{"id":44,"date":"2024-04-04T07:30:18","date_gmt":"2024-04-04T04:30:18","guid":{"rendered":"https:\/\/sisu.ut.ee\/huvitavkeemia\/54-mittemetallide-keemilised-omadused\/"},"modified":"2025-04-22T11:25:17","modified_gmt":"2025-04-22T08:25:17","slug":"54-mittemetallide-keemilised-omadused","status":"publish","type":"page","link":"https:\/\/sisu.ut.ee\/huvitavkeemia\/54-mittemetallide-keemilised-omadused\/","title":{"rendered":"5.4. Mittemetallide keemilised omadused"},"content":{"rendered":"<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Mittemetallilised omadused on seotud aatomite v\u00f5imega liita elektrone. Mittemetallide aatomid on v\u00f5rreldes metalliaatomitega suhteliselt v\u00e4ikesed (vaata joonist 1). <\/span><\/span><\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1035\" height=\"415\" class=\"alignnone wp-image-315\" style=\"width: 800px; height: 321px;\" title=\"thumbnail_image004.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/thumbnail_image004.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/thumbnail_image004.png 1035w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/thumbnail_image004-300x120.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/thumbnail_image004-1024x411.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/thumbnail_image004-768x308.png 768w\" sizes=\"auto, (max-width: 1035px) 100vw, 1035px\"><\/p>\n<h6 style=\"text-align: center;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">Joonis 1. Peaalar\u00fchma aatomiraadiused pikomeetrites. <\/span><\/span>Allikas:\u00a0<a title=\"\" href=\"https:\/\/ptable.com\/?lang=et#Properties\/Radius\/Calculated\" target=\"_blank\" rel=\"noopener\" data-url=\"https:\/\/ptable.com\/?lang=et#Properties\/Radius\/Calculated\">https:\/\/ptable.com\/?lang=et#Properties\/Radius\/Calculated<\/a><\/h6>\n<h5>Mittemetallide aatomid v\u00f5ivad elektrone nii liita kui ka loovutada.<\/h5>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">V\u00e4liskihis on mittemetallidel elektrone palju rohkem\u00a0(neli kuni kaheksa) kui metalliaatomitel. Allpool on toodud\u00a0 m\u00f5nede mittemetallide ja metallide elektronvalmid.\u00a0Punaselt on m\u00e4rgitud v\u00e4liskihid ja ja neil paiknevad elektronid. V\u00e4liskihi elektronid saavad osaleda keemilise sideme moodustamises. Element soovib saavutada olukorda, kus v\u00e4liskiht on t\u00e4itunud maksimaalselt kaheksa elektroniga ehk saavutanud v\u00e4\u00e4risgaasidega sarnase oleku (okteti reegel).\u00a0Elektronvalemitest n\u00e4eme, et s\u00fcsinik v\u00f5ib liita maksimaalselt 4 elektroni, aga samas saab ka loovutada maksimaalselt 4 elektroni.<b> <\/b>Seega erinevalt metallidest v\u00f5ivad mittemetalliaatomid elektrone nii loovutada kui ka liita.<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1067\" height=\"533\" class=\"alignnone wp-image-316\" style=\"width: 450px; height: 225px;\" title=\"elektron_kihid.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/elektron_kihid.png\" alt=\"Elektronkihid\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/elektron_kihid.png 1067w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/elektron_kihid-300x150.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/elektron_kihid-1024x512.