Organic Chemistry (Italiano) — Avanzato (C1/C2) 1: Chemical Kinetics, Equilibrium, Electrochemistry & Organic Functional Groups

Question 1

What thermodynamic equation connects standard cell potential (E°cell) to the equilibrium constant (K) at 298.15 K?

Accepted Answer

E°cell = $$(R*T / (n*F)) * ln(K) = (0.0592 V / n) * log10(K)$$.

Question 2

Why are aliphatic amines basic and nucleophilic in organic reactions?

Accepted Answer

The nitrogen atom possesses a non-bonding lone pair of electrons available to accept a proton (Brønsted base) or attack electrophilic centers (Lewis base/nucleophile).

Question 3

What condition involving ion product (Qsp) and solubility product (Ksp) indicates that a precipitate will form?

Accepted Answer

A precipitate forms when $$Qsp > Ksp$$ (supersaturated solution).

Question 4

What is the general differential rate law for a reaction $$aA + bB$$ -> products, and how are reaction orders determined?

Accepted Answer

Rate = $$k[A]^m[B]^n$$, where m and n are reaction orders with respect to A and B, determined strictly experimentally (not from stoichiometric coefficients).

Question 5

What products are obtained by oxidizing a primary alcohol versus a secondary alcohol with strong oxidizing agents (e.g., KMnO4 or Jones reagent)?

Accepted Answer

Primary alcohols are oxidized to carboxylic acids (via aldehyde intermediates); secondary alcohols are oxidized to ketones (tertiary alcohols resist oxidation).

Question 6

How are primary (1°), secondary (2°), and tertiary (3°) alcohols classified structurally?

Accepted Answer

By the number of carbon atoms bonded to the carbinol carbon carrying the -OH group: 1° is bonded to one carbon, 2° to two carbons, and 3° to three carbons.

Question 7

Write the Arrhenius equation and identify all variables and physical constants.

Accepted Answer

$$k = A * exp(-Ea / (R*T))$$, where k is rate constant, A is pre-exponential frequency factor, Ea is activation energy, R is gas constant (8.314 J/(mol*K)), and T is temperature in Kelvin.

Question 8

What is the relationship between enantiomers and diastereomers in stereochemistry?

Accepted Answer

Enantiomers are non-superimposable mirror-image stereoisomers with identical physical properties except optical rotation; diastereomers are stereoisomers that are not mirror images and possess different physical and chemical properties.

Question 9

What is the rate-determining step (RDS) in a multi-step reaction mechanism?

Accepted Answer

The slowest elementary step with the highest activation energy barrier, which dictates the overall reaction rate and rate law.

Question 10

What functional group results from the condensation reaction between a carboxylic acid derivative and an amine?

Accepted Answer

An amide bond (-CO-NRR').

Question 11

In an electrochemical cell, which electrode is the site of oxidation, and which is the site of reduction?

Accepted Answer

Oxidation always occurs at the anode (An Ox); reduction always occurs at the cathode (Red Cat).

Question 12

How is the standard cell potential (E°cell) calculated from standard reduction potentials (E°red)?

Accepted Answer

E°cell = E°red(cathode) - E°red(anode). A positive E°cell denotes a thermodynamically spontaneous reaction.

Question 13

What is dynamic chemical equilibrium, and what is true regarding forward and reverse reaction rates?

Accepted Answer

A closed system state where the rates of forward and reverse reactions are equal ($$rf = rr$$), resulting in constant macroscopic concentrations over time.

Question 14

How do galvanic cells and electrolytic cells differ in spontaneity and external energy requirements?

Accepted Answer

Galvanic cells produce electrical energy spontaneously from chemical reactions ($$ΔG < 0$$, Ecell $$> 0$$); electrolytic cells consume external electrical voltage to drive non-spontaneous reactions ($$ΔG > 0$$, Ecell $$< 0$$).

Question 15

Which plotted variables yield a straight line for zero-order, first-order, and second-order integrated rate laws?

