Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Textbook Question
Chapter 2, Problem 6CTQ
It is impossible to draw a legitimate Lewis structure of a neutral
a. The +1 cation,
b. Draw the Lewis structure for
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2. 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?
2. 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.
Consider lewis structure of NH3. how many Ione pairs are on nitrogen:
1
2
4
0
3
When the predicted Lewis structure of ArO3, ^2+ is drawn correctly, how many lone pairs are on the central atom?
O A.3 O B. 2 O C.o O D.4 O E.1
How many valence electrons would an AX4 molecule have if A was a group 6A atom and X was from group 7 A?
O A. 32 О B. 36 O C. 30 O D. 28 O E. 34
Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
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- This Lewis structure for SF5+ is drawn incorrectly. What error was made when determining the number of valence electrons?arrow_forwardConsider the following compounds: CO2, SO2, KrF2, SO3, NF3, IF3, CF4, SF4, XeF4, PF5, TF5, and SCl6. These 12 compounds are all examples of different molecular structures. Draw the Lewis structures for each and predict the molecular structures. Predict the bond angles and the polarity of each. (A polar molecule has a net dipole moment, while a nonpolar molecule does not.) See Exercises 25 and 26 for the molecular structures based on the trigonal bipyramid and the octahedral geometries.arrow_forwardWhich element will have 5 electrons in its Lewis dot symbol? a. Argon b. Boron c. Carbon d. Phosphorus e. Sulfur Which of the following elements can only form one bond in a Lewis structure? a. O b. C c. N d. Al e. H Write the correct Lewis dot structure for O2. Which statement correctly describes the structure of the whole molecule? a. There is a double bond and four lone pairs. b. There is a double bond and six lone pairs. c. There is a single bond and four lone pairs. d. There is a single bond and six lone pairs. e. There is a single bond, a double bond, and six lone pairs.arrow_forward
- 1. Which element will have 5 electrons in its Lewis dot symbol? a. Argon b. Boron c. Carbon d. Phosphorus e. Sulfur 2. Which of the following elements can only form one bond in a Lewis structure? a. O b. C c. N d. Al e. H 3. Write the correct Lewis dot structure for O2. Which statement correctly describes the structure of the whole molecule? a. There is a double bond and four lone pairs. b. There is a double bond and six lone pairs. c. There is a single bond and four lone pairs. d. There is a single bond and six lone pairs. e. There is a single bond, a double bond, and six lone pairs. 4. The electron pair in a C - F bond could be considered… a. Closer to C because Carbon has a larger radius and thus exerts greater control over the shared electron pair b. Closer to F because Fluorine has a higher electronegativity than Carbon c. Closer to C because Carbon has a lower electronegativity than Fluorine d. An inadequate model since the bond is ionic e. Centrally…arrow_forward3. Draw a legitimate Lewis structure for the following molecules. a. C2H6 b. CsH10 C. CH,0 d. HNOarrow_forward1. Given the following atom:(1) NCl3. (2) OCS, C is the central atoma. Write the Lewis structure.b. Count valence electrons.c. Distribute the electrons such that all atoms obey octet rule.d. Draw the Lewis structure. 2. Draw the resonance structures for the carbonate ion, CO32–arrow_forward
- 1. Determine the Lewis structure, shape, and polarity of the following molecules a. BrO2-, bromite ion b. BrO3-, bromate ion c, Cl207, dichlorine heptoxide 2. Write all the valid Lewis structures of bromate ion.arrow_forwardConsider the generic polyatomic ion XY3". Element X is the least electronegative. For neutral atoms, element X has 7 valence electrons and element Y has 6. The highest occupied principal energy level of the central atom is greater than 2. A. How many total valence electrons are in the molecule. B. Draw a BEST Lewis structure (i.e. a major resonance contributor) for this molecule. Show all valence electrons on your structure. C. If you haven't already, add the formal charge of each atom to the structure. Show at least one sample calculation for formal charge. D. Outline 4 short bullet points (~several words each) that explain why your structure from part B is the best one. Hint: think about what makes a valid structure and what makes a best structure. E. Perform a calculation to determine the average bond order between the X and Y atoms in your structure from part B. No credit will be given for just a number. F. Draw one more valid resonance structure other than the one from part B.…arrow_forwardANS 152 252 2P 12. What is the chemical formula of the compound formed by Barium ion and sulfate ion2ANS E ANS A 13. Write chemical symbols for the following ions: a. Sulfate ion Ans SO42- b. Sulfur ion ANS S-2 14. Write the Lewis Structure for N₂ 15. Write the Lewis Structure for SC1z (S is the center atom) 16. The bed in O₂ is a. Non- b. Polar covalent c. Ionic ited States) covalent ANS eer Services Accessibility: Unavailable Focusarrow_forward
- a. Draw the Lewis structure of SeCl4.b. Draw the Lewis structure of SF6.c. Draw the Lewis structure of BCl3.arrow_forwardA. HSCH3 Step 1. Draw the lewis structure Step 2. Description of shape: Central Atom 1= ___ Electron groups = ___ ____ non bonding= ____ total Central Atom 2= ___ Electron groups = ___ ____ non bonding= ____ total Electron group arrangement for central atom 1: Electron group arrangement for central atom 2: Geometry (shape) around central atom 1: Geometry (shape) around central atom 2: Step 3: List and Name all bond angles and give the degree.arrow_forwardThe Lewis structure of ozone (O3) is given below. Are there any resonance structures? If yes, how many? а. There are no resonance structures for ozone. b. There are 2 resonance structures for ozone. C. There are 3 resonance structures for ozone. a.arrow_forward
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