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/elektron_kihid-768x384.png 768w\" sizes=\"auto, (max-width: 1067px) 100vw, 1067px\"><\/p>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Aatomite v\u00e4ikeste m\u00f5\u00f5tmete t\u00f5ttu on tuumalaengu m\u00f5ju v\u00e4liskihi elektronidele k\u00fcllaltki suur ja seet\u00f5ttu hoitakse v\u00e4liskihi elektrone aatomis k\u00f5vasti kinni ning mittemetalliaatomitele pole eriti\u00a0iseloomulik neid loovutada. V\u00e4ga paljudes reaktsioonides mittemetalliaatomid pigem seovad elektrone. Mittemetall on tavaliselt seda aktiivsem, mida elektronegatiivsem on vastav element. Elektronegatiivsus on suurus, mis iseloomustab keemilise elemendi aatomi v\u00f5imet keemilise sideme moodustamisel t\u00f5mmata enda poole \u00fchist elektronpaari. Elektronegatiivsuse v\u00e4\u00e4rtus on seotud aatomiehitusega ning sooviga saavuta v\u00e4lisele elektronkihile maksimaalselt kaheksa elektroni. Enamik mittemetallidel on kaheksast v\u00e4lise elektronkihi elektronist puudu ainult m\u00f5ni elektron, seega nad hea meelega liidavad elektrone. Aatomite elektronegatiivsuse v\u00e4\u00e4rtused on toodud joonisel 2. <\/span><\/span><\/p>\n<h6 style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1664\" height=\"862\" class=\"alignnone wp-image-314\" style=\"width: 800px; height: 414px;\" title=\"screenshot_2022-03-25_at_10.57.53.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_10.57.53.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_10.57.53.png 1664w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_10.57.53-300x155.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_10.57.53-1024x530.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_10.57.53-768x398.png 768w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-25_at_10.57.53-1536x796.png 1536w\" sizes=\"auto, (max-width: 1664px) 100vw, 1664px\"><br><span lang=\"ET\"><span style=\"line-height: 107%;\">Joonis 2. Aatomite elektronegatiivsuse v\u00e4\u00e4rtused<\/span><\/span><\/h6>\n<h5><span lang=\"ET\"><span style=\"line-height: 107%;\">Mittemetallidest k\u00f5ige aktiivsemad on halogeenid ja\u00a0 k\u00f5ige v\u00e4hem aktiivsed on v\u00e4\u00e4risgaasid.<\/span><\/span><\/h5>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Mittemetallidest k\u00f5ige aktiivsemad on halogeenid (asuvad VIIA r\u00fchmas). K\u00f5ige suurema aktiivsusega neist on fluor (F<sub>2<\/sub>). Fluor reageerib praktiliselt k\u00f5ikide teiste lihtainetega juba toatemperatuuril.<\/span><\/span><span lang=\"ET\"><span style=\"line-height: 107%;\"> Mittemetallilised omadused ja nende keemiline aktiivsus oks\u00fcdeerjana suurenevad r\u00fchmas alt \u00fcles\u00a0ning perioodis vasakult paremale. <\/span><\/span><\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1548\" height=\"888\" class=\"alignnone wp-image-310\" style=\"width: 700px; height: 402px;\" title=\"screenshot_2022-03-24_at_13.31.57.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.31.57.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.31.57.png 1548w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.31.57-300x172.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.31.57-1024x587.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.31.57-768x441.png 768w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.31.57-1536x881.png 1536w\" sizes=\"auto, (max-width: 1548px) 100vw, 1548px\"><\/p>\n<p>\u00a0<\/p>\n<h6 style=\"text-align: center;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">Joonis 3. Mittemetallide omaduste muutus perioodiliuss\u00fcsteemis<\/span><\/span><\/h6>\n<h5>Mittemetallilised omadused suurenevad perioodis vasakult paremale ja r\u00fchmas alt \u00fcles.<\/h5>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Teiste mittemetallide (nt N<sub>2<\/sub>, H<sub>2<\/sub>) reageerimisel metallide ja teiste mittemetallidega vajavad reaktsioonid kuumutamist v\u00f5i katal\u00fcsaatoreid. <\/span><\/span>Mittemetallilised omadused suurenevad perioodis vasakult paremale ja r\u00fchmas alt \u00fcles.