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23:[["$","$L32",null,{"feature":"flashcards"}],"$L33",["$","$L34",null,{"href":"/gcse/chemistry/aqa/flame-tests/flashcards","label":"8.3.1 Flame tests","subjectCode":"gcse_chemistry__aqa","surface":"flashcards"}],["$","$L35",null,{"runner":["$","div",null,{"className":"min-h-0 flex-1 overflow-hidden bg-background","children":["$","$L36",null,{"decks":[{"id":"56532d4c-2fea-4167-b3ec-f7e50267b458","title":"8.3.1 Flame tests Flashcards","topicId":"abd9cffe-daba-5f28-93d0-452d784f46ad","topicSlug":"flame-tests","cards":[{"id":"a2bef250-a482-490b-85f7-a04590ff7d07","cardType":"basic","points":1,"front":"What does a flame test identify?","back":"Certain metal ions, using the colour they give a Bunsen flame.","mcqOptions":[{"text":"Certain metal ions, using the colour they give a Bunsen flame.","correct":true,"explanation":"Heating certain metal ions excites their electrons. The characteristic colour emitted as the electrons return to lower energy levels can be used to identify the metal ion."},{"text":"Certain negative ions, using the colour they give a Bunsen flame.","correct":false,"explanation":"Flame colours are associated with positive metal ions, not negative ions. Certain metal ions can be identified because their excited electrons emit characteristic colours."},{"text":"All metal ions, using the colour they give a Bunsen flame.","correct":false,"explanation":"Not every metal ion produces a clear, distinctive flame colour. Flame tests identify only certain metal ions, while many metals, particularly transition metals, give unclear results."},{"text":"Certain non-metal atoms, using the colour they give a Bunsen flame.","correct":false,"explanation":"The test is not used to identify non-metal atoms. Its characteristic colours come from excited electrons in certain positive metal ions within the heated compound."}]},{"id":"7d6c9fea-9eb5-482c-b0a0-047a5bea201d","cardType":"basic","points":1,"front":"What produces the colour in a flame test?","back":"The metal ion in the compound.","mcqOptions":[{"text":"The metal ion in the compound.","correct":true,"explanation":"Energy from the flame excites electrons associated with the metal ion. When those electrons fall to lower energy levels, they emit the metal ion’s characteristic colour."},{"text":"The negative ion in the compound.","correct":false,"explanation":"Confusing the two ions in an ionic compound leads to this answer. The characteristic flame colour is produced by the metal ion, not the negative ion."},{"text":"The covalent molecule in the compound.","correct":false,"explanation":"Flame tests concern ionic compounds rather than a covalent molecule producing the diagnostic colour. The heated metal ion emits the characteristic colour used for identification."},{"text":"The Bunsen gas in the compound.","correct":false,"explanation":"The Bunsen gas supplies heat but is not part of the tested compound. The metal ion in the sample produces the characteristic flame colour."}]},{"id":"9ea5a4b6-700d-457b-b1f8-ac92c9903f05","cardType":"basic","points":1,"front":"What happens to a metal atom when it forms a metal ion?","back":"It loses one or more electrons.","mcqOptions":[{"text":"It loses one or more electrons.","correct":true,"explanation":"A metal atom forms a positive ion by losing one or more negatively charged electrons. Its nucleus remains unchanged during this ordinary chemical process."},{"text":"It gains one or more electrons.","correct":false,"explanation":"Gaining electrons forms a negative ion, which is typical of many non-metals. A metal atom forms its positive ion by losing one or more electrons."},{"text":"It loses one or more protons.","correct":false,"explanation":"Chemical ion formation changes the number of electrons, not the nucleus. A metal atom loses one or more electrons; losing protons would change the element itself."},{"text":"It shares one or more electrons.","correct":false,"explanation":"Sharing electrons describes covalent bonding rather than the formation of a metal ion. A metal atom becomes positively charged by losing one or more electrons."}]},{"id":"11bd603b-e201-4086-b87c-a562704b558c","cardType":"basic","points":2,"front":"Why do some metals give no clear flame-test colour?","back":"Many metals, including most transition metals, do not give a clear colour.","mcqOptions":[{"text":"Many metals, including most transition metals, do not give a clear colour.","correct":true,"explanation":"Many metals do not emit a sufficiently distinctive visible flame colour for identification. This limitation applies particularly to most transition metals."