CHEM/PHYS Flashcards
(152 cards)
1
Q
Venturi Effect
A
Reduction in fluid pressure when fluid flows through a constricted tube; for air the outside air has a higher static pressure then the oxygen flowing in the tube and can flow into it
2
Q
N (newtons) units?
A
kg x m/s^2
3
Q
watts units
A
Kg* m^2/s^2
4
Q
power eqn
A
power= work/ time SO power= force * velocity
(in watts)
5
Q
work eqn
A
work = force * displacement
(joules)
6
Q
vector
A
characterized by magnitude and direction (ex. velocity, displacement, force)
7
Q
scalar
A
quantity with magnitude only (ex distance)
8
Q
component vector
A
indicates the influence of a vector in a certain direction
X= horizontal velocity * cos ()
Y= vertical velocity * sin ()
9
Q
universal gravitational eqn
A
Force of gravity = (Gm1m2)/r^2
10
Q
Newtons first law
A
an object will stay in motion/ at rest unless acted on by another force (inertia)
Fnet= m*a = 0
11
Q
Newtons 2nd law
A
F=ma
12
Q
Newtons 3rd law
A
for every rxn/force in nature there is an equal and opposite rxn
Force of ab = - Force of ba
13
Q
kinematic eqn with no displacement
A
V= V0 + at
14
Q
kinematic eqn with no final velocity
A
x= v0*t +(at^2)/2
where x = displacement
15
Q
force of gravity (weight on earth)
A
Fg = m*g)
(fg = force of gravity)
16
Q
kinematic eqn no time
A
Vf^2 = V0^2 + 2ax
17
Q
kinematic eqn no acceleration
A
displacement = avg velocity *time
18
Q
centripetal force
A
only force in uniform circular motion; points inwards
Fc = (m * v^2) / r
19
Q
nucleophilicity
A
capacity of a molecule to act as a nucleophile
20
Q
how does nucleophilicity change in a polar protic solvent
A
large nucleophiles = incr nucleophilicity
small nucleophiles = more basic
21
Q
dispersion
A
the separation of light into its component wavelengths when passing through a medium (ex a prism)
22
Q
diffraction
A
the spreading or bending of light waves (ex. single/ double slit experiment)
23
Q
chromatic abberation
A
the dispersive effect with a spherical lens (causes blurriness as light can not be focused on a specific convergence point)
**only in lenses not mirrors
24
Q
refraction
A
the bending of light as it passes through media with different index of refraction (n)
25
index of refraction
speed of light/ speed of light through medium
(speed of light = 3 x 10 ^8 m/s)
26
snells law
n1sin1 = n2sin2
where 1 is one medium and 2 is another
27
what products will form when a symmetric anhydride and water react? what about asymmetric?
carboxylic acid
if asymmetric multiple products will arise
28
what products will form when an asymmetric anhydride and water react?
multiple products will form
29
how do catalysts affect k and Keq?
catalysts increase the rate of reaction by increasing k and do not affect the keq
30
how to make an electrophile more electrophilic?
protonate it (protonation pulls electrons away from the central carbon- making it more positive- and more electrophilic)
31
nucleophile
negative charge (contain e- pair for binding); they seek a positive thing (ex nucleus of an atom)
32
electrophile
"electron loving" typically have a positive charge; accept electrons in chemical rxns
have electron withdrawing group that places partial pos on carbon OR have a polarizable pi bond
ex: halogens
33
if delta G > 0
the reaction will not be spontaneous
34
decomposition reaction
the separation of a single compound into its two or more elemental parts or simpler compunds
35
disproportionation reaction
a type of redox reaction in which an element undergoes both reduction and oxidation to form two different products
36
oxidation reaction
a reaction in which a substance loses electrons
37
reduction reaction
a reaction in which a substance gains electrons
38
human sound range in Hz
20 to 20,000 Hz
39
how do the sound waves used by ultrasounds compare to those of human hearing ability
ultrasounds use sound waves at the upper threshold of human hearing ability (around 20,000 Hz)
40
when a wave changes a medium what happens to the wavelength, speed, and frequency?
wavelength and speed change
frequency remains constant (to conserve energy)
41
sound waves are what type of wave?
