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24:[["$","$L32",null,{"feature":"flashcards"}],"$L33",["$","$L34",null,{"href":"/igcse/chemistry/cie/properties-of-metals/flashcards","label":"Properties of metals","subjectCode":"igcse_chemistry__cie","surface":"flashcards"}],["$","$L35",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L36",null,{"decks":[{"id":"9e767d56-b789-4420-826a-ab86b604c0a3","title":"Properties of metals Flashcards","topicId":"60417f05-452c-5e9b-b388-e830875eca8b","topicSlug":"properties-of-metals","cards":[{"id":"f74e7b25-e228-47b8-a054-50a191895b23","cardType":"basic","points":1,"front":"What charged particles form the regular lattice in a solid metal?","back":"Positive metal ions.","mcqOptions":[{"text":"Positive metal ions.","correct":true,"explanation":"Metal atoms lose outer electrons, leaving positively charged ions arranged in a regular lattice. The delocalised electrons move between these fixed ions rather than forming the lattice themselves."},{"text":"Negative non-metal ions.","correct":false,"explanation":"Negative non-metal ions occur in ionic compounds, not as the particles forming a pure metal lattice. Metals contain positive metal ions surrounded by delocalised electrons."},{"text":"Delocalised electrons.","correct":false,"explanation":"Delocalised electrons move throughout the metal and are not fixed into regular lattice positions. The lattice is formed by positive metal ions, while the electrons occupy the spaces between them."},{"text":"Neutral metal atoms.","correct":false,"explanation":"Metal atoms lose their outer electrons in metallic bonding, so the lattice particles are charged rather than neutral. The regular lattice consists of positive metal ions."}]},{"id":"0fff090f-cece-4bcb-86ec-33722af5e29b","cardType":"cloze","points":null,"front":"The lost outer electrons in metals become [ ], forming a [ ].","back":"The lost outer electrons in metals become delocalised, forming a sea of electrons.","mcqOptions":[{"text":"The lost outer electrons in metals become delocalised, forming a sea of electrons.","correct":true,"explanation":"In metallic bonding, outer electrons are no longer attached to individual atoms. They become delocalised and move through the structure as a sea of electrons around positive metal ions."},{"text":"The lost outer electrons in metals become localised, forming a sea of electrons.","correct":false,"explanation":"Localised electrons remain associated with particular atoms or bonds, so they cannot form the mobile electron sea in a metal. The correct terms are delocalised and sea of electrons."},{"text":"The lost outer electrons in metals become delocalised, forming a layer of positive ions.","correct":false,"explanation":"Delocalised electrons form a mobile electron sea, not a layer of positive ions. The positive ions are the lattice particles, while the correct completed phrase ends with sea of electrons."},{"text":"The lost outer electrons in metals become shared, forming a network of covalent bonds.","correct":false,"explanation":"Sharing electrons in covalent bonds describes covalent substances, not metallic bonding. In metals, electrons become delocalised and form a sea of electrons."}]},{"id":"46e44ad1-515a-4895-bd37-cf043984239c","cardType":"basic","points":1,"front":"In chemical reactions, what do metals generally do with their outer electrons?","back":"They lose outer electrons to form positive ions.","mcqOptions":[{"text":"They lose outer electrons to form positive ions.","correct":true,"explanation":"Metals have relatively few outer electrons and generally lose them during reactions. Losing negative electrons leaves the atoms positively charged, producing positive metal ions."},{"text":"They gain outer electrons to form negative ions.","correct":false,"explanation":"Gaining electrons is typical of non-metals, which form negative ions. Metals generally lose outer electrons, leaving positive ions because they have more protons than electrons."},{"text":"They share outer electrons to form molecules.","correct":false,"explanation":"Sharing outer electrons is characteristic of covalent bonding between non-metal atoms. In typical reactions, metals lose outer electrons and form positive ions rather than molecules."},{"text":"They lose protons to form negative ions.","correct":false,"explanation":"Chemical reactions involve electrons, not the loss of protons from the nucleus. Metals lose outer electrons, and this produces positive ions because the remaining protons outnumber the electrons."}]},{"id":"4e8426d4-ec21-4b07-b6ba-d9ded8e648a7","cardType":"basic","points":2,"front":"Which structural feature lets metals conduct heat and electricity?","back":"Delocalised electrons move through the lattice.","mcqOptions":[{"text":"Delocalised electrons move through the lattice.","correct":true,"explanation":"Delocalised electrons are free to move throughout a metal lattice. Their movement transfers electrical charge and thermal energy, allowing metals to conduct electricity and heat effectively."