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[
{
"slide": 1,
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"text_description": "Meet Carbon\nCarbon (C)\nAtomic number 6 places carbon in Group 14. Four valence electrons make it tetravalent, able to form four covalent bonds.\nQuick check: How many valence electrons does carbon have?",
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{
"slide": 2,
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"fragment_index": -1,
"text_description": "What is a Covalent Bond?\nElectron sharing in H₂\nSharing Electrons: The Hydrogen Molecule\nA covalent bond forms when atoms share electrons to fill their outer shell.\nIn H₂, two hydrogen atoms share one electron each, creating a single shared pair.\nKey Points:",
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"text_description": "Covalent bond = electron sharing, not transfer.",
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{
"fragment_index": 2,
"text_description": "Hydrogen molecule has 1 shared pair (2 electrons).",
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},
{
"fragment_index": 3,
"text_description": "Sharing lets each H feel its shell is full.",
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{
"slide": 3,
"fragments": [
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"fragment_index": 1,
"text_description": "Single Bond",
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{
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"text_description": "",
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{
"fragment_index": 2,
"text_description": "One Pair Shared = Single Covalent Bond",
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},
{
"fragment_index": 3,
"text_description": "A single covalent bond forms when two atoms share one pair of electrons.",
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{
"fragment_index": 4,
"text_description": "In a hydrogen molecule (H₂), each hydrogen donates one electron to the shared pair.",
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{
"fragment_index": 5,
"text_description": "Key Points:\nExactly 2 electrons in the bond pair.\nRepresented by a single dash: H–H.",
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},
{
"slide": 4,
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"fragment_index": -1,
"text_description": "Double Bond\nLewis structure of O₂ showing a double bond\nWhat is a Double Covalent Bond?\nA double covalent bond forms when two atoms share two pairs of electrons.\nThe oxygen molecule \\(O_2\\) is held together by one double bond.\nKey Points:",
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{
"fragment_index": 1,
"text_description": "2 shared electron pairs = 4 electrons.",
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{
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"text_description": "Represented by two lines: O = O.",
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{
"fragment_index": 3,
"text_description": "Oxygen \\(O_2\\) is a common example.",
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]
},
{
"slide": 5,
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"fragment_index": -1,
"text_description": "Triple Bond\nLewis structure of N₂\nThree shared pairs\nA triple bond forms when two atoms share three electron pairs.\nNitrogen molecule (N₂) is held together by this strong triple bond.\nKey Points:\n3 shared pairs = 6 bonding electrons.\nNotation: N≡N.\nTriple bonds are very strong, making N₂ inert.",
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{
"slide": 6,
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"text_description": "Diamond – A Carbon Allotrope\n3-D tetrahedral lattice of diamond\nWhy is diamond so hard and non-conductive?\nDiamond is an allotrope of carbon where every atom forms four strong covalent bonds in a tetrahedral arrangement.\nThis rigid, endless 3-D lattice leaves no free electrons, making diamond extremely hard and a poor conductor.\nKey Points:",
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"fragment_index": 1,
"text_description": "Allotrope: carbon atoms in a continuous tetrahedral network.",
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{
"fragment_index": 2,
"text_description": "Each carbon forms 4 sp³ covalent bonds.",
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},
{
"fragment_index": 3,
"text_description": "No mobile electrons, so electricity cannot pass.",
"image_description": ""
},
{
"fragment_index": 4,
"text_description": "Strong bonds in all directions give extreme hardness.",
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}
]
},
{
"slide": 7,
"fragments": [
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"fragment_index": -1,
"text_description": "Methane Molecule\nElectron dot diagram of methane\nElectron Dot Structure of Methane\nMethane, formula CH₄, is the simplest alkane.\nCarbon forms four single covalent bonds, one with each hydrogen.\nEach bond shares a pair of electrons, filling carbon’s octet and hydrogen’s duet.\nAfter this slide, you can draw methane’s electron dot structure yourself.\nKey Points:\nWrite element symbols: C in center, four H around.\nPlace one dot from carbon and one from each hydrogen to form each bond.\nCheck: carbon has 8 shared electrons, every hydrogen has 2.",
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{
