{"id":26,"date":"2024-04-04T07:30:16","date_gmt":"2024-04-04T04:30:16","guid":{"rendered":"https:\/\/sisu.ut.ee\/huvitavkeemia\/41-aatomi-ehitus-ja-elementide-omadused\/"},"modified":"2025-04-17T11:25:00","modified_gmt":"2025-04-17T08:25:00","slug":"41-aatomi-ehitus-ja-elementide-omadused","status":"publish","type":"page","link":"https:\/\/sisu.ut.ee\/huvitavkeemia\/41-aatomi-ehitus-ja-elementide-omadused\/","title":{"rendered":"4.1. Aatomi ehitus ja elementide omadused"},"content":{"rendered":"<h2><span lang=\"et\"><span style=\"line-height: 115%;\">Milleks peaksime teadma aatomi ehitust?<\/span><\/span><\/h2>\n<p><span lang=\"et\"><span style=\"line-height: 115%;\">Ained koosnevad erinevatest\u00a0aatomitest, molekulidest v\u00f5i ioonidest. Aatomiehitus ja aatomitevahelised\u00a0sidemed m\u00e4\u00e4ravad aine omadused. J\u00e4rgnevast videost saadki tuletada meelde aatomiehituse p\u00f5hiteadmised ja aatomiehituse seosed perioodilisustabeliga.<\/span><\/span><\/p>\n<p><\/p><div class=\"ratio ratio-16x9 mb-3\"><div class=\"video-placeholder-wrapper video-placeholder-wrapper--16x9\">\n\t\t\t    <div class=\"video-placeholder d-flex justify-content-center align-items-center\">\n\t\t\t        <div class=\"overlay text-white p-2 w-100 text-center d-block justify-content-center align-items-center\">\n\t\t\t            <div>Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega.<\/div>\n\t\t\t            <button class=\"btn btn-secondary btn-sm mt-1 consent-change\">Muuda n\u00f5usolekut<\/button>\n\t\t\t        <\/div>\n\t\t\t    <\/div>\n\t\t\t<\/div>\n<\/div>\n<h6>Allikas:\u00a0<a title=\"\" href=\"https:\/\/youtu.be\/DTwdlVdi1pM\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/youtu.be\/DTwdlVdi1pM\"><span style=\"background: white;\"><span style=\"line-height: 115%;\"><span style=\"color: #1155cc;\"><span style=\"text-decoration: none;\">https:\/\/youtu.be\/DTwdlVdi1pM<\/span><\/span><\/span><\/span><\/a><\/h6>\n<p>T\u00e4nap\u00e4evase aatomimudeli ehk kvantmehaanilise mudeli l\u00f5id austria teadlane E. Schr\u00f6dinger\u00a0ja saksa teadlane W. Heisenberg. Selle teooria kohaselt liiguvad elektronid kindlas ruumiosas, moodustades tuuma \u00fcmber elektronpilve. Jooniselt 1 n\u00e4ed heeliumi aatomit:\u00a0k\u00f5ige tumedamad alad t\u00e4histavad piirkonda, kus elektroni leidumise t\u00f5en\u00e4olisus on k\u00f5ige suurem.<\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"692\" height=\"694\" class=\"wp-image-127 aligncenter\" style=\"width: 300px; height: 301px;\" title=\"screenshot_2022-03-15_at_11.48.41.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.48.41.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.48.41.png 692w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.48.41-300x300.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.48.41-150x150.png 150w\" sizes=\"auto, (max-width: 692px) 100vw, 692px\"><\/p>\n<h6 style=\"text-align: center;\">Joonis 1. Heeliumi aatomi kvantmehaaniline kujutus, v\u00e4lja on suurendatud heeliumi tuum, kus on n\u00e4ha kahte neutronit ja kahte prootonit. Allikas: <a title=\"\" href=\"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/9\/97\/Helium_atom.png\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/9\/97\/Helium_atom.png\"><span style=\"color: #1155cc;\">https:\/\/upload.wikimedia.org\/wikipedia\/commons\/9\/97\/Helium_atom.png<\/span><\/a><\/h6>\n<p>Ruumiosa aatomis, kus elektroni leidumise t\u00f5en\u00e4osus on suur, on orbitaal. Joonisel 2 on toodud orbitaalide erinevad kujud ja nimed.