It is to be verified whether imine is reduced in the given reaction, by calculating the oxidation state of the carbon and nitrogen atoms of the C = N group before and after the reaction. Further, it is to be determined whether imine gains electrons, and if so, how many. Concept introduction: The oxidation state of an atom can be calculated using two steps. First is to assign proper number of valence electrons to the atom. In this case, both electrons of a lone pair are assigned to the atom on which they appear. In a covalent bond, all the electrons are assigned to the more electronegative atom. If the two bonded atoms are the same or have comparable electronegativities, then electrons get divided equally to both the atoms. Second is by comparing the assigned valence electrons to an atom to the atom’s group number. In this, each excess electron contributes -1 charge, while each electron the atom is lacking contributes +1 charge to the oxidation state. If a reactant species has a carbon atom that gains a bond to H or loses a bond to O during the course of the reaction, that species is typically undergoing reduction.

Question

Want to see the full answer?

Answer 1

Question

Chapter 17, Problem 17.38P

Interpretation Introduction

Interpretation:

It is to be verified whether imine is reduced in the given reaction, by calculating the oxidation state of the carbon and nitrogen atoms of the C=N group before and after the reaction. Further, it is to be determined whether imine gains electrons, and if so, how many.

Concept introduction:

The oxidation state of an atom can be calculated using two steps.

First is to assign proper number of valence electrons to the atom. In this case, both electrons of a lone pair are assigned to the atom on which they appear. In a covalent bond, all the electrons are assigned to the more electronegative atom. If the two bonded atoms are the same or have comparable electronegativities, then electrons get divided equally to both the atoms.

Second is by comparing the assigned valence electrons to an atom to the atom’s group number. In this, each excess electron contributes -1 charge, while each electron the atom is lacking contributes +1 charge to the oxidation state.

If a reactant species has a carbon atom that gains a bond to H or loses a bond to O during the course of the reaction, that species is typically undergoing reduction.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Below is the SN1 reaction of (S)-3-chlorocyclohexene and hydroxide (OH). Draw the missing curved arrows, lone pairs of electrons, and nonzero formal charges. In the third box, draw the two enantiomeric products that will be produced. 5th attempt Please draw all four bonds at chiral centers. Draw the two enantiomeric products that will be produced. Draw in any hydrogen at chiral centers. 1000 4th attempt Feedback Please draw all four bonds at chiral centers. 8. R5 HO: See Periodic Table See Hint H Cl Br Jid See Periodic Table See Hint

Show that a molecule with configuration π4 has a cylindrically symmetric electron distribution. Hint: Let the π orbitals be equal to xf and yf, where f is a function that depends only on the distance from the internuclear axis.

(a) Verify that the lattice energies of the alkali metal iodides are inversely proportional to the distances between the ions in MI (M = alkali metal) by plotting the lattice energies given below against the internuclear distances dMI. Is the correlation good? Would a better fit be obtained by plotting the lattice energies as a function of (1 — d*/d)/d, as theoretically suggested, with d* = 34.5 pm? You must use a standard graphing program to plot the graph. It generates an equation for the line and calculates a correlation coefficient. (b) From the graph obtained in (a), estimate the lattice energy of silver iodide. (c) Compare the results of (b) with the experimental value of 886 kJ/mol. If they do not agree, explain the deviation.