VCE Chemistry: Organic Compounds and Functional Groups

Recap - Organic Chemistry

Organic Compounds:
- Haloalkanes contain carbon, hydrogen, and at least one halogen atom.
- Alcohols and carboxylic acids contain carbon, hydrogen, and oxygen.
Functional Groups:
- The chemically reactive part of a molecule affecting its properties.
- Definition: Specific groups of atoms within a compound that affect the properties of the compound.
Categories of organic compounds include:
- Alkanes: e.g., ethane $( ext{CH}3 ext{CH}3)$ .
- Alkenes: e.g., ethene $( ext{CH}2 ext{CH}2)$ .
- Haloalkanes: e.g., chloroethane $( ext{CH}3 ext{CH}2 ext{Cl})$ .
- Alcohols: e.g., ethanol $( ext{CH}3 ext{CH}2 ext{OH})$ .
- Carboxylic acids: e.g., ethanoic acid $( ext{CH}_3 ext{COOH})$ .

Haloalkanes

Definition:
- Organic compounds that have one or more halogen atoms (F, Cl, Br, or I) bonded to a carbon atom in the carbon chain.
General Formula:
- $ext{C}x ext{H}y ext{X}_z$ where X represents halogens.
Polar Bonds:
- C-X bonds are polar due to halogens being electronegative, resulting in dipole-dipole interactions between molecules, leading to higher boiling points compared to alkanes and alkenes of similar carbon chains.
Synthesis Role:
- Haloalkanes serve as intermediates in chemical syntheses.
Environmental Notice:
- CFCs (chlorofluorocarbons), a type of haloalkane, have been phased out due to their ozone-depleting properties.
Solubility:
- Haloalkanes are generally not water-soluble.

Naming Haloalkanes

Steps to Name Haloalkanes:
1. Name the alkane part, use the smallest number for halogens.
2. Add the halogen prefix to the front, indicating its position.
Prefixes for Halogens:
- Fluoro (F), Chloro (Cl), Bromo (Br), Iodo (I).
Side Chain Multipliers:
- Di (2), Tri (3), Tetra (4), Penta (5).

Worked Example: Naming Haloalkane

Example Structure:
- Compound structure for naming:
  $ext{H}_3 ext{C}- ext{C}( ext{Cl})( ext{H})- ext{C}( ext{I})( ext{H})- ext{N}( ext{H})$
Sample Answer:
- Name: 3,4-dichloro-3-iodoheptane.
- Breaking Down the Name:
- Position of functional group: 3,4.
- Type of halogen functions: dichloro (2 chloro), iodo (1 iodo).

Alcohols

Functional Group:
- Hydroxyl group (-OH).
Definition:
- An organic compound that has a hydroxyl (-OH) group bonded to a carbon atom in the parent chain.
Common Examples:
- n-Propanol (Propyl alcohol): $ext{C}3 ext{H}8 ext{O}$ , propan-1-ol and propan-2-ol.
- Cholesterol: $ext{C}{27} ext{H}{46} ext{O}$ .

Properties of Alcohols

Hydroxyl groups are polar, enhancing solubility in water for small-chain alcohols.
Alcohols exhibit higher boiling points than alkanes due to hydrogen bonding.
General Formula for Alcohols:
- $ext{C}x ext{H}{2} ext{OH}$ .

Naming Alcohols

Naming Rules:
1. Identify the longest continuous carbon chain containing the hydroxyl group.
2. Use the suffix 'ol'.
Common Mistakes:
- Misspelling names results in penalties.

Carboxylic Acids

Functional Group:
- Carboxyl (-COOH).
Definition:
- An organic compound that contains a carboxyl functional group.
Common Names and Formulas:
- Methanoic acid (formic acid): $ext{HCOOH}$ .
- Ethanoic acid (acetic acid): $ext{CH}_3 ext{COOH}$ .
General Formula:
- $ext{C}x ext{H}y ext{COOH}$ .

Properties of Carboxylic Acids

Highly polar, can form dimers via hydrogen bonding, resulting in elevated boiling points compared to alcohols and alkanes.
Typically, small molecules are water-soluble.
Classified as weak acids in chemical behavior.

Naming Carboxylic Acids

Naming Rules:
1. Identify the longest chain containing the carboxyl group, which has priority number 1.
2. Use the suffix 'oic acid'.
Examples:
- Methanoic acid: $ext{HCOOH}$ ; Ethanoic acid: $ext{CH}_3 ext{COOH}$ .

Overview of Water as a Unique Chemical

Water is unique because it exists naturally in three states of matter at Earth's surface: solid, liquid, and gas.
The continuous movement of water through our ecosystem is known as the Water Cycle.
- The water cycle describes the transitions of water between solid (ice), liquid (water), and gas (water vapor).

Importance of Water

Despite covering approximately 71% of the Earth's surface, only 3% of Earth's water is drinkable, with just 1% of that being accessible for human use.

Study Design Dot Points

Examine the existence of water in all three states at Earth's surface.
Analyze the distribution and proportion of available drinking water.

Risks Associated with Dihydrogen Monoxide (DHMO)

DHMO, commonly known as water, has several associated risks despite being vital for life:
- Soil Erosion: Contributes to the erosion of soil.
- Acid Rain Component: DHMO is also known as hydroxyl acid and is a major component of acid rain, which can harm ecosystems and structures.
- Tissue Damage: Prolonged exposure to solid DHMO (ice) can cause severe tissue damage, especially in extreme temperatures.
- Metal Corrosion: Accelerates the corrosion and rusting of many metals, impacting infrastructure.
- Burns: Gaseous DHMO (steam) can cause severe burns upon contact with skin.
- Greenhouse Effect: Contributes to the greenhouse effect, impacting climate change.

Availability of Drinking Water

Potable Water: Water that is safe enough to drink. Various sources include:
- Rivers flowing through protected catchments.
- Water obtained directly from rivers or lakes.
- Groundwater: Water held underground in the soil or in pores and fractures of rock.
- Rainwater collected from roofs and stored in tanks.
- Desalinated Seawater: Seawater treated to remove salt for drinking purposes.
- Reservoirs: Key sources of household water in Australian cities, supplied by rivers.

Assessing the Drinking Water Sources

Quiz Questions:
- Where is most of the drinkable water found on Earth?
- A. Ice
- B. Lakes
- C. Groundwater
- D. Oceans
- E. I don’t know.
Correct Answers Include Corporations of Groundwater, Lakes, and Ice as sources of drinkable water, though oceanic sources are not directly drinkable.

Key Definitions and Concepts

Water Cycle: The process where water circulates from the Earth’s surface to the atmosphere and back, undergoing various transformations between its states.
Potable Water: Describes water that is safe for drinking and meets health standards.

Summary of Water Properties

Water’s unique physical and thermal properties affect its movement and behavior in the environment.
The dependence on water cycles and sources directly relates to human consumption needs.

Importance of Water

Water's Significance: Constitutes approximately 80% of living organisms.
Age-related Variability: Water composition varies with age, spanning from infancy (80% water) to elder years (50%).

VCE Chemistry Overview

Unit Focus: Unit 2 Area of Study 1: Exploring the Interaction of Chemicals with Water
Lesson Theme: Understanding water as a unique chemical through its physical and thermal properties.

Lesson Topics

Anomalous Properties of Water (H₂O):
- Explanation of unique characteristics, particularly focusing on hydrogen bonding.
- Discuss trends in boiling points of Group 16 hydrides.
- Examination of ice's density in comparison to liquid water at low temperatures.
- Analysis of specific heat capacity including units and symbol utilization.
- Discussion on the relatively high latent heat of vaporization and its effect on ocean temperature regulation and aquatic life.

Key Definitions

Hydrogen Bonding:
- The interaction between hydrogen and electronegative atoms like oxygen, nitrogen, or fluorine, creating strong intermolecular forces.
Polar Molecule:
- A molecule exhibiting significantly different electronegativities between its constituent atoms, resulting in partial positive and negative charges.
Dispersion Forces:
- Temporary intermolecular forces that result from the uneven distribution of electrons within molecules, significantly weaker than hydrogen bonds.

