Thursdsay: Flame test lab today (lab report due 9/21)

Friday: Complete flame test lab report

 

 

Honors Chemistry: Electron structure notes and assignments

Electron Structure Notes and Assignments

 

SC3 Students will use the modern atomic theory to explain the characteristics of atoms.

f. Relate light emission and the movement of electrons to element identification.

 

 

Atomic Theory test day assignment:  Read sections 11.1 A& B.  Define wavelength, frequency, photon.  Copy the table part of Figure 11.4

 

Definitions: 

wavelength - distance between successive peaks or troughs in a wave (lambda)

frequency - the number of waves (cycles) past a point in space (nu)

hertz (Hz) - cycles per second

photon – a particle of electromagnetic radiation (light)

quantum - the smallest quantity of energy that can be emitted or absorbed as electromagnetic radiation  (a packet of energy)  (See figure 11.11 & 11.12 on page 368)

 

electromagnetic spectrum (Pg 362).  Need to know relative size & energy.

 

Students will be given constants for the problems on test.  No need to memorize them.

lambda x nu = c  (3.00 x 10⁸ m/s):  nano = 10^-9 m Solve for each variable.

    Sample A and Practice problem on worksheet (File: ws light equations)

 E = h x nu    h = 6.63 x 10^-34 Js  (A joule is a unit of energy.)    Solve for each variable.

    Sample B and Practice problem on worksheet

Homework problems on worksheet. 

 

"Flame Test of Metal Salts" Lab

 

Heisenberg uncertainty principle:  It is fundamentally impossible to know both the location and momentum/velocity of a electron at the same time.

    Implication: No circular orbits.  Bohr got it wrong.  They have orbitals – more on that later.

 

"The Atom" video with worksheet.  See Figure 11.7 on page 365.

ground state - lowest energy of electron/atom

excited state - some higher energy state (one or more electrons have gained energy and jumped up higher (further out) energy

See page 367 (Figures 11.8 to 11.10)

 

Absorption spectrum - Atom is absorbing (gaining) energy.  Move to higher, excited state

Emission spectrum - Atom is emitting (letting go) of energy.  Return to lower state

 

Homework: Read Sections 11.1 C & 11.2 A & B.  Complete Flame test lab report

 

Orbital - wave functions that show an electron’s probability density.  Page 371 (3D region around the nucleus that describes an electron’s probable location.)  Each orbital can hold 2 e-

 

Quiz Questions:

A. How many electrons can the ___ orbitals hold if filled?

B. How many kinds of orbitals can be in the ___ energy level?

C. What are the orbitals of the __ energy level? (s,p,d,f)

D. How many ___ orbitals are there?

E. At most, how many electrons can the ___ energy level hold?

 

2. So how do the electrons fill these orbitals?

Aufbau Principle:  An electron occupies the lowest-energy orbital that can receive it.

SO: Diagonal chart.

 

Homework:  electron configuration of O(#8) to Ca(#20) & Co, Br, Kr, Hg

 

    Exceptions: Fig 11.22 on page 381 (Not required this year.)

 

Pauli exclusion principle: (page 375) Two electrons can occupy the same orbital if and only if they have opposite spin.

 

degenerate orbitals - orbitals that have the same energy

 

Hund's rule: 

·     Single electrons with the same spin must occupy each equal-energy (sublevel) orbital before additional electrons with opposite spin can occupy the same orbitals.

·     Every equal-energy orbital gets one electron with the same spin before any orbital gets two.

·     Maximize the number of degenerate orbitals with parallel spin.

·     School bus analogy

Orbital configuration through nitrogen. (See page 377-378)

 

Homework: Write orbital notation of O through Ca and Br

 

 

Recall Bohr atomic model.  Show energy level only. 

Homework:  Bohr diagrams for Be(#4) to Ca(#20) & Co, Br, Kr, Hg

 

Lewis dot structure – last energy level only

 

Homework: Lewis dot structures for #8 (O) to #20 Ca. and Co, Br, Kr, Hg

 

Short cut on electron configuration using Noble gases:  Previous noble gas in [ ], then rest of electron configuration.

 

Homework: Short cut for Be, F, Na, P, Co, Bi

 

 

Quantum numbers:

    n = principle quantum number (1, 2, 3, etc)

    l = orbital quantum number (0=s, 1=p, 2=d, etc.)

    m_l (sometimes just "m") = magnetic quantum number (s = 0)

    (p = -1,0,+1)   (d = -2,-1,0,+1,+2)  (f = -3,-2,-1,0,+1,+2,+3)

    m_s (sometimes just "s") = spin quantum number (+1/2, -1/2)

 

Homework: Write a consistent set of quantum numbers for: Be, F, Na, P, Co

 

AP Chemistry: Week of 9/14

Monday: 1st & 2nd period - Lab 11 due.  Homework: Page 761, #47b, 49ac, 53, 67 and Prelab 18

Tuesday: 4th period - Lab 11.  Lab 18 due on Thursday, 9/17.

Wednesday: AP-style Worksheet [answers: #1a(62 g/mol), 1b(C₂H₆O₂),  #2a(C₆H₅), #2b(0.666 molal), #2c(6.8^oC/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.)]

Thursday: Study for test.  Review List:

Definitions of molarity, molality, mass percent, mole fraction, colligative properties

    Recall handy-dandy chart.

Henry's Law (P = kC)

Raoult's Law (Psoln = Xsolvent Posolvent)

    volatile solutes:  Psoln = XAPoA + XBPoB + ...

boiling point elevation and freezing point depression (DT = imK)

osmotic pressure: π = iMRT  (Also see page 557, #86)

solubility product: Ksp = [A]a[B]b

Friday: Test Solutions.

Homework:  Read pages 393-398.  Page 428, #23