Curriculum

Science Grade 10

Grade 10 Science

0/13

Interactive Worksheets

0/2

Text lesson

Chapter 4: Carbon and its Compounds

Grade 10 Science · Chapter 4

Carbon and Its Compounds

Master covalent bonding, organic chemistry, homologous series, and the reactions of ethanol & ethanoic acid — everything you need for Grade 10 exams.

Covalent Bonds

Organic Chemistry

Soaps & Detergents

Exam Ready

📚 What You Will Learn

① Bonding in Carbon — The Covalent Bond

② Allotropes of Carbon

③ Versatile Nature of Carbon

④ Chains, Branches and Rings

⑤ Functional Groups & Homologous Series

⑥ Chemical Reactions of Carbon Compounds

⑦ Ethanol & Ethanoic Acid (Key Compounds)

⑧ Soaps & Detergents

⑨ 10+ Worked Examples

⑩ Practice Sets A–D with Answers

💧	Section 1: Introduction to Carbon Why is carbon so incredibly special?

Carbon is one of the most remarkable elements on the periodic table. Despite making up only 0.02% of the Earth’s crust (as minerals like carbonates and coal) and only 0.03% of the atmosphere (as carbon dioxide), carbon is the backbone of all life on Earth. Every living organism — including you — is built from carbon-based compounds.

Chemists have identified millions of carbon compounds, outnumbering the compounds of all other elements combined. This extraordinary variety comes from two unique abilities of carbon: tetravalency (four bonding arms) and catenation (the ability to bond to other carbon atoms to form long chains).

💡 Key Fact

Carbon has atomic number 6. Its electron configuration is 2, 4 — meaning it has 4 valence electrons. Carbon always forms exactly 4 bonds, whether single, double, or triple bonds.

⚛	Section 2: The Covalent Bond Sharing electrons to achieve noble gas configuration

Why Doesn’t Carbon Form Ions?

Carbon needs 4 more electrons to complete its outer shell. It cannot do this by gaining or losing electrons because:

❌ Gaining 4 electrons → C⁴⁻

A nucleus with only 6 protons cannot hold 10 electrons — the repulsion would be too great.

❌ Losing 4 electrons → C⁴⁺

Removing 4 electrons requires an enormous amount of energy — not feasible under normal conditions.

✅ The Solution: Electron Sharing (Covalent Bond)

Carbon shares its 4 valence electrons with other atoms. Each shared pair of electrons counts toward the outer shell of both atoms. This is called a covalent bond.

📚 Definition

Covalent Bond

A covalent bond is formed when two atoms share one or more pairs of electrons, allowing each atom to achieve a completely filled outer shell (noble gas configuration). Covalent compounds have strong bonds within molecules but weak forces between molecules, giving them low melting and boiling points.

📊 Types of Covalent Bonds — Visual Diagram

Single Bond

H−H (1 shared pair)

e.g. H₂, CH₄

Double Bond

O=O (2 shared pairs)

e.g. O₂, C₂H₄

Triple Bond

N≡N (3 shared pairs)

e.g. N₂, C₂H₂

⚙ Methane (CH₄) — Electron Dot Diagram

	H
H	C	H
	H

Methane (CH₄) — Tetrahedral

Formula: CH₄

Type of bonds: 4 single covalent bonds

Bond angle: 109.5° (tetrahedral)

Carbon’s valence electrons: 4 (shared with 4 hydrogen atoms)

Common uses: CNG (Compressed Natural Gas), biogas, cooking fuel

💎	Section 3: Allotropes of Carbon Same element, dramatically different structures and properties

ALLOTROPE	STRUCTURE	BONDS PER C	KEY PROPERTY	USES
Diamond 💎	Rigid 3D tetrahedral network	4 single bonds	Hardest natural substance	Jewellery, cutting tools, drills
Graphite ✍	Layered hexagonal sheets	3 bonds + 1 free e⁻	Conducts electricity	Pencils, electrodes, lubricant
Fullerene (C₅₀) ⚽	Football-shaped spherical cage	3 bonds	Hollow nanocage	Drug delivery, nanotechnology

Allotrope Structure Diagrams (HTML Table Representations)

Diamond Structure



	C

Each C bonds to 4 others
Forms rigid 3D lattice

Graphite Structure

Hexagonal layers
Layers slide = lubricant

C₅₀ Fullerene

60 C atoms in sphere
Like a football (geodesic)

☘	Section 4: The Versatile Nature of Carbon Tetravalency, Catenation, Chains, Branches & Rings

⚡ Property 1

Tetravalency

Carbon has 4 valence electrons, giving it a valency of 4. This means every carbon atom can form exactly 4 bonds — with hydrogen, oxygen, nitrogen, chlorine, sulphur, or other carbon atoms. This allows for an enormous variety of compound structures.

