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all topics deck Flashcards

1
Q

epimers

A

sugars that differ only by the configuration around one C atom

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2
Q

anomeric carbon

A

alpha - OH points down

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3
Q

sphingolipids

A

class of lipids found frequently in biological membranes

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4
Q

ceramide

A

fatty acid joined to a sphingosine via amide linkage

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5
Q

sphingosine

A

an 18 carbon amino alcohol

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6
Q

rules for oxidation states

A

standard state = 0

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7
Q

electronegativities

A

FONClBrISCH

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8
Q

Aufbau principle

A

e- occupy the lowest energy orbitals available

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9
Q

hund’s rule

A

e- in the same subshell occupy available orbitals singly before pairing up

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10
Q

pauli exclusion principle

A

no 2 e- in the same atom can have the same set of four quantum numbers

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11
Q

diamagnetic

A

all of its e- are spin paired

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12
Q

paramagnetic

A

atom’s e- are all NOT spin paired

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13
Q

alpha decay

A

reducing the number of protons & neutrons

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14
Q

beta decay

A

each type involves the transmutation of a neutron into a proton through the action of the weak nuclear force

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15
Q

beta minus decay

A

too many neutrons -> convert into proton and electron

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16
Q

beta plus decay

A

contains too few neutrons -> converts proton into a neutron and a positron (antiparticle)

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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

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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

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19
Q

gamma photons (gamma rays)

A

have neither mass nor charge

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20
Q

transition metals & color

A

Electron transitions between nondegenerate d orbitals gives transition metal complexes vivid colors.

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21
Q

coordinate covalent bonds

A

one atom donates both of the shared electrons in a bond

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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

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23
Q

relative strength of ionic systems

A

q1q2/r

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24
Q

metallic solids

A

have a sea of valence electrons, aka conduction electrons

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25
Q

intermolecular forces

A

relatively weak interactions that take place between neutral molecules

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26
Q

centripetal forces do ___ work

A

no work

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27
Q

projectile motion equations

A

x = 2(V^2)(sin)*(cos)/g

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28
Q

perfectly inelastic collisions

A

maximum possible loss of KE

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29
Q

conservation of total angular momentum

A

Li=Lf

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30
Q

interesting property of conductors

A

excess charge moves to the surface. no net charge within the body of the conductor –> no electrostatic field inside a conductor

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31
Q

positively charged particles naturally tend to move toward ____ potential

A

lower potential

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32
Q

negatively charged particles naturally tend to move toward ____ potential

A

higher potential

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33
Q

an electron moving through a potential difference of 1V experiences a KE change of

A

1.6x10^-19 J = 1 eV

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34
Q

(True/False) If the electric potential at a point is 0. That electric field at that same point is nonzero.

A

True.

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35
Q

(True/False) The electric field at a point is zero. The electric potential at the same point is nonzero.

A

True.

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36
Q

going back to series combination bring ____

A

bring I

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37
Q

going back to parallel combination bring ____

A

bring V

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38
Q

magnetic forces can cause particles to ___.

A

magnetic forces do NO work –> KE is constant –> they cannot affect the speed of a particle

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39
Q

magnetic fields are created by ____ and act on ___

A

magnetic fields are created by moving charged particles and can only act on moving charged particles

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40
Q

RH rule for magnetic force

A

thumb = velocity

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41
Q

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

A

Uniform ciruclar motion

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42
Q

finding the direction of magnetic field loops (RH rule for current carrying wires)

A

thumb = direction of I (the current)

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43
Q

ferromagnetic

A

certain metals form permanent magnets

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44
Q

permanent bar magnets have magnetic fields bc of

A

the e-

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45
Q

special property of oscillating system that undergoes SHM versus non-ideal oscillating system

A

frequency (f) and period (T) do NOT depend on amplitude.

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46
Q

galvanometer

A

sensitively measures current using the interaction between currents and magnetic fields

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47
Q

the internal resistance of an ammeter is as ____ as possible

A

the internal resistance of an ammeter is as small as possible

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48
Q

the internal resistance of a voltmeter is as ____ as possible

A

the internal resistance of a voltmeter is as large as possible

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49
Q

for a given capacitor, capacitance is ____

A

for a given capacitor, capacitance is constant

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50
Q

capacitors in parallel have the same _____

A

same voltage

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51
Q

capacitors in series have the same _____

A

same charge

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52
Q

The time required for a particle to make one revolution in a uniform magnetic field

A

does NOT depend on r or v.

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53
Q

archimedes’ principle

A

the magnitude of the buoyant force is equal to the weight of the fluid displaced by the object

54
Q

requirements for a fluid to be considered an ideal fluid

A

the fluid is in compressible.

55
Q

bernoulli effect

A

the pressure is lower where the flow speed is greater

56
Q

the pressure is _____ where the flow speed is greater

A

the pressure is lower where the flow speed is greater

57
Q

the pressure is _____ where the flow speed is greater

A

lower

58
Q

tension

A

stretching forces

59
Q

compression

A

squeezing forces

60
Q

shear

A

bending forces

61
Q

tensile or compressive strain

A

change in length / original length

62
Q

shear strain

A

distance of shear / original length

63
Q

stress is _______

A

stress is pressure

64
Q

strain is ________

A

strain is change

65
Q

hooke’s law

A

stress = modulus x strain

66
Q

_________ within all parts of an ideal fluid is the same

A

total energy [density] within all parts of an ideal fluid is the same

67
Q

_________ within all parts of an ideal fluid is the same

A

total energy [density]

68
Q

flow rate

A

how much fluid flows per a unit of time

69
Q

flow speed

A

how fast the fluid moves

70
Q

water leaves the host at a speed of 4 m/s

A

flow speed

71
Q

the hose ejects water 4 L of water every second

A

flow rate

72
Q

incompressible

A

density remains constant

73
Q

if a liquid is incompressible its ______ ______ must be the same everywhere along the pipe

A

if a liquid is incompressible its flow rate must be the same everywhere along the pipe

74
Q

if a liquid is incompressible its ______ ______ must be the same everywhere along the pipe

A

flow rate

75
Q

bernoulli’s equation can be applied to gases if ….