longitudinal
42
longitudinal waves
waves in which oscillation of the material is parallel to the direction of propogation
(ex. sound)
43
transverse waves
waves which oscillates perpandicular to the direction of of its propagation
44
standing waves
waveforms with steady nodes and antinodes that form from the interference of incident and reflected waves at a boundary (oscillate but do not more in space; aka stationary waves)
45
doppler effect
quantifies the perceived change in frequency of sound due to relative movement between the source and detector (as detector approaches source frequency heard f'> frequency, f; as detector moves away from source f'
46
saponification
the reaction used to make soap
base (NaOH or KOH) promoted hydrolysis of a triglyceride (ester) to create carboxylate salt (soap) and water
47
amide
amine derivative of a carboxylic acid
48
amine
ammonia derivative; R3N where no more than 2 of the R groups can be Hydrogens and the R can not be a carbonyl group (it can be a carbon)
49
Leydig cells
signaled by LH hormone to release testosterone in mails
50
Sertoli cells
signaled by FSH in males for sperm production
51
State functions
not path dependent just depend on final and initial points
examples: (VG PHEST)
volume, Gibbs free energy, pressure, enthalpy, int energy, entropy, temp
52
electrophilic substitution reactions
involve aromatic ring (switching attached functional group with an electrophile)
53
nucleophilic substitution reaction
(most likely rxn if not aromatic, carbonyl, or pi bonds)
nucleophile attacks electrophile to push out leaving group
(aka neg species comes in to attach to partial pos species pushing out the leaving group)
54
nucleophilic addition reaction
involves carbonyl groups; usually entails a CO double bond turning into tertiary sigma bond (O usually bonds to H)
55
electrophilic addition reaction
usually involves pi bonds (not C=O)
pi bond is broken by an incoming electrophile bonded to a hydrogen or smog of sim nature
ex. c=c reacting with HBr to make CH3CH2Br
56
capacitor capacitance eqn
C= Q/V
where q= charge
c= capacitance
V voltage applied
57
dielectric constant (k)
represents any change to capacitance and its ability to store electrical (potential) energy
58
electromagnetic spectrum (order of incr freq or decr wavelength)
radio waves
Info red (microwaves)
visible light
UV rays
X rays
gamma rays
59
visible light wavelength in nm
ROYGBIV (in decr wavelength)
red- 700 ish (625 to 750)
orange- 590- 625
yellow- 565-590
green- 500 to 565
blue- 485- 500
indigo- 450- 485
violet- 400 ish (380 to 450)
60
energy stored by a capacitor eqn
Energy stored= 1/2 QV
61
optic D DUV Mnemonic
Diverging mirror and lenses always are:
Diminished
Upright
Virtual
62
what type of mirror can produce a real image
only concave mirrors (this only occurs when the object distance > focal length from mirrors surface)
63
concave mirror ________ light and a concave lens _______ light (converges or diverges)
cc mirror-- converging
cc lens-- diverging
64
total internal reflection equation
sin theta = n2/n1
65
what type of molecule is most likely found in a salt bridge
a molecule that disassociates to form ions (an anion and a cation) like mgSO4
66
red cat; an ox
reduction occurs at cathode
oxidation occurs at anode
67
electrodes
where oxidation and reduction occur in electrochemical cells (anode and cathode)
68
electromotive force (emf)
the voltage or electrical potential difference of the cell
if pos= cell is able to release energy (spont- neg delta G)
if neg= cell must absorb energy (nonspont- pos delta G)
69
galvanic (voltaic) cells
spontaneous oxidation.reduction occurs generating electrical energy
(two separate electrolyte solutions (half cells) connected by a conductive material (usually by salt bridge) connects anode to cathode)
70
electrolytic cells
the opposite of galvanic cells; house nonspont oxidation/reduction rxns that req energy input to proceed
71
Ecell eqn
Ecell = E red,cathode- E red,anode
***when subtracting do not multiply potentials by mols oxidized or reduced bc potential of each electrode does not depend on size of electrode rather its identity
72
oxidation state
the charge that an atom would have if the compound was composed of ions (# of electrons an atom can donate/ accept to form a bond with another atom)
ex. NH3 --> NH4+ (N has an oxidation state of -3 in both and H +1)
ex. Mg + 2HCl --> MgCl2 + H2 (Mg changed from 0 to 2+; Cl remained -1; H changed from +1 to 0)
73
extrapolation
extending a curve beyond the range of existing data points
74
interpolation
extending a curve to cover a point that lies between two existing data points
75
fractional distillation
uses differences in boiling point between two substances to separate two liquids by evaporation and condensation
76
boiling point is most affected by hydrogen bonds or molecular weight?
