Kenneth Kang
Wednesday, June 25, 1997
Term Definition
Valence the electrons in the highest occupied energy level of an
ElectronsValence element's atom
Electrons
isoelectronicisoelec two ions that share an electron shell configuration
tronic
Electron dot a depiction of valence electrons as dots drawn around the
structuresElectron symbol of the element
dot structures
octet ruleoctet Atoms react by changing the number of their electrons so
rule as to acquire the stable electron structure of a noble
gas.
anionanion negatively charged ion
cationcation positively charged ion
halied ionshalied the Ions that form from group 7A
ions
ionic bondbondionic forces of attraction that bind opposite charged ions
together
coordination the number of ions of opposite charge that surround each
numbercoordination ion in a crystal
number
metallic consist of the attraction of the free-floating valence
bondbondmetallic electrons for the positively charged metal ions
Table 1: Chapter 13 Terms
Term Definition
structure chemical formulas that show the arrangement of atoms in
formulastructure molecules and polyatomic ions
formula
single covalent formed when a pair of electrons is shared between two
bondbondsingle atoms
covalent
unshared pairsunshared the pairs of valence electrons that are not shared
pairs between atoms
double covalent two shared pairs of electrons
bondbonddouble
covalent
triple covalent three shared pairs of electrons
bondbondtriple
covalent
coordinate covalent when one atom contributes both bonding electrons in a
bondbondcoordinate covalent bond
covalent
resonanceresonance when two or more equally valid electron dot structures
can be written for a molecule
paramagneticparamagneti a substance that shows a relatively strong attraction
c to an external magnetic field
molecular the overlapping atomic orbitals of two covalently
orbitalmolecular bonded atoms
orbital
bonding orbitalbonding a molecular orbital whose energy is lower than that of
orbital the atomic orbitals from which it is formed
antibonding a molecular orbital whose energy is higher than that of
orbitalantibonding the atomic orbitals from which it is formed
orbital
sigma bondbondsigma a bonded orbital that is symmetriacal along the axis
connecting the two nuclei
pi bondbondpi a sausage-shaped region above and below the bond axis
tetrahedral 109.5°
angletetrahedral angle
VSEPR theoryVSEPR because electrons paires repel, molecules adjust so
theory that the valence-electron are as far apart as possible
(valence-shell electron-pair repulsion)
hybridizationhybridizat several atomic orbitals mix to form the same number of
ion equivalent hybrid orbitals
nonpolar covalent a bond where electrons are shared equall y
bondbondnonpolar
covalent
polar covalent a bond of two unlike atoms where electrons are hogged
bondbondpolar covalent by one of them
polar bondbondpolar the same as a polar covalent bond
polar moleculepolar one end is slightly negative and the other end is
molecule slightly positive
dipoledipole a molecule with two poles
bond dissociation the energy required to break a single bond
energybonddissociation
energy
van der Waals all weak attractions between molecules
forcesvan der Waals
forces
dispersion weakest of all molecular interactions-thought to be
forcesdispersion caused by the motion of electrons
forces
dipole polar molecules' attraction to one another
interactionsdipole
interactions
hydrogen attractive forces in which hydrogen that is covealently
bondbondhydrogen bonded to a very electronegative atom in the same
molecule or a nearby molecule
network solidsnetwork stable substances whose atoms are all covalently bonded
solids to each other
Table 2: Chapter 14 Terms
Terms Definition
surface the inward force or pull which tends to minimize the surface
tensionsurface area of a liquid
tension
surfactantssurfac decreases surface tension (SURFace ACtive AgeNTS)
tants
aqueous water samples containing dissolved solids
solutionsaqueous
solutions
solventsolvent the dissolving medium
solutesolute the dissolved particles
solvationsolvatio a solute dissolving
n
effloresceefflore when a hydrate, with a higher vapor pressure than water,
sce loses the water of hydration
water of water in a crystal
hydrationwater
of hydration
hygroscopichygros compounds that remove moisture from air
copic
desiccantsdesicca hydgroscopic substances that are used as drying agents
nts
deliquescentdeliq compounds that remove sufficiant water from the air to
uescent dissolve and form solutions
electrolyteselect compounds that conduct an ellectric current in aqueous
rolytes solution or molten state
nonelectrolytesno coumpouds that do not conduct an electric current in aqueous
