Abstract
Lewis structures or Lewis dot structures show the way in which the atoms in the molecule are linked to each other, as well as the arrangement of valent electrons of all atoms in the molecule. Applying simple rules, which are more in accordance with the molecular orbital theory, the dot structures even of complicated molecules can be written with ease. If beside those rules we apply the VSEPR theory, we can deduce the structure and the shape of the molecule, and from the structure of the molecule, we can deduce the hybridization of the atoms. When we calculate the formal charges, from their values we can conclude if the structure is stable or more stable resonance structures exist. If the molecule in consideration contains atoms from the third period and on, in that case, more stable structures can be obtained by the formation of multiple bonds and expanded valence shell. In the present paper, the application of the above mentioned is shown step by step on several examples. This work is licensed under a Creative Commons Attribution 4.0 International License.
Highlights
Lewis dot structures show the way in which the atoms in the molecule are linked to each other
which are more in accordance with the molecular orbital theory
even of complicated molecules can be written with ease
Summary
Sažetak Lewisove strukture ili elektronske strukturne formule prikazuju na koji su način atomi u molekuli međusobno povezani te raspored valentnih elektrona svih atoma u molekuli. 3. Atomi nemetala koji se ne razlikuju znatno po elektronegativnosti međusobno se povezuju tako da se nespareni elektroni različitih atoma povezuju tvoreći zajedničke, vezne parove – kovalentnu vezu (slika 1). 4. Ako se atomi znatno razlikuju po elektronegativnosti (razlika relativnih koeficijenata elektronegativnosti prema Linusu Paulingu ≥ 1,7),[4,5] elektroni se premještaju s jednog atoma na drugi tako da nastaju suprotno nabijeni ioni, koji se zatim povezuju elektrostatskim silama – ionskom vezom (slika 2). U molekulama vodika, H2, klora, Cl2, klorovodika, HCl, vode, H2O, i klorovog(I) oksida ili diklorova monoksida (Cl2O), čije su Lewisove strukturne formule prikazane na slici 1 te višestruke veze, koje čine dva, odnosno tri zajednička elektronska para zbog čega ih zovemo dvostrukom i trostrukom vezom Razlikujemo jednostruku kovalentnu vezu koja postoji npr. u molekulama vodika, H2, klora, Cl2, klorovodika, HCl, vode, H2O, i klorovog(I) oksida ili diklorova monoksida (Cl2O), čije su Lewisove strukturne formule prikazane na slici 1 te višestruke veze, koje čine dva, odnosno tri zajednička elektronska para zbog čega ih zovemo dvostrukom i trostrukom vezom
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