Unit 3 AP CHEM

AP Chemistry Unit 3 Study Guide (15th edition)

Unit Topics from College Board (and alignment to text sections)

1. Intermolecular and interparticle forces (11.2, 11.5)

2. Properties of solids (ch 12)

3. Solids, liquids and gasses (11.1)

4. Ideal gas law (10.3, 10.4, lab) 

5. Kinetic molecular theory (10.5, 10.6, Phet, POGIL)

6. Deviation from ideal gas law (10.7)

7. Solutions and mixtures (4.5, 13.1)

8. Representations of solutions (13.1)

9. Separations of solutions and mixtures (1.3, lab, see ch 13 slides)

10. Solubility (13.2,  13.3)

11. Spectroscopy and the electromagnetic spectrum (6.1-6.3, see ch 6 slides)

12. Properties of photons (6.2, labs)

13. Beer-Lambert law (14.2 p. 572, lab, Phet)

College Board assignments:

AP daily video notes 3.1-3.3 (6 videos) 

AP topic questions 3.1-3.3 (6 MCQ questions)

AP daily video notes 3.4-3.6 (6 videos)

AP topic questions 3.4-3.6 (9 MCQ questions)

AP daily video notes 3.7-3.10 (5 videos)

AP topic questions 3.7-3.10 (9 MCQ questions) 

AP daily video notes 3.11-3.13 (4 videos)

AP topic questions 3.11-3.13 (9 MCQ questions))

AP 3.1-3.13 FRQ topic questions 

Unit 3 college board progress check MCQ, FRQ

Worksheets: 

Phet: gas laws and KMT (classwork)

https://phet.colorado.edu/en/simulation/gas-properties

POGIL: Maxwell Boltzmann distribution, Q 1-30 (classwork)

POGIL: deviations from ideal gas law, Q 1-26 (skip)

Phet: Beer Lambert law https://phet.colorado.edu/en/simulation/beers-law-lab

Lab exercises:

• Molar volume of a gas (collecting gasses over water, Mg and HCl): demonstration

• Separation of a dye mixture using paper chromatography; with pre-lab

• Gas emission spectra quantitative lab

Textbook assignments

• Reading the text is optional, as needed to support material in slides and AP daily videos. 

• For problems, you must show your work to receive credit.

• Check your answers for accuracy in the back of the book. Re-do work after checking answers if necessary.

Chapter 11 (corresponds to AP daily videos 1-3)

Problems ch 11 #  1, 2, 8, 11, 17, 19, 21, 23, 25, 27, 51, 53 (page 460-464)

Intermolecular forces Bozeman video https://www.youtube.com/watch?v=-QqTwJzi7Wo

In class: slides for ch 11 section 1, 2, 5

Chapter 10 (corresponds to AP daily videos 4-6)

Problems ch 10.1-3 # 13, 33, 39, 47 (page 424-425)

Problems ch 10.4 # 61, 63 (page 426-427), and Practice Exercise under 10.11 on page 407 (Voyager space probe question, use mole fraction)

Problems ch 10.5-7 # 75, 79, 89 (page 427-428) (for 79b, just answer for average speed of molecules)

Phet: gas laws and KMT

Maxwell-Boltzmann distribution POGIL, Q 1-30

Deviations from Ideal gas law POGIL, Q 1-26 (SKIP)

In class: slides for ch 10 sections 1-7

Chapter 13, 4.5, 1.3 (corresponds to AP daily videos 7-10)

Problems ch 13 # 3, 7, 15, 27, 29, 31, 33, 43 (page 557-560)

In class: slides for ch 13 section 1-3, slides for chapter 4 section 5 (in ch 13 slides)

Chapter 6 (corresponds to AP daily videos 11-13)

Problems ch 6 # 17, 21, 25, 29 a-b (page 249-250)

Spectroscopy and Beer Lambert Bozeman video  https://www.youtube.com/watch?v=OQwTcl9TeUM

