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[
{
"slide": 1,
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"text_description": "Meet Covalent Bonds\nTwo hydrogen atoms share one electron pair to form H₂.\nAtoms share electrons to stay stable\nA covalent bond forms when two atoms share one or more pairs of electrons.\nExample: In hydrogen gas (H₂) each H atom shares its single electron, so both feel a full first shell.\nKey Points:\nCovalent bond = shared electron pair.\nHydrogen + Hydrogen → H₂ by sharing one pair.\nSharing keeps both atoms electrically neutral.",
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"slide": 2,
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"text_description": "Carbon’s Four Hands\nModel of methane \\(CH_4\\)\nCarbon Valency = 4\nCarbon has four valence electrons, giving it a valency of 4.\nBy sharing each electron with a hydrogen atom, carbon forms methane, \\(CH_4\\).\nKey Points:",
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"text_description": "Carbon’s valency is 4.",
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"text_description": "Methane \\(CH_4\\) proves this: carbon bonds with 4 hydrogens.",
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{
"slide": 3,
"fragments": [
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"fragment_index": -1,
"text_description": "Single, Double, Triple\nBond multiplicity counts shared pairs. Goal: spot the difference between single, double and triple covalent bonds.\nPro Tip:\nMore shared pairs = stronger and shorter bond.",
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{
"fragment_index": 1,
"text_description": "1\nSingle Bond\nAtoms share one electron pair. Longest and weakest covalent bond.",
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{
"fragment_index": 2,
"text_description": "2\nDouble Bond\nAtoms share two pairs. Stronger and shorter than a single bond.",
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{
"fragment_index": 3,
"text_description": "3\nTriple Bond\nAtoms share three pairs. Shortest and strongest covalent bond.",
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]
},
{
"slide": 4,
"fragments": [
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"fragment_index": -1,
"text_description": "Diamond – A Hard Giant\nTetrahedral network of carbon atoms\nDiamond is an allotrope of carbon built from a continuous tetrahedral network.\nEach carbon atom shares electrons with four others, forming strong covalent bonds in 3-D.\nKey Points:",
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"text_description": "Pure carbon allotrope made only of C–C bonds.",
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{
"fragment_index": 2,
"text_description": "4 bonds per atom give a rigid tetrahedral lattice.",
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{
"fragment_index": 3,
"text_description": "Endless 3-D lattice makes diamond the hardest natural material.",
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}
]
},
{
"slide": 5,
"fragments": [
{
"fragment_index": -1,
"text_description": "Graphite – Layers that Slide\nLayered Structure & Properties",
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{
"fragment_index": 1,
"text_description": "Graphite is an allotrope of carbon built from flat, hexagonal sheets stacked one above another.",
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{
"fragment_index": 2,
"text_description": "Weak forces between the layered sheets let them slide easily, so graphite feels soft and writes smoothly.",
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{
"fragment_index": 3,
"text_description": "Each carbon contributes one delocalised electron that moves within a sheet, giving the material good electrical conductivity.",
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{
"fragment_index": 4,
"text_description": "Key Points:\nAllotrope: Graphite has layered sheets of carbon atoms.\nLayer sliding → softness; free electrons within a sheet → conductivity.",
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}
]
},
{
"slide": 6,
"fragments": [
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"fragment_index": -1,
"text_description": "Diamond vs Graphite\nDiamond\nGraphite\nKey Similarities",
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{
"fragment_index": 1,
"text_description": "Hardest natural substance; resists scratching.",
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},
{
"fragment_index": 2,
"text_description": "Electrical insulator; no free electrons.",
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},
{
"fragment_index": 3,
"text_description": "Transparent, brilliant crystal lattice.",
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},
{
"fragment_index": 4,
"text_description": "Soft, layers slide easily; marks paper.",
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},
{
"fragment_index": 5,
"text_description": "Good electrical conductor; delocalised electrons.",
"image_description": ""
},
{
