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Organic Chemistry 1 > Chapter 3 > Flashcards

Chapter 3 Flashcards

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1
Q

A theory where an acid is a substance that can donate (lose) a proton; a base is a substance that can accept (or remove) a proton

A

Brønsted-Lowry acid-base theory

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2
Q

A substance that can donate (or lose) a proton

A

Brønsted-Lowry acid

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3
Q

A substance that can accept (or remove) a proton

A

Brønsted-Lowry base

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4
Q

A chemical species that bears an electrical charge

A

Ion

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5
Q

The molecule or ion that forms when an acid loses its proton

A

Conjugate base

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6
Q

The molecule or ion that forms when a base accepts a proton

A

Conjugate acid

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7
Q

A substance that can transfer two protons

A

Diprotic acid

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8
Q

When an ionic compound dissolves in water

A

Solvated

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9
Q

Ions that play no part in the acid-base reaction

A

Spectator ions

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10
Q

A reaction involving ions as reactants, intermediates, or products; occur through the heterolysis of covalent bonds

A

Ionic reaction

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11
Q

Show the direction of electron flow in a reaction mechanism; point from source of electron or electron pair to the atom receiving the electron or electron pair. Double-barbed arrows indicate movement of a pair of electrons; single-barbed arrows indicate the movement of a single electron. They are never used to show the movement of atoms

A

Curved arrows

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12
Q

An acid is an electron pair acceptor, and a base is an electron pair donor

A

Lewis acid-base theory

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13
Q

Is an electron pair acceptor

A

Lewis acid

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14
Q

Is an electron pair donor

A

Lewis base

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15
Q

The cleavage of a covalent bond so that one fragment departs with both of the electrons of the covalent bond that joined them; normally produces positive and negative ions

A

Heterolysis

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16
Q

A chemical species in which a trivalent carbon atom bears a formal positive charge

A

Carbocation

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17
Q

A chemical species in which a carbon atom bears a formal negative charge

A

Carbanion

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18
Q

A Lewis acid, an electron-pair acceptor, an electron-seeking reagent

A

Electrophile

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19
Q

A Lewis base, an electron pair donor that seeks a positive center in a molecule

A

Nucleophile

20
Q

The strength of an acid is related to its acidity content, Ka or to its pKa. The larger the value of the Ka or the smaller the value of its pKa, the stronger the acid

A

Acid strength

21
Q

An equilibrium constant related to the strength of an acid

A

Acidity constant (Ka)

22
Q

A constant that expresses the position of an equilibrium; it’s calculated by multiplying the molar concentrations of the products together and then dividing this number by the number obtained by multiplying together the molar concentrations of the reactants

A

Equilibrium constant (Keq)

23
Q

The negative logarithm of the acidity content, Ka

A

pKa

24
Q

The strength of a base is inversely related to the strength of its conjugate acid; weaker the conjugate acid, the stronger the base. If the conjugate acid has a large pKa, the base will be strong

A

Base strength

25
Q

The molecule or ion that forms when an acid loses its proton

A

Conjugate base

26
Q

An intrinsic electron-attracting or electron-releasing effect that results from a nearby dipole in the molecule and that is transmitted through space and through the bonds of a molecule

A

Inductive effect

27
Q

The capacity to do work

A

Energy

28
Q

Results from the motion of an object

A

Kinetic energy

29
Q

Stored energy; it exists when attractive or repulsive forces exist between objects

A

Potential energy

30
Q

The change in enthalpy after a system in its standard state has undergone a transformation to another system, also in its standard state

A

Enthalpy change (dH*)

31
Q

A reaction that evolves heat; for this type of reaction, dH* is negative

A

Exothermic reaction

32
Q

A reaction that absorbs heat; for this type of reaction, dH* is positive

A

Endothermic reaction

33
Q

The change in free energy between two systems in their standard states

A

Free-energy change (dG*)

34
Q

The change in entropy between two systems in their standard states; the more random a system is, the greater its entropy

A

Entropy change (dS*)

35
Q

An effect by which a substituent exerts either an electron-releasing or electron-withdrawing effect through the pi system of the molecule

A

Resonance

36
Q

The dispersal of electrons (or of electrical charge); always stabilizes a system

A

Delocalization effect

37
Q

An effect on the rate of reaction (or on the equilibrium constant) caused by the replacement of a hydrogen atom by another atom or group; includes those effects caused by the size of the atom or group, called steric effects, and those effects caused by the ability of the group to release or withdraw electrons, called electronic effects

A

Substituent effect

38
Q

A solvent whose molecules have a hydrogen atom attached to a strongly electronegative element such as oxygen or nitrogen

A

Protic solvent

39
Q

The conjugate acid of an alcohol

A

Protonated alcohol/alkyloxonium ion

40
Q

A chemical species with an oxygen atom that bears a formal positive charge

A

Oxonium ion

41
Q

A step-by-step description of the events that are postulated to take place at the molecular level as reactants are converted to products

A

Reaction mechanisms

42
Q

A reaction in which one group replaces another in a molecule

A

Substitution reaction

43
Q

An effect that restricts the use of certain solvents with strong acids and bases. On principle, no acid stronger than the conjugate acid of a particular solvent can exist to an appreciable extent in that solvent, and no base stronger than the conjugate base of the solvent can exist to an appreciable extent in that solvent

A

Leveling effect of a solvent

44
Q

Alkynes with a proton attached to a triply bonded carbon

A

Terminal alkynes

45
Q

RO- ions

A

Alkoxide ions

Organic Chemistry 1 (10 decks)

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