🔗 Property 2

Catenation

Carbon can bond to other carbon atoms to form long chains, branched chains, and ring structures. No other element does this to the same extent. Chains can range from 2 to thousands of carbon atoms, and may contain single, double, or triple bonds.

📑 Types of Carbon Chain Structures

Straight Chain

C — C — C — C
Butane: C₄H₁₀

All carbons in a single line. Example: n-butane, ethane, propane

Branched Chain

C — C — C
      |
      C
Isobutane: C₄H₁₀

Branch off main chain. Same formula, different structure = structural isomers

Ring Structure

Cyclohexane C₆H₁₂

Carbon atoms join in a closed ring. e.g. cyclohexane, benzene

📚 Definition

Structural Isomers

Compounds that have the same molecular formula but different structural arrangements of atoms are called structural isomers. For example, both n-butane and isobutane have the formula C₄H₁₀ but different structures, giving them slightly different physical properties.

⚒	Section 5: Functional Groups & Homologous Series How chemical groups determine compound behaviour

What is a Functional Group?

A functional group is an atom or group of atoms attached to a carbon chain that determines the chemical properties of the compound. The functional group remains constant in a homologous series, regardless of the chain length.

CLASS	FUNCTIONAL GROUP	PREFIX / SUFFIX	EXAMPLE
Alcohol	—OH	Suffix: -ol	Ethanol (C₂H₅OH)
Aldehyde	—CHO	Suffix: -al	Ethanal (CH₃CHO)
Ketone	—CO—	Suffix: -one	Propanone (CH₃COCH₃)
Carboxylic Acid	—COOH	Suffix: -oic acid	Ethanoic acid (CH₃COOH)
Haloalkane	—X (Cl, Br, I)	Prefix: chloro-/bromo-	Chloromethane (CH₃Cl)
Alkene	C=C	Suffix: -ene	Ethene (C₂H₄)

Homologous Series — Alkanes

A homologous series is a family of carbon compounds where each successive member differs by a —CH₂— unit (mass difference of 14 u). They share the same functional group and similar chemical properties, but physical properties (like boiling point) gradually change.

NAME	FORMULA	NO. OF C	BOILING POINT (K)	COMMON USE
Methane	CH₄	1	111	CNG, biogas
Ethane	C₂H₆	2	184	Fuel
Propane	C₃H₈	3	231	LPG cylinder
Butane	C₄H₁₀	4	273	Lighter gas
Pentane	C₅H₁₂	5	309	Solvent

Notice: Boiling point increases as the number of carbon atoms increases. General formula for alkanes: C_nH_2n+2

🔥	Section 6: Chemical Reactions of Carbon Compounds Combustion, Oxidation, Addition & Substitution

🔥 1. Combustion

Carbon compounds burn in air to produce CO₂ and H₂O. Saturated compounds burn with a clean blue flame; unsaturated ones produce a sooty yellow flame.

CH₄ + 2O₂ → CO₂ + 2H₂O + Energy

🔄 3. Addition Reaction

Unsaturated hydrocarbons (alkenes, alkynes) add H₂ in the presence of Ni or Pd catalyst to become saturated. Used in vegetable oil hydrogenation.

CH₂=CH₂ + H₂ → CH₃—CH₃
(Nickel catalyst, heat)

⚖ 2. Oxidation

Alcohols can be oxidised to carboxylic acids using oxidising agents like alkaline KMnO₄ (potassium permanganate) or acidified K₂Cr₂O₇ (potassium dichromate).

CH₃CH₂OH → CH₃COOH
(Ethanol → Ethanoic acid)

⚡ 4. Substitution Reaction

Saturated hydrocarbons react with Cl₂ in sunlight. One hydrogen is replaced by one chlorine atom at a time.