Water and Group 16 Hydrides

Comparison: Water's melting and boiling points are significantly higher than other Group 16 hydrides due to stronger hydrogen bonds.
- Group 16 Hydride Melting and Boiling Points:
- Water (H₂O): Melting Point: 0°C, Boiling Point: 100°C
- Hydrogen Sulfide (H₂S): Melting Point: -82°C, Boiling Point: -60.7°C
- Hydrogen Selenide (H₂Se): Melting Point: -66°C, Boiling Point: -41.5°C
- Hydrogen Telluride (H₂Te): Melting Point: -49°C, Boiling Point: -2.2°C
- Hydrogen Polonide (H₂Po): Melting Point: -35°C, Boiling Point: 36.1°C

Specific Heat Capacity of Water

Definition:
- Specific heat capacity is the quantity of energy (in Joules) required to increase the temperature of a specific quantity (usually 1g) of a substance by 1°C.
Specific Heat Values:
- Water: 4.18 J/g/°C
- Ethanol: 2.4 J/g/°C
- Sand: 0.48 J/g/°C
- Copper: 0.3 J/g/°C
- Lead: 0.16 J/g/°C
- Iron: 0.45 J/g/°C

Heat Capacity Calculation

Equation: $E = mc imes riangle T$
Interpretation: The heat energy (E) required to change the temperature of a given mass (m) of substance by a particular temperature change ( $riangle T$ ) can be calculated using specific heat capacity (c).
Example Calculation:
1. To find the energy needed to heat 220 mL of water by 20°C:
2. Volume of Water: 220 mL
3. Density of Water: 0.997 g/mL
4. Mass of Water: $m = 220 ext{ mL} imes 0.997 ext{ g/mL} = 219.34 ext{ g}$
5. Temperature Change: $riangle T = 20°C$
6. Specific Heat: $c = 4.18 ext{ J/g/°C}$
7. Energy Calculation: $E = 219.34 ext{ g} imes 4.18 ext{ J/g/°C} imes 20°C = 18336.82 ext{ J}$
8. Convert to kJ: $= rac{18336.82}{1000} = 18.34 ext{ kJ}$

Density of Water in Different States

Comparative Density:
- Liquid water is denser than solid water (ice).
- Ice floats due to lower density resulting from the unique geometric arrangement of hydrogen bonds.

Definitions

Density: The mass of a substance per unit of volume.

Latent Heat

Definition:
- Latent heat is the energy absorbed or released by a substance during a phase change (e.g., solid to liquid, liquid to gas) without a change in temperature.
Examples of Phase Changes:
- Melting: Solid to liquid (fusion).
- Vaporization: Liquid to gas.
- Freezing: Liquid to solid.
- Condensation: Gas to liquid.

Latent Heat Values for Water

Latent Heat of Fusion: $6.0 ext{ kJ/mol}$
Latent Heat of Vaporization: $44.0 ext{ kJ/mol}$

Importance of Latent Heat in Living Systems

Example 1: Cooling Mechanism
- Sweating cools the body by evaporating sweat, which takes away significant heat energy.
Example 2: Water Cycle
- Constant evaporation and condensation rates maintain ecosystem balance due to high latent heat of vaporization.

Worked Examples

Calculating Latent Heat:
- To find the heat needed to evaporate 230 g of water at 100 °C:
  - Calculate moles: $n(H₂O) = rac{230 ext{ g}}{18.0 ext{ g/mol}} o 12.77 ext{ mol}$
  - Heat energy calculation: $q = n imes L o q = 12.77 ext{ mol} imes 44 ext{ kJ/mol} = 562.88 ext{ kJ}$
Final Temperature Calculation:
- Calculate the final temperature of water when heated with energy:
- $E = m imes c imes riangle T$
- E = 12 kJ → $riangle T = 41°C$

Summary of Key Points

Water shows strong intermolecular forces, particularly hydrogen bonding, resulting in notable physical and thermal properties.
These properties have significant implications on ecological and biological processes, supporting life on Earth.

Key Terms Recap

Hydrogen Bonding: Strong interactions arising between H and electronegative atoms.
Polar: Difference in electronegativities creating an uneven charge distribution.
Specific Heat Capacity: Amount of energy required to raise the temperature of a given mass by 1°C.
Density: Mass per unit volume.
Latent Heat: Energy involved in changes of state.