<\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1640\" height=\"832\" class=\"alignnone wp-image-128\" style=\"width: 700px; height: 355px;\" title=\"screenshot_2022-03-15_at_11.50.17.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.50.17.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.50.17.png 1640w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.50.17-300x152.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.50.17-1024x519.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.50.17-768x390.png 768w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.50.17-1536x779.png 1536w\" sizes=\"auto, (max-width: 1640px) 100vw, 1640px\"><\/p>\n<h6 style=\"text-align: center;\">Joonis 2. Erinevate orbitaalide nimed ja kujud. Allikas: <a title=\"\" href=\"https:\/\/energywavetheory.com\/atoms\/orbital-shapes\/\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/energywavetheory.com\/atoms\/orbital-shapes\/\"><span style=\"color: #1155cc;\">https:\/\/energywavetheory.com\/atoms\/orbital-shapes\/<\/span><\/a><\/h6>\n<p>Orbitaalid paiknevad kindlatel energiatasemetel. Aatomi energiatasemete arvu n\u00e4itab perioodi number. \u00dchele orbitaalile saab paigutada maksimaalselt kaks elektroni, mis peavad olema vastasspinnidega. Spinn iseloomustab elektroni p\u00f6\u00f6rlemist oma telje \u00fcmber ning tal v\u00f5ivad olla vastavalt p\u00f6\u00f6rlemissuunale ainult kaks v\u00e4\u00e4rtust. Kui orbitaal on t\u00e4itunud kahe elektroniga, siis moodustab see elektronpaari. Orbitaale ja nende t\u00e4itumist m\u00e4rgitakse ruutskeemi abil, kus kastike t\u00e4histab orbitaali ja nool \u00fcles ning nool alla t\u00e4histab vastassuunalise spinniga elektrone.<\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1426\" height=\"208\" class=\"alignnone wp-image-129\" style=\"width: 617px; height: 90px;\" title=\"screenshot_2022-03-15_at_11.52.35.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.52.35.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.52.35.png 1426w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.52.35-300x44.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.52.35-1024x149.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_11.52.35-768x112.png 768w\" sizes=\"auto, (max-width: 1426px) 100vw, 1426px\"><\/p>\n<p>Esimesel energiatasemel on sf\u00e4\u00e4riline 1<i>s<\/i>-orbitaal (1 t\u00e4histabki esimest energiataset). Teises kihis on juba kaks alakihti:<i> <\/i>2<i>s<\/i>\u00a0ja 2<i>p<\/i>\u00a0(orbitaalide kujusid esimesel kahel energiatasemel saad vaadata videost 1).\u00a0 <em>p<\/em><i>\u2013<\/i>orbitaale on kokku kolm, mis asetsevad ruumis eri suundades (vaata joonist 2) ning p-orbitaalid saavad t\u00e4ituda kokku maksimaalselt 6 elektroniga.<\/p>\n<p><\/p><div class=\"ratio ratio-16x9 mb-3\"><div class=\"video-placeholder-wrapper video-placeholder-wrapper--16x9\">\n\t\t\t    <div class=\"video-placeholder d-flex justify-content-center align-items-center\">\n\t\t\t        <div class=\"overlay text-white p-2 w-100 text-center d-block justify-content-center align-items-center\">\n\t\t\t            <div>Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega.<\/div>\n\t\t\t            <button class=\"btn btn-secondary btn-sm mt-1 consent-change\">Muuda n\u00f5usolekut<\/button>\n\t\t\t        <\/div>\n\t\t\t    <\/div>\n\t\t\t<\/div>\n<\/div>\n<h6>Video 1. Erinevate orbitaalide kujud kahel esimesel energiatasemel. Allikas: <a title=\"\" href=\"https:\/\/www.youtube.com\/watch?v=VfBcfYR1VQo\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/www.youtube.com\/watch?v=VfBcfYR1VQo\"><span style=\"color: #1155cc;\">https:\/\/www.youtube.com\/watch?v=<\/span><\/a><a href=\"https:\/\/www.youtube.com\/watch?v=VfBcfYR1VQo\"><span style=\"color: #1155cc;\">VfBcfYR1VQo<\/span><\/a><\/h6>\n<p>Vaatame, kuidas orbitaalid t\u00e4ituvad elektronidega. Teises perioodis on s\u00fcsiniku aatom j\u00e4rjenumbriga 6, mis n\u00e4itab tuumalaengut ja ka elektronide koguarvu aatomis. 1s-orbitaalil on 2 elektroni, seej\u00e4rel 2s-orbitaalil 2 elektroni ja kolmel 2p-orbitaalil ka 2 elektroni. Iga kast skeemil t\u00e4histab \u00fchte orbitaali ning t\u00e4itub maksimaalselt kahe elektroniga. 2p orbitaalid t\u00e4ituvad \u00fchtlaselt samapidi spinnidega elektronidega. S\u00fcsiniku aatomi korral j\u00e4\u00e4b \u00fcks <em>p<\/em>\u2013 orbitaal t\u00fchjaks. Viimase kihi elektronid (s\u00fcsiniku korral 2s ja 2p orbitaalil asetsevad elektronid) saavad osaleda keemiliste sidemete moodustamises. N\u00e4ed, et s\u00fcsiniku aatom saab liita maksimaalselt neli elektroni. Samas v\u00f5ib s\u00fcsinik keemilise sideme moodustamisel ka k\u00f5ik viimase kihi elektronid loovutada. Joonisel 3 on toodud elektronide t\u00e4itumise j\u00e4rjekord s\u00fcsiniku aatomis. Pane t\u00e4hele, et joonisel on orbitaalid kindlal energiatasemel, esimese kihi orbitaal on madalama energiaga ning teise kihi orbitaal on juba m\u00f5nev\u00f5rra suurema energiaga.<\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"600\" height=\"432\" class=\"wp-image-131 aligncenter\" style=\"width: 556px; height: 400px;\" title=\"c_aatomi_orbitaalide_taitumine_elektronidega.gif\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/c_aatomi_orbitaalide_taitumine_elektronidega.gif\" alt=\"pilt\"><\/p>\n<h6 style=\"text-align: center;\">Joonis 3.\u00a0S\u00fcsiniku aatomi ruutskeem ja orbitaalide t\u00e4itumine elektronidega<\/h6>\n<p>Kolmandas elektronkihis on juba kolm alakihti ja kolme erinevat t\u00fc\u00fcpi orbitaale:\u00a0<i>s<\/i>, <i>p<\/i>\u00a0ja <i>d<\/i>. <em>d<\/em><i>\u2013<\/i>alakihis on\u00a0viis\u00a0orbitaali, j\u00e4relikult mahutab d-alakiht\u00a0\u00a0kokku 10 elektroni.<\/p>\n<p>Niisiis, esimese kolme elektronkihi vahel jaotuvad elektronid j\u00e4rgnevalt:<\/p>\n<ol>\n<li>elektronkihis saab olla kuni 2 elektroni, mis asetsevad 1s-orbitaalil;<\/li>\n<li>elektronkihis saab olla kuni 8 elektroni, 2 elektroni 2s- ja 6 elektroni 2p-orbitaalidel;<\/li>\n<li>elektronkihis saab olla kuni 18 elektroni, 2 elektroni 3s-orbitaalil, 6 elektroni 3p- ja 10 elektroni 3d-orbitaalidel.<\/li>\n<\/ol>\n<p>Elektronide paiknemist aatomi elektronkihtidel saab lihtsustatult v\u00e4ljendada elektronskeemi, t\u00e4psemalt aga elektronvalemi abil. N\u00e4iteks s\u00fcsiniku korral on elektronskeem ja elektronvalem j\u00e4rgmised:<\/p>\n<p style=\"margin-left: 40px;\"><img loading=\"lazy\" decoding=\"async\" width=\"748\" height=\"268\" class=\"alignnone wp-image-130\" style=\"width: 279px; height: 100px;\" title=\"screenshot_2022-03-15_at_12.18.15.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.18.15.