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gain electrons, not lose them. Losing electrons produces a positive ion because electrons carry negative charge, so the correct answer is a cation."},{"text":"A neutral atom (no charge).","correct":false,"explanation":"A neutral atom has equal numbers of protons and electrons. Losing electrons creates an imbalance with more positive charge, so the correct answer is a cation."},{"text":"A cation (negative ion).","correct":false,"explanation":"The term cation is correct, but its charge is positive, not negative. Losing electrons removes negative charge, so the correct answer is a cation (positive ion)."}]},{"id":"22741c94-b0d6-488b-98be-ba2215a7d178","cardType":"basic","points":1,"front":"What particle is formed when an atom gains electrons?","back":"An anion (negative ion).","mcqOptions":[{"text":"An anion (negative ion).","correct":true,"explanation":"Gaining negatively charged electrons gives the atom more electrons than protons, producing a negatively charged ion called an anion."},{"text":"A cation (positive ion).","correct":false,"explanation":"Cations form when atoms lose electrons. Gaining electrons adds negative charge, so the correct answer is an anion (negative ion)."},{"text":"A neutral atom (no charge).","correct":false,"explanation":"A neutral atom has balanced positive and negative charges. Gaining electrons creates excess negative charge, so the correct answer is an anion."},{"text":"An anion (positive ion).","correct":false,"explanation":"The term anion is correct, but anions are negative, not positive. Gaining electrons adds negative charge, so the correct answer is an anion (negative ion)."}]},{"id":"92b416db-4976-4d49-99af-41ea5ad3f836","cardType":"cloze","points":null,"front":"In ionic bonding, metals usually [ ] electrons while non-metals usually gain electrons.","back":"In ionic bonding, metals usually lose electrons while non-metals usually gain electrons.","mcqOptions":[{"text":"lose","correct":true,"explanation":"Metals have relatively few outer-shell electrons and usually lose them to form positive ions, while non-metals gain electrons to form negative ions."},{"text":"gain","correct":false,"explanation":"Gaining electrons is usually the behaviour of non-metals, not metals. Metals typically lose outer-shell electrons and form positive ions, so the correct term is lose."},{"text":"share","correct":false,"explanation":"Sharing electrons is characteristic of covalent bonding. In ionic bonding, metals usually lose electrons and non-metals gain them, so the correct term is lose."},{"text":"transfer","correct":false,"explanation":"Electrons are transferred between atoms overall, but metals specifically lose electrons during this process. The correct term describing metals is lose."}]},{"id":"98a72c9e-5362-4556-baf0-539217a5e4d0","cardType":"cloze","points":null,"front":"In ionic bonding, metals usually lose electrons while non-metals usually [ ] electrons.","back":"In ionic bonding, metals usually lose electrons while non-metals usually gain electrons.","mcqOptions":[{"text":"gain","correct":true,"explanation":"Non-metals usually gain electrons to fill their outer shell and form negatively charged ions, while metals usually lose electrons."},{"text":"lose","correct":false,"explanation":"Losing electrons is usually associated with metals forming positive ions. Non-metals generally gain electrons to form negative ions, so the correct term is gain."},{"text":"share","correct":false,"explanation":"Sharing electrons occurs in covalent bonding rather than the usual ionic process. Non-metals in ionic bonding gain electrons, so the correct term is gain."},{"text":"transfer","correct":false,"explanation":"Electrons are transferred between particles during ionic bonding, but non-metals specifically gain them. The correct term describing non-metals is gain."}]},{"id":"6746ad62-0f8b-404e-afab-47c3ede85e8e","cardType":"basic","points":1,"front":"Why do atoms form ions in terms of stability?","back":"To achieve a full outer shell of electrons.","mcqOptions":[{"text":"To achieve a full outer shell of electrons.","correct":true,"explanation":"Atoms form ions to reach a more stable electron arrangement, usually with a full outer shell like the noble gases."},{"text":"To achieve an empty outer shell of electrons.","correct":false,"explanation":"An empty outer shell is not the usual stable arrangement for the resulting ion. Atoms form ions to achieve a full outer shell of electrons."},{"text":"To achieve a full inner shell of electrons.","correct":false,"explanation":"The inner shells are normally already filled and are not the focus of ion formation. Atoms form ions to achieve a full outer shell of electrons."},{"text":"To achieve an equal number of protons and neutrons.","correct":false,"explanation":"Ion formation changes electrons, not the numbers of protons or neutrons. Atoms form ions to achieve a full outer shell of electrons."