Kaplan Chemistry

Front 1

Anomers

Back 1

A subtype of epimers in which the chiral carbon with inverted configurations was the carbonyl carbon (anomeric carbon)

Front 2

Ceramide

Back 2

The simplest sphingolipid, with a single hydrogen as its head group

Front 3

Cerebroside

Back 3

A sphingolipid containing a carbohydrate as a head group

Front 4

Colligative Properties

Back 4

Vapor pressure depression, boiling point elevation, freezing point depression, and osmotic pressure

Front 5

Diprotic

Back 5

Containing 2 hydrogens (acid), or being able to pick up 2 hydrogens (base)

Front 6

Ganglioside

Back 6

A sphingolipid with a head group containing an oligosaccharide and one or more N-acetylneuraminic acid (NANA) molecules

Front 7

Globoside

Back 7

A sphingolipid with multiple carbohydrate groups attached as a head group

Front 8

Glucogenic

Back 8

Amino acids that can be converted into intermediates that feed into gluconeogenesis
(All amino acids, except Leucine and Lysine)

Front 9

Glycerol

Back 9

3-carbon alcohol backbone for glycerophospholipids, sphingolipids and triacylglycerols

Front 10

Glycosphingolipid

Back 10

A sphingolipid with a head group composed of sugars; includes cerebrosides and globosides

Front 11

Hess's Law

Back 11

A relationship that states that the total change in any state function is the same regardless of steps, and is equal to the difference between initial and final values of that state function

Front 12

Hormone-sensitive lipase

Back 12

The enzyme responsible for the mobilization of fatty acids from adipocytes; responds to a decrease in insulin levels

Front 13

Jacob-Monod Model

Back 13

The description of the structure and function of operons in prokaryotes, in which operons have structural genes, an operator site, a promoter site, and a regulator gene

Front 14

Lyase

Back 14

An enzyme that catalyzes the cleavage or synthesis of a molecule without the addition or loss of water

Front 15

Mutarotation

Back 15

the rapid interconversion between different anomers of a sugar

Front 16

NAD+ vs. NADP+

Back 16

NAD+: in ETC
NADP+: in PPP and immune function

Front 17

pKa

Back 17

The pH at which half of the molecules of a given acid are deprotonated;
[HA] = [A-]

Front 18

Prenylation

Back 18

The addition of lipid groups to a molecule

Front 19

Q Cycle

Back 19

The shuttling of electrons between uniquinol and ubiquinone in the inner mitochondrial membrane as a part of Complex III's function

Front 20

Reducing Sugars

Back 20

can reduce other compounds, and can be detected by Tollen's or Benedict's reagent

Front 21

Sialic Acid

Back 21

The common name of N-acetylneuraminic acid (NANA), which is the terminal portion of the head group in a ganglioside

Front 22

Sphingolipid

Back 22

A lipid containing sphingosine or sphingoid backbone, bonded to fatty acid tails;
Include ceramide, sphingomyelins, glycosphingolipids, and gangliosides

Front 23

Sphingomyelin

Back 23

A sphingolipid containing a sphingosine backbone and a phosphate head group

Front 24

Terpene

Back 24

A class of lipids built from isoprene moieties; have carbon groups in multiples of 5

Front 25

Tight Junctions

Back 25

cell-cell junctions that prevent the paracellular transport of materials; tight junctions form a collar around cells and link cells within a single layer

Front 26

Aldol Condensation

Back 26

A reaction where an aldehyde or a ketone acts as both the electrophile and nucleophile, resulting in the formation of a carbon-carbon bond in a new molecule, called an aldol

Front 27

Azimuthal Quantum Number (l)

Back 27

Describes the subshell in which an electron is found; possible values range from 0 to n-1
l=0=s
l=1=p

l=2=d

l=3=f

Front 28

Constitutional Isomers

Back 28

Molecules that have the same molecular formulas but different connectivity; also called structural isomers

Front 29

Deshielding

Back 29

The phenomenon of atoms pulling electron density away from surrounding atoms; in NMR spectroscopy, pulls a group further downfield on the spectrum

Front 30

Diastereomers

Back 30

Non-mirror-image configurational isomers that differ at at least one, but not all, chiral carbons;
Have different chemical and physical properties

Front 31

Doublet

Back 31

2 peaks of identical intensity in an NMR spectrum that are equally spaced around the true chemical shift of a group of protons;
results from splitting by another hydrogen