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.18.15.png 748w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.18.15-300x107.png 300w\" sizes=\"auto, (max-width: 748px) 100vw, 748px\"><\/p>\n<p>Elektronskeem n\u00e4itab k\u00f5igepealt summaarset elektronide arvu ja seej\u00e4rel elektronide jaotust elektronkihtides. Elektronvalemis n\u00e4itavad suured numbrid elektronkihi numbrit, t\u00e4hed t\u00e4histavad alamkihtide liike\u00a0ning numbrid astendajates n\u00e4itavad elektronide arvu alamkihtidel.\u00a0\u00a0<\/p>\n<p>Elektronvalemi koostamisel on abiks joonisel 4 toodud skeem, mis n\u00e4itab orbitaalide t\u00e4itumise j\u00e4rjekorda.<\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"376\" height=\"362\" class=\"alignnone wp-image-138\" style=\"width: 200px; height: 193px;\" title=\"elektronide_taitumine_4_1.gif\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/elektronide_taitumine_4_1.gif\" alt=\"pilt\"><\/p>\n<h6 style=\"text-align: center;\">Joonis 4.\u00a0Orbitaalide t\u00e4itumise j\u00e4rjekord<\/h6>\n<p><\/p><div class=\"accordion mb-3\">\n        <div class=\"accordion-item accordion-item--white\">\n        <h2 class=\"accordion-header\" id=\"accordion-69d5d36fb9dd3-heading\">\n            <button class=\"accordion-button collapsed\" type=\"button\" data-bs-toggle=\"collapse\" data-bs-target=\"#accordion-69d5d36fb9dd3-collapse\" aria-expanded=\"true\" aria-controls=\"accordion-69d5d36fb9dd3-collapse\">\u00dclesanne 1<\/button>\n        <\/h2>\n        <div id=\"accordion-69d5d36fb9dd3-collapse\" class=\"accordion-collapse collapse\" aria-labelledby=\"accordion-69d5d36fb9dd3-heading\">\n            <div class=\"accordion-body\">\n\n\n<div class=\"h5p-iframe-wrapper\"><div class=\"video-placeholder-wrapper video-placeholder-wrapper--fixed\" style=\"height: 366px;\">\n\t\t\t    <div class=\"video-placeholder d-flex justify-content-center align-items-center\">\n\t\t\t        <div class=\"overlay text-white p-2 w-100 text-center d-block justify-content-center align-items-center\">\n\t\t\t            <div>Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega.<\/div>\n\t\t\t            <button class=\"btn btn-secondary btn-sm mt-1 consent-change\">Muuda n\u00f5usolekut<\/button>\n\t\t\t        <\/div>\n\t\t\t    <\/div>\n\t\t\t<\/div>\n<\/div>\n\n\n<p><\/p><\/div>\n        <\/div>\n        <\/div>\n    <\/div>\n<h2>Keemiliste elementide omadused<\/h2>\n<p>Perioodilisustabelis on elemendid reastatud tuumalaengu kasvu j\u00e4rjekorras. Elemendid asetsevad nii, et need peegeldavad ka aatomiehituse ning omaduste muutust perioodis ja r\u00fchmas. Teades elemendi asukohta perioodilisuse s\u00fcsteemis, saame teha j\u00e4reldusi tema omaduste kohta.<\/p>\n<h5><a href=\"https:\/\/youtu.be\/MnXnHY4tOjA\" target=\"_blank\" rel=\"noopener\"><img loading=\"lazy\" decoding=\"async\" width=\"168\" height=\"130\" class=\"alignnone wp-image-81\" style=\"width: 50px; height: 39px; float: right;\" title=\"screenshot_2022-02-11_at_13.55.20.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-02-11_at_13.55.20.png\" alt=\"video\"><\/a><a title=\"\" href=\"https:\/\/youtu.be\/MnXnHY4tOjA\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/youtu.be\/MnXnHY4tOjA\">Liht- ja liitainete, metalliliste ja mittemetalliliste elementide kohta vaata siit.