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Review > Blueprint FL1: C/P > Flashcards

Blueprint FL1: C/P Flashcards

1
Q

**

hypertonic solutions

A

have lots of solute, little water

cause water to flow out of the cell into the solution

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2
Q

hypotonic solutions

A

have lots of water, little solute

cause water to flow from the solution into the cell

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3
Q

phase diagram

A
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4
Q

boiling point

A

the temperature at which the vapor pressure of a solution is equal to the atmospheric pressure above it

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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

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6
Q

degree of ionization

A

the proportion of neutral particles, such as those in a gas or aqueous solution, that are ionized

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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⁻)

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8
Q

equilibrium equation

A
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9
Q

equilibrium expression for autoionization of water

A
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10
Q

london dispersion forces

A

the weaksest intermolecular force

results from the temporary dipoles as electrons move around in a nonpolar molecule

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11
Q

sulfite

A
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12
Q

sulfate

A
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13
Q

(fresh) water density

A

1g/mL

1kg/L

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14
Q

alpha decay

A
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15
Q

beta plus decay is also known as….

A

positron emission

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16
Q

beta plus decay

A
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17
Q

beta minus decay

A
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18
Q

positron definition

A

a particle with the same mass as an electron but with a positive charge

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19
Q

beta minus decay is also known as….

A

electron emission

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20
Q

gamma emission

A

no change in the mass or atomic number

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21
Q

mass number

A

number of protons and neutrons

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22
Q

atomic number

A

number of protons

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23
Q

gamma rays are a form of …

A

ionizing radiation

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24
Q

what makes a carbon chiral?

A

must have 4 unique groups attached

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25
Q

enantiomers

A

two molecules which are non superimposable mirror images of another

wedges and dashes are switched

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26
Q

mass spectrometry

A

used to measure the mass-to-charge ratio of molecules by breaking the molecules into smaller ion fragments

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27
Q

-oic acid is the suffix for which functional group?

A

carboxylic acids

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28
Q

aldehyde structure

A
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29
Q

carboxylate

A

the conjugate base of carboxylic acid

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30
Q

-al suffix

A

aldehyde

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31
Q

aqueous phase vs organic phasse

A

The aqueous phase contains water and other charged ions and species

The organic phase contains uncharged species and neutral compounds

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32
Q

extraction

A

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

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33
Q

volatile meaning

A

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

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34
Q

distillation

A

the process of separating the components of a liquid mixture through selective evaporation and condensation

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35
Q

vacuum distillation

A

vacuum distillation lowers the pressure above the solution to lower the boiling point and allow for a quicker distillation

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36
Q

how do boiling chips prevent bumping

A

the chips trap air in cavities to form solvent vapor bubbles slowly and continuously as opposed to superheating and boiling at all once!

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37
Q

which molecules have higher boiling points?

smaller vs larger

A

larger

they have stronger IM forces that hold them together

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38
Q

which molecules have higher boiling points

polar vs nonpolar

A

polar

they have higher IM forces between the + and - parts of the molecules

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39
Q

hydrogen bonds

A

a dipole-dipole attraction between hydrogen atoms and very electronegative atoms, typically F, O, or N

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40
Q

donor and acceptor in hydrogen bonds

A
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41
Q

formal charge

A

valence electrons in nonbonded atom - (bonds + dots)

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42
Q

how to determine valence electrons on a non-bonded atom

A
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43
Q

conservation of eneregy

KE and PE

A
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44
Q

gravitational potential energy

A
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45
Q

kinetic energy

A
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46
Q

stereocenter

A

an atom which makes a molecule chiral

4 distinct groups attached

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47
Q

sp3 hybridized atoms

A

have 4 groups (bonds and lone pairs)

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48
Q

sp2 hybridized atoms

A

have 3 groups (bonds and lone pairs)

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49
Q

sp hybridized atoms

A

have 2 groups (bonds and lone pairs)

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50
Q

sp3 d2 hybridized atoms

A

have 6 groups (bonds or lone pairs)

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51
Q

sp3 d hybridized atoms

A

have 5 groups (bonds and lone pairs)

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52
Q

s hybridized atoms

A

have 1 group (1 bond)

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53
Q

what group on the periodic table have full valence shells

A
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54
Q

oxidation state

A

the total number of electrons which have been removed from or added to an element

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55
Q

torque equation

A
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56
Q

sin (90) = …

A

1

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57
Q

sin (180) = …

A

0

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58
Q

sin (0) = …

A

0

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59
Q

cos (0) = …

A

1

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60
Q

cos (45) = …

A

0

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61
Q

cos (180) = …

A

-1

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62
Q

average velocity

A
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63
Q

milli

A

10 ^ -3

1/1000

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64
Q

non competitive inhibitor

A

binds to an allosteric site to alter the active site so the substrate can no long binder

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65
Q

competitive inhibitor

A

bind to the active site of the enzyme to block substrate binding

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66
Q

uncompetitive inhibitor

A

bind to the enzyme-substrate complex (not the free enzyme)