Front 32

Downfield

Back 32

Movement toward the left in an NMR spectrum

Front 33

Enantiomers

Back 33

Nonsuperimposable mirror images of a chiral molecule; have all the same physical and chemical properties except for rotation of plane-polarized light and reactions in a chiral environment

Front 34

Fingerprint Region

Back 34

In an IR spectrum, the region of 1500 to 400 cm(^-1) where more complex vibration patterns, caused by the motion of the molecule as a whole, can be seen; it is characteristic of each individual molecule

Front 35

Fischer Esterification

Back 35

The formation of an ester from a carboxylic acid and an alcohol in acidic conditions

Front 36

Flash Column Chromatography

Back 36

A technique that speeds up column chromatography by forcing the solvent through the column by increasing pressure with a nonreactive gas

Front 37

Fractional Distillation

Back 37

A modified form of distillation used to separate 2 liquids with similar boiling points (less than 25 degrees Celsius apart); uses a fractionation column, which contains inert materials onto which the liquids can condense and reflux back into the reaction vial, allowing more refined separation.

Front 38

Gabriel (malonic-ester) Synthesis

Back 38

A method synthesizing amino acids that uses potassium pthalimide and diethyl bromomalonate followed by an alkyl halide; 2 substitution reactions are followed by hydrolysis and decarboxylation

Front 39

Gas Chromatography

Back 39

A type of chromatography used to separate vaporizable compounds; the stationary phase is a crushed metal or polymer, and the mobile phase is a nonreactive gas

Front 40

Highest Occupied Molecular Orbital (HOMO)

Back 40

The highest-energy molecular orbital containing electrons; in UV spectroscopy, electrons are excited from the HOMO to the LUMO

Front 41

Jones Oxidation

Back 41

An oxidation reaction in which primary alcohols are oxidized to carboxylic acids and secondary alcohols are oxidized to ketones; requires CrO3 dissolved with dilute sulfuric acid in acetone

Front 42

Lowest Unoccupied Molecular Orbital (LUMO)

Back 42

The lowest energy molecular orbital that does not contain electrons; in UV spectroscopy, electrons are excited from the HUMO to the LUMO

Front 43

Meso Compound

Back 43

A molecule that has chiral centers but is not optically active because it has an internal plane of symmetry

Front 44

Michael Addition

Back 44

A reaction in which a carbanion attacks an alpha,beta-unsaturated carbonyl

Front 45

Multiplet

Back 45

Peaks that have more than 4 shifts in NMR spectroscopy

Front 46

Node

Back 46

In orbital structure, an area where the probability of finding an electron is zero

Front 47

p-orbital

Back 47

An atomic orbital that is composed of 2 lobes located symmetrically about the nucleus and contains a node

Front 48

Partitioning

Back 48

When components in a sample adhere differentially to the mobile and stationary phases of a chromatographic setup; this causes the different substances to migrate at different speeds through the stationary phase

Front 49

Principal Quantum Number (n)

Back 49

Describes the shell in which an electron is found; values range from 1 to infinity

Front 50

Retro-aldol Reaction

Back 50

The reverse of an Aldol Condensation Reaction, in which a carbon-carbon bond is cleaved with heat and base, yielding 2 aldehydes, 2 ketones, or one of each

Front 51

s-orbital

Back 51

An atomic orbital that is spherical and symmetrical, centered on the nucleus

Front 52

sp

Back 52

50% s-character and 50% p-character

Front 53

sp2

Back 53

33% s-character and 67% p-character

Front 54

sp3

Back 54

25% s-character and 75% p-character

Front 55

Spin quantum number (Ms)

Back 55

Describes the intrinsic spin of the 2 electrons in an orbital by arbitrarily assigning one of the electrons a spin of +(1/2) and the other a spin of -(1/2)

Front 56

Staggered Conformation

Back 56

When a molecule has no overlapping substituents along the line of sight between 2 carbons, as in a Newman projection

Front 57

Stationary Phase

Back 57

A solid medium onto which a sample is placed for chromatography; also called the adsorbent

Front 58

Strecker Synthesis

Back 58

A method of synthesizing amino acids that uses condensation between an aldehyde and hydrogen cyanide, followed by hydrolysis

Front 59

Transesterification

Back 59

The process that transforms one ester to another when an alcohol acts as a nucleophile and displaces the alkoxy group on an ester

Front 60

Triplet

Back 60

3 peaks with an area ratio of 1:2:1 in an NMR spectrum that are centered around the true chemical shift of a group of protons; results from splitting by 2 equivalent hydrogens