CH₄ + Cl₂ → CH₃Cl + HCl
(In presence of sunlight)

💉	Section 7: Ethanol & Ethanoic Acid Two commercially vital carbon compounds

🍶 Ethanol (C₂H₅OH)

Also called: Ethyl alcohol

Physical Properties:

• Liquid at room temperature

• Melting point: 156 K | Boiling point: 351 K

• Completely miscible with water

Chemical Properties:

• Reacts with Na to release H₂ gas

• Dehydration with conc. H₂SO₄ at 443 K produces ethene

• Oxidised to ethanoic acid

🔌 Uses:

Alcoholic drinks (dilute), tincture iodine, cough syrups, fuel (ethanol blend), antiseptic

⚠ Warning:

Pure (absolute) ethanol or methanol ingestion is toxic and can cause death. Methanol can cause permanent blindness.

🍭 Ethanoic Acid (CH₃COOH)

Also called: Acetic acid

Physical Properties:

• Melting point: 290 K (freezes in winter!)

• Boiling point: 391 K

• Pure form called glacial acetic acid

Chemical Properties:

• Weak acid (partial ionisation unlike HCl)

• Reacts with base (NaOH) → sodium ethanoate + water

• Reacts with carbonates → CO₂ gas evolved

• Reacts with ethanol + acid catalyst → ester (fruity smell)

🔌 Uses:

Vinegar (5–8% solution), food preservative in pickles, solvent, making synthetic fibres

🧪 Esterification Reaction — Diagram

Ethanoic Acid

CH₃COOH

Ethanol

C₂H₅OH

→

conc. H₂SO₄

Ester (sweet smell)

CH₃COOC₂H₅

Water

H₂O

Saponification (reverse reaction): Treating ester with NaOH solution regenerates alcohol + sodium salt of the acid. This is how soap is made.

🧼	Section 8: Soaps & Detergents The chemistry of cleansing — hydrophilic & hydrophobic ends

Soaps are sodium or potassium salts of long-chain carboxylic acids. They are made by the saponification of fats and oils with NaOH. Detergents are similar but contain sulphonate or sulphate groups and work even in hard water.

Soap Molecule Structure — How It Works

Soap Molecule

🗓 HYDROPHILIC HEAD

—COO⁻ Na⁺

Loves water · Ionic end

🌿 HYDROPHOBIC TAIL

CH₃(CH₂)ⁿ—

Hates water · Loves oil/grease

How Soap Removes Grease — 3 Steps:

Step 1: Hydrophobic tails of soap molecules embed into the grease/oil droplet, surrounding it.

Step 2: Hydrophilic heads face outward toward the water, forming a ball called a micelle.

Step 3: The micelle (grease trapped inside) is carried away when rinsed with water. Grease is emulsified.

Micelle Formation


GREASE

● Blue = hydrophilic head ─ Orange = hydrophobic tail

Soap vs Detergent — Key Differences

PROPERTY	SOAP	DETERGENT
Chemical nature	Sodium/potassium salt of fatty acid	Sulphonates or sulphates
Works in hard water?	❌ No — forms scum	✅ Yes — effective
Biodegradable?	✅ Yes	❌ Some are non-biodegradable
Source	Natural fats/oils + NaOH	Petroleum / synthetic chemicals

📝	Worked Examples 10 step-by-step solved problems

🆕 Example 1 — Covalent Bonds

Question: Explain why carbon forms covalent bonds instead of ionic bonds.

▼ Show Step-by-Step Solution

Step 1: Identify carbon’s atomic number = 6. Electron configuration = 2, 4. Valence electrons = 4.

Step 2: To form C⁴⁻ (gain 4e⁻): Nucleus has only 6 protons but must hold 10 electrons. The repulsion would be too large — energetically unfavourable.

Step 3: To form C⁴⁺ (lose 4e⁻): Requires an enormous ionisation energy to remove 4 electrons, leaving only 2 electrons for 6 protons — also unfavourable.

Conclusion: Carbon resolves this by sharing its 4 valence electrons with other atoms — forming 4 covalent bonds. This gives carbon (and its bonding partners) a complete outer shell without gaining or losing electrons.

