[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-665346-105":3,"detail-sidebar-cat-0-en-105":80,"doc-detail-665346-en":130},{"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":73,"head_meta":75,"extra_data":77,"updated_unix":79},105,"en","14-bonding","1.4 - Bonding","","Explains bonding in chemistry, starting with ionic bonding formed when metals lose electrons to become cations and non-metals gain electrons to become anions, creating strong electrostatic attraction between oppositely charged ions. Covers covalent bonding where shared electron pairs form between non-metals, plus coordinate bonding when both electrons in the bond pair come from the same atom. Introduces polar bonds, electronegativity, polarity (polar vs non-polar covalent, and when bonds become ionic), and then details intermolecular forces: dipole-dipole, induced dipole-induced dipole (van der Waals), and hydrogen bonding, including effects on boiling points and solubility.",{"@graph":14,"@context":72},[15,34,55],{"@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/14-bonding/665346/",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/14-bonding/665346.png","ImageObject",300,407,{"name":42,"@type":43},"CatatanPagi","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-30","2026-10-29",true,{"@type":52,"interactionType":53,"userInteractionCount":33},"InteractionCounter",{"@type":54},"ViewAction",{"@type":56,"mainEntity":57},"FAQPage",[58,64,68],{"name":59,"@type":60,"acceptedAnswer":61},"What distinguishes ionic bonding from covalent bonding?","Question",{"text":62,"@type":63},"Ionic bonding involves electron transfer from a metal to a non-metal, forming oppositely charged ions that attract strongly. Covalent bonding involves sharing electrons between atoms, typically within the outermost shells.","Answer",{"name":65,"@type":60,"acceptedAnswer":66},"How does electronegativity relate to bond polarity?",{"text":67,"@type":63},"Electronegativity measures how strongly atoms attract bonding electrons. Unequal electronegativity pulls shared electrons toward the more electronegative atom, creating partial charges (δ- and δ+), which makes the bond polar.",{"name":69,"@type":60,"acceptedAnswer":70},"What intermolecular forces are included besides hydrogen bonding?",{"text":71,"@type":63},"The notes cover dipole-dipole forces and induced dipole-induced dipole forces (van der Waals forces). Hydrogen bonds are presented as special intermolecular forces involving hydrogen bonded to highly electronegative atoms with lone pairs.","https://schema.org",{"og:url":32,"og:type":74,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":76,"canonical":32},"index,follow",{"doc_id":78,"site_id":7},665346,1793299150,{"code":4,"msg":81,"data":82},"success",[83,87,91,94,99,104,109,114,119,122,126],{"id":22,"doc_module":4,"doc_module_name":25,"category_name":84,"show_sort_weight":85,"slug":86},"Story & Novel",90,"story-novel",{"id":26,"doc_module":4,"doc_module_name":25,"category_name":88,"show_sort_weight":89,"slug":90},"Literature",80,"literature",{"id":33,"doc_module":4,"doc_module_name":25,"category_name":29,"show_sort_weight":92,"slug":93},70,"exam",{"id":95,"doc_module":4,"doc_module_name":25,"category_name":96,"show_sort_weight":97,"slug":98},5,"Comic",60,"comic",{"id":100,"doc_module":4,"doc_module_name":25,"category_name":101,"show_sort_weight":102,"slug":103},6,"Technology",50,"technology",{"id":105,"doc_module":4,"doc_module_name":25,"category_name":106,"show_sort_weight":107,"slug":108},7,"Healthcare",40,"healthcare",{"id":110,"doc_module":4,"doc_module_name":25,"category_name":111,"show_sort_weight":112,"slug":113},8,"Research & Report",30,"research-report",{"id":115,"doc_module":4,"doc_module_name":25,"category_name":116,"show_sort_weight":117,"slug":118},9,"Religion & Spirituality",20,"religion-spirituality",{"id":117,"doc_module":4,"doc_module_name":25,"category_name":120,"show_sort_weight":117,"slug":121},"World Cup","world-cup",{"id":123,"doc_module":4,"doc_module_name":25,"category_name":124,"show_sort_weight":123,"slug":125},10,"Lifestyle","lifestyle",{"id":127,"doc_module":4,"doc_module_name":25,"category_name":128,"show_sort_weight":95,"slug":129},19,"General","general",{"code":4,"msg":81,"data":131},{"doc_id":78,"user_id":132,"nickname":42,"user_avatar":133,"doc_module":4,"category_id":33,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":33,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":26,"language":139,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":140,"faqs":141,"seo_title":142,"seo_description":12,"update_tm":79,"read_time":95},962090894170,"https://ap-avatar.wpscdn.com/davatar_6f874abed73319feea01a86fa6f0fab8","1.4 – Bonding  \n\n| When a metal and a non-metal react together, the metal atom loses electrons and becomes a cation (+), and the non-metal gains electrons and becomesan anion (-) . There are strong electrostatic forces of attraction between these oppositely charged ions. This is called ionic bonding.