},{"text":"Many metals, including most alkali metals, do not give a clear colour.","correct":false,"explanation":"Alkali metals commonly produce strong characteristic colours, such as sodium’s yellow and potassium’s lilac. Most transition metals, rather than most alkali metals, give no clear colour."},{"text":"Many metals, including most group 2 metals, do not give a clear colour.","correct":false,"explanation":"Several group 2 ions give recognisable colours, including calcium’s orange-red flame. It is most transition metals that generally fail to produce a clear flame-test colour."},{"text":"Many metals, including most reactive metals, do not give a clear colour.","correct":false,"explanation":"Reactivity does not determine whether a clear flame colour appears; several very reactive metals produce distinctive colours. Most transition metals are the important group giving unclear results."}]},{"id":"94ca375a-59fd-45ff-a2ca-6ee8902f3ed9","cardType":"basic","points":1,"front":"What does a flame test identify - the metal ion or the negative ion?","back":"It identifies the metal ion, not the negative ion.","mcqOptions":[{"text":"It identifies the metal ion, not the negative ion.","correct":true,"explanation":"The observed colour comes from electronic transitions associated with the positive metal ion. The negative ion does not provide the characteristic flame-test identification."},{"text":"It identifies the negative ion, not the metal ion.","correct":false,"explanation":"This reverses the roles of the ions in the compound. A flame test identifies certain positive metal ions from their characteristic colours, not negative ions."},{"text":"It identifies the whole compound, not the metal ion.","correct":false,"explanation":"Different compounds containing the same metal ion can produce the same flame colour. The test identifies the metal ion rather than uniquely identifying the whole compound."},{"text":"It identifies the neutral atom, not the negative ion.","correct":false,"explanation":"The tested substance contains ions, and the diagnostic colour is attributed to its metal ion. The test is not described as identifying a neutral metal atom."}]},{"id":"1f81dd4c-e66a-4029-a42b-61ed47665f92","cardType":"cloze","points":null,"front":"A flame test identifies certain [ ] by the colour they give a Bunsen flame.","back":"A flame test identifies certain metal ions by the colour they give a Bunsen flame.","mcqOptions":[{"text":"metal ions","correct":true,"explanation":"Certain metal ions emit characteristic visible colours when heated in a Bunsen flame, allowing the ion in an unknown sample to be identified."},{"text":"negative ions","correct":false,"explanation":"Negative ions do not provide the diagnostic colours in this test. A flame test identifies certain metal ions through the characteristic light they emit when heated."},{"text":"non-metal atoms","correct":false,"explanation":"The test is not designed to identify non-metal atoms. Its characteristic colours are used to distinguish certain positive metal ions in compounds."},{"text":"covalent molecules","correct":false,"explanation":"Covalent molecules are not the species identified by standard flame tests. The observed characteristic colour is used to identify certain metal ions."}]},{"id":"045d7a11-5977-4df4-9d93-c4b9e5b63b8b","cardType":"basic","points":2,"front":"How should a nichrome wire be cleaned before testing?","back":"Dip it in dilute hydrochloric acid, then heat it until the flame has no colour.","mcqOptions":[{"text":"Dip it in dilute hydrochloric acid, then heat it until the flame has no colour.","correct":true,"explanation":"Dilute hydrochloric acid removes contaminating residues from the nichrome wire. Heating until no colour remains confirms that ions from a previous sample are no longer affecting the flame."},{"text":"Dip it in distilled water, then heat it until the flame has no colour.","correct":false,"explanation":"Distilled water may not remove stubborn ionic contamination from the wire. Dilute hydrochloric acid is used before heating until the flame shows no colour."},{"text":"Dip it in dilute nitric acid, then heat it until the flame has no colour.","correct":false,"explanation":"Substituting another laboratory acid is a common method error. The specified cleaning procedure uses dilute hydrochloric acid, followed by heating until the flame is colourless."},{"text":"Dip it in concentrated hydrochloric acid, then heat it until the flame has no colour.","correct":false,"explanation":"Using concentrated acid is unnecessary and more hazardous. The wire should be dipped in dilute hydrochloric acid and heated until it produces no flame colour."