Chapter 10 - Liquids and Solids
Day 1
08/17
Syllabus
- Introduction to intermolecular forces
- Ask, “What makes an ideal gas, ideal?” at end. Lead into
liquids.
Canvas Exams
Day 2
08/19
Intermolecular Forces
Opener
Outlines of Theoretical Chemistry - Getman - 1913 - pg.
79
PDF
- Show intermolecular forces graph
- Draw structures and discuss boiling points (PDF)
- IMF strength
- Predominant IMF
- Mass/size
- Surface area
- Viscosity
- Correlates with IMF strength
- Decreases with increasing temperature
- Surface Tension
- Correlates with IMF strength
- Decreases with increasing temperature
Canvas Exams
- Intermolecular Forces
- Viscosity
- Surface Tension
Day 3
08/22
Opener
Principles of Physical Chemistry - Brey - 1958 - pg.
25-26
PDF
- Volatile vs non-volatile
- Phase Transitions
- q = Hgas - Hliquid
= ΔHvap
- q = Hliquid -
Hsolid = ΔHfus
- latent heat of vaporization, ΔHvap
- latent heat of fusion, ΔHfus
- latent heat of sublimation, ΔHsub = ,
ΔHfus + ΔHvap
- Compare reverse process
- -ΔHcondensation = ΔHvap
- -ΔHfreezing = ΔHfus
- -ΔHdeposition = ΔHsub
- Compare/contrast different values for ΔHvap and
ΔHfus (extensive property)
- Example: Water, 43.98 kJ mol-1; acetic acid 23.36 kJ
mol-1
- If 10 mol of each were vaporized at the same temperature, water
would require more heat to vaporize
- Vapor Pressure
- Equilibrium of vapor and liquid at some temperature
- Note: As vaporization occurs, the liquid cools - must be done slowly
to ensure equilibrium
- Increases with increasing temperature
Canvas Exams
Day 4
8/24
- Clausius-Clapeyron
- Relates vapor pressure and temperature
- Show “extensive property” of ΔHvap for Canvas
Exam (Question 5)
Canvas Exams
Day 5
08/26
- Discuss HW Exam Policies
- Phase Diagrams
- Heating Curves
- For heating a substance (extensive property)
- For phase transitions (extensive property)
- latent heat of vaporization
- latent heat of fusion
Canvas Exams
Day 6
08/29
Opener
Outlines of Theoretical Chemistry - Getman - 1913 - pg.
128–130
PDF
- Solids
- General types
- Unit cells (cubic) - pg. 130
- Equivalent atoms
- Empirical formula
Chapter 11 - Solutions
Day 7
8/31
Opener
Outlines of Theoretical Chemistry - Getman - 1913 - pg.
145
PDF
- Solutions
- Concentration Units (Part 1)
- Concentration doesn’t change with mass/volume of solution
- Whiteboard work PDF
No Canvas Exam – Fundamentals Exam at 6PM
Day 8
9/2
- Solubility
- Concentration Units (Part 2)
Canvas Exams
HW Exam 10 due 9/4 at 5AM
Day 9
9/7
- Solubility
- “Like dissolves like”
- Gases
- Solubility vs temperature
- Solubility vs pressure
- Henry’s Law
- Inorganics
- Solubility vs temperature
Canvas Exams
Day 10
9/9
- Solubility
- Organics
- Solubility vs IMFs
- Aryl halides – more dispersion – decreasing solubility
- armoatics/resonance/hybrid orbitals
- Electrolytes
- Van’t Hoff factor
- Difference between moles of X and moles of particles
- NaCl(aq) → Na+(aq) +
Cl–(aq) 1 mol NaCl vs 2 mol of dissolved
particles
- Van’t Hoff flashcards (slides)
Canvas Exams
Day 11
9/12
- Colligative Properties
- Board work
- Vapor pressure lowering
- Freezing point depression