nelectrolytes solution or the molten state
weak a solution where only a fraction of the solute exists as ions
electrolyteelectr
olyteweak
strong a large portion of the solute exists as ions when dissolved
electrolyteelectr
olytestrong
suspensionssuspen mixtures from which some of the particles will settle slowly
sions upon standing
colloidscolloids mixtures containing particles that are intermediate in size
between those of suspensions and true solutions
Tyndall the scattering of visible light in all directions
effectTyndall
effect
Brownian the chaotic movement of collodial particles
motionBrownian
motion
emulsionsemulsion colloidal dispersion of liquids in liquids
s
Table 3: Chapter Terms
Terms Definition
saturated a solution conting the maximum amount of solute for a
solutionsaturated given amount of solvent at a constant temperature
solution
solubilitysolubility the amount of substance that dissolves in a given
quantity of solvent at a given temperature to produce a
saturated solution
unsaturatedunsaturated a solution that contains less solute than a saturated
solution
misciblemiscible two liquids that dissolve each other
immiscibleimmiscible liquids that are insoluble in one another
Henry's LawHenry's at a given temperature, the solutbility of a gas in a
Law liquidis directly proportional to the pressure of the
gas above the liquid
supersaturated a solution which containes more solute than it can
solutionsupersaturated theoretically hold at a given temperature
solution
concentrationconcentra a measure of the amount of solute that is dissolved in a
tion given quantity of solvent
dilute solutiondilute a solution that contains only a small amount of solute
solution
concentrated a solution that contains a large amount of solute
solutionconcentrated
solution
molaritymolarity the number of moles of a solute dissolved in 1 L of
solution
colligative properties that depend on the number of dissolved
propertiescolligative particles of a given mass of solvent
properties
boiling point the difference in temperature between the boiling points
elevationboiling of a solution and of the pure solvent
point elevation
freezing point the difference in temperature between the freezing
depressionfreezing points of a solution and of the pure solvent
point depression
molalitymolality the numnber of moles of solute dissolved in 1 kilgram of
solvent
mole fractionmole the ratio of the moles of solute in solution to the
fraction total number of moles of both solvent and solute
molal boiling point (Kb of Tb = Kbm ) the change in boiling point for a 1
elevation molal solution of a nonvolatile molecular solute
constantmolal boiling
point elevation
constant
molal freezing point the change in the freezing point for a 1 molal solution
depression of a nonvolatile molecular solute
constantmolal
freezing point
depression constant
Table 4: Chapter 16 Terms
Chapter 25 Hydrocarbon Compounds
Terms Definition
alkanesalkanes hydrocarbons that contain only single covalent bonds
continuous chain contain any number of carbon atoms in a straight
alkanescontinuous chain chain
alkanes
homologous constant increament of change in molecular structure
serieshomologous series from one compound in the series to the next
condensed structural diagrams which leave out some bonds and atoms from
formulacondensed the structural formula
structural formula
IUPAC SystemIUPAC System the system of naming organic compounds
(International Union of Pure and Applied Chemistry)
substituentsubstituent an atom or a group of atoms that can take the place
of a hydrogen atom on a parent hydrocarbon molecule
alkyl groupalkyl group a hydrocarbon substituent
branced chain an alkane with one or more alkyl groups
alkanebranced chain
alkane
hydrocarbonshydrocarbons organic compounds that contain only carbon and
hydrogen
structural compounds that have the same molecular formula but
isomersstructural isomers different molecular structures
unsaturated organic compound containing double and triple
compoundsunsaturated carbon-carbon bonds
compounds
alkenesalkenes organic compounds containing carbon-carbon double
bonds
alkynesalkynes organic compounds containing carbon-carbon triple
bonds
trans configurationtrans where the substituted groups are o opposite side s
configuration of the double bond
cis configurationcis where the substitued groups are on the smae side of
configuration the double bond
geometric where compounds differ only in the geometry of their
isomersgeometric isomers substituted groups
asymmetric a carbon with four different groups attached
carbonasymmetric carbon
stereoisomersstereoisomers molecules of the same molecular structure that
differ only in the arrangement of the atoms in space
