SO2 Lewis Structure - Sulfur Dioxide

This chemistry video tutorial explains how to draw the lewis structure of SO2 also known as Sulfur Dioxide. It discusses the molecular geometry, bond angle, hybridization and formal charges of the SO2 molecule. It also answers the question if SO2 is polar or nonpolar?

Molecular Geometry - Free Formula Sheet:

Chemistry 1 Final Exam Review:

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How To Draw Lewis Structures:

VSEPR Theory:

Molecular Geometry:

Lewis Dot Structures:

Lewis Structures of Ionic Compounds:

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Octet Rule Exceptions:

Resonance Structures:

Polar and Nonpolar Molecules:

Formal Charge Calculations:

Lewis Structures - Mega Review:

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Hybridization of Atomic Orbitals:

Molecular Orbital Theory:

Dipole Dipole Forces of Attraction:

Hydrogen Bonding:

Unit Cell Chemistry:

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Final Exams and Video Playlists:

Full-Length Videos and Worksheets:

[reem]

I was confused too at first, because sulfur isn't obeying to the octet rule and has 10 electrons instead of 8, turns out S and other atoms can hold more than 8 electrons, such as S, P, Si, Cl. This occurs due to the presence of d orbitals that can accommodate the extra electrons.
Also atoms can have less than octet of electrons such as: H(2e), Be(4e), Al(6e), B(6e).

[datnigwr]

i wish this guy was my chemistry teacher

[mickymikemike]

I can't thank you enough, really, your video helps me go through the chemistry exam

[RGUTIERREZable]

Awesome. Would like to know why multiples of 8?

[saravanakumark]

Suggestion for A video; please make chemistry videos from the syllabus of IIT JAM exam.. One of the toughest exams in India.. Please..

[kanaeroseweld]

Does this mean every time Sulfur is the central atom, it will always have 1 lone pair?

[celinkosixolani]

Okay, I'm confused, isn't it sulphur two lone pairs and 2 bonding electrons, and oxygen too has two and two bonding electrons

And we cannot bond lone pairs to those single bonding electrons?

[SophiaWai]

I'm confused. Please help!


If the Lewis structure of SO2 should be S being doublely bonded to each of O atom rather than S being doublely bonded to just one O atom because the first structure is more stable, then why is the similar molecule O3 being doublely bonded to just one O and why can't the structure of O3 be central O being doublely bonded to each of another O atom? According to that formal charge should be the same with the central charge, O=S=O is more stable and suitable structure than O=S-O, then O=O=O meets it while O=O-O doesn't.

[thencfolf]

I don’t even know what this video is about






But YouTube recommended it to me, so okay :)

[عبيرأبومياله]

i wanna ask question ..How we can know if this structure is more stabilise?

[fatmasairafi]

How can I contact u i have a question

[AbhinavKumar-vfmz]

Hello sir I need a help I want to know that what is So13 pls help....🙏🙏🙏

[cookiesncream_]

didn’t know about not following the octet rule o-o

[graywolf]

How did you know that sulfur was the central atom?

[element]

Sulfur's octet is overfilled here