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What particles it contains
How those particles are bonded
How the particles are arranged

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

What particles it contains
How those particles are bonded
How the particles are arranged

","correct":true,"explanation":"Bulk properties depend on which particles make up a material, the bonding between those particles, and their arrangement. These features determine how the material behaves on a large scale."},{"text":"

The size of its particles
The colour of the material
The material’s temperature

","correct":false,"explanation":"Particle size, colour and temperature can affect some observations, but they are not the three fundamental factors used to explain bulk properties. The correct factors are particles, bonding and arrangement."},{"text":"

How many particles it contains
How quickly particles are moving
How much space it occupies

","correct":false,"explanation":"These describe some physical conditions rather than the underlying structure. Bulk properties are determined by the particles present, how they are bonded and how they are arranged."},{"text":"

Its mass
Its volume
Its density

","correct":false,"explanation":"Mass, volume and density are measurable properties, not the structural factors that determine a material’s bulk behaviour. The relevant factors are particle type, bonding and arrangement."}]},{"id":"af2fb6eb-3cd0-41a1-b7c8-d56bac69862e","cardType":"basic","points":2,"front":"Why can carbon form a vast range of different organic compounds?","back":"

Forms four covalent bonds
Can bond to other carbon atoms in chains or rings

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

Forms four covalent bonds
Can bond to other carbon atoms in chains or rings

","correct":true,"explanation":"Carbon has four outer-shell electrons available for bonding and can form four covalent bonds. Carbon atoms can also join into chains or rings, producing many different structures."},{"text":"

Forms six covalent bonds
Can bond to other carbon atoms in chains or rings

","correct":false,"explanation":"Carbon does not usually form six covalent bonds. Its ability to form four bonds, together with carbon-carbon chains and rings, explains the huge variety of organic compounds."},{"text":"

Forms two covalent bonds
Can bond to other carbon atoms in chains or rings

","correct":false,"explanation":"Carbon-carbon double bonds can occur, but they are not the main reason for the range of compounds. The key points are four covalent bonds and chains or rings of carbon atoms."},{"text":"

Forms four ionic bonds
Can bond to other carbon atoms in straight lines only

","correct":false,"explanation":"Carbon can form bonds with many elements, but this statement omits its four-bond capacity and incorrectly limits its structures. Chains and rings are central to organic diversity."}]},{"id":"53e52b86-4629-4754-8d6d-20f18d4ee24b","cardType":"cloze","points":null,"front":"A [ ] is a strong chemical bond formed when two atoms share a pair of electrons.","back":"A covalent bond is a strong chemical bond formed when two atoms share a pair of electrons.","mcqOptions":[{"text":"covalent bond","correct":true,"explanation":"A covalent bond forms when two atoms share a pair of electrons. This sharing gives the atoms a more stable outer electron arrangement."},{"text":"ionic bond","correct":false,"explanation":"An ionic bond forms through electron transfer and electrostatic attraction between oppositely charged ions, not by sharing an electron pair. Sharing a pair describes a covalent bond."},{"text":"metallic bond","correct":false,"explanation":"A metallic bond is the attraction between positive metal ions and delocalised electrons in a metal lattice. It does not describe two atoms sharing one electron pair."},{"text":"hydrogen bond","correct":false,"explanation":"A hydrogen bond is an intermolecular attraction involving hydrogen and electronegative atoms, rather than the strong shared-electron bond within a molecule. The correct term is covalent bond."}]},{"id":"f885ed36-4bf1-4f92-ade9-2dc90dd58bfb","cardType":"cloze","points":null,"front":"An [ ] is a different structural form of the same element where atoms are arranged and bonded differently.","back":"An allotrope is a different structural form of the same element where atoms are arranged and bonded differently.","mcqOptions":[{"text":"allotrope","correct":true,"explanation":"An allotrope is one of several structural forms of the same element. Different arrangements and bonding can give allotropes different physical properties."},{"text":"isotope","correct":false,"explanation":"An isotope is an atom of the same element with a different number of neutrons. Isotopes differ in mass, not because their atoms have different structural arrangements and bonding."},{"text":"compound","correct":false,"explanation":"A compound contains atoms of two or more different elements chemically bonded together. A different structure of one element is called an allotrope."},{"text":"polymer","correct":false,"explanation":"A polymer is a substance made from many repeating monomer units. It is not the general term for a different structural form of the same element."}]},{"id":"17b6daaa-c757-4a74-adc9-53fe0ab7abca","cardType":"basic","points":3,"front":"Why does diamond have a very high melting point?","back":"