<\/p>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">K\u00f5ige v\u00e4hem aktiivsed mittemetallid on VIIIA r\u00fchma elemendid \u2013 v\u00e4\u00e4risgaasid.<\/span><\/span><\/p>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Metallidega reageerimisel k\u00e4ituvad mittemetallid oks\u00fcdeerijatena, liites endaga metalli aatomite poolt loovutatavad elektronid. N\u00e4iteks v\u00e4\u00e4vli reaktsioonil naatriumiga v\u00e4\u00e4vel seob elektrone ja Na-aatomid loovutavad elektrone (joonis 4).<\/span><\/span><\/p>\n<h5><span lang=\"ET\"><span style=\"line-height: 107%;\">Metallidega reageerimisel k\u00e4ituvad mittemetallid oks\u00fcdeerijatena.<\/span><\/span><\/h5>\n<p style=\"margin-left: 40px;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">2Na + S <\/span><\/span><span lang=\"EN-US\"><span style=\"background: white;\"><span style=\"line-height: 107%;\"><span style=\"color: black;\">\u2192<\/span><\/span><\/span><\/span> <span lang=\"ET\"><span style=\"line-height: 107%;\">Na<sub>2<\/sub>S<\/span><\/span><\/p>\n<p style=\"margin-left: 40px;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">Na \u2013 1e<sup>\u2013<\/sup> <\/span><\/span><span lang=\"EN-US\"><span style=\"background: white;\"><span style=\"line-height: 107%;\"><span style=\"color: black;\">\u2192<\/span><\/span><\/span><\/span><span lang=\"ET\"><span style=\"line-height: 107%;\"> Na<sup>+<\/sup>\u00a0\u00a0 redutseerija oks\u00fcdeerub<\/span><\/span><\/p>\n<p style=\"margin-left: 40px;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">S + 2e<sup>\u2013<\/sup> <\/span><\/span><span lang=\"EN-US\"><span style=\"background: white;\"><span style=\"line-height: 107%;\"><span style=\"color: black;\">\u2192<\/span><\/span><\/span><\/span><span lang=\"ET\"><span style=\"line-height: 107%;\"> S<sup>2-<\/sup> oks\u00fcdeerija redutseerub<\/span><\/span><\/p>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Sel viisil reageerides saavutavad mittemetallid ja metallid p\u00fcsiva oleku \u2013 v\u00e4liskiht on maksimaalselt t\u00e4itunud kaheksa elektroniga (vt joonist 4).<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"1498\" height=\"888\" class=\"alignnone wp-image-311\" style=\"width: 700px; height: 415px;\" title=\"screenshot_2022-03-24_at_13.39.30.png\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.39.30.png\" alt=\"pilt\" srcset=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.39.30.png 1498w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.39.30-300x178.png 300w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.39.30-1024x607.png 1024w, https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/screenshot_2022-03-24_at_13.39.30-768x455.png 768w\" sizes=\"auto, (max-width: 1498px) 100vw, 1498px\"><\/p>\n<h6 style=\"text-align: center;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">Joonis 4. Na<sub>2<\/sub>S tekkimine aatomite tasandil. Naatriumiaatomid loovutavad elektrone ja tekivad Na<sup>+<\/sup>-katioonid. V\u00e4\u00e4vliaatom seob elektrone,\u00a0 tekivad S<sup>2-<\/sup>-anioonid.<\/span><\/span><\/h6>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">V\u00e4\u00e4vli ja naatriumi reaktsioon toimub juba toatemepratuuril segu uhmerdamisel. Videost (joonis 5) on n\u00e4ha, et h\u00f5\u00f5rdumise tulemusena suurendatakse kokkupuutepinda ja segu s\u00fcttib p\u00f5lema.<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"600\" height=\"338\" class=\"alignnone wp-image-312\" title=\"na_ja_vaavli_reaktsioon.gif\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/na_ja_vaavli_reaktsioon.gif\" alt=\"pilt\"><\/p>\n<h6 style=\"text-align: center;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">Joonis 5. Naatriumi ja v\u00e4\u00e4vli reageerimine, saadusena tekib naatriumsulfiid (Na<sub>2<\/sub>S). V\u00e4\u00e4vel k\u00e4itub oks\u00fcdeerijana ja naatrium redutseerijana.