}]},{"id":"550ffc77-6f89-4421-be56-37229a3899f7","cardType":"basic","points":1,"front":"Predict the charge of an ion formed by a Group 6 element.","back":"$$2-$","mcqOptions":[{"text":"$$2-$","correct":true,"explanation":"Group 6 atoms have six outer-shell electrons and usually gain two electrons to complete the shell, giving the ion a charge of $2-$."},{"text":"$$6-$","correct":false,"explanation":"The group number shows six outer electrons, not a six-minus charge. A Group 6 atom gains two electrons to fill its shell, giving $2-$."},{"text":"$$2+$","correct":false,"explanation":"A positive charge would result from losing electrons, but Group 6 atoms usually gain two electrons. Their ion therefore has charge $2-$."},{"text":"$$3-$","correct":false,"explanation":"Group 6 atoms need two more electrons, not three, to complete their outer shell. Gaining two electrons gives the ion charge $2-$."}]},{"id":"8775613c-03df-4590-8dc6-c91572615545","cardType":"basic","points":1,"front":"Predict the charge of an ion formed by a Group 3 element.","back":"$$3+$","mcqOptions":[{"text":"$$3+$","correct":true,"explanation":"Group 3 atoms have three outer-shell electrons and usually lose all three to leave a full shell underneath, forming an ion with charge $3+$."},{"text":"$$3-$","correct":false,"explanation":"Group 3 elements usually lose three outer electrons rather than gain them. Losing negative electrons leaves a positive ion with charge $3+$."},{"text":"$$2+$","correct":false,"explanation":"The charge is not found by assuming two electrons are lost. Group 3 atoms usually lose three outer electrons, producing charge $3+$."},{"text":"$$1+$","correct":false,"explanation":"Group 3 atoms have three outer-shell electrons available to lose, not just one. Losing all three produces the characteristic ion charge $3+$."}]},{"id":"17ab3889-4780-47ad-9222-e302060dfafe","cardType":"basic","points":1,"front":"Identify the formula for the Ammonium ion.","back":"$$NH_4^+$","mcqOptions":[{"text":"$$NH_4^+$","correct":true,"explanation":"The ammonium ion consists of one nitrogen atom bonded to four hydrogen atoms and has an overall positive charge, written as $NH_4^+$."},{"text":"$$NH_3$","correct":false,"explanation":"$$NH_3$ is ammonia, a neutral molecule, not the ammonium ion. Ammonium forms when ammonia gains a hydrogen ion, giving the formula $NH_4^+$."},{"text":"$$NO_4^+$","correct":false,"explanation":"Ammonium contains hydrogen, not oxygen. Its formula has one nitrogen, four hydrogen atoms and a positive charge: $NH_4^+$."},{"text":"$$NH_4^-$","correct":false,"explanation":"Ammonium is positively charged, so the sign is plus rather than minus. The correct formula is $NH_4^+$, containing four hydrogen atoms."}]},{"id":"261d9bcf-6d02-4881-aca3-9bbc83eb08df","cardType":"basic","points":1,"front":"Identify the formula for the Sulfate ion.","back":"$$SO_4^{2-}$","mcqOptions":[{"text":"$$SO_4^{2-}$","correct":true,"explanation":"Sulfate contains one sulfur atom and four oxygen atoms and carries an overall charge of $2-$, giving the formula $SO_4^{2-}$."},{"text":"$$SO_3^{2-}$","correct":false,"explanation":"This is sulfite, which has three oxygen atoms. Sulfate has four oxygen atoms and an overall $2-$ charge, so its formula is $SO_4^{2-}$."},{"text":"$$NO_3^{-}$","correct":false,"explanation":"This is the nitrate ion, not sulfate. Sulfate contains sulfur bonded with four oxygen atoms and has the formula $SO_4^{2-}$."},{"text":"$$CO_3^{2-}$","correct":false,"explanation":"This is the carbonate ion, which contains carbon rather than sulfur. The sulfate ion contains sulfur and four oxygen atoms, giving $SO_4^{2-}$."}]},{"id":"76543a6d-5091-4149-bd47-afb8b5d3cca8","cardType":"basic","points":1,"front":"What does the Roman numeral in iron(III) represent?","back":"The ion has a $3+$ charge ($Fe^{3+}$).","mcqOptions":[{"text":"The ion has a $3+$ charge ($Fe^{3+}$).","correct":true,"explanation":"The Roman numeral specifies the positive charge on a transition-metal ion. Iron(III) therefore means that each iron ion has a $3+$ charge, written $Fe^{3+}$."},{"text":"The ion has a $2+$ charge ($Fe^{2+}$).","correct":false,"explanation":"A $2+$ charge corresponds to iron(II), not iron(III). The Roman numeral III specifies an iron ion with a $3+$ charge, written $Fe^{3+}$."},{"text":"The ion has a $3-$ charge ($Fe^{3-}$).","correct":false,"explanation":"The numeral gives the magnitude of the ion’s positive charge, not a negative charge. Iron(III) is the cation $Fe^{3+}$, with a $3+$ charge."},{"text":"The formula contains three iron ions ($Fe_3$).","correct":false,"explanation":"The Roman numeral does not count iron ions in a formula. It identifies the charge on each iron ion, so iron(III) means $Fe^{3+}$."