- Boiling point elevation
- Osmotic pressure
Canvas Exams
- Colligative Properties
Chapter 12 - Kinetics
Day 12
9/14
Opener
Outlines of Theoretical Chemistry - Getman - 1913 - pg.
161
PDF
- Chemical Kinetics and Reaction Velocity
- Average rate
- Instantaneous rate
- Rate expression
- Board work
Canvas Exams
Day 13
9/16
Opener
Outlines of Theoretical Chemistry - Getman - 1913 - pg.
164
PDF
- Rate laws (PDF)
- Multi-step vs. elementary step
- Method of Initial rates
Canvas Exams
Day 14
9/19
- Integrated Rate laws PDF
- Rate constant units
- Half-life
- Molecularity
Canvas Exams
Day 16
9/23
- Overview (PDF)
- Kinetics Excel Worksheet (XLSX)
- N2O4
Rate Data (Butterworths, 1973)
- ΔH, ΔS, ΔG, K, k
- Reaction energy diagram
Day 17
9/26
- Review energy diagrams
- Catalysts and enzymes (PDF)
- Arrhenius and equilibrium board work (PDF)
- Arrhenius plot (k vs. T; ln(k) vs 1/T)
- Finding Ea
- Finding K from ΔG°
- Finding Krev
Canvas Exams
Chapter 13 – Equilibrium
Day 18
9/28
- Equilibrium board work (PDF)
- Equilibrium expression from rate laws
- ICE Tables and equilibrium problems
- NO2 at 25 °C
- Cubic functions
- Small ‘x’ approximation
Day 19
9/30
- Correcting the equilibrium constants (PDF)
- Equilibrium board work (PDF)
Day 20
10/3
- Equilibrium problems – Different types
- Q vs. K
Canvas Exams
Day 21
10/5
- Take-Home Exam – Instructions
- Review
Canvas Exams
Day 22
10/07
- Equilibrium concentrations vs. equilibrium pressures
- Le Chatelier’s Principle
- Transforming K
Canvas Exams
Day 23
10/10
- Ksp, solubility, and thermodynamics (Link)
Chapter 14 – Acid/Base Equilibria
Day 24
10/12
- Oxidation-Reduction reactions
- Acid-ionization reactions
- Strong vs. weak acids (Ka)
- 3 M HCl vs HF equilibria and pH
Day 25
10/17
- Acid/Base definitions
- Identifying conjugates
Canvas Exams
Day 26
10/19
- Ka/Kb/Kw
- pKa/pKb/pKw
- pH/pOH/pKw
- Acidic/basic salts
Day 27
10/21
- Recap
- Salts
- pH of strong/weak acid solutions
- pH of water (at varying T)
- Percent ionization
- Introduction to buffers
Canvas Exams
- Acid Base Relationships
- Acid Ionization
Day 28
10/24
- Buffers and Henderson-Hasselbalch
Canvas Exams
Chapter 15 – Other Equilibria
Day 31
10/31
- Recap Ksp
- Common ion
- Formation constant
Canvas Exams
Chapter 16 – Thermodynamics
Day 32
11/02
- Recap ΔH, ΔS, and ΔG
- Entropy – predictions
Day 34
11/07
- Gibbs free energy
- ΔG, K, and Q
- Exam instructions
Day 35
11/09
No formal class meeting – Comprehensive Exam 6PM
Day 36
11/11
- Thermodynamics: Energy scaling with reaction amount
Chapter 17 - Electrochemistry
Day 37
11/14
- Exam recap
- Refresh of redox reactions (PDF)
- Oxidation-Reduction
- Oxidation states
Day 38
11/16
- Notes (PDF)
- Half-reactions
- Galvanic cell
- Cell notation
- Ecell, ΔG°, K
Day 39
11/18
- Nernst Equation
- Concentration Cell
Day 40
11/26
- Quantitative electrochemistry
Chapter 21
Day 41
11/28
- Isotopic notation
- Radioactivity
- Balancing nuclear reactions
Day 42
11/30
- Nuclear kinetics
- Mass-energy equivalence
- Fusion/Fission
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## Chapter 10 - Liquids and Solids

