Concept explainers
Determine what is wrong with each Lewis structure and write the correct structure.
a.
b.
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d.
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INTRODUCTORY CHEMISTRY-W/MOD.MASTERING.
- Draw an acceptable Lewis structure for each compound, assuming the atoms are connected as arranged.arrow_forward1. draw the lewis structure of NO3 -1. 2. How many resonance structures can you draw?arrow_forward2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule before identifying the shape of the molecule? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.arrow_forward
- T'he incomplete Lewis structure below shows all the atoms and sigma bonds for a particular molecule, but nothing else. The molecule has a net charge of 0. Fill in any missing electrons to create the best Lewis structure for the molecule. Make sure to include any non-zero formal charges. H. H. H нн Harrow_forwardI am not sure if I'm right on the answers I did. Thanks for helping.arrow_forward4. Molecule: XeF2 indicate the number of available electrons that are in the molecule. in the space to the right connect all of the atoms ae = Trial Structure: to the central atom and then make each atom follow the octet rule (duet rule for hydrogen). How many electrons are necessary in the trial structure? ne = Circle the correct ne = ae ne ae relationship between ne and ae. Draw the corrected Lewis Structure to the right. Add Later: e- geometry: molecular geom: Hybridization:arrow_forward
- Draw the Lewis structure of the compound whose structure is given below. H,C 1. H,C – CH,arrow_forward1. How can you tell if a compound is covalent? 2. What distinguishes a covalent bond from an ionic bond? 3. How do you know how many valence electrons an atom has? 4. What is electronegativity? Is electronegativity a property of atoms or bonds? 5. What is polarity? Is polarity a property of atoms or bonds? 6. Describe in detail the N-F bond in terms of the relevant electronegativities and polarities. 7. What does VSEPR stand for and how does it allow one to predict the shapes of covalent molecules?arrow_forwardDraw the Lewis structure (with formal charges) of the chemical species: 1. CINO2 (N is the central atom) 2. CO3^2- 3. NO2- 4. SO3 5. BrNO2 (N is the central atom) 6. HCO3- (H is bonded to one of the O's) 7. SeO2 8. HC2O4- (each C has two O atoms and H is on one of the O's) 9. HNO3 (H is bonded to one of the O's) 10. CH3NO2 11. HCO2- (H and both O's are bonded to C)arrow_forward
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