}]},{"id":"df9b3d27-26f0-4363-a519-cb06a5f1e476","cardType":"cloze","points":null,"front":"An ionic bond is the strong [ ] between oppositely charged ions.","back":"An ionic bond is the strong electrostatic attraction between oppositely charged ions.","mcqOptions":[{"text":"electrostatic attraction","correct":true,"explanation":"Positive and negative ions attract through electrostatic forces. This strong electrostatic attraction between oppositely charged ions is the definition of an ionic bond."},{"text":"covalent attraction","correct":false,"explanation":"Electron sharing produces covalent bonds rather than ionic bonds. An ionic bond is the strong electrostatic attraction between oppositely charged positive and negative ions."},{"text":"magnetic attraction","correct":false,"explanation":"Magnetic attraction concerns magnetic fields and is not responsible for ionic bonding. Ionic bonds result from electrostatic attraction between ions carrying opposite electrical charges."},{"text":"gravitational attraction","correct":false,"explanation":"Gravitational attraction between individual particles is negligible and does not form ionic bonds. The bonding force is electrostatic attraction between oppositely charged ions."}]},{"id":"54256d64-de51-471f-9ec7-c2689d504d75","cardType":"cloze","points":null,"front":"An ionic bond is the strong electrostatic attraction between [ ].","back":"An ionic bond is the strong electrostatic attraction between oppositely charged ions.","mcqOptions":[{"text":"oppositely charged ions","correct":true,"explanation":"Cations and anions carry positive and negative charges respectively, so they attract electrostatically. This attraction between oppositely charged ions forms an ionic bond."},{"text":"similarly charged ions","correct":false,"explanation":"Similarly charged ions repel rather than attract, so they cannot provide the stated electrostatic attraction. Ionic bonds form between oppositely charged ions."},{"text":"oppositely charged atoms","correct":false,"explanation":"Atoms must first gain or lose electrons to become charged ions. Ionic bonding is specifically the electrostatic attraction between oppositely charged ions, not neutral atoms."},{"text":"shared electron pairs","correct":false,"explanation":"Shared electron pairs hold atoms together in covalent bonds. Ionic bonds instead arise from electrostatic attraction between positive and negative ions."}]},{"id":"fcb5ce44-005d-4faa-b87b-a0b2d3e03f73","cardType":"basic","points":1,"front":"What must be true about the overall charge of an ionic compound?","back":"It must be neutral (total positive charge equals total negative charge).","mcqOptions":[{"text":"It must be neutral (total positive charge equals total negative charge).","correct":true,"explanation":"An ionic compound contains ions in a ratio that balances their charges. Its total positive charge therefore equals its total negative charge, making the compound neutral overall."},{"text":"It must be positive (total positive charge exceeds total negative charge).","correct":false,"explanation":"An individual ion can be positive, but a complete ionic compound cannot have excess positive charge. Its positive and negative charges must balance, making it neutral overall."},{"text":"It must be negative (total negative charge exceeds total positive charge).","correct":false,"explanation":"An individual ion can be negative, but a complete ionic compound cannot have excess negative charge. Its total positive and negative charges must be equal."},{"text":"It must have equal numbers of ions (positive ions equal negative ions).","correct":false,"explanation":"Equal numbers of positive and negative ions are not always required, as their charge magnitudes may differ. The total charges, rather than the numbers of ions, must balance."}]},{"id":"493013b0-99a0-449c-b3b4-319d6a74a928","cardType":"basic","points":1,"front":"Determine the formula for aluminium oxide ($Al^{3+}$ and $O^{2-}$).","back":"$$Al_2O_3$","mcqOptions":[{"text":"$$Al_2O_3$","correct":true,"explanation":"Two $Al^{3+}$ ions provide a total charge of $6+$, while three $O^{2-}$ ions provide $6-$. These charges balance in $Al_2O_3$."},{"text":"$$Al_3O_2$","correct":false,"explanation":"This reverses the required subscripts, producing charges of $9+$ from aluminium and $4-$ from oxide. Charge balance requires two aluminium ions and three oxide ions: $Al_2O_3$."},{"text":"$$AlO$","correct":false,"explanation":"A one-to-one ratio gives charges of $3+$ and $2-$, so the compound would not be neutral. The smallest balanced ratio gives $Al_2O_3$."},{"text":"$$AlO_3$","correct":false,"explanation":"This treats aluminium and oxide as though their charges balance in a one-to-three ratio. Their lowest common charge is six, giving the neutral formula $Al_2O_3$."}]},{"id":"e19c4205-e9ab-4134-ad02-f8dd373a6089","cardType":"basic","points":1,"front":"Why are brackets used in the formula $Ca(NO_3)_2$?","back":"To show there is more than one compound ion (nitrate) present.","mcqOptions":[{"text":"To show there is more than one compound ion (nitrate) present.","correct":true,"explanation":"The subscript $2$ applies to the entire nitrate ion inside the brackets. It therefore shows that two complete nitrate ions are present for each calcium ion."