A

pressure changes are small

76
Q

viscosity

A

the force of cohesion between molecules in a fluid

77
Q

viscosity

A

the resistance to flow

78
Q

efflux speed

A

sqrt(2gD)

79
Q

calorie

A

heat required to raise 1 g of water 1 C

80
Q

1 cal = _ J

A

4.2

81
Q

when a substance absorbs or releases heat, one of two things can happen:

A

either its temperature changes OR

82
Q

specific tells how ____ it is to changing its ___

A

resistant; temperature

83
Q

specific tells how ____ it is to changing its ___

A

specific tells how resistant it is to changing its temperature

84
Q

hydrogen bonding is (weaker/stronger/equivalent) to dipole-dipole interactions?

A

stronger

85
Q

during the phase transition of a substance the temperature of a substance _____

A

does not change

86
Q

during the phase transition of a substance the temperature of a substance _____

A

during the phase transition of a substance the temperature of a substance does not change

87
Q

boyles law

A

P1V1=P2V2

88
Q

charles law

A

V1/T1=V2/T2

89
Q

avogrado’s law

A

if both gases at stp, then equal volumes will mean equal moles of each gas

90
Q

salt solubility rules (these rules are 99% reliable)

A
  1. all group I and ammonium salts are soluble
91
Q

phase solubility rules (these rules are 95% reliable)

A
  1. solubility of solids in liquids tends to increase with increasing temperature
92
Q

solubility of solids in liquids tends to _______ with increasing temperature

A

increase

93
Q

solubility of gases in liquids tends to _______ with increasing temperature

A

decrease

94
Q

solubility of gases in liquids tends to _______ with increasing pressure

A

increase

95
Q

volatile

A

high vapor pressure and vaporize more easily

96
Q

reaction rate is determined by:

A
  1. how frequently the molecules collide
97
Q

chemical equilibrium is a ______ equilibrium

A

dynamic

98
Q

dynamic equilibrium (in the context of chemistry) is defined as

A

the molecules are still reacting but there is no net change in the system

99
Q

Arrehenius definition of an acid

A

acids ionize in water to produce H+ ions

100
Q

Arrehenius definition of an base

A

bases ionize in water to produce OH- ions

101
Q

Bronsted and lowry definition of acid

A

acids are proton (H+) donors

102
Q

Bronsted and lowry definition of base

A

bases are proton (H+) acceptors

103
Q

lewis acd

A

lewis acids are electron pair acceptors

104
Q

lewis base

A

lewis bases are electron pair donors

105
Q

lewis acid/base definitions frequently result in the formation of ____

A

coordinate covalent bonds

106
Q

lewis acid/base definitions frequently result in the formation of ____

A

lewis acid/base definitions frequently result in the formation of coordinate covalent bonds

107
Q

whenever a substance can act as either an acid or a base it is called _______

A

amphoteric

108
Q

y x 10 ^ -n

A

pH will be between (n-1) and n

109
Q

closer to n-1

A

y > 3

110
Q

closer to n

A

y < 3

111
Q

if K < 10 ^ -4 then you can assume that x is ____ for the weak acid disassociation problems

A

negligible

112
Q

Activation energy tells you something about

A

how fast a reaction occurs

113
Q

Gibbs free energy tells you something about

A

whether or not the reaction will occur

114
Q

Integral proteins are the only component that affect

A

membrane transport/trafficking

115
Q

Integral proteins are a membrane component that (pass all the way/anchor outside the membrane/anchor inside facing the cytoplasm)

A

pass all the way through the membrane

116
Q

DNA probe hybridization experiments are used for

A

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
Q

microtubules

A

determine cell shape

118
Q

microtubles are important for this specific cells function _______

A

leukocytes

119
Q

phagocytosis requires that the cell

A

changes shapes so that it may surround and engulf large extracellular particles

120
Q

metallic solids

A

sea of e-

121
Q

ionic solids

A

intramolecular force = IMF

122
Q

network solids

A

covalent bonds = both IMF and intramolecular force

123
Q

molecular solids

A

intramolecular force = covalent

124
Q

strongest IMF for solids trend

A

IS > NS > Metallic Solids > Molecular Solids

125
Q

STP

A

273 K = 0 C

126
Q

aromaticity

A
  1. planar (i.e. cannot be sp3 anywhere)
127
Q

SHM Equation for spring (x=…)

A

x = A[sin((k/m)1/2t)]

128
Q

small angle approximation for double slit

A

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

129
Q

Arrhenius Equation

A

k = Ae-Ea/(RT)

130
Q

wavelength of the photon that is absorbed or emitted

A

1/λ = RH ( 1 / (1/ninitial2 – 1/nfinal2) )

Rydberg constant =
Rh = 1.097×107 m-1.

131
Q

formula used to estimate the energy differences between electron energy levels

A

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)

sciences (16 decks)

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