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Examples compare maximum bond counts in elements across the 2nd and 3rd periods, including promotion energy considerations, octet rule and hypervalence, resonance and formal charges.",{"@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/research-report/","Research & Report",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/document/molecular-structure-and-bonding-lewis-concept-and-atomic-bonding-rules/657126/",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/molecular-structure-and-bonding-lewis-concept-and-atomic-bonding-rules/657126.png","ImageObject",300,407,{"name":42,"@type":43},"How to eat","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-30","2026-10-26",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",6,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"What foundational knowledge is needed to understand molecular compound formation and structure?","Question",{"text":63,"@type":64},"You need periodic table information (groups and periods), electron and valence electron counting, electronic structure (ground/excited states), the 2-electron requirement for a bond, atomic orbitals and quantum numbers, and the Lewis concept/structure.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"How do quantum numbers relate to an electron’s properties in orbitals?",{"text":68,"@type":64},"The document links n to size, l to shape, m to orientation, and s to spin, and uses the Pauli principle and Hund’s rule to account for how electrons fill quantum states.",{"name":70,"@type":61,"acceptedAnswer":71},"How can elements form more than four bonds, and what limits apply?",{"text":72,"@type":64},"For n > 2, empty low-level d orbitals allow more than four bonds; for the 3rd period the maximum bond number is stated as 7. The 2nd period is limited to 4 bonds because only four orbitals are available, tying this to the octet rule.","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},657126,1793085443,{"code":4,"msg":82,"data":83},"success",[84,88,92,96,101,105,110,114,119,122,126],{"id":22,"doc_module":4,"doc_module_name":25,"category_name":85,"show_sort_weight":86,"slug":87},"Story & Novel",90,"story-novel",{"id":26,"doc_module":4,"doc_module_name":25,"category_name":89,"show_sort_weight":90,"slug":91},"Literature",80,"literature",{"id":33,"doc_module":4,"doc_module_name":25,"category_name":93,"show_sort_weight":94,"slug":95},"Exam",70,"exam",{"id":97,"doc_module":4,"doc_module_name":25,"category_name":98,"show_sort_weight":99,"slug":100},5,"Comic",60,"comic",{"id":55,"doc_module":4,"doc_module_name":25,"category_name":102,"show_sort_weight":103,"slug":104},"Technology",50,"technology",{"id":106,"doc_module":4,"doc_module_name":25,"category_name":107,"show_sort_weight":108,"slug":109},7,"Healthcare",40,"healthcare",{"id":111,"doc_module":4,"doc_module_name":25,"category_name":29,"show_sort_weight":112,"slug":113},8,30,"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":97,"slug":129},19,"General","general",{"code":4,"msg":82,"data":131},{"doc_id":79,"user_id":132,"nickname":42,"user_avatar":133,"doc_module":4,"category_id":111,"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":55,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":115,"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":143,"read_time":144},962093541613,"https://ap-avatar.wpscdn.com/davatar_9964176cb1d06d4a9deccf72a44ae3dc","Molecular structure and bonding  \nTo understand the formation and structure of molecular compounds, first one has to learn, recognize, use, count, take into account:  \n• the periodic table with groups and periods,  \n• the number of electrons and valence electrons (i.e. count electrons),(2 (K), 8 (L) = 2 + 6, 18 (M) = 2 + 6 + 10, 32 (N) = 2 + 6 + 10 + 14, etc. ),  \n• the electronic structure (ground state, exited state),• the need of 2 electrons for a bond,  \n•atomic orbitals and quantum states (with quantum numbers n, m, l, s),• the energy levels of the different shells, subshells, orbitals,  \n• the maximum number of shells, subshells, orbitals, and electrons,  \n• the numbers and/or maximum numbers of bonds, an atom likes to or can build or have,  \n• the Lewis concept/structure.  \nEnergies of the atomic shells K, L, M, N and the subshells/orbitals s, p, d, f  \n← Start of 3d elements (Sc)  \nAtomic number Z  \nEnergy increases with increasing n, and is high between the shells (except d and f) .  \nn → size, l → shape, m → orientation, s → spin of e, Pauli principle (not all 4 quantum numbers can be equal), Hund‘s rule (spin maximizing) .  \nIt is useful to learn also the maximum number of shells (n), subshells/orbitals (s, p, d, f), and electrons an atom can have.  \nShell n Orbital Nunber of Number of electrons in  \norbitals orbital shell (2n2)  \nThe next step is to find the numbers and/or maximum numbers of bonds, an atom likes to or can have, e.g. in hydrogen compounds of group 4 to 8 elements.  \nMain group  \nElectron * configuration  \nNumber of possible bonds  \nExisting H compouns  \nLewis formula  \n/4 *  \nnone  \nuse – instead of :  \n* Promotion/exitation of an 1s electron ofC, Si to 1p needs a lot of energy (460 kJ/mol for C), but is compensated by the formation of 2 additional bonds (CH4 instead of CH2) .  \nFor promotion to a d level, the energy is to high.  \nElectron configuration and number of bonds for elements of 2. period  \nAtom or ion  \nNumber of bonds  \nNumber * of electrons  \nExamples  \nElectron configuration  \nElements of 2. period can build not more than 4 bonds, because there are only 4 orbitals available → octett rule. Consider ground states (Pauli, Hund), exited states.  \n* Number of electrons in bonds  \nElectron configuration and number of bonds for elements of 3. period  \nAtom or ion  \nNumber Number * Examples of bonds of electrons  \nElectron configuration  \nFor n > 2 one can have more than 4 bonds, because there are empty low-level d orbitals avaiable. For elements of 3. period, the maximum number of bonds is 7.  \n* Number of electrons in bonds  \nHighest number of bonds is equivalent to the main group number.  \nElement Group Number of bonds  \nP 5 3, 5  \nS 6 2, 4, 6  \nCl 7 1, 3, 5, 7  \nSome examples:  \nSiF62-, PF5, SF6 do exist CF62-, NF5, OF6 do not exist  \nExamples: Lewis structure of N2 , NH3 , NO2-, NO3-, S2 , SO2 , SO3 , SO32 . Those which are not necessarily resonance structures/hybrids are marked with an asterisk. → Octett rule, hypervalence, formal charges  \n-are used instead of :  \n* No other resonance structure","cbCaiq5Xc1fKb9HB","https://ap.wps.com/l/cbCaiq5Xc1fKb9HB","pdf",675679,"English","# Molecular prerequisites for bonding\n## Periodic table, electron counting, valence\n## Electronic structure: ground vs excited states\n# Atomic shells and quantum states\n## Energy levels and quantum numbers\n## Pauli principle and Hund’s rule\n# Bond capacity and main-group trends\n## Maximum shells/subshells/orbitals and electrons\n## Number of bonds and main-group relation\n# Examples and rules in practice\n## Second-period bond limits and octet rule\n## Third-period bond expansion via d orbitals\n## Lewis formulas, resonance, hypervalence, and formal charges","[{\"question\":\"What foundational knowledge is needed to understand molecular compound formation and structure?\",\"answer\":\"You need periodic table information (groups and periods), electron and valence electron counting, electronic structure (ground/excited states), the 2-electron requirement for a bond, atomic orbitals and quantum numbers, and the Lewis concept/structure.\"},{\"question\":\"How do quantum numbers relate to an electron’s properties in orbitals?\",\"answer\":\"The document links n to size, l to shape, m to orientation, and s to spin, and uses the Pauli principle and Hund’s rule to account for how electrons fill quantum states.\"},{\"question\":\"How can elements form more than four bonds, and what limits apply?\",\"answer\":\"For n \\u003e 2, empty low-level d orbitals allow more than four bonds; for the 3rd period the maximum bond number is stated as 7. The 2nd period is limited to 4 bonds because only four orbitals are available, tying this to the octet rule.\"}]","Molecular structure and bonding - Lewis concept and atomic bonding rules | PDF",1792974525,23]