all topics deck Flashcards
epimers
sugars that differ only by the configuration around one C atom
anomeric carbon
alpha - OH points down
sphingolipids
class of lipids found frequently in biological membranes
ceramide
fatty acid joined to a sphingosine via amide linkage
sphingosine
an 18 carbon amino alcohol
rules for oxidation states
standard state = 0
electronegativities
FONClBrISCH
Aufbau principle
e- occupy the lowest energy orbitals available
hund’s rule
e- in the same subshell occupy available orbitals singly before pairing up
pauli exclusion principle
no 2 e- in the same atom can have the same set of four quantum numbers
diamagnetic
all of its e- are spin paired
paramagnetic
atom’s e- are all NOT spin paired
alpha decay
reducing the number of protons & neutrons
beta decay
each type involves the transmutation of a neutron into a proton through the action of the weak nuclear force
beta minus decay
too many neutrons -> convert into proton and electron
beta plus decay
contains too few neutrons -> converts proton into a neutron and a positron (antiparticle)
electron capture
capture an electron from the closest electron shell (n=1) use it in the conversion of a proton into a neutron
a nucleus is in an excited energy state
usually is the case after a nucleus has undergone alpha or any type of beta decay
gamma photons (gamma rays)
have neither mass nor charge
transition metals & color
Electron transitions between nondegenerate d orbitals gives transition metal complexes vivid colors.
coordinate covalent bonds
one atom donates both of the shared electrons in a bond
electron configuration of half filled subshells
electron configurations of transition metals like Cu will excite an electron from a 4s orbital into a 3d orbital to gain stability
relative strength of ionic systems
q1q2/r
metallic solids
have a sea of valence electrons, aka conduction electrons
intermolecular forces
relatively weak interactions that take place between neutral molecules
centripetal forces do ___ work
no work
projectile motion equations
x = 2(V^2)(sin)*(cos)/g
perfectly inelastic collisions
maximum possible loss of KE
conservation of total angular momentum
Li=Lf
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
positively charged particles naturally tend to move toward ____ potential
lower potential
negatively charged particles naturally tend to move toward ____ potential
higher potential
an electron moving through a potential difference of 1V experiences a KE change of
1.6x10^-19 J = 1 eV
(True/False) If the electric potential at a point is 0. That electric field at that same point is nonzero.
True.
(True/False) The electric field at a point is zero. The electric potential at the same point is nonzero.
True.
going back to series combination bring ____
bring I
going back to parallel combination bring ____
bring V
magnetic forces can cause particles to ___.
magnetic forces do NO work –> KE is constant –> they cannot affect the speed of a particle
magnetic fields are created by ____ and act on ___
magnetic fields are created by moving charged particles and can only act on moving charged particles
RH rule for magnetic force
thumb = velocity
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
finding the direction of magnetic field loops (RH rule for current carrying wires)
thumb = direction of I (the current)
ferromagnetic
certain metals form permanent magnets
permanent bar magnets have magnetic fields bc of
the e-
special property of oscillating system that undergoes SHM versus non-ideal oscillating system
frequency (f) and period (T) do NOT depend on amplitude.
galvanometer
sensitively measures current using the interaction between currents and magnetic fields
the internal resistance of an ammeter is as ____ as possible
the internal resistance of an ammeter is as small as possible
the internal resistance of a voltmeter is as ____ as possible
the internal resistance of a voltmeter is as large as possible
for a given capacitor, capacitance is ____
for a given capacitor, capacitance is constant
capacitors in parallel have the same _____
same voltage
capacitors in series have the same _____
same charge
The time required for a particle to make one revolution in a uniform magnetic field
does NOT depend on r or v.
archimedes’ principle
the magnitude of the buoyant force is equal to the weight of the fluid displaced by the object
requirements for a fluid to be considered an ideal fluid
the fluid is in compressible.