Accepted Answer

Zero-order: $$[A]$$ vs t (slope = -k); First-order: $$ln[A]$$ vs t (slope = -k); Second-order: $$1/[A]$$ vs t (slope = +k).

Question 16

Write the Nernst equation for calculating non-standard cell potential (Ecell).

Accepted Answer

Ecell = E°cell $$- (R*T / (n*F)) * ln(Q) = E$$°cell - (0.0592 V / n) * log10(Q) at 298 K.

Question 17

According to Le Chatelier's principle, how does increasing system pressure by decreasing volume affect a gaseous equilibrium?

Accepted Answer

The equilibrium shifts toward the side of the balanced equation with fewer total moles of gas to relieve the pressure.

Question 18

What is the solubility product constant (Ksp) expression for the dissolution of silver chromate, $$Ag2CrO4(s) <-> 2$$ $$Ag+(aq) + CrO4^2-(aq)$$?

Accepted Answer

$$Ksp = [Ag+]^2 * [CrO4^2-]$$, with solids omitted from mass action expressions.

Question 19

What defines a chiral center (stereocenter) in an organic molecule?

Accepted Answer

An sp3-hybridized tetrahedral carbon atom bonded to four chemically distinct substituent groups.

Question 20

What chemical transformation occurs during Fischer esterification?

Accepted Answer

A carboxylic acid reacts with an alcohol in the presence of an acid catalyst to produce an ester and water via nucleophilic acyl substitution.

Question 21

What is the role of a salt bridge in a galvanic (voltaic) cell?

Accepted Answer

To maintain electrical neutrality by permitting spectator anions to migrate toward the anode and cations toward the cathode, preventing charge buildup.

Question 22

How does a chemical catalyst accelerate a reaction without being consumed?

Accepted Answer

It provides an alternative reaction pathway with a lower activation energy (Ea), increasing rate constants of both forward and reverse reactions equally.

Question 23

How does raising the temperature affect the equilibrium constant (K) for an exothermic reaction versus an endothermic reaction?

Accepted Answer

For an exothermic reaction (heat as product), increasing T decreases K (shifts left); for an endothermic reaction (heat as reactant), increasing T increases K (shifts right).

Question 24

What is the relationship between the equilibrium constants Kc and Kp for an ideal gas reaction?

Accepted Answer

$$Kp = Kc * (R*T)^Δn$$, where Δn = (moles of gaseous products) - (moles of gaseous reactants), and $$R = 0.08206 L*atm/(mol*K)$$.

Question 25

What is the half-life equation for a first-order chemical reaction, and why is it unique?

Accepted Answer

$$t_1/2 = ln(2) / k ≈ 0.693 / k$$; it is completely independent of the initial reactant concentration $$[A]0$$.

Question 26

What structural feature distinguishes an aldehyde from a ketone?

Accepted Answer

Both contain a carbonyl group ($$C=O$$); an aldehyde has the carbonyl bonded to at least one hydrogen atom (terminal R-CHO), while a ketone has the carbonyl bonded to two carbon groups (internal R-CO-R').

Question 27

What defines an electrophile versus a nucleophile in organic reaction mechanisms?

Accepted Answer

An electrophile is an electron-deficient species (Lewis acid) seeking electron density; a nucleophile is an electron-rich species with a lone pair or pi bond (Lewis base) that donates electrons to form a bond.

Question 28

What defines aromaticity in planar cyclic conjugated molecules according to Hückel's rule?

Accepted Answer

The ring must be cyclic, planar, fully conjugated with a continuous ring of p-orbitals, and contain (4n + 2) pi electrons (where n is a non-negative integer: 2, 6, 10, 14...).

Question 29

What thermodynamic equation relates standard Gibbs free energy change (ΔG°) to standard cell potential (E°cell)?

Accepted Answer

ΔG° = -n * F * E°cell, where n is moles of transferred electrons and F is Faraday's constant (96,485 C/mol e-).

Question 30

How does comparing the reaction quotient (Q) to the equilibrium constant (K) predict the direction of net reaction?

