| A method used to identify metal ions by observing the characteristic color produced in a flame. | Flame Test |
| What is the purpose of a flame test in chemistry? | To identify metal ions based on the colors they emit in a flame. |
| A wire made of nickel-chromium alloy, often used in flame tests to hold samples. | Nichrome Wire |
| Why is a nichrome wire used in flame tests? | It allows for the easy attachment and observation of the sample in the flame. |
| A common laboratory device producing a single open flame, used for various applications including flame tests. | Bunsen Burner |
| How is a flame test conducted? | By dipping a nichrome wire into the unknown compound and placing it in the flame of a Bunsen burner. |
| The distinctive colors emitted by metal ions during a flame test. | Colors in Flame Tests |
| Which metal ions can be identified using a flame test? | Lithium, sodium, potassium, calcium, and copper ions. |
| The requirement that the test for any ion must produce a unique result. | Unique Test for Ions |
| Why must the flame test for ions be unique? | To accurately identify and distinguish different ions. |
| The challenge of identifying mixtures of ions in a flame test. | Difficulty in Detecting Mixtures |
| Why is it difficult to detect mixtures of ions in a flame test? | Some colors may be masked by others, leading to ambiguity in the results. |
| The phenomenon where the color produced by one ion conceals or alters the color of another ion in a mixture. | Masking Effect |
| What is the masking effect in flame tests? | It occurs when the colors of different ions in a mixture interfere with each other, making identification challenging. |
| The process of determining the metal ions present in a compound using flame tests. | Identifying Metal Compounds |
| What information can be obtained by identifying metal ions in a compound through flame tests? | Insights into the composition and nature of the compound. |
| A method used to identify metal ions by observing the formation of precipitates when reacting with sodium hydroxide. | Sodium Hydroxide Test |
| How is the sodium hydroxide test used to identify metal ions? | By observing the formation of precipitates, which are characteristic of specific metal ions. |
| A solid formed during a chemical reaction in a solution. | Precipitate |
| What is a precipitate in the context of metal ion testing with sodium hydroxide? | It is a solid formed when a metal ion reacts with sodium hydroxide. |
| The compound formed when a metal reacts with hydroxide ions. | Metal Hydroxide |
| What is the significance of metal hydroxides in the sodium hydroxide test? | They are formed as precipitates and aid in identifying specific metal ions. |
| The reaction where iron(II) forms a green precipitate when treated with sodium hydroxide. | Iron(II) and Sodium Hydroxide |
| What color precipitate is formed when iron(II) reacts with sodium hydroxide? | Green. |
| The reaction where iron(III) forms a brown precipitate when treated with sodium hydroxide. | Iron(III) and Sodium Hydroxide |
| What color precipitate is formed when iron(III) reacts with sodium hydroxide? | Brown. |
| The reaction where copper(II) forms a blue precipitate when treated with sodium hydroxide. | Copper(II) and Sodium Hydroxide |
| What color precipitate is formed when copper(II) reacts with sodium hydroxide? | Blue. |
| The reaction where aluminium forms a white precipitate when treated with sodium hydroxide. | Aluminium and Sodium Hydroxide |
| What color precipitate is formed when aluminium reacts with sodium hydroxide? | White. |
| The reaction where calcium forms a white precipitate when treated with sodium hydroxide. | Calcium and Sodium Hydroxide |
| What color precipitate is formed when calcium reacts with sodium hydroxide? | White. |
| The reaction where magnesium forms a white precipitate when treated with sodium hydroxide. | Magnesium and Sodium Hydroxide |
| What color precipitate is formed when magnesium reacts with sodium hydroxide? | White. |
| The process of determining the metal ions present by observing the characteristic precipitates formed with sodium hydroxide. | Identifying Metal Ions |
| Why is the sodium hydroxide test valuable in identifying metal ions? | It produces distinctive precipitates that help identify specific metal ions. |
| The use of a surplus amount of sodium hydroxide in a chemical test. | Excess Sodium Hydroxide |
| Why is excess sodium hydroxide used in identifying white precipitates? | It helps distinguish between different white precipitates. |
| The compound formed when aluminium reacts with sodium hydroxide. | Aluminium Hydroxide. |
| What happens to aluminium hydroxide when excess sodium hydroxide is added? | It redissolves. |
| The compound formed when calcium or magnesium reacts with sodium hydroxide. | Calcium Hydroxide and Magnesium Hydroxide |
| What is the behavior of calcium hydroxide and magnesium hydroxide when excess sodium hydroxide is added? | It does not redissolve and remains as a precipitate. |
| To dissolve again after previously forming a precipitate. | Redissolve |
| Which of the white precipitates redissolves in excess sodium hydroxide? | Aluminium Hydroxide. |
| The process of telling the difference between aluminium and calcium or magnesium precipitates by observing their behavior with excess sodium hydroxide. | Distinguishing Aluminium and Calcium/Magnesium Precipitates |
| How does the behavior of white precipitates help in distinguishing between aluminium and calcium ions? | Aluminium precipitate redissolves, while calcium precipitate and magnesium precipitate does not, in excess sodium hydroxide. |
| A test used to confirm the identity of a substance. | Confirmatory Test |
| How can excess sodium hydroxide be considered a confirmatory test for certain metal ions? | It confirms the identity of aluminium ions based on the redissolution of the precipitate. |
| The ability of a substance to dissolve in a solvent. | Solubility |
| What does the redissolution of aluminium hydroxide indicate about its solubility in excess sodium hydroxide? | Aluminium hydroxide is soluble in excess sodium hydroxide. |
| The ability of a precipitate to remain unchanged in a solution. | Precipitate Stability |
| How does the stability of a precipitate influence its behavior with excess sodium hydroxide? | Less stable precipitates, like aluminium hydroxide, may redissolve. |
| The act of visually examining a reaction or substance. | Visual Observation |
| How can one visually observe the difference between aluminium and calcium precipitates in the presence of excess sodium hydroxide? | By noting the redissolution of aluminium hydroxide while calcium hydroxide remains unchanged. |