Additional Formulas

Heat Energy Calculation: $q = n imes L$
Change in Energy: $E = mc imes riangle</li></ul><h5 id="7b1bd921-7708-488c-b13a-b9de94d01827" data-toc-id="7b1bd921-7708-488c-b13a-b9de94d01827" collapsed="false" seolevelmigrated="true">Common Acids in Household and Industrial Applications</h5><ul><li>Hydrochloric Acid (HCl): Main component of stomach acid.</li><li>Sulfuric Acid (H₂SO₄): Used in car batteries.</li><li>Nitric Acid (HNO₃): Used in manufacturing fertilizers, dyes, and explosives.</li><li>Ethanoic Acid (CH₃COOH): Found in vinegar.</li><li>Carbonic Acid (H₂CO₃): Found in carbonated soft drinks.</li><li>Phosphoric Acid (H₃PO₄): Used in fertilizer manufacturing.</li></ul><h5 id="ced3012b-0fdf-4c0d-84cd-7f5df3c6e074" data-toc-id="ced3012b-0fdf-4c0d-84cd-7f5df3c6e074" collapsed="false" seolevelmigrated="true">Common Bases in Household and Industrial Applications</h5><ul><li>Sodium Hydroxide (NaOH): Utilized in drain and oven cleaners.</li><li>Ammonia (NH₃): Used in household cleaners, fertilizers, and explosives.</li><li>Calcium Hydroxide (Ca(OH)₂): Used as garden lime to adjust soil pH.</li><li>Magnesium Hydroxide (Mg(OH)₂): A key ingredient in some antacids.</li><li>Sodium Carbonate (Na₂CO₃): Used to manufacture washing powder.</li><li>Note: Bases can be as corrosive as acids and may cause chemical burns.</li></ul><h5 id="4ec32c96-43ef-47d5-b809-804327f783ca" data-toc-id="4ec32c96-43ef-47d5-b809-804327f783ca" collapsed="false" seolevelmigrated="true">Brønsted-Lowry Theory</h5><ul><li>Defines acid-base properties in terms of proton (H⁺) transfer.<ul><li>Brønsted-Lowry Acid: A proton donor</li><li>Brønsted-Lowry Base: A proton acceptor</li></ul></li><li>Mnemonic to remember the process: Acids Donate, Bases Accept (A.D.B.A.).</li><li>H⁺ in solution can be represented as either hydronium ion (H₃O⁺) or just H⁺.</li></ul><h5 id="8f86d8b7-f6e7-4b7b-9028-7c197f4db9fa" data-toc-id="8f86d8b7-f6e7-4b7b-9028-7c197f4db9fa" collapsed="false" seolevelmigrated="true">Amphiprotic Species</h5><ul><li>An amphiprotic species can act as an acid or a base depending on the reaction partner.<ul><li>Example Reactions:</li><li>HCl(aq) + H₂O(l) ⇌ H₃O⁺(aq) + Cl⁻(aq)</li><li>NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq)</li></ul></li></ul><h5 id="e96c430d-923c-4e0f-bf63-fd82037feabb" data-toc-id="e96c430d-923c-4e0f-bf63-fd82037feabb" collapsed="false" seolevelmigrated="true">Classification of Acids</h5><ul><li>Acids are classified based on the number of protons they can donate:<ol><li>Monoprotic Acids: Can donate 1 proton (e.g., HCl, CH₃COOH).</li><li>Diprotic Acids: Can donate 2 protons (e.g., H₂SO₄, H₂CO₃).</li><li>Triprotic Acids: Can donate 3 protons (e.g., H₃PO₄).</li></ol></li><li>Diprotic and triprotic acids do not donate all protons simultaneously.</li></ul><h5 id="dea5795c-b48d-477a-8ffb-337cb973781c" data-toc-id="dea5795c-b48d-477a-8ffb-337cb973781c" collapsed="false" seolevelmigrated="true">Example of Hydrogen Donation for Phosphoric Acid (H₃PO₄)</h5><ol><li>$ H₃PO₄(aq) + H₂O(l) ⇌ H₂PO₄⁻(aq) + H₃O⁺(aq) $- First hydrogen donation</li><li>$ H₂PO₄⁻(aq) + H₂O(l) ⇌ HPO₄²⁻(aq) + H₃O⁺(aq) $- Second hydrogen donation</li><li>$ HPO₄²⁻(aq) + H₂O(l) ⇌ PO₄³⁻(aq) + H₃O⁺(aq) $- Third hydrogen donation</li></ol><h5 id="6b1fef22-fbd8-4f9a-a8d2-61fa7c3d0268" data-toc-id="6b1fef22-fbd8-4f9a-a8d2-61fa7c3d0268" collapsed="false" seolevelmigrated="true">Understanding Hydrogen Donation of Carbonic Acid (H₂CO₃)</h5><ul><li>Potential hydrogen donations:<ul><li>A. 0</li><li>B. 1</li><li>C. 2</li><li>D. 3</li><li>E. I don’t know.</li></ul></li></ul><h5 id="78b079d4-3c13-453c-8f5b-15e4c8ba280d" data-toc-id="78b079d4-3c13-453c-8f5b-15e4c8ba280d" collapsed="false" seolevelmigrated="true">Strength and Concentration of Acids and Bases</h5><ul><li>Strong vs. Weak:<ul><li>Strong Acids: Ionize completely in solution and produce virtually no unreacted acid molecules.</li><li>Example:$ HCl(aq) + H₂O(l) → H₃O⁺(aq) + Cl⁻(aq) $</li><li>Weak Acids: Partially ionize, resulting in a small number of dissociated molecules along with a large number of unreacted acid molecules.</li><li>Example:$ CH₃COOH(aq) + H₂O(l) ⇌ CH₃COO⁻(aq) + H₃O⁺(aq) $</li></ul></li><li>Bases also follow similar ionization characteristics with complete ionization (strong) or partial ionization (weak).</li><li>Full Arrow (→) indicates a reaction with a strong acid or base.</li></ul><h5 id="8a7d8953-7b94-4e7c-a1a0-3564b415fbc7" data-toc-id="8a7d8953-7b94-4e7c-a1a0-3564b415fbc7" collapsed="false" seolevelmigrated="true">Distinction Between Strength and Concentration</h5><ul><li>Strength: Refers to the substance’s willingness to ionize (tendency to dissociate).</li><li>Concentration: Refers to the amount of acid or base ions present within a solution (amount of dissolved substance).</li></ul><h4 id="3d695617-a2a3-458b-9885-c0d44e95402d" data-toc-id="3d695617-a2a3-458b-9885-c0d44e95402d" collapsed="false" seolevelmigrated="true">What Would Happen If You Had No Stomach Acid?</h4><ul><li>Stomach Acid Role:<ul><li>Stomach acid (hydrochloric acid, HCl) is essential for digestion.</li><li>Without it, the body would struggle with breaking down food, especially proteins.</li><li>May lead to nutrient deficiencies and gastrointestinal issues.</li></ul></li></ul><h4 id="0f51f9a9-26bd-4c68-8491-c2dfd398fe81" data-toc-id="0f51f9a9-26bd-4c68-8491-c2dfd398fe81" collapsed="false" seolevelmigrated="true">Chemical Interaction with Water</h4><ul><li>Unit Focus:<ul><li>VCE Chemistry Unit 2: Area of Study 1</li><li>Topic: How do chemicals interact with water?</li></ul></li></ul><h5 id="8f68c955-3fef-4008-a89f-310726240d50" data-toc-id="8f68c955-3fef-4008-a89f-310726240d50" collapsed="false" seolevelmigrated="true">Acid-Base (Proton Transfer) Reactions</h5><ul><li>Definition of Acid-Base Reactions:<ul><li>Reactions where protons (H+) are transferred between reactants.</li></ul></li></ul><h4 id="a8d216d2-35e7-4bf2-b9d3-4b5b716fdac6" data-toc-id="a8d216d2-35e7-4bf2-b9d3-4b5b716fdac6" collapsed="false" seolevelmigrated="true">Reactions of Acids and Bases</h4><ul><li>General Reaction Formula:<ul><li>When an acid reacts with a base: $ \text{acid} + \text{base} \rightarrow \text{salt} + \text{water} $</li><li>Salt is defined generally as any ionic compound, not exclusively NaCl.</li></ul></li></ul><h5 id="1209ee3f-8d88-48d6-bdf9-1802317b162e" data-toc-id="1209ee3f-8d88-48d6-bdf9-1802317b162e" collapsed="false" seolevelmigrated="true">Neutralization Reactions</h5><ul><li>Known as a neutralization reaction when an acid and base interact.</li><li>Produces salt and water as primary products.</li></ul><h6 id="244bb65f-aaaf-496e-a5db-6eaf9614a65c" data-toc-id="244bb65f-aaaf-496e-a5db-6eaf9614a65c" collapsed="false" seolevelmigrated="true">Reaction Types:</h6><ol><li>Acid + Metal Hydroxide<ul><li>Produces salt and water.</li><li>Example: $ \text{sulfuric acid (H}2\text{SO}4\text{)} + \text{sodium hydroxide (NaOH)} \rightarrow \text{sodium sulfate (Na}2\text{SO}4\text{)} + \text{water (H}_2\text{O)} $</li><li>Full Equation: $ \text{H}2\text{SO}4(aq) + 2\text{NaOH}(aq) \rightarrow \text{Na}2\text{SO}4(aq) + 2\text{H}_2\text{O}(l) $</li><li>Ionic Equation: $ 2\text{H}^+(aq) + 2\text{OH}^-(aq) \rightarrow 2\text{H}_2\text{O}(l) $</li></ul></li><li>Acid + Metal Carbonate<ul><li>Produces salt, water, and carbon dioxide.</li><li>Example: $ \text{nitric acid (HNO}3\text{)} + \text{magnesium carbonate (MgCO}3\text{)} \rightarrow \text{magnesium nitrate (Mg(NO}3\text{)}2) + \text{water (H}2\text{O)} + \text{carbon dioxide (CO}2\text{)} $</li><li>Full Equation: $ 2\text{HNO}3(aq) + \text{MgCO}3(s) \rightarrow \text{Mg(NO}3\text{)}2(aq) + \text{H}2\text{O}(l) + \text{CO}2(g) $</li><li>Ionic Equation: $ 2\text{H}^+(aq) + \text{MgCO}3(s) \rightarrow \text{Mg}^{2+}(aq) + \text{H}2\text{O}(l) + \text{CO}_2(g)

Ionic Equations in Reactions

The practice of removing spectator ions in ionic equations is essential for clarity.
Importance of States:
- Always denote states in equations to gain marks in evaluations.

Examples of Acid-Base Reactions

Practice Problem:
- Write balanced full and ionic equations for the reaction between hydrochloric acid and calcium carbonate:
- Full Balanced Equation:
- Ionic Equation:
- Grades are assigned for correctly including states.

Antacids and Their Functionality

Definition:
- Antacids are bases that neutralize stomach acid to relieve discomfort from heartburn, indigestion, or upset stomach.
Reaction Details:
- Antacids react with stomach acid producing salt, water, and sometimes carbon dioxide.

Examples of Antacids:

Types and Active Ingredients:
- Alka-Seltzer: Sodium bicarbonate ($ ext{NaHCO}_3$) in dissolvable tablets.
- Tums: Calcium carbonate ($ ext{CaCO}_3$) in chewable tablets.
- Mylanta: Magnesium hydroxide ($ ext{Mg(OH)}_2$) in chewable tablets or liquid.
- QuickEze: Calcium carbonate in chewable tablets.

Quiz on Active Ingredients in Antacids

Question: Which is not an active ingredient?
- A. Calcium carbonate
- B. Magnesium hydroxide
- C. Hydrochloric acid (correct answer)
- D. Sodium bicarbonate

Terminology:

Monomer (n.): Molecule that reacts with other molecules to form larger molecules (polymers).
Polymer (n.): Molecule produced naturally or synthetically from monomers bonded together.
n: Represents the number of monomers linked in the polymer, indicating molecule length continues.

Addition Polymerisation

The core building blocks of addition polymers are introduced.
- Monomers:
- Must contain a carbon-carbon (C=C) double bond or a carbon-carbon (C≡C) triple bond.
- Example:
  - Monomers: Alkenes or alkynes.
  - Undergo an addition polymerisation reaction.
  - Result: One product formed, named from monomer (e.g., if the monomer is ethene, the polymer is called ‘polyethene’).

Definitions:

Alkene (n.): Hydrocarbon with at least one double carbon-to-carbon bond.
Alkyne (n.): Hydrocarbon with at least one triple carbon-to-carbon bond.
Addition Polymerisation (n.): The chemical reaction between monomers that results in a polymer.

Condensation Polymerisation

Explanation of condensation polymers:
- Building blocks called monomers contain functional groups that can cause condensation.
- Monomers:
- Generally consist of two functional groups, such as hydroxyl/amine and carboxyl groups.
- Result: Two products formed - the condensation polymer and a small molecule (typically water).

Deep Dive on Functional Groups:

Functional Group (n.): Specific group of atoms defining the properties of a compound.
Condensation Polymerisation (n.): Chemical reaction leading to a polymer formation plus water.
- R A H + R B OH → R A B R + H2O

Natural Condensation Polymerisation

Natural polymerisation occurs in organisms, such as:
- Example: Formation of proteins and carbohydrates.