Front 61

Upfield

Back 61

Movement to the right in an NMR spectrum

Front 62

Wavenumber

Back 62

An analog of frequency used for infrared spectra instead of wavelength

Front 63

Adiabatic Process

Back 63

A process that occurs without the transfer of heat into or out of the system

Front 64

Alkali Metals

Back 64

Elements in Group IA;
Highly reactive, readily losing one valence electron to form ionic compounds with nonmetals

Front 65

Alkaline Earth Metals

Back 65

Elements in Group IIA;
2+ cations with similar properties as Alkali Metals

Front 66

Arrhenius Acid

Back 66

A species that donates hydroxide ions (OH-) in aqueous solutions

Front 67

Aufbau Principle

Back 67

The concept that electrons fill energy levels in order of increasing energy levels in order of increasing energy, completely filling one sublevel before begining to fill the next

Front 68

Balmer Series

Back 68

Part of the emission spectrum for hydrogen, representing transitions of an electron from energy levels n > 2 to n=2

Front 69

Base Dissociation Constant (Kb)

Back 69

The equilibrium constant that measures the degree of dissociation for a base under specific conditions

Front 70

Boyle's Law

Back 70

The law stating that at constant temperature, the volume of a gaseous sample is inversely proportional to its pressure

Front 71

Bronsted-Lowry Acid

Back 71

A proton donor

Front 72

Bronsted-Lowry Base

Back 72

A proton acceptor

Front 73

Chalcogens

Back 73

Elements in Group VIA;
The group contains metals, nonmetals (like Oxygen), and metalloids;
Typically form -2 anions

Front 74

Charle's Law

Back 74

The law stating that the volume of a gas at constant pressure is directly proportional to its absolute (kelvin) temperature.

Front 75

Concentration Cell

Back 75

A cell that creates an electromotive force (emf or voltage) using a single chemical species in half-cells of varying concentration

Front 76

Dalton's Law of Partial Pressures

Back 76

The law stating that the sum of the partial pressures of the components of a gaseous mixture must equal the total pressure of the sample

Front 77

Daniell Cell

Back 77

An electrochemical cell in which the anode is the site of Zn metal oxidation and the cathode is the site of Cu++ ion reduction

Front 78

Delocalized Orbitals

Back 78

Molecular orbitals in which electron density is spread over an entire molecule, or a portion thereof, rather than being localized between two atoms

Front 79

Deposition

Back 79

Gas --> solid,
Or the buildup of a solid precipitate onto an electrode in electrochemical reactions

Front 80

Disproportionation (Dismutation)

Back 80

A redox reaction in which the same species acts as the oxidizing agent and as the oxidizing agent and as the reducing agent

Front 81

Effusion

Back 81

Movement of gas from one compartment to another under pressure through a small opening; follows Graham's law

Front 82

Electrolysis

Back 82

The process in which an electrical current is used to power an otherwise nonspontaneous decomposition reaction

Front 83

Emission Spectrum

Back 83

A series of discrete lines at characteristic frequencies, each representing the energy emitted when electrons in an atom return from an excited state to their ground state

Front 84

Faraday Constant (F)

Back 84

The total charge on 1 mole of electrons
F= 96,485 C/mol e-

Front 85

First Law of Thermodynamics

Back 85

The law stating that the total energy of a system and its surroundings remain constant

Front 86

First-order reaction

Back 86

A reaction in which the rate is directly proportional to the concentration of only one reactant

Front 87

Formal Charge

Back 87

The conventional assignment of charges to individual atoms of a Lewis structure for a molecule;
The total number of valence electrons in the free atom minus the total number of electrons when the atom is bonded

Front 88

Galvanic Cell

Back 88

An electrochemical cell that uses a spontaneous oxidation-reduction reaction to generate an electromotive force;
Also called a voltaic cell

Front 89

Gay-Lussac's Law

Back 89

The law stating that the pressure of a gaseous sample at constant volume is directly proportional to its absolute temperature

Front 90

Graham's Law

Back 90

The law stating that the rate of effusion or diffusion for a gas is inversely proportional to the square root of the gas's molar mass

Front 91

Henderson-Hasselbalch equation

Back 91

Equation showing the relationship of the pH or pOH of a solution of a solution to the pKa or pKb and the ratio of the concentrations of the dissociated species

Front 92

Henry's Law

Back 92

The law stating that the mass of a gas that dissolves in a solution is directly proportional to the partial pressure of the gas above the solution

Front 93

Hess's Law

Back 93

The law stating that the energy change in an overall reaction is equal to the sum of the energy changes in the individual reactions that comprise it

