Chemistry Flashcards
1
Q
anything that has mass and occupies space
A
matter
2
Q
amount of matter contained in an object
A
mass
3
Q
amount of space occupied by matter
A
volume
4
Q
4th state of matter, also called liquid crystal, mesophase, supercritical fluid
A
plasma
5
Q
this is strongly influenced by electric and magnetic fields with a hot ionized gas consisting of approximately equal numbers of positively charged ions and negatively charged electrons
A
plasma
6
Q
5th state of matter, also called a super atom, and has many properties of a super fluid
A
bose-einstein condensate
7
Q
m/v
A
density
8
Q
density of water
A
1 g/ml=1 g/cm³=1000 kg/m³
9
Q
ratio of the density of a sample and the density of a reference substance
A
specific gravity (unitless quantity)
10
Q
specific gravity formula
A
SG=tsample/treference
11
Q
ratio between the weights of equal volumes of a sample and water
A
apparent specific gravity
12
Q
formula for apparent specific gravity
A
SGapparent=Wsample/Wwater
13
Q
ratio between the weights in a vacuum of equal volumes of a sample and water
A
true specific gravity
14
Q
formula for true specific gravity
A
SGtrue=Wvsample/Wvwater
15
Q
Specific Volume
A
SV=1/SG
16
Q
when H2O freezes the volume that the same mass of H2O occupies increases because
A
the molecules become more highly organized
17
Q
highly organized molecules mean
A
increase in volume, decrease in density
18
Q
ability to float
A
buoyancy
19
Q
ability to be drawn out into wires
A
ductility
20
Q
ability to be hammered into sheets
A
malleability
21
Q
ability to return to its original shape after being deformed
A
elasticity
22
Q
ability to resist flow
A
viscosity
23
Q
measure of disorder of a thermodyamic system
A
entropy
24
Q
amount of energy stored in an object
A
energy
25
the number of valence electrons is close to completing the octet rule, accepts electrons during ionic bonding, forms anions when ionized
non-metals
26
the number of valence electrons is small, donates electrons during ionic bonding, forms cations when ionized
metals
27
can act as a metal or non-metal depending on the conditions
metalloids
28
components are a pair of anion group and a cation group, electrons are transferred from the cation to the anion
ionic
29
components are both anion groups, electrons are shared within the bond
covalent
30
components are both metals, components are stored in a sea of electrons
metallic
31
commonly called solutions, where only 1 phase is discernable
homogenous
32
measure of the relative amounts of the components of a solution
concentration
33
the component that dissolves in the solution
solute
34
the component that dissolves other components of the solution
solvent
35
the maximum amount of solute that can be dissolved in a particular solvent under specific conditions, often expressed as a ratio or other measures of concentration
solubility [g of solute/100 g of solvent]
36
contains less solute than the maximum quantity of solute that is normally possible at a given temperature [haven't reached the solubility of your solute]
unsaturated, no crystal formation
37
contains the max amount of solute that is normally possible at a given temperature
saturated, crystal formation
38
contains more solute than normally expected for a saturated solution (unusual amount at a specified temperature]
supersaturated, unstable, triggers fast crystal formation
39
molarity formula
M=moles of solute/liters of solution
40
molality formula
m=moles of solute/kg of solvent
41
mass percent
[mass of solute/mass of solution] x 100
42
volume percent
[volume of solute/volume of solvent] x 100
43
relative amount of solute in a sol'n
saturation
44
IMF charges occur, these IMFs can decrease volume of liquid because of strong interactions that occur in your liquids, this also accounts for changes
on the usage of molality
45
used to describe a certain amount of molecules
moles
46
1 mole = avogadro's number
6.02 x10²³
47
number of equivalent weights of a solute per liter of the solution
