Drag the appropriate labels to their respective targets. Note: not all labels can be used. Reset Help oC(sp? ) H(s) oC(sp? H(s) loC(sp? ) C(sp? loC(sp" )

Drag the appropriate labels to their respective targets. Note: not all labels can be used. Reset Help oC(sp? ) H(s) oC(sp? H(s) loC(sp? ) C(sp? loC(sp" ) = C(sp'~ lC(sp? ) _ C(sps - #C(p) C(p) I~C(sp? ) C(sp? ~C(sp? ) C(sp' #C( sp? ) C(sp Submit Request Answer Part G For CHzSH draw an appropriate Lewis structure_ Draw the molecule by placing atoms on the grid and connecting them wlth bonds: Include all lone pairs of electrons: 3k

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Here we've got the orbital model of a molecule that contains carbon bonded to 2, hydrogen double bonded to a carbon that is bonded to 1 hydrogen and another carbon which is bonded to 3. Hydrogen is, and it wants us to identify first what these bonds are well, each hydrogen has a 1 s bond that overlaps with a hybridized orbital 1 s; orbital, sorry that overlaps with a hybridized orbital carbon with 3 electron groups, that's s, p 2 hybridized, all single Bonds are sigma bonds, so this is a sigma carbon s, p, 2, to a hydrogen s, that's how we would describe these 2 bonds. The next 1 is the second bond, the pi bond associated with carbon carbon. So it's going to be a pie. Carbon p to a carbon p, which is an option and then the next 1 is this bond right here, it's a single bond! So it's a sigmal bond. We'Ve got a carbon to a carbon. This carbon is sp 2 hybridized with 3 electron groups, and this carbon is sp 3 hybridized with 4 electron groups and then last of all, it wants all of these they're single bonds. So they'll also be sigma. There'S a carbon with 4 electron groups. So it's sp. 3 hybridized bonding to a hydrogen that just has an s unhybridized atomic orbital. I hope that.

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