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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

Draw a structure for the model, N the molecule polar or non-polar’ explain?
Discuss the stability of each of these species based on the octet rule and formal charges;
Draw the three constitutional isomers that have the formula C5H12.
The formula C4H10O results in seven isomers. See how many you can draw.
Determine whether these structures represent the same compound or isomers;
Calculate the DU for these formulas and draw two constitutional isomer for each:(a) C10H22(b) C9H16(c) C6H6
Convert these structures to skeletal structures:
Convert these skeletal structures to line structures:
Determine whether these structures represent the same compound or isomers:
Calculate the DU for these formulas and draw two constitutional isomer for each:(a) C10H20O(b) C6H9N(c) C7H14F2(d) C6H8CIN(e) C9H15NO
Determine the DU for each of these structures:
What kinds of attractive intermolecular forces are found in each of these compounds?(a) CH3CH2CH3(b) CH3OCH3(c) CaCl2(d) CH3OH
Show the hydrogen bond that is present in liquid ammonia, NH3(l)
Explain whether you would expect KBr or CH3Br to have the higher melting point.
Which of these isomers would you expect to have the higher boiling point: Explain?CH3CH2CH2OH or CH3CH2OCH3
Which of these compounds would you expect to be more soluble in water? Explain?
Which functional group is present in each of thesecompounds?
Convert the following structures to skeletal structures:
Convert the following shorthand representations to structures showing all of the atoms, bonds, and unshared electron pairs:
Name the functional group(s) present in each of the compounds in Problem 2.17.
Name the functional group(s) present in each of the compounds in Problem 2.18.
Determine whether these structures represent the same compound orisomers:
Draw all the isomers for each of these formulas. The total number for each is given in parentheses.(a) C3H8O (3)(b) C4H9Cl (4)(c) C4H8 (5)(d) C7H16 (9)
The formula C4H8O has many isomers.(a) Draw three isomers that have a carbon oxygen double bond. What functional group is present in each of them?(b) Draw three alcohols with this formula.(c) Draw an
Four of the ten isomers of C5H10, are shown in Figure 2.5. Draw four other isomers with this formula.
Calculate the DU for each of these formulas and draw a structure that meets the listed restriction:(a) C5H9NO (not an amine)(b) C7H12O (a ketone)(c) C6H14O (does not hydrogen bond)(d) C7H8 (an
Can C8H17N have a nitride as its functional group? Explain.
Show all the different hydrogen bonds (hat would occur in a mixture of (a) CH3CH2OH and H2O (b) CH3OHand
One of these isomeric alcohols has mp = 26°C and bp = 82°C; the other has mp = – 90°C and hp = 117°C. Explain which isomer has the higher melting point and which has the higher boiling point.
Explain the differences in the boiling points between the members of’ each of these pairs of compounds:(a) CH3 (CH2)6 CH3
Explain the difference in the melting points of these isomers:
Explain which compound you expect to have the higher melting point.
Explain which compound you expect to have the higher boiling point.
Which of these two salts would your expect to be more soluble in hexane(C6H14)?
Benzene and hexane are both liquids at room temperature. Do you expect benzene and hexane to be miscible? Do you expect benzene and water to be miscible? Explain.
One of these isomers is miscible with water, and the other is nearly insoluble. Explain.
Because of two hydrogen bonds, carboxylic acids show a very strong attractive force between two molecules that persists even in the gas phase. Show this hydrogen bonding between two carboxylic acid
Bond strengths can be used to estimate the relative stability of isomers that have different bonds. The isomer that has the larger total bond energy is more stable. One of the following isomers is
Bond strengths can be used to estimate the relative stability of isomers that have different bonds. The isomer that has the larger total bond energy is more stable. One of the following isomers is
One of the isomers of C5H12 reacts with Cl2 in the presence of light to produce three isomers of C5H11Cl: This reaction replaces am one of the hydrogen?s of C5H12 with a Cl. What arc the structures
On reaction with Cl2 in the presence of light, an unknown compound with the formula C5H10 gives only one isomer of C5H9Cl (see problem 2.39). What is the DU of the unknown compound? Show the
Explain how the dipole moment for CH3Cl (μ = 1.9 D) can be larger than the dipole moment for CH3F (μ = 1.8 D).
Peptides arc smaller versions of proteins and have similar functional groups. What functional groups are present in this peptide?
Glucose is a typical carbohydrate. What functional groups are present in glucose? What would you predict about the water solubility of glucose, oiler a reason why nature uses carbohydrates rather
Amino acids such as alanine actually exist as species called zwitterions, with a positive charge on the nitrogen and a negative charge on the oxygen. Explain what effect you expect this to have on
What is the DU of estrone, a female sex hormone? Use the number of carbons and oxygen?s in estrone to calculate the number of hydrogen?s it has.
Explain whether each pair of models represents isomers or the same compound. (All represent compounds with the formula C7H16.) Draw structures for each compound represented by the models.
Explain whether each pair of models represent isomers or the same compound. Draw structures for each compound represented by the models.
The following models represent three isomers of C6H4Cl2. Explain which of these compounds does not have a dipole moment.