Key Takeaway on Natural Condensation:

Polymer (n.): Molecule produced naturally or synthetically from bonded monomers.
Example:
- Amino acids can condense to form proteins (Amino acid monomer → Polymer + H2O = Protein).

Artificial Condensation Polymerisation

Overview of synthetically produced plastics:
- Not all polymers are classified as plastics; polymers can be both natural or synthetic.
- Plastic (n.): Molecule produced synthetically from bonded monomers.

Example of Artificial Condensation:

Production of polyesters used in fabrics:
- HO - OH + C - C OH + n → a dicarboxylic acid + a polyester + a dialcohol

Multiple Choice Activity

Identify the type of polymerisation reaction and name a functional group in one of the monomers.
Example Reaction:
- O OH + OH → HO C C HO

Properties of Addition Polymers

Non-polar monomers produce non-polar polymers:
- Intermolecular forces: Dispersion forces are the strongest between chains.
- Properties: Relatively flexible.

Deep Dive Examples:

Ethene → Polyethene:
- Weak dispersion force between chains.
Chloroethene → Polychloroethene (PVC):
- Strong dipole-dipole forces between polychloroethene chains.

Properties of Polar Polymers

Polar monomers lead to polar polymers:
- Stronger intermolecular forces such as dipole-dipole attractions or hydrogen bonds.
- More rigid compared to non-polar polymers.

Deep Dive on Polar Example:

Kevlar Chains:
- Hydrogen bonding within polymer chains.

Types of Polyethene

Low Density Polyethene (LDPE):
- Formed under high temperature and pressure; branched structures result in lower density.
- Properties:
- Lower density than HDPE
- Soft, opaque, but transparent in thin forms
- Insulator of electricity
High Density Polyethene (HDPE):
- Produced under low temperature and pressure with less branching.
- Properties:
- Higher density than LDPE
- Hard and allows light to pass through
- Insulator of electricity

Summary of Polyethene Properties:

LDPE:
- Density: ext{density} = rac{ ext{mass}}{ ext{volume}} $</li></ul></li><li>HDPE:<ul><li>Tightly packed polymer structure with minimal branching.</li></ul></li></ul><h4 id="f7e99ab1-56b3-49f9-8896-b1868e4b10f5" data-toc-id="f7e99ab1-56b3-49f9-8896-b1868e4b10f5" collapsed="false" seolevelmigrated="true">Thermoplastic vs. Thermosetting Polymers</h4><ul><li>Thermoplastics:<ul><li>Linear polymers that soften when heated, allowing for reshaping.</li><li>Weak intermolecular forces.</li></ul></li></ul><h6 id="ef5f913b-7ca8-45f6-b905-6c4e38efb321" data-toc-id="ef5f913b-7ca8-45f6-b905-6c4e38efb321" collapsed="false" seolevelmigrated="true">Thermosets:</h6><ul><li>Cross-linked polymers that do not melt on heating due to strong covalent cross-links.</li><li>Example: Bowling ball.</li><li>Elastomers:<ul><li>Contain some cross-links allowing elasticity without complete rigidity.</li></ul></li></ul><h5 id="f5aa55dc-fe1a-41de-9ace-3115c89e72cc" data-toc-id="f5aa55dc-fe1a-41de-9ace-3115c89e72cc" collapsed="false" seolevelmigrated="true">Self-Ionisation of Water</h5><ul><li>Definition: Pure water undergoes a tiny degree of ionisation with itself due to its amphiprotic nature.<ul><li>Chemical Equation: $ \text{H}2\text{O (l)} + \text{H}2\text{O (l)} \rightleftharpoons \text{H}_3\text{O}^+ (aq) + \text{OH}^- (aq) $</li></ul></li><li>Ionization: The conversion of a substance into ions.</li></ul><h5 id="bf33c036-351d-4b95-a728-2afc89f59323" data-toc-id="bf33c036-351d-4b95-a728-2afc89f59323" collapsed="false" seolevelmigrated="true">Ionic Product of Water (K_w)</h5><ul><li>Key Takeaway:<ul><li>At 25°C, the concentrations of hydrogen and hydroxide ions can be expressed as: $ [\text{H}_3\text{O}^+] = [\text{OH}^-] = 1.00 \times 10^{-7}\,\text{M} $</li><li>This leads to the ionic product of water being: $ K_w = 1.00 \times 10^{-14}\,\text{M}^2 $</li></ul></li><li>Concentration Relationships:<ul><li>If$ [\text{H}_3\text{O}^+] $decreases, then$ [\text{OH}^-] $increases (and vice versa).</li><li>Definitions based on acidity:</li><li>Acidic solutions:$ [\text{H}_3\text{O}^+] > 10^{-7}\,\text{M} $and$ [\text{OH}^-] < 10^{-7}\,\text{M} $</li><li>Basic solutions:$ [\text{H}_3\text{O}^+] < 10^{-7}\,\text{M} $and$ [\text{OH}^-] > 10^{-7}\,\text{M} $</li><li>Neutral solutions:$ [\text{H}_3\text{O}^+] = [\text{OH}^-] = 10^{-7}\,\text{M} $</li></ul></li><li>Formula for Ionic Product:<ul><li>$ Kw = [\text{H}3\text{O}^+] \times [\text{OH}^-] = 1.00 \times 10^{-14}\,\text{M}^2 $</li></ul></li><li>Note: The relationship stated is only applicable at 25°C.</li></ul><h5 id="c7557af3-61a2-4647-8cb9-423a377ed51d" data-toc-id="c7557af3-61a2-4647-8cb9-423a377ed51d" collapsed="false" seolevelmigrated="true">Worked Examples</h5><h6 id="a3e4b91d-9136-4aa2-a6df-a118348ac38c" data-toc-id="a3e4b91d-9136-4aa2-a6df-a118348ac38c" collapsed="false" seolevelmigrated="true">Example 1: Concentration of HCl Solution</h6><ul><li>Given: Concentration of HCl = 0.10 M at 25°C.</li><li>Calculation:<ul><li>Since HCl completely ionizes in water, $ [\text{H}_3\text{O}^+] = 0.10\,\text{M} $</li><li>To find$ [\text{OH}^-] $: $ Kw = [\text{H}3\text{O}^+][\text{OH}^-] = 1.00 \times 10^{-14}\,\text{M}^2 $</li><li>Rearranging formula: $ [\text{OH}^-] = \frac{1.00 \times 10^{-14}}{0.10} = 1.0 \times 10^{-13}\,\text{M} $.</li></ul></li></ul><h6 id="3ed8f59f-dba4-4cc2-836c-06231de78ed4" data-toc-id="3ed8f59f-dba4-4cc2-836c-06231de78ed4" collapsed="false" seolevelmigrated="true">Example 2: Multiple Choice</h6><ul><li>Question: Calculate the$ [\text{H}_3\text{O}^+] $at 25°C in a solution with$ [\text{OH}^-] = 0.05\,\text{M} $.</li><li>Calculation:<ul><li>Using$ Kw $:$ \text{H}3\text{O}^+ = \frac{K_w}{[\text{OH}^-]} = \frac{1.00 \times 10^{-14}}{0.05} = 2.0 \times 10^{-13}\,\text{M} $.</li></ul></li></ul><h5 id="ffd99629-34b0-4735-88a4-fc8561351be1" data-toc-id="ffd99629-34b0-4735-88a4-fc8561351be1" collapsed="false" seolevelmigrated="true">pH Measurement</h5><ul><li>Definition of pH: Measurement of acidity, typically on a scale of 0-14.</li><li>Key Formula:<ul><li>$ \text{pH} = -\log{10} [\text{H}3\text{O}^+] $</li><li>This can be rearranged as: $ [\text{H}_3\text{O}^+] = 10^{-\text{pH}} $</li></ul></li></ul><h6 id="38c8e987-47f0-4a81-a36d-3ce85268e8cd" data-toc-id="38c8e987-47f0-4a81-a36d-3ce85268e8cd" collapsed="false" seolevelmigrated="true">Example 3: pH Calculation</h6><ul><li>Calculate the pH of a solution with$ [\text{H}_3\text{O}^+] = 0.20\,\text{M} $.<ul><li>Solution: $ \text{pH} = -\log_{10}(0.20) = 0.692 $.</li></ul></li></ul><h6 id="58f2914f-fdb2-490b-9c24-415d70fecf00" data-toc-id="58f2914f-fdb2-490b-9c24-415d70fecf00" collapsed="false" seolevelmigrated="true">Example 4: Ba(OH) at 25°C</h6><ul><li>Given: Concentration of$ \text{Ba(OH)}_2 = 0.01\,\text{M} $</li><li>Note: Each molecule of$ \text{Ba(OH)}_2 $produces two hydroxide ions, thus:<ul><li>$ [\text{OH}^-] = 2 \times 0.01 = 0.02\,\text{M} $</li><li>Calculate pH:</li><li>Using$ Kw $:$ [\text{H}3\text{O}^+] = \frac{K_w}{[\text{OH}^-]} = \frac{1.00 \times 10^{-14}}{0.02} = 5.00 \times 10^{-13}\,\text{M} $<ul><li>$ \text{pH} = -\log_{10}(5.00 \times 10^{-13}) = 12.3 $.</li></ul></li></ul></li></ul><h6 id="549bee2a-6907-48fa-965e-940fe977772c" data-toc-id="549bee2a-6907-48fa-965e-940fe977772c" collapsed="false" seolevelmigrated="true">Example 5: pH from given pH value</h6><ul><li>Given: pH = 4.0 at 25°C.</li><li>Calculation:<ul><li>$ [\text{H}_3\text{O}^+] = 10^{-4.0} = 0.0001\,\text{M} $</li><li>Then,$ [\text{OH}^-] = \frac{1.00 \times 10^{-14}}{0.0001} = 1.0 \times 10^{-10}\,\text{M} $.</li></ul></li></ul><h5 id="edb3c127-c7c2-4aff-80dc-729159b4041c" data-toc-id="edb3c127-c7c2-4aff-80dc-729159b4041c" collapsed="false" seolevelmigrated="true">Summary of Key Terms</h5><ul><li>Ionisation: The process of converting a substance into ions.</li><li>Ionic Products: The product of the concentrations of ionic species.</li><li>Acidity: The level of acid present in a substance.</li><li>pH Scale: A logarithmic scale that quantifies acidity.</li></ul><h4 id="18b70bd0-3742-40ad-b958-de8a0b1019ed" data-toc-id="18b70bd0-3742-40ad-b958-de8a0b1019ed" collapsed="false" seolevelmigrated="true">Acid-Base (Proton Transfer) Reactions in VCE Chemistry</h4><ul><li>Focus: Interactions of chemicals with water.</li><li>Overview of the lesson structure:<ul><li>Comparison of pH measurements through various methods.</li><li>Joined focus on accuracy and precision in measurement.</li></ul></li></ul><h4 id="7c9236e7-be6d-434a-9abc-c40f2c6ae155" data-toc-id="7c9236e7-be6d-434a-9abc-c40f2c6ae155" collapsed="false" seolevelmigrated="true">Overview of Lesson Content</h4><ul><li>Major components covered in this lesson:<ul><li>Accuracy and Precision in Measurement</li><li>Illustrated with various indicators and pH meters.</li><li>Indicators</li><li>Importance and role in determining pH levels of solutions.</li><li>pH Meters</li><li>How they are used to gauge acidity or basicity.</li></ul></li></ul><h4 id="469821e5-86ba-45d3-ba77-3a92e4509640" data-toc-id="469821e5-86ba-45d3-ba77-3a92e4509640" collapsed="false" seolevelmigrated="true">Understanding Indicators</h4><ul><li>Definition of Indicators: Substances that change colour based on pH levels.</li><li>Why are indicators necessary?<ul><li>Many acids and bases are colourless in a solution, making visual determination of pH impractical.</li></ul></li></ul><h5 id="2713c98a-4000-47e8-a24b-3dae1f06995a" data-toc-id="2713c98a-4000-47e8-a24b-3dae1f06995a" collapsed="false" seolevelmigrated="true">Types of Indicators</h5><ol><li>Natural Indicators<ul><li>Found in nature and exhibit colour changes in the presence of acids or bases.</li><li>Examples:<ul><li>Red cabbage.</li><li>Flower petals from specific types like hydrangea.</li><li>Turmeric.</li></ul></li></ul></li><li>Commercial Indicators<ul><li>Manufactured chemicals or chemical-coated substances that indicate pH changes.</li><li>Examples:<ul><li>Universal indicator.</li><li>Litmus paper.</li><li>Phenolphthalein.</li></ul></li></ul></li></ol><h4 id="ad0c4726-2fad-4930-af68-71dfa48def45" data-toc-id="ad0c4726-2fad-4930-af68-71dfa48def45" collapsed="false" seolevelmigrated="true">The pH Meter</h4><ul><li>Definition: Instrument used to measure the acidity or alkalinity of a solution.</li><li>Functionality:<ul><li>Measures hydrogen ion concentration in a solution.</li></ul></li><li>Key Terms:<ul><li>Acidity: The amount of acid present in a substance.</li><li>Alkalinity: The capacity of a substance to neutralize acids.</li></ul></li></ul><h4 id="c36634a4-24f7-4afb-9714-7aedeecbeac7" data-toc-id="c36634a4-24f7-4afb-9714-7aedeecbeac7" collapsed="false" seolevelmigrated="true">Activities - Multiple Choice Questions</h4><h5 id="99a5eb29-dfdf-4ed9-96fb-476bb910c085" data-toc-id="99a5eb29-dfdf-4ed9-96fb-476bb910c085" collapsed="false" seolevelmigrated="true">Natural vs Commercial Indicators</h5><ul><li>Question: Identify which is not a natural indicator:<ul><li>A. Red cabbage</li><li>B. Turmeric</li><li>C. Litmus paper</li><li>D. Flower petals</li><li>E. I don’t know.