molecules capable of hydrogen bonding have a higher boiling point than molecules of larger MW due to interaction strength
ex. 1-chlorobutane has lower BP than 1-butanol which contains a Hydroxyl group
77
oxidation of ________ alcohols is difficult to accomplish
tertiary due to the required breaking c--c bond breaking
78
radius of curvature
the radius of an imaginary sphere that would be created if a curved surface were to continue forever in both directions
**more curved surface = smaller radius of curvature
**flatter surface= larger radius of curvature
79
electric field (E in newtons per coulomb) eqn
E = V/d where V is voltage (in J per C) and d is distance across which voltage is applied (in m)
80
Hz is equal to
s^-1
ex: if freq = 4 s^-1 it also = 4 Hz
(F= 1/T) frequency can be found by 1/time of one period
81
dipole- dipole interactions
interaction in polar molecules between the partial positive end of one molecule and the partial negative end of another
82
London dispersion forces
occur between all molecules (regardless of polarity) induces a temporary dipole interaction between adjacent molecules (weakest interaction)
83
at the equivalent point the concentrations of acid and base are:
equal
can solve by using Ka or Kb = ([acid][base])/[congugate] ---> since conc acid =base it can be Kb or Ka= [x]^2/[conj]
84
alkali metals
group 1 of the periodic table (Li, Na, K, Rb, Cs)
85
alkaline earth metals
group 2 of the periodic table (ex. Ca)
86
metalloid
elements that have properties between metals and non metals (ex. Si, As, Te)
***this does not occur because a molecule contains metal and non metal components theses terms refer just to one element alone
87
periodic trends: which part of the table is more likely to gain and which is more likely to lose an atom
the left side of the table will more readily lose an e-
the right side of the table (excluding noble gases) will most likely gain electrons
***trend due to electron affinities
88
sublimation
the phase change from solid to gas
89
critical point
the point of a phase change graph that separate gas, liquid, and solid stages ( no distinction)
90
boiling point
the temperature at which the vapor pressure equals the ambient pressure (change from liquid to gas)
91
ambient pressure
the pressure of the surrounding air, gas or liquid in contact with an object in a specific location
92
Sodium Borohydride (NaBH4)
weak reducing agent able to reduce ketones to aldehydes and alcohols but NOT STRONG enough to reduce esters or carboxylic acids
93
random order mechanism
the order in which the substrates bind the enzyme does not matter
94
ordered mechanism
the order in which the substrates bind the enzyme matters; one substrate has to bind before the other can
95
ping pong mechanism (aka double displacement)
the first substrate binds to an enzyme casing the enzyme to change into a m modified form; the first product is then released allowing the second substrate to bond returning the enzyme to its original form
96
buffering capacity of a buffer
a buffer has a buffering capacity of +/- 1 pH unit
97
surface tension
the tension of a surface film of a liquid due to the attraction of particles (H bonds) allowing things of weight smaller than the surface tension to stay on top of the water and not sink in
98
hydrostatic pressure
hydrostatic pressure is the pressure exerted on an object by the liquid it is submerged in
P=pgh
where P is the fluid pressure; p is the fluid density; g is the acceleration due to gravity; h is the depth in liquid
99
viscosity
measure of a fluids internal resistance to flow (the thickness' semi fluidness of a liquid)
100
buoyancy
the upward force that results from immersion in a fluid
buoyant force= - pgV
p= fluid density; g= acceleration due to gravity; V= fluid volume
101
reflection
the change in direction of a wave back into the media of origin at the interface between two different media
102
polarization
the orienting of electric fields of waves of light in parallel directions
103
which saturated fatty acid will be the most water soluble
the fatty acid with the shortest hydrocarbon chain as hydrocarbons are very non polar
104
when pH is less than the pKa the molecule will be
protonated (the free H+ in the solution will be picked up by the molecule to make the equilibrium more happy)
105
when pH is more than the pka the molecule will be
in its deprotonated form (the system wants to get closer to equilibrium so the molecule will deprotonate to create more available H+ and get closer to pH)
106
b- decay
the atomic number increases by one
(a neutron is transformed into a proton)
an e- is emitted
107
b+ decay
the atomic number decreases by 1
(a proton turns into a neutron)
a positron is emmited
108
gamme decay
no atomic number change or transformation
photons emitted
109
alpha decay
the atomic number decreases by 2
no transformation occurs
a Helium atom is emitted
110
divalent
having a valence of two (could be positive or negative for example: Mg, Fe, Zn which are all 2+)
111
Amp (or A) units
Coulomb per second (C/s)
112
Coulomb units
Amps per second
113
conductors
conductors contain free and bound electrons; free electrons organize themselves on the surface (which part of surface depends on direction of external charge) to cancel out external charges so that the internal charge within the conductor is 0