Draw the structures of the compounds represented by these models and explain which would have the larger solubility in water. (The red atoms are oxygen’s.)
Draw the structures of the compounds represented by these models and explain which would have the higher melting point.
These models show the three isomers of C5H12. Explain which isomer would produce only one C5H11Cl isomer on reaction with Cl2 in the presence of light.
Determine the degree of un-saturation for these compounds.
Draw a 3s atomic orbital and compare it to a 2s orbital.
Show an atomic orbital energy level diagram for these atoms:(a) Si(b) Al(c) Cl
Explain whether the electron arrangement for these atoms is the ground state or an excitedstate:
Show an energy level diagram for the MOs for He2 and show how the electrons would be arranged in these MOs.
Indicate the type of atomic orbital’s that are overlapping to form each of the different kinds of bonds in CH3OCH3 (For example, a carbon sp3 AO and a hydrogen Is AO). What kinds of orbitals are
What is the hybridization at the N and each C in this molecule? Indicate the type of bond and the orbitals that are overlapping to form it for each of the designated bonds (for example, ?CSP3 + H1s).
Consider hydrogen cyanide, H – C ≡ N.(a) What is the hybridization at the N at the C?(b) What are the types of the three CN bonds? What orbital’s overlapping to form them?(c) In what type of
What is the hybridization at each C in this molecule? Indicate the type of bond and the orbital's that are overlapping to form it for each of the designated bonds?
Show the hybridization at each of the atoms, except H, in these molecules. Indicate the type of each designated bond and the orbital's that are overlapping to form it.
Circle the conjugated pi bonds, if any, in the following compounds?
What is the hybridization at the indicated atoms in these compounds?
Explain whether or not these structures represent resonance structures?
Explain why the structure on the right is not a valid resonance structure for the structure on the left?
Rank the stability of these resonance structures?
Discuss the actual structure and the amount of resonance stabilization for the examples shown in problem 3.14.
Show the important resonance structures for these species. Use the curved arrow convention to show how the electrons are moved to create each new resonance structure.
Draw the important resonance structures for these species. Use the curved arrow convention to show how the electrons are moved to create each new resonance structure. Discuss the relative
Show energy level diagram for the MOs of these compounds?
Show the location of the two planar nodes in this 3d atomic orbital?
What is the hybridization at all atoms, except hydrogen's in these compounds?
Show the hybridization at each of the atoms, except H, in these molecules. Indicate the type of each designated bond and the orbital's that are overlapping to form it?
What is the hybridization at all atoms, except hydrogen's, in these compounds?
Draw the p orbital's that compose the conjugated part of these molecules:
Show the important resonance structures for these compounds. Use the curved arrow convention to show how the electrons are moved to create each new resonance structure.
In these examples the additional structure or structures are not important contributors to the resonance hybrid for the compound represented by the first structure, explain.
Draw the important resonance structures for these species and discuss the contribution of each to the resonance hybrid. Explain whether the species has a large or a small amount of resonance
Explain why this carbocation is considerably more stable than this structure would suggest:
Explain why one of these anions is much more stable than the other:
Explain why one of these carbocations is much more stable than the other:
Show energy level diagrams for the MOS of these compounds:
The energy level diagram for the MOs of CH2 = CH2 is shown if Figure 3.24. Show a similar diagram for the lowest-energy excited state of this molecule.
Consider the species formed by the addition of an extra electron to H2 so that there are three electrons and a negative charge. Show an energy level diagram for the MOs of this species. Is there
Draw an energy level diagram for the excited state of H2. Is there still a bond between the hydrogen’s?
Consider H2C = C = CH2. What is the hybridization and geometry at each C? Indicate the bond types for each of the carbon-carbon bonds. Draw the molecule, showing the overall geometry and the p
Draw resonance structures for this anion. Remember, sulfur can have 10 or even 12 electrons in its valence shell.
Phenanthrene has five total resonance structures. One is shown here. Draw the other four. Which carbon-carbon bond of Phenanthrene would your predict to be the shortest?
Show the three additional resonance structures for anthracene. Discuss whether the experimental bond lengths shown in the following structure are in accord with predictions based on these resonance
One general reaction of radicals is the coupling of one with another to form a bond, as shown in the following equation: The following coupling reaction gives two products. Show the structures of
Show a MO energy level diagram for the neutral molecule HeH. Use this diagram to explain whether HeH is expected to stable or not?
What is the hybridization at each nitrogen of the amino acid histidine? What kind of orbital is occupied by the unshared pair of electrons on each nitrogen? Explain.
At a pH of 10.8, the amino acid arginine exists primarily as the following dipolar ion. Show the resonance structures for the cationic part of arginine and discuss their relative contributions to the
Indicate the hybridization at each atoms other than hydrogen, in the compounds represented by these models. Draw structures for each compound represented by the models.
Draw structures for each compound represented by these models and indicate the conjugated part of the compounds?
Draw all the important resonance structures for the compounds represented by these models?
Draw structure for the neutral molecule represented by the following model. Explain whether the octet rule is satisfied at each atom of the compound. Draw all of the important resonance structures
Indicate whether each of these species can act as an acid, a base, or both:
Show the conjugate acids of these species:

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