normality
48
normality formula
N=number of equivalent weights/L of solution
49
grams of solute/gram equivalent weight of solute
number of equivalent weight
50
Molarity x factor
Normality
51
refers to the acidic hydrogen [hydronium]
acid factor
52
refers to the number of hydroxide
base factor
53
used to convert mass of substance to moles of substance
molecular weight
54
all alkali metals (group 1a) are
soluble
55
all those with ammonium ion [NH₄⁺] are
soluble
56
all nitrates [NO₃⁻] are
soluble
57
all acetates [C₂H₃O₂⁻] are
soluble
58
all chlorides [Cl⁻] bromides [Br⁻] iodides [I⁻] are soluble except
Ag⁺, Hg₂²⁺, Pb²⁺
59
most sulfates [SO₄²⁻] are soluble except
BaSO₄, PbSO₄, SrSO₄, Hg₂SO₄
60
all hydroxides [OH⁻] are insoluble except those of
Group 1A, Ba(OH)₂, Sr(OH)₂, Ca(OH)₂
61
all sulfides are insoluble except those of
group 1A, group 2A, NH₄⁺
62
all carbonates [CO₃²⁻] are insoluble except those of NH₄⁺ and those of
NH₄⁺ and those of group 1A
63
all phosphates [PO₄³⁻] are insoluble except
NH₄⁺ and those Group1A
64
pressure needed to prevent osmosis which is the spontaneous net movement of solvent molecules through a semi-permeable membrane into a region of higher solute concentration
osmotic pressure
65
osmotic pressure formula
πV=nRT
66
the addition of nonvolatile solute to a volatile solvent will diminish the escaping tendency of the solvent thereby lowering the vapor pressure of the solution
vapor pressure lowering
67
raoult's law
ΔP=P°Xₛₒₗᵤₜₑ
68
is the temperature at which the vapor pressure of the liquid becomes equal to the external atmospheric pressure [1 atm=760 mmHg]
boiling point
69
the boiling point of a pure solvent is increased by the addition of a non-volatile solute, and the elevation can be measure by
ebullioscopy
70
ebullioscopy
ΔTբ=iKbm
71
is the temperature at which the solid and liquid phases are in equilibrium under an external pressure of 1 atm
freezing point
72
the freezing point of a pure solvent is lowered by the addition of a solute which is insoluble in the solid solvent, and the measurement of this difference is called cryoscopy
freezing point depression
73
freezing point depression formula
ΔTբ=iKբm
74
mixtures wherein 2 or more distinct phases are discernable
heterogenous
75
suspended particles are too large and too heavy to be carried by the motion of the particles in which they are suspended in causing them to settle after sometime
suspensions
76
suspended particles are small and light enough to be carried by the movement of the particles in which they are suspended in
colloids
77
solid in solid colloid
solid sol
78
solid in liquid colloid
sol
79
solid in gas colloid
solid aerosol
80
liquid in solid colloid
gel
81
liquid in liquid colloid
emulsion
82
liquid in gas colloid
aerosol
83
gas in solid colloid
solid foam
84
gas in liquid colloid
foam
85
mass of proton
1.67 x 10⁻²⁷ or 1 amu
86
mass of neutrons
1.67 x 10⁻²⁷ or 1 amu
87
mass of electrons
9.11 x 10⁻³¹
88
mass of the atom is concentrated on the
nucleus
89
atomic number [Z]
number of protons
90
mass number [A]
sum of protons and neutrons
91
charge [q]
difference of the protons and electrons
92
relative abundance of a certain isotope compared to all the isotopes of the same element
percent natural balance
93
weighted average of the mass numbers of the isotopes of that particular element
atomic weight
94
ISOTOPES: atoms of the same element that have the same number of protons but different number of neutrons, thus their mass numbers are
different
95
elements having the same number of neutrons
isotones
96
atomic species having the same mass number but different atomic numbers
isobars
97
elements having the same number of electrons
isoelectronic
98
who discovered atoms as the basic unit of matter
democritus
99
who discovered the billiard ball model
john dalton
100
who discovered the plum pudding model and the electron
j.j. thomson
101
who discovered the gold foil experiment and the proton?