cyclic hydrocarbonscyclic caompounds that contain a hydrocarbon ring
hydrocarbons
aliphatic all hydrocarbons compounds which do not contain
compoundsaliphatic rings
compounds
arenesarenes unsaturated cyclic hydrocarbons
aromatic compoundaromatic any substance in whic the bonding is like that of
compound benzene
crackingcracking a controlled process by which hydrocarbons are
broken down or rearranged into smaller, more useful
molecules
Table 5: Terms
Term Definition
functional a specific arrangement of atoms in an organic compound that is
groupfunctional capable of characteristic chemical reaction
group
halocarbonshaloc a class of organic compounds containing covalently bonded
arbons fluorine, chlorine, bromine, or iodine
alkyl halocarbons in which a halogen is attached to a carbon of an
halidesalkyl aliphatic chain
halides
aryl halocarbons in which a halogen is attached to a carbon of an
halidesaryl arene ring
halides
substitutionsubs the replacement of an atom or group of atoms by another atom
titution or group of atoms
alcoholalcohol organic compounds with ah -OH group
hydroxyl the -OH group in alcohols
grouphydroxyl
group
fermentationferm the production of ethanol from sugars by the action of yeast
entation or bacteria
denatured ethanol with an added substance to make it toxic
alcoholdenatured
alcohol
addition a substance is added at the double or triple bond of an alkene
reactionaddition or alkyne
reaction
hydration the addition of water to an alkene
reactionhydratio
n reaction
hydrogenation hydrogen is added to a carbon-carbon double bond to give an
reactionhydrogen alkane
ation reaction
carbonyl carbon atom and an oxygen atom joined by a double bond
groupcarbonyl
group
aldehydesaldehyd organic compounds in which the carbonyl group is always joined
es to at lease one hydrogen: RCHO
ketonesketones organic compounds in which the carbon of the carbonyl group is
joined to two other carbons: RCOR
carboxylic compounds with a carboxyl group
actidscarboxylic
actids
carboxyl a carbonyl group attached to a hydroxyl group
groupcarboxyl
group
fatty contiuous chain carboxylic acids
acidsfatty
acids
esthersesthers compounds in which oxygen is bonded to two carbon groups:
R-O-R
dehydrogenation the loss of hydrogen
reactiondehydrog
enation
reaction
Benedict's used for aldehyde detection
testBenedict's
test &
Fehling's
testFehling's
test
estersesters derivatives of carboxylic acids in which the -OH of the
carboxyl group has been replaced by an -OR from an alcohol
polymerpolymer a large molecule formed by the covalent bonding of repeating
smaller molecules
monomersmonomers molecules tha t combine top form the repeating unit of a
polymer
carbohydratecarb monomers and polymers of aldehydes and ketones that have
ohydrate numerous hydroxy groups attached
monosaccharidesm simplest carbohydrate molecules, simple sugars
onosaccharides
disaccharidesdis sugars which are formed from two monosaccharides
accharides
polysaccharidesp the linkage of many monosaccharide monomers
olysaccharides
lipidlipid a larg class of relatively water-insoluble compound that
includes fats, oils, and waxes
waxeswaxes esters of long-chain fatty acides and long-chain alcohols
triglyceridestri triesters of long chain fatty acids and glycerol
glycerides
saponificationsa hydrolysis of oils or fats by boiling them with aqueous sodium
ponification hydroxide, making soap
amino acidamino a compound whch contains amino (-NH4) and carboxylic acid
acid (-COOS) groups in the same molecule
zwitterionszwitt internal salts of amino acids
erions
peptidepeptide any combination of amino acids in which the amino group of one
acid is united with the carboxylic acid group of another
peptide the bond between the carbonyl rgoup of one amino acid and the
bondpeptide nitrogen of the next amino acid in the peptide chain
bond
polypeptidepolyp any peptide with more than ten amino acid residues
eptide
proteinprotein a peptide with more than about 100 amino acids
nucleic acids polymers found primarily in cell nuclei
nucleotides monomers that make up DNA and RNA
Table 6: Terms
Term Definition
reaction ratereaction the number of atoms, ions or molecules that react in a
rate give time to form products
activation the minumum energy colliding particles must have in
energyactivation order to react
energy
activated the arrangement of atoms at the peak of the activation
complexactivated energy barrier
complex
transition the activated complex
statetransition state
heterogeneous reactions carred out with heterogeneous miztures of
reactionsheterogeneous reactants
reactions
inhibitorinhibitor a substance that interferes with catalysis
rate lawrate law e.g.