### Day 1

08/17

**Syllabus**

* Introduction to *intermolecular forces*
  * Ask, "What makes an ideal gas, ideal?" at end. Lead into liquids.

**Canvas Exams**

* Syllabus

### Day 2

08/19

*Intermolecular Forces*

<details>
<summary>**Opener**</summary>
<div id = "dropdown">

*Outlines of Theoretical Chemistry* - Getman - 1913 - pg. 79

[PDF](liquids-introduction.pdf)

![](liquids-introduction.jpg){width=50%}

</div>
</details> 

* Show *intermolecular forces graph*
* Draw structures and discuss boiling points ([PDF](imfs-and-bps.pdf))
  * IMF strength
  * Predominant IMF
  * Mass/size
  * Surface area
* *Viscosity*
  * Correlates with IMF strength
  * Decreases with increasing temperature
* *Surface Tension*
  * Correlates with IMF strength
  * Decreases with increasing temperature
  
**Canvas Exams**

* Intermolecular Forces
* Viscosity
* Surface Tension

### Day 3

08/22

<details>
<summary>**Opener**</summary>
<div id = "dropdown">

*Principles of Physical Chemistry* - Brey - 1958 - pg. 25-26

[PDF](vapor-pressure.pdf)

![](vapor-pressure-1.jpg){width=50%}

![](vapor-pressure-2.jpg){width=50%}

![](vapor-pressure-3.jpg){width=50%}

![](vapor-pressure-4.jpg){width=50%}

![](vapor-pressure-5.jpg){width=50%}

</div>
</details> 

* Volatile vs non-volatile
* Phase Transitions
  * *q* = *H*<sub>gas</sub> - *H*<sub>liquid</sub> = &Delta;*H*<sub>vap</sub>
  * *q* = *H*<sub>liquid</sub> - *H*<sub>solid</sub> = &Delta;*H*<sub>fus</sub>
  * latent heat of vaporization, &Delta;*H*<sub>vap</sub>
  * latent heat of fusion, &Delta;*H*<sub>fus</sub>
  * latent heat of sublimation, &Delta;*H*<sub>sub</sub> = , &Delta;*H*<sub>fus</sub> + &Delta;*H*<sub>vap</sub>
  * Compare reverse process
    * -&Delta;*H*<sub>condensation</sub> = &Delta;*H*<sub>vap</sub>
    * -&Delta;*H*<sub>freezing</sub> = &Delta;*H*<sub>fus</sub>
    * -&Delta;*H*<sub>deposition</sub> = &Delta;*H*<sub>sub</sub>
* Compare/contrast different values for &Delta;*H*<sub>vap</sub> and &Delta;*H*<sub>fus</sub> (extensive property)
  * Example: Water, 43.98 kJ mol<sup>-1</sup>; acetic acid 23.36 kJ mol<sup>-1</sup>
  * If 10 mol of each were vaporized at the same temperature, water would require more heat to vaporize
* Vapor Pressure
  * Equilibrium of vapor and liquid at some temperature
    * Note: As vaporization occurs, the liquid cools - must be done slowly to ensure equilibrium
  * Increases with increasing temperature

    
**Canvas Exams**

* Enthalpy
* Vapor pressure

### Day 4

8/24

* Clausius-Clapeyron
  * Relates vapor pressure and temperature
  * Show "extensive property" of &Delta;*H*<sub>vap</sub> for Canvas Exam (Question 5)
    
**Canvas Exams**

* Clausius-Clapeyron

### Day 5

08/26

* Discuss HW Exam Policies
* Phase Diagrams
* Heating Curves
  * For heating a substance (extensive property)
    * specific heat
  * For phase transitions (extensive property)
    * latent heat of vaporization
    * latent heat of fusion

**Canvas Exams**

* Phases
* Heating Curves


### Day 6

08/29

<details>
<summary>**Opener**</summary>
<div id = "dropdown">

*Outlines of Theoretical Chemistry* - Getman - 1913 - pg. 128–130

[PDF](solids.pdf)

![](solids-1.jpg){width=50%}

![](solids-2.jpg){width=50%}

![](solids-3.jpg){width=50%}

</div>
</details> 

* Solids
  * General types
  * Unit cells (cubic) - pg. 130
  * Equivalent atoms
  * Empirical formula

<br>

## Chapter 11 - Solutions

### Day 7

8/31

<details>
<summary>**Opener**</summary>
<div id = "dropdown">

*Outlines of Theoretical Chemistry* - Getman - 1913 - pg. 145

[PDF](solutions.pdf)

![](solutions-1.jpg){width=50%}

</div>
</details>


* Solutions
  * Types
* Concentration Units (Part 1)
  * Concentration doesn't change with mass/volume of solution
  * Whiteboard work [PDF](solutions-whiteboard.pdf)