Giant covalent structure
Each atom forms four strong covalent bonds
Requires large energy to break bonds

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

Giant covalent structure
Each atom forms four strong covalent bonds
Requires large energy to break bonds

","correct":true,"explanation":"Diamond has a giant covalent structure in which every carbon atom forms four strong covalent bonds. A large amount of energy is therefore needed to break the network."},{"text":"

Simple molecular structure
Each molecule has weak intermolecular forces
Requires small energy to separate molecules

","correct":false,"explanation":"Diamond is not made of separate molecules held by weak forces. Its giant covalent network contains many strong bonds, so melting requires a large energy input."},{"text":"

Metallic structure
Each atom forms metallic bonds
Requires large energy to move electrons

","correct":false,"explanation":"Diamond does not have metallic bonding or mobile electrons. Its high melting point comes from four strong covalent bonds per carbon atom throughout a giant network."},{"text":"

Layered molecular structure
Each atom forms three weak bonds
Requires small energy to separate layers

","correct":false,"explanation":"The strength of diamond is not caused by weak forces between layers; that feature belongs to graphite. Diamond has a three-dimensional giant covalent network with four bonds per atom."}]},{"id":"bb9d8c19-4635-406f-8bb7-1b22673e00f4","cardType":"basic","points":2,"front":"Why is graphite used as a lubricant?","back":"

Weak forces between layers
Layers can slide over each other

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

Weak forces between layers
Layers can slide over each other

","correct":true,"explanation":"Graphite consists of layers with weak forces between them. The layers can slide over one another easily, reducing friction and allowing graphite to act as a lubricant."},{"text":"

Strong forces between layers
Layers can slide over each other

","correct":false,"explanation":"Strong forces between layers would prevent them sliding freely and increase friction. Graphite lubricates because weak forces allow its layers to move over one another."},{"text":"

Metallic bonds between layers
Layers can slide over each other

","correct":false,"explanation":"Graphite’s layers are not held together by metallic bonds. Weak intermolecular forces between the layers allow sliding, which produces the lubricating effect."},{"text":"

Weak forces within layers
Layers cannot slide over each other

","correct":false,"explanation":"If the layers were fixed rigidly, they could not slide and graphite would not reduce friction effectively. The relevant property is weak attraction between adjacent layers."}]},{"id":"96476515-c8f9-44ec-b68f-bcfb4a7417d7","cardType":"basic","points":3,"front":"Explain why graphite conducts electricity but diamond does not.","back":"

Graphite has delocalised electrons (3 bonds per atom)
Diamond has no free electrons (4 bonds per atom)
In graphite, electrons are free to move and carry charge

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

Graphite has delocalised electrons (3 bonds per atom)
Diamond has no free electrons (4 bonds per atom)
In graphite, electrons are free to move and carry charge

","correct":true,"explanation":"Each graphite carbon forms three covalent bonds, leaving one delocalised electron per atom. These electrons move through the structure and carry electrical charge, unlike in diamond."},{"text":"

Graphite has no free electrons (4 bonds per atom)
Diamond has delocalised electrons (3 bonds per atom)
In diamond, electrons are free to move and carry charge

","correct":false,"explanation":"Diamond’s electrons are not delocalised because each carbon forms four covalent bonds. Graphite conducts through its one delocalised electron per carbon atom."},{"text":"

Graphite has localised electrons (4 bonds per atom)
Diamond has no free electrons (3 bonds per atom)
In graphite, electrons are fixed in place and cannot carry charge

","correct":false,"explanation":"Both materials contain covalent bonds, but graphite has three bonds per carbon and one mobile electron. Diamond has four bonds per carbon, leaving no free electrons to carry charge."},{"text":"

Graphite has delocalised electrons (3 bonds per atom)
Diamond has no free electrons (4 bonds per atom)
In graphite, layers are free to slide and carry charge