<\/a><\/h5>\n<h3>Aatomraadius<\/h3>\n<p>Elektronkihtide arv suureneb r\u00fchmades\u00a0\u00fclalt alla ja seet\u00f5ttu ka aatomraadius suureneb. Perioodis vasakult paremale aatomraadius v\u00e4heneb, sest tuumalaeng suureneb ja tuuma m\u00f5ju elektronkihitidele on suurem. Perioodilisuse s\u00fcsteemis aatomraadius kasvab diagonaalselt \u00fclevalt paremalt alla vasakule (joonis 5).<\/p>\n<h6 style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"2038\" height=\"932\" class=\"wp-image-137 aligncenter\" style=\"width: 800px; height: 366px;\" title=\"screenshot_2022-03-25_at_13.43.14.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14.png 2038w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14-300x137.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14-1024x468.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14-768x351.png 768w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14-1536x702.png 1536w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_13.43.14-1920x878.png 1920w\" sizes=\"auto, (max-width: 2038px) 100vw, 2038px\">Joonis 5. Aatomraadiuse muutus perioodilisuse s\u00fcsteemis<\/h6>\n<h3>Metalliliste elementide omadused<\/h3>\n<h5>R\u00fchmas \u00fclevalt alla metallilised omadused tugevnevad.<\/h5>\n<p>Metallilistel elementidel on v\u00e4liskihtidel suhteliselt v\u00e4he elektrone. Aatomi tuum ei hoia elektrone eriti tugevalt kinni ja seet\u00f5ttu loovutavad metallilised elemendid kergesti elektrone.\u00a0R\u00fchmas \u00fclevalt alla elektronkihtide arv suureneb ja seet\u00f5ttu tuuma m\u00f5ju viimasele elektronkihile v\u00e4heneb ning metall loovutab kergemini elektrone.\u00a0Element on seda metallilisem, mida lihtsamalt see loovutab elektrone. Seet\u00f5ttu r\u00fchmas \u00fclevalt alla metallilised omadused tugevnevad. T\u00fc\u00fcpilisteks n\u00e4ideteks on I A ja II A r\u00fchma metallid. I A r\u00fchma metallidel on viimasel <i>s<\/i>-orbitaalil ainult \u00fcks elektron, see loovutatakse kergesti ja tekib palju stabiilsem metallikatioon v\u00f5rreldes metalliaatomiga.<\/p>\n<p style=\"margin-left: 40px;\">Na \u2013 e<sup>\u2013 <\/sup><span lang=\"et\" style=\"background: white;\">\u2192 Na<\/span><sup><span lang=\"et\" style=\"background: white;\">+<\/span><\/sup><\/p>\n<h5>A-r\u00fchma elementide maksimaalne ok\u00fcdatsiooniaste \u00fchendis on v\u00f5rdne r\u00fchma numbriga.<\/h5>\n<p>Elektronide loovutamisel k\u00e4itub metalli aatom redutseerijana ja metalli oks\u00fcdatsiooniaste kasvab. Kui on loovutatud k\u00f5ik v\u00e4liskihi elektronid, siis on elemendil maksimaalne oks\u00fcdatsiooniaste. I A ja II A r\u00fchma metallid loovutavad k\u00f5ik oma v\u00e4liskihi elektronid. Seet\u00f5ttu n\u00e4itab I A ja II A r\u00fchma metallide r\u00fchmanumber nende maksimaalset\u00a0oks\u00fcdatsiooniastet.<\/p>\n<p>I A r\u00fchma metallidel on \u00fchendites oks\u00fcdatsiooniaste alati<b> I<\/b>, n\u00e4iteks NaOH, LiCl, KBr \u00fchendites:<\/p>\n<p style=\"margin-left: 40px;\"><img loading=\"lazy\" decoding=\"async\" width=\"312\" height=\"90\" class=\"alignnone wp-image-134\" style=\"width: 104px; height: 30px;\" title=\"screenshot_2022-03-15_at_12.36.54.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.36.54.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.36.54.png 312w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.36.54-300x87.png 300w\" sizes=\"auto, (max-width: 312px) 100vw, 312px\"><\/p>\n<p>II A r\u00fchma elementide maksimaalne oks\u00fcdatsiooniaste on alati <b>II<\/b>, Mg(OH)<sub>2<\/sub>, BaCl<sub>2<\/sub>, CaO:<\/p>\n<p style=\"margin-left: 40px;\"><img loading=\"lazy\" decoding=\"async\" width=\"312\" height=\"90\" class=\"alignnone wp-image-135\" style=\"width: 104px; height: 30px;\" title=\"screenshot_2022-03-15_at_12.37.07.