Accepted Answer

If $$Q < K$$, forward reaction proceeds (shifts right); if $$Q = K$$, system is at equilibrium; if $$Q > K$$, reverse reaction proceeds (shifts left).

Question 31

What are the units of the rate constant (k) for zero-order, first-order, and second-order chemical reactions?

Accepted Answer

Zero-order: M/s (mol/(L*s)); First-order: $$s^-1$$; Second-order: $$M^-1 * s^-1$$ (L/(mol*s)).

Question 32

What is the common ion effect on salt solubility?

Accepted Answer

The solubility of a sparingly soluble salt is markedly decreased in the presence of a soluble second salt that shares a common ion, driven by Le Chatelier's shift.

#	Front (Term / Question)	Back (Definition / Answer)
1	What thermodynamic equation connects standard cell potential (E°cell) to the equilibrium constant (K) at 298.15 K?	E°cell = (RT / (nF)) * ln(K) = (0.0592 V / n) * log10(K).
2	Why are aliphatic amines basic and nucleophilic in organic reactions?	The nitrogen atom possesses a non-bonding lone pair of electrons available to accept a proton (Brønsted base) or attack electrophilic centers (Lewis base/nucleophile).
3	What condition involving ion product (Qsp) and solubility product (Ksp) indicates that a precipitate will form?	A precipitate forms when Qsp > Ksp (supersaturated solution).
4	What is the general differential rate law for a reaction aA + bB -> products, and how are reaction orders determined?	Rate = k[A]^m[B]^n, where m and n are reaction orders with respect to A and B, determined strictly experimentally (not from stoichiometric coefficients).
5	What products are obtained by oxidizing a primary alcohol versus a secondary alcohol with strong oxidizing agents (e.g., KMnO4 or Jones reagent)?	Primary alcohols are oxidized to carboxylic acids (via aldehyde intermediates); secondary alcohols are oxidized to ketones (tertiary alcohols resist oxidation).
6	How are primary (1°), secondary (2°), and tertiary (3°) alcohols classified structurally?	By the number of carbon atoms bonded to the carbinol carbon carrying the -OH group: 1° is bonded to one carbon, 2° to two carbons, and 3° to three carbons.
7	Write the Arrhenius equation and identify all variables and physical constants.	k = A * exp(-Ea / (RT)), where k is rate constant, A is pre-exponential frequency factor, Ea is activation energy, R is gas constant (8.314 J/(molK)), and T is temperature in Kelvin.
8	What is the relationship between enantiomers and diastereomers in stereochemistry?	Enantiomers are non-superimposable mirror-image stereoisomers with identical physical properties except optical rotation; diastereomers are stereoisomers that are not mirror images and possess different physical and chemical properties.
9	What is the rate-determining step (RDS) in a multi-step reaction mechanism?	The slowest elementary step with the highest activation energy barrier, which dictates the overall reaction rate and rate law.
10	What functional group results from the condensation reaction between a carboxylic acid derivative and an amine?	An amide bond (-CO-NRR').
11	In an electrochemical cell, which electrode is the site of oxidation, and which is the site of reduction?	Oxidation always occurs at the anode (An Ox); reduction always occurs at the cathode (Red Cat).
12	How is the standard cell potential (E°cell) calculated from standard reduction potentials (E°red)?	E°cell = E°red(cathode) - E°red(anode). A positive E°cell denotes a thermodynamically spontaneous reaction.
13	What is dynamic chemical equilibrium, and what is true regarding forward and reverse reaction rates?	A closed system state where the rates of forward and reverse reactions are equal (rf = rr), resulting in constant macroscopic concentrations over time.
14	How do galvanic cells and electrolytic cells differ in spontaneity and external energy requirements?	Galvanic cells produce electrical energy spontaneously from chemical reactions (ΔG < 0, Ecell > 0); electrolytic cells consume external electrical voltage to drive non-spontaneous reactions (ΔG > 0, Ecell < 0).
