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Consider the shorthand structure below (which also does not show lone pair electrons on N_ O,or S):OH(5 pts cach) Fill in the correct number next to the atomic symb...

Question

Consider the shorthand structure below (which also does not show lone pair electrons on N_ O,or S):OH(5 pts cach) Fill in the correct number next to the atomic symbol, for the molecular formula of this compound: H = C = N = S =(6) (5 pts cach) For each of the atoms indicated by a, b, C, indicate the hybrid atomic orbitals you would expect it to be using to bond.(b) (5 pts each) For each of the angles indicated by & B; % indicate the approximate bond angle in degrees, that you would expect; b

Consider the shorthand structure below (which also does not show lone pair electrons on N_ O,or S): OH (5 pts cach) Fill in the correct number next to the atomic symbol, for the molecular formula of this compound: H = C = N = S = (6) (5 pts cach) For each of the atoms indicated by a, b, C, indicate the hybrid atomic orbitals you would expect it to be using to bond. (b) (5 pts each) For each of the angles indicated by & B; % indicate the approximate bond angle in degrees, that you would expect; based on the hybrid atomic orbital picture



Answers

For each molecule listed below, predict its molecular
shape and bond angle, and identify the hybrid orbitals.
Drawing the Lewis structure might help you.
$$\begin{array}{ll}{\text { a. } \mathrm{SCl}_{2}} & {\text { c. HOF }} \\ {\text { b. } \mathrm{NH}_{2} \mathrm{Cl}} & {\text { d. } \mathrm{BF}_{3}}\end{array}$$

The given representation is the Louis structure off the molecules auction. He has a bond angle of 132. Auction B has a born angle of 115 while option see, the angle is 180 degrees.

So in chemistry. The molecular geometry, which is also known as our molecular structure, is the three D structure or arrangement of atoms in a molecule that is defined by the ex wives that access so by understanding the molecular structure of a compound. This can help us determine a number of physical and chemical properties about that compound. So in this podcast we will just be looking at the lower structure, molecular shape on bond angle as well as hybrid orbital's to, for example, with SCL to. This is a bank confirmation with 104.5 degree bonding angles and SP three hybridization an H two c Out has try gurnal para middle confirmation with 107 degree bonding angles on SP three hybridization next year of H O F, which is banned 104.5 degree bonding angles and SP three hampered ization. And lastly, we have BF three, which is tribunal plane are with bonding angles off 120 degrees and SP two hybridization

Working with some chemistry basics again here. So this entire podcast syriza's aimed at covering chemistry basics while we starting with subjects such as periodic trends and chemical properties, all of which, under, pending more advanced levels off our chemistry. So what we're having to do is draw three dimensional orbital representation for each of our molecules. So with our first run, we have C H 20 So we have our carbon, and it s B two hybridized hydrogen is just have the Ivana sorbitol. So we have a Sigma interaction, which is the one I've just drawn. But then because we have the carbon, I'll present we also have this hi interaction Using an extra peel Butel, you have to learn pads in the remaining oxygen orbital's where we have SP two hybridization for both atoms. So next we have H two carbon double bond, carbon, hydrogen, carbon hydrogen double bond, C. H. Two. So again, we're starting off with our carbon orbital's hydrogen. Or in the one I saw, the tools that spherical we have a segment bond between the fast C eight. We also have a pie interaction between a second pi over. It'll on each carbon. We don't have a sigma interaction only with the middle two carbons. Do you have another hydrogen in a oneness? Orbital? Now we can work on our final carbon interaction two or hydrogen have a pie interaction again. So this is the sigma inside. And then this is the pie. So finally we have one more example. We have H two C double bond. See double bond. See double bond C H two. So I'll drop my carbons from my sigma interactions fast. Now I'll draw on my ch interactions. Now we can add on our remaining orbital's of which is used for bombing rpai bonds. So fastly we have a pipe bond here hand. So remember our sigma is inside That is the direct head to head overlap off our pill bottles All pie interaction is the parallel overlap. So remember P interactions looked like this sigma on then pie. So just forming two more pie bonds on that completes our comic

So here we've got some bonding examples where we have molecules on screen and we're just gonna go through on draw our arts geometries, and then we're going to be naming them as well as giving them bond angles. So firstly, we have seen us for with our central carbon, we have four florins arranged in a tetra heaved roll geometry. Now we have no lone pairs because carbon is in group for And so all of our out of electrons on our carbon are used up. And now each of our Florence has a full lock tap. They have three loan pas, and our bond angle is 109.5. So now moving on to our next example where we have an F three and so we have all central nitrogen. And then we have our florins arranged in a para middle formation. Where are bond angle is approximately 101.9 degrees. One a 1.9. I've also read 102.5103 degrees. There depends on the text, but you're looking at. And now because nitrogen is in group five, it will have a lone power on the top Now if we look a BF three so boron is in group three. So again all of its electrons will be used up in bonding Pass here and we will have a try Gona play not with bond angles of about 120 degrees. So moving on to beryllium die hydride We've got central beryllium and then because it is in group to ask to outer electrons and so that this confirmation is linear where both of beryllium electrons used on both of the electrons from both protons also used we have a linear structure with 180 degrees and it's probably worth noting that this is a non polar molecule and not the only molecule Thus far that has been polar Is this one here? So now moving on to our last example of sf six we have our central sulphur is in group six so it can facilitate six atoms around it. However, these atoms do need to be small and so we use flooring which are very small molecules and here we have an Octa he'd roll geometry and then we've got bond angles here of 90 degrees between our florins and again This is non polar molecule because all of our individual die polls do cancel out


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