"fragment_index": 6,
"text_description": "Black and shiny, layered structure.",
"image_description": ""
},
{
"fragment_index": 7,
"text_description": "Both are pure carbon allotropes.",
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},
{
"fragment_index": 8,
"text_description": "Strong covalent bonds give high melting points.",
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}
]
},
{
"slide": 7,
"fragments": [
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"text_description": "Saturated Chains\nBall-and-stick model of ethane\nEthane: a Saturated Hydrocarbon\nEthane (C₂H₆) shows what “saturated” means.\nIts two carbons share one single C–C bond; each carbon is filled by hydrogen.\nQuiz: Propane has ___ carbon–carbon double bonds.\nKey Points:",
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"fragment_index": 1,
"text_description": "Only single bonds between carbon atoms.",
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{
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"text_description": "Follow general formula \\(C_nH_{2n+2}\\).",
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]
},
{
"slide": 8,
"fragments": [
{
"fragment_index": -1,
"text_description": "Homologous Series\n{% if context %}\n{{ context }}\n{% endif %}\n{% if source %}\nSource: {{ source }}\n{% endif %}",
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{
"fragment_index": 1,
"text_description": "Homologous Series",
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},
{
"fragment_index": 2,
"text_description": "A group of organic compounds with the same general formula. Each successive member differs by exactly one \\(–\\mathrm{CH_{2}}\\) unit. This constant gap causes gradual changes in physical properties.",
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},
{
"slide": 9,
"fragments": [
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"text_description": "Isomers of Butane\nStraight-chain (n-butane) vs branched (iso-butane)\nOne formula, two shapes",
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{
"fragment_index": 1,
"text_description": "Butane \\( \\mathrm{C_4H_{10}} \\) exhibits structural isomerism.",
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{
"fragment_index": 2,
"text_description": "It exists as a straight chain and a branched ‘T’, sharing the same formula but different atom arrangement.",
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{
"fragment_index": 3,
"text_description": "Key Points:\nStraight chain: CH\n3\n-CH\n2\n-CH\n2\n-CH\n3\nBranched chain: (CH\n3\n)\n3\n-CH\nDifferent shapes ⇒ different physical properties; branched boils lower.\nDemonstrates how one formula can give multiple structures.",
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{
"slide": 10,
"fragments": [
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"text_description": "Name That Formula!\nPractice your formula recognition: drag each alkane name onto its correct molecular formula.\nDraggable Items\nMethane\nEthane\nPropane\nButane\nDrop Zones\nCH₄\nC₂H₆\nC₃H₈\nC₄H₁₀\nTip:\nRemember: the number of hydrogens is twice the carbons plus 2 for alkanes.\nCheck 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=\"${itemId}\"]`);\n\n if (draggedItem && dropZone) {\n dropZone.appendChild(draggedItem);\n dropZone.querySelector('.text-center').style.display = 'none';\n }\n }\n\n // Check answers functionality\n checkAnswersBtn.addEventListener('click', () => {\n const answers = {\n 'zone-1': 'item-1',\n 'zone-2': 'item-2',\n 'zone-3': 'item-3',\n 'zone-4': 'item-4'\n };\n let correct = 0;\n Object.keys(answers).forEach(zoneId => {\n const zone = document.querySelector(`[data-id=\"${zoneId}\"]`);\n const child = zone.querySelector('.draggable-item');\n if (child && child.dataset.id === answers[zoneId]) {\n correct += 1;\n }\n });\n feedbackArea.classList.remove('hidden');\n feedbackContent.innerHTML = `<p class=\"text-gray-800\">You matched ${correct} of 4 correctly.</p>`;\n });",
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},
{
"slide": 11,
"fragments": [
{
"fragment_index": -1,
"text_description": "Key Takeaways\nThank You!\nWe hope you can now recall the main points of carbon chemistry.",
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{
"fragment_index": 1,
"text_description": "Recap: Carbon forms covalent bonds by sharing electrons.",
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},
{
"fragment_index": 2,
"text_description": "It can make single, double, and triple bonds.",
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{
"fragment_index": 3,
"text_description": "Catenation lets carbon build long chains and rings.",
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{
"fragment_index": 4,
"text_description": "Different atom arrangements cause isomerism.",
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{
"fragment_index": 5,
"text_description": "Network structures create diamond, graphite, and other allotropes.",
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}
]
}
]