},{"text":"Positive metal ions move through the lattice.","correct":false,"explanation":"Positive metal ions are held in fixed positions in the lattice and cannot flow through the solid. Delocalised electrons move and transfer charge and thermal energy."},{"text":"Covalent bonds move through the lattice.","correct":false,"explanation":"Covalent bonds are localised bonds between atoms and do not move through a metal lattice. Conductivity comes from mobile delocalised electrons."},{"text":"Neutrons move through the lattice.","correct":false,"explanation":"Neutrons remain inside atomic nuclei and do not move through the lattice to carry charge or heat. The mobile particles responsible are delocalised electrons."}]},{"id":"2335f79c-0478-40a9-a2ff-9cbc445def38","cardType":"basic","points":2,"front":"Why are non-metals generally poor electrical conductors?","back":"Their electrons are locked in covalent bonds.","mcqOptions":[{"text":"Their electrons are locked in covalent bonds.","correct":true,"explanation":"In most non-metals, electrons are held in localised covalent bonds or lone pairs. They cannot move freely through the substance, so non-metals generally conduct electricity poorly."},{"text":"Their electrons are free to move through the lattice.","correct":false,"explanation":"Electrons that are free to move would carry charge efficiently, as in metals. Non-metals are generally poor conductors because their electrons are locked in covalent bonds."},{"text":"Their protons are locked in covalent bonds.","correct":false,"explanation":"Protons are confined within atomic nuclei and are not involved in covalent bonds. The relevant particles are electrons, which are generally locked in covalent bonds in non-metals."},{"text":"Their electrons are transferred between positive ions.","correct":false,"explanation":"Electron transfer between ions is associated with ionic bonding, not the usual structure of non-metals. Their electrons are generally locked in covalent bonds, preventing electrical conduction."}]},{"id":"5b3fb1d8-321f-4f7d-8f19-ac3271b52fa4","cardType":"cloze","points":null,"front":"Carbon in the form of [ ] is a rare conducting non-metal exception.","back":"Carbon in the form of graphite is a rare conducting non-metal exception.","mcqOptions":[{"text":"graphite","correct":true,"explanation":"Graphite has layers of carbon atoms with one delocalised electron per carbon atom. These electrons can move through the layers, allowing graphite to conduct electricity despite being a non-metal."},{"text":"diamond","correct":false,"explanation":"Diamond’s carbon atoms each form four strong covalent bonds, leaving no delocalised electrons available to carry charge. The conducting carbon allotrope is graphite."},{"text":"graphene oxide","correct":false,"explanation":"Graphene oxide contains oxygen-containing groups that disrupt the continuous electron system and reduce conductivity. The standard rare conducting non-metal exception is graphite."},{"text":"charcoal","correct":false,"explanation":"Charcoal is an impure, disordered form of carbon and is not the named allotrope used for this property. The recognised conducting non-metal exception is graphite."}]},{"id":"eb404170-238d-4ec0-87c2-f8c9a2c0aa15","cardType":"cloze","points":null,"front":"A [ ] material can be rolled into sheets; a [ ] material can be drawn into wires.","back":"A malleable material can be rolled into sheets; a ductile material can be drawn into wires.","mcqOptions":[{"text":"A malleable material can be rolled into sheets; a ductile material can be drawn into wires.","correct":true,"explanation":"Malleability is the ability to be hammered or rolled into sheets, whereas ductility is the ability to be stretched or drawn into wires. These properties arise from metallic bonding."},{"text":"A ductile material can be rolled into sheets; a malleable material can be drawn into wires.","correct":false,"explanation":"The two definitions have been reversed. Rolling into sheets describes malleability, while being drawn into wires describes ductility."},{"text":"A brittle material can be rolled into sheets; a ductile material can be drawn into wires.","correct":false,"explanation":"Brittle materials fracture rather than deform into sheets, so they are not malleable. Rolling into sheets requires a malleable material; drawing into wires requires a ductile one."},{"text":"A malleable material can be rolled into sheets; a elastic material can be drawn into wires.","correct":false,"explanation":"Elasticity means returning to the original shape after a force is removed, not forming wires. The wire-forming property is ductility, while sheet-forming remains malleability."}]},{"id":"2de32a68-b8d3-4724-8926-59095eb84cce","cardType":"basic","points":2,"front":"Why can metals bend without shattering?","back":"

