Blueprint FL1: C/P Flashcards
(190 cards)
1
Q
**
hypertonic solutions
A
have lots of solute, little water
cause water to flow out of the cell into the solution
2
Q
hypotonic solutions
A
have lots of water, little solute
cause water to flow from the solution into the cell
3
Q
phase diagram
A
4
Q
boiling point
A
the temperature at which the vapor pressure of a solution is equal to the atmospheric pressure above it
5
Q
why is solid water less dense than liquid water
A
the lattice arrangement allows water molecules to be more spread out than in a liquid
6
Q
degree of ionization
A
the proportion of neutral particles, such as those in a gas or aqueous solution, that are ionized
7
Q
autoionization of water
A
a proton is transferred from one water molecule to another to produce a hydronium ion (H₃O⁺) and a hydroxide ion (OH⁻)
8
Q
equilibrium equation
A
9
Q
equilibrium expression for autoionization of water
A
10
Q
london dispersion forces
A
the weaksest intermolecular force
results from the temporary dipoles as electrons move around in a nonpolar molecule
11
Q
sulfite
A
12
Q
sulfate
A
13
Q
(fresh) water density
A
1g/mL
1kg/L
14
Q
alpha decay
A
15
Q
beta plus decay is also known as….
A
positron emission
16
Q
beta plus decay
A
17
Q
beta minus decay
A
18
Q
positron definition
A
a particle with the same mass as an electron but with a positive charge
19
Q
beta minus decay is also known as….
A
electron emission
20
Q
gamma emission
A
no change in the mass or atomic number
21
Q
mass number
A
number of protons and neutrons
22
Q
atomic number
A
number of protons
23
Q
gamma rays are a form of …
A
ionizing radiation
24
Q
what makes a carbon chiral?
A
must have 4 unique groups attached
25
enantiomers
two molecules which are non superimposable mirror images of another
wedges and dashes are switched
26
mass spectrometry
used to measure the mass-to-charge ratio of molecules by breaking the molecules into smaller ion fragments
27
-oic acid is the suffix for which functional group?
carboxylic acids
28
aldehyde structure
29
carboxylate
the conjugate base of carboxylic acid
30
-al suffix
aldehyde
31
aqueous phase vs organic phasse
The aqueous phase contains water and other charged ions and species
The organic phase contains uncharged species and neutral compounds
32
extraction
when the components of mixture are soluble in two different types of solutions, we can mix them with these 2 solutions and allow them to separate; thus separating the 2 components of the mixture
Then we can evaporate the solvents to be left with the solid components of the original mixture
33
volatile meaning
describes how easily a substance will vaporize (turn into a gas or vapor)
| high volatile substances are more likely to exist as a gas/vapour
34
distillation
the process of separating the components of a liquid mixture through selective evaporation and condensation
35
vacuum distillation
vacuum distillation lowers the pressure above the solution to lower the boiling point and allow for a quicker distillation
36
how do boiling chips prevent bumping
the chips trap air in cavities to form solvent vapor bubbles slowly and continuously as opposed to superheating and boiling at all once!
37
which molecules have higher boiling points?
| smaller vs larger
larger
they have stronger IM forces that hold them together
38
which molecules have higher boiling points
| polar vs nonpolar
polar
they have higher IM forces between the + and - parts of the molecules
39
hydrogen bonds
a dipole-dipole attraction between hydrogen atoms and very electronegative atoms, typically F, O, or N
40
donor and acceptor in hydrogen bonds
41
formal charge
valence electrons in nonbonded atom - (bonds + dots)
42
how to determine valence electrons on a non-bonded atom
43
conservation of eneregy
| KE and PE
44
gravitational potential energy
45
kinetic energy
46
stereocenter
an atom which makes a molecule chiral
4 distinct groups attached
47
sp3 hybridized atoms
have 4 groups (bonds and lone pairs)
48
sp2 hybridized atoms
have 3 groups (bonds and lone pairs)
49
sp hybridized atoms
have 2 groups (bonds and lone pairs)
50
sp3 d2 hybridized atoms
have 6 groups (bonds or lone pairs)
51
sp3 d hybridized atoms
have 5 groups (bonds and lone pairs)
52
s hybridized atoms
have 1 group (1 bond)
53
what group on the periodic table have full valence shells
54
oxidation state
the total number of electrons which have been removed from or added to an element
55
torque equation
56
sin (90) = ...
1
57
sin (180) = ...
0
58
sin (0) = ...
0
59
cos (0) = ...
1
60
cos (45) = ...