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67
Q

competitive inhibition (km and vmax effects)

A

km is increased (lower affinity for substrate)
vmax is unaffacted

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68
Q

uncompetitive inhibition (km and vmax effects)

A

km is decreased (they increase binding affinity because it stabilizes the ES complex)
vmax is decreased

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69
Q

noncompetitive inhibition (km and vmax effect)

A

Km is unaffected
vmax is reduced

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70
Q

thiol

A
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71
Q

carboxyl group

A
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72
Q

pKa meaning

A

the pH at which a group will donate/lose a proton (H+ atom)

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73
Q

acid vs base

bronsted lowry (protons)

A

acids: donate protons (H+ atoms)
bases: accept protons (H+ atoms)

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74
Q

equivalence point

titration curve

A

the point in a titration where the amount of titrant added is enough to completely neutralize the analyte solution

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75
Q

tera (T)

A

a trillion

10^12

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76
Q

Giga (G)

A

a billion

10^9

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77
Q

Mega (M)

A

a million

10^6

78
Q

Kilo (K)

A

a thousand

10^3

79
Q

Deci (d)

A

1/10

10^-1

80
Q

centi (c)

A

1/100

10^-2

81
Q

milli (m)

A

1/1000

10^-3

82
Q

micro (μ)

A

1/1,000,000

10^-6

83
Q

nano (n)

A

1/1,000,000,000

10^-9

84
Q

pico (p)

A

10^-12

85
Q

Newton’s third law

A

for every action (force) in nature there is an equal and opposite reaction

86
Q

inert meaning

A

a substance that is not chemically reactive

87
Q

diatomic nitrogen in the atmosphere is inert in that…

A

the triple bond makes it very stable and unreactive

88
Q

acetone structure

A
89
Q

ideal bond angle: linear electron pair geometry

A

180 degrees

90
Q

ideal bond angle: trigonal planar electron pair geometry

A

120 degrees

91
Q

ideal bond angle: tetrahedral electron pair geometry

A

109.5 degrees

92
Q

power formula

A

work / time

93
Q

power unit

A

watts = joules / second

94
Q

power of resistor

formula (x3)

A
95
Q

power of resistor

meaning

A

the rate that energy is dissipated by the resistor

96
Q

total resistance : resistors in parallel

A
97
Q

total resistance: resistors in series

A
98
Q

total voltage drop: resistors in series

A

the total voltage drop will be the sum of the voltage drop across all resistors

99
Q

total voltage drop: resistors in parallel

A

the total voltage drop will equal the voltage drop at each individual resistor

100
Q

oxidation vs reduction

A
101
Q

reduction

in terms of hydrogens and oxygens

A

the addition of hydrogen or removal of oxygen

102
Q

oxidation

in terms of hydrogen and oxygen

A

the removal of hydrogen or addition of oxygen

103
Q

KMnO4 (Potassium Permanganate)

oxidizing or reducing agent

A

oxidizing agent

will donate an oxygen, causing another substance to be oxidized

104
Q

H2 with Pd

reagent

A

this is a very strong reducing agent, meaning it will add hydrogens wherever it can and turn all double bonds into single bonds

105
Q

oxidizing vs reducing agent

A

oxidizing agents: cause other substance to be oxidized, are themselves reduced
reducing agents: cause other substance to be reduced, are themselves oxidized

106
Q

list the steroid hormones (5)

A

testosterone, progesterone, estrogen, aldosterone, cortisol

107
Q

lnsulin (hormone type)

A

peptide hormone

108
Q

lyase

A

an enzyme that catalyzes the breaking of bonds

109
Q

isomerase

A

an enzyme that converts a molecule from one isomer to another

110
Q

transferase

A

an enzyme that transfers functional groups from one molecule to another

111
Q

oxidoreductase

A

an enzyme that catalyzes redox reactions

112
Q

infrared spectroscopy

A

used to determine functional groups in molecules

113
Q

IR spectroscopy: fingerprint region

A

this is the area below (to the right of) 1500; unique to each molecule

114
Q

IR spectroscopy: diagnostic / functional region

A

this is the area above (to the left of) 1500; the peaks tell you the functional groups present in your substance

115
Q

carbonyl group wavenumer

IR spectroscopy

A

sharp peak around 1750

116
Q

OH group wavelength

IR spectroscopy

A

broad peak around 3300

117
Q

NH group wavelength

IR spectroscopy

A

broad peak around 3300

118
Q

disulfide bridge

A

a link between thiol groups in two cysteine residues

119
Q

thiol group

A
120
Q

sulfide structure

A

Another name for thioether

121
Q

chiral center

A

an atom attached to 4 distinct groups

122
Q

reduction potential

A

the tendency of a chemical species to be reduced by electrons

123
Q

reduction potential units

A

volts

124
Q

A solution with a greater reduction potential than another species will …

A

have a greater affinity for electrons and tend to receive electrons from the other species