Ion layers slide over each other.
Electron sea holds the lattice together.

","mcqOptions":[{"text":"

Ion layers slide over each other.
Electron sea holds the lattice together.

","correct":true,"explanation":"When a metal is bent, layers of positive ions can slide while the delocalised electron sea continues attracting them. The metallic bonding is therefore maintained instead of the structure shattering."},{"text":"

Ion layers break apart.
Electron sea holds the lattice together.

","correct":false,"explanation":"If ion layers broke apart, the metallic structure would fail rather than bend. Metals bend because ion layers slide over each other while the electron sea maintains attraction."},{"text":"

Covalent layers slide over each other.
Electron sea holds the lattice together.

","correct":false,"explanation":"Metal atoms are not joined in covalent layers. Metals bend because ion layers slide over each other, with the electron sea preserving the attraction between ions."},{"text":"

Ion layers slide over each other.
Covalent bonds hold the lattice together.

","correct":false,"explanation":"Covalent bonds are not responsible for holding a metal lattice together. The correct explanation is that the electron sea maintains attraction as ion layers slide."}]},{"id":"74621937-10b4-4906-8430-ef011eb85e15","cardType":"basic","points":2,"front":"Why do metals generally have high melting and boiling points?","back":"Strong electrostatic attraction between ions and delocalised electrons.","mcqOptions":[{"text":"Strong electrostatic attraction between ions and delocalised electrons.","correct":true,"explanation":"Metallic bonding is strong because oppositely charged positive ions and delocalised electrons attract electrostatically throughout the structure, so considerable energy is needed to separate the particles during melting or boiling."},{"text":"Weak electrostatic attraction between atoms and shared electrons.","correct":false,"explanation":"Weak attractions would require little energy to overcome and therefore give low melting and boiling points. Metals instead contain strong attraction between positive ions and delocalised electrons."},{"text":"Strong covalent bonds between molecules and delocalised electrons.","correct":false,"explanation":"Metals do not usually consist of molecules joined by covalent bonds. Their high melting and boiling points result from strong electrostatic attraction between positive ions and delocalised electrons."},{"text":"Strong ionic attraction between neutral atoms and fixed electrons.","correct":false,"explanation":"The particles in a metal are positive ions, not neutral atoms, and the electrons are delocalised rather than fixed. Their attraction to the ions produces the high melting and boiling points."}]},{"id":"5d760b2e-c8cd-4637-aba6-18d9c4893b1c","cardType":"cloze","points":null,"front":"Many non-metals have [ ], causing [ ].","back":"Many non-metals have weak intermolecular forces, causing low melting and boiling points.","mcqOptions":[{"text":"Many non-metals have weak intermolecular forces, causing low melting and boiling points.","correct":true,"explanation":"Weak intermolecular forces between non-metal molecules are easily overcome, so little energy is needed to separate the molecules and produce low melting and boiling points."},{"text":"Many non-metals have strong intermolecular forces, causing low melting and boiling points.","correct":false,"explanation":"Strong intermolecular forces require more energy to overcome and would raise melting and boiling points. The usual explanation for many non-metals is weak intermolecular forces."},{"text":"Many non-metals have weak intermolecular forces, causing high melting and boiling points.","correct":false,"explanation":"Weak intermolecular forces are easily overcome, so they lead to low rather than high melting and boiling points. High values would require strong attractions between particles."