So starting with per day we are going to assign the hybridization of the numbered atoms and also give the bond angles surrounding that pattern. So starting with a we have die. It'll either and I already drawn them on how they were given in the text book. And the first atom is this oxygen here. So it has to bonds and two lone pairs of electrons, So does sp three hybridized. And since the electron geometries tetra hydro Um we know that it will be less than one of 9.5 since two lone pairs of electrons will actually push the carbons closer together. And for the second atom is this carbon, It has four bonds. So this Sp three hybridized and as tetra hydro Um electron geometry and shape and has no lone pairs of electrons. So we know that they will all have ideal bond angles of one of 9.5°. Moving on to part B. We have caffeine and the first adam to give the hybridization is this carbon here. So we know that it has two Single bonds and a double bond. So it's sp two hybridized And we'll have bond angles of 120°. The next atom is this carbon also is sp three hybridized and has bond angles of 1 20 and last on the caffeine is this nitrogen, which has two bonds, one single bond, one double bond and a lone pair of electrons Making it sp two hybridized. And we'll have bond angles of slightly less than 120° because that lone pair of electrons again pushes the bonds closer together. Can you get a bent shape for part C. We have a seagull salicylic acid. The first item to give the hybridization of visits oxygen, which has two bonds and two lone pairs. So it is sp three hybridized With bond angles of less than 1.09.5. Next is this oxygen that has one bond, so one double bond in two lone pairs, so does sp two hybridized, and the angle between the carbon and the oxygen Is 1 80°. And this carbon here is sp two hybridized. Inside has three bonds And we'll have bond angles of 120° in party. We have nicotine. This first carbon has four bonds, So it's sp three hybridized. And although the bond angles are 109.5 since etc federal shape Number two is this carbon That it is sp two hybridized. It has three bonds And it's trickle planner shape, so has bond angles of 120. Next is this nitrogen that has to bonds So one double bond, one single bond in a lone pair, So the three regions of electron density making an sp two hybridized, and the long pair of electrons pushes the bombs closer together. Some sort of 120. The bond angle. This bond angle here on the inside Will be slightly less than 120°. Yeah, For number four is this nitrogen that has three bonds and a lone pair of electrons. So it's sp three hybridized and as bond angles a bit less than one of 9.5 because one of the regions of electron density is a lone pair of electrons pushing the bonds closer together and lost. Is this carbon that is sp three hybridized instead of four bonds And the bond angles are one oh 9.5 degrees and says Petra federal shape. And lastly in part E, The F. D. Greene. And the first item is this nitrogen that is three bonds, 1 lone pair. So it's sp three hybridized with bond angles of a bit less than 1 to 9.5 degrees, since it's tetra hydro electron geometry, but there's a long pair of electrons pushing the atoms that's bound to closer together. 2nd is this carbon that has for bonds, So it's sp three hybridized, none of them are lone pairs, so they are all ideal bond angles of one or 9.5. Next is this carbon That is sp two hybridized with bond angles of 120. And lastly, is this oxygen that has to bonds and two lone pairs. So it's sp three hybridized with bond angles of less than 109.5°.