YOUR NEXT DISCOVERY

Chemical Bonds in Matter: Made Absolutely Simple, Fun and Easy!

Follow electrons. Explain salt, water, metal and diamond.

7 Units38 MissionsAbout 13 hoursCourse map

Complete the Course to Earn a Certificate and Join the Hall of Fame

An inviting chemistry workbench shows a water-shaped model, a pair of joined atoms and an alternating ion crystal. Colours identify model parts; sizes are illustrative.
•••Report a problem (opens in a new tab)
A charge-accounting desk places one large positive token beside two negative tokens, above a blank calculation area. The course will supply exact charges; token size is decorative.

A CLOSER LOOK

Particles, forces and stable arrangements

Explain how tiny particles connect and why materials behave differently.

See it. Try it. Make it yours.

  1. Particles, forces and stable arrangements

  2. Ions, formulas and ionic materials

  3. Build and test electron models

Beginner of any age; no prior chemistry; simple-English support. · What to know before you start

Bring with you: Count small whole numbers. Add, subtract and multiply them. Read a short sentence in English with time to pause. No chemistry knowledge is assumed.

Explain how tiny particles connect and why materials behave differently.

From no chemistry to strong introductory bonding reasoning: construct and audit formulas and electron models; explain stability, shape, polarity and material behaviour; compare competing evidence; and build unfamiliar bond-energy accounts. Every quantitative operation and model limit is taught before it is required. Completion alone does not establish long-term retention or laboratory competence.

By the end, you can…

  • Interpret particles, charge, electron arrangements and energy records before predicting bonding.
  • Build and audit ion formulas, including charged groups, and connect lattice interactions to material properties.
  • Construct unfamiliar Lewis structures and molecular-ion accounts; use formal charge, resonance and exceptions correctly.
  • Infer molecular shape from electron groups and evaluate the combined effect of bond polarity and geometry.
  • Explain metals, networks, layers and molecular solids using their actual particles and movable charge.
  • Compare intermolecular attractions and explain boiling, dissolving, saturation and solution conduction.
  • Build multi-step bond-energy accounts and solve unfamiliar combined structure, state and evidence cases.

For another Course

  • Quantum calculations, orbital wavefunctions and hybridisation derivations.
  • Organic reaction mechanisms and detailed crystal coordination calculations.
  • Full thermodynamic equilibrium and Born-Haber calculations.
  • Laboratory procedures, laboratory certification and advanced spectroscopy.

YOUR LEARNING PATH

One idea leads to the next.

0 of 38 Missions completed or proven
Unit 1

Particles, forces and stable arrangements

Interpret particles, charge, electron arrangements and energy records before predicting bonding.

  1. What is a material made of?Mission 1 of 38Locked. Distinguish an atom, an element, a molecule and a compound.
  2. Read what a particle picture actually saysMission 2 of 38Locked. Classify samples and translate particle pictures into counts without confusing a whole sample with one particle.
  3. Why can tiny parts attract?Mission 3 of 38Locked. Count electric charge and distinguish attraction from repulsion.
  4. The electrons that matter mostMission 4 of 38Locked. Use a simple shell model and recognise its limits.
  5. Why atoms can stay togetherMission 5 of 38Locked. Explain a stable bonding distance and read a qualitative energy-versus-distance record.
  6. Use a table without memorising a tableMission 6 of 38Locked. Use supplied main-group positions and shell counts to predict comparable outer-electron and ion patterns.
Unit 2

Ions, formulas and ionic materials

Build and audit ion formulas, including charged groups, and connect lattice interactions to material properties.

  1. Losing and gaining electronsMission 7 of 38Locked. Calculate simple ion charges without changing the element.
  2. A salt is a whole patternMission 8 of 38Locked. Explain ionic bonding and distinguish a lattice from a molecule.
  3. Make the charge balanceMission 9 of 38Locked. Construct simple neutral ionic formulas from given charges.
  4. Keep a charged group togetherMission 10 of 38Locked. Construct and audit formulas containing polyatomic ions and parentheses.
  5. Compare the pulls in an ionic structureMission 11 of 38Locked. Compare ionic interactions using charge and separation while recognising limits of one-factor predictions.
  6. When can salt carry charge?Mission 12 of 38Locked. Connect ionic structure to conduction, melting and brittleness.
Unit 3

Build and test electron models

Construct unfamiliar Lewis structures and molecular-ion accounts; use formal charge, resonance and exceptions correctly.

