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[
{
"slide": 1,
"fragments": [
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"fragment_index": -1,
"text_description": "Atoms and Molecules\nFrom the smallest particles emerge the wonders of matter.",
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"slide": 2,
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"text_description": "Early Ideas of Divisibility\nParmanu / Atom\nAround 500 BC, Indian and Greek thinkers proposed that continuous cutting of matter ends with one indivisible particle—Kanad’s “Parmanu” and Democritus’ “Atom”.\nKey Characteristics:\nMaharishi Kanad (India): named the smallest particle “Parmanu”.\nDemocritus (Greece): called the indivisible particle “Atom”.\nIdeas were philosophical; no experiments supported them then.\nExample:\nKeep halving a grain of rice mentally until only an undividable speck remains—this speck is the imagined atom.",
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{
"slide": 3,
"fragments": [
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"fragment_index": -1,
"text_description": "Laws of Chemical Combination\nTwo Fundamental Laws\nLaw of Conservation of Mass states that during a chemical reaction, total mass of reactants equals total mass of products. Law of Constant Proportions says a pure compound always has the same elements in a fixed mass ratio, wherever obtained.\nFormulated by Antoine Lavoisier (1789) and Joseph Proust (1799), these laws laid the groundwork for modern stoichiometry.",
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{
"slide": 4,
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"fragment_index": -1,
"text_description": "Law of Conservation of Mass\nClosed flask set-up showing ignition tube immersion (Fig 3.1)\nClosed-Flask Precipitation Experiment\nA corked conical flask holds sodium sulphate solution; an ignition tube containing barium chloride solution is suspended inside and weighed.\nThe flask is tilted to mix both liquids, forming a white barium sulphate precipitate. Re-weighing shows the same total mass.\nKey Points:\nInitial and final balance readings are identical.\nCork keeps the system closed; no matter escapes.\nMass is conserved in every chemical reaction.",
"image_description": "images/fig3_1_closed_flask.png"
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{
"slide": 5,
"fragments": [
{
"fragment_index": 1,
"text_description": "Law of Constant Proportions",
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"fragment_index": 2,
"text_description": "Fixed Mass Ratio",
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{
"fragment_index": 3,
"text_description": "A pure compound always contains the same elements combined in an unchanging mass ratio, whatever its source or preparation.",
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"fragment_index": 4,
"text_description": "Examples → Water (H₂O): H : O = 1 : 8 • Ammonia (NH₃): N : H = 14 : 3",
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{
"slide": 6,
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"fragment_index": -1,
"text_description": "Dalton’s Atomic Theory\nDalton listed six postulates that explain the laws of conservation of mass and constant proportions.\nPro Tip:\nPostulates 1–2 justify conservation of mass, while 5–6 explain constant proportions in compounds.",
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"fragment_index": 1,
"text_description": "1\nMatter is Atomic\nAll matter is made of extremely small particles called atoms that take part in chemical reactions.",
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{
"fragment_index": 2,
"text_description": "2\nIndivisible & Indestructible\nAtoms cannot be created, divided or destroyed during any chemical change.",
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"fragment_index": 3,
"text_description": "3\nIdentical in an Element\nAtoms of the same element have identical mass and chemical properties.",
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"fragment_index": 4,
"text_description": "4\nDifferent Across Elements\nAtoms of different elements differ in mass and chemical behaviour.",
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"fragment_index": 5,
"text_description": "5\nSimple Ratios Form Compounds\nAtoms combine in simple whole-number ratios to produce compounds.",
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"fragment_index": 6,
"text_description": "6\nFixed Composition\nIn a given compound, the kind and relative number of atoms remain constant.",
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{
"slide": 7,
"fragments": [
{
"fragment_index": -1,
"text_description": "How Big is an Atom?\nRelative sizes from atomic radius to an apple (not to scale)\nThe Nanometre World\nRelative Size Chart:",
"image_description": "images/atom_size_scale_bar.png"
},
{
"fragment_index": 1,
"text_description": "Atomic radius of hydrogen is about 0.1 nm or \\(1 \\times 10^{-10}\\) m.",
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{
"fragment_index": 2,
"text_description": "One nanometre is one-billionth of a metre; stack 10 million atoms to match this page’s thickness.",
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},
{
"fragment_index": 3,
"text_description": "Hydrogen atom ≈ 0.1 nm",
"image_description": ""
},
{
"fragment_index": 4,
"text_description": "Water molecule ≈ 0.3 nm",
"image_description": ""
},
{
"fragment_index": 5,
"text_description": "Grain of sand ≈ 0.1 mm (1 × 10\n5\nnm)",
"image_description": ""
},
{
"fragment_index": 6,
"text_description": "Apple ≈ 10 cm (1 × 10\n8\nnm)",
"image_description": ""
}
]
},
{
"slide": 8,
"fragments": [