15	Which plotted variables yield a straight line for zero-order, first-order, and second-order integrated rate laws?	Zero-order: [A] vs t (slope = -k); First-order: ln[A] vs t (slope = -k); Second-order: 1/[A] vs t (slope = +k).
16	Write the Nernst equation for calculating non-standard cell potential (Ecell).	Ecell = E°cell - (RT / (nF)) * ln(Q) = E°cell - (0.0592 V / n) * log10(Q) at 298 K.
17	According to Le Chatelier's principle, how does increasing system pressure by decreasing volume affect a gaseous equilibrium?	The equilibrium shifts toward the side of the balanced equation with fewer total moles of gas to relieve the pressure.
18	What is the solubility product constant (Ksp) expression for the dissolution of silver chromate, Ag2CrO4(s) <-> 2 Ag+(aq) + CrO4^2-(aq)?	Ksp = [Ag+]^2 * [CrO4^2-], with solids omitted from mass action expressions.
19	What defines a chiral center (stereocenter) in an organic molecule?	An sp3-hybridized tetrahedral carbon atom bonded to four chemically distinct substituent groups.
20	What chemical transformation occurs during Fischer esterification?	A carboxylic acid reacts with an alcohol in the presence of an acid catalyst to produce an ester and water via nucleophilic acyl substitution.
21	What is the role of a salt bridge in a galvanic (voltaic) cell?	To maintain electrical neutrality by permitting spectator anions to migrate toward the anode and cations toward the cathode, preventing charge buildup.
22	How does a chemical catalyst accelerate a reaction without being consumed?	It provides an alternative reaction pathway with a lower activation energy (Ea), increasing rate constants of both forward and reverse reactions equally.
23	How does raising the temperature affect the equilibrium constant (K) for an exothermic reaction versus an endothermic reaction?	For an exothermic reaction (heat as product), increasing T decreases K (shifts left); for an endothermic reaction (heat as reactant), increasing T increases K (shifts right).
24	What is the relationship between the equilibrium constants Kc and Kp for an ideal gas reaction?	Kp = Kc * (RT)^Δn, where Δn = (moles of gaseous products) - (moles of gaseous reactants), and R = 0.08206 Latm/(mol*K).
25	What is the half-life equation for a first-order chemical reaction, and why is it unique?	t_1/2 = ln(2) / k ≈ 0.693 / k; it is completely independent of the initial reactant concentration [A]0.
26	What structural feature distinguishes an aldehyde from a ketone?	Both contain a carbonyl group (C=O); an aldehyde has the carbonyl bonded to at least one hydrogen atom (terminal R-CHO), while a ketone has the carbonyl bonded to two carbon groups (internal R-CO-R').
27	What defines an electrophile versus a nucleophile in organic reaction mechanisms?	An electrophile is an electron-deficient species (Lewis acid) seeking electron density; a nucleophile is an electron-rich species with a lone pair or pi bond (Lewis base) that donates electrons to form a bond.
28	What defines aromaticity in planar cyclic conjugated molecules according to Hückel's rule?	The ring must be cyclic, planar, fully conjugated with a continuous ring of p-orbitals, and contain (4n + 2) pi electrons (where n is a non-negative integer: 2, 6, 10, 14...).
29	What thermodynamic equation relates standard Gibbs free energy change (ΔG°) to standard cell potential (E°cell)?	ΔG° = -n * F * E°cell, where n is moles of transferred electrons and F is Faraday's constant (96,485 C/mol e-).
30	How does comparing the reaction quotient (Q) to the equilibrium constant (K) predict the direction of net reaction?	If Q < K, forward reaction proceeds (shifts right); if Q = K, system is at equilibrium; if Q > K, reverse reaction proceeds (shifts left).
31	What are the units of the rate constant (k) for zero-order, first-order, and second-order chemical reactions?	Zero-order: M/s (mol/(Ls)); First-order: s^-1; Second-order: M^-1 s^-1 (L/(mol*s)).
32	What is the common ion effect on salt solubility?	The solubility of a sparingly soluble salt is markedly decreased in the presence of a soluble second salt that shares a common ion, driven by Le Chatelier's shift.

Flashcards (32)