ernest rutherford
102
who discovered the neutron
james chadwick
103
who discovered the planetary model
niels bohr
104
who discovered the quantum theory
erwin schrodinger
105
usually malleable and ductile, highly conductive for heat and electricity, low electronegativities and ionization energies, high melting points and densities
metals
106
brittle solids, poor conductors of heat and electricity, high electronegativities and ionization energies
non-metals
107
properties are in between metals and non-metals, reactivity depends on the elements to be reacted with
metalloids
108
soft metallic solids, shiny and lustrous; reacts vigorously with water to produce hydroxides
alkali metals [group 1A]
109
harder than 1A metals; shiny, lustrous, and oxidizes easily
alkaline earth metals [group 2A]
110
boron group or earth metals
group 3A
111
carbon group or tetrels
group 4A
112
nitrogen group or pnictogens
group 5A
113
oxygen group or chalcogens
group 6A
114
halogens, reactive non-metals
group 7A
115
unreactive under ordinary circumstances; usually found as monoatomic gases
group 8A [noble gases]
116
hard metallic; shiny and lustrous; dense and have high melting points, usually have high oxidation states
transition metals
117
Group B inclusions
transition metals, lanthanides, actinides
118
lightest element
hydrogen
119
densest element
osmium
120
only metal liquid at room temperture
mercury
121
only non metal liquid at room temperature
bromine
122
most abundant intracellular cation
potassium
123
most abundant extracellular cation
sodium
124
most abundant gas in the air
nitrogen
125
most abundant element on earth
oxygen
126
most abundant metal on earth
aluminum
127
most abundant noble gas
argon
128
desire for an electron, desire for negativity, near octet
electronegativity
129
most electronegative
flourine
130
tendency of an electron to bond, increases from left to right along a period, decreases from top to bottom along a column/group
electronegativity
131
energy needed to remove an electron form an atom, increases from left to right along a period, decreases from top to bottom along a column/group
ionization energy
132
energy released when an electron is added to an atom, positive when energy is released and negative when absorbed, increases from left to right along a period, decreases from top to bottom along a column/group
electron affinity
133
farthest extent of the presence of electron decrease from left to right a period, increases from top to bottom along a column/group
atomic size/radius
134
bond between a metal and non-metal [cation and anion], form crystals, high melting and boiling points, hard and brittle, poor conductors when solid, good conductors when dissolved in water
ionic bond
135
bond between non-metals [anions], most have relatively low melting and boiling points, soft and relatively flexible, more flammable, many are insoluble in water and those that do dissolve do not conduct electricity
covalent/molecular bond
136
with unequal sharing
polar bond
137
with equal sharing
nonpolar bond
138
electronegativity difference greater than 0.4 but less than 1.7
polar compound
139
electronegativity difference less than 0.4
nonpolar compound
140
electronegativity difference greater than 1.7
ionic compound
141
types of covalent bonds
pi bond and sigma bond
142
end to end overlap of orbitals; stronger type of bond
sigma bond
143
lateral or sideways overlap of orbitals
pi bond
144
bond between metals [cations] have moderately high melting points, malleable and ductile, good conductors of heat and electricity
metallic bond
145
occurs when orbitals combine to form a hybrid orbital during bond formation
hybrid orbital
146
s orbital combines with 3 p orbitals to form 4 hybridized orbitals
sp³
147
s orbital combines with 2 p orbitals to form 3 hybridized orbitals and 1 normal orbital
