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Halogens

A-Level AQA Chemistry

This pack of flashcards encompasses the physical and chemical properties of halogens, their reactivity, trends in periodic properties, and reactions with sulfuric acid. It covers electronegativity, melting and boiling points, reducing power of halides, and specifics of disproportionation and redox reactions involving chlorine, bromine, and iodine. Additionally, it addresses the use of chlorine in water treatment, and the nomenclature of chlorates and sulfates.

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"Describe the reactions and observations when iodide reacts with concentrated sulfuric acid."	"White steamy fumes of HI are evolved. Black solid and purple fumes of iodine are also evolved. A yellow solid of sulfur and a gas with a bad egg smell, H2S, are produced."
"Define chlorates and sulfates according to IUPAC convention."	"Chlorates and sulfates are compounds of chlorine and sulfur with oxygen, named with the relevant oxidation number in roman numerals."
"What is the purpose of using a mixture of NaCl and NaClo?"	"The mixture is used as bleach and to disinfect/kill bacteria."
"How does chlorine react with cold dilute NaOH solution?"	"Chlorine reacts with cold dilute NaOH to form NaCl and NaClo, and the solution becomes colorless."
"What causes the greenish color of chlorine water to fade?"	"The greenish color fades as chlorine reacts with water to produce O2 gas."
"What happens when chlorine is bubbled through water in the presence of sunlight?"	"Chlorine reacts with water to form HCl and HClo, and produces O2 gas."
"Describe disproportionation reactions of chlorine."	"Disproportionation is a reaction where chlorine simultaneously oxidizes and reduces."
"Describe the physical properties of fluorine."	"Fluorine is a very pale yellow gas and highly reactive."
"Define the role of H2SO4 in the reaction of bromide with concentrated sulfuric acid."	"H2SO4 acts as an acid in the first step producing HBr and then acts as an oxidizing agent in the second redox step."
"What are the observations when bromide reacts with concentrated sulfuric acid?"	"White steamy fumes of HBr are evolved. Orange fumes of bromine are also evolved."
"What happens fluoride and chloride react with concentrated sulfuric acid?"	"No redox reactions occur. Only acid-base reactions occur."
"Describe the reducing power of halides as you go down group 7."	"The reducing power of the halides down group 7."
"Describe the trend in melting and boiling points of halogens."	"The melting and boiling points increase down the group as the intermolecular forces get larger."
"How does the electronegativity change as you go down the halogens group?"	"The electronegativity decreases down the group."
"Define electronegativity."	"Electronegativity is the relative tendency of an atom in a molecule to attract electrons in a covalent bond to itself."
"What is the color and reactivity of chlorine?"	"Chlorine is a greenish gas and highly reactive."

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Describe the reactions and observations when iodide reacts with concentrated sulfuric acid.

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White steamy fumes of HI are evolved. Black solid and purple fumes of iodine are also evolved. A yellow solid of sulfur and a gas with a bad egg smell, H2S, are produced.