bernoulli effect
the pressure is lower where the flow speed is greater
the pressure is _____ where the flow speed is greater
the pressure is lower where the flow speed is greater
the pressure is _____ where the flow speed is greater
lower
tension
stretching forces
compression
squeezing forces
shear
bending forces
tensile or compressive strain
change in length / original length
shear strain
distance of shear / original length
stress is _______
stress is pressure
strain is ________
strain is change
hooke’s law
stress = modulus x strain
_________ within all parts of an ideal fluid is the same
total energy [density] within all parts of an ideal fluid is the same
_________ within all parts of an ideal fluid is the same
total energy [density]
flow rate
how much fluid flows per a unit of time
flow speed
how fast the fluid moves
water leaves the host at a speed of 4 m/s
flow speed
the hose ejects water 4 L of water every second
flow rate
incompressible
density remains constant
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
if a liquid is incompressible its ______ ______ must be the same everywhere along the pipe
flow rate
bernoulli’s equation can be applied to gases if ….
pressure changes are small
viscosity
the force of cohesion between molecules in a fluid
viscosity
the resistance to flow
efflux speed
sqrt(2gD)
calorie
heat required to raise 1 g of water 1 C
1 cal = _ J
4.2
when a substance absorbs or releases heat, one of two things can happen:
either its temperature changes OR
specific tells how ____ it is to changing its ___
resistant; temperature
specific tells how ____ it is to changing its ___
specific tells how resistant it is to changing its temperature
hydrogen bonding is (weaker/stronger/equivalent) to dipole-dipole interactions?
stronger
during the phase transition of a substance the temperature of a substance _____
does not change
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
boyles law
P1V1=P2V2
charles law
V1/T1=V2/T2
avogrado’s law
if both gases at stp, then equal volumes will mean equal moles of each gas
salt solubility rules (these rules are 99% reliable)
- all group I and ammonium salts are soluble
phase solubility rules (these rules are 95% reliable)
- solubility of solids in liquids tends to increase with increasing temperature
solubility of solids in liquids tends to _______ with increasing temperature
increase
solubility of gases in liquids tends to _______ with increasing temperature
decrease
solubility of gases in liquids tends to _______ with increasing pressure
increase
volatile
high vapor pressure and vaporize more easily
reaction rate is determined by:
- how frequently the molecules collide
chemical equilibrium is a ______ equilibrium
dynamic
dynamic equilibrium (in the context of chemistry) is defined as
the molecules are still reacting but there is no net change in the system
Arrehenius definition of an acid
acids ionize in water to produce H+ ions
Arrehenius definition of an base
bases ionize in water to produce OH- ions
Bronsted and lowry definition of acid
acids are proton (H+) donors
Bronsted and lowry definition of base
bases are proton (H+) acceptors
lewis acd
lewis acids are electron pair acceptors
lewis base
lewis bases are electron pair donors
lewis acid/base definitions frequently result in the formation of ____
coordinate covalent bonds
lewis acid/base definitions frequently result in the formation of ____
lewis acid/base definitions frequently result in the formation of coordinate covalent bonds
whenever a substance can act as either an acid or a base it is called _______
amphoteric
y x 10 ^ -n
pH will be between (n-1) and n
closer to n-1
y > 3
closer to n
y < 3
if K < 10 ^ -4 then you can assume that x is ____ for the weak acid disassociation problems
negligible
Activation energy tells you something about
how fast a reaction occurs
Gibbs free energy tells you something about
whether or not the reaction will occur
Integral proteins are the only component that affect
membrane transport/trafficking
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
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
microtubules
determine cell shape
microtubles are important for this specific cells function _______
leukocytes
phagocytosis requires that the cell
changes shapes so that it may surround and engulf large extracellular particles
metallic solids
sea of e-
ionic solids
intramolecular force = IMF
network solids
covalent bonds = both IMF and intramolecular force
molecular solids
intramolecular force = covalent
strongest IMF for solids trend
IS > NS > Metallic Solids > Molecular Solids
STP
273 K = 0 C
aromaticity
- planar (i.e. cannot be sp3 anywhere)
SHM Equation for spring (x=…)
x = A[sin((k/m)1/2t)]
small angle approximation for double slit
normal dsinθ = mλ
small angle approx:
tanθ = sinθ = y/L
dy/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
Arrhenius Equation
k = Ae-Ea/(RT)
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.
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)