sp²
148
s orbital combines with 1 p orbital to form 2 hybridized orbitals and 2 normal orbitals
sp¹
149
[carbon chemical bonds] sp³ hybrid orbitals form sigma bonds with orbitals of other atoms
single bonds
150
[carbon chemical bonds] 1 sp² hybrid from each atom form a sigma bond and 1 p orbital from each atom form a pi bond
double bonds
151
[carbon chemical bonds] 1 sp¹ hybrid from each atom form a sigma bond and 2 p orbitals from each atom form 2 pi bonds
triple bonds
151
presence of double or triple bonds increases
reactivity
152
saturated hydrocarbons do not have
triple or double bonds
153
shows the simplest ratio of the amounts of atoms of each component elements
empirical formula
154
shows the actual amounts of each of the atoms of the component elements
molecular formula
155
shows the approximate arrangement of the atoms within the molecule
structural formula
156
[molecular geometry] steric number 2, no lone pairs
linear
157
[molecular geometry] steric number 3, no lone pairs
trigonal planar
158
[molecular geometry] steric number 3, 1 lone pair
bent or angular
159
[molecular geometry] steric number 4, no lone pairs
tetrahedral
160
[molecular geometry] steric number 4, 1 lone pair
trigonal pyramidal
161
[molecular geometry] steric number 4, 2 lone pairs
bent or angular <<109 degrees
162
[molecular geometry] steric number 5, no lone pairs
trigonal bypiramidal
163
[molecular geometry] steric number 5, 1 lone pair
sawhorse or seesaw
164
[molecular geometry] steric number 5, 2 lone pairs
t-shape
165
[molecular geometry] steric number 6, no lone pairs
octahedral
166
[molecular geometry] steric number 6, 1 lone pair
square pyramid
167
[molecular geometry] steric number 6, 2 lone pairs
square planar
168
[molecular geometry] steric number 6, 3 lone pairs
t shape <90 degrees
169
[molecular geometry] steric number 6, 4 lone pairs
linear, vertical 180 degrees
170
influences the final structure of the molecule, boiling and freezing points, heat capacity, solubility
intermolecular forces of attraction
171
attraction between the opposing poles of dipole molecules
electrostatic interactions
172
types of electrostatic interactions
dipole-dipole, ion-dipole, ion-induced dipole, hydrogen bonding
173
weakest electrostatic interaction, sum of all the attractive ad repulsive forces between and within the molecules
van der waals
174
relative amount of particles present in a sample, avogadro's sample
6.022 x 10²³
175
[gases] an ideal gas is where all interactions between the molecules are only through collisions that are assumed to be completely elastic, gases have no volume, exists in STP of 0 degrees C and 1atm
ideal gas concept
176
[gases] at stp, 1 mole of a gas is occupies 22.4 L
22.4 L
177
[gases] ideal gas equation
PV=nRT
178
in PV=nRT, n is for
the number of moles
179
in PV=nRT, r is equal to
0.0821 [(L*atm)/mol*K]
180
in using gas laws the unit of temperature must be in
kelvin
181
a particular amount of gas at constant temperature increase in volume when the pressure is decreased
boyle's law
182
boyle's law equation
P₁V₁=P₂V₂
183
a particular amount of gas in a constant pressure increases in volume when the temperature is increased
charles law
184
charles law equation
V₁/T₁=V₂/T₂
185
a particular amount of gas in a constant volume increase in temperature when the pressure is increased
gay-lussac's law
186
gay-lussac's law equation
P₁/T₁=P₂/T₂
187
a gas in a constant pressure and temperature increases in volume when the amount of particles is increased
avogadro's law
188
combined gas law equation
P₁V₁/V₁n₁=P₂V₂/V₂n₂
189
avogadro's law equation
V₁/n₁=V₂/n₂
190
dalton's law is also called
law of partial pressures
191
the pressure of a mixture of gases is the sum of the pressures of the individual components
Ptotal = P₁ + P₂ +...