No Canvas Exam -- Fundamentals Exam at 6PM

### Day 8

9/2

* Solubility
  * Unsaturated
  * Saturated
* Concentration Units (Part 2)
  * [Concentration Conversions](https://dornshuld.chemistry.msstate.edu/books/chemistry/concentration-conversions.html)
  * Whiteboard work [PDF](conc-conversions.pdf)
  * Demonstrate that any mass could be assumed... concentration doesn't change
  
**Canvas Exams**

* Concentration Units

HW Exam 10 due 9/4 at 5AM

### Day 9

9/7

* Solubility
  * "Like dissolves like"
  * Gases
    * Solubility vs temperature
      * CO<sub>2</sub> in warming oceans
    * Solubility vs pressure
    * [Henry's Law](henrys-law.pdf)
  * Inorganics
    * Solubility vs temperature

**Canvas Exams**

* Henry's Law

### Day 10

9/9

* Solubility
  * Organics
    * Solubility vs IMFs
    * Aryl halides -- more dispersion -- decreasing solubility
      * armoatics/resonance/hybrid orbitals
* [Electrolytes](electrolytes.pdf)
  * Van't Hoff factor
  * Difference between moles of X and moles of particles
    * NaCl(*aq*) &rarr; Na<sup>+</sup>(*aq*) + Cl<sup>–</sup>(*aq*) &nbsp;&nbsp;&nbsp; 1 mol NaCl vs 2 mol of dissolved particles
  * Van't Hoff flashcards ([slides](https://dornshuld.chemistry.msstate.edu/slides/vant-hoff/))


**Canvas Exams**

* Electrolytes

### Day 11

9/12

* Colligative Properties
  * [Board work](colligative-properties.pdf)
  * Vapor pressure lowering
  * Freezing point depression
  * Boiling point elevation
  * Osmotic pressure

**Canvas Exams**

1. Colligative Properties

## Chapter 12 - Kinetics

### Day 12

9/14

<details>
<summary>**Opener**</summary>
<div id = "dropdown">

*Outlines of Theoretical Chemistry* - Getman - 1913 - pg. 161

[PDF](kinetics-introduction.pdf)

![](kinetics-introduction-1.jpg){width=50%}

![](kinetics-introduction-2.jpg){width=50%}

</div>
</details> 


* Chemical Kinetics and Reaction Velocity
* Average rate
* Instantaneous rate
* Rate expression
* [Board work](reaction-rates-1.pdf)

**Canvas Exams**

* Average Rates

### Day 13

9/16

<details>
<summary>**Opener**</summary>
<div id = "dropdown">

*Outlines of Theoretical Chemistry* - Getman - 1913 - pg. 164

[PDF](rate-law.pdf)

![](rate-law-1.jpg){width=50%}

![](rate-law-2.jpg){width=50%}

![](rate-law-3.jpg){width=50%}


![](rate-law-4.jpg){width=50%}

</div>
</details> 

* Rate laws ([PDF](rate-laws.pdf))
  * Multi-step vs. elementary step
* Method of Initial rates

**Canvas Exams**

* Method of Initial Rates

### Day 14

9/19

* Integrated Rate laws [PDF](int-rate-law-half-life.pdf)
* Rate constant units
* Half-life
  * Derive zeroth-order
* Molecularity

**Canvas Exams**

* Integrated Rate Laws

### Day 15

9/21

* Arrhenius Equation ([PDF](arrhenius-equation.pdf))
* [NO<sub>2</sub> Rate Data](no2-rate-data-butterworths-1973.pdf) (Butterworths, 1973)

**Canvas Exams**

* Arrhenius Equation

### Day 16

9/23

* Overview ([PDF](thermo-and-kinetics.pdf))
* Kinetics Excel Worksheet ([XLSX](no2-worksheet.xlsx))
* [N<sub>2</sub>O<sub>4</sub> Rate Data](n2o4-rate-data-butterworths-1973.pdf) (Butterworths, 1973)
* &Delta;*H*, &Delta;*S*, &Delta;*G*, *K*, *k*
* Reaction energy diagram

### Day 17

9/26

* Review energy diagrams
* Catalysts and enzymes ([PDF](catalysts-and-enzymes.pdf))
* Arrhenius and equilibrium board work ([PDF](arrhenius-and-equilibrium.pdf))
  * Arrhenius plot (k vs. T; ln(k) vs 1/T)
  * Finding *E*<sub>a</sub>
  * Finding *K* from &Delta;*G*&deg;
  * Finding *K*<sub>rev</sub>

