Concept explainers
Determine what is wrong with each ionic Lewis structure and write the correct structure.
a.
b.
c.
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Introductory Chemistry (6th Edition)
- Sketch the Lewis structures for CIF2+ and CIF2. How many lone pairs and bond pairs surround the Cl atom in each ion?arrow_forwardDraw the attraction between a water molecule and a molecule of BrCl4F. Br is the central atom in an expanded octet - count your electrons carefully. First, draw one molecule and add the partial charges where needed - use the ΔEN to determine the types of bonds. Then, draw the second molecule so that the δ+ on one molecule lines up across from the δ- on the other. Since we can't draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. BrCl4F has one __________ bond between the Br and F with ΔEN = ____________ , and four ________ bonds between the Br and Cl with a ΔEN = _________ . The central Br has 6 REDs and the molecule is symmetrical/asymmetrical (answer is ___________ ) making it a polar/nonpolar (answer is __________ ) molecule. The central Br has a ___________ charge and the F has a ________ charge. H2O has 2 ____________ bonds with a ΔEN = ___________ . H2O has 4 REDs and is symmetrical/asymmetrical (answer…arrow_forwardLewis structure for sulfur dioxide S02 Number of electrons set(groups)? Number of bonding electron sets (groups)? Number of non-bonding electron sets (groups) or lone pairs? How many bonds have a dipole ? If so do the dipole cancel each out?arrow_forward
- 1) Discuss the advantages and disadvantages of using the molecular models (ball and stick) as learning aids. Recommend an alternative to using this method for modeling molecules. 2) Build C6H6 as a ring. What do you notice about the placement of the bonds? This is an example of resonance. What is a resonant Lewis structure? 3) Explain how a diminished and expanded octet can be formed.arrow_forwardNhy is resonance structure A and resonance structure B not the same structure? If you rotate the molecule like a spicket handle (l. e. clockwise with the C at the center and the R group remaining in place as you look down the C - R bond) wouldn't you get the same thing? Why are these not equivalent structures? Resonance structure A t Resonance structure B Actual structurearrow_forwardIn the Lewis model, we use resonance forms to represent the two equivalent bonds. True or false? Explain how?arrow_forward
- a) Draw the Lewis Structure of I3- OR (I3 minus). How many total nonbonding electrons surround the central I atom? b) Draw the Lewis Structure of PF5 (OR P F5). How many electron pairs (not total electrons) surround the P atom. c) Draw the Lewis Structure of NO3-1 (OR N O3 minus). What is the formal charge of N?arrow_forwardDraw the Lewis Structure for each covalent system a-e below, and answer the question that follows: Electronegativites: H = 2.1 C = 2.5, B = 2.0N = 3.0, 0 = 3.5 S = 2.5, F = 4.0, Xe = 2.6 a. (OF 2 )Is this molecular POLAR or NONPOLAR? b. (XeF2) What is the geometry of this molecule? c. (SO 3 ^ 2- )What is the polyatomic ion geometry? (Assume "S" obeys octet) d.( CH 2 F 2 )Is this molecular POLAR or NONPOLAR? e.( BF 3 )Is this molecular POLAR NONPOLARarrow_forwardWrite the Lewis structure for each molecule. SF2arrow_forward
- 1. What is the formal charge on each atom in CH3Cl and the Lewis structure for it? 2. What is the formal charge on each atom in PH4 nd the Lewis structure for it? 3. What is the formal charge on each atom in HNO3 and the Lewis structure for it?arrow_forwardDraw the Lewis Structure of CH3OCH3 Molecular Geometry? Ideal Bond Angles? Are there Polar Bonds Present (Indicate on Lewis do structure Is there an Overall Dipole? Octet rule violator and how?arrow_forwardThree Lewis structures are given below. For each set of Lewis structures in the boxes below build molecular models and determine the shape of each molecule.arrow_forward
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