192
the rate at which a gas diffuses is inversely proportional to the root of its density or mass
law of effusion
193
law of effusion formula
R₁/R₂ = √t₁/t₂
194
all chemical reactions follow the law of
conservation of mass
195
[type of rxn] 2 or more elements or compounds combine to make a more complex substance
synthesis
196
[type of rxn] compounds break down into simpler substances
decomposition/analysis
197
[type of rxn] occurs when 1 element replaces another one in a compound
single replacement
198
[type of rxn] occurs when different atoms in 2 different compounds trade places
double replacement
199
fuel + O₂ -> CO₂ +H₂O
complete combustion
200
fuel + O₂ -> CO₂ + H₂O + residues
incomplete combustion
201
electron transfer from 1 atom to another
redox reaction
202
[type of redox reaction] loss of electrons
oxidation
203
[type of redox reaction] gain of electrons
reduction
204
GEROA
gain of electrons is reduction among oxidizing agents
205
LEORA
loss of electrons is reduction among reducing agents
206
acid + base -> salt + H₂O
neutralization reaction
207
[stoichiometry] reactant that is first to be totally consumed halting further reactions
limiting reagent
208
[stoichiometry] reactant that is left when the limiting reagent is consumed
excess reagent
209
[energy] the total energy of an object or system
enthalpy
210
[energy] reactions that require addition of energy. this means that the product has higher enthalpy than the reactants
endothermic
211
[energy] reactions that require removal of energy. this means that the product has lower enthalpy than the reactants
exothermic
212
[energy] energy required to start a reaction
activation energy
213
[energy] reactions that require a very small activation energy and can start without external interference
spontaneous reactions
214
[energy] any substance that increases the rate of the reaction without being consumed
catalyst
215
[equilibrium] reactions whose products can spontaneously react to form the original reactants thereby reversing the reaction
reversible reactions
216
[equilibrium] state of reaction at which the rate of the forward and reverse reactions are the same producing a condition where the concentrations of the reactant and the products remain relatively constant
equilibrium
216
equilibrium constant K can be derived as
kₑq = [C]ˡ[D]ᵐ/[A]ʲ[B]ᴰ
217
when an equilibrium system is subjected to a change in temp., pressure, or concentration of a reacting species, the system responds by attaining a new equilibrium that partially offsets the impact of the change
le chatelier's principle
218
[le chatelier's] effects of changing the amount of reacting species
if the concentration of 1 of the reacting species is increased, it will favor the reaction in which the species is consumed
219
[le chatelier's] effects of changing in pressure or volume of equilibrium
if the pressure of an equilibrium mixture of gases is increased, the volume is reduced, a net reaction occurs in the direction producing fewer moles of gases
220
[le chatelier's] effects of temperature on equilibrium
raising the temp. of an equilibrium mixture shifts the equilibrium condition in the direction of endothermic reaction
221
[le chatelier's] effects of catalysts on equilibrium
a catalyst has no effect on the condition of equilibrium in a reversible reaction
222
[dissociation] ____ occurs when a compound separates into its component molecules
dissociation
223
[acid-base def.] arrhenius acid
H⁺ producer
224
[acid-base def.] arrhenius base
OH⁻ producer
225
[acid-base def.] bronsted-lowry acid
H⁺ donor
226
[acid-base def.] bronsted-lowry base
H⁺ acceptor
227
[acid-base def.] lewis acid
electron pair acceptor
228
[acid-base def.] lewis base
electron pair donor
229
[acid-base] typically sour in taste and are corrosive to most metals
acids
230
[acid-base] typically bitter in taste, and are slippery to touch
bases
231
[conjugate acids and bases] bronsted-lowrey acid
protonated bronsted base
232
[conjugate acids and bases] bronsted-lowrey base
deprotonate bronsted acid
233
acids dissociate to produce
H+ ions and anions
234
bases dissociate to form
OH- ions and cations
235
acids/bases that have dissociation constants close to 1
strong acids/bases
236
