SOLVED: Consider the molecules CF4 and SF4. (a) “Draw” Lewis structures for each. Since it is difficult to actually “draw” the structure in this online format, describe the Lewis structure in words. F

How To Draw Lewis Structures
How To Draw Lewis Structures

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Consider the molecules CF4 and SF4.
(a) “Draw” Lewis structures for each.
Since it is difficult to actually “draw” the structure in this online format, describe the Lewis structure in words. For example, in describing NH3: the molecule has a total of 8 valence electrons. A central nitrogen atom is surrounded by hydrogen atoms. There is one pair of shared electrons between each of the hydrogen atoms and the nitrogen atom. There is one lone pair of electrons around the nitrogen.
(b) Name the molecular geometry for each.
(c) Identify the polar molecule and explain why one molecule is polar, whereas the other is nonpolar.

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02:16

Draw the Lewis dot structures for SF₄ and SF₆. What is the electron pair geometry name and the molecular geometry name for each? Calculate the formal charge for both sulfurs and one of the fluorines. Are the bonds polar? Why? Is the whole molecule polar? Why?

05:16

For each compound, draw the Lewis structure, determine the geometry using VSEPR theory, determine whether the molecule is polar, identify the hybridization of all interior atoms, and make a sketch of the molecule, according to valence bond theory, showing orbital overlap.a. COF2 (carbon is the central atom)b. S2Cl2 (ClSSCl)c. SF4

01:57

Up until now, you’ve been drawing first a Lewis dot diagram (two-dimensional, shows lone electron pairs) and then a separate diagram showing molecule shape (three-dimensional, no lone pairs shown). Now begin combining the two, drawing one structure showing both threedimensional shape and all lone pairs. Draw such a structure for each of the following polyatomic ions. Name each shape, and indicate whether the ion has an overall dipole moment. If so, draw the dipole moment vector. (Hint: It’s a good idea to continue to draw a regular Lewis diagram first, even though you do not show it in your final answer.)(a) $\mathrm{CN}^{-}$(b) $\mathrm{ClO}_{4}^{-}$(c) $\mathrm{PCl}_{4}^{+}$(d) $\mathrm{NO}_{2}^{-}$

02:20

For each of the following molecules, determine: (a) whether ithas polar bonds; (b) what its molecular shape is; (c) whether themolecule is polar. You will need to draw the Lewis structuresfirst.(i) H2CO. C is the central atom; the other atoms are bonded toit.(ii) BCl3. B is the central atom.

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You are watching: SOLVED: Consider the molecules CF4 and SF4. (a) “Draw” Lewis structures for each. Since it is difficult to actually “draw” the structure in this online format, describe the Lewis structure in words. F. Info created by THVinhTuy selection and synthesis along with other related topics.

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