Organic Chemistry
11th Edition
ISBN: 9781118133576
Author: T. W. Graham Solomons, Craig Fryhle
Publisher: Wiley, John & Sons, Incorporated
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Question
Chapter 1, Problem 5PP
(a)
Interpretation Introduction
Interpretation:
The Lewis structure of the molecules difluoromethane
Concept introduction:
➢ The Lewis structure of a molecule is a representation of the molecule in which the valence electrons of the atomsareshown.
➢ The number of valence electrons of an atom is equal to the group number to which it belongs. Bonding atoms attaina stable electronic configuration and a stable atom generally has eight electrons in itsvalence shell.
➢ To attain a stable configuration, atoms share their electrons with each other.
(b)
Interpretation Introduction
Interpretation:
The Lewis structure of the moleculeschloroform
Concept introduction:
➢ The Lewis structure of a molecule is a representation of the molecule in which the valence electrons of the atomsareshown.
➢ The number of valence electrons of an atom is equal to the group number towhich it belongs. Bonding atoms attaina stable electronic configuration and a stable atom generally has eight electrons in itsvalence shell.
➢ To attain a stable configuration, atoms share their electrons with each other.
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Draw complete Lewis structures for the following condensed structural formulas.(a) CH3(CH2)3CH(CH3)2 (b) (CH3)2CHCH2Cl(c) CH3CH2COCN (d) CH2CHCHO(e) (CH3)3CCOCHCH2 (f) CH3COCOOH
3.72 (*) Identify the mistakes contained within the following
structures.
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(b)
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Draw a Lewis Structure for each of the following species and assign formal charge where appropriate. Using electronegative values from the period table that was provided identify polar covalent bonds and label the atoms δ+ and δ−. For each of the molecules indicate whether or not it has a dipole moment. (a)CH5N (b) HCN (c) H2CO (d) CH3NC(e) CH3SOCH3 (f) H6BN
Chapter 1 Solutions
Organic Chemistry
Ch. 1 - Prob. 1PPCh. 1 - Prob. 2PPCh. 1 - Prob. 3PPCh. 1 - Prob. 4PPCh. 1 - Prob. 5PPCh. 1 - Prob. 6PPCh. 1 - Prob. 7PPCh. 1 - Prob. 8PPCh. 1 - Prob. 9PPCh. 1 - Prob. 10PP
Ch. 1 - Prob. 11PPCh. 1 - Prob. 12PPCh. 1 - Prob. 13PPCh. 1 - Prob. 14PPCh. 1 - Prob. 15PPCh. 1 - Prob. 16PPCh. 1 - Prob. 17PPCh. 1 - Prob. 18PPCh. 1 - Prob. 19PPCh. 1 - Prob. 20PPCh. 1 - Prob. 21PPCh. 1 - Practice Problem 1.22 Which of the following...Ch. 1 - Prob. 23PPCh. 1 - Prob. 24PPCh. 1 - Practice Problem 1.25
What do the bond angles of...Ch. 1 - Prob. 26PPCh. 1 - Practice Problem 1.27
Use VSEPR theory to predict...Ch. 1 - Practice Problem 1.28 Predict the bond angles of...Ch. 1 - 1.29 Which of the following ions possess the...Ch. 1 - 1.30 Write a Lewis structure for each of the...Ch. 1 - Prob. 31PCh. 1 - Add any unshared electrons to give each element an...Ch. 1 - Prob. 33PCh. 1 - What is the molecular formula for each of the...Ch. 1 - Prob. 35PCh. 1 - Prob. 36PCh. 1 - 1.37 Write bond-line formulas for all of the...Ch. 1 - Prob. 38PCh. 1 - Prob. 39PCh. 1 - Prob. 40PCh. 1 - Prob. 41PCh. 1 - (a) Cyanic acid (HOCN) and isocyanic acid (HN=C=O)...Ch. 1 - Consider a chemical species (either a molecule or...Ch. 1 - 1.44 Consider a chemical species like the one in...Ch. 1 - 1.45 Consider another chemical species like the...Ch. 1 - Draw a three-dimensional orbital representation...Ch. 1 - Ozone (O3) is found in the upper atmosphere where...Ch. 1 - Write resonance structures for the azide ion, N3....Ch. 1 - Write structural formulas of the type indicated:...Ch. 1 - Prob. 50PCh. 1 - 1.51 In Chapter 15 we shall learn how the...Ch. 1 - Prob. 52PCh. 1 - (a) Consider a carbon atom in its ground state....Ch. 1 - Open computer molecular models for dimethyl ether,...Ch. 1 - Boron is a group IIIA element. Open the molecular...Ch. 1 - 1.56 There are two contributing resonance...Ch. 1 - Prob. 1LGPCh. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Consider the compound with the following condensed...Ch. 1 - Prob. 7LGPCh. 1 - Prob. 8LGP
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- (a) Draw a line drawing for the Lewis diagram given below. Hint start converting the Lewis to a VSEPR diagram. H H H +4 H H (b) What is the line drawing for a chemical species with the condensed molecular formula -H CH3CHC(CH3)CH(CH3)2. Hint start by converting the condensed formula to a Lewis diagram....then you solve this just like Question 1(a)!. (c) Of course, concepts can be examined in reverse! Draw a VSEPR diagram THAT IS ALSO A BEST LEWIS DIAGRAM, for the chemical that has the following line drawing: H₂N IOarrow_forward1.3 3 (a) Give the structural formulae of all the chain isomers of C₂H₁2 12. (b) Give two position isomers of the molecule that has the following molecular formula: CH 10 (c) Give the two functional group isomers having the molecular formula: C₂H₂Oarrow_forwardUsing just a periodic table (not a table of electronegativities), decide which of these is likely to be the most polar bond. Explain your answer! (a) C-F (b) S-F (c) Si-F (d) O-Farrow_forward
- Draw a Lewis structure for each species. (i) CH3OSO2OCH3 (ii) CH3C(NH)CH3 (iii) (CH3)3CNOarrow_forwardWhat's More (A) Activity 2.1: Synthesizing concepts Directions: Complete the table below with correct answers. The first one is done for you. Lewis Structure with correct geometry Covalent Geometry Name Polar or Nonpolar? Compound :ö =c=ö: Nonpolar Linear CO2 CH4 NH3 SF4 XEOF4 SF6 What's More (B)arrow_forward5. A molecule with the formula C,H is a(n): (a) hexane (b) propane (c) decane (d) butane (e) ethanearrow_forward
- 2b) NH₂ NH₂arrow_forwardDraw the shapes of the following molecules and ions in 3-dimension. Show clearly any lone pairs of electrons on the central atom, state the number of bond pairs and lone pairs of electrons on the central atom and name the shape of the molecule or ion. (a) SiCI4, silicon tetrachloride (b) PBr3, phosphorus tribromide (c) CI2O, dichlorine oxide Provide everything stated in the instructions for each compound.arrow_forward(i) Draw a complete Lewis dot structure for each of the following compounds. Clearly (ii) indicate all bonds and lone electrons, as well as the formal charge of each atom in the compound. a) NO3 b) NH4* c) CO2arrow_forward
- Draw electron dot and cross diagrams for the following compounds. Only the outermost shell of electrons needs to be shown. Use a different dot or cross for each atom or ion. (a) CH3COOH, ethanoic acid (b) S2Cl2, disulfur dichloride (c) O22, peroxide ion Provide everything stated in the instructions.arrow_forwardConvert each of the following molecular models into a skeletal structure, and give the formula of each. Only the connections between atoms are shown; multiple bonds are not indicated (gray=C, red =O, blue =N, ivory = H)arrow_forwardCan you help me answer and explain 3.37arrow_forward
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