0
61
cos (180) = ...
-1
62
average velocity
63
milli
10 ^ -3
1/1000
64
non competitive inhibitor
binds to an allosteric site to alter the active site so the substrate can no long binder
65
competitive inhibitor
bind to the active site of the enzyme to block substrate binding
66
uncompetitive inhibitor
bind to the enzyme-substrate complex (not the free enzyme)
67
competitive inhibition (km and vmax effects)
km is increased (lower affinity for substrate)
vmax is unaffacted
68
uncompetitive inhibition (km and vmax effects)
km is decreased (they increase binding affinity because it stabilizes the ES complex)
vmax is decreased
69
noncompetitive inhibition (km and vmax effect)
Km is unaffected
vmax is reduced
70
thiol
71
carboxyl group
72
pKa meaning
the pH at which a group will donate/lose a proton (H+ atom)
73
acid vs base
| bronsted lowry (protons)
acids: donate protons (H+ atoms)
bases: accept protons (H+ atoms)
74
equivalence point
| titration curve
the point in a titration where the amount of titrant added is enough to completely neutralize the analyte solution
75
tera (T)
a trillion
10^12
76
Giga (G)
a billion
10^9
77
Mega (M)
a million
10^6
78
Kilo (K)
a thousand
10^3
79
Deci (d)
1/10
10^-1
80
centi (c)
1/100
10^-2
81
milli (m)
1/1000
10^-3
82
micro (μ)
1/1,000,000
10^-6
83
nano (n)
1/1,000,000,000
10^-9
84
pico (p)
10^-12
85
Newton's third law
for every action (force) in nature there is an equal and opposite reaction
86
inert meaning
a substance that is not chemically reactive
87
diatomic nitrogen in the atmosphere is inert in that...
the triple bond makes it very stable and unreactive
88
acetone structure
89
ideal bond angle: **linear** electron pair geometry
180 degrees
90
ideal bond angle: **trigonal planar** electron pair geometry
120 degrees
91
ideal bond angle: tetrahedral electron pair geometry
109.5 degrees
92
power formula
work / time
93
power unit
watts = joules / second
94
power of resistor
| formula (x3)
95
power of resistor
| meaning
the rate that energy is dissipated by the resistor
96
total resistance : resistors in parallel
97
total resistance: resistors in series
98
total voltage drop: resistors in series
the total voltage drop will be the sum of the voltage drop across all resistors
99
total voltage drop: resistors in parallel
the total voltage drop will equal the voltage drop at each individual resistor
100
oxidation vs reduction
101
reduction
| in terms of hydrogens and oxygens
the addition of hydrogen or removal of oxygen
102
oxidation
| in terms of hydrogen and oxygen
the removal of hydrogen or addition of oxygen
103
KMnO4 (Potassium Permanganate)
| oxidizing or reducing agent
**oxidizing agent**
| will donate an oxygen, causing another substance to be oxidized
104
H2 with Pd
| reagent
this is a very strong reducing agent, meaning it will add hydrogens wherever it can and turn all double bonds into single bonds
105
oxidizing vs reducing agent
oxidizing agents: cause other substance to be oxidized, are themselves reduced
reducing agents: cause other substance to be reduced, are themselves oxidized
106
list the steroid hormones (5)
testosterone, progesterone, estrogen, aldosterone, cortisol
107
lnsulin (hormone type)
peptide hormone
108
lyase
an enzyme that catalyzes the breaking of bonds
109
isomerase
an enzyme that converts a molecule from one isomer to another
110
transferase
an enzyme that transfers functional groups from one molecule to another
111
oxidoreductase
an enzyme that catalyzes redox reactions
112
infrared spectroscopy
used to determine functional groups in molecules
113
IR spectroscopy: fingerprint region
this is the area below (to the right of) 1500; unique to each molecule
114
IR spectroscopy: diagnostic / functional region
this is the area above (to the left of) 1500; the peaks tell you the functional groups present in your substance
115
carbonyl group wavenumer
| IR spectroscopy
sharp peak around 1750
116
OH group wavelength
| IR spectroscopy
broad peak around 3300
117
NH group wavelength
| IR spectroscopy
broad peak around 3300
118
disulfide bridge
a link between thiol groups in two cysteine residues
119
thiol group
120
sulfide structure
Another name for thioether
121
chiral center
an atom attached to 4 distinct groups
122
reduction potential
the tendency of a chemical species to be reduced by electrons
123
reduction potential units
volts
124
A solution with a greater reduction potential than another species will ...