<\/span><\/span><\/h6>\n<p><span lang=\"ET\"><span style=\"line-height: 107%;\">Samas v\u00f5ivad mittemetallid loovutada elektrone reageerimisel m\u00f5ne endast aktiivsema mittemetalliga, st k\u00e4ituda redutseerijana. N\u00e4iteks regeerimisel hapnikuga on v\u00e4\u00e4vel redutseerija: <\/span><\/span><\/p>\n<p style=\"margin-left: 40px;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">S (t) + O<sub>2<\/sub>(g) \u2192 SO<sub>2<\/sub>(g)<\/span><\/span><\/p>\n<p style=\"margin-left: 40px;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">S<sup>0<\/sup> \u2013 4e<sup>\u2013<\/sup> \u2192 S<sup>IV<\/sup> redutseerija oks\u00fcdeerub<\/span><\/span><\/p>\n<p style=\"margin-left: 40px;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">O<sub>2<\/sub><sup>0<\/sup> + 4e<sup>\u2013 <\/sup>\u2192 2 O<sup>-II\u00a0<\/sup>oks\u00fcdeerija redutseerub<\/span><\/span><\/p>\n<p style=\"text-align: center;\"><img loading=\"lazy\" decoding=\"async\" width=\"600\" height=\"688\" class=\"alignnone wp-image-313\" style=\"width: 262px; height: 300px;\" title=\"vaavel_ja_hapnik_vaavli_polemine_sinise_leegiga.gif\" src=\"https:\/\/sisu.ut.ee\/wp-content\/uploads\/sites\/524\/vaavel_ja_hapnik_vaavli_polemine_sinise_leegiga.gif\" alt=\"pilt\"><\/p>\n<h6 style=\"text-align: center;\"><span lang=\"ET\"><span style=\"line-height: 107%;\">Joonis 6. V\u00e4\u00e4vli ja hapniku reaktsioonil k\u00e4itub v\u00e4\u00e4vel redutseerijana. V\u00e4\u00e4vel p\u00f5leb sinaka leegiga, saadusena tekib v\u00e4rvusetu ja m\u00fcrgine gaas v\u00e4\u00e4veldioksiid (SO<sub>2<\/sub>). Hapnikuga reageerimiseks on vaja k\u00f5rgemat temperatuuri ehk kuumutamist.<\/span><\/span><\/h6>\n<p><\/p><div class=\"accordion mb-3\">\n        <div class=\"accordion-item accordion-item--white\">\n        <h2 class=\"accordion-header\" id=\"accordion-69dc02e410fa4-heading\">\n            <button class=\"accordion-button collapsed\" type=\"button\" data-bs-toggle=\"collapse\" data-bs-target=\"#accordion-69dc02e410fa4-collapse\" aria-expanded=\"true\" aria-controls=\"accordion-69dc02e410fa4-collapse\">\u00dclesanne 1<\/button>\n        <\/h2>\n        <div id=\"accordion-69dc02e410fa4-collapse\" class=\"accordion-collapse collapse\" aria-labelledby=\"accordion-69dc02e410fa4-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>Mittemetallilised omadused on seotud aatomite v\u00f5imega liita elektrone. Mittemetallide aatomid on v\u00f5rreldes metalliaatomitega suhteliselt v\u00e4ikesed (vaata joonist 1). Joonis 1. Peaalar\u00fchma aatomiraadiused pikomeetrites. Allikas:\u00a0https:\/\/ptable.com\/?lang=et#Properties\/Radius\/Calculated Mittemetallide aatomid v\u00f5ivad elektrone nii liita kui ka loovutada. V\u00e4liskihis on mittemetallidel elektrone palju rohkem\u00a0(neli kuni &#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-44","page","type-page","status-publish","hentry"],"acf":[],"_links":{"self":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/44","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=44"}],"version-history":[{"count":4,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/44\/revisions"}],"predecessor-version":[{"id":1277,"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/pages\/44\/revisions\/1277"}],"wp:attachment":[{"href":"https:\/\/sisu.ut.ee\/huvitavkeemia\/wp-json\/wp\/v2\/media?parent=44"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}