specific rate a proportinality constant relating the concetration of
constantspecific rate reactants to the rate of reaction
constant
first-order the reaction rate is proporional to the concentration of
reactionfirst-order only one reactant
reaction
elementary reactants are concerted to products in a single step
reactionelementary
reaction
reaction all of the elementarty reactions of a complex reaction
mechanismreaction
mechanism
intermediateintermedia a product of areaction that immediate becomes a reactant
te of another reaction
law of disorderlaw of things move spontaneously in the direction of maximum
disorder chaos or disorder
entropyentropy the measure of disorder of a system
standard of the substance at a stable state at 25 °C and 1 atm
entropystandard of
entropy
spontaneous reactions that are known to produce the written products
reactionspontaneous
reaction
non-spontaneous do not give products under the specified conditions
reactionsnon-spontaneo
us reactions
free energyfree the energy availible to do work when a reaction occurs
energy
exergonicexergonic spontaneous reactions that release free energy
endergonicendergonic nonspontaneous reactions that absorb free energy
Gibbs free energy, is the maximum amount of energy that can be coupled to
change inGibbs free another process to do useful work
energy, change in
reversible the conversion of reactants into products and the
reactionreversible conversion of products into reactants occur
reaction simultaneously
chemical when the forward and backward reactions are taking place
equilibriumchemical at the same rate
equilibrium
equilibrium the relative concentration of the reactants and products
positionequilibrium at equilibrium
position
equilibrium Keq, the ratio of product concentrations to reactant
constantequilibrium concentrations with each concentration raied to the
constant power given by the number of moles of that substance in
the balanced chemical equation
Châtelier's If a stress is applied to a system in a dynamic
principleChâtelier's equilibrium, the system changes to relive the stress
principle
Table 7: Chapter 17
The kinetic theory of reaction / matter is where the particles have to collide with enough energy against each other. Reaction rates are affected by temperature, concentration, particle size, and catalysts.
Term Definition
hydroxide ionhydroxide ion OH-
hydronium ionhydronium ion H3O+
self-ionizationself-ionizat the reaction in which two water molecules react to
ion give ions
neutral solutionneutral any aqueous solutio in which the H+ and the OH-
solution concentrations are 1.0 10-7 mol / L
ion-product constant for the product of concetrations of the hydrogen ions
waterion-product constant and hydroxide ions in water
for water
acidic solutionsacidic the H+ concentration is greater than the OH-
solutions concentration
basic solutionsbasic the H+ concentration is less than the OH-
solutions concentration
alkaline solutionsalkaline same as basic solutions
solutions
*pH the negative logarithm of the hydrogen-ion
concentration
monoprotic acid any acid that containese one ionizable hydrogen
diprotic acid any acid that contains two ionizable protons
triprotic acid any acid that containes three ionizable protons
hydrogen-ion donor the Brønstead-Lowry theory's acid
hydrogen-ion acceptor the Brønstead-Lowry theory's base
conjugate acid the particle formed when a base gains a hydrogen
ion
conjugate base the particle formed when an acid has donated a
hydrogen ion
conjugate acid-base pair two substances that are related by the loss or gain
of a single hydrogen ion
amphoteric a substance that can act as both an acid and a base
Lewis acid a substance that can accept a pair of electrons to
form a covalent bond
Lewis base a substance that can donate a pair of electrons to
form a covalent bond
weak acids acids that ionize only slightly in aqueous solution
acid dissociation constant the ratio of the concentration of the dissociated
form of an acid to the undissociated form
strong bases bases that dissociate completely into metal ions
and hydroxide ions in aqueous solution
strong acids acids that completely ionize in aqueous solution
weak bases bases that do not dissociate completely in aqueous
solution
base dissociation constant the ratio of the concentration of the dissociated