}]},{"id":"bfb2dc80-1a03-40e1-8431-1a2d6137b4cc","cardType":"basic","points":1,"front":"Where should the test wire be held in the Bunsen flame?","back":"At the edge of a roaring blue flame.","mcqOptions":[{"text":"At the edge of a roaring blue flame.","correct":true,"explanation":"The edge of a roaring blue flame provides strong heating without the yellow luminosity of incomplete combustion, so the sample’s characteristic colour can be seen clearly."},{"text":"At the edge of a yellow safety flame.","correct":false,"explanation":"A yellow safety flame can mask the sample colour with its own yellow light. The wire should be held at the edge of a roaring blue flame."},{"text":"At the centre of a flickering yellow flame.","correct":false,"explanation":"A flickering yellow flame is cooler and its yellow colour interferes with the observation. The correct position is at the edge of a roaring blue flame."},{"text":"At the base of a quiet orange flame.","correct":false,"explanation":"An orange flame indicates unsuitable combustion and may obscure the test colour. The sample wire belongs at the edge of a hot, roaring blue flame."}]},{"id":"0cdb7c9c-f979-4da1-9d1f-96239c6ba217","cardType":"basic","points":2,"front":"Why must the wire be cleaned between samples?","back":"To prevent a leftover ion producing a false colour.","mcqOptions":[{"text":"To prevent a leftover ion producing a false colour.","correct":true,"explanation":"An ion remaining from the previous sample could emit its own characteristic colour. Cleaning removes this contamination so the observed colour belongs to the current sample."},{"text":"To prevent a hot wire producing a false colour.","correct":false,"explanation":"The nichrome wire must be hot to heat the sample, so its temperature is not the contamination problem. Cleaning removes leftover ions that could produce a false colour."},{"text":"To prevent a blue flame producing a false colour.","correct":false,"explanation":"A roaring blue flame is deliberately used because it does not obscure the observation. The wire is cleaned to remove leftover ions that could create a false colour."},{"text":"To prevent a negative ion producing a false colour.","correct":false,"explanation":"The diagnostic contamination is a leftover metal ion from an earlier sample, not the sample’s negative ion. That metal ion could introduce its characteristic flame colour."}]},{"id":"3278b0b5-afd9-47de-808b-0ba4d4286d3d","cardType":"basic","points":1,"front":"What should be done after observing a flame colour?","back":"Record the colour and match it to known metal ions.","mcqOptions":[{"text":"Record the colour and match it to known metal ions.","correct":true,"explanation":"Recording the observed colour allows it to be compared with reference flame colours. A match can then indicate which known metal ion is present."},{"text":"Ignore the colour and match it to known metal ions.","correct":false,"explanation":"Ignoring the observation leaves no reliable result to compare. The flame colour must be recorded and then matched with the characteristic colours of known metal ions."},{"text":"Change the colour and match it to known metal ions.","correct":false,"explanation":"The observed colour is evidence and must not be altered. It should be recorded accurately before being compared with the colours produced by known metal ions."},{"text":"Heat the colour and match it to known metal ions.","correct":false,"explanation":"The sample is heated to produce the colour, but the colour itself cannot be heated. After observation, record it and compare it with known metal-ion colours."}]},{"id":"17c51992-1762-4342-a0ba-9538c5c3b4fd","cardType":"cloze","points":null,"front":"A yellow, dirty flame can [ ] of the sample.","back":"A yellow, dirty flame can hide the true colour of the sample.","mcqOptions":[{"text":"hide the true colour","correct":true,"explanation":"A luminous yellow flame produces strong background light that can overwhelm the sample’s characteristic emission, hiding its true flame-test colour and making identification unreliable."},{"text":"intensify the true colour","correct":false,"explanation":"The yellow light does not strengthen the sample’s characteristic colour; it competes with and masks it. A clean roaring blue flame is needed to reveal the true colour."},{"text":"identify the negative ion","correct":false,"explanation":"A flame test identifies certain metal ions rather than negative ions. A yellow, dirty flame merely masks the sample’s true colour and reduces the test’s reliability."},{"text":"remove the true colour","correct":false,"explanation":"The characteristic emission is still produced, but the dirty flame’s yellow light overwhelms the observation rather than removing it. It therefore hides the sample’s true colour."