},{"text":"To show there is more than one calcium ion (calcium) present.","correct":false,"explanation":"The brackets do not indicate multiple calcium ions; calcium appears outside them with no subscript. They show that the whole nitrate ion occurs twice."},{"text":"To show there is more than one oxygen atom (oxide) present.","correct":false,"explanation":"Individual oxygen atoms are already counted by the $3$ inside $NO_3$. The brackets ensure the outer $2$ multiplies the entire nitrate ion, not oxygen alone."},{"text":"To show there is more than one covalent bond (in nitrate) present.","correct":false,"explanation":"Brackets in an ionic formula do not represent covalent bonds. They group the atoms of nitrate so that the outer subscript applies to two complete nitrate ions."}]},{"id":"bf1a7ad8-ea1c-45c7-b47c-a9c434534961","cardType":"cloze","points":null,"front":"In a dot-and-cross diagram for ionic bonding, electrons are [ ] rather than shared.","back":"In a dot-and-cross diagram for ionic bonding, electrons are transferred rather than shared.","mcqOptions":[{"text":"transferred","correct":true,"explanation":"During ionic bonding, one atom loses electrons and another gains them. The electrons are therefore transferred, producing oppositely charged ions that attract electrostatically."},{"text":"delocalised","correct":false,"explanation":"Delocalised electrons are associated with metallic bonding, where electrons move through a lattice. In ionic bonding, electrons are transferred from one atom to another."},{"text":"pooled","correct":false,"explanation":"Pooling electrons suggests that several atoms collectively share them, which is not ionic bonding. Ionic diagrams show electrons being transferred to form positive and negative ions."},{"text":"created","correct":false,"explanation":"Electrons are conserved during chemical bonding and are not created. In ionic bonding, existing outer-shell electrons are transferred from metal atoms to non-metal atoms."}]},{"id":"1d643da6-f32e-441a-88f0-9c8c3ee5ab11","cardType":"cloze","points":null,"front":"In a dot-and-cross diagram for ionic bonding, electrons are transferred rather than [ ].","back":"In a dot-and-cross diagram for ionic bonding, electrons are transferred rather than shared.","mcqOptions":[{"text":"shared","correct":true,"explanation":"Ionic bonding involves transfer of electrons from one atom to another, producing oppositely charged ions. Sharing electrons is characteristic of covalent bonding, not ionic bonding."},{"text":"lost equally","correct":false,"explanation":"Electrons are not lost equally by both atoms in ionic bonding. One atom transfers electrons to another, forming positive and negative ions; the correct term is “shared” for the contrast in the sentence."},{"text":"paired together","correct":false,"explanation":"Pairing electrons describes part of covalent bonding, where atoms share electron pairs. Ionic bonding instead involves electrons being transferred between atoms, so the correct word is “shared” in this comparison."},{"text":"rearranged randomly","correct":false,"explanation":"Ionic bonding does not involve random electron rearrangement. Electrons move from one atom to another to form oppositely charged ions, contrasting with electrons being “shared” in covalent bonding."}]},{"id":"6c3128d8-c1d1-4fbd-a46c-fa3c3193a455","cardType":"basic","points":1,"front":"Describe the structure of a giant ionic lattice.","back":"A regular repeating arrangement of many positive and negative ions.","mcqOptions":[{"text":"A regular repeating arrangement of many positive and negative ions.","correct":true,"explanation":"A giant ionic lattice is a regular three-dimensional arrangement in which positive and negative ions repeat in a fixed pattern, held together by strong electrostatic attractions."},{"text":"A random scattered arrangement of many positive and negative ions.","correct":false,"explanation":"The ions are not randomly scattered. They occupy a regular repeating structure because attractions between oppositely charged ions hold them in an ordered lattice."},{"text":"A single linear arrangement of many positive and negative ions.","correct":false,"explanation":"A giant ionic lattice is not a single line of ions. It extends throughout the solid in a regular three-dimensional repeating arrangement of positive and negative ions."},{"text":"A regular repeating arrangement of neutral atoms and molecules.","correct":false,"explanation":"Ionic lattices contain positive and negative ions rather than neutral atoms and molecules. The charged particles repeat regularly throughout the giant structure."}]},{"id":"b01b8af0-1c1b-491f-aedc-db3e1bf94c3d","cardType":"basic","points":3,"front":"Why do ionic compounds have high melting points?","back":"