114
blood pressure ratio
ratio of systolic to diastolic pressures (systolic is higher of the two and on top where as diastolic is lower and on bottom)
115
relationship between thermodynamic stability and ratio of products
For a thermodynamic mixture of isomeric products, the relative mole ratio of products is directly related to the relative stability of these products
116
energy stored by a capacitor eqn
E= 1/2(C*V^2) or E=1/2(Q*V)
because Q=CV
(energy in J)
117
charge of a capacitor eqn
Q=C*V (charge in coulombs, C)
118
relative thermodynamic stability of isomeric compounds can be determined experimentally by:
heats of combustion; the thermodynamic stability can be determined by the amount of heat produced when the compounds are combusted, less heat released means greater stability
119
_______ can be used to experimentally determine the energy required to separate the liquid molecules from each other
boiling points
120
most acidic proton
the most acidic hydrogen produces the most stable compound when it is removed; larger eneg differences are more acidic protons (for example a C-H bond will have a less acidic proton then a N-H bond)
121
how to tell if a substance is acidic or basic when comparing Ka and Kb
if Ka> Kb then the substance is acidic
if Kb> Ka then the substance is basic
(Ka*Kb=Kw so Ka or Kb could be given as Kw/Kb or Kw/Ka respectively)
122
limiting reagent
which ever reagent is used up first in a reaction (could be demonstrated by saying there was excess of the other reactant or by saying equal quantities are used but the molar ratio requires more LR per ER)
123
lowest energy electron configuration
ideally all subshells are filled going from lowest to highest (one note is 4s comes before 3d and 4p fills after 3d)
aka ground state
124
d subshells
have 5 orbitals and can hold up to 10 e-
125
p subshells
have 3 orbitals and can hold up to 6e-
126
s subshells
have 1 orbital and can hold up to 2e-
127
how to identify an oxidation reduction rxn
a table is given and the reactants have different reduction potentials OR
the products have different oxidation states then the reactants
128
chelate formation
a metal ion is bound to multiple ligands through multiple coordination sites
129
precipitate formation
a reaction which involves the formation of solid during the course of the reaction (not due to evaporation) (cations and anions in an aq solution react to form insoluble ionic solid)
130
spacing of uniform electric field lines
they are equally spaced at and between both electrodes
131
oxidoreductases
enzymes that catalyze oxidation-reduction reactions (ex. hydroxylation of a methyl group)
132
oxidizing agents
ex: FAD, NAD+, O2
substances which can accept hydrogens causing the other substance to be oxidized while the cofactor (ex FAD) is reduced (ex FADH2)
133
oxidation and reduction in terms of hydrogens
oxidation- loss of H
reduction- gain of H
134
steroid structure
4 fused rings (3 cyclohexane and one cyclopentane)
135
dilution of a buffer (ph change)
causes no pH changes; it dilutes everything causing the pH to remain the same, or barely change
136
sodium is included in solutions to
balence charge
137
formation of a peptide bond produces what by-product?
H2O (18 amu)
138
experimental conditions needed for reliable Michaelis mentor enzyme kinetics
-initial velocity is measured under steady state conditions
-solution pH remains constant at all [S]
-[enzyme] is lower than [substrate]
-measurements are taken BEFORE rxn reaches equilibrium (other wise V0 would be impossible to tell)
139
"amic acid"
compound is a carboxylic derivative containing a nitrogen in place of the usual hydroxyl group (OH)
140
"oic or ic acid"
structure contains a carboxylic acid
formic- H replaces alpha carbon (1c)
acetic- 2 carbons
benzoic- contains a benzene ring at alpha carbon
----------------- (prolly wont need to know the next 2 bc they're weird but:)
Valeric- 5c
caproic-6c
141
lewis base vs acid
lewis base- any species which can donate e- (ex Oxygen or almost anything neg charge
lewis acid- any species which can accept e- (ex H+ or almost anything pos charged)
142
pyrrole ring
a five-membered ring containing a nitrogen atom
143
transferase
an enzyme that catalyzes the movement of something (for ex. the movement of a functional group turning cytosine to methyl cytosine)
144
Keq (equilibrium constant)
keq= [products]/ reactants
**can be inserted into -RTln(Keq)= delta G eqn
145
isoelectric focusing; when will a protein be pos or neg?
when the pH is less than the pI the protein is positive; when the pH is more than the pI it is negative
146
isoelectric point
the pH at which the net charge on a protein is zero
147
volumetric flow rate eqn
volumetric flow rate= Area*Velocity
148
wavelength from speed of sound in certain medium eqn
Velocity= frequency * wavelength
149
Ksp (solubility equilibrium eqn)
Ksp = [A+]^a [B-]^b
A+= cation in aq solution
B-= anion in aq solution
a,b= relative concentrations of a and b
150
spontaneity of rxn when Keq is /= to 1?
Keq< 1--- rxn is nonspont forwards
Keq> 1--- rxn is spont forwards
Keq= 1 --- rxn is at eq
151
oxygen in its standard state is?
a diatomic gas
152
carbon in its standard state is?
a covalent network solid
