all topics deck Flashcards
1
Q
epimers
A
sugars that differ only by the configuration around one C atom
2
Q
anomeric carbon
A
alpha - OH points down
3
Q
sphingolipids
A
class of lipids found frequently in biological membranes
4
Q
ceramide
A
fatty acid joined to a sphingosine via amide linkage
5
Q
sphingosine
A
an 18 carbon amino alcohol
6
Q
rules for oxidation states
A
standard state = 0
7
Q
electronegativities
A
FONClBrISCH
8
Q
Aufbau principle
A
e- occupy the lowest energy orbitals available
9
Q
hund’s rule
A
e- in the same subshell occupy available orbitals singly before pairing up
10
Q
pauli exclusion principle
A
no 2 e- in the same atom can have the same set of four quantum numbers
11
Q
diamagnetic
A
all of its e- are spin paired
12
Q
paramagnetic
A
atom’s e- are all NOT spin paired
13
Q
alpha decay
A
reducing the number of protons & neutrons
14
Q
beta decay
A
each type involves the transmutation of a neutron into a proton through the action of the weak nuclear force
15
Q
beta minus decay
A
too many neutrons -> convert into proton and electron
16
Q
beta plus decay
A
contains too few neutrons -> converts proton into a neutron and a positron (antiparticle)
17
Q
electron capture
A
capture an electron from the closest electron shell (n=1) use it in the conversion of a proton into a neutron
18
Q
a nucleus is in an excited energy state
A
usually is the case after a nucleus has undergone alpha or any type of beta decay
19
Q
gamma photons (gamma rays)
A
have neither mass nor charge
20
Q
transition metals & color
A
Electron transitions between nondegenerate d orbitals gives transition metal complexes vivid colors.
21
Q
coordinate covalent bonds
A
one atom donates both of the shared electrons in a bond
22
Q
electron configuration of half filled subshells
A
electron configurations of transition metals like Cu will excite an electron from a 4s orbital into a 3d orbital to gain stability
23
Q
relative strength of ionic systems
A
q1q2/r
24
Q
metallic solids
A
have a sea of valence electrons, aka conduction electrons
25
intermolecular forces
relatively weak interactions that take place between neutral molecules
26
centripetal forces do ___ work
no work
27
projectile motion equations
x = 2*(V^2)*(sin)*(cos)/g
28
perfectly inelastic collisions
maximum possible loss of KE
29
conservation of total angular momentum
Li=Lf
30
interesting property of conductors
excess charge moves to the surface. no net charge within the body of the conductor --> no electrostatic field inside a conductor
31
positively charged particles naturally tend to move toward ____ potential
lower potential
32
negatively charged particles naturally tend to move toward ____ potential
higher potential
33
an electron moving through a potential difference of 1V experiences a KE change of
1.6x10^-19 J = 1 eV
34
(True/False) If the electric potential at a point is 0. That electric field at that same point is nonzero.
True.
35
(True/False) The electric field at a point is zero. The electric potential at the same point is nonzero.
True.
36
going back to series combination bring ____
bring I
37
going back to parallel combination bring ____
bring V
38
magnetic forces can cause particles to ___.
magnetic forces do NO work --> KE is constant --> they cannot affect the speed of a particle
39
magnetic fields are created by ____ and act on ___
magnetic fields are created by moving charged particles and can only act on moving charged particles
40
RH rule for magnetic force
thumb = velocity
41
if the velocity of charged particle is perpendicular to the magnetic field (i.e. angle between v and B is 90) then the subsequent motion of the particle is
Uniform ciruclar motion
42
finding the direction of magnetic field loops (RH rule for current carrying wires)
thumb = direction of I (the current)
43
ferromagnetic
certain metals form permanent magnets
44
permanent bar magnets have magnetic fields bc of
the e-
45
special property of oscillating system that undergoes SHM versus non-ideal oscillating system
frequency (f) and period (T) do NOT depend on amplitude.
46
galvanometer
sensitively measures current using the interaction between currents and magnetic fields
47
the internal resistance of an ammeter is as ____ as possible
the internal resistance of an ammeter is as _small_ as possible
48
the internal resistance of a voltmeter is as ____ as possible
the internal resistance of a voltmeter is as _large_ as possible
49
for a given capacitor, capacitance is ____
for a given capacitor, capacitance is constant
50
capacitors in parallel have the same _____
same voltage
51
capacitors in series have the same _____
same charge
52
The time required for a particle to make one revolution in a uniform magnetic field
does NOT depend on r or v.
53
archimedes' principle
the magnitude of the buoyant force is equal to the weight of the fluid displaced by the object
54
requirements for a fluid to be considered an ideal fluid
the fluid is in compressible.