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.37.07.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.37.07.png 312w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.37.07-300x87.png 300w\" sizes=\"auto, (max-width: 312px) 100vw, 312px\"><span style=\"font-size: revert; font-weight: var(--bs-body-font-weight); text-align: var(--bs-body-text-align);\">.<\/span><\/p>\n<p>Teades elemendi oks\u00fcdatsiooniastet \u00fchendis, saad kirjutada vastavaid oksiidide, h\u00fcdroksiidide ja soolade valemeid.<\/p>\n<h3>Mittemetalliliste elementide omadused<\/h3>\n<h5><a href=\"https:\/\/ptable.com\/#Properties\" target=\"_blank\" rel=\"noopener\"><img loading=\"lazy\" decoding=\"async\" width=\"168\" height=\"130\" class=\"alignnone wp-image-81\" style=\"width: 50px; height: 39px; float: right;\" title=\"screenshot_2022-02-11_at_13.55.20.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-02-11_at_13.55.20.png\" alt=\"video\"><\/a><a title=\"\" href=\"https:\/\/ptable.com\/#Properties\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/ptable.com\/#Properties\">Erinevaid trende perioodilisuse tabelis, elementide omadusi ning t\u00fc\u00fcpilisi valemeid saad vaadata v\u00e4ga p\u00f5nevas animeeritud perioodilisuse tabelis.<\/a><span lang=\"et\" style=\"background: white;\">\u00a0<\/span><\/h5>\n<p>Mittemetallilised elemendid paiknevad perioodilisuse tabelis paremal. Nende elementide aatomituuma m\u00f5ju v\u00e4liskihi elektronidele on tugev, mis tingib suhteliselt v\u00e4ikse aatomraadiuse. K\u00f5ige mittemetallilisem element on VII A r\u00fchma element fluor (F). Mittemetalli aatomid pigem liidavad elektrone, et t\u00e4ita osaliselt t\u00e4itunud v\u00e4line elektronkiht. Elektronide liitmisel mittemetall k\u00e4itub oks\u00fcdeerijana ja sellest tekib mittemetalli anioon. Elektronide liitmisel oks\u00fcdatsiooniaste kahaneb:<\/p>\n<p style=\"margin-left: 40px;\">Cl + e<sup>\u2013 <\/sup><span lang=\"et\" style=\"background: white;\">\u2192 Cl<\/span><sup><span lang=\"et\" style=\"background: white;\">\u2013<\/span><\/sup><br>S + 2e<sup>\u2013 <\/sup><span lang=\"et\" style=\"background: white;\">\u2192 S<\/span><sup><span lang=\"et\" style=\"background: white;\">2-<\/span><\/sup><span lang=\"et\" style=\"background: white;\">.<\/span><\/p>\n<p><span lang=\"et\" style=\"background: white;\">Enamik mittemetallide aatomeid saavad ka elektrone loovutada, st k\u00e4ituvad ka redutseerijana.<\/span><\/p>\n<h5>Mittemetallide minimaalne oks\u00fcdatsiooniaste on<br>\u2013 (8 \u2013 r\u00fchma number).<\/h5>\n<p><span lang=\"et\" style=\"background: white;\">Mittemetallide minimaalne oks\u00fcdatsiooniaste on v\u00f5rdne v\u00e4liskihi orbitaalide t\u00fchjade kohtade arvuga. Kokku mahub v\u00e4liskihile\u00a0 8 elektroni. Elemendi r\u00fchmanumber n\u00e4itab elektronide arvu v\u00e4liskihil, seega puuduolevate elektronide arvu saame leida 8 \u2013 elemendi r\u00fchmanumber. <\/span>Seega on mittemetallide minimaalne oks\u00fcdatsiooniaste \u2013 (8 \u2013 r\u00fchma number). <span lang=\"et\" style=\"background: white;\">Minimaalne oks\u00fcdatsiooniaste on n\u00e4iteks \u00fchendites metallidega.