[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-343678-105":3,"doc-detail-343678-en":81,"detail-sidebar-cat-0-en-105":98},{"code":4,"msg":5,"data":6},0,"ok",{"site_id":7,"language":8,"slug":9,"title":10,"keywords":11,"description":12,"schema_data":13,"social_meta":74,"head_meta":76,"extra_data":78,"updated_unix":80},105,"en","topic-4-bonding-ionic-bonding-and-structure","Topic 4 - Bonding - Ionic bonding and structure","","Topic 4: Bonding explains how ions form and how ionic compounds are built from cations and anions. It details electron loss and gain, electrostatic attraction, lattice formation, and electron shell representations, including examples such as sodium chloride. The content also connects ionic structure to physical properties: low volatility, high melting and boiling points, electrical conductivity in molten state, and solubility in polar solvents. It then introduces covalent bonding basics, including shared electrons, bond types, and bond polarity.",{"@graph":14,"@context":73},[15,34,56],{"@type":16,"itemListElement":17},"BreadcrumbList",[18,23,27,31],{"item":19,"name":20,"@type":21,"position":22},"https://docshare.wps.com","Home","ListItem",1,{"item":24,"name":25,"@type":21,"position":26},"https://docshare.wps.com/document/","Document",2,{"item":28,"name":29,"@type":21,"position":30},"https://docshare.wps.com/document/exam/","Exam",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/document/topic-4-bonding-ionic-bonding-and-structure/343678/",4,{"url":32,"name":10,"@type":35,"image":36,"author":41,"headline":10,"publisher":44,"fileFormat":47,"inLanguage":8,"description":12,"dateModified":48,"datePublished":49,"encodingFormat":47,"isAccessibleForFree":50,"interactionStatistic":51},"DigitalDocument",{"url":37,"@type":38,"width":39,"height":40},"https://docshare.wps.com/thumbnails/topic-4-bonding-ionic-bonding-and-structure/343678.png","ImageObject",300,407,{"name":42,"@type":43},"Eliana","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/vnd.openxmlformats-officedocument.wordprocessingml.document","2026-11-07","2026-09-22",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",16,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"How do cations and anions form during ionic bonding?","Question",{"text":63,"@type":64},"Metals form cations by losing valence electrons, while non-metals form anions by gaining electrons. The electron transfer changes the atom’s net charge.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"Why do ionic compounds usually have high melting temperatures and low volatility?",{"text":68,"@type":64},"Ionic bonds create strong electrostatic attraction within a lattice, requiring significant energy to break. At room temperature there is insufficient energy to disrupt the lattice, so ionic compounds have low volatility and high melting temperatures.",{"name":70,"@type":61,"acceptedAnswer":71},"When can ionic compounds conduct electricity?",{"text":72,"@type":64},"Solid ionic compounds cannot conduct because ions are fixed in place within the crystal lattice. When molten, ions are free to move, allowing electrical conductivity.","https://schema.org",{"og:url":32,"og:type":75,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":77,"canonical":32},"index,follow",{"doc_id":79,"site_id":7},343678,1790392279,{"code":4,"msg":82,"data":83},"success",{"doc_id":79,"user_id":84,"nickname":42,"user_avatar":85,"doc_module":4,"category_id":33,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":86,"file_id":87,"file_url":88,"file_type":89,"file_size":90,"view_count":55,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":91,"language":92,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":93,"faqs":94,"seo_title":95,"seo_description":12,"update_tm":96,"read_time":97,"preview_page_count":4},4398048949847,"https://ap-avatar.wpscdn.com/avatar/400002536579ef2da7f?