acids/bases that have dissociation constants far from 1
weak acids/bases
237
[strong/weak acid] HCl
strong acid
238
[strong/weak acid] H2SO4
strong acid
239
[strong/weak acid] Nitric Acid (HNO3)
strong acid
240
[strong/weak acid] Perchloric Acid (HClO4)
strong acid
241
when acids and bases are in aqueous state, they _____ into their respective ions
dissociate
242
acidity of a substance depend on the concentrations of its
dissociated ions
243
process of determining the concentration of a substance by slowly adding another substance with a known concentration
titration
244
[titration] substance with known concentration to be added
titrant
245
[titration] substance whose unknown concentration is to be determined
analyte
246
[titration] substances that changes property under certain conditions to signal when to stop adding the titrant
indicator
247
[acid-base titration] added titrants neutralizes the analyte
equivalence point
248
[acid-base titration] point when the pH changes the color of the indicator
end point
249
pH = 7
strong acid-strong base
250
pH < 7
strong acid-weak base
251
pH > 7
weak acid-strong base
252
acid + base -> salt + H2O
neutralization reaction
253
[acid-base rxn] resist drastic change in pH contain weak acid and base pairs
buffers
254
[thermochem] amount of heat needed to changethe temp. of 1 g of a substance by 1 degree celsius
C [specific heat capacity]
255
amount of heat required to transform 1 g of substance from liquid to gas or gas to liquid
heat of vaporization [ΔHᵥ]
256
amount of heat required to transform 1 g of a substance from solid to liquid or liquid to solid
heat of fusion [ΔHբ]
257
change in temperature formula
Q = mCqΔT
258
change in phase formula
Q = mΔH
259
common properties of organic compounds
usually combustible, generally have low melting and boiling pts, usually less soluble in water, usually slow to react because they are usually covalent molecules, most have high molecular weights
260
sources of organic compounds
nature, synthesis, fermentation
261
valence electrons of carbon
4
262
what group is carbon in in the periodic table?
group 4A
263
carbon is capable of catenation and _____
hybridization
264
is the ability of carbon to bond with itself and form long chains of organic compounds
catenation
265
concept of mixing non-equivalent atomic orbitals to form equivalent or degenerate hybrid orbitals to form single, double, and triple bonds
hybridization
266
what is the shape, bond angle, and bond type of sp3 orbital?
tetrahedral, 109.5, single
267
what is the shape, bond angle, and bond type of sp2 orbital?
trigonal planar, 120, double
268
what is the shape, bond angle, and bond type of sp orbital?
linear, 180, triple
269
[org chem] different compounds that have the same molecular formula
isomers
270
[forms of isomerism] form if isomerism in which molecules with the same molecular formula have different bonding patterns and atomic organization
structural isomerism
271
[type of structural isomerism] differ in the arrangement of C atoms usually due to the presence of branching
chain isomerism
272
examples of chain isomerism
n-butane, isobutane
273
[type of structural isomerism] the isomers have the same molecular formula but differs mainly in the attached functional groups
functional isomerism
274
examples of functional isomerism
ether and alcohol, aldehyde and ketone
275
[type of structural isomerism] differs in the position of unsaturated bonds (double and triple bonds) or functional groups
positional isomerism
276
examples of positional isomerism
meta isomer, ortho isomer, para isomer
277
[forms of isomerism] isomers that have the same molecular formula and sequence of bonded atoms (constitution), but differ in the 3-dimensional orientations of their atom space
stereoisomerism
278
[types of stereoisomerism] occurs among double bonds
geometric/configurational isomerism
279
[type of geometric isomerism] cis-trans isomerism: the molecule in which the 2 of the same atoms are on the same side of the double bond is known as
cis isomer
280
[type of geometric isomerism] cis-trans isomerism: molecule with the 2 of the same atoms in the opposite side of the double bond is called
trans isomer
281
[type of geometric isomerism] E-Z isomerism: the higher priority groups are on opposite sides of the double bond