<\/span><\/p>\n<p style=\"margin-left: 40px;\"><img loading=\"lazy\" decoding=\"async\" width=\"422\" height=\"90\" class=\"alignnone wp-image-136\" style=\"width: 141px; height: 30px;\" title=\"screenshot_2022-03-15_at_12.37.32.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.37.32.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.37.32.png 422w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-15_at_12.37.32-300x64.png 300w\" sizes=\"auto, (max-width: 422px) 100vw, 422px\"><\/p>\n<p><\/p><div class=\"accordion mb-3\">\n        <div class=\"accordion-item accordion-item--white\">\n        <h2 class=\"accordion-header\" id=\"accordion-69d5d36fb9de5-heading\">\n            <button class=\"accordion-button collapsed\" type=\"button\" data-bs-toggle=\"collapse\" data-bs-target=\"#accordion-69d5d36fb9de5-collapse\" aria-expanded=\"true\" aria-controls=\"accordion-69d5d36fb9de5-collapse\">\u00dclesanne 2<\/button>\n        <\/h2>\n        <div id=\"accordion-69d5d36fb9de5-collapse\" class=\"accordion-collapse collapse\" aria-labelledby=\"accordion-69d5d36fb9de5-heading\">\n            <div class=\"accordion-body\">\n\n\n<div class=\"h5p-iframe-wrapper\"><div class=\"video-placeholder-wrapper video-placeholder-wrapper--fixed\" style=\"height: 366px;\">\n\t\t\t    <div class=\"video-placeholder d-flex justify-content-center align-items-center\">\n\t\t\t        <div class=\"overlay text-white p-2 w-100 text-center d-block justify-content-center align-items-center\">\n\t\t\t            <div>Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega.<\/div>\n\t\t\t            <button class=\"btn btn-secondary btn-sm mt-1 consent-change\">Muuda n\u00f5usolekut<\/button>\n\t\t\t        <\/div>\n\t\t\t    <\/div>\n\t\t\t<\/div>\n<\/div>\n\n\n<p><\/p><\/div>\n        <\/div>\n        <\/div>\n    <\/div>","protected":false},"excerpt":{"rendered":"<p>Milleks peaksime teadma aatomi ehitust? Ained koosnevad erinevatest\u00a0aatomitest, molekulidest v\u00f5i ioonidest. Aatomiehitus ja aatomitevahelised\u00a0sidemed m\u00e4\u00e4ravad aine omadused. J\u00e4rgnevast videost saadki tuletada meelde aatomiehituse p\u00f5hiteadmised ja aatomiehituse seosed perioodilisustabeliga. Kolmandate osapoolte sisu n\u00e4gemiseks palun n\u00f5ustu k\u00fcpsistega. Muuda n\u00f5usolekut Allikas:\u00a0https:\/\/youtu.be\/DTwdlVdi1pM T\u00e4nap\u00e4evase aatomimudeli &#8230;<\/p>\n","protected":false},"author":269,"featured_media":0,"parent":0,"menu_order":0,"comment_status":"closed","ping_status":"closed","template":"","meta":{"_acf_changed":false,"inline_featured_image":false,"footnotes":""},"class_list":["post-26","page","type-page","status-publish","hentry"],"acf":[],"_links":{"self":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/26","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages"}],"about":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/types\/page"}],"author":[{"embeddable":true,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/users\/269"}],"replies":[{"embeddable":true,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/comments?post=26"}],"version-history":[{"count":10,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/26\/revisions"}],"predecessor-version":[{"id":1243,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/26\/revisions\/1243"}],"wp:attachment":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/media?parent=26"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}