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"fragment_index": -1,
"text_description": "Modern Symbols of Elements\nChemical Symbol\nA unique one- or two-letter code approved by IUPAC for every element. The first letter is always capital, the second (if any) lowercase. Several symbols stem from Latin names.\nKey Characteristics:\nOne-letter or two-letter code, e.g., H, O, Cl.\nFirst letter uppercase; second lowercase, e.g., Na, Al.\nLatin-derived when English name repeats, e.g., Fe (ferrum), K (kalium).\nStandardised globally by IUPAC for clear scientific communication.\nExample:\nHydrogen = H, Aluminium = Al, Iron = Fe (from “ferrum”).",
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{
"slide": 9,
"fragments": [
{
"fragment_index": -1,
"text_description": "Atomic Mass Unit (u)\n\\[1\\,\\text{u} \\;=\\; \\frac{1}{12}\\,\\text{mass of one }^{12}\\text{C atom}\\]\nVariable Definitions\nApplications",
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"fragment_index": 1,
"text_description": "u\natomic mass unit",
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},
{
"fragment_index": 2,
"text_description": "\\(^{12}\\)C\ncarbon-12 atom used as reference",
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{
"fragment_index": 3,
"text_description": "Relative Atomic Mass\nAtomic masses are compared to the C-12 scale and expressed in u.",
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{
"fragment_index": 4,
"text_description": "Molar Mass Link\n1 mol of any element has mass (in g) equal to its atomic mass in u.",
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{
"fragment_index": 5,
"text_description": "Universal Standard\nProvides a consistent unit for chemistry and physics calculations.",
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{
"slide": 10,
"fragments": [
{
"fragment_index": -1,
"text_description": "Molecules\nMolecule\nSmallest particle of an element or compound that can exist alone and retains all its chemical properties.\nKey Characteristics:\nExample:\nO₂ illustrates diatomic molecules, while S₈ shows polyatomic nature, helping you distinguish types by atomicity.",
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{
"fragment_index": 1,
"text_description": "Atomicity = number of atoms present in a molecule.",
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{
"fragment_index": 2,
"text_description": "Monoatomic (atomicity 1): single-atom molecules e.g., He, Ar.",
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},
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"fragment_index": 3,
"text_description": "Diatomic (atomicity 2): two-atom molecules e.g., O₂.",
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},
{
"fragment_index": 4,
"text_description": "Polyatomic (atomicity >2): many-atom molecules e.g., S₈.",
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{
"slide": 11,
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"text_description": "Ions and Polyatomic Ions\nIon\nAn ion is an atom or group of atoms carrying a net charge due to electron loss or gain. Positive ions are cations, e.g., Na⁺ and NH₄⁺. Negative ions are anions, such as Cl⁻, or the polyatomic ion SO₄²⁻. Ions act as discrete formula units in ionic compounds.",
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{
"slide": 12,
"fragments": [
{
"fragment_index": -1,
"text_description": "Writing Chemical Formulae\nUse the valency crossover rule to derive correct formulae for binary and polyatomic compounds.",
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{
"fragment_index": 1,
"text_description": "1\nList Symbols\nWrite chemical symbols of the combining elements or polyatomic ions. Metal or cation is written first.",
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{
"fragment_index": 2,
"text_description": "2\nAssign Valencies\nAbove each symbol note its valency / charge—the combining capacity that must be satisfied.",
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"fragment_index": 3,
"text_description": "3\nCross & Drop Sign\nCross over the numerical valencies and write them as subscripts to the other element. Drop the charge sign.",
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"fragment_index": 4,
"text_description": "4\nSimplify\nDivide all subscripts by their highest common factor. Remove ‘1’. The formula is charge-balanced and simplest.",
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{
"fragment_index": 5,
"text_description": "Pro Tip:\nAlways verify total positive charge equals total negative charge; if not, revisit valencies and subscripts.",
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},
{
"slide": 13,
"fragments": [
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"fragment_index": -1,
"text_description": "Build the Formula!\n{% if intro %}\nBalance charges with valency. Drag Mg²⁺, Na⁺, NH₄⁺ onto Cl⁻, SO₄²⁻ and PO₄³⁻ to build \\( \\mathrm{MgCl_2}, \\mathrm{Na_2SO_4}, (\\mathrm{NH_4})_3\\mathrm{PO_4} \\).\n{% endif %}\nDraggable Items\n{% for item in draggable_items %}\n{{ item.label }}\n{% endfor %}\nDrop Zones\n{% for zone in drop_zones %}\n{{ zone.label }}\n{% endfor %}\n{% if tip %}\nTip:\nTotal positive charge must equal total negative charge in the final compound.