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Lewis Dot Structure For Germanium

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Last Updated: 22 October 2020

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Draw Lewis dot structures and resonance structures for following. Some hints are give. {matheq}{CO2}{endmatheq} plus two more dots for each of {matheq}\textrm{:O::C::O:}{endmatheq} {matheq}{O}{endmatheq} {matheq}{NO2}{endmatheq} {matheq}\textrm{:O::C::O:}{endmatheq} {matheq}\textrm{:O::C::O:}{endmatheq} notice that some of resonance structures may not satisfy the octet rule. {matheq}\textrm{:O::C::O:}{endmatheq} molecule has an odd number of electrons, and the octet rule cannot be satisfied for nitrogen atom. Draw resonance structures of {matheq}\textrm{:O::C::O:}{endmatheq} resonance structure are shown on the right here. Note that only locations of double and single bonds change here. What are formal charges for {matheq}\textrm{:O::C::O:}{endmatheq} atoms? What are formal charges for oxygen atoms that are single bond and double bond to {matheq}\textrm{:O::C::O:}{endmatheq} respectively? Please work these numbers out. Formal charges: {matheq}\textrm{:O::C::O:}{endmatheq} + 1; {matheq}\textrm{:O::C::O:}{endmatheq} 0; {matheq}\textrm{:O::C::O:}{endmatheq} most stable structure has least formal charge. In a stable structure, adjacent atoms should have formal charges of opposite signs. More stable structure, more it contributes to the resonance structure of molecule or ion. All three structures above are the same, only the double bond rotates.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions

Formal charge rules

Draw Lewis dot structure for {matheq}{SO2}{endmatheq} {matheq}\mathrm{ :\overset{\Large{..}}O : :\overset{\Large{..}}S : :\overset{\Large{..}}O :}{endmatheq} put all atoms together to make a molecule and check to see if it satisfies the octet rule. {matheq}\begin{alignat}{1} :&\overset{\Large{..}}{ O} : :&&\overset{\Large{..}}{ S} : :&&\overset{\Large{..}}{ O} : &&\textrm{ <= octet rule not satisfied}\ &\,0 &&\,0 &&\,0 &&\textrm{ formal charge} \end{alignat}{endmatheq} adjusts bonding electrons SO that octet rules apply to all atoms. {matheq}\begin{alignat}{1} &:\underset{\Large{..}}{\overset{\Large{..}}{ O}} &&:\overset{\Large{..}}{ S} : :&&\overset{\Large{..}}{ O} : &&\textrm{ <- octet rule satisfied}\ &\,{-1} &&\,{+1} &&\,0 &&\textrm{ formal charge} \end{alignat}{endmatheq} since leave {matheq}{O}{endmatheq} has 6 unshared plus 2 shared electrons, it effectively has 7 electrons for 6 - valence - electron {matheq}{O}{endmatheq} and thus its formal charge is - 1. The formal charge for {matheq}{O}{endmatheq} = 6 - 6 - = - 1. The formal charge for {matheq}{S}{endmatheq} = 6 - 2 - = + 1. There is yet another structure that does not satisfy the octet rule, but it's reasonable structure:

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions.

* Please keep in mind that all text is machine-generated, we do not bear any responsibility, and you should always get advice from professionals before taking any actions

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