</li></ul></li></ul><h5 id="5240cefa-4343-44ff-aa73-4f40449e1bdf" data-toc-id="5240cefa-4343-44ff-aa73-4f40449e1bdf" collapsed="false" seolevelmigrated="true">Accuracy and Precision</h5><ul><li>Definition Clarification:<ul><li>Precision: Ability to yield consistent results through repeated measurement.</li><li>Accuracy: Results are close to the established or true value.</li></ul></li></ul><h4 id="99956fb4-6f4b-424e-a792-08aeb801b512" data-toc-id="99956fb4-6f4b-424e-a792-08aeb801b512" collapsed="false" seolevelmigrated="true">Accuracy and Precision in pH Measurement</h4><ul><li>Observations on pH indicators:<ul><li>Tend to provide less accurate and precise readings than pH meters.</li><li>Limitations of pH indicators:</li><li>Offer only a pH range.</li><li>May vary slightly across trials.</li></ul></li><li>Comparison:<ul><li>pH meters: Higher accuracy and precision, providing reproducible results and including inbuilt calibration functions.</li></ul></li></ul><h4 id="0a87b8ca-dc53-4eca-9236-3752e9d7150a" data-toc-id="0a87b8ca-dc53-4eca-9236-3752e9d7150a" collapsed="false" seolevelmigrated="true">Practical Applications of Measurements</h4><h6 id="e9894f32-29bb-4b92-aacb-00eca76145ef" data-toc-id="e9894f32-29bb-4b92-aacb-00eca76145ef" collapsed="false" seolevelmigrated="true">Example Experiment on Vitamin C</h6><ul><li>Participants tested mass of vitamin C in a multivitamin tablet, claiming 60 mg per tablet.</li><li>Hypothetical results choices to classify according to precision and accuracy:<ul><li>A) 61 mg, 60 mg, 59 mg, 62 mg (high precision, high accuracy)</li><li>B) 55 mg, 60 mg, 62 mg, 59 mg (low precision and accuracy)</li><li>C) 57 mg, 66 mg, 61 mg, 64 mg (mixed)</li><li>D) 55 mg, 56 mg, 55 mg, 54 mg (high precision, low accuracy)</li><li>E) I don’t know.</li></ul></li></ul><h4 id="6d6c7cff-b4af-4315-b863-a6c5764c09c0" data-toc-id="6d6c7cff-b4af-4315-b863-a6c5764c09c0" collapsed="false" seolevelmigrated="true">Summary of Key Terms and Concepts</h4><ul><li>Precision: Ability to reproduce close results.</li><li>Accuracy: Closeness of results to true or accepted values.</li><li>pH Indicators: Natural and commercial indicators that change colour in response to pH levels.</li><li>pH Meter: Accurate and precise tool for measuring acidity/alkalinity by assessing hydrogen ion concentration.</li></ul><h6 id="eef61109-007c-48b4-bed2-b87aff5303b9" data-toc-id="eef61109-007c-48b4-bed2-b87aff5303b9" collapsed="false" seolevelmigrated="true">Acid Rain</h6><ul><li>Definition: Natural rainfall is slightly acidic due to dissolved carbon dioxide from the atmosphere, forming carbonic acid ( $ H2CO3 $).</li><li>Mechanism of Acid Formation:<ul><li>Gases in the atmosphere combine with water vapor.</li><li>Resulting acidic precipitation appears as sulfuric acid and nitric acid.</li></ul></li><li>Forms of Acidic Precipitation:<ul><li>This precipitation can occur as rain, snow, or fog.</li></ul></li></ul>Key Terms:<ul><li>Natural Rainfall (adj.): Water falling through the water cycle, naturally has a slight acidity due to dissolved substances.</li><li>Dissolves (v.): Refers to the process of becoming mixed and included in the liquid.</li><li>Atmosphere (n.): The mass of gas surrounding Earth.</li></ul><h5 id="16467c78-b0b0-4009-bd84-ee9159e4b35f" data-toc-id="16467c78-b0b0-4009-bd84-ee9159e4b35f" collapsed="false" seolevelmigrated="true">Sources of Acid Rain</h5><ul><li>Human Sources:<ul><li>Industrial processes, emissions from factories, power plants, and vehicles.</li></ul></li><li>Natural Sources:<ul><li>Emissions from volcanic eruptions and biological processes occurring in land, wetlands, and oceans that add acid-producing gases to the atmosphere.</li></ul></li></ul>Key Term:<ul><li>Emissions (n.): Things being released or discharged into the atmosphere.</li></ul><h5 id="a62daaae-9cc2-4b0e-ad41-31e914d640aa" data-toc-id="a62daaae-9cc2-4b0e-ad41-31e914d640aa" collapsed="false" seolevelmigrated="true">Ocean Acidity</h5><ul><li>Chemical Reaction:<ul><li>Carbon dioxide readily reacts with water to form carbonic acid: $ CO2(g) + H2O(l)
 ightarrow H2CO3(aq) $</li></ul></li><li>Key Characteristics of Carbonic Acid:<ul><li>Carbonic acid is a diprotic acid that can dissociate in two steps:</li><li>$ H2CO3
 ightleftharpoons H^+(aq) + HCO_3^-(aq) $I</li><li>$ HCO3^-(aq) ightleftharpoons H^+(aq) + CO3^{2-}(aq) $</li><li>Produces:</li><li>Hydronium ions ($ H^+(aq) $)</li><li>Hydrogen carbonate ions ($ HCO_3^-(aq) $)</li><li>Carbonate ions ($ CO_3^{2-}(aq) $)</li></ul></li><li>Carbonate Equations:<ul><li>Calcium carbonate and its dissociation: $ CaCO3(s) ightleftharpoons Ca^{2+}(aq) + CO3^{2-}(aq) $</li></ul></li></ul><h5 id="3056cde2-8bc8-4c65-9edf-42fcf1076f33" data-toc-id="3056cde2-8bc8-4c65-9edf-42fcf1076f33" collapsed="false" seolevelmigrated="true">Effects of Ocean Acidity on Marine Life</h5><ul><li>Impacts on Organisms:<ul><li>Affected Organisms: Marine invertebrates, e.g., plankton and sea snails, utilize calcium and carbonate ions for protective structures made of calcium carbonate.</li><li>Issue: Decreased carbonate ion concentration affects the ability of these organisms to maintain their calcium carbonate structures (shells).</li></ul></li></ul>Key Terms:<ul><li>Marine (adj.): Relating to or found in the ocean.</li><li>Invertebrate (n.): An animal that lacks a backbone.</li></ul><h4 id="32ae5d47-e4b5-46f0-b687-19d167bbf848" data-toc-id="32ae5d47-e4b5-46f0-b687-19d167bbf848" collapsed="false" seolevelmigrated="true">Solubility</h4><h5 id="3d71d3b0-cd01-4c40-acdb-bcefb68cfbb8" data-toc-id="3d71d3b0-cd01-4c40-acdb-bcefb68cfbb8" collapsed="false" seolevelmigrated="true">Definition</h5><ul><li>Solubility: A measure of how much solute will dissolve in a given amount of solvent at a specified temperature.</li></ul><h5 id="fa36e38b-f67d-434c-8b29-a8647fcddf3c" data-toc-id="fa36e38b-f67d-434c-8b29-a8647fcddf3c" collapsed="false" seolevelmigrated="true">Key Terms</h5><ul><li>Saturated Solution:<ul><li>A solution in which no more solute can be dissolved at a particular temperature.</li></ul></li><li>Unsaturated Solution:<ul><li>A solution that contains less solute than needed to make it saturated and can dissolve more solute.</li></ul></li><li>Supersaturated Solution:<ul><li>An unstable solution that contains more dissolved solute than a saturated solution.</li></ul></li></ul><h5 id="89b774fc-ef2a-4c09-969e-cce14b2d5f31" data-toc-id="89b774fc-ef2a-4c09-969e-cce14b2d5f31" collapsed="false" seolevelmigrated="true">Deep Dive</h5><ul><li>Solvent (n.): A substance that dissolves solutes to form solutions.</li><li>Solute (n.): A substance that is dissolved in another substance.</li><li>Illustration of concepts: Solvent → Solution → Solute</li></ul><h4 id="52fa13d6-c1f1-433c-b60a-f3586eee148f" data-toc-id="52fa13d6-c1f1-433c-b60a-f3586eee148f" collapsed="false" seolevelmigrated="true">Concentration</h4><h5 id="b51c7a79-f9f7-43a2-931b-6e09b0262fbf" data-toc-id="b51c7a79-f9f7-43a2-931b-6e09b0262fbf" collapsed="false" seolevelmigrated="true">Definition</h5><ul><li>Concentration (n.): The quantity of substance dissolved in a quantity of solution.</li></ul><h5 id="adeced86-f67b-42b0-a4a6-f5dd372a0cd4" data-toc-id="adeced86-f67b-42b0-a4a6-f5dd372a0cd4" collapsed="false" seolevelmigrated="true">Units of Concentration</h5><h6 id="bc444882-038d-465b-9c9c-61732e2aa0d7" data-toc-id="bc444882-038d-465b-9c9c-61732e2aa0d7" collapsed="false" seolevelmigrated="true">Common Units</h6><ul><li>Mass of solute per litre of solution (g/L)</li><li>Moles of solute per litre of solution (mol/L)</li><li>Parts per million (ppm)</li><li>Percentage by mass (%m/m)</li><li>Percentage by volume (%v/v)</li><li>Percentage mass/volume (%m/v)</li></ul><h5 id="45d2decf-c7ac-4583-a084-e43cebf73efd" data-toc-id="45d2decf-c7ac-4583-a084-e43cebf73efd" collapsed="false" seolevelmigrated="true">Concentration Calculations</h5><h6 id="ac4997da-80c3-4207-81eb-fecc911097bc" data-toc-id="ac4997da-80c3-4207-81eb-fecc911097bc" collapsed="false" seolevelmigrated="true">Example Calculation</h6><ul><li>Concentration (g/L): Indicates the amount of solid solute (in grams) dissolved in solution, e.g., salt in seawater.</li><li>Ppm is used for very small quantities:<ul><li>Equivalents: mg/L, µg/g</li><li>Formula:$ \text{Concentration (g/L)} = \frac{\text{mass of solute (in g)}}{\text{volume of solution (in L)}} $</li></ul></li></ul><h6 id="41b84fda-7661-40f8-aeeb-50e47ba244d0" data-toc-id="41b84fda-7661-40f8-aeeb-50e47ba244d0" collapsed="false" seolevelmigrated="true">Percentage by Mass</h6><ul><li>Describes the mass of solute per 100 g of solution (%m/m).</li><li>Example:<ul><li>Saline solution: 0.9%(w/w) indicates 0.9 g of sodium chloride per 100 g of saline solution.</li><li>Alcohol content: 15%(v/v) means 15.0 mL of alcohol for every 100 mL of wine.</li></ul></li></ul><h4 id="ed2031a9-b8ff-4ffd-97d0-1b6696f659b5" data-toc-id="ed2031a9-b8ff-4ffd-97d0-1b6696f659b5" collapsed="false" seolevelmigrated="true">Molarity</h4><h5 id="b296e91d-4446-49f6-926a-fae515f46e35" data-toc-id="b296e91d-4446-49f6-926a-fae515f46e35" collapsed="false" seolevelmigrated="true">Definition</h5><ul><li>Molarity (n.): Number of moles of solute per litre of solution, denoted as M.