","correct":false,"explanation":"The layers sliding explains graphite’s lubricating property, not its electrical conductivity. Conductivity comes from graphite’s delocalised electrons, which diamond lacks because of its four bonds per atom."}]},{"id":"d53042f4-ee24-47d8-a283-41b11cfc4169","cardType":"basic","points":1,"front":"What is the structure of graphene?","back":"A single layer of graphite (one atom thick).","mcqOptions":[{"text":"A single layer of graphite (one atom thick).","correct":true,"explanation":"Graphene is one atom thick: it is a single layer of graphite. Its carbon atoms form a giant covalent sheet with useful strength and electrical conductivity."},{"text":"Several layers of graphite (many atoms thick).","correct":false,"explanation":"Several layers of graphite form a thicker graphite structure, not graphene. Graphene specifically consists of just one atom-thick layer."},{"text":"A single layer of diamond (one atom thick).","correct":false,"explanation":"A single layer of diamond would not be graphene because diamond has a three-dimensional bonding arrangement. Graphene is a one-atom-thick graphite layer."},{"text":"A molecular layer of carbon (one atom thick).","correct":false,"explanation":"Graphene is not a molecular carbon sheet made of separate molecules. Its carbon atoms are covalently bonded in one continuous layer of graphite."}]},{"id":"642e92ce-78f9-4e5c-98fc-2e131c143b6c","cardType":"cloze","points":null,"front":"[ ] are carbon molecules arranged in hollow shapes like spheres or tubes.","back":"Fullerenes are carbon molecules arranged in hollow shapes like spheres or tubes.","mcqOptions":[{"text":"Fullerenes","correct":true,"explanation":"Fullerenes are allotropes of carbon whose atoms form hollow molecular structures, including spherical buckyballs and cylindrical carbon nanotubes."},{"text":"Alkanes","correct":false,"explanation":"Alkanes are hydrocarbons containing only single carbon-carbon bonds; they are not defined by hollow structures. The carbon molecules forming hollow spheres or tubes are fullerenes."},{"text":"Carbonates","correct":false,"explanation":"Carbonates are compounds containing the carbonate ion, $CO_3^{2-}$, rather than hollow carbon molecules. Fullerenes are the carbon structures described."},{"text":"Polymers","correct":false,"explanation":"Polymers are long-chain molecules made from repeating monomers, not carbon molecules specifically defined by hollow shapes. Such hollow carbon structures are fullerenes."}]},{"id":"1ac4ffae-faaa-4942-aa14-79107fdcadf7","cardType":"basic","points":2,"front":"Why do ionic compounds have high melting points?","back":"Strong electrostatic forces of attraction between ions in a giant lattice require high energy to overcome.","mcqOptions":[{"text":"Strong electrostatic forces of attraction between ions in a giant lattice require high energy to overcome.","correct":true,"explanation":"Oppositely charged ions experience strong electrostatic attraction throughout the giant ionic lattice. A large amount of thermal energy is therefore needed to separate them during melting."},{"text":"Strong covalent bonds between ions in a giant lattice require high energy to overcome.","correct":false,"explanation":"Ionic lattices are held together by electrostatic attraction, not covalent bonds. Their high melting points result from the large energy needed to overcome strong attractions between oppositely charged ions."},{"text":"Strong magnetic forces of attraction between ions in a giant lattice require high energy to overcome.","correct":false,"explanation":"Magnetic forces are not responsible for bonding in ionic compounds. Strong electrostatic forces between oppositely charged ions extend throughout the giant lattice and require substantial energy to overcome."},{"text":"Strong electrostatic forces of attraction between molecules in a simple structure require high energy to overcome.","correct":false,"explanation":"Ionic compounds do not consist of separate molecules. Their ions form a giant lattice held by strong electrostatic attractions, which require considerable energy to overcome."}]},{"id":"4b7e6ea4-bfa6-4438-ba48-591182992720","cardType":"basic","points":2,"front":"Why do ionic compounds conduct electricity when molten but not when solid?","back":"

Solid: ions are fixed in a lattice
Molten: ions are free to move and carry charge

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

Solid: ions are fixed in a lattice
Molten: ions are free to move and carry charge