form of a base to the undissociated form
Table 8: Chapter 18
Terms Definition
neutralization reactions bin which an acid and a base react in an aqueous
reaction solution to produce a slat and water
standard solution the solution of known concentration
end point the point at which neutralization is acheived
titration the addition of a known amount of solutoin to determine
the volume or concentration of another solution
equivalentequivalent the amount of an acid or base that will give one mole of
hydrogen or hydroxide ions
gram equivalentgram the mass of one equivalent of a substance
equivalent
normalitynormality the concentration expressed as the number of equivalents
of solute in 1 L of solution
equivalence the point of neutralization
pointequivalence
point
salt hydrolysissalt the cation or anions of the dissociated salt accept
hydrolysis hydrogen ions from water or donate hydrogen ions to water
buffersbuffers solutions in which the pH remains relatively constant when
small amounts of acid or base are added
buffer the amount of acid or base that may be added to a buffer
capacitybuffer solution before a significant change in pH occurs
capacity
solutbility product the product of the concentration terms each raised to the
constantsolutbility power of the coefficient of the substance in the
product constant dissociation equation
common ioncommon an ion that is common to both salts
ion
common ion the lowering of the solubility of a substance by the
effectcommon ion addition of a common ion
effect
Table 9: Chapter 19
Term Definition
oxidation--reduction the chemical changes that occur when electrons are
reactionsoxidation--reducti transferred between reactants
on reactions
redox reactionsredox oxidation--reduction reactions
reactions
oxidationoxidation -the combination of an element with oxygen
-loss of electrons
reductionreduction -the loss of oxygen from a compound
-gain of electrons
reducing agentreducing the substance in a redox reaction that donates
agent electrons
oxidizing agentoxidizing the substance in a redox reaction that accepts
agent electrons
oxidation numberoxidation a positive or negative number assiggned to an atom
number according to a set of arbitrary rules
oxidation number change a redox equation is balanced by comparing the
methodoxidation number increases and decreases in oxidation number
change method
half-reaction the method used to balance redox equations by
methodhalf-reaction method balancing oxidation and reduction half-reactions
half-reactionhalf-reaction an equation showing either the reduction or the
oxidation of a species in an oxidation-reduction
reaction
Table 10: Chapter 20
Terms Definition
radioactivityradioac the process by which uranium gives off rays
tivity
radiationradiation the penetrating rays emmited by a radioactive substance
radioisotopesradiois certain isotopes that have unstable nuclei
otopes
radioactive the process by which an unstable nucleus loses energy by
decayradioactive emitting radiation
decay
alpha helium nuclei
radiationalpha
radiation
alpha two protons and two neutraons which have a double postive
particlesalpha charge.
particles
beta raditationbeta fast moving electrons
raditation
gamma electromagnetic radiation
radiationgamma
radiation
band of neutron v proton plot
stablityband of
stablity
positronpositron a particle with the mass of an electron but a postive
charge
half-lifehalf-life the time required for one-half of the atoms of a
radioisotope to emit radition and decay to products
transmutationtransmu the conversion of an atom of one element to an atom of
tation another element
transuranium the elements in the periodic table with atomic numbers
elementstransuranium above 92
elements
fissionfission the splitting of a nucleus into smaller fragments
neutron a method to slow down neutrons so that they can be
moderationneutron captured by the reactor fuel to continue the chain reactio
moderation
neutron decreases the number of slow neutrons
absorbtionneutron
absorbtion
fusionfusion two nuclei combining to produce a nucleus of heavier mass
ionizing radiation that knocks electrons off some atoms of the
radiationionizing bombarded substance to produce ions
radiation
geiger a gas-filled metal tube to detect radiation
countergeiger
counter
scintillation a phosphor used to detect radiation
counterscintillation