\n{% endif %}\n{{ check_answers_text or 'Check Answers' }}\nResults\n// Drag and drop functionality\n const draggableItems = document.querySelectorAll('.draggable-item');\n const dropZones = document.querySelectorAll('.drop-zone');\n const checkAnswersBtn = document.getElementById('checkAnswersBtn');\n const feedbackArea = document.getElementById('feedbackArea');\n const feedbackContent = document.getElementById('feedbackContent');\n \n // Drag and drop event listeners\n draggableItems.forEach(item => {\n item.addEventListener('dragstart', handleDragStart);\n item.addEventListener('dragend', handleDragEnd);\n });\n \n dropZones.forEach(zone => {\n zone.addEventListener('dragover', handleDragOver);\n zone.addEventListener('drop', handleDrop);\n zone.addEventListener('dragenter', handleDragEnter);\n zone.addEventListener('dragleave', handleDragLeave);\n });\n \n function handleDragStart(e) {\n e.target.classList.add('opacity-50');\n e.dataTransfer.setData('text/plain', e.target.dataset.id);\n }\n \n function handleDragEnd(e) {\n e.target.classList.remove('opacity-50');\n }\n \n function handleDragOver(e) {\n e.preventDefault();\n }\n \n function handleDragEnter(e) {\n e.preventDefault();\n e.target.closest('.drop-zone').classList.add('border-green-500', 'bg-green-50');\n }\n \n function handleDragLeave(e) {\n e.target.closest('.drop-zone').classList.remove('border-green-500', 'bg-green-50');\n }\n \n function handleDrop(e) {\n e.preventDefault();\n const dropZone = e.target.closest('.drop-zone');\n dropZone.classList.remove('border-green-500', 'bg-green-50');\n \n const itemId = e.dataTransfer.getData('text/plain');\n const draggedItem = document.querySelector(`[data-id=\"${itemId}\"]`);\n \n if (draggedItem && dropZone) {\n dropZone.appendChild(draggedItem);\n dropZone.querySelector('.text-center').style.display = 'none';\n }\n }\n \n // Check answers functionality\n checkAnswersBtn.addEventListener('click', () => {\n // Implementation for checking answers would go here\n feedbackArea.classList.remove('hidden');\n feedbackContent.innerHTML = '<p class=\"text-green-600\">Answers checked! Review your results above.</p>';\n });",
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{
"slide": 14,
"fragments": [
{
"fragment_index": -1,
"text_description": "Molecular & Formula Unit Mass\n\\[ M = \\sum_{i} n_{i} \\times A_{i} \\]\nVariable Definitions\nApplications\nSource: NCERT Science – Atoms & Molecules",
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{
"fragment_index": 1,
"text_description": "\\(M\\)\nMolecular / formula unit mass (u)",
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},
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"fragment_index": 2,
"text_description": "\\(n_{i}\\)\nNumber of atoms/ions of element\ni",
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"text_description": "\\(A_{i}\\)\nRelative atomic mass of element\ni\n(u)",
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"text_description": "Water (H₂O)\n\\(M = 2 \\times 1 + 16 = 18\\,\\text{u}\\)",
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{
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"text_description": "Calcium Chloride (CaCl₂)\n\\(M = 40 + 2 \\times 35.5 = 111\\,\\text{u}\\)",
"image_description": ""
}
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},
{
"slide": 15,
"fragments": [
{
"fragment_index": -1,
"text_description": "Quick Check\nQuestion\nWhich postulate of Dalton’s atomic theory explains the Law of Conservation of Mass?\n1\nAtoms combine in small whole-number ratios.\n2\nAtoms are indivisible and can neither be created nor destroyed.\n3\nAtoms of the same element are identical.\n4\nAtoms of different elements have different masses.\nSubmit Answer\nCorrect!\nDalton stated that atoms are indivisible and indestructible, so total mass remains constant during reactions.\nIncorrect\nReview Dalton’s postulates—the Law of Conservation of Mass follows from the indestructibility of atoms.\nconst correctOption = 1;\n const answerCards = document.querySelectorAll('.answer-card');\n const submitBtn = document.getElementById('slide-15-b7k3qz-submitBtn');\n const feedbackCorrect = document.getElementById('slide-15-b7k3qz-feedbackCorrect');\n const feedbackIncorrect = document.getElementById('slide-15-b7k3qz-feedbackIncorrect');\n \n let selectedOption = null;\n \n answerCards.forEach((card, index) => {\n card.addEventListener('click', () => {\n answerCards.forEach(c => c.classList.remove('border-blue-500', 'bg-blue-50'));\n card.classList.add('border-blue-500', 'bg-blue-50');\n selectedOption = index;\n });\n });\n \n submitBtn.addEventListener('click', () => {\n if (selectedOption === null) return;\n \n if (selectedOption === correctOption) {\n feedbackCorrect.classList.remove('hidden');\n feedbackIncorrect.classList.add('hidden');\n } else {\n feedbackIncorrect.classList.remove('hidden');\n feedbackCorrect.classList.add('hidden');\n }\n });",
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{
"slide": 16,
"fragments": [
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"fragment_index": -1,
"text_description": "Key Takeaways\nAtoms → Molecules → Matter",
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"fragment_index": 1,
"text_description": "Law of Conservation\nTotal mass stays constant in every chemical reaction.",
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"fragment_index": 2,
"text_description": "Law of Definite Proportions\nElements combine in fixed mass ratios to form a compound.",
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"fragment_index": 3,
"text_description": "Atomic Concept\nAn atom is the smallest reactive unit and remains unchanged during reactions.",
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"fragment_index": 4,
"text_description": "Building Matter\nAtoms join as molecules or ions, giving rise to all visible matter.",
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{
"fragment_index": 5,
"text_description": "Formula Writing\nUse valency or ion charge to cross-combine symbols into neutral chemical formulas.",
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