🆕 Example 2 — Naming Carbon Compounds

Question: Name the compound with formula CH₃—CH₂—CH₂—OH

▼ Show Step-by-Step Solution

Step 1: Count carbon atoms in the longest chain = 3 carbons → base name = propan

Step 2: Identify functional group → —OH group = alcohol → suffix is -ol

Step 3: Since suffix starts with a vowel (-ol), drop the ‘e’ from propane → propan

Answer: Propan-1-ol (or Propanol)

🆕 Example 3 — Homologous Series

Question: Is CH₃OH, C₂H₅OH, C₃H₇OH a homologous series? Justify.

▼ Show Solution

Check 1: Same functional group? Yes — all contain —OH (alcohol group). ✅

Check 2: Consecutive members differ by —CH₂—?

CH₃OH → C₂H₅OH: difference = CH₂ (14 u) ✅

C₂H₅OH → C₃H₇OH: difference = CH₂ (14 u) ✅

Conclusion: YES — this is a homologous series called alcohols (alkanols). Similar chemical properties, but boiling point increases with each member.

🆕 Example 4 — Combustion Reaction

Question: Write the balanced equation for complete combustion of propane (C₃H₈).

▼ Show Solution

Step 1: Write unbalanced equation: C₃H₈ + O₂ → CO₂ + H₂O

Step 2: Balance carbon: 3 C on left → 3CO₂ on right

Step 3: Balance hydrogen: 8 H on left → 4H₂O on right

Step 4: Balance oxygen: 3CO₂ = 6 O; 4H₂O = 4 O; total = 10 O atoms → 5O₂

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O + Heat

🆕 Example 5 — Isomers

Question: Draw two structural isomers of butane (C₄H₁₀) and explain how they differ.

▼ Show Solution

Isomer 1: n-Butane

C — C — C — C

Straight chain · BP = 273 K

Isomer 2: Isobutane

C — C — C
|
C

Branched chain · BP = 261 K

Difference: Both have formula C₄H₁₀ but different structures. n-Butane has a lower boiling point than isobutane due to different surface areas and intermolecular forces. Same molecular formula, different physical properties = structural isomers.

🆕 Example 6 — Oxidation

Question: What happens when ethanol is treated with alkaline KMnO₄?

▼ Show Solution

Observation: The purple/violet colour of KMnO₄ disappears (decolorisation indicates oxidation).

Reaction type: Oxidation (oxygen is added to ethanol)

CH₃CH₂OH + [O] → CH₃COOH

Ethanol → Ethanoic acid (via oxidising agent)

KMnO₄ role: It is the oxidising agent — it provides the oxygen needed to convert the alcohol to an acid.

🆕 Example 7 — Esterification

Question: Describe the esterification reaction and write its equation.

▼ Show Solution

Definition: Esterification is the reaction between an acid and an alcohol in the presence of a catalyst (conc. H₂SO₄) to form an ester and water.

CH₃COOH + C₂H₅OH → CH₃COOC₂H₅ + H₂O

(Ethanoic acid + Ethanol → Ethyl ethanoate + Water)

Reverse: The ester can be converted back by treating with NaOH — called saponification (used in soap-making).

🆕 Example 8 — Addition Reaction

Question: What is hydrogenation and why is it used in the food industry?

▼ Show Solution

Hydrogenation: Addition of H₂ to an unsaturated hydrocarbon (alkene or alkyne) in the presence of Ni or Pd catalyst to produce a saturated compound.

Vegetable oil (unsaturated) + H₂ → Vegetable fat (saturated)

[Ni catalyst, heat]

Food industry use: Vegetable oils are converted into solid fats (like margarine/vanaspati) for longer shelf life and suitable texture. However, unsaturated fats are healthier — choose oils over saturated fats when possible.

🆕 Example 9 — Soaps & Hard Water

Question: Why do soaps not work well in hard water? How do detergents solve this?

▼ Show Solution

Hard water contains dissolved calcium (Ca²⁺) and magnesium (Mg²⁺) ions.

Problem: Soap reacts with these ions to form insoluble calcium or magnesium stearate — a white precipitate called “scum”. This wastes soap and leaves residue on clothes and skin.

2C₁₇H₃₅COONa + Ca²⁺ → (C₁₇H₃₅COO)₂Ca ↓ + 2Na⁺
(Soap) + (Hard water ion) → Scum precipitate

Detergent solution: Detergents contain sulphonate or sulphate groups whose calcium/magnesium salts remain soluble in water, so no scum forms. They work effectively in both hard and soft water.

🆕 Example 10 — Allotropes

Question: Diamond and graphite are both made of carbon. Why are their properties so different?