have a greater affinity for electrons and tend to receive electrons from the other species
125
"H" in thermodynamics
enthalphy
126
"S" in thermodynamics
entropy
127
Gibb's free energy
| equation
128
spontaneous reactions
| delta G
negative delta G
129
nonspontaneous reactions
| delta G
positive delta G
130
delta H = +
delta S = +
spontaneous at high temperatures
131
delta H = +
delta S = -
non spontaneous
132
delta H = -
delta S = -
spontaneous at low temperatures
133
delta H = -
delta S = +
spontaneous
134
how do enzymes speed up reactions
by reducing the activation energy barrier
135
Keq
equilibrium constant
136
equilibrium constant equation
137
Keq > 1
| greater than
higher concnetration of products than reactants at equilibrium
138
Keq < 1
| less than
Higher concentration of reactants than products at equilibrium
139
Keq = 1
Equal concentrations of reactants and products at equilibrium
140
standard free energy change
| symbol
141
net standard free energy change for a multi-step reaction
this will be the sum of the standard free energy changes for each step of the reaction
142
ln (<1) = ...
negative number
143
ln (>1) = ...
positive number
144
# l
ln (0) = ...
undefined
| you can only take the natural log of a number greater than 0
145
ln (<0) = ...
indefined
| you can only take the natural log of a number greater than 0
146
Gibb's free energy equation
147
relationship between angle of incidence and angle of reflection
the two are always equal
148
refraction
the bending of the path of light as it passes from one material into another material
149
index of refraction
a dimensionless number that gives the indication of the light bending ability of that medium
150
total internal reflection
this is when light is refracted past the critical angle such that the light is redirected back into the original medium
151
critical angle
the angle of incidence where the angle of refraction is 90°, and thus the light runs along the interface between the two medium
152
Snell's Law
153
critical angle
| formula
just set the angle of refraction in snells law to 90, and sin 90 = 1
154
index of refraction of air
n = 1
155
if light is going from a medium with a lower index of refraction to a higher one, the light will ...
bend towards the normal
156
total internal reflection can only result when...
a ray of light begins in a higher-index material and reaches a boundary with a lower-index one (ex. going from water to air)
157
phosphate structure
PO4 (3-)
158
phosphate charge
-3
159
if Keq of the forward reaction is x, Keq of the reverse reaction will be...
1 / X
160
alkoxide
the conjugate base of an alcohol
161
heat of formation
the amount of heat absorbed or released when one mole of a compound is formed from its constituent elements
enthalpy of formation
162
exothermic reaction
a reaction in which energy is released in the form of light or heat
163
endothermic reaction
a reaction in which energy (heat) is abosrbed from its surroundings into the system
164
∆H is negative
the reaction is exothermic - gives off heat
165
∆H is positive
endothermic - energy/heat is absorbed from surroundings into the system
166
delta H in thermodynamics
change in ENTHALPY
167
enthalpy
the total heat content of a system
equivalent to the system's internal energy plus the product of volume and pressure
168
enthalpy
| formula
169
Hess's Law
the total enthalpy change for the reaction is the sum of all changes
170
The standard enthalpy of formation of any pure element in its standard state (ex. C, N2, O2, etc.) equals ...
zero!
171
carbocations are very...
| reactuve / unreactive
reactive!
they do not have a full octet and are thus very unstable
172
high entropy (s) value = ...
high disorder!
173
force units
Newtons
174
resistor
a device that impedes the flow of charge in a circuit
175
galvanic/voltaic cell (battery)
an electrochemical cell in which an electric current is generated from spontaneous Oxidation-Reduction reactions
energy is being released
176
electrolytic cell
an electrochemical cell that utilizes an external source of electrical energy to drive a thermodynamically unfavourable reaction
177
capacitor
a device that stores electrical energy in an electric field by accumulating electric charges on two closely spaced surfaces that are insulated from each other
178
opaque
not see-through (oppsite of transparent)
179
at standard temperature, metals are ...
solid
| except mercury (liquid)
180
force of static friction
181
normal force of an object on an incline
normal force will equal perpendicular force mgcos theta
182
list the nucleotides in DNA
183
nucleotides in RNA
thymine is replaced with uracil
184
DNA base pairs always have ....
a purine paired with a pyrimidine
185
what are the purines
186
what are the pyrimidines
187
the adenine - thymine base pairs have ... hydrogen bonds
two
188
the cysteine - guanine base pair has ... hydrogen bonds
three
189
reduction
the addition of hydrogen or removal of oxygen atoms from a compound
190
-ide suffix
A negatively charged molecule