**Canvas Exams**

* Energy Diagrams

## Chapter 13 – Equilibrium

### Day 18

9/28

* Equilibrium board work ([PDF](equilibrium-1.pdf))
* Equilibrium expression from rate laws
* ICE Tables and equilibrium problems
  * NO<sub>2</sub> at 25 &deg;C
  * Cubic functions
  * Small 'x' approximation

### Day 19

9/30

* Correcting the equilibrium constants ([PDF](finding-equilibrium-constant.pdf))
* Equilibrium board work ([PDF](equilibrium-2.pdf))
  * NO<sub>2</sub> at 727 &deg;C

### Day 20

10/3

* Equilibrium problems -- Different types
* *Q* vs. *K* 

**Canvas Exams**

* Equilibrium Basics

### Day 21

10/5

* Take-Home Exam -- Instructions
* Review
  * Kinetics and Equilibrium

**Canvas Exams**

* Equilibrium

### Day 22

10/07

* Equilibrium concentrations vs. equilibrium pressures
  * *K*<sub>c</sub> vs. *K*<sub>p</sub>
* Le Chatelier's Principle
* Transforming *K*

**Canvas Exams**

* Le Chatelier's Principle

### Day 23

10/10

* *K*<sub>sp</sub>, solubility, and thermodynamics ([Link](https://dornshuld.chemistry.msstate.edu/books/chemistry/solubility-product-ksp.html))

## Chapter 14 – Acid/Base Equilibria

### Day 24

10/12

* Oxidation-Reduction reactions
  * Oxidation numbers
* Acid-ionization reactions
  * Strong vs. weak acids (*K*<sub>a</sub>)
  * 3 *M* HCl vs HF equilibria and pH

### Day 25

10/17

* Acid/Base definitions
* Identifying conjugates

**Canvas Exams**

* Acid Base Basics

### Day 26

10/19

* *K*<sub>a</sub>/*K*<sub>b</sub>/*K*<sub>w</sub>
* p*K*<sub>a</sub>/p*K*<sub>b</sub>/p*K*<sub>w</sub>
* pH/pOH/p*K*<sub>w</sub>
* Acidic/basic salts

### Day 27

10/21

* Recap
  * Salts
  * pH of strong/weak acid solutions
  * pH of water (at varying *T*)
* Percent ionization
* Introduction to buffers

**Canvas Exams**

* Acid Base Relationships
* Acid Ionization

### Day 28

10/24

* Buffers and Henderson-Hasselbalch

**Canvas Exams**

* Buffers

### Day 29

10/26

* Titrations

### Day 30

10/28

* Titrations

## Chapter 15 -- Other Equilibria

### Day 31

10/31

* Recap *K*<sub>sp</sub>
* Common ion
* Formation constant

**Canvas Exams**

* Solubility Product

## Chapter 16 -- Thermodynamics

### Day 32

11/02

* Recap &Delta;*H*, &Delta;*S*, and &Delta;*G*
* Entropy -- predictions

### Day 33

11/04

* Entropy

### Day 34

11/07

* Gibbs free energy
* &Delta;*G*, *K*, and *Q*
* Exam instructions

### Day 35

11/09

No formal class meeting -- Comprehensive Exam 6PM


### Day 36

11/11

* Thermodynamics: Energy scaling with reaction amount

## Chapter 17 - Electrochemistry

### Day 37

11/14

* Exam recap
* Refresh of redox reactions ([PDF](oxidation-numbers-redox.pdf))
  * Oxidation-Reduction
  * Oxidation states

### Day 38

11/16

* Notes ([PDF](electrochem-1.pdf))
* Half-reactions
* Galvanic cell
* Cell notation
* *E*<sub>cell</sub>, &Delta;*G*&deg;, *K*

### Day 39

11/18

* Nernst Equation
* Concentration Cell

### Day 40

11/26

* Quantitative electrochemistry

## Chapter 21

### Day 41

11/28

* Isotopic notation
* Radioactivity
* Balancing nuclear reactions

### Day 42

11/30

* Nuclear kinetics
* Mass-energy equivalence
* Fusion/Fission

<br>
<br>