▼ Show Solution

PROPERTY	DIAMOND	GRAPHITE
Structure	3D tetrahedral network	2D hexagonal layers
Bonds per C atom	4 single bonds	3 bonds + 1 delocalized e⁻
Hardness	Hardest natural substance	Soft and slippery (layers slide)
Electricity	Does not conduct	Conducts (free e⁻ in layers)

Conclusion: It is the difference in bonding arrangement — not the element itself — that creates such dramatically different properties. This illustrates how structure determines function in chemistry.

📋	Practice Sets A–D Test your knowledge — answers included

📄 Practice Set A — Multiple Choice (Conceptual)

A1. The atomic number of carbon is:

(a) 4 (b) 6 (c) 12 (d) 2

A2. Which of these is a property of covalent compounds?

(a) High melting point (b) Conduct electricity freely (c) Low boiling point (d) Form ions in solution

A3. The general formula for alkanes is:

(a) C_nH_2n (b) C_nH_2n+2 (c) C_nH_2n-2 (d) C_nH_n

A4. The functional group —COOH represents:

(a) Alcohol (b) Ketone (c) Carboxylic acid (d) Aldehyde

A5. Vinegar is a solution of:

(a) 5–8% ethanol in water (b) 5–8% ethanoic acid in water (c) Pure acetic acid (d) Lactic acid

▼ View Answers

A1: (b) 6 | A2: (c) | A3: (b) C_nH_2n+2 | A4: (c) Carboxylic acid | A5: (b)

📄 Practice Set B — Short Answer Questions

B1. Differentiate between saturated and unsaturated hydrocarbons with one example each.

B2. What is catenation? Why is it uniquely exhibited by carbon?

B3. What is the IUPAC name for CH₃COCH₃?

B4. State two differences between soap and detergent.

B5. What happens when ethanoic acid reacts with Na₂CO₃?

▼ View Answers

B1: Saturated hydrocarbons contain only C–C single bonds (e.g. ethane C₂H₆). Unsaturated hydrocarbons contain at least one double or triple bond (e.g. ethene C₂H₄).

B2: Catenation is the ability of carbon to bond with other carbon atoms forming long chains. It is unique to carbon because the C–C bond is strong and stable, and carbon’s small size allows for effective orbital overlap.

B3: Propanone (also called acetone)

B4: (i) Soap forms scum in hard water; detergents do not. (ii) Soap is biodegradable; many detergents are not.

B5: Ethanoic acid reacts with sodium carbonate to produce sodium ethanoate, water, and CO₂ gas (effervescence). Equation: 2CH₃COOH + Na₂CO₃ → 2CH₃COONa + H₂O + CO₂↑

📄 Practice Set C — Long Answer Questions

C1. Explain the cleansing action of soap with the help of a diagram. Why does soap not work in hard water?

C2. Draw the electron dot structure for: (a) NH₃ (b) H₂O (c) N₂

C3. Compare the physical and chemical properties of ethanol and ethanoic acid in a table format.

C4. Name the following compounds: (a) C₂H₅Cl (b) CH₂=CH₂ (c) CH₃CHO (d) CH₃CH₂CH₂OH

▼ View Answers

C1: See Section 8 — Soap molecules surround grease droplets with hydrophobic tails embedded in grease and hydrophilic heads in water, forming micelles. In hard water, Ca²⁺/Mg²⁺ react with soap to form insoluble scum, preventing micelle formation.

C2: (a) NH₃ — N with 3 bonding pairs + 1 lone pair; (b) H₂O — O with 2 bonding pairs + 2 lone pairs; (c) N₂ — N triple bond with 1 lone pair each

C3: Ethanol — liquid, BP 351 K, neutral, reacts with Na to give H₂; Ethanoic acid — liquid, BP 391 K, acidic (pH ~3), reacts with Na₂CO₃ to give CO₂

C4: (a) Chloroethane (b) Ethene (c) Ethanal (d) Propan-1-ol

📄 Practice Set D — Equations & Reactions

D1. Write the balanced equation for combustion of ethanol.

D2. Write the equation for the substitution reaction of methane with chlorine.

D3. What products form when ethanoic acid reacts with NaOH? Write the equation.

D4. Write the addition reaction of ethene with H₂ in presence of Ni.