Beer Lambert Phet

In class: slides for ch 6 section 1-3

Key concepts text chapter 6

6.1

• Electromagnetic spectrum, Fig 6.4

• Wavelength and frequency are inversely proportional

• Energy and frequency are directly proportional 

6.2

• Photoelectric effect explained light’s particle nature

• Photon = packet of energy (particle)

• Quantum = smallest packet of energy that can be emitted or absorbed as electromagnetic radiation

6.1-6.2 calculations

E = h v 

c = λ v

109 nm = 1 m (or 1 nm = 10-9 m)

c = speed of light = 3.00 x 108m/s

h = Planck’s constant = 6.626 x 10-34 J s

Hertz = Hz = one wave per sec = 1/s = sec-1

6.3

• Differences in absorption or emission are related to specific electron transitions

• When a photon is absorbed or emitted by an atom, its energy is increased or decreased by an amount equal to the energy of the photon

• Ground state vs. excited state

Key concepts text chapter 10

10.1

• Characteristics of gasses

10.3

• Background: gas pressure is due to collisions between gas particles, and collisions between particles and the walls of the container

• Ideal Gas Law: PV=nRT (given on test)

  • P, V are inversely proportional

  • P, n; P, T; V, n; V, T are directly proportional 

  • R = ideal gas constant = 0.08206 L*atm/mol*K (given on test)

• Convert all temperatures to K to solve gas laws: K = C + 273

• Use the Ideal Gas Law to derive other laws that describe relationships among P, V, n, T: Sample Exercises 10.4, 10.5, 10.6

• Gas density = (pressure) (molar mass)

(R) (temperature)

Conceptual only: understand that density is directly proportional to pressure and molar mass and inversely proportional to temperature

10.4

• Total pressure of a gas = sum of partial pressures

  • P total = P1 + P2 + P3 + P4….

• Given a gas mixture and data about the gas mixture, use law of partial pressures to solve for total pressure

  • P = nRT/V

  • P total = (n1 + n2 + n3 + n4…) RT/V

  • Partial pressure of gas a is:   Pa = na RT/V

• Mole fraction of a gas (call it gas 1) in a gas mixture: 

  • X1 = moles gas 1 / moles total gas = n1/nt

• Partial pressure of a gas (call it gas 1) in a gas mixture:

  • P1 = (n1/nt) Pt = X1Pt

10.5

• Understand kinetic molecular theory of gasses: p. 418

• Distribution of molecular speed Fig 10.13

• Maxwell Boltzmann distribution: fraction of molecules vs. average kinetic energy, at specific temperature

• Average kinetic energy of gas particles KE= ½ mv2 (from 5.1)

• Average KE and speed are proportional to Kelvin temperature

10.7

• What causes deviations from Ideal Gas Law (qualitative only)

  • High pressure / low volume (liquefication conditions)

  • Low temperature

  • Attractive forces between particles

  • Large particle size/ large particle volume

Key concepts text chapter 11

11.1

General properties of liquids vs. solids vs. gasses

11.2

Table 11.2: Intramolecular vs. intermolecular forces, relative strengths

Intermolecular forces

London dispersion forces or dispersion forces

Dipole-dipole forces or dipole-dipole interactions

(These 2 are collectively called van der Waals forces)

Hydrogen bonding or H-bonding: requires H-O, H-N, or H-F

Ion-dipole forces

11.5

What is vapor pressure, effect of temperature and pressure on vapor pressure

Effect of IMFs on vapor pressure, boiling point

Maxwell-Boltzmann curve, Fig 11.23

Key concepts text chapter 13, 4.5, 1.3

1.3

Solutions (homogeneous mixtures) can be separated by distillation or chromatography

Filtration cannot separate a homogeneous mixture

4.5 

Molarity, unit of concentration,  M = moles solute/L solution

Moles = M x L

Sample Exercise 4.11, 4.12, 4.13

Dilution, M1V1 = M2V2

13.1

Intermolecular forces & effect on solution formation

solute-solute, solvent-solvent, solute-solvent

(Energetics is not covered in AP unit 3)

13.2

Definition of solubility

13.3

Solute-solvent interactions: like dissolves like

Substances with similar intermolecular interactions tend to be soluble with each other