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# Draw the Lewis structure for each molecule.$$\mathrm{H}_{2} \mathrm{S}$$

## see drawing

Chemical Bonding

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### Video Transcript

okay for this question, we are going to be drawing the Louis structure of H two s. We're gonna start by counting the number of valence electrons we need. So we have to hide regions each with one Valence. Electron plus suffers in the group six. So group is gonna have six valence electrons, which equals a total of eight valence electrons that are open for bonding. A shortcut to determine the number of bonds that there o b is suited. Determine the number of total electrons needed to satisfy the octet rules. Hydrogen is an exception. Where only needs two electrons to satisfy the octet rule. And then we have sulfur needing eight electrons to satisfy its octet rule, which ends up coming out to 12. If we subtract the total number of electrons minus the number of valence electrons available, we end up getting four. Look for electrons that are gonna be shared. And if we divide that by two to make a pair, a pair of electrons equals a bond. So we're gonna have to bonds in our Louis structure. So drawing Louis structure, sulfur is gonna be in the center as there's ah, hydrogen is always on the exterior as there's only one electron to be shared. So sulfur has six valence electrons, so we'll go around to draw six Valence Electron. So we have two openings that the hydrogen can go into. So how did it has won balance? Electron and then for every shared pair of electrons will equal Eko Vaillant Bond. So our final Louis structure will be for H two s. Is this?