125
Q

“H” in thermodynamics

A

enthalphy

126
Q

“S” in thermodynamics

A

entropy

127
Q

Gibb’s free energy

equation

A
128
Q

spontaneous reactions

delta G

A

negative delta G

129
Q

nonspontaneous reactions

delta G

A

positive delta G

130
Q

delta H = +
delta S = +

A

spontaneous at high temperatures

131
Q

delta H = +
delta S = -

A

non spontaneous

132
Q

delta H = -
delta S = -

A

spontaneous at low temperatures

133
Q

delta H = -
delta S = +

A

spontaneous

134
Q

how do enzymes speed up reactions

A

by reducing the activation energy barrier

135
Q

Keq

A

equilibrium constant

136
Q

equilibrium constant equation

A
137
Q

Keq > 1

greater than

A

higher concnetration of products than reactants at equilibrium

138
Q

Keq < 1

less than

A

Higher concentration of reactants than products at equilibrium

139
Q

Keq = 1

A

Equal concentrations of reactants and products at equilibrium

140
Q

standard free energy change

symbol

A
141
Q

net standard free energy change for a multi-step reaction

A

this will be the sum of the standard free energy changes for each step of the reaction

142
Q

ln (<1) = …

A

negative number

143
Q

ln (>1) = …

A

positive number

144
Q

l

ln (0) = …

A

undefined

you can only take the natural log of a number greater than 0

145
Q

ln (<0) = …

A

indefined

you can only take the natural log of a number greater than 0

146
Q

Gibb’s free energy equation

A
147
Q

relationship between angle of incidence and angle of reflection

A

the two are always equal

148
Q

refraction

A

the bending of the path of light as it passes from one material into another material

149
Q

index of refraction

A

a dimensionless number that gives the indication of the light bending ability of that medium

150
Q

total internal reflection

A

this is when light is refracted past the critical angle such that the light is redirected back into the original medium

151
Q

critical angle

A

the angle of incidence where the angle of refraction is 90°, and thus the light runs along the interface between the two medium

152
Q

Snell’s Law

A
153
Q

critical angle

formula

A

just set the angle of refraction in snells law to 90, and sin 90 = 1

154
Q

index of refraction of air

A

n = 1

155
Q

if light is going from a medium with a lower index of refraction to a higher one, the light will …

A

bend towards the normal

156
Q

total internal reflection can only result when…

A

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
Q

phosphate structure

A

PO4 (3-)

158
Q

phosphate charge

A

-3

159
Q

if Keq of the forward reaction is x, Keq of the reverse reaction will be…

A

1 / X

160
Q

alkoxide

A

the conjugate base of an alcohol

161
Q

heat of formation

A

the amount of heat absorbed or released when one mole of a compound is formed from its constituent elements

enthalpy of formation

162
Q

exothermic reaction

A

a reaction in which energy is released in the form of light or heat

163
Q

endothermic reaction

A

a reaction in which energy (heat) is abosrbed from its surroundings into the system

164
Q

∆H is negative

A

the reaction is exothermic - gives off heat

165
Q

∆H is positive

A

endothermic - energy/heat is absorbed from surroundings into the system

166
Q

delta H in thermodynamics

A

change in ENTHALPY

167
Q

enthalpy

A

the total heat content of a system

equivalent to the system’s internal energy plus the product of volume and pressure

168
Q

enthalpy

formula

A
169
Q

Hess’s Law

A

the total enthalpy change for the reaction is the sum of all changes

170
Q

The standard enthalpy of formation of any pure element in its standard state (ex. C, N2, O2, etc.) equals …

A

zero!

171
Q

carbocations are very…

reactuve / unreactive

A

reactive!

they do not have a full octet and are thus very unstable

172
Q

high entropy (s) value = …

A

high disorder!

173
Q

force units

A

Newtons

174
Q

resistor

A

a device that impedes the flow of charge in a circuit

175
Q

galvanic/voltaic cell (battery)

A

an electrochemical cell in which an electric current is generated from spontaneous Oxidation-Reduction reactions

energy is being released

176
Q

electrolytic cell

A

an electrochemical cell that utilizes an external source of electrical energy to drive a thermodynamically unfavourable reaction

177
Q

capacitor

A

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
Q

opaque

A

not see-through (oppsite of transparent)

179
Q

at standard temperature, metals are …

A

solid

except mercury (liquid)

180
Q

force of static friction

A
181
Q

normal force of an object on an incline

A

normal force will equal perpendicular force mgcos theta

182
Q

list the nucleotides in DNA

A
183
Q

nucleotides in RNA

A

thymine is replaced with uracil

184
Q

DNA base pairs always have ….

A

a purine paired with a pyrimidine

185
Q

what are the purines

A
186
Q

what are the pyrimidines

A
187
Q

the adenine - thymine base pairs have … hydrogen bonds

A

two

188
Q

the cysteine - guanine base pair has … hydrogen bonds

A

three

189
Q

reduction

A

the addition of hydrogen or removal of oxygen atoms from a compound

190
Q

-ide suffix

A

A negatively charged molecule

Review (28 decks)

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