  1. One shared pairMission 13 of 38Locked. Explain a covalent bond and count a shared electron pair once.
  2. Build simple electron drawingsMission 14 of 38Locked. Account for all valence electrons in water, methane and ammonia.
  3. Two pairs or three?Mission 15 of 38Locked. Read single, double and triple bonds without confusing atom and electron counts.
  4. Build a Lewis model from an electron budgetMission 16 of 38Locked. Construct and audit a simple neutral Lewis structure from supplied atom connections and valence counts.
  5. Count electrons in a charged moleculeMission 17 of 38Locked. Construct electron budgets and simple Lewis accounts for positively and negatively charged polyatomic ions.
  6. Check the bookkeeping at each atomMission 18 of 38Locked. Calculate formal charges from a Lewis structure and use their sum and distribution to audit a candidate model.
  7. When one Lewis drawing is not enoughMission 19 of 38Locked. Identify valid resonance forms and explain why the actual electron distribution is not a switch between separate molecules.
  8. Know when the octet model is too smallMission 20 of 38Locked. Distinguish an electron-budget error from a stated electron-deficient, odd-electron or expanded-count Lewis example.
Unit 4

Three-dimensional shape and polarity

Infer molecular shape from electron groups and evaluate the combined effect of bond polarity and geometry.

  1. Sharing can be unequalMission 21 of 38Locked. Distinguish a polar bond from full ion charge.
  2. Turn an electron account into a shapeMission 22 of 38Locked. Use a repeatable procedure to distinguish electron-group geometry, atom positions and a flat drawing.
  3. Shape changes the whole resultMission 23 of 38Locked. Use electron regions and molecular shape to compare overall polarity.
  4. Five directions: which positions stay occupied?Mission 24 of 38Locked. Use a five-group model to infer atom shapes, lone-pair positions and symmetry.
  5. Six directions and opposite positionsMission 25 of 38Locked. Use a six-group model to infer shapes and whole-molecule polarity from occupied positions.
Unit 5

Extended structures and material evidence

Explain metals, networks, layers and molecular solids using their actual particles and movable charge.

  1. A metal shares across many atomsMission 26 of 38Locked. Explain conduction and bending in a simple metallic-bonding model.
  2. Same element, different structureMission 27 of 38Locked. Compare molecular and network structures using diamond and graphite.
  3. Choose a structure from several observationsMission 28 of 38Locked. Use controlled material observations to compare ionic, metallic, network and molecular explanations.
Unit 6

Between molecules and inside solutions

Compare intermolecular attractions and explain boiling, dissolving, saturation and solution conduction.

  1. Attractions between moleculesMission 29 of 38Locked. Distinguish bonds inside molecules from attractions between them.
  2. Heat a sample without changing its moleculesMission 30 of 38Locked. Explain evaporation, boiling and pressure effects without confusing thermal motion with bond breaking.
  3. Compare all the attractions, not just one labelMission 31 of 38Locked. Use molecular structure and controlled observations to compare intermolecular attractions and explain several bulk properties.
  4. Why does one substance dissolve?Mission 32 of 38Locked. Use competing attractions to explain selected dissolving cases and honest limits.
  5. Explain what dissolves, what remains and what carries chargeMission 33 of 38Locked. Use particle and energy accounts to explain solution formation, saturation, ion formation and precipitation.
Unit 7

Energy accounts and independent investigation

Build multi-step bond-energy accounts and solve unfamiliar combined structure, state and evidence cases.

  1. Breaking costs; making releasesMission 34 of 38Locked. Use a bond-energy balance to distinguish released from absorbed energy.
  2. Build the energy total yourselfMission 35 of 38Locked. Construct and interpret a bond-energy ledger from balanced molecular records and supplied energy values.
  3. Test a structure claimMission 36 of 38Locked. Use several observations to compare bonding explanations.
  4. Choose the method without being told the topicMission 37 of 38Locked. Solve mixed unfamiliar cases by selecting and linking appropriate charge, electron, shape, material and energy models.
  5. The mystery-material deskMission 38 of 38Locked. Combine charge, formulas, structure, state and energy to judge unfamiliar material explanations.Mastery Challenge

A Debsie Course · Beginner of any age; no prior chemistry; simple-English support.