Giant lattice with many ions
Strong electrostatic attractions in all directions
Large amount of energy needed to overcome attractions

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

Giant lattice with many ions
Strong electrostatic attractions in all directions
Large amount of energy needed to overcome attractions

","correct":true,"explanation":"A giant ionic lattice contains many oppositely charged ions. Strong electrostatic attractions act in all directions, so a large amount of energy is needed to separate the ions."},{"text":"

Giant lattice with many ions
Strong covalent bonds in all directions
Large amount of energy needed to overcome attractions

","correct":false,"explanation":"The lattice contains strong electrostatic attractions between oppositely charged ions, not covalent bonds. These attractions require a large amount of energy to overcome, giving ionic compounds high melting points."},{"text":"

Small lattice with few ions
Strong electrostatic attractions in all directions
Small amount of energy needed to overcome attractions

","correct":false,"explanation":"Ionic compounds have giant lattices containing many ions, so many attractions must be overcome. This requires a large amount of energy, not a small amount."},{"text":"

Giant lattice with many ions
Weak electrostatic attractions in one direction
Large amount of energy needed to overcome attractions

","correct":false,"explanation":"The attractions are strong and act in all directions throughout the lattice. Saying they are weak or limited to one direction underestimates the forces responsible for the high melting point."}]},{"id":"e2f2871d-f09c-47d8-8496-2cbb9135b6bd","cardType":"cloze","points":null,"front":"Melting an ionic compound provides enough energy for ions to [ ] from their fixed positions in the lattice.","back":"Melting an ionic compound provides enough energy for ions to move away from their fixed positions in the lattice.","mcqOptions":[{"text":"move away","correct":true,"explanation":"Heating supplies enough energy to overcome the attractions holding ions in their fixed lattice positions. The ions can then move away from those positions as the solid melts."},{"text":"gain electrons","correct":false,"explanation":"Melting changes the movement of the ions but does not usually change their charges by adding electrons. The energy allows the ions to “move away” from fixed lattice positions."},{"text":"form covalent bonds","correct":false,"explanation":"Melting an ionic compound does not convert its ions into covalently bonded particles. The lattice breaks down because ions gain enough energy to “move away” from fixed positions."},{"text":"become neutral","correct":false,"explanation":"The ions remain charged when an ionic compound melts. They become mobile because they can “move away” from their fixed positions, not because their charges disappear."}]},{"id":"63a96283-e062-49c5-a161-ce90b791313f","cardType":"cloze","points":null,"front":"Melting an ionic compound provides enough energy for ions to move away from their [ ] in the lattice.","back":"Melting an ionic compound provides enough energy for ions to move away from their fixed positions in the lattice.","mcqOptions":[{"text":"fixed positions","correct":true,"explanation":"In a solid ionic lattice, each ion is held in a fixed position by electrostatic attractions. Melting gives the ions enough energy to move away from these positions."},{"text":"nearest electrons","correct":false,"explanation":"Ions in a lattice do not move away from electrons as the key description of melting. They move away from their fixed positions when enough energy overcomes lattice attractions."},{"text":"opposite charges","correct":false,"explanation":"Opposite charges cause the attractions that hold the lattice together, but ions do not move away from their charges. They move away from their fixed positions when the compound melts."},{"text":"surrounding atoms","correct":false,"explanation":"The relevant change during melting is not movement away from surrounding atoms. Ions gain energy and leave their fixed positions in the lattice, becoming able to move around."}]},{"id":"eab13fef-3770-4d2c-8360-bc23689205f8","cardType":"basic","points":2,"front":"Why do solid ionic compounds not conduct electricity?","back":"Ions are fixed in the lattice and cannot move to carry charge.","mcqOptions":[{"text":"Ions are fixed in the lattice and cannot move to carry charge.","correct":true,"explanation":"A solid ionic lattice contains charged ions, but they are held in fixed positions and cannot move through the solid. Without mobile charge carriers, the solid cannot conduct electricity."},{"text":"Ions are neutral in the lattice and cannot move to carry charge.","correct":false,"explanation":"The particles in an ionic solid remain charged ions, not neutral particles. They cannot conduct because the ions are fixed in place and cannot move to carry charge."},{"text":"Ions are fixed in the lattice and can move freely to carry charge.","correct":false,"explanation":"The ions are fixed in the solid lattice, so they cannot move freely through the substance. Ionic compounds conduct only when their ions become mobile."},{"text":"Electrons are fixed in the lattice and cannot move to carry charge.","correct":false,"explanation":"Ionic solids conduct poorly because their ions, rather than delocalised electrons, are fixed in the lattice. The correct explanation identifies ions as unable to move and carry charge."}]},{"id":"b4fb1fc5-f09c-41d8-9178-b4b75c695b05","cardType":"basic","points":2,"front":"Under what two conditions can ionic compounds conduct electricity?","back":"