},{"text":"Many non-metals have strong metallic bonds, causing high melting and boiling points.","correct":false,"explanation":"Metallic bonding is characteristic of metals, not most non-metals. Many non-metals have weak intermolecular forces, which explains their low melting and boiling points."}]},{"id":"4a424f8d-9083-425e-9b84-f0dfeac5200f","cardType":"basic","points":1,"front":"What is formed when most metals react with oxygen?","back":"A solid metal oxide.","mcqOptions":[{"text":"A solid metal oxide.","correct":true,"explanation":"Oxygen combines with the metal to form a metal oxide. These products are generally solids because the ions or atoms are held in a strong structure."},{"text":"A solid metal hydroxide.","correct":false,"explanation":"Metal hydroxides form when metals react with water, not simply oxygen. Reaction with oxygen produces a metal oxide, which is generally a solid."},{"text":"A dissolved metal oxide.","correct":false,"explanation":"Oxygen reacting directly with a metal does not produce a dissolved product. The usual product is a solid metal oxide; dissolving would require a separate reaction with a solvent."},{"text":"A gaseous metal oxide.","correct":false,"explanation":"Most metal oxides formed in these reactions are solid substances rather than gases. The expected general product is a solid metal oxide."}]},{"id":"a0dae306-919e-44d0-916e-2b793ec76549","cardType":"basic","points":2,"front":"Write the balanced equation for magnesium burning in oxygen.","back":"$2\\text{Mg} + \\text{O}_2 \\to 2\\text{MgO}$","mcqOptions":[{"text":"$2\\text{Mg} + \\text{O}_2 \\to 2\\text{MgO}$","correct":true,"explanation":"Two magnesium atoms react with one oxygen molecule to form two magnesium oxide units, giving two magnesium and two oxygen atoms on each side of the equation."},{"text":"$\\text{Mg} + \\text{O}_2 \\to \\text{MgO}$","correct":false,"explanation":"This leaves two oxygen atoms on the left but only one on the right. The smallest whole-number balancing requires two magnesium atoms and two magnesium oxide units."},{"text":"$2\\text{Mg} + \\text{O}_2 \\to \\text{MgO}_2$","correct":false,"explanation":"The formula of magnesium oxide is MgO, not MgO₂. Balancing MgO gives two MgO units for each O₂ molecule, so the correct equation uses coefficients 2, 1, and 2."},{"text":"$\\text{Mg} + \\text{O}_2 \\to 2\\text{MgO}$","correct":false,"explanation":"Although the oxygen atoms balance here, only one magnesium atom is present on the left and two on the right. A coefficient of 2 is also needed before magnesium."}]},{"id":"f4cc2172-afe4-462a-8cdb-136afa3fc111","cardType":"cloze","points":null,"front":"Cold water forms a metal [ ]; steam forms a metal [ ].","back":"Cold water forms a metal hydroxide; steam forms a metal oxide.","mcqOptions":[{"text":"Cold water forms a metal hydroxide; steam forms a metal oxide.","correct":true,"explanation":"Reaction with cold water produces a metal hydroxide and hydrogen. With steam, the hydroxide is not stable at high temperature and the product is a metal oxide instead."},{"text":"Cold water forms a metal oxide; steam forms a metal hydroxide.","correct":false,"explanation":"The products have been reversed. Cold water supplies conditions for hydroxide formation, whereas hot steam leads to a metal oxide because any hydroxide decomposes."},{"text":"Cold water forms a metal hydride; steam forms a metal oxide.","correct":false,"explanation":"Metal hydrides are not the general products of these reactions. Cold water produces a metal hydroxide, while steam produces a metal oxide and hydrogen."},{"text":"Cold water forms a metal hydroxide; steam forms a metal hydride.","correct":false,"explanation":"Steam does not generally form a metal hydride in this reaction. It produces a metal oxide because the high temperature causes the hydroxide intermediate to decompose."