}]},{"id":"ff4ccd43-ff13-4ec8-a2fa-4af0d2dfa4f0","cardType":"basic","points":1,"front":"What colour does the lithium ion, $\\text{Li}^+$, produce?","back":"Crimson red.","mcqOptions":[{"text":"Crimson red.","correct":true,"explanation":"Lithium ions produce a characteristic crimson-red flame. This colour distinguishes lithium from calcium’s orange-red and sodium’s yellow in standard flame tests."},{"text":"Orange-red.","correct":false,"explanation":"Orange-red is the characteristic flame colour of calcium ions, a common confusion with lithium. Lithium ions produce a deeper crimson-red flame."},{"text":"Yellow.","correct":false,"explanation":"A strong yellow flame indicates sodium ions, not lithium ions. Lithium is identified by its characteristic crimson-red flame colour."},{"text":"Lilac.","correct":false,"explanation":"Lilac is the characteristic flame colour produced by potassium ions. Lithium ions instead produce a distinctive crimson-red flame."}]},{"id":"5fdd6bb6-7796-4cca-9556-5e7bc5e689a7","cardType":"basic","points":1,"front":"What colour does the sodium ion, $\\text{Na}^+$, produce?","back":"Yellow.","mcqOptions":[{"text":"Yellow.","correct":true,"explanation":"Sodium ions produce an intense characteristic yellow flame. The colour is strong enough that small traces of sodium contamination can mask other flame-test colours."},{"text":"Crimson red.","correct":false,"explanation":"Crimson red is the characteristic colour of lithium ions. Sodium ions produce a much more intense yellow flame in a flame test."},{"text":"Lilac.","correct":false,"explanation":"Lilac identifies potassium ions rather than sodium ions. The characteristic flame-test colour of sodium is a strong, easily observed yellow."},{"text":"Green.","correct":false,"explanation":"Green is associated with copper ions in GCSE flame tests. Sodium ions are identified by the intense yellow colour they produce."}]},{"id":"ffc2caf8-96ec-4469-be8f-e45457d1f7ac","cardType":"basic","points":1,"front":"What colour does the potassium ion, $\\text{K}^+$, produce?","back":"Lilac.","mcqOptions":[{"text":"Lilac.","correct":true,"explanation":"Potassium ions produce a characteristic lilac flame. This pale purple colour distinguishes potassium from sodium’s yellow and lithium’s crimson red."},{"text":"Yellow.","correct":false,"explanation":"Yellow is the characteristic flame colour of sodium ions and can easily mask weaker colours. Potassium ions instead produce a lilac flame."},{"text":"Crimson red.","correct":false,"explanation":"Crimson red identifies lithium ions, not potassium ions. Potassium produces the pale purple colour described as lilac in a flame test."},{"text":"Orange-red.","correct":false,"explanation":"Orange-red is produced by calcium ions in a flame test. Potassium ions give the distinctly different pale purple colour called lilac."}]},{"id":"43e003b9-010a-477e-bdb2-2b7b25038579","cardType":"basic","points":1,"front":"What colour does the calcium ion, $\\text{Ca}^{2+}$, produce?","back":"Orange-red.","mcqOptions":[{"text":"Orange-red.","correct":true,"explanation":"Calcium ions produce a characteristic orange-red flame. Careful description distinguishes this colour from lithium’s deeper crimson-red flame."},{"text":"Crimson red.","correct":false,"explanation":"Crimson red is produced by lithium ions and is easily confused with calcium’s result. Calcium ions give an orange-red flame instead."},{"text":"Yellow.","correct":false,"explanation":"Yellow is the characteristic flame colour of sodium ions, not calcium ions. Calcium produces a less yellow, orange-red flame."},{"text":"Green.","correct":false,"explanation":"Green is the characteristic GCSE flame-test colour for copper ions. Calcium ions are identified by the orange-red colour they produce."}]},{"id":"cefdccd7-0618-4997-9e9f-0c5097b96dd1","cardType":"basic","points":1,"front":"What colour does the copper ion, $\\text{Cu}^{2+}$, produce?","back":"Green.","mcqOptions":[{"text":"Green.","correct":true,"explanation":"Copper ions produce a characteristic green flame in the GCSE flame test. This clearly differs from the red, yellow and lilac colours of the other listed ions."},{"text":"Lilac.","correct":false,"explanation":"Lilac is the characteristic flame colour of potassium ions. Copper ions produce a green flame under the standard GCSE flame-test conditions."},{"text":"Yellow.","correct":false,"explanation":"Yellow identifies sodium ions and may dominate when sodium contamination is present. A clean sample containing copper ions produces a green flame."},{"text":"Orange-red.","correct":false,"explanation":"Orange-red is the characteristic flame colour produced by calcium ions. Copper ions are distinguished by the green colour they give the flame."