counter
film badgefilm several layers of photo graphic film covered with black
badge lighproof paper encased in a plastic or metal holder
Table 11:
acidic solutions, 10
activated complex, 9
activation energy, 9
addition reaction, 7
alcohol, 7
aldehydes, 8
aliphatic compounds, 7
alkaline solutions, 10
alkanes, 6
alkenes, 6
alkyl group, 6
alkyl halides, 7
alkynes, 6
alpha particles, 12
alpha radiation, 12
amino acid, 8
anion, 1
antibonding orbital, 3
aqueous solutions, 4
arenes, 7
aromatic compound, 7
aryl halides, 7
asymmetric carbon, 7
band of stablity, 12
basic solutions, 10
Benedict's test, 8
bent triatomic, 4
beta raditation, 12
boiling point elevation, 5
bond
coordinate covalent, 2
covalent, 3
dissociation energy, 3
double covalent, 2
hydrogen, 3
ionic, 1, 2
metallic, 1, 2
nonpolar covalent, 3
pi, 3
polar, 3
polar covalent, 3
sigma, 3
single covalent, 2
triple covalent, 2
bonding orbital, 2
branced chain alkane, 6
Brownian motion, 5
buffer capacity, 11
buffers, 11
carbohydrate, 8
carbonyl group, 7
carboxyl group, 8
carboxylic actids, 8
cation, 1
Châtelier's principle, 9
chemical equilibrium, 9
cis configuration, 6
colligative properties, 5
colloids, 5
common ion, 11
common ion effect, 11
concentrated solution, 5
concentration, 5
condensed structural formula, 6
continuous chain alkanes, 6
coordination number, 1
cracking, 7
cyclic hydrocarbons, 7
dehydrogenation reaction, 8
deliquescent, 4
denatured alcohol, 7
desiccants, 4
Diamagnetic, 4
dilute solution, 5
dipole, 3
dipole interactions, 3
disaccharides, 8
dispersion forces, 3
ductile, 2
effloresce, 4
electrolyte
strong, 5
weak, 5
electrolytes, 4
Electron dot structures, 1
elementary reaction, 9
emulsions, 5
endergonic, 9
entropy, 9
equilibrium constant, 9
equilibrium position, 9
equivalence point, 11
equivalent, 11
esters, 8
esthers, 8
exergonic, 9
fatty acids, 8
Fehling's test, 8
fermentation, 7
film badge, 13
first-order reaction, 9
fission, 12
free energy, 9
freezing point depression, 5
functional group, 7
fusion, 13
gamma radiation, 12
geiger counter, 13
geometric isomers, 7
Gibbs free energy, change in, 9
gram equivalent, 11
half-life, 12
half-reaction, 12
half-reaction method, 12
halied ions, 1
halocarbons, 7
Henry's Law, 5
heterogeneous reactions, 9
homologous series, 6
Hybrid States, 4
hybridization, 3
hybridized electron state, 3
hydration reaction, 7
hydrocarbons, 6
hydrogenation reaction, 7
hydronium ion, 10
hydroxide ion, 10
hydroxyl group, 7
hygroscopic, 4
immiscible, 5
inhibitor, 9
intermediate, 9
ionizing radiation, 13
ion-product constant for water, 10
isoelectronic, 1, 2
IUPAC System, 6
ketones, 8
kinetic theory, 10
law of disorder, 9
linear triatomic, 4
lipid, 8
malleable, 2
miscible, 5
molal boiling point elevation constant, 6
molal freezing point depression constant, 6
molality, 6
molarity, 5
mole fraction, 6
molecular orbital, 2
monomers, 8
monosaccharides, 8
network solids, 3
neutral solution, 10
neutron absorbtion, 12
neutron moderation, 12
nonelectrolytes, 5
non-spontaneous reactions, 9
normality, 11
octet rule, 1
oxidation, 12
oxidation number, 12
oxidation number change method, 12
oxidation--reduction reactions, 11
oxidizing agent, 12
paramagnetic, 2, 4
peptide, 8
peptide bond, 8
polar molecule, 3
polymer, 8
polypeptide, 8
polysaccharides, 8
positron, 12
protein, 8
radiation, 12
radioactive decay, 12
radioactivity, 12
radioisotopes, 12
rate law, 9
reaction mechanism, 9
reaction rate, 9
redox reactions, 12
reducing agent, 12
reduction, 12
resonance, 2
reversible reaction, 9
salt hydrolysis, 11
saponification, 8
saturated solution, 5
scintillation counter, 13
self-ionization, 10
solubility, 5
solutbility product constant, 11
solute, 4
solvation, 4
Rate of, 6
solvent, 4
specific rate constant, 9
spontaneous reaction, 9
standard of entropy, 9
stereoisomers, 7
structural isomers, 6
structure formula, 2
substituent, 6
substitution, 7
supersaturated solution, 5
surface tension, 4
surfactants, 4
suspensions, 5
tetrahedral, 4
tetrahedral angle, 3
trans configuration, 6
transition state, 9
transmutation, 12
transuranium elements, 12
Triagonal bipyramidal, 4
triglycerides, 8
trigonal planar, 4
Tyndall effect, 5
unsaturated, 5
unsaturated compounds, 6
unshared pairs, 2
Valence Electrons, 1
van der Waals forces, 3
VSEPR theory, 3
water of hydration, 4
waxes, 8
zwitterions, 8