}]},{"id":"2133da1f-9ae3-48b4-b935-c44fb11dc437","cardType":"basic","points":1,"front":"What gas is produced when metals react with cold water or steam?","back":"Hydrogen gas.","mcqOptions":[{"text":"Hydrogen gas.","correct":true,"explanation":"The metal displaces hydrogen from water. The hydrogen atoms pair to form hydrogen gas, while the metal forms a hydroxide with cold water or an oxide with steam."},{"text":"Oxygen gas.","correct":false,"explanation":"Oxygen is a reactant in many metal oxidation reactions, not the gas displaced from water. Metals reacting with cold water or steam release hydrogen gas."},{"text":"Carbon dioxide gas.","correct":false,"explanation":"Carbon dioxide is not present in the usual metal-water reaction and is not displaced by metals. The gas formed is hydrogen, produced when water is reduced."},{"text":"Nitrogen gas.","correct":false,"explanation":"Nitrogen is not a component of water and is not released in this reaction. Metals reacting with cold water or steam produce hydrogen gas."}]},{"id":"8a7a3708-f3cb-419e-ad97-157baf097e8e","cardType":"basic","points":2,"front":"Why do magnesium, zinc and iron need steam rather than cold water?","back":"They are less reactive, so cold-water reactions are too slow.","mcqOptions":[{"text":"They are less reactive, so cold-water reactions are too slow.","correct":true,"explanation":"Magnesium, zinc and iron are below the most reactive metals in the reactivity series. They react too slowly with cold water, but steam provides more energy and increases the reaction rate."},{"text":"They are more reactive, so cold-water reactions are too fast.","correct":false,"explanation":"These metals are not more reactive than metals such as potassium, sodium and calcium. Their cold-water reactions are too slow, so steam is used to provide higher-temperature conditions."},{"text":"They are less reactive, so cold-water reactions are too fast.","correct":false,"explanation":"Lower reactivity means a reaction is slower, not faster. Magnesium, zinc and iron need steam because their reactions with cold water are too slow to be useful."},{"text":"They are unreactive, so steam cannot react with them.","correct":false,"explanation":"These metals are reactive enough to react with steam, although not quickly with cold water. Calling them unreactive would incorrectly suggest that steam produces no reaction."}]},{"id":"c102f8de-4e7f-449f-9575-0ffc73180eb3","cardType":"basic","points":2,"front":"Why does steam produce a metal oxide rather than a hydroxide?","back":"The metal hydroxide thermally decomposes immediately.","mcqOptions":[{"text":"The metal hydroxide thermally decomposes immediately.","correct":true,"explanation":"Steam provides high-temperature conditions. Any metal hydroxide formed initially breaks down immediately into a metal oxide and water, so the oxide is observed as the final product."},{"text":"The metal hydroxide dissolves immediately.","correct":false,"explanation":"Dissolving does not explain formation of the oxide during reaction with steam. The hydroxide undergoes thermal decomposition at the high temperature, producing the metal oxide and water."},{"text":"The metal hydroxide freezes immediately.","correct":false,"explanation":"Steam is hot, so freezing is not the relevant process. The high temperature instead causes the metal hydroxide to thermally decompose into a metal oxide and water."},{"text":"The metal hydroxide oxidises the hydrogen immediately.","correct":false,"explanation":"The hydroxide does not produce the oxide by oxidising hydrogen. Thermal decomposition directly converts the hydroxide into a metal oxide and water at high temperature."}]},{"id":"aff958b9-cbe4-44be-a6ea-b34b38bffc4f","cardType":"basic","points":2,"front":"What are the products of metal + dilute acid?","back":"

