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Paul Flowers, Klaus Theopold, Richard Langley, William R. Robinson
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Chapter 7, Problem 95
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Identify the electron pair geometry and the molecular structure of each of the following molecules:(a) $\mathrm{ClNO}(\mathrm{N} \text { is the central atom })$(b) $\mathrm{CS}_{2}$(c) $\mathrm{Cl}_{2} \mathrm{CO}(\mathrm{C} \text { is the central atom) }$(d) $\mathrm{Cl}_{2} \mathrm{SO}$ (S is the central atom)(e) $\mathrm{SO}_{2} \mathrm{F}_{2}$ (S is the central atom)(f) $\mathrm{XeO}_{2} \mathrm{F}_{2}$ (Xe is the central atom)(g) $\mathrm{ClOF}_{2}^{+}$ (Cl is the central atom)
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Video by Jennifer Hudspeth
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09:29
07:51
Predict the electron pair geometry and the molecular structure of each of the following:(a) IOF5 (I is the central atom)(b) POCl3 (P is the central atom)(c) Cl2SeO (Se is the central atom)(d) ClSO+(S is the central atom)(e) F2SO (S is the central atom)(f) $\mathrm{NO}_{2}^{-}$(g) $\mathrm{SiO}_{4}^{4-}$
03:39
Predict the electron pair geometry and the molecular structure of each of the following:(a) IOF $_{5}$ (I is the central atom)(b) $\mathrm{POCl}_{3}$ (P is the central atom)(c) $\mathrm{Cl}_{2} \mathrm{SeO}$ (Se is the central atom)(d) $\mathrm{ClSO}^{+}$ (S is the central atom)(e) $\mathrm{F}_{2} \mathrm{SO}$ (S is the central atom)(f) $\mathrm{NO}_{2}^{-}$(g) $\operatorname{SiO}_{4}^{4-}$
01:41
Determine the electron and molecular geometries of each molecule. (Hint: Determine the geometry around each of the two central atoms.)(a) $\mathrm{C}_{2} \mathrm{H}_{2}$ (skeletal structure HCCH)(b) $\mathrm{C}_{2} \mathrm{H}_{4}$ (skeletal structure $\mathrm{H}_{2} \mathrm{CCH}_{2}$ )(c) $C_{2} H_{6}$ (skeletal structure $\mathrm{H}_{3} \mathrm{CCH}_{3}$ )
06:36
Identify the hybridization of the central atom in each of the following molecules and ions that contain multiple bonds:(a) ClNO (N is the central atom)(b) $\mathrm{CS}_{2}$(c) $\mathrm{Cl}_{2} \mathrm{CO}$ (C is the central atom)(d) Cl_SO (S is the central atom)(e) $\mathrm{SO}_{2} \mathrm{F}_{2}$ (S is the central atom)(f) $\mathrm{XeO}_{2} \mathrm{F}_{2}$ (Xe is the central atom)(g) $\mathrm{ClOF}_{2}+(\mathrm{Cl}$ is the central atom)
Transcript
Hi there. In this problem, we have several formulas that we’re trying to determine the electron pair geometry as well as the molecular structure. For those I believe, the best way to do this is to set up a little table the first column of my table. I am going to have valence electrons, so I’m going to add up and determine the total number of electrons that should be in my dot structure. Next, I am going to sketch out that dot structure for each one because we need that to determine the electron pair geometry and eventually the molecular structure. So let’s go again. Let’s go ahead and get started with letter A. We have C L N o looking at the periodic table. Chlorine has seven valence electrons. Nitrogen has five and oxygen has six. It gives me a total of 18 sketching this out, Do you remember? We want each element to end up with eight valence electrons and use those 18 dots that we have available to us. The only way to make this happen for this problem is if we have a double bond located between the nitrogen and the oxygen. So if we look at this. This gives us two atoms bonded to the low to the central atom. So there are two atoms bonded to the nitrogen and on the nitrogen there’s one lone pair. So in other words, there are three electron regions. So this gives us an electron pair geometry of trig onal planer. In this geometry, since there are only two atoms bonded to the central atom, we’re going to end up with a molecular structure that is bent. Okay, so electron pair geometry. Try Donald plainer. The molecular structure is bent. Let’s move on to letter B. Let her be. We have C s to that will give us 16 Valence electrons. This is going to be very much like CEO to when we draw its structure here is going to be a double bond to each of the sulfur atoms and no lone pairs on the carbon. So as we look at this, there are two atoms bonded and zero lone pairs. So our total number of electron regions are too, which makes this linear. Since there’s an atom bonded on each side there, the actual molecular structure is all swollen ear, so both linear for the electron pair geometry and the molecular structure moving on to letters C Let her see We have C l to c e o adding up the electrons, valence, electrons that we have to work with. I get 24 sketching this out. I find that the only way to make this work out is to have a double bond to the oxygen and then single bonds to each of the chlorine. So I got structure ends up looking like that. That means there are three atoms bonded to the central atom and zero lone pairs means that gives us a total of three…