D5. Write the equation for saponification of an ester.

▼ View Answers

D1: C₂H₅OH + 3O₂ → 2CO₂ + 3H₂O + Energy

D2: CH₄ + Cl₂ → CH₃Cl + HCl (sunlight)

D3: CH₃COOH + NaOH → CH₃COONa + H₂O

D4: CH₂=CH₂ + H₂ → CH₃—CH₃ (Ni catalyst, heat)

D5: CH₃COOC₂H₅ + NaOH → C₂H₅OH + CH₃COONa

📚 Chapter Summary

Carbon & Its Compounds — Key Points

⚛ Covalent Bonds

Carbon forms covalent bonds by sharing electrons. Strong bonds within molecules but weak forces between them = low melting/boiling points, poor conductors.

🔗 Catenation & Tetravalency

Carbon’s 4 valence electrons (tetravalency) and ability to bond with other carbons (catenation) produce millions of compounds — more than all other elements combined.

♨ Homologous Series

Compounds with the same functional group that differ by —CH₂— form a homologous series. Same chemical properties, gradual change in physical properties.

🔥 Reactions

Carbon compounds undergo combustion, oxidation, addition, and substitution reactions. Saturated compounds are less reactive; unsaturated are more reactive.

🍶 Key Compounds

Ethanol (C₂H₅OH) — alcohol, solvent, fuel. Ethanoic acid (CH₃COOH) — acetic acid/vinegar, weak acid, food preservative. Esters — sweet-smelling, made by esterification.

🧼 Soaps & Detergents

Soaps = Na/K salts of fatty acids. Cleanse by micelle formation. Fail in hard water. Detergents work in hard and soft water but some are non-biodegradable.

🏅 Exam Quick-Check — 8 Must-Know Points

1 Carbon forms 4 covalent bonds due to 4 valence electrons (tetravalency)

2 Diamond = hardest (4 bonds, 3D) | Graphite = conductor (3 bonds + free e⁻)

3 Homologous series members differ by —CH₂— (14 u)

4 Alkanes: C_nH_2n+2 | Alkenes: C_nH_2n | Alkynes: C_nH_2n-2

5 Ethanol = BP 351 K | Ethanoic acid = BP 391 K, MP 290 K (glacial)

6 Esterification: Acid + Alcohol → Ester + Water (conc. H₂SO₄ catalyst)

7 Soaps form scum in hard water; detergents work in both hard and soft water

8 KMnO₄/K₂Cr₂O₇ are oxidising agents — convert alcohols to carboxylic acids

This comprehensive Grade 10 Science study guide covers Chapter 4 on Carbon and Its Compounds, including covalent bonding, allotropes of carbon (diamond, graphite, and fullerene), the versatile nature of carbon through tetravalency and catenation, organic chemistry fundamentals including functional groups, homologous series nomenclature (alkanes, alkenes, alkynes, alcohols, aldehydes, ketones, and carboxylic acids), chemical reactions of carbon compounds such as combustion, oxidation, addition, and substitution reactions, and detailed study of ethanol and ethanoic acid. The page also explains the chemistry of soaps and detergents, including micelle formation and cleansing action. Aligned to Grade 10 Science curriculum with 10 worked examples and four practice sets with answers to help students prepare for board examinations.

Curriculum

Science Grade 10

Grade 10 Science

Interactive Worksheets

Chapter 4: Carbon and its Compounds

Carbon and Its Compounds

📚 What You Will Learn

Section 1: Introduction to Carbon

Section 2: The Covalent Bond

Why Doesn’t Carbon Form Ions?

📊 Types of Covalent Bonds — Visual Diagram

⚙ Methane (CH₄) — Electron Dot Diagram

Section 3: Allotropes of Carbon

Allotrope Structure Diagrams (HTML Table Representations)

Section 4: The Versatile Nature of Carbon

📑 Types of Carbon Chain Structures

Section 5: Functional Groups & Homologous Series

What is a Functional Group?

Homologous Series — Alkanes

Section 6: Chemical Reactions of Carbon Compounds

Section 7: Ethanol & Ethanoic Acid

🧪 Esterification Reaction — Diagram

Section 8: Soaps & Detergents

Soap Molecule Structure — How It Works

Soap vs Detergent — Key Differences

Worked Examples

Practice Sets A–D

Carbon & Its Compounds — Key Points