","correct":true,"explanation":"In a solid ionic lattice, the charged ions cannot change position. Melting releases them from fixed positions, allowing them to move and transport electrical charge."},{"text":"

Solid: ions are free to move in a lattice
Molten: ions are fixed in place and cannot carry charge

","correct":false,"explanation":"This reverses the states: ions are fixed in place in the solid but become mobile when molten. Only the molten compound therefore has moving charged particles that can conduct."},{"text":"

Solid: electrons are fixed in a lattice
Molten: electrons are free to move and carry charge

","correct":false,"explanation":"Ionic conduction is caused by moving ions, not delocalised electrons. The ions are fixed in a solid lattice but become free to move when the compound melts."},{"text":"

Solid: molecules are fixed in a lattice
Molten: molecules are free to move and carry charge

","correct":false,"explanation":"Ionic compounds contain charged ions rather than neutral molecules. Their solid ions are fixed, whereas their molten ions can move through the liquid and carry charge."}]},{"id":"42c6104a-09e2-4ff7-b8ee-d23ff3de3f5c","cardType":"basic","points":2,"front":"Why do simple molecular substances like $CO_2$ have low boiling points?","back":"Only weak intermolecular forces between molecules must be overcome, which requires little energy.","mcqOptions":[{"text":"Only weak intermolecular forces between molecules must be overcome, which requires little energy.","correct":true,"explanation":"Boiling separates intact molecules, so only the weak attractions between different molecules are overcome. Little energy is needed, giving simple molecular substances low boiling points."},{"text":"Only strong covalent bonds within molecules must be overcome, which requires little energy.","correct":false,"explanation":"The covalent bonds within $CO_2$ molecules are strong, but they are not broken during boiling. Only weak intermolecular forces are overcome, so little energy is required."},{"text":"Only strong intermolecular forces between molecules must be overcome, which requires little energy.","correct":false,"explanation":"Simple molecular substances have weak, not strong, intermolecular attractions. Because these weak forces require little energy to overcome, substances such as $CO_2$ have low boiling points."},{"text":"Only weak ionic bonds between molecules must be overcome, which requires little energy.","correct":false,"explanation":"Ionic bonds occur between oppositely charged ions and are not present between $CO_2$ molecules. Its low boiling point results from weak intermolecular forces requiring little energy to overcome."}]},{"id":"43382f03-0fa3-4e07-adf4-fe5e51022bd4","cardType":"cloze","points":null,"front":"When a simple molecular substance melts, the [ ] within the molecules are not broken.","back":"When a simple molecular substance melts, the covalent bonds within the molecules are not broken.","mcqOptions":[{"text":"covalent bonds","correct":true,"explanation":"Melting separates or rearranges whole molecules by overcoming intermolecular forces. The strong covalent bonds holding the atoms together within each molecule remain intact."},{"text":"intermolecular forces","correct":false,"explanation":"Intermolecular forces act between separate molecules and are overcome during melting, so they do not remain intact. The covalent bonds within each molecule are not broken."},{"text":"ionic bonds","correct":false,"explanation":"Simple molecular substances do not contain ionic bonds between their atoms. Their atoms are joined by covalent bonds, which remain unbroken when the substance melts."},{"text":"metallic bonds","correct":false,"explanation":"Metallic bonds occur in giant metallic structures, not within simple molecules. The bonds inside simple molecules are covalent and are not broken during melting."}]},{"id":"9ef01f65-847f-494d-8ef8-1eb5529d74ab","cardType":"basic","points":2,"front":"How do metals conduct electricity?","back":"Delocalised electrons are free to move through the giant metallic structure and carry charge.","mcqOptions":[{"text":"Delocalised electrons are free to move through the giant metallic structure and carry charge.","correct":true,"explanation":"Metals contain delocalised electrons that are not attached to one particular atom. These mobile negatively charged particles move through the structure and carry electrical charge."},{"text":"Positive metal ions are free to move through the giant metallic structure and carry charge.","correct":false,"explanation":"The positive metal ions vibrate but remain in fixed lattice positions in a solid metal. Electrical conduction occurs because delocalised electrons move through the structure."},{"text":"Localised electrons are free to move through the giant metallic structure and carry charge.","correct":false,"explanation":"Localised electrons are bound to particular atoms or bonds and cannot travel through the metal. Metals conduct because their delocalised electrons are mobile charge carriers."},{"text":"Delocalised protons are free to move through the giant metallic structure and carry charge.","correct":false,"explanation":"Protons remain inside atomic nuclei and do not move through a metallic lattice. The mobile charged particles responsible for conduction are delocalised electrons."}]},{"id":"fd9e600b-6515-442f-b627-6cf1723424a7","cardType":"basic","points":1,"front":"A substance is at $25^{\\circ}C$. Its melting point is $-10^{\\circ}C$ and its boiling point is $50^{\\circ}C$. What is its state?","back":"Liquid","mcqOptions":[{"text":"Liquid","correct":true,"explanation":"The temperature, $25^{\\circ}C$, is above the melting point but below the boiling point. The substance has therefore melted but has not boiled, so it is liquid."