\u003Cbr>Dot and cross diagrams show how ionic bonds form. |  |  |  |  |  |  |  |\n| --- | --- | --- | --- | --- | --- | --- | --- |\n| Li x\u003Cbr>2.1\u003Cbr>Li x\u003Cbr>2.1\u003Cbr>\u003Cbr>\u003Cbr>| 1 electron |  | | | +\u003Cbr>+ | \u003Cbr>[2 .8]2- | 2- |\n|  | | |  |  |  |  |  |\n\nIonic bonding  \n\n| \u003Cbr>Covalent bonding\u003Cbr>When non-metals bond together, each atom gives one electron to form a bond pair in which the electron spins are opposed. A covalent bond is the electrostatic attraction between the positive nuclei of the bonded atoms and the shared electrons between them. Atoms only share electrons in their outermost shells.\u003Cbr>Dot and cross diagrams show how covalent bonds form. |  |  |  |\n| --- | --- | --- | --- |\n| | H   H\u003Cbr>O\u003Cbr>(water, H2O) | | O ~~ ~~ O\u003Cbr>(oxygen, O2) |\n| Single bonds |  | Double bonds |  |\n\nCoordinate bonding  \nThe same as a covalent bond but both electrons forming the bond pair come from the same atom.  \nH  \nH  \nO +  \nx  \nx  \n+  \nH   \n+  \nHydronium Ion  \nVery few compounds are purely ionic or purely covalent. Many substances contain bonds that are intermediate in character between pure covalent and pure ionic bonds. These are called polar bonds. The degree of ionic or covalent character depends on the difference in electronegativity between the bonded atoms. The greater the difference in electronegativity, the greater the ionic character.  \n\n| \u003Cbr>Electronegativity and polarity\u003Cbr>Electronegativity is a measure of how strongly atoms attract electrons in a covalent bond. The higher the electronegativity value, the better the element can attract bonding electrons.\u003Cbr>In a covalent bond, the electron pair is not usually shared exactly evenly between the two atoms. Normally, the atoms have different electronegativities and the bonding electrons are pulled towards the more electronegative atom. This atom will take up a slightly negative charge and the other becomes slightly positive. The partial charges are written above the atoms using the symbol δ (delta) . The bond is said to be polar. |  |\n| --- | --- |\n| Shared electrons pulled towards chlorine | δ+ X δ -H ~~ ~~ Cl\u003Cbr>\u003Cbr>|\n| If the two atoms are the same, the atoms have equal electronegativities, so the electrons are equally shared and the bond is said to be non-polar.\u003Cbr>Electrons H  x  H\u003Cbr>equally \u003Cbr>shared \u003Cbr>In general, bonds where the electronegativity difference between the two atoms is less than about 0.4 will be non-polar covalent bonds. If the electronegativity difference is between 0.4 and about 1.9 then they will be polar covalent bonds. If the difference is about 2.0 or more, they will be ionic. |  |\n\n1.4 – Bonding  \nForces between molecules  \nYou need to know about three types: dipole-dipole forces, induced dipole-induced dipole forces and hydrogen bonds.  \nDipole-dipole forces  \nPolar molecules have dipoles, one end has a slightly positive charge, the other a slightly negative charge due to a difference in electronegativities between the atoms in the molecule. If these dipoles arrange themselves so that the negative region of one molecule is close to the positive region of another molecule, there will be an attraction between them.  \nH ~~ ~~ Cl     H ~~ ~~ Cl     H ~~ ~~ Cl  \nPermanent dipole-dipole interactions between HCl molecules  \nEven molecules with no dipoles show intermolecular bonding. Electrons are in constant motion around the nuclei; therefore at any particular moment the distribution of the electron cloud around the nuclei will not be symmetrical. At this moment, the molecule would have a temporary dipole.  \nδ - δ+ δ - δ+  \nThe δ+ end of the molecule can pull the electron cloud of a neighbouring molecule towards it, giving the left side of that molecule a δ-cha","cbCaiutadWGKxLyC","https://ap.wps.com/l/cbCaiutadWGKxLyC","pdf",518400,"English","# Forces between molecules\n## Dipole-dipole forces\n## Induced dipole-induced dipole forces\n## Hydrogen bonds","[{\"question\":\"What distinguishes ionic bonding from covalent bonding?\",\"answer\":\"Ionic bonding involves electron transfer from a metal to a non-metal, forming oppositely charged ions that attract strongly. Covalent bonding involves sharing electrons between atoms, typically within the outermost shells.\"},{\"question\":\"How does electronegativity relate to bond polarity?\",\"answer\":\"Electronegativity measures how strongly atoms attract bonding electrons. Unequal electronegativity pulls shared electrons toward the more electronegative atom, creating partial charges (δ- and δ+), which makes the bond polar.\"},{\"question\":\"What intermolecular forces are included besides hydrogen bonding?\",\"answer\":\"The notes cover dipole-dipole forces and induced dipole-induced dipole forces (van der Waals forces). Hydrogen bonds are presented as special intermolecular forces involving hydrogen bonded to highly electronegative atoms with lone pairs.\"}]","1.4 - Bonding | PDF"]