}]},{"id":"b619b90b-3d57-4267-a65c-fca207cc098d","cardType":"cloze","points":null,"front":"The flame colour of the potassium ion, $\\text{K}^+$, is [ ].","back":"The flame colour of the potassium ion, $\\text{K}^+$, is lilac.","mcqOptions":[{"text":"lilac","correct":true,"explanation":"Potassium ions produce a lilac flame when heated, although sodium contamination can be intense enough to obscure this colour in a mixture."},{"text":"yellow","correct":false,"explanation":"Yellow is the characteristic flame colour of sodium, not potassium. Potassium ions give a lilac flame, so confusing these two common flame tests leads to this choice."},{"text":"green","correct":false,"explanation":"Green is associated with ions such as copper(II), rather than potassium. The correct observation for potassium ions is a lilac flame colour."},{"text":"brick-red","correct":false,"explanation":"Brick-red is produced by calcium ions, not potassium ions. Potassium is identified by its lilac flame, provided a stronger colour does not mask it."}]},{"id":"9f7f50da-7341-4381-a65b-5778c2c17d83","cardType":"basic","points":2,"front":"Why can a flame test fail to detect a metal ion in a mixture?","back":"A stronger flame colour can hide a weaker one.","mcqOptions":[{"text":"A stronger flame colour can hide a weaker one.","correct":true,"explanation":"In a mixture, the more intense flame emission dominates what is seen, so it can conceal the weaker colour and prevent that metal ion from being detected."},{"text":"A weaker flame colour can hide a stronger one.","correct":false,"explanation":"A weaker emission cannot normally conceal a more intense one. The stronger flame colour is what masks the weaker result, making the hidden ion difficult to detect."},{"text":"The metal ions react together and produce no flame colour.","correct":false,"explanation":"The ions do not generally cancel each other’s flame emissions by reacting together. A stronger observed flame colour can instead mask a weaker one."},{"text":"The sample becomes too hot and burns without producing light.","correct":false,"explanation":"Heating excites electrons and causes the characteristic light emission; excessive heat is not the usual reason for a missed result. Masking occurs when another colour is stronger."}]},{"id":"4e94795e-7165-44d2-8a9f-13326c339775","cardType":"basic","points":2,"front":"Which ion most easily masks other flame colours?","back":"The sodium ion, because its yellow colour is strong.","mcqOptions":[{"text":"The sodium ion, because its yellow colour is strong.","correct":true,"explanation":"Sodium ions produce an especially intense yellow flame, so even a small amount of sodium can dominate the observation and obscure colours from other ions."},{"text":"The potassium ion, because its lilac colour is strong.","correct":false,"explanation":"Potassium gives a lilac flame, but this colour is relatively easily obscured. Sodium is the ion most likely to mask other flame colours because its yellow emission is intense."},{"text":"The calcium ion, because its red colour is strong.","correct":false,"explanation":"Calcium produces a brick-red flame, but it is not usually the strongest interfering colour. Sodium’s intense yellow flame is the common cause of masking."},{"text":"The copper(II) ion, because its green colour is strong.","correct":false,"explanation":"Copper(II) ions can produce a green or blue-green flame, but sodium is the principal masking ion because its yellow flame is particularly intense."}]},{"id":"f9d463d0-5dd8-435a-9672-440069673da5","cardType":"cloze","points":null,"front":"A flame test result can be masked when a sample contains a mixture of ions and a [ ] hides a weaker one.","back":"A flame test result can be masked when a sample contains a mixture of ions and a strong colour hides a weaker one.","mcqOptions":[{"text":"strong colour","correct":true,"explanation":"A strong colour produces the most visible flame emission, allowing it to dominate the observation and hide the weaker colour from another ion in the mixture."},{"text":"weak colour","correct":false,"explanation":"A weak colour is the one likely to be hidden, not the one doing the masking. The sentence should refer to a strong colour hiding a weaker one."},{"text":"pale colour","correct":false,"explanation":"A pale colour has relatively low intensity and would be less able to obscure another result. A strong colour is needed to mask a weaker flame colour."},{"text":"different colour","correct":false,"explanation":"Simply being different does not make a flame colour dominant. The important property is intensity: a strong colour can hide a weaker one in the mixture."}]}]}],"examCountdown":{"examDate":"2027-05-17","paperLabel":"Paper 1"},"heading":"8.3.1 Flame tests","title":"8.3.1 Flame tests Flashcards","topbar":{"backHref":"/gcse/chemistry/aqa/flashcards"},"topicSidebar":"$L37"}]}],"topicId":"abd9cffe-daba-5f28-93d0-452d784f46ad","walled":"$L38"}],"$L39","$L3a"]