Front 94

Hund's Rule

Back 94

The rule that electrons will fill into separate orbitals with parallel spins before pairing within an orbital

Front 95

Intermolecular Vs. Intramolecular

Back 95

Inter- :between molecules
Intra- :within a molecule

Front 96

Isobaric Process

Back 96

A process that occurs at constant pressure

Front 97

Law of Mass Action

Back 97

The form of the equilibrium constant;
has the concentrations of products over concentrations of reactants, each raised to their stoichiometric coefficients

Front 98

Maxwell-Boltzmann Distribution Curve

Back 98

The distribution of the molecular speeds of gas particles at a given temperature;
As temperature increases, average speed increases and the distribution becomes wider and flatter

Front 99

Mixed-Order Reaction

Back 99

A reaction in which the reaction order changes over time in the rate law

Front 100

Molality (m)

Back 100

moles of solute / Kg of solvent

Front 101

Molarity (M)

Back 101

moles of solute / L of solution

Front 102

Normality (N)

Back 102

a concentration unit equal to the number of equivalents per liter of solution

Front 103

Raoult's Law

Back 103

A law stating that the partial pressure of a component in a solution is proportional to the mole fraction of that component in the solution;
Provides an explanation for vapor pressure depression seen in solutions

Front 104

Reaction Quotient (Q)

Back 104

Has the same form as the equilibrium constant, but the concentrations of products and reactants may not be at equlibrium;
When compared to Keq, it dictates the direction a reaction will proceed spontaneously

Front 105

Second Law of Thermodynamics

Back 105

The law stating that all spontaneous processes lead to an increase in the entropy of the universe

Front 106

Spectator Ions

Back 106

Ions involved in a reaction that do not change formula, charge, or phase;
Normally omitted from the net ionic equation

Front 107

Adiabatic

Back 107

A thermodynamic process that occurs with no heat exchange

Front 108

Antinode

Back 108

A point of zero displacement in a standing wave

Front 109

Archimedes Principle

Back 109

States that a body immersed in a volume of fluid experiences a buoyant force equal to the weight of the displaced fluid

Front 110

Attenuation

Back 110

The loss of energy of a propagating wave as a result of nonconservative forces; also known as damping

Front 111

Bernoulli's Equation

Back 111

An equation that relates static and dynamic pressure for a fluid to the pressure exerted on the walls of a tube and the speed of the fluid

Front 112

Confounding

Back 112

An error that results when a causal variable is associated with 2 other variables in a study but is not accounted for;
May falsely indicate that the 2 variables are associated

Front 113

Coulomb's Law

Back 113

Relates the electrostatic force between 2 charged particles to their charges and the distance between them

Front 114

Dielectric Material

Back 114

An insulating material used to increase capacitance

Front 115

Equipoise

Back 115

The state of not knowing whether there is a difference between two interversions;
Ethically necessary for comparative study of the interventions

Front 116

External Validity

Back 116

The ability to apply findings of a research study to other populations;
Also called generalizability

Front 117

FINER method

Back 117

A way to determine the usefulness of a research question on the basis of feasibility, interest, novelty, ethics, and relevance

Front 118

Focal Length

Back 118

The distance from a mirror or lens to the focal point

Front 119

Focal Point

Back 119

The point at which rays of light parallel to the axis of a mirror or lens converge, or from which they appear to diverge when reflected by a mirror or refracted by a lens

Front 120

Hawthorne Effect

Back 120

The tendency for research participants to change their behavior because they know they are being observed

Front 121

Kirchoff's Laws

Back 121

Rules that describe the conservation of charge and conservation of charge and conservation of energy within an electric circuit; includes the junction rule and loop rule

Front 122

Mass defect

Back 122

The difference between the sum of the masses of unbound nucleons forming a nucleus and the mass of that nucleus in the bound state

Front 123

Null Hypothesis

Back 123

The hypothesis of no difference;
Given enough statistical evidence, the null hypothesis may be rejected (idgi???)

Front 124

Pascal's Principle

Back 124

States that pressure applied to a noncompressible fluid is distributed equally to all points within that fluid and the walls of the container

Front 125

Poiseuille's Law

Back 125

Relates viscosity, tube dimensions, and pressure differentials to the rate of flow between 2 points in a system

Front 126

Snell's Law

Back 126

Relates the incident angle, refracted angle, and indices of refraction for two media

Front 127

Venturi Effect

Back 127

Describes the relationship between the continuity equation and Bernoulli's equation;
As cross-sectional area of a tube decreases, the speed of the fluid increases, and the pressure exerted on the walls of the tube decreases