</li></ul><h5 id="d851a0c1-7c16-4dda-bdff-0bbce1394a11" data-toc-id="d851a0c1-7c16-4dda-bdff-0bbce1394a11" collapsed="false" seolevelmigrated="true">Calculation Methodology</h5><ul><li>If given the mass of solute:<ul><li>Formula:$ n = \frac{m}{M_r} $</li><li>Concentration formula:$ c = \frac{n}{V} $</li></ul></li><li>Units:<ul><li>Concentration in mol/L, Unit - M</li><li>Number of moles, Unit - mol</li><li>Volume in litres, Unit - L</li></ul></li></ul><h4 id="a1a062f9-ee04-4e03-a473-2222da3e6106" data-toc-id="a1a062f9-ee04-4e03-a473-2222da3e6106" collapsed="false" seolevelmigrated="true">Worked Examples</h4><h5 id="cd74fb6b-1c71-4b3e-a529-4bc7d94e9101" data-toc-id="cd74fb6b-1c71-4b3e-a529-4bc7d94e9101" collapsed="false" seolevelmigrated="true">Example 1: Molar Concentration Calculation</h5><ul><li>Problem: Calculate the concentration, in mol/L, of a solution containing 16.8 mg of AgNO₃ dissolved in 150 mL.</li><li>Steps:<ol><li>Volume conversion:$ V(AgNO_3) = \frac{150}{1000} = 0.150 L $</li><li>Mass conversion:$ m(AgNO_3) = \frac{16.8}{1000} = 0.0168 g $</li><li>Molar mass calculation:</li><li>$ Mr(AgNO3) = 107.9 + 14.0 + (3 \times 16.0) = 169.9 g/mol $</li><li>Calculate moles:$ n(AgNO3) = \frac{m}{Mr} = \frac{0.0168}{169.9} = 9.89 \times 10^{-5} mol $</li><li>Calculate molar concentration:$ C(AgNO_3) = \frac{n}{V} = \frac{9.89 \times 10^{-5}}{0.150} = 6.59 \times 10^{-4} M $</li></ol></li></ul><h5 id="77b23fdc-7a78-4b75-964c-15ac7e0376d8" data-toc-id="77b23fdc-7a78-4b75-964c-15ac7e0376d8" collapsed="false" seolevelmigrated="true">Example 2: Dilution Calculation</h5><h6 id="03005b35-f693-4012-a457-9c77aadd6a2e" data-toc-id="03005b35-f693-4012-a457-9c77aadd6a2e" collapsed="false" seolevelmigrated="true">Definition</h6><ul><li>Dilution (n.): Lowering the concentration of solute in a solution by adding more solvent.</li></ul><h6 id="3bb81bc3-59cc-43a4-8006-36e07c15ffa0" data-toc-id="3bb81bc3-59cc-43a4-8006-36e07c15ffa0" collapsed="false" seolevelmigrated="true">Formula for Dilution</h6><ul><li>$ C1V1 = C2V2 $</li></ul><h6 id="f21802d5-8a05-41a5-a6bd-669575867f53" data-toc-id="f21802d5-8a05-41a5-a6bd-669575867f53" collapsed="false" seolevelmigrated="true">Worked Example for Dilution</h6><ul><li>Problem: Calculate the concentration of the solution formed when 10.0 mL of water is added to 5.0 mL of 1.2 M HCl.</li><li>Steps:<ul><li>Identify C₁ and V₁:</li><li>$ C1 = 1.2M, V1 = 5.0 mL $</li><li>Total volume:$ V_2 = 10.0 + 5.0 = 15.0 mL $</li><li>Find new concentration:</li><li>$ C2 = \frac{C1V1}{V2} = \frac{1.2 \times 5.0}{15.0} = 0.40 M $</li></ul></li></ul><h4 id="9a7bba91-0d65-4c1b-9718-e33fb2e96007" data-toc-id="9a7bba91-0d65-4c1b-9718-e33fb2e96007" collapsed="false" seolevelmigrated="true">Multiple Choice Activities</h4><h6 id="acf16004-c3f4-4973-ba87-f2c7ab9b9b06" data-toc-id="acf16004-c3f4-4973-ba87-f2c7ab9b9b06" collapsed="false" seolevelmigrated="true">Activity Example 1: Concentration of Ammonia</h6><ul><li>Calculate the amount in moles of ammonia (NH₃) in 25.0 mL of a 0.3277 M ammonia solution.</li><li>Choices: A. 81.9 mol B. 13.1 mol C. 0.00131 mol D. 8.19 × 10⁻³ mol E. I don’t know.</li></ul><h6 id="8a6fcc77-de89-463b-aa54-2e8d7d95c826" data-toc-id="8a6fcc77-de89-463b-aa54-2e8d7d95c826" collapsed="false" seolevelmigrated="true">Activity Example 2: ppm Calculation</h6><ul><li>Concentration, in ppm, of a 0.00200 M solution of NaCl, remember ppm = mg/L.</li><li>Choices: A. 0.117 ppm B. 1.17 ppm C. 117 ppm D. 1117 ppm E. I don’t know.</li></ul> <ul><li>Solubility: The amount of solute dissolved in the solvent.</li><li>Concentration: Quantity of solute divided by the quantity of solvent, represented in various units.</li><li>Molarity: Number of moles of solute per litre of solution.</li><li>Dilution: Process of decreasing the concentration of a solution by adding solvent.</li></ul><h4 id="f3067404-4efd-4018-803c-61287428dee5" data-toc-id="f3067404-4efd-4018-803c-61287428dee5" collapsed="false" seolevelmigrated="true">Unsaturated, Saturated, and Supersaturated Solutions</h4><ul><li>Definitions:<ul><li>Unsaturated: A solution containing less solute than can be dissolved at a given temperature (below the curve).</li><li>Saturated: A solution that has the maximum amount of solute dissolved at a given temperature (on the curve).</li><li>Supersaturated: A solution that contains more solute than the solubility limit at a given temperature (above the curve).</li></ul></li></ul><h4 id="ecd0e1d4-ab63-47b7-9ad9-af1dce91f962" data-toc-id="ecd0e1d4-ab63-47b7-9ad9-af1dce91f962" collapsed="false" seolevelmigrated="true">Predicting Saturation Using Solubility Curves</h4><ul><li>Example Activity:<ul><li>At 70°C, determine the mass of KCl in a saturated solution from the solubility curve.</li><li>Options: 40 g, 44 g, 49 g, 54 g, I don't know.</li></ul></li></ul><h4 id="e11c08bc-8063-4317-b77b-77a11359e826" data-toc-id="e11c08bc-8063-4317-b77b-77a11359e826" collapsed="false" seolevelmigrated="true">Solid Precipitation from Solutions</h4><ul><li>Solubility curves can also predict the amount of solute that will precipitate when the solution temperature changes.</li><li>Application:<ul><li>Supersaturation: Predicting the mass of crystals formed in a supersaturated solution as conditions change.</li></ul></li></ul><h4 id="99402f8f-264c-48b2-b8af-65d6edaea0b9" data-toc-id="99402f8f-264c-48b2-b8af-65d6edaea0b9" collapsed="false" seolevelmigrated="true">Solubility of Gases</h4><ul><li>Gases generally become less soluble as temperature increases.<ul><li>This phenomenon is relevant for environmental science as rising water temperatures impact gas levels in aquatic ecosystems.</li><li>Example gases include:</li><li>Methane</li><li>Oxygen</li><li>Carbon Monoxide</li><li>Nitrogen</li><li>Helium</li></ul></li></ul><h4 id="14f3656c-377f-4238-bc2f-0dcf74219f71" data-toc-id="14f3656c-377f-4238-bc2f-0dcf74219f71" collapsed="false" seolevelmigrated="true">Worked Examples</h4><ul><li>Example Problem:<ul><li>Calculate how many grams of potassium nitrate (KNO3) will dissolve in 100 g of water at 40°C.</li><li>Sample Solution: Approximately 60 g of KNO3.</li></ul></li></ul><h4 id="126e5ee5-c871-4353-af8d-7ff851f42392" data-toc-id="126e5ee5-c871-4353-af8d-7ff851f42392" collapsed="false" seolevelmigrated="true">Impact of Temperature on Solubility for KNO3</h4><ul><li>Activity: At 40°C, if 50 g of KNO3 is dissolved and the temperature is reduced to 20°C, determine the mass of KNO3 crystals that will form.<ul><li>Options: 15 g, 20 g, 25 g, 30 g, I don't know.</li></ul></li></ul><h4 id="df531f60-b5ae-4854-8a2e-e31b77b2ca36" data-toc-id="df531f60-b5ae-4854-8a2e-e31b77b2ca36" collapsed="false" seolevelmigrated="true">Eutrophication</h4><ul><li>Definition: Eutrophication is the process by which water bodies become enriched with minerals and nutrients, leading to excessive algae growth.</li><li>Implications for water quality:<ul><li>Increased algae can deplete oxygen levels, harming aquatic life.</li></ul></li></ul><h4 id="cb2a6009-c2b2-4c9a-9d61-73c943794462" data-toc-id="cb2a6009-c2b2-4c9a-9d61-73c943794462" collapsed="false" seolevelmigrated="true">Precipitation for Water Purification</h4><ul><li>Water treatment through precipitation involves using aluminum salts (e.g., alum) to remove nutrients:<ul><li>Alum reacts with water to form aluminum hydroxide:<ul><li>$ ext{Alum} + H2O ightarrow Al(OH)3(aq) $</li></ul></li><li>Phosphate ions react with aluminum hydroxide to form insoluble aluminum phosphate:<ul><li>$ Al(OH)3(aq) + PO4^{3-}(aq)
 ightarrow AlPO_4(s) + 3OH^{-} (aq) $</li></ul></li></ul></li></ul><h4 id="5a7c14b4-e6d9-4e4a-925f-58474a1eaf37" data-toc-id="5a7c14b4-e6d9-4e4a-925f-58474a1eaf37" collapsed="false" seolevelmigrated="true">Mole Recap</h4><ul><li>Definition of Mole:<ul><li>A measurement used in chemistry to facilitate calculations of the number of atoms in a substance.</li><li>Analogous to a standard dozen (12 eggs) or pair (2 socks).</li><li>Avogadro’s Number (Nᴀ):</li><li>Defined as$ 6.02 \times 10^{23} $, representing the number of units in one mole of any substance.</li></ul></li><li>Key Takeaways:<ul><li>Mole (n): The unit of amount of substance in the International System of Units.</li><li>Avogadro’s Number (n): The number of units (particles, molecules, atoms) in one mole of any substance.</li></ul></li><li>Link: Referenced prior knowledge learned about Avogadro’s constant and the mole in Unit 1, Area of Study 2: Quantifying Atoms and Compounds.</li></ul><h4 id="dd3534f2-1127-4c2d-88aa-06dd08d3a9c7" data-toc-id="dd3534f2-1127-4c2d-88aa-06dd08d3a9c7" collapsed="false" seolevelmigrated="true">Mole Formulas</h4><ul><li>Three Key Formulas for Calculation:<ul><li>Mass to Moles:$ n = \frac{m}{M}
 - Where:
 - $n$ = number of moles
 - $m$ = mass in grams
 - $M$ = molar mass in g/mol
- Moles and Particles Relationship: n = \frac{N}{N_A}
 - Where:
 - $N$ = total number of particles
 - $N_A$ = Avogadro’s constant
- Concentration and Volume Relation: c = \frac{n}{V}
 - Where:
 - $c$ = concentration in mol/L
 - $V$ = volume in L.