E isomer
282
[type of geometric isomerism] E-Z isomerism: the higher priority groups are on the same sides of the double bond
Z isomer
283
[types of stereoisomerism] results from the different ways an atom flexes and bends due to rotation along a single bond or ring flipping among cyclic structures
conformational isomers
284
[types of stereoisomerism] isomers which differ in their ability to rotate plane polarized light
optical isomers
285
[optical isomers] structural requirement for optical activity, carbon with 4 different functional groups or substituents
chiral center
286
types of optical isomers
enantiomers, diastereomers, meso compounds
287
chain or branched chain of organic compounds whose longest chain is made of carbon atoms only
aliphatic compounds
288
aliphatic compounds made up of only hydrogen and carbon
hydrocarbons
289
[type of hydrocarbon] hydrocarbons wherein all carbons are attached together only with single bonds
saturated hydrocarbons
290
properties of saturated hydrocarbons
colorless, tasteless, odorless; boiling and melting pts increases as molecular weight increases while London Dispersion Forces increases, non-polar practically insoluble in water but soluble in organic solvents, stable due to strong c-c and c-h bonds, sigma bonded, tetrahedral
291
CH4
methane
292
C2H6
ethane
293
C3H8
propane
294
C4H10
n-butane
295
(CH3)3CH
isobutane
296
C5H12
n-pentane
297
(CH3)CHCH2
isopentane
298
(CH3)4C
neopentane
299
[common rxns] CH4 + 202 -> CO2 +H2O
oxidation with oxygen in air
300
[common rxns] CH4 +CL2 -> HCl + CH3Cl
halogen substitution
301
[common rxns] occurs when bacteria oxidizes a hydrocarbon underaerobic conditions
biological oxidation
302
[type of hydrocarbon] hydrocarbons containing double or triple bonds
unsaturated hydrocarbons
303
[types & nomenclatures of unsaturated hydrocarbons] properties: non polar, stable due to strong c-c, c-h bonds, sigma and pi bonds, double bond, trigonal planar
alkenes
304
[types & nomenclatures of unsaturated hydrocarbons] properties: triple bond, have 2 pi bonds, very reactive
alkyne
305
[common reactions for alkenes and alkynes] produces glycol
oxidation
306
[common reactions for alkenes and alkynes] hydrogen is bonded to replace double or triple bonds making the compound more saturated
reduction
307
[common reactions for alkenes and alkynes] acids bond across double or triple bonds
addition
308
[common reactions for alkenes and alkynes] unsaturated molecules combine with each other to form polymers with higher molecular weight
polymerization
309
[types & nomenclatures of unsaturated hydrocarbons] hydrocarbons that contain the hydroxyl group OH, product of primary oxidation
alcohols
310
classifications of alcohols
primary, secondary, tertiary
311
properties of alcohols
soluble in water but solubility decreases as molecular weight increases, low boiling and melting points but increases with molecular weight
312
alcohols with 2 or more OH groups
glycols
313
[common reactions in alcohols] reaction with acids to form esters
glycols
314
[common reactions in alcohols] primary alcohols oxidize into aldehydes, secondary alcohols oxidize into ketones
oxidation
315
most common aldehydes
carbohydrates
316
[types & nomenclatures of unsaturated hydrocarbons] contains a carbonyl group at the end of the chain
aldehydes
317
properties of aldehydes
carbonyl group is attached to the end of the alkyl chain, and is a serious air pollutant
318
example of aldehyde that is very toxic to microorganisms and is used as an embalming fluid
formalin
319
example of aldehyde that is a common industrial manufacturing chemical
acetyldehyde
320
[types & nomenclatures of unsaturated hydrocarbons] carbonyl group in the middle of alkyl chain, commonly used as solvents and for industrial manufacturing
ketones
321
[type of ketone] simplest ketone produced from the oxidation of isopropyl alcohol
acetone [dimethyl ketone]
322
[type of ketone] produced from the oxidation of 2-butanol
methyl ethyl ketone
323
properties of ketone
can be oxidized to form its corresponding acid
324
[types & nomenclatures of unsaturated hydrocarbons] highest oxidation state or organic compounds, contains 1 or more carboxyl group
carboxylic acids
325
most common carboxylic acid
free-fatty acids
326
actual source of bod energy are
fats
327
[types of c. acids] contain 1 carboxylic group, commonly known as fatty acids
saturated monocarboxylic
328
[types of c. acids] form metallic acids, can be reduced into saturated acids, used as food by microorganisms
unsaturated monocarboxylic
329
principal acids of unsaturated monocarboxylic
acrylic, oleic, linoleic
330
[types of c. acids] the most important species are the ones that have 2 carboxylic groups one on each end
polycarboxyllic
331
[types of c. acids] contains OH other than c. acid, some species are optically active
hydroxy
332
[types & nomenclatures of unsaturated hydrocarbons] formed by the reaction between acids and alcohols, commonly used in chemical manufacturing, solvents, flavoring extracts and perfumes
esters
333
most common ester
triglycerides
334
alcohol groups and fatty acids are
esterified
335
[types & nomenclatures of unsaturated hydrocarbons] formed by treating alcohols with strong dehydrating agents, has an oxygen sandwiched between 2 organic groups, widely used as a solvent, highly flammable
ethers
336
ethers are susceptible to forming peroxides that are highly explosive when exposed to
air
337
ethers are resistant to
biological oxidation
338
[types & nomenclatures of unsaturated hydrocarbons] organic compounds that contain halogens
alkyl halides and halogenated aliphatic compounds
339
[types & nomenclatures of unsaturated hydrocarbons] nitrogen containing aliphatic compounds
amines, amides, nitriles
340
common example of amines
amino acids
341
[types & nomenclatures of unsaturated hydrocarbons] derived from the reaction between organic acids and ammonia
amides
342
[type of nitrogen containing a. compounds] called naphthenes, have 2 H atoms connected to each C atom
cyclic aliphatic compounds
343
[type of nitrogen containing a. compounds] contains sulfur
mercaptans and thioalcohols
344
cyclic organic compounds with alternating single and double bonds
aromatic compounds
345
parent compound of aromatic compounds
benzene
346
[aromatic hydrocarbons] benzene examples
toluene, ethylbenzete
347
[aromatic hydrocarbons] polyring hydrocarbon example
naphthalene
348
types of aromatic copounds
aromatic hydrocarbons and phenols
349
types of aromatic hydrocarbons
benzenes and polyring hydrocarbons
350
[type of aromatic compound] contains OH
phenols
351
types of phenols
monohydroxy phenols, polyhydroxy phenols
352
[type of monohydroxy phenols] contains alkyl groups
cresols and other alkylphenols
353
[type of monohydroxy phenols] contains chlorine
chlorinated phenols
354
cyclic organic compounds with double bonds or with other elements in the ring
heterocyclic compounds
355
[common food and related compounds] types of carbohydrates
monosaccharides, disaccharides, polysaccharides
356
types of monosaccharides
glucose, fructose, galactose, mannose
357
sweet monosaccharide
fructose
358
types of disaccharides
sucrose [table sugar], maltose
359
fructose is also a
ketohexose
360
glucose is also a
aldohexose
361
[fats, oils, waxes] fatty acid glycerides that are solid at room temp.
fats
362
[fats, oils, waxes] fatty acid glycerides that are liquid at room temp.
oil
363
[fats, oils, waxes] esters of long-chain acids and alcohols
waxes
364
building blocks of protein
amino acids
365
[other organic compounds] contains surfactants that consists of il soluble parts and water soluble parts
detergents
366
[other organic compounds] derived from saponification of fats and oils
soaps
367
[additional] indicator: benedicts solution
simple carbohydrates turns brick red for positive
368
[additional] indicator: iodine solution
complex carbohydrates turns black if positive
369
[additional] indicator: biuret solution
protein, turns violet black if positive
370
[additional] indicator: sudan IV
lipids, turns reddish-orange if positive
371
[additional] examples of non-polar amino acids
glycine, alanine, valine, leucine, isoleucine, methionine, tryptophan, phenylalanine, proline
372
[additional] examples of polar amino acids
serine, threonine, cysteine, tyrosine, asparagine, glutamine
373
[additional] examples of polar charged amino acids
acidic: aspartic acid, glutamic acid; basic: lysine, arginine, histidine