55
bernoulli effect
the pressure is lower where the flow speed is greater
56
the pressure is _____ where the flow speed is greater
the pressure is _lower_ where the flow speed is greater
57
the pressure is _____ where the flow speed is greater
lower
58
tension
stretching forces
59
compression
squeezing forces
60
shear
bending forces
61
tensile or compressive strain
change in length / original length
62
shear strain
distance of shear / original length
63
stress is _______
stress is pressure
64
strain is ________
strain is change
65
hooke's law
stress = modulus x strain
66
_________ within all parts of an ideal fluid is the same
total energy [density] within all parts of an ideal fluid is the same
67
_________ within all parts of an ideal fluid is the same
total energy [density]
68
flow rate
how much fluid flows per a unit of time
69
flow speed
how fast the fluid moves
70
water leaves the host at a speed of 4 m/s
flow speed
71
the hose ejects water 4 L of water every second
flow rate
72
incompressible
density remains constant
73
if a liquid is incompressible its ______ ______ must be the same everywhere along the pipe
if a liquid is incompressible its flow rate must be the same everywhere along the pipe
74
if a liquid is incompressible its ______ ______ must be the same everywhere along the pipe
flow rate
75
bernoulli's equation can be applied to gases if ....
pressure changes are small
76
viscosity
the force of cohesion between molecules in a fluid
77
viscosity
the resistance to flow
78
efflux speed
sqrt(2*g*D)
79
calorie
heat required to raise 1 g of water 1 C
80
1 cal = _ J
4.2
81
when a substance absorbs or releases heat, one of two things can happen:
either its temperature changes OR
82
specific tells how ____ it is to changing its ___
resistant; temperature
83
specific tells how ____ it is to changing its ___
specific tells how _resistant_ it is to changing its _temperature_
84
hydrogen bonding is (weaker/stronger/equivalent) to dipole-dipole interactions?
stronger
85
during the phase transition of a substance the temperature of a substance _____
does not change
86
during the phase transition of a substance the temperature of a substance _____
during the phase transition of a substance the temperature of a substance _does not change_
87
boyles law
P1V1=P2V2
88
charles law
V1/T1=V2/T2
89
avogrado's law
if both gases at stp, then equal volumes will mean equal moles of each gas
90
salt solubility rules (these rules are 99% reliable)
1. all group I and ammonium salts are soluble
91
phase solubility rules (these rules are 95% reliable)
1. solubility of solids in liquids tends to increase with increasing temperature
92
solubility of solids in liquids tends to _______ with increasing temperature
increase
93
solubility of gases in liquids tends to _______ with increasing temperature
decrease
94
solubility of gases in liquids tends to _______ with increasing pressure
increase
95
volatile
high vapor pressure and vaporize more easily
96
reaction rate is determined by:
1. how frequently the molecules collide
97
chemical equilibrium is a ______ equilibrium
dynamic
98
dynamic equilibrium (in the context of chemistry) is defined as
the molecules are still reacting but there is no net change in the system
99
Arrehenius definition of an acid
acids ionize in water to produce H+ ions
100
Arrehenius definition of an base
bases ionize in water to produce OH- ions
101
Bronsted and lowry definition of acid
acids are proton (H+) donors
102
Bronsted and lowry definition of base
bases are proton (H+) acceptors
103
lewis acd
lewis acids are electron pair acceptors
104
lewis base
lewis bases are electron pair donors
105
lewis acid/base definitions frequently result in the formation of ____
coordinate covalent bonds
106
lewis acid/base definitions frequently result in the formation of ____
lewis acid/base definitions frequently result in the formation of _coordinate covalent bonds_
107
whenever a substance can act as either an acid or a base it is called _______
amphoteric
108
y x 10 ^ -n
pH will be between (n-1) and n
109
closer to n-1
y > 3
110
closer to n
y < 3
111
if K < 10 ^ -4 then you can assume that x is ____ for the weak acid disassociation problems
negligible
112
Activation energy tells you something about
how fast a reaction occurs
113
Gibbs free energy tells you something about
whether or not the reaction will occur
114
Integral proteins are the only component that affect
membrane transport/trafficking
115
Integral proteins are a membrane component that (pass all the way/anchor outside the membrane/anchor inside facing the cytoplasm)
pass all the way through the membrane
116
DNA probe hybridization experiments are used for
The probes for the experiment were designed to hybridize with sequences from normal individuals and would hybridize with mutants to varying degrees based on the severity of the mutation
117
microtubules
determine cell shape
118
microtubles are important for this specific cells function _______
leukocytes
119
phagocytosis requires that the cell
changes shapes so that it may surround and engulf large extracellular particles
120
metallic solids
sea of e-
121
ionic solids
intramolecular force = IMF
122
network solids
covalent bonds = both IMF and intramolecular force
123
molecular solids
intramolecular force = covalent
124
strongest IMF for solids trend
IS > NS > Metallic Solids > Molecular Solids
125
STP
273 K = 0 C
126
aromaticity
1. planar (i.e. cannot be sp3 anywhere)
127
SHM Equation for spring (x=...)
x = A[sin((k/m)1/2t)]
128
small angle approximation for double slit
normal d*sinθ = mλ
small angle approx:
tanθ = sinθ = y/L
d*y/L = mλ
y is the distance from the center band to the bright or dark band being measured
L is the distance from the slits to the screen.
d = distance between slits
129
Arrhenius Equation
k = Ae-Ea/(RT)
130
wavelength of the photon that is absorbed or emitted
1/λ = RH ( 1 / (1/ninitial2 – 1/nfinal2) )
Rydberg constant =
Rh = 1.097×107 m-1.
131
formula used to estimate the energy differences between electron energy levels
ΔE = E(final) – E(initial) = Re ( 1/nfinal2 – 1/ninitial2 )
Rydberg energy =
Re = -2.18×10-18 J
energy change associated with photon that is absorbed or emitted
n=1 lowest energy state
n=infinity (estimate ionization energy)