"slide": 8,
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"text_description": "Saturated: Ethane\nBall-and-stick model of ethane\nEthane is a saturated hydrocarbon\nEthane \\(C_2H_6\\) is an alkane with two carbon atoms and six hydrogens.\nAll its C–C and C–H bonds are single, leaving no space for extra atoms—so it is termed “saturated.”\nKey Points:\nAlkanes contain only single covalent bonds.\nSingle bonds make the molecule saturated.\nEthane is the simplest saturated hydrocarbon after methane.",
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"slide": 9,
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"text_description": "Unsaturated: Ethene\nStructural formula of ethene showing the C=C bond.\nEthene – An Unsaturated Hydrocarbon\nEthene \\( \\mathrm{C_2H_4} \\) is the simplest alkene and an unsaturated hydrocarbon.\nIts carbon–carbon double bond is easy to spot and makes the molecule highly reactive.\nKey Points:",
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"text_description": "Has one C=C double bond.",
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{
"fragment_index": 2,
"text_description": "Unsaturated: fewer hydrogens than an alkane.",
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},
{
"fragment_index": 3,
"text_description": "Double bond can open for addition of atoms.",
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{
"fragment_index": 4,
"text_description": "Hence more reactive than ethane (single bonds only).",
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}
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{
"slide": 10,
"fragments": [
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"text_description": "Isomers of Butane\nn-butane (straight) vs iso-butane (branched)\nSame formula, two different shapes\nKey Points:",
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{
"fragment_index": 1,
"text_description": "Butane has molecular formula \\( \\mathrm{C_4H_{10}} \\).",
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{
"fragment_index": 2,
"text_description": "It can join its four carbon atoms in a straight or branched chain, creating two distinct molecules.",
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},
{
"fragment_index": 3,
"text_description": "Different structures with the same formula are called\nisomers\n.",
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},
{
"fragment_index": 4,
"text_description": "Straight-chain isomer: n-butane.",
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},
{
"fragment_index": 5,
"text_description": "Branched isomer: iso-butane (2-methylpropane).",
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},
{
"fragment_index": 6,
"text_description": "Isomerism shows that one formula can yield different structures and properties.",
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},
{
"slide": 11,
"fragments": [
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"text_description": "Match Name & Formula\nPractice nomenclature: drag each hydrocarbon name onto its matching molecular formula. Goal — pair every compound correctly.\nDraggable Items\nMethane\nEthane\nEthene\nButane\nDrop Zones\nCH₄\nC₂H₆\nC₂H₄\nC₄H₁₀\nTip:\nCount the number of C and H atoms to guide your match.\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=\"${itemId}\"]`);\n \n if (draggedItem && dropZone) {\n dropZone.appendChild(draggedItem);\n dropZone.querySelector('.text-center').style.display = 'none';\n }\n }\n \n // Check answers functionality\n checkAnswersBtn.addEventListener('click', () => {\n let correct = 0;\n dropZones.forEach(zone => {\n const item = zone.querySelector('.draggable-item');\n if (!item) return;\n const id = item.dataset.id;\n if (\n (id === 'methane' && zone.dataset.id === 'ch4') ||\n (id === 'ethane' && zone.dataset.id === 'c2h6') ||\n (id === 'ethene' && zone.dataset.id === 'c2h4') ||\n (id === 'butane' && zone.dataset.id === 'c4h10')\n ) {\n correct++;\n }\n });\n feedbackArea.classList.remove('hidden');\n if (correct === 4) {\n feedbackContent.innerHTML = '<p class=\"text-green-600 font-semibold\">Excellent! All pairs are correct.</p>';\n } else {\n feedbackContent.innerHTML = `<p class=\"text-red-600 font-semibold\">${4 - correct} match(es) need correction. Try again!</p>`;\n }\n });",
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{
"slide": 12,
"fragments": [
{
"fragment_index": -1,
"text_description": "Key Takeaways\nThank You!\nWe hope you found this lesson informative and engaging.",
"image_description": ""
},
{
"fragment_index": 1,
"text_description": "Carbon is tetravalent, so it forms strong covalent bonds.",
"image_description": ""
},
{
"fragment_index": 2,
"text_description": "Single, double, and triple bonds share one, two, or three electron pairs.",
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},
{
"fragment_index": 3,
"text_description": "Carbon’s versatility creates allotropes such as diamond and graphite.",
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{
"fragment_index": 4,
"text_description": "Alkanes are saturated; alkenes and alkynes are unsaturated.",
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{
"fragment_index": 5,
"text_description": "Isomerism means the same formula can form different structures.",
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}
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]