},{"text":"Solid","correct":false,"explanation":"A substance is solid only below its melting point. Since $25^{\\circ}C$ is higher than $-10^{\\circ}C$ but lower than the boiling point, the substance is liquid."},{"text":"Gas","correct":false,"explanation":"A substance becomes a gas only at or above its boiling point. Since $25^{\\circ}C$ is below $50^{\\circ}C$ and above the melting point, it is liquid."},{"text":"Solid and liquid","correct":false,"explanation":"At a temperature strictly between its melting and boiling points, a pure substance is in one phase rather than a solid-liquid mixture. Its state is liquid."}]},{"id":"ecde6d41-dcbb-4039-9b72-2152e20c57ed","cardType":"cloze","points":null,"front":"A nanometre ($nm$) is equivalent to $\\text{[...]}$.","back":"A nanometre ($nm$) is equivalent to $\\boxed{1 \\times 10^{-9} \\text{ m}}$.","mcqOptions":[{"text":"$$1 \\times 10^{-9} \\text{ m}$","correct":true,"explanation":"The SI prefix nano- means one billionth, so one nanometre equals $0.000000001$ metres, written in standard form as $1 \\times 10^{-9} \\text{ m}$."},{"text":"$$1 \\times 10^{-6} \\text{ m}$","correct":false,"explanation":"The exponent $-6$ corresponds to the prefix micro-, so this value is one micrometre. Nano- means one billionth: $1 \\times 10^{-9} \\text{ m}$."},{"text":"$$1 \\times 10^{-3} \\text{ m}$","correct":false,"explanation":"The exponent $-3$ corresponds to the prefix milli-, making this one millimetre rather than one nanometre. A nanometre is $1 \\times 10^{-9} \\text{ m}$."},{"text":"$$1 \\times 10^{9} \\text{ m}$","correct":false,"explanation":"A positive exponent makes this one billion metres, reversing the direction of the conversion. Nano- denotes one billionth of a metre, or $1 \\times 10^{-9} \\text{ m}$."}]},{"id":"86e07164-b3b5-485e-b995-a1ac736aec12","cardType":"basic","points":1,"front":"What is the typical diameter range of a nanoparticle?","back":"Between $1 \\text{ nm}$ and $100 \\text{ nm}$.","mcqOptions":[{"text":"Between $1 \\text{ nm}$ and $100 \\text{ nm}$.","correct":true,"explanation":"Nanoparticles are defined as particles with diameters from $1 \\text{ nm}$ to $100 \\text{ nm}$. Below this range, dimensions approach the scale of individual atoms."},{"text":"Between $0.01 \\text{ nm}$ and $1 \\text{ nm}$.","correct":false,"explanation":"This range is mainly below the accepted nanoparticle scale and approaches atomic dimensions. Nanoparticles typically have diameters between $1 \\text{ nm}$ and $100 \\text{ nm}$."},{"text":"Between $1 \\text{ nm}$ and $1000 \\text{ nm}$.","correct":false,"explanation":"Extending the upper limit to $1000 \\text{ nm}$ includes particles larger than the nanoparticle definition. The accepted diameter range is $1 \\text{ nm}$ to $100 \\text{ nm}$."},{"text":"Between $100 \\text{ nm}$ and $10{,}000 \\text{ nm}$.","correct":false,"explanation":"This shifts the entire range above the usual nanoparticle scale. A nanoparticle has a typical diameter between $1 \\text{ nm}$ and $100 \\text{ nm}$."}]},{"id":"c642007b-035b-4eba-912c-dc9a672c056d","cardType":"basic","points":1,"front":"How does the surface area to volume ratio change as particle size decreases?","back":"The ratio increases (becomes larger).","mcqOptions":[{"text":"The ratio increases (becomes larger).","correct":true,"explanation":"Reducing particle size exposes more surface area relative to the amount of material inside. Therefore, the surface area to volume ratio becomes larger."},{"text":"The ratio decreases (becomes smaller).","correct":false,"explanation":"This reverses the relationship between size and surface area to volume ratio. As particles become smaller, the ratio increases because proportionally more material is exposed at the surface."},{"text":"The ratio stays constant (does not change).","correct":false,"explanation":"The ratio is not independent of particle size. For similarly shaped particles, surface area to volume ratio increases as their characteristic length decreases."},{"text":"The ratio first decreases (then becomes constant).","correct":false,"explanation":"There is no initial decrease or fixed lower-size threshold in this geometric relationship. As particle size decreases, surface area to volume ratio consistently increases."}]},{"id":"b23d84c1-afd0-43b0-88af-6a685438c2ea","cardType":"basic","points":1,"front":"Why are nanoparticle catalysts often more effective than bulk material catalysts?","back":"They have a high surface area to volume ratio, providing more sites for reactions to occur.","mcqOptions":[{"text":"They have a high surface area to volume ratio, providing more sites for reactions to occur.","correct":true,"explanation":"A high surface area to volume ratio exposes more catalyst particles to reactants. This supplies more active sites, increasing the frequency of successful reactions."},{"text":"They have a low surface area to volume ratio, providing more sites for reactions to occur.","correct":false,"explanation":"A low surface area to volume ratio would expose fewer active sites and reduce effectiveness. Nanoparticles are effective because their surface area to volume ratio is high."},{"text":"They have a larger particle diameter than bulk material, providing more sites for reactions to occur.","correct":false,"explanation":"Nanoparticles are much smaller than pieces of bulk material, not larger. Their small diameter produces a high surface area to volume ratio and more exposed reaction sites."},{"text":"They have a higher activation energy for reactions, causing reactions to occur more quickly.","correct":false,"explanation":"A higher activation energy would make successful reactions less frequent, not more frequent. Nanoparticles improve effectiveness by exposing more catalytic sites through their high surface area to volume ratio."}]},{"id":"a41cff7e-8038-45dc-a3da-8d39d57b08d6","cardType":"basic","points":2,"front":"Give two potential risks of nanoparticles in the human body.","back":"