_k=1778318612642679267","Topic 4: Bonding\n4.1\nIonic bonding and structure\n4.1.1\nPositive ions (cations) form by metals losing valence electrons\n4.1.2\nNegative ions (anions) form by non-metals gaining electrons\n4.1.3\nThe number of electrons lost or gained is determined by the electron configuration of the atom\n4.1.4\nThe ionic bond is due to electrostatic attraction between oppositely charged ions\n4.1.5\nUnder normal conditions, ionic compounds are usually solids with lattice structures\n4.1.6\nDeduction of the formula and name of an ionic compound from its component ions, including polyatomic ions\n4.1.7\nExplanation of the physical properties of ionic compounds (volatility, electrical conductivity and solubility) in terms of their structure\nIons\nAtoms have a neutral charge as their negative electrons and positive protons balance out\nHowever, ions are formed when atoms gain or lose electrons\nThe charge is changed by adding or removing electrons from an atom\nCations are atoms that lose electrons and therefore have a positive net charge\nTherefore, positive ions are called cations\nAnions are atoms that gain electrons and therefore have a negative net charge\nTherefore, negative ions are called anions\nIonic Bonding\nIonic bonds form as a result of the electrostatic attraction between oppositely charged ions\nAn electrostatic attraction is the attraction of oppositely charged of particles/objects\nThis bond only occurs between metals and non-metals\nThe metal will have a positive charge, while the non-metal will have a negative charge\nThe opposite charges create an electrostatic attraction between the ions, causing them to form a neutral lattice\nThe charge of the ions will cancel each other out\nFormation of an ionic compound\nWhen metals react with non-metals electrons are transferred from the metal to the non-metal forming an ion\nIonic compounds are balanced as the negative and positive charges balance each other out\nThe formation of an ionic compound can be represented using electron shell diagrams\nExample: When sodium and chlorine react together to form sodium chloride the electron that a sodium atom loses to form a stable sodium ion is gained by a chlorine atom to for a stable chlorine ion\nChemical Charge\nRemember, noble gas configuration is the most stable so most elements will try to reach it by either losing or gaining electrons\nTo find the ionic charge of an element the periodic table can be used:\nGroup 1, 2, 3 elements form ions with charges of 1+, 2+ and 3+ respectively\nGroup 15, 16, 17 elements form ions with charges of 3-, 2-, 1- respectively\nElements in group 14 can lose 4 electrons but can also gain 4 electrons\nPhysical Properties of Ionic Compounds\nThe electrostatic force of attraction between oppositely charged ions arrange in a 3D structure called a lattice\nThis is possible because the ions are held together by their opposite charges, and each ion will be surrounded by 6 other different ions\nFor the most stable arrangement positively charged ions are packed as closely as possible to the negative charged ions, while ions of the same charge are as far apart as possible. This maximizes electrostatic attraction between the ions, while minimizing repulsion\nUnder normal conditions, ionic compounds are usually solids with lattice structures\nThe lattice structure of an ionic compound can be used to explain their physical properties\nVolatility\nVolatility: The tendency of a substance to vaporize\nIonic compounds have ionic bonds which are very strong meaning that a lot of energy is needed to break its bonds. Thus at room temperature there isn’t enough energy to break the lattice.\nExample: If you leave salt in a room for 100 years it will be the same, it won’t turn into a gas because it’s non-volatile\nTherefore ionic compounds can be described as having a low volatility or being non-volatile\nHigh melting temperatures\nAs mentioned before ionic bonds are very strong and a lot of energy is needed to break its bond\nHence ionic compounds have high melting temperatures","cbCaids5ejKLUowG","https://ap.wps.com/l/cbCaids5ejKLUowG","docx",490995,11,"English","# Topic 4: Bonding\n## 4.1 Ionic bonding and structure\n## 4.2 Covalent bonding","[{\"question\":\"How do cations and anions form during ionic bonding?\",\"answer\":\"Metals form cations by losing valence electrons, while non-metals form anions by gaining electrons. The electron transfer changes the atom’s net charge.\"},{\"question\":\"Why do ionic compounds usually have high melting temperatures and low volatility?\",\"answer\":\"Ionic bonds create strong electrostatic attraction within a lattice, requiring significant energy to break. At room temperature there is insufficient energy to disrupt the lattice, so ionic compounds have low volatility and high melting temperatures.\"},{\"question\":\"When can ionic compounds conduct electricity?\",\"answer\":\"Solid ionic compounds cannot conduct because ions are fixed in place within the crystal lattice. 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