Multiple Choice Activity

Question: Which formula(s) would you need to use to calculate the concentration of a substance when given the mass (in grams) and volume?
- A. n = n \times N_A $</li><li>B.$ c = \frac{n}{V} $</li><li>C.$ n = \frac{m}{M} $</li><li>D.$ n = \frac{m}{M} $and$ c = \frac{n}{V} $</li><li>E. I don’t know.</li></ul></li></ul><h4 id="e259dd0a-ea35-4304-a11d-e29ff33e8d16" data-toc-id="e259dd0a-ea35-4304-a11d-e29ff33e8d16" collapsed="false" seolevelmigrated="true">Standard Solution</h4><ul><li>Definition:<ul><li>A standard solution is a solution of accurately known concentration, prepared using a known mass of a primary standard.</li></ul></li><li>Importance:<ul><li>Accurate preparation is crucial for ensuring reliable and accurate results and calculations.</li></ul></li></ul><h4 id="a21c84b3-6582-466b-a765-781d585ca243" data-toc-id="a21c84b3-6582-466b-a765-781d585ca243" collapsed="false" seolevelmigrated="true">Preparation of Standard Solution</h4><ul><li>Key Takeaway:<ul><li>Standard Solution (n): A solution with accurately known concentration from a primary standard.</li><li>Primary Standard (n): A reagent that is very pure and accurately reflects the number of moles the substance contains.</li></ul></li></ul><h4 id="aeae6f39-c81f-4f4e-a4fd-771f90b124bd" data-toc-id="aeae6f39-c81f-4f4e-a4fd-771f90b124bd" collapsed="false" seolevelmigrated="true">Primary Standard Criteria</h4><ul><li>Requirements for a Substance to be a Primary Standard:<ul><li>Readily obtainable in pure form.</li><li>Has known chemical formula.</li><li>Easy to store without deteriorating or reacting with the atmosphere.</li><li>High molar mass to minimize errors in weighing.</li><li>Inexpensive.</li></ul></li><li>Examples of Primary Standard Substances:<ul><li>Bases:</li><li>Anhydrous Sodium Carbonate (Na₂CO₃)</li><li>Sodium Borate (Na₂B₄O₇·10H₂O)</li><li>Acids:</li><li>Hydrated Oxalic Acid (H₂C₂O₄·2H₂O)</li><li>Potassium Hydrogen Phthalate (KH(C₈H₄O₄)).</li></ul></li></ul><h4 id="f82e3df2-5922-4594-95fd-bfaa31253233" data-toc-id="f82e3df2-5922-4594-95fd-bfaa31253233" collapsed="false" seolevelmigrated="true">Calculations Involving Acids and Bases</h4><ul><li>Overview:<ul><li>Using stoichiometry, properties of an ‘unknown substance’ can be determined using a ‘known substance.’ In volumetric analysis, the standard solution serves as the known.</li></ul></li><li>Key Takeaway:<ul><li>Stoichiometry (n): A section of chemistry involving relationships between reactants and/or products.</li><li>Volumetric Analysis (n): Methods of quantitative chemical analysis that determine the amount of a substance by measuring the volume it occupies.</li></ul></li></ul><h4 id="fb37796b-8a0b-47b1-a23d-7613f2340e08" data-toc-id="fb37796b-8a0b-47b1-a23d-7613f2340e08" collapsed="false" seolevelmigrated="true">Steps for Calculating Unknown Quantities</h4><ol><li>Write the balanced equation for the reaction.</li><li>Calculate the amount, in moles, of the known substance.</li><li>Use the mole ratios from the balanced equation to calculate the amount of the unknown substance.</li><li>Apply the appropriate formulas to determine the required quantities of the unknown substance (e.g.,$ m = n \times M_r $,$ c = \frac{n}{V}).

VCE Chemistry: Organic Compounds and Functional Groups

Recap - Organic Chemistry

Haloalkanes

Naming Haloalkanes

Worked Example: Naming Haloalkane

Alcohols

Properties of Alcohols

Naming Alcohols

Carboxylic Acids

Properties of Carboxylic Acids

Naming Carboxylic Acids

Overview of Water as a Unique Chemical

Importance of Water

Study Design Dot Points

Risks Associated with Dihydrogen Monoxide (DHMO)

Availability of Drinking Water

Assessing the Drinking Water Sources

Key Definitions and Concepts

Summary of Water Properties

Importance of Water

VCE Chemistry Overview

Lesson Topics

Key Definitions

Water and Group 16 Hydrides

Specific Heat Capacity of Water

Heat Capacity Calculation

Density of Water in Different States

Definitions

Latent Heat

Latent Heat Values for Water

Importance of Latent Heat in Living Systems

Worked Examples

Summary of Key Points

Key Terms Recap

Additional Formulas

Ionic Equations in Reactions

Examples of Acid-Base Reactions

Antacids and Their Functionality

Examples of Antacids:

Quiz on Active Ingredients in Antacids

Terminology:

Addition Polymerisation

Definitions:

Condensation Polymerisation

Deep Dive on Functional Groups:

Natural Condensation Polymerisation

Key Takeaway on Natural Condensation:

Artificial Condensation Polymerisation

Example of Artificial Condensation:

Multiple Choice Activity

Properties of Addition Polymers

Deep Dive Examples:

Properties of Polar Polymers

Deep Dive on Polar Example:

Types of Polyethene

Summary of Polyethene Properties:

Multiple Choice Activity

Volume-Volume Stoichiometry

Earth's Atmosphere

Overview of Earth's Atmosphere

Layers of the Atmosphere

Measuring Gases

Greenhouse Gases

Natural Greenhouse Effect

Enhanced Greenhouse Effect

Greenhouse Gas Emissions

Major Contributing Factors

Multiple Choice Activity

Summary of Key Concepts

Key Terms

Behavior of Gases

Ideal Gases

Observed Properties of Gases (Multiple Choice Activity)

Understanding Pressure in Gases

Worked Example of Pressure Conversion

Universal Gas Law

Standard Laboratory Conditions (SLC)

Worked Example on Calculating Pressure Turns Out In Another Scenario

Summary

Definitions