9. Think of 3 examples, (not the same ones as ppt), ofexceptions to the octet rule and explain why they are exceptions.1.2.3.10. Draw Lewis structures for molecular oxygen and ozone(03). Use these structures to explain why one is more reactivethan the other and which will have a longer bond length. Includeresonance structures.11. Write the Lewis Structure for each molecule/ion and includeresonance structures.a. CHO₂b. SO3c. NO₁₂

Answered: 9. Think of 3 examples, (not the same…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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valence electrons - He in lone pair POST-LAB QUESTIONS - bonds to ATOMS 1. Sodium azide, NaN3, is commonly used in automobile airbags, since it decom- poses explosively to form nitrogen gas. Complete the skeleton structure shown below for the azide ion, N₂, and any other resonance structures that may be applicable. b. Use formal charge to determine which resonance structure is most important. C. Use VSEPR theory to predict the molecular shape (linear or bent). FORMAL CHARGE a. ( 100 N N + N Na NI N2 IN 3 INA chang and indicate bond angles
Show how these elements combine into octet-rule ionic compounds, as in the first example. First, draw atomic Lewis structures for the atoms and their O.R. ions. Show their charges, and use them to find the unit formula, and the name. Then draw atomic Lewis structures for all atoms in the formula unit together, show with arrows how all e s are transferred to make the ions, and draw the Lewis structure of the ionic compound. Unit formula Atoms O.R. ions Name Transfer e s with arrows Lewis Structure LizN le 1e 30 Lithium Li. + •N• Li. •N• Li. Li 30 Li Li Li :N: nitride )le Li. Pb and K and H
4. Determine the enthalpy of reaction for the below (you will need to use a bond dissociation energy (BDE) table from book/internet): a. (CH3)2CH2 + Brz > (CH3)2CHBr + HBr b. (CH3)3CH + Br₂ → (CH3)3CBr + HBr
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Draw the lewis structure with formal charges. If the lewis structure has resonance please show all possible resonance structures. 4. SO3
Determine if the structural formula below is an acceptable Lewis structures for organic compounds. Point out the problems in cases where structure is invalid. :0: CH3 CH-C-Ö-CH–CH3 A. This is not the correct Lewis structure. B. No, All atoms do not have a zero formal charge, therefore this is not the correct Lewis structure. C. All atoms have a zero formal charge, therefore this is the correct Lewis structure. D. Oxygen has a formal charge of 1+.
Considering the structure on the far left as the original resonance structure, which of the subsequent resonance structures (A-D) is implausible. Explain why you believe the resonance structure to be implausible.
A newly discovered element Bm has 6 valence electrons. How many total valence electrons are in the BmH2 molecule, a molecule that Bm forms with hydrogen? Draw a valid Lewis Structure for the molecule BmH2 that Bm forms with hydrogen and use the Lewis structure to determine the number of lone pairs of electrons around the central Bm atom in this molecule. What is the formal charge of Bm in BmH2? (Number and sign) What is the hybridization of Bm according to the hybrid orbital model?
1.1 Define electronegativity and explain why electronegativity increases with atomic number within a period of the Periodic Table. 1.2 Describe the type of bonding that exists in F2 (g) molecule. How does this type of bonding differ from that found in the HF (g) molecule? 1.3 Define hydrogen bonding using examples. 1.4 PH3 and NH3 moleculea are the same shape but the molecules are non-polar and polar respectively. Explain why this is so. 1.5 Give an example of molecule that has a coordinate covalent bond. 1.6 Draw a Lewis structure for each of the following molecules of ions: a) HF3 b) CIO3-
Each molecule listed below is formed by sharing electrons between atoms when the atoms within the molecule are bonded together. Molecule A: Cl 2 Molecule B: CCI 4 · Molecule C: NH 3 34. In the box provided in your answer booklet, draw the electron-dot (Lewis) structure for the NH 3 molecule. [1] 35. Explain why CCI 4 is classified as a nonpolar molecule. (1] 36. Explain why-NIshas stronger-intermolecular forces of attraction than Ct2. f} 37. Explain how the bonding in KCl is different from the bonding in molecules A, B, and C. [1]
Answer 1 2 3

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