Salt
Hydrogen gas

","mcqOptions":[{"text":"

Salt
Hydrogen gas

","correct":true,"explanation":"A metal reacting with a dilute acid displaces hydrogen ions from the acid, producing a salt containing the metal and releasing hydrogen gas."},{"text":"

Salt
Water

","correct":false,"explanation":"Salt and water are produced in acid neutralisation by a base or alkali. A reactive metal instead forms a salt and hydrogen gas with dilute acid."},{"text":"

Metal oxide
Hydrogen gas

","correct":false,"explanation":"A metal oxide and hydrogen can form when some metals react with steam, not with dilute acid. Dilute acid produces a salt and hydrogen gas."},{"text":"

Salt
Carbon dioxide

","correct":false,"explanation":"Salt, water and carbon dioxide are characteristic products of an acid reacting with a carbonate. A metal reacting with dilute acid produces salt and hydrogen gas."}]},{"id":"9f7a46bd-e5f1-483c-b30e-ff94be44c371","cardType":"cloze","points":null,"front":"Metals above [ ] in the reactivity series react with dilute acids.","back":"Metals above hydrogen in the reactivity series react with dilute acids.","mcqOptions":[{"text":"hydrogen","correct":true,"explanation":"Metals above hydrogen are sufficiently reactive to displace hydrogen ions from dilute acids, forming a salt and hydrogen gas. Metals below hydrogen do not normally react."},{"text":"carbon","correct":false,"explanation":"Carbon is used as a reference when deciding whether metal oxides can be reduced by carbon. Hydrogen is the relevant dividing point for reactions with dilute acids."},{"text":"copper","correct":false,"explanation":"Copper is below hydrogen and does not react with typical dilute acids, but it is not the reference point. Metals above hydrogen react with dilute acids."},{"text":"magnesium","correct":false,"explanation":"Magnesium reacts readily with dilute acids, but less reactive metals such as zinc and iron do too. The actual threshold in the reactivity series is hydrogen."}]},{"id":"0c781a63-cded-4b8d-81ec-e89656fd6bde","cardType":"basic","points":2,"front":"Write the balanced equation for zinc reacting with hydrochloric acid.","back":"$\\text{Zn} + 2\\text{HCl} \\to \\text{ZnCl}_2 + \\text{H}_2$","mcqOptions":[{"text":"$\\text{Zn} + 2\\text{HCl} \\to \\text{ZnCl}_2 + \\text{H}_2$","correct":true,"explanation":"One zinc atom forms zinc chloride, requiring two chloride ions from two HCl molecules. The two remaining hydrogen atoms combine to form one hydrogen molecule."},{"text":"$\\text{Zn} + \\text{HCl} \\to \\text{ZnCl}_2 + \\text{H}_2$","correct":false,"explanation":"Using only one HCl leaves one chlorine and one hydrogen atom on the left, while the products contain two of each. The coefficient before HCl must be 2."},{"text":"$\\text{Zn} + 2\\text{HCl} \\to \\text{ZnCl} + \\text{H}_2$","correct":false,"explanation":"Zinc forms $\\text{Zn}^{2+}$ ions, so its chloride is $\\text{ZnCl}_2$, not $\\text{ZnCl}$. The balanced equation uses two HCl molecules and produces $\\text{H}_2$."},{"text":"$2\\text{Zn} + 2\\text{HCl} \\to 2\\text{ZnCl}_2 + \\text{H}_2$","correct":false,"explanation":"Doubling zinc requires doubling zinc chloride, but two HCl molecules cannot supply the four chlorine atoms then needed. The simplest balanced ratio is $1:2:1:1$."}]},{"id":"7689fabb-42b4-4856-b024-45cc7275bcb6","cardType":"basic","points":3,"front":"Write the state-symbol equation for heated magnesium reacting with steam.","back":"$\\text{Mg}\\text{(s)} + \\text{H}_2\\text{O}\\text{(g)} \\to \\text{MgO}\\text{(s)} + \\text{H}_2\\text{(g)}$","mcqOptions":[{"text":"$\\text{Mg}\\text{(s)} + \\text{H}_2\\text{O}\\text{(g)} \\to \\text{MgO}\\text{(s)} + \\text{H}_2\\text{(g)}$","correct":true,"explanation":"Heated magnesium removes oxygen from steam, forming solid magnesium oxide and hydrogen gas. The equation is balanced with one atom of magnesium and oxygen on each side."},{"text":"$\\text{Mg}\\text{(s)} + 2\\text{H}_2\\text{O}\\text{(g)} \\to \\text{Mg(OH)}_2\\text{(s)} + \\text{H}_2\\text{(g)}$","correct":false,"explanation":"Magnesium hydroxide is associated with magnesium reacting very slowly with cold water. When heated magnesium reacts with steam, the solid product is magnesium oxide, $\\text{MgO}$."},{"text":"$\\text{Mg}\\text{(s)} + \\text{H}_2\\text{O}\\text{(l)} \\to \\text{MgO}\\text{(s)} + \\text{H}_2\\text{(g)}$","correct":false,"explanation":"The question specifies steam, so water must have the gaseous state symbol, $\\text{(g)}$, rather than the liquid symbol, $\\text{(l)}$. The other substances have the correct states."},{"text":"$\\text{Mg}\\text{(g)} + \\text{H}_2\\text{O}\\text{(g)} \\to \\text{MgO}\\text{(s)} + \\text{H}_2\\text{(g)}$","correct":false,"explanation":"Heating magnesium sufficiently for reaction does not mean it becomes gaseous; magnesium remains solid under the reaction conditions. Its state symbol must therefore be $\\text{(s)}$."}]}]}],"examCountdown":null,"heading":"Properties of metals","title":"Properties of metals Flashcards","topbar":{"backHref":"/igcse/chemistry/cie/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"60417f05-452c-5e9b-b388-e830875eca8b","walled":"$L38"}],"$L39","$L3a"]