May enter cells or the bloodstream
Could damage organs or cause inflammation

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

May enter cells or the bloodstream
Could damage organs or cause inflammation

","correct":true,"explanation":"Their extremely small size may allow nanoparticles to cross biological barriers and enter cells or blood. Their effects are uncertain, but possible organ damage and inflammation are concerns."},{"text":"

May make blood radioactive inside the body
Could emit gamma rays or cause radiation sickness

","correct":false,"explanation":"Nanoparticles are not necessarily radioactive and do not inherently emit ionising radiation. Genuine concerns include their ability to enter cells or blood and potentially damage organs or cause inflammation."},{"text":"

May reproduce inside cells or the bloodstream
Could cause viral infections or spread between people

","correct":false,"explanation":"This confuses nanoparticles with living pathogens. Nanoparticles cannot reproduce or cause viral infections, but they may enter cells or the bloodstream and potentially harm organs."},{"text":"

May melt inside cells or the bloodstream
Could boil the blood or burn internal organs

","correct":false,"explanation":"Nanoparticles do not normally melt at body temperature or boil blood. The realistic concerns are that they may cross into cells or blood and cause inflammation or organ damage."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"Properties of materials","title":"Properties of materials Flashcards","topbar":{"backHref":"/gcse/chemistry/ocr/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"c8d97e88-4736-5823-b5c0-120786429f82","walled":"$L38"}],"$L39","$L3a"]