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[{"id":978134,"front":"Describe the reactions and observations when iodide reacts with concentrated sulfuric acid.","back":"White steamy fumes of HI are evolved. Black solid and purple fumes of iodine are also evolved. A yellow solid of sulfur and a gas with a bad egg smell, H2S, are produced.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"When iodide reacts with concentrated sulfuric acid, several reactions and observations occur. White steamy fumes of hydrogen iodide (HI) are released, indicating the formation of a gaseous compound. Additionally, black solid iodine and purple fumes of iodine are evolved, suggesting the presence of elemental iodine. The reaction also produces a yellow solid of sulfur and a gas with a foul odor resembling rotten eggs, hydrogen sulfide (H2S). These observations indicate the formation of multiple compounds and the release of gases during the reaction.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978140,"front":"Define chlorates and sulfates according to IUPAC convention.","back":"Chlorates and sulfates are compounds of chlorine and sulfur with oxygen, named with the relevant oxidation number in roman numerals.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":1,"explanation":"Chlorates and sulfates are named using the IUPAC convention, which specifies the use of roman numerals to indicate the oxidation state of the central element (chlorine or sulfur) in the compound. This naming system provides a clear and systematic way to identify and differentiate between different compounds containing these elements.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978139,"front":"What is the purpose of using a mixture of NaCl and NaClo?","back":"The mixture is used as bleach and to disinfect/kill bacteria.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":2,"explanation":"The purpose of using a mixture of NaCl and NaClo is to utilize their properties as a bleach and disinfectant. NaClO, also known as sodium hypochlorite, is a powerful oxidizing agent that can effectively kill bacteria and other microorganisms. When combined with NaCl, sodium chloride, it enhances the bleaching and disinfecting properties of the mixture. This combination is commonly used in cleaning and sanitizing applications.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978138,"front":"How does chlorine react with cold dilute NaOH solution?","back":"Chlorine reacts with cold dilute NaOH to form NaCl and NaClo, and the solution becomes colorless.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":3,"explanation":"Chlorine reacts with cold dilute NaOH solution to form sodium chloride (NaCl) and sodium hypochlorite (NaClo). This reaction is important in water treatment, as sodium hypochlorite is a disinfectant. The colorless solution indicates the completion of the reaction.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978137,"front":"What causes the greenish color of chlorine water to fade?","back":"The greenish color fades as chlorine reacts with water to produce O2 gas.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":4,"explanation":"Chlorine water's greenish color fades due to a chemical reaction with water, leading to the production of O2 gas. This reaction alters the composition of the chlorine water, resulting in the loss of its original color.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978136,"front":"What happens when chlorine is bubbled through water in the presence of sunlight?","back":"Chlorine reacts with water to form HCl and HClo, and produces O2 gas.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":5,"explanation":"When chlorine is bubbled through water in the presence of sunlight, a chemical reaction occurs. Chlorine reacts with water molecules to form hydrochloric acid (HCl) and hypochlorous acid (HClO). Additionally, oxygen gas (O2) is produced as a byproduct of this reaction. The presence of sunlight likely provides the energy needed to drive the reaction forward.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978135,"front":"Describe disproportionation reactions of chlorine.","back":"Disproportionation is a reaction where chlorine simultaneously oxidizes and reduces.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":6,"explanation":"Disproportionation reactions of chlorine involve the same element undergoing both oxidation and reduction simultaneously. This occurs because chlorine can exist in multiple oxidation states, allowing it to both gain and lose electrons within the same reaction. This unique behavior is a key characteristic of chlorine chemistry.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978125,"front":"Describe the physical properties of fluorine.","back":"Fluorine is a very pale yellow gas and highly reactive.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":7,"explanation":"Fluorine's pale yellow color is due to its gaseous state, and its high reactivity is a result of its electronegativity, making it eager to form bonds with other elements. These properties are fundamental to understanding its behavior in chemical reactions and its applications in various industries.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978133,"front":"Define the role of H2SO4 in the reaction of bromide with concentrated sulfuric acid.","back":"H2SO4 acts as an acid in the first step producing HBr and then acts as an oxidizing agent in the second redox step.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":8,"explanation":"Concentrated sulfuric acid (H2SO4) serves a dual role in the reaction. Initially, it acts as an acid, facilitating the formation of HBr. Subsequently, it functions as an oxidizing agent, driving the redox reaction. This dual functionality of H2SO4 is crucial in the overall reaction mechanism.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978132,"front":"What are the observations when bromide reacts with concentrated sulfuric acid?","back":"White steamy fumes of HBr are evolved. Orange fumes of bromine are also evolved.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":9,"explanation":"When bromide reacts with concentrated sulfuric acid, the white steamy fumes of hydrogen bromide (HBr) are observed due to the reaction producing HBr gas. Additionally, the orange fumes of bromine are seen, indicating the presence of bromine gas as a product of the reaction.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978131,"front":"What happens fluoride and chloride react with concentrated sulfuric acid?","back":"No redox reactions occur. Only acid-base reactions occur.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":10,"explanation":"When fluoride and chloride react with concentrated sulfuric acid, no redox reactions occur. This is because sulfuric acid is a strong acid and will only undergo acid-base reactions with fluoride and chloride ions. This is due to the high reactivity of sulfuric acid as a strong dehydrating agent.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978130,"front":"Describe the reducing power of halides as you go down group 7.","back":"The reducing power of the halides down group 7.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":11,"explanation":"As you go down Group 7, the reducing power of the halides increases. This is because the atomic radius increases, leading to a weaker attraction between the nucleus and the outermost electrons. As a result, the outermost electrons are more easily lost, making the halides better reducing agents. Additionally, the electronegativity decreases down the group, further enhancing the reducing power.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978129,"front":"Describe the trend in melting and boiling points of halogens.","back":"The melting and boiling points increase down the group as the intermolecular forces get larger.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":12,"explanation":"The trend in melting and boiling points of halogens is due to the increase in the size of the atoms down the group, leading to stronger van der Waals forces. This results in higher melting and boiling points as more energy is required to overcome these forces.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978128,"front":"How does the electronegativity change as you go down the halogens group?","back":"The electronegativity decreases down the group.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":13,"explanation":"As you move down the halogens group, the electronegativity decreases. This is because the atomic size increases, resulting in a larger distance between the nucleus and the outermost electrons. As a result, the attraction between the nucleus and the electrons decreases, leading to a lower electronegativity. This trend can be explained by the shielding effect of inner electron shells, which reduces the effective nuclear charge experienced by the outermost electrons.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978127,"front":"Define electronegativity.","back":"Electronegativity is the relative tendency of an atom in a molecule to attract electrons in a covalent bond to itself.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":14,"explanation":"Electronegativity is a fundamental concept in chemistry, indicating an atom's ability to attract shared electrons in a chemical bond. It's crucial for understanding bond polarity and reactivity. It's quantitatively measured using various scales like Pauling or Mulliken.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":978126,"front":"What is the color and reactivity of chlorine?","back":"Chlorine is a greenish gas and highly reactive.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":15,"explanation":"Chlorine's greenish color is due to its absorption of red light, and its high reactivity is due to its strong electron-attracting ability. This makes it highly reactive with other elements, particularly metals, and it is used in various industrial processes because of this reactivity.","deleted_at":null,"flashcard_deck_id":"28rgG","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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