When molten (melted)
When aqueous (dissolved in water)

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

When molten (melted)
When aqueous (dissolved in water)

","correct":true,"explanation":"In a molten compound, the lattice has broken down and ions can move. In an aqueous solution, dissolved ions are also mobile, allowing both substances to conduct electricity."},{"text":"

When solid (crystallised)
When aqueous (dissolved in water)

","correct":false,"explanation":"A solid ionic compound has ions fixed in its lattice, so it cannot conduct. Conductivity occurs when the compound is molten or aqueous, allowing ions to move."},{"text":"

When molten (melted)
When gaseous (evaporated)

","correct":false,"explanation":"The molten condition is correct, but gaseous is not the expected condition for ionic compounds in this syllabus. The second condition is aqueous, when dissolved ions can move through water."},{"text":"

When aqueous (dissolved in water)
When solid (crystallised)

","correct":false,"explanation":"Aqueous ionic compounds conduct because their ions are mobile, but solid compounds do not conduct because their ions are fixed. The other conducting condition is molten."}]},{"id":"6af58027-7648-4d5c-afc6-58c3579611ff","cardType":"basic","points":2,"front":"Why does a molten ionic compound conduct electricity?","back":"The lattice breaks down and the ions are mobile (free to move).","mcqOptions":[{"text":"The lattice breaks down and the ions are mobile (free to move).","correct":true,"explanation":"Melting supplies enough energy to overcome the forces holding the ionic lattice together. The ions are then free to move and carry charge through the molten compound."},{"text":"The lattice remains intact and the ions are mobile (free to move).","correct":false,"explanation":"If the lattice remained intact, the ions would stay restricted to fixed positions. Melting allows conduction because the lattice breaks down and the ions become mobile."},{"text":"The lattice breaks down and the electrons are mobile (free to move).","correct":false,"explanation":"Ionic compounds conduct when their ions move, not because they contain mobile delocalised electrons. Melting breaks down the lattice and releases charged ions to move."},{"text":"The lattice breaks down and the ions are neutral (unable to move).","correct":false,"explanation":"The ions remain charged and become able to move when the lattice breaks down. Neutral, immobile particles could not carry electric charge through the molten compound."}]}]}],"examCountdown":{"examDate":"2027-05-19","paperLabel":"Paper 1"},"heading":"Ionic bonding","title":"Ionic bonding Flashcards","topbar":{"backHref":"/igcse/chemistry/edexcel/flashcards"},"topicSidebar":"$L36"}]}],"topicId":"96942975-